{"pkgId":"26","subjectId":"704","fullwidthLayout":false,"contentData":{"PACKAGE_NAME":"Bahrain Curriculum Full Access","PACKAGE_SLUG":"bahrain-full","PACKAGE_IMG":"file_387203896_1592480631.png","ADMCOURSE_ID":"147","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","STANDARD_NAME":"Bahrain","ADMSUBJECT_ID":"704","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","CAT_NAME":"\u0627\u0644\u0645\u0631\u0643\u0628\u0627\u062a \u0627\u0644\u0623\u064a\u0648\u0646\u064a\u0629","CONT_ID":"568","CONT_TITLE":"Ionic Compounds","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E\r\n \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E\r\n \r\n\u003Cdiv\u003EIonic compounds consist of positively charged cations and negatively charged anions. Ionic compounds are solid at room temperature. They are brittle in nature. 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These compounds are highly soluble in water and conduct electricity in aqueous state only.\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Learning objectives\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;After completing this module, you will be able to:\u0026lt;br\u0026gt;- Identify ionic compounds.\u0026lt;br\u0026gt;- Demonstrate the solubility of ionic compounds.\u0026lt;br\u0026gt;- Examine the electrical conductivity of ionic compounds.\u0026lt;br\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0627\u0644\u0645\u0631\u0643\u0628\u0627\u062a \u0627\u0644\u0623\u064a\u0648\u0646\u064a\u0629","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"},{"CONT_ID":"508","CATEGORY_ID":"1","CONT_TITLE":"Formation of Ionic Bonds","CONT_SLUG":"formation-of-ionic-bonds","CONT_TITLE_AR":"","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAn ionic bond is the electrostatic attraction between two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion. Elements in columns 1, 2, and 3 on the periodic chart are likely to form ionic bonds with elements in columns 15, 16, and 17.\u003C\/div\u003E \r\n\u003Cdiv\u003E\u003Cbr\u003E\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E\u003Cbr\u003E\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to: \u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain what is an ionic compound. \u003C\/div\u003E \r\n\u003Cdiv\u003E- Form ionic compounds.\u003C\/div\u003E","CONT_DESC_AR":"","BACKING_FILE":null,"FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":null,"MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200432","TOPIC_ID":"hs200432","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200432.jpg","PUBLIC_BANNER_IMG":"HS200432.jpg","PUBLIC_VIDEO":"pvideo_hs200432.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/fuvvXfCCOBg","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"0","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"Overview:\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;An ionic bond is the electrostatic attraction between two oppositely charged ions. 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E\u0026lt;span style=\u0026quot;color: rgb(38, 50, 56); font-family: Roboto, sans-serif;\u0026quot;\u0026gt;lements in columns 1, 2, and 3 on the periodic chart are likely to form ionic bonds with elements in columns 15, 16, and 17.\u0026lt;\/span\u0026gt;\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Learning objectives\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;After completing this module, you will be able to:\u0026lt;br\u0026gt;\u0026amp;nbsp;- Explain what is an ionic compound.\u0026lt;br\u0026gt;\u0026amp;nbsp;- Form ionic compounds.\u0026lt;br\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u062a\u0643\u0648\u064a\u0646 \u0627\u0644\u0631\u0648\u0627\u0628\u0637 \u0627\u0644\u0623\u064a\u0648\u0646\u064a\u0629","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"},{"CONT_ID":"504","CATEGORY_ID":"1","CONT_TITLE":"Today\u0027s Periodic Table","CONT_SLUG":"todays-periodic-table","CONT_TITLE_AR":"","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EThe Periodic table is the systematic arrangement of 118 elements in the increasing order of their atomic number. The rows in the periodic table are called periods and the columns in the periodic table are called groups.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain what groups and periods are.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the criteria for placing elements in the periodic table.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Provide a suitable name for each group.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Arrange elements according to their atomic number.\u003C\/div\u003E","CONT_DESC_AR":"","BACKING_FILE":null,"FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":null,"MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200413","TOPIC_ID":"hs200413","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200413.jpg","PUBLIC_BANNER_IMG":"HS200413.jpg","PUBLIC_VIDEO":"pvideo_hs200413.