{"id":12798,"date":"2020-06-28T09:56:40","date_gmt":"2020-06-28T09:56:40","guid":{"rendered":"https:\/\/chemistryscore.com\/?post_type=glossary&#038;p=12798"},"modified":"2020-06-28T09:56:40","modified_gmt":"2020-06-28T09:56:40","slug":"trigonal-planar","status":"publish","type":"glossary","link":"https:\/\/chemistryscore.com\/definition\/trigonal-planar\/","title":{"rendered":"Trigonal Planar"},"content":{"rendered":"<h2>Trigonal Planar Definition:<\/h2>\n<p>The\u00a0<b>trigonal planar<\/b>\u00a0geometry is a type of atomic arrangement arising from the sp2 hybridization. It adopted by an atom that has a\u00a0<a class=\"glossaryLink \" style=\"box-sizing: border-box; margin: 0px; padding: 0px; border-width: 0px 0px 1px; border-color: initial; border-image: initial; outline: 0px; font-variant: inherit; font-stretch: inherit; line-height: inherit; vertical-align: baseline; font-family: inherit; font-size: 16px; font-style: inherit; font-weight: inherit; background-color: transparent; color: #00a8e2; text-decoration: none !important; transition: all 0.3s ease 0s; box-shadow: none; border-style: initial initial dotted initial;\" href=\"https:\/\/chemistryscore.com\/definition\/steric-number\/\" data-cmtooltip=\"&lt;h2&gt;Steric Number Definition:&lt;\/h2&gt;\nThe\u00a0&lt;b&gt;Steric Number&lt;\/b&gt;\u00a0for an atom is the total number of sigma bonds formed and the number of\u00a0&lt;a class=&quot;glossaryLink &quot; style=&quot;box-sizing: border-box; margin: 0px; padding: 0px; border-width: 0px 0px 1px; border-color: initial; border-image: initial; outline: 0px; font-variant: inherit; font-stretch: inherit; line-height: inherit; vertical-align: baseline; font-family: inherit; font-size: 16px; font-style: inherit; font-weight: inherit; background-color: transparent; color: #00a8e2; text-decoration: none !important; transition: all 0.3s ease 0s; box-shadow: none; border-style: initial initial dotted initial;&quot; href=&quot;https:\/\/chemistryscore.com\/definition\/lone-pair\/&quot; data-cmtooltip=&quot;&lt;h2&gt;Lone Pair Definition:&lt;\/h2&gt;\nA\u00a0&lt;b&gt;Lone Pair\u00a0&lt;\/b&gt;or non-bonding pair is one pair of unshared or nonbinding electrons on an atom.\n&lt;h2&gt;Lone Pair Explained:&lt;\/h2&gt;\nAn easy way to identify the lone pair electrons is by examining the lewis dot structure of the atom. The structure shows the total number of valence electrons that comprise both the bonding electrons as well as the non-binding\/lone pair electrons.&lt;br \/&gt;Examples \u2013&lt;br \/&gt;&lt;img class=&quot;aligncenter size-full wp-image-6944&quot; src=&quot;https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/Lone-Pair-1024x218.png&quot; sizes=&quot;(max-width: 1024px) 100vw, 1024px&quot; srcset=&quot;https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/Lone-Pair-1024x218.png 1024w, https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/Lone-Pair-1024x218-300x64.png 300w, https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/Lone-Pair-1024x218-768x164.png 768w&quot; alt=&quot;&quot; width=&quot;1024&quot; height=&quot;218&quot; \/&gt;\n&lt;em&gt;(However, note that not all nonbonding pairs of electrons are considered to be lone pairs. Examples of which include transition metals wherein the non-bonding pairs do not influence molecular geometry. This concept will be further explained in the valence shell electron pair repulsion theory (VSEPR theory) and the inert pair effect that explains the shapes of molecules.)&lt;\/em&gt;&quot;&gt;lone pair&lt;\/a&gt;\u00a0electrons on the respective atom.\n&lt;h2&gt;Steric Number Explained:&lt;\/h2&gt;\nThe steric number is an important concept covered under the VSEPR theory. The number is calculated mainly for the central atom of the compound which is then used to predict the geometry of the compound. In other words, the number indicated the total number of bonding and non-bonding electrons of the atom that is repelling each other. This repulsion causes the electron pairs to arrange themselves in a particular geometry.&lt;br \/&gt;See, VSEPR Theory, Trigonal Planar, Trigonal Pyramidal, Tetrahedral.&lt;br \/&gt;Example \u2013\n&lt;img class=&quot;aligncenter size-full wp-image-7857&quot; src=&quot;https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/stericnumber-1024x345.png&quot; sizes=&quot;(max-width: 1024px) 100vw, 1024px&quot; srcset=&quot;https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/stericnumber-1024x345.png 1024w, https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/stericnumber-1024x345-300x101.png 300w, https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/stericnumber-1024x345-768x259.png 768w&quot; alt=&quot;&quot; width=&quot;1024&quot; height=&quot;345&quot; \/&gt;\nRecall, a double bond has one sigma and one pi while a triple bond has one sigma and two pi bonds.