To draw the Lewis structure for PH2Cl (phosphine chloride), follow these steps:<\/p>\n\n\n\n
Step 1: Count the Total Number of Valence Electrons<\/h3>\n\n\n\n\n- Phosphorus (P) is in group 15, so it has 5 valence electrons.<\/li>\n\n\n\n
- Hydrogen (H) is in group 1, so each H atom contributes 1 electron. There are 2 hydrogens, so they contribute 2 electrons in total.<\/li>\n\n\n\n
- Chlorine (Cl) is in group 17, so it has 7 valence electrons.<\/li>\n<\/ul>\n\n\n\n
Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.<\/p>\n\n\n\n
Step 2: Arrange the Atoms<\/h3>\n\n\n\n\n- Phosphorus (P) is the central atom because it is less electronegative than chlorine (Cl) and can form more bonds.<\/li>\n\n\n\n
- Place the two hydrogens (H) and the chlorine (Cl) atoms around phosphorus.<\/li>\n<\/ul>\n\n\n\n
Step 3: Connect Atoms with Single Bonds<\/h3>\n\n\n\n\n- Place a single bond (one shared pair of electrons) between phosphorus and each of the hydrogen atoms, and another single bond between phosphorus and chlorine. This uses 6 electrons (3 bonds \u00d7 2 electrons per bond).<\/li>\n<\/ul>\n\n\n\n
Step 4: Distribute Remaining Electrons<\/h3>\n\n\n\n\n- After forming the 3 single bonds, there are 8 electrons remaining (14 total – 6 used in bonding).<\/li>\n\n\n\n
- These remaining electrons should be placed as lone pairs around the atoms. Since chlorine is more electronegative, it will take 3 lone pairs (6 electrons). This satisfies chlorine\u2019s octet.<\/li>\n\n\n\n
- The remaining 2 electrons go as a lone pair on phosphorus.<\/li>\n<\/ul>\n\n\n\n
Step 5: Check for Octets<\/h3>\n\n\n\n\n- Phosphorus has 3 bonds (6 electrons) and 1 lone pair (2 electrons), giving it 8 electrons around it, fulfilling the octet rule.<\/li>\n\n\n\n
- Hydrogen atoms are each bonded to phosphorus with a single bond, giving each hydrogen 2 electrons, which satisfies the duet rule for hydrogen.<\/li>\n\n\n\n
- Chlorine has 3 lone pairs (6 electrons) and 1 bond (2 electrons), giving it 8 electrons, fulfilling the octet rule for chlorine.<\/li>\n<\/ul>\n\n\n\n
Final Lewis Structure:<\/h3>\n\n\n\n
The final structure for PH2Cl is:<\/p>\n\n\n\n
H
|
H - P - Cl
|
lone pair on P
<\/code><\/pre>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- Phosphorus (P) forms 3 bonds: one with each hydrogen and one with chlorine.<\/li>\n\n\n\n
- Chlorine (Cl) has 3 lone pairs and 1 bond to phosphorus.<\/li>\n\n\n\n
- Hydrogen (H) atoms each form a single bond with phosphorus and have no lone pairs.<\/li>\n\n\n\n
- The structure satisfies the octet rule for chlorine and phosphorus and the duet rule for hydrogen.<\/li>\n<\/ul>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-833.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Lewis structure for PH2Cl The Correct Answer and Explanation is: To draw the Lewis structure for PH2Cl (phosphine chloride), follow these steps: Step 1: Count the Total Number of Valence Electrons Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons. Step 2: […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-246282","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=246282"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246282"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246282"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.<\/p>\n\n\n\n
Step 2: Arrange the Atoms<\/h3>\n\n\n\n\n- Phosphorus (P) is the central atom because it is less electronegative than chlorine (Cl) and can form more bonds.<\/li>\n\n\n\n
- Place the two hydrogens (H) and the chlorine (Cl) atoms around phosphorus.<\/li>\n<\/ul>\n\n\n\n
Step 3: Connect Atoms with Single Bonds<\/h3>\n\n\n\n\n- Place a single bond (one shared pair of electrons) between phosphorus and each of the hydrogen atoms, and another single bond between phosphorus and chlorine. This uses 6 electrons (3 bonds \u00d7 2 electrons per bond).<\/li>\n<\/ul>\n\n\n\n
Step 4: Distribute Remaining Electrons<\/h3>\n\n\n\n\n- After forming the 3 single bonds, there are 8 electrons remaining (14 total – 6 used in bonding).<\/li>\n\n\n\n
- These remaining electrons should be placed as lone pairs around the atoms. Since chlorine is more electronegative, it will take 3 lone pairs (6 electrons). This satisfies chlorine\u2019s octet.<\/li>\n\n\n\n
- The remaining 2 electrons go as a lone pair on phosphorus.<\/li>\n<\/ul>\n\n\n\n
Step 5: Check for Octets<\/h3>\n\n\n\n\n- Phosphorus has 3 bonds (6 electrons) and 1 lone pair (2 electrons), giving it 8 electrons around it, fulfilling the octet rule.<\/li>\n\n\n\n