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/jnMKcnEqf5o","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"0","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"Overview:\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;The Periodic table is the systematic arrangement of 118 elements in the increasing order of their atomic number. The rows in the periodic table are called periods and the columns in the periodic table are called groups.\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Learning objectives\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain what groups and periods are.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain the criteria for placing elements in the periodic table.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Provide a suitable name for each group.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Arrange elements according to their atomic number.\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a \u0627\u0644\u062d\u062f\u064a\u062b","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"},{"CONT_ID":"503","CATEGORY_ID":"1","CONT_TITLE":"Nucleic Acids","CONT_SLUG":"nucleic-acid","CONT_TITLE_AR":"","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003ENucleic acids are biomolecules present in living cells, especially DNA (deoxyribonucleic acid) or RNA (ribonucleic acid), whose molecules consist of many nucleotides linked in a long chain. Nucleic acid is made up of nucleotides. A nucleotide consists of a sugar, phosphate and nitrogenous base.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain what a nucleic acid is.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Describe the structure of a nucleotide.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify the different components of RNA and DNA.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Construct a nucleic acid.\u003C\/div\u003E","CONT_DESC_AR":"","BACKING_FILE":null,"FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":null,"MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200408","TOPIC_ID":"hs200408","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200408.jpg","PUBLIC_BANNER_IMG":"HS200408.jpg","PUBLIC_VIDEO":"pvideo_hs200408.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/L5hwt0XTjzc","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"0","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"Overview:\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Nucleic acids are biomolecules present in living cells, especially DNA (deoxyribonucleic acid) or RNA (ribonucleic acid), whose molecules consist of many nucleotides linked in a long chain. Nucleic acid is made up of nucleotides. 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Atoms which attain noble gas configuration are non reactive in nature and are called stable atoms. Atoms which do not attain noble gas configuration are reactive in nature and are called unstable atoms.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the conditions for an atom to be stable.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Describe how an atom can be made stable or unstable.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify stable and unstable atoms.\u003C\/div\u003E","CONT_DESC_AR":"","BACKING_FILE":null,"FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":null,"MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200310","TOPIC_ID":"hs200310","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200310.jpg","PUBLIC_BANNER_IMG":"HS200310.jpg","PUBLIC_VIDEO":"pvideo_hs200310.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/1B18nNgKKDc","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"0","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"Overview:\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Atoms become chemically stable by losing or gaining to fill up their outermost electron shell to a configuration nearest to that of a noble gas. Atoms which attain noble gas configuration are non reactive in nature and are called stable atoms. Atoms which do not attain noble gas configuration are reactive in nature and are called unstable atoms.\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Learning objectives\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain the conditions for an atom to be stable.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Describe how an atom can be made stable or unstable.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Identify stable and unstable atoms.\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0627\u0644\u0630\u0631\u0627\u062a \u0627\u0644\u0645\u0633\u062a\u0642\u0631\u0629 \u0648\u063a\u064a\u0631 \u0627\u0644\u0645\u0633\u062a\u0642\u0631\u0629","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - 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atom.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Define ions.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify the type of ion formed by a neutral atom according to its place in the periodic table.