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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":"2019-05-03 00:00:00","CREATED_BY":"1","UPDATED_ON":"2020-06-25 10:15:57","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":"Application of VSEPR theory","ADMSUBJECT_ID":"1181","ADMCOURSE_ID":"347","DISPLAY_NAME":"","DISPLAY_NAME_AR":"","SUBJECT_NAME":"Chemical Bonding \u0026 Structures","SUBJECT_NAME_AR":"","SUBJECT_DESC":"Description","SUBJECT_DESC_AR":"","SUBJECT_IMG":null,"SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"High School Chemistry","COUNTRY_ID":"335","SHORT_NAME":"UCL-New","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. The number of atoms bonded to a central atom combined with the number of pairs of its non-bonding valence electrons is called its steric number.\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; explain Valence shell electron pair repulsion (VSEPR) theory\u0026lt;br \/\u0026gt;\n\u0026amp;bull; predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms","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.ss200034","TOPIC_ID":"ss200034","IS_PUBLISH":"Y","IS_PUBLIC":"Y","CONT_PRICE":null,"PUBLIC_IMG":"thumb_SS200034.jpg","PUBLIC_BANNER_IMG":"SS200034.jpg","PUBLIC_VIDEO":"pvideo_ss200034.mp4","PUBLIC_VIDEO_URL":"https:\/\/youtu.be\/RVz4Vp1j4nQ","DIST":null,"SHOW_ON_HOME":"N","CONTROLLER_REQUIRED":"Y","DOMAIN":"3","CONCEPT":"0","STATUS":"A","EXPIRY_DAYS":null,"CREATED_ON":"2019-05-03 00:00:00","CREATED_BY":"1","UPDATED_ON":"2020-06-25 10:15:57","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 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.\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":"VSEPR Theory","ADMSUBJECT_ID":"1181","ADMCOURSE_ID":"347","DISPLAY_NAME":"","DISPLAY_NAME_AR":"","SUBJECT_NAME":"Chemical Bonding \u0026 Structures","SUBJECT_NAME_AR":"","SUBJECT_DESC":"Description","SUBJECT_DESC_AR":"","SUBJECT_IMG":null,"SUBJECT_BANNER_IMG":null,"SUBJECT_PRICE":null,"IS_FEATURED":"N","COURSE_NAME":"High School Chemistry","COUNTRY_ID":"335","SHORT_NAME":"UCL-New","DOMAIN_NAME":"STEM"}]}