- Hydrogen atoms are each bonded to phosphorus with a single bond, giving each hydrogen 2 electrons, which satisfies the duet rule for hydrogen.<\/li>\n\n\n\n
- Chlorine has 3 lone pairs (6 electrons) and 1 bond (2 electrons), giving it 8 electrons, fulfilling the octet rule for chlorine.<\/li>\n<\/ul>\n\n\n\n
Final Lewis Structure:<\/h3>\n\n\n\n
The final structure for PH2Cl is:<\/p>\n\n\n\n
H
|
H - P - Cl
|
lone pair on P
<\/code><\/pre>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- Phosphorus (P) forms 3 bonds: one with each hydrogen and one with chlorine.<\/li>\n\n\n\n
- Chlorine (Cl) has 3 lone pairs and 1 bond to phosphorus.<\/li>\n\n\n\n
- Hydrogen (H) atoms each form a single bond with phosphorus and have no lone pairs.<\/li>\n\n\n\n
- The structure satisfies the octet rule for chlorine and phosphorus and the duet rule for hydrogen.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Lewis structure for PH2Cl The Correct Answer and Explanation is: To draw the Lewis structure for PH2Cl (phosphine chloride), follow these steps: Step 1: Count the Total Number of Valence Electrons Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons. Step 2: […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-246282","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=246282"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246282"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246282"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Step 3: Connect Atoms with Single Bonds<\/h3>\n\n\n\n\n- Place a single bond (one shared pair of electrons) between phosphorus and each of the hydrogen atoms, and another single bond between phosphorus and chlorine. This uses 6 electrons (3 bonds \u00d7 2 electrons per bond).<\/li>\n<\/ul>\n\n\n\n
Step 4: Distribute Remaining Electrons<\/h3>\n\n\n\n\n- After forming the 3 single bonds, there are 8 electrons remaining (14 total – 6 used in bonding).<\/li>\n\n\n\n
- These remaining electrons should be placed as lone pairs around the atoms. Since chlorine is more electronegative, it will take 3 lone pairs (6 electrons). This satisfies chlorine\u2019s octet.<\/li>\n\n\n\n
- The remaining 2 electrons go as a lone pair on phosphorus.<\/li>\n<\/ul>\n\n\n\n
Step 5: Check for Octets<\/h3>\n\n\n\n\n- Phosphorus has 3 bonds (6 electrons) and 1 lone pair (2 electrons), giving it 8 electrons around it, fulfilling the octet rule.<\/li>\n\n\n\n
- Hydrogen atoms are each bonded to phosphorus with a single bond, giving each hydrogen 2 electrons, which satisfies the duet rule for hydrogen.<\/li>\n\n\n\n
- Chlorine has 3 lone pairs (6 electrons) and 1 bond (2 electrons), giving it 8 electrons, fulfilling the octet rule for chlorine.<\/li>\n<\/ul>\n\n\n\n
Final Lewis Structure:<\/h3>\n\n\n\n
The final structure for PH2Cl is:<\/p>\n\n\n\n
H
|
H - P - Cl
|
lone pair on P
<\/code><\/pre>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- Phosphorus (P) forms 3 bonds: one with each hydrogen and one with chlorine.<\/li>\n\n\n\n
- Chlorine (Cl) has 3 lone pairs and 1 bond to phosphorus.<\/li>\n\n\n\n
- Hydrogen (H) atoms each form a single bond with phosphorus and have no lone pairs.<\/li>\n\n\n\n
- The structure satisfies the octet rule for chlorine and phosphorus and the duet rule for hydrogen.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Lewis structure for PH2Cl The Correct Answer and Explanation is: To draw the Lewis structure for PH2Cl (phosphine chloride), follow these steps: Step 1: Count the Total Number of Valence Electrons Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons. Step 2: […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-246282","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=246282"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246282"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246282"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Step 4: Distribute Remaining Electrons<\/h3>\n\n\n\n\n- After forming the 3 single bonds, there are 8 electrons remaining (14 total – 6 used in bonding).<\/li>\n\n\n\n
- These remaining electrons should be placed as lone pairs around the atoms. Since chlorine is more electronegative, it will take 3 lone pairs (6 electrons). This satisfies chlorine\u2019s octet.<\/li>\n\n\n\n
- The remaining 2 electrons go as a lone pair on phosphorus.<\/li>\n<\/ul>\n\n\n\n
Step 5: Check for Octets<\/h3>\n\n\n\n\n- Phosphorus has 3 bonds (6 electrons) and 1 lone pair (2 electrons), giving it 8 electrons around it, fulfilling the octet rule.<\/li>\n\n\n\n