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Classify ions as anions or cations.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Categorize ions as monovalent, divalent, or 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\u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EValence shell electron pair repulsion (VSEPR) theory is used in chemistry to predict the three-dimensional shapes of molecules from the number of electron pairs surrounding their central atoms. Molecules can have linear, trigonal planar, bent, tetrahedral, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal or pentagonal bipyramidal geometries.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Construct molecules having linear, trigonal planar, bent, tetrahedral, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal and pentagonal bipyramidal geometries.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Apply VSEPR theory to predict the three-dimensional shapes of molecules.\u003C\/div\u003E","CONT_DESC_AR":"Valence shell electron pair repulsion (VSEPR)\u0026amp;nbsp;theory\u0026amp;nbsp;is used in chemistry to predict the three-dimensional shapes of molecules from the number of electron pairs surrounding their central atoms. Molecules can have linear, trigonal planar, bent, tetrahedral, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal or pentagonal bipyramidal geometries.\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation you will be able to:\u0026lt;br \/\u0026gt;\n- construct molecules having linear, trigonal planar, bent, tetrahedral, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal and pentagonal bipyramidal geometries\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n- apply VSEPR theory to predict the three-dimensional shapes of molecules","BACKING_FILE":null,"FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.ss200035","TOPIC_ID":"ss200035","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_SS200035.jpg","PUBLIC_BANNER_IMG":"SS200035.jpg","PUBLIC_VIDEO":"pvideo_ss200035.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/gR_7S2Lk39g","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;div\u0026gt;Overview:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Valence shell electron pair repulsion (VSEPR) theory is used in chemistry to predict the three-dimensional shapes of molecules from the number of electron pairs surrounding their central atoms. Molecules can have linear, trigonal planar, bent, tetrahedral, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal or pentagonal bipyramidal geometries.\u0026amp;nbsp;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Learning Objectives:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Construct molecules having linear, trigonal planar, bent, tetrahedral, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal and pentagonal bipyramidal geometries.\u0026amp;nbsp;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Apply VSEPR theory to predict the three-dimensional shapes of molecules.\u0026lt;\/div\u0026gt;\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u062a\u0637\u0628\u064a\u0642\u0627\u062a \u0646\u0638\u0631\u064a\u0629 \u0641\u064a\u0633\u0628\u0631","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"},{"CONT_ID":"371","CATEGORY_ID":"1","CONT_TITLE":"VSEPR Theory","CONT_SLUG":"vsepr-theory","CONT_TITLE_AR":"VSEPR Theory","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E \u003Cdiv\u003E  \u003Cbr\u003E \u003C\/div\u003E \u003Cdiv\u003EValence shell electron pair repulsion (VSEPR) theory suggests that the electron pairs surrounding the central atom repel each other and tend to occupy such positions around the central atom that minimize this repulsion. According to this theory, the geometry of a molecule depends upon the total number of electron pairs present around the central atom.\u003C\/div\u003E \u003Cdiv\u003E  \u003Cbr\u003E \u003C\/div\u003E \u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \u003Cdiv\u003E  \u003Cbr\u003E \u003C\/div\u003E \u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \u003Cdiv\u003E- Explain valence shell electron pair repulsion (VSEPR) theory.\u003C\/div\u003E \u003Cdiv\u003E- Predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.\u003C\/div\u003E","CONT_DESC_AR":"According to valence shell electron pair repulsion (VSEPR) theory, the valence electron pairs surrounding an atom mutually repel each other. They adopt an arrangement that minimizes this repulsion, thus determining its molecular geometry. This means that bonding and non-bonding electrons will repel each other as far away as geometrically possible. 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According to this theory, the geometry of a molecule depends upon the total number of electron pairs present around the central atom.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;span style=\u0026quot;font-weight: bold;\u0026quot;\u0026gt;Learning Objectives:\u0026lt;\/span\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain valence shell electron pair repulsion (VSEPR) theory.