\">steric number<\/a>\u00a0of 3 and all 3 bonds formed by the central atom lie in one plane and are separated by 120\u00b0.<\/p>\n<h2>Trigonal Planar Explained:<\/h2>\n<p>Example \u2013 BF<sub>3<\/sub><\/p>\n<p><img fetchpriority=\"high\" decoding=\"async\" class=\"aligncenter size-full wp-image-8083\" src=\"https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/trigonalplanar-768x408.png\" sizes=\"(max-width: 768px) 100vw, 768px\" srcset=\"https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/trigonalplanar-768x408.png 768w, https:\/\/chemistryscore.com\/wp-content\/uploads\/2019\/11\/trigonalplanar-768x408-300x159.png 300w\" alt=\"\" width=\"768\" height=\"408\" \/><\/p>\n","protected":false},"excerpt":{"rendered":"<p>Trigonal Planar Definition: The\u00a0trigonal planar\u00a0geometry is a type of atomic arrangement arising from the sp2 hybridization. It adopted by an atom that has a\u00a0steric number\u00a0of 3 and all 3 bonds formed by the central atom lie in one plane and are separated by 120\u00b0. Trigonal Planar Explained: Example \u2013 BF3<\/p>\n","protected":false},"author":5,"featured_media":0,"menu_order":0,"template":"","meta":{"ocean_post_layout":"","ocean_both_sidebars_style":"","ocean_both_sidebars_content_width":0,"ocean_both_sidebars_sidebars_width":0,"ocean_sidebar":"","ocean_second_sidebar":"","ocean_disable_margins":"enable","ocean_add_body_class":"","ocean_shortcode_before_top_bar":"","ocean_shortcode_after_top_bar":"","ocean_shortcode_before_header":"","ocean_shortcode_after_header":"","ocean_has_shortcode":"","ocean_shortcode_after_title":"","ocean_shortcode_before_footer_widgets":"","ocean_shortcode_after_footer_widgets":"","ocean_shortcode_before_footer_bottom":"","ocean_shortcode_after_footer_bottom":"","ocean_display_top_bar":"default","ocean_display_header":"default","ocean_header_style":"","ocean_center_header_left_menu":"","ocean_custom_header_template":"","ocean_custom_logo":0,"ocean_custom_retina_logo":0,"ocean_custom_logo_max_width":0,"ocean_custom_logo_tablet_max_width":0,"ocean_custom_logo_mobile_max_width":0,"ocean_custom_logo_max_height":0,"ocean_custom_logo_tablet_max_height":0,"ocean_custom_logo_mobile_max_height":0,"ocean_header_custom_menu":"","ocean_menu_typo_font_family":"","ocean_menu_typo_font_subset":"","ocean_menu_typo_font_size":0,"ocean_menu_typo_font_size_tablet":0,"ocean_menu_typo_font_size_mobile":0,"ocean_menu_typo_font_size_unit":"px","ocean_menu_typo_font_weight":"","ocean_menu_typo_font_weight_tablet":"","ocean_menu_typo_font_weight_mobile":"","ocean_menu_typo_transform":"","ocean_menu_typo_transform_tablet":"","ocean_menu_typo_transform_mobile":"","ocean_menu_typo_line_height":0,"ocean_menu_typo_line_height_tablet":0,"ocean_menu_typo_line_height_mobile":0,"ocean_menu_typo_line_height_unit":"","ocean_menu_typo_spacing":0,"ocean_menu_typo_spacing_tablet":0,"ocean_menu_typo_spacing_mobile":0,"ocean_menu_typo_spacing_unit":"","ocean_menu_link_color":"","ocean_menu_link_color_hover":"","ocean_menu_link_color_active":"","ocean_menu_link_background":"","ocean_menu_link_hover_background":"","ocean_menu_link_active_background":"","ocean_menu_social_links_bg":"","ocean_menu_social_hover_links_bg":"","ocean_menu_social_links_color":"","ocean_menu_social_hover_links_color":"","ocean_disable_title":"default","ocean_disable_heading":"default","ocean_post_title":"","ocean_post_subheading":"","ocean_post_title_style":"","ocean_post_title_background_color":"","ocean_post_title_background":0,"ocean_post_title_bg_image_position":"","ocean_post_title_bg_image_attachment":"","ocean_post_title_bg_image_repeat":"","ocean_post_title_bg_image_size":"","ocean_post_title_height":0,"ocean_post_title_bg_overlay":0.5,"ocean_post_title_bg_overlay_color":"","ocean_disable_breadcrumbs":"default","ocean_breadcrumbs_color":"","ocean_breadcrumbs_separator_color":"","ocean_breadcrumbs_links_color":"","ocean_breadcrumbs_links_hover_color":"","ocean_display_footer_widgets":"default","ocean_display_footer_bottom":"default","ocean_custom_footer_template":"","footnotes":""},"jetpack_sharing_enabled":true,"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v14.9 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Trigonal Planar - Learn Chemistry Online | ChemistryScore<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/chemistryscore.com\/definition\/trigonal-planar\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Trigonal Planar - Learn Chemistry Online | ChemistryScore\" \/>\n<meta property=\"og:description\" content=\"Trigonal Planar Definition: The\u00a0trigonal planar\u00a0geometry is a type of atomic arrangement arising from the sp2 hybridization. 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