- Hydrogen atoms are each bonded to phosphorus with a single bond, giving each hydrogen 2 electrons, which satisfies the duet rule for hydrogen.<\/li>\n\n\n\n
- Chlorine has 3 lone pairs (6 electrons) and 1 bond (2 electrons), giving it 8 electrons, fulfilling the octet rule for chlorine.<\/li>\n<\/ul>\n\n\n\n
Final Lewis Structure:<\/h3>\n\n\n\n
The final structure for PH2Cl is:<\/p>\n\n\n\n
H
|
H - P - Cl
|
lone pair on P
<\/code><\/pre>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- Phosphorus (P) forms 3 bonds: one with each hydrogen and one with chlorine.<\/li>\n\n\n\n
- Chlorine (Cl) has 3 lone pairs and 1 bond to phosphorus.<\/li>\n\n\n\n
- Hydrogen (H) atoms each form a single bond with phosphorus and have no lone pairs.<\/li>\n\n\n\n
- The structure satisfies the octet rule for chlorine and phosphorus and the duet rule for hydrogen.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Lewis structure for PH2Cl The Correct Answer and Explanation is: To draw the Lewis structure for PH2Cl (phosphine chloride), follow these steps: Step 1: Count the Total Number of Valence Electrons Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons. Step 2: […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-246282","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=246282"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246282"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246282"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Step 5: Check for Octets<\/h3>\n\n\n\n\n- Phosphorus has 3 bonds (6 electrons) and 1 lone pair (2 electrons), giving it 8 electrons around it, fulfilling the octet rule.<\/li>\n\n\n\n
- Hydrogen atoms are each bonded to phosphorus with a single bond, giving each hydrogen 2 electrons, which satisfies the duet rule for hydrogen.<\/li>\n\n\n\n
- Chlorine has 3 lone pairs (6 electrons) and 1 bond (2 electrons), giving it 8 electrons, fulfilling the octet rule for chlorine.<\/li>\n<\/ul>\n\n\n\n
Final Lewis Structure:<\/h3>\n\n\n\n
The final structure for PH2Cl is:<\/p>\n\n\n\n
H
|
H - P - Cl
|
lone pair on P
<\/code><\/pre>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- Phosphorus (P) forms 3 bonds: one with each hydrogen and one with chlorine.<\/li>\n\n\n\n
- Chlorine (Cl) has 3 lone pairs and 1 bond to phosphorus.<\/li>\n\n\n\n
- Hydrogen (H) atoms each form a single bond with phosphorus and have no lone pairs.<\/li>\n\n\n\n
- The structure satisfies the octet rule for chlorine and phosphorus and the duet rule for hydrogen.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Lewis structure for PH2Cl The Correct Answer and Explanation is: To draw the Lewis structure for PH2Cl (phosphine chloride), follow these steps: Step 1: Count the Total Number of Valence Electrons Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons. Step 2: […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-246282","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=246282"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246282"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246282"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Final Lewis Structure:<\/h3>\n\n\n\n
The final structure for PH2Cl is:<\/p>\n\n\n\n
H
|
H - P - Cl
|
lone pair on P
<\/code><\/pre>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- Phosphorus (P) forms 3 bonds: one with each hydrogen and one with chlorine.<\/li>\n\n\n\n
- Chlorine (Cl) has 3 lone pairs and 1 bond to phosphorus.<\/li>\n\n\n\n
- Hydrogen (H) atoms each form a single bond with phosphorus and have no lone pairs.<\/li>\n\n\n\n
- The structure satisfies the octet rule for chlorine and phosphorus and the duet rule for hydrogen.<\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Lewis structure for PH2Cl The Correct Answer and Explanation is: To draw the Lewis structure for PH2Cl (phosphine chloride), follow these steps: Step 1: Count the Total Number of Valence Electrons Thus, the total number of valence electrons is:5(P)+2\u00d71(H)+7(Cl)=14 valence electrons.5 (P) + 2 \\times 1 (H) + 7 (Cl) = 14 \\text{ valence electrons.}5(P)+2\u00d71(H)+7(Cl)=14 valence electrons. Step 2: […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-246282","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=246282"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246282\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246282"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246282"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}