\u0026amp;nbsp;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.\u0026lt;\/div\u0026gt;\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0646\u0638\u0631\u064a\u0629 \u0641\u064a\u0633\u0628\u0631","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"},{"CONT_ID":"279","CATEGORY_ID":"1","CONT_TITLE":"Structure of Phenol","CONT_SLUG":"structure-of-phenol","CONT_TITLE_AR":"Structure of Phenol","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EIn phenol, hydroxy functional group is directly attached to the sp2 hybridized carbon atom of the benzene ring. The interaction of six unhybridized 2pz orbitals of carbon atoms of the benzene ring leads to the formation of delocalized pi-electron clouds.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify the functional group present in phenol.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the charge distribution of the phenol molecule using its electrostatic potential map.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the orbital structure of phenol.\u003C\/div\u003E","CONT_DESC_AR":"In phenol hydroxy functional group is directly attached to the sp2 hybridised carbon atom of the benzene ring. The interaction of six unhybridised 2pz orbitals of carbon atoms of the benzene ring leads to the formation of delocalised pi-electron clouds.\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation, you will be able to:\u0026lt;br \/\u0026gt;\n- identify functional groups present in phenol\u0026lt;br \/\u0026gt;\n- explain the charge distribution of the phenol molecule using an electrostatic potential map\u0026lt;br \/\u0026gt;\n- explain the orbital structure of phenol","BACKING_FILE":"ss200049.apk","FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.ss200049","TOPIC_ID":"ss200049","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_SS200049.jpg","PUBLIC_BANNER_IMG":"ss200049.jpg","PUBLIC_VIDEO":"pvideo_ss200049.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/y_oKx7y2T7o","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;div\u0026gt;Overview:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;In phenol, hydroxy functional group is directly attached to the sp2 hybridized carbon atom of the benzene ring. The interaction of six unhybridized 2pz orbitals of carbon atoms of the benzene ring leads to the formation of delocalized pi-electron clouds.\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Learning Objectives:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Identify the functional group present in phenol.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain the charge distribution of the phenol molecule using its electrostatic potential map.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain the orbital structure of phenol.\u0026lt;\/div\u0026gt;\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0627\u0644\u062a\u0631\u0643\u064a\u0628 \u0627\u0644\u0628\u0646\u0627\u0626\u064a \u0644\u0644\u0641\u064a\u0646\u0648\u0644","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"},{"CONT_ID":"262","CATEGORY_ID":"1","CONT_TITLE":"Structure of Benzene","CONT_SLUG":"structure-of-benzene","CONT_TITLE_AR":"Structure of Benzene","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EThe molecular formula of benzene is C6H6. Kekul\u00e9 proposed that six carbon atoms of benzene are joined to each other by alternate single and double bonds to form a hexagonal ring. The orbital structure of benzene suggests that each carbon atom in benzene ring is sp2 hybridized.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E  \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify Kekul\u00e9 structures and the modern symbol of benzene.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the orbital structure of benzene.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the charge distribution of the benzene molecule using its electrostatic potential map.\u003C\/div\u003E","CONT_DESC_AR":"The molecular formula of benzene is C6H6 Kekule proposed that six carbon atoms of benzene are joined to each other by alternate single and double bonds to form a hexagonal ring. The orbital structure of benzene suggests that each carbon atom in benzene ring is sp2\u0026amp;nbsp;hybridised.\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation, you will be able to:\u0026lt;br \/\u0026gt;\n- identify Kekul\u0026amp;eacute; structures and the modern symbol of benzene\u0026lt;br \/\u0026gt;\n- explain the orbital structure of benzene\u0026lt;br \/\u0026gt;\n- explain the charge distribution of the benzene molecule using its electrostatic potential map","BACKING_FILE":"ss200043.apk","FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.ss200043","TOPIC_ID":"ss200043","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_SS200043.jpg","PUBLIC_BANNER_IMG":"SS200043.jpg","PUBLIC_VIDEO":"pvideo_ss200043.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/0FPZELqrUf4","DIST":null,"SHOW_ON_HOME":"Y","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;p\u0026gt;Overview:\u0026lt;\/p\u0026gt;\r\n\u0026lt;p\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/p\u0026gt;\r\n\u0026lt;p\u0026gt;The molecular formula of benzene is C6H6. Kekul\u00e9 proposed that six carbon atoms of benzene are joined to each other by alternate single and double bonds to form a hexagonal ring. 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The crystalline structure of graphite consists of layers or sheets of carbon atoms. In these layers, each carbon atom is joined to three other carbon atoms by strong covalent bonds to form hexagonal rings. Various graphite layers are held together by weak Van der Waals forces.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the layered structure of graphite.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Describe the physical properties of graphite.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Recognize the hybridization of carbon atoms in graphite.\u003C\/div\u003E","CONT_DESC_AR":"Crystal of graphite consists of layers or sheets of carbon atoms. In these layers, each carbon atom is joined to three other carbon atoms by strong covalent bonds to form hexagonal rings. Various graphite layers are held together by weak Van der Walls forces.\u0026lt;br \/\u0026gt;\n\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation, you will be able to:\u0026lt;br \/\u0026gt;\n\u0026amp;bull; explain the layered structure of graphite\u0026lt;br \/\u0026gt;\n\u0026amp;bull; describe the physical properties of graphite\u0026lt;br \/\u0026gt;\n\u0026amp;bull; recognize the hybridization of carbon atoms in graphite","BACKING_FILE":"ss200048.apk","FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.ss200048","TOPIC_ID":"ss200048","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_SS200048.jpg","PUBLIC_BANNER_IMG":"SS200048.jpg","PUBLIC_VIDEO":"pvideo_ss200048.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/gq2NqZsYfUs","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;div\u0026gt;Overview:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Graphite is a crystalline allotrope of carbon. The crystalline structure of graphite consists of layers or sheets of carbon atoms. In these layers, each carbon atom is joined to three other carbon atoms by strong covalent bonds to form hexagonal rings. Various graphite layers are held together by weak Van der Waals forces.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Learning Objectives:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain the layered structure of graphite.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Describe the physical properties of graphite.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Recognize the hybridization of carbon atoms in graphite.\u0026lt;\/div\u0026gt;\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0627\u0644\u062a\u0631\u0643\u064a\u0628 \u0627\u0644\u0628\u0646\u0627\u0626\u064a 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\r\n\u003Cdiv\u003EIn the ground state of the atoms, electrons first occupy the lowest energy orbital available to them and once the lower energy orbitals are filled, the electron can enter into higher energy orbital. \u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the energy order of the orbitals in an atom.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Arrange the electrons in different orbitals in order of increasing energy.\u003C\/div\u003E","CONT_DESC_AR":"In the ground state of the atoms, electrons first occupy the lowest energy orbital available to them and once the lower energy orbitals are filled, the electron can enter into higher energy orbital.\u0026lt;br \/\u0026gt;\n\u0026lt;br 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The four hydrogen atoms in methane molecule spread out evenly around the carbon atom, leading to the tetrahedral structure.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Write the molecular formula of methane.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the hybridization of the carbon atom in methane.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Describe the tetrahedral structure of methane.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Calculate the number of covalent bonds present in methane.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Predict the C-H bond length and the H-C-H bond angle in methane.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Describe the electrostatic potential map of methane.\u003C\/div\u003E","CONT_DESC_AR":"A methane molecule contains one carbon and four hydrogen atoms. The four hydrogen atoms in methane molecule spread out evenly around the carbon atom, leading to the tetrahedral structure.\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation you will be able to:\u0026lt;br \/\u0026gt;\n\u0026amp;bull; write the molecular formula of methane\u0026lt;br \/\u0026gt;\n\u0026amp;bull; explain the hybridisation of the carbon atom in methane\u0026lt;br \/\u0026gt;\n\u0026amp;bull; describe the tetrahedral structure of methane\u0026lt;br \/\u0026gt;\n\u0026amp;bull; calculate the number of covalent bonds present in methane\u0026lt;br \/\u0026gt;\n\u0026amp;bull; predict the C-H bond length and the H-C-H bond angle in methane\u0026lt;br \/\u0026gt;\n\u0026amp;bull; describe the electrostatic potential map of methane","BACKING_FILE":"hs200078.apk","FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200078","TOPIC_ID":"hs200078","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200078.jpg","PUBLIC_BANNER_IMG":"HS200078.jpg","PUBLIC_VIDEO":"pvideo_hs200078.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/KyIxUUo8mzg","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;div\u0026gt;Overview:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;A methane molecule contains one carbon and four hydrogen atoms. 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It is an aldehyde molecule containing two carbon atoms. Ethanal has five single bonds and one carbon-oxygen double bond.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the structure of ethanal.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify the functional group present in ethanal.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain the types of covalent bonds present in ethanal.\u003C\/div\u003E","CONT_DESC_AR":"Ethanal is commonly known as acetaldehyde. It is an aldehyde molecule containing two carbon atoms. Ethanal has five single bonds and one carbon-oxygen double bond.\u0026lt;br \/\u0026gt;\n\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation , you will be able to:\u0026lt;br \/\u0026gt;\n\u0026amp;bull; explain the structure of ethanal\u0026lt;br \/\u0026gt;\n\u0026amp;bull; identify the functional group present in ethanal\u0026lt;br \/\u0026gt;\n\u0026amp;bull; compare the molecular formula, structural formula, bond-line formula, and ball and stick model","BACKING_FILE":"hs200038.apk","FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200038","TOPIC_ID":"hs200038","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200038.jpg","PUBLIC_BANNER_IMG":"HS200038.jpg","PUBLIC_VIDEO":"pvideo_hs200038.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/OCIqGn4fCMc","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;div\u0026gt;Overview:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Ethanal is commonly known as acetaldehyde. It is an aldehyde molecule containing two carbon atoms. 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It is an alcohol molecule containing the hydoxy functional group. An ethanol molecule has eight single bonds.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify functional groups present in ethanol.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain types of covalent bonds present in ethanol.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Predict the type of hybridization of carbon and oxygen atoms in ethanol molecule.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Explain charge distribution of an ethanol molecule using its electrostatic potential map.\u003C\/div\u003E","CONT_DESC_AR":"Ethanol is commonly known as ethyl alcohol. It is an alcohol molecule containing the hydoxy functional group. An ethanol molecule has eight single bonds.\u0026lt;br \/\u0026gt;\n\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation , you will be able to:\u0026lt;br \/\u0026gt;\n\u0026amp;bull; identify functional groups present in ethanol\u0026lt;br \/\u0026gt;\n\u0026amp;bull; explain types of covalent bonds present in ethanol\u0026lt;br \/\u0026gt;\n\u0026amp;bull; predict the type of hybridization of carbon and oxygen atoms in an ethanol molecule\u0026lt;br \/\u0026gt;\n\u0026amp;bull; explain charge distribution of an ethanol molecule using its electrostatic potential map","BACKING_FILE":"hs200074.apk","FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200074","TOPIC_ID":"hs200074","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200074.jpg","PUBLIC_BANNER_IMG":"HS200074.jpg","PUBLIC_VIDEO":"pvideo_hs200074.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/NdG5hheY5ok","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;div\u0026gt;Overview:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Ethanol is commonly known as ethyl alcohol. It is an alcohol molecule containing the hydoxy functional group. An ethanol molecule has eight single bonds.\u0026amp;nbsp;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Learning Objectives:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Identify functional groups present in ethanol.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain types of covalent bonds present in ethanol.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Predict the type of hybridization of carbon and oxygen atoms in ethanol molecule.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Explain charge distribution of an ethanol molecule using its electrostatic potential map.\u0026lt;\/div\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0627\u0644\u062a\u0631\u0643\u064a\u0628 \u0627\u0644\u0628\u0646\u0627\u0626\u064a \u0644\u0644\u0625\u064a\u062b\u0627\u0646\u0648\u0644","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"},{"CONT_ID":"173","CATEGORY_ID":"1","CONT_TITLE":"Valence Electrons","CONT_SLUG":"valence-electrons","CONT_TITLE_AR":"Valence Electrons","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EValence electrons are the electrons present in the outermost shell of an atom. Since they are involved in the formation of a molecule, they decide the valency of the atom.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Identify the outermost shell of an atom.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Count the number of valence electrons present in an atom.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Predict the number of valence electrons in the atoms of groups 1, 2, and 13 to 18 using the periodic table.\u003C\/div\u003E","CONT_DESC_AR":"Valence electrons are the electrons present in the outermost shell of an atom. The number of valence electrons in the atoms of groups 1,2 and 13 to 18 equals the ones digit of the group members.\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nIn this simulation , you will be able to:\u0026lt;br \/\u0026gt;\n- identify outermost shell of an atom\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n- count valence electrons present in an atom\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n- predict the number of valence electrons in the atoms of groups 1, 2 and 13 to 18 using periodic table\u0026lt;br \/\u0026gt;\n\u0026amp;nbsp;","BACKING_FILE":"hs200070.apk","FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200070","TOPIC_ID":"hs200070","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200070.jpg","PUBLIC_BANNER_IMG":"HS200070.jpg","PUBLIC_VIDEO":"pvideo_hs200070.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/ksLodK-mJ8c","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"Overview:\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Valence electrons are the electrons present in the outermost shell of an atom. 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On moving left to right in the periodic table, the atomic radius decreases with the atomic number. Down the group, the atomic radius increases.\u003C\/div\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E \r\n\u003Cdiv\u003E- Predict the trends of atomic radii in the periodic table.\u003C\/div\u003E \r\n\u003Cdiv\u003E- Compare the atomic radii of the elements.\u003C\/div\u003E","CONT_DESC_AR":"The atomic radius of a chemical element is the distance from the center of the nucleus to the boundary of the surrounding cloud of electrons. On moving left to right in the periodic table, the atomic radius decreases with the atomic number. Down the group, the atomic radius increases in conjunction to the atomic number.\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\n\u0026lt;strong\u0026gt;Learning Objectives\u0026lt;\/strong\u0026gt;\u0026lt;br \/\u0026gt;\n\u0026lt;br \/\u0026gt;\nAfter playing the simulation, you will be able to:\u0026amp;nbsp;\u0026lt;br \/\u0026gt;\n\u0026amp;bull; calculate the valency of elements\u0026lt;br \/\u0026gt;\n\u0026amp;bull; predict the placement of elements in the periodic table using valency","BACKING_FILE":null,"FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":"","MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200012","TOPIC_ID":"hs200012","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200012.jpg","PUBLIC_BANNER_IMG":"hs200012.jpg","PUBLIC_VIDEO":"pvideo_hs200012.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/InBee94xfgk","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"0000-00-00 00:00:00","CREATED_BY":"1","UPDATED_ON":"2017-12-29 10:51:37","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"\u0026lt;div\u0026gt;Overview:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;The atomic radius of a chemical element is the distance from the center of the nucleus to the outmost boundary of the surrounding cloud of electrons. On moving left to right in the periodic table, the atomic radius decreases with the atomic number. Down the group, the atomic radius increases.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;Learning Objectives:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;br\u0026gt;\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;\u0026lt;div\u0026gt;After completing this module, you will be able to:\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Predict the trends of atomic radii in the periodic table.\u0026lt;\/div\u0026gt;\u0026lt;div\u0026gt;- Compare the atomic radii of the elements.\u0026lt;\/div\u0026gt;\u0026lt;\/div\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"\u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a: \u0646\u0635\u0641 \u0627\u0644\u0642\u0637\u0631 \u0627\u0644\u0630\u0631\u064a","ADMSUBJECT_ID":"704","ADMCOURSE_ID":"147","DISPLAY_NAME":"Bahrain - Grade 11 - Chemistry","DISPLAY_NAME_AR":"Bahrain - Grade 11 - Chemistry","SUBJECT_NAME":"Chemistry","SUBJECT_NAME_AR":"Chemistry","SUBJECT_DESC":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.\u003Cbr\u003E","SUBJECT_DESC_AR":"\u062a\u0634\u0631\u062d \u0648\u064e\u062d\u064e\u062f\u0627\u062a \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0644\u0644\u0635\u0641 \u0627\u0644\u062d\u0627\u062f\u064a \u0639\u0634\u0631 \u062a\u0637\u0648\u0631 \u0627\u0644\u062c\u062f\u0648\u0644 \u0627\u0644\u062f\u0648\u0631\u064a\u060c \u0648\u062a\u0642\u0648\u062f \u062a\u0644\u0643 \u0627\u0644\u062a\u0637\u0648\u0631\u0627\u062a \u0625\u0644\u0649 \u0646\u0645\u0648\u0630\u062c \u0628\u0648\u0631 \u0627\u0644\u0630\u0631\u064a\u060c \u0648\u0627\u0644\u0646\u0645\u0648\u0630\u062c \u0627\u0644\u0645\u064a\u0643\u0627\u0646\u064a\u0643\u064a \u0627\u0644\u0643\u0645\u064a \u0644\u0644\u0630\u0631\u0629. \u062a\u0646\u0627\u0642\u0634 \u0643\u0630\u0644\u0643 \u0627\u0644\u0627\u062a\u0632\u0627\u0646\u060c \u0648\u0627\u0644\u062a\u0631\u0627\u0628\u0637 \u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0626\u064a\u060c \u0627\u0644\u062a\u0631\u0643\u064a\u0628\u0627\u062a \u0627\u0644\u062c\u0632\u064a\u0626\u064a\u0629 \u0648\u0627\u0644\u0643\u064a\u0645\u064a\u0627\u0621 \u0627\u0644\u0639\u0636\u0648\u064a\u0629.","SUBJECT_IMG":"bahrain_grade11_chemistry.jpg","SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"Grade 11","COUNTRY_ID":"280","SHORT_NAME":"Bahrain","DOMAIN_NAME":"STEM"}],"levelObject":["Compounds","Solubility","Electrical Conductivity","Miscible"],"contData":{"CONT_ID":"568","CATEGORY_ID":"1","CONT_TITLE":"Ionic Compounds","CONT_SLUG":"ionic-compounds","CONT_TITLE_AR":"","CONT_DESC":"\u003Ch3\u003EOverview:\u003C\/h3\u003E\r\n \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E\r\n \r\n\u003Cdiv\u003EIonic compounds consist of positively charged cations and negatively charged anions. Ionic compounds are solid at room temperature. They are brittle in nature. These compounds are highly soluble in water and conduct electricity in aqueous state only.\u003C\/div\u003E\r\n \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E\r\n \r\n\u003Ch3\u003ELearning Objectives:\u003C\/h3\u003E\r\n \r\n\u003Cdiv\u003E \r\n \u003Cbr\u003E \r\n\u003C\/div\u003E\r\n \r\n\u003Cdiv\u003EAfter completing this module, you will be able to:\u003C\/div\u003E\r\n \r\n\u003Cdiv\u003E- Identify ionic compounds.\u003C\/div\u003E\r\n \r\n\u003Cdiv\u003E- Demonstrate the solubility of ionic compounds.\u003C\/div\u003E\r\n \r\n\u003Cdiv\u003E- Examine the electrical conductivity of ionic compounds.\u003C\/div\u003E","CONT_DESC_AR":"","BACKING_FILE":null,"FILE_UID":null,"SCORM_COURSE_ID":null,"CONT_SRC":null,"MOD_FILES":null,"FOLDER_NAME":null,"CONTTYPE_ID":"9","ANDROID_PKG":"com.umety.vr.hs200314","TOPIC_ID":"hs200314","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_HS200314.jpg","PUBLIC_BANNER_IMG":"HS200314.jpg","PUBLIC_VIDEO":"pvideo_hs200314.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/rqIx2k9cru4","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"2017-10-06 05:54:22","CREATED_BY":"0","UPDATED_ON":"2024-10-08 09:57:40","UPDATED_BY":"2","CONT_ORDER":"0","X_ROTATION":null,"Y_ROTATION":null,"Z_ROTATION":null,"BG_COLOR":"0x000000","X_POSITION":null,"Y_POSITION":null,"Z_POSITION":null,"TEMP_DESC":"Overview:\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Ionic compounds consist of positively charged cations and negatively charged anions. Ionic compounds are solid at room temperature. They are brittle in nature. These compounds are highly soluble in water and conduct electricity in aqueous state only.\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;Learning objectives\u0026lt;br\u0026gt;\u0026lt;br\u0026gt;After completing this module, you will be able to:\u0026lt;br\u0026gt;- Identify ionic compounds.\u0026lt;br\u0026gt;- Demonstrate the solubility of ionic compounds.\u0026lt;br\u0026gt;- Examine the electrical conductivity of ionic compounds.\u0026lt;br\u0026gt;","IS_ANALYTICS":"Y","VR_ENABLE":"Y","VR_SESSION_ENABLE":"Y","YOUTUBE_URL":null,"CONT_TYPE":"VR Module","CAT_NAME":"Ionic compounds","DISPLAY_NAME":"NGSS New - Middle School - Physical Science","DISPLAY_NAME_AR":"NGSS New - Middle School - Physical Science","SUBJECT_IMG":"569.jpg","ADMSUBJECT_ID":"569","SUBJECT_NAME":"Physical Science","SUBJECT_NAME_AR":"Physical Science","ADMCOURSE_ID":"191","COURSE_NAME":"Middle School","COUNTRY_ID":"287","STANDARD_ID":"287","SHORT_NAME":"NGSS","LANG_ID":null,"LOCALE_TITLE":null,"LOCALE_DESC":null,"DIR":null,"LANG_NAME":null,"DOMAIN_NAME":"STEM","DOMAIN_DESC":"STEM"},"checkLang":["English - US","\u4e2d\u6587","\u0639\u0631\u0628\u064a","Espa\u00f1ol","Polski","Ti\u1ebfng Vi\u1ec7t","\ud55c\uad6d\uc5b4"],"devices":["UmetyVR","WebXR"]}