{"id":222261,"date":"2025-05-31T07:32:30","date_gmt":"2025-05-31T07:32:30","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=222261"},"modified":"2025-05-31T07:32:32","modified_gmt":"2025-05-31T07:32:32","slug":"for-each-of-the-following","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/31\/for-each-of-the-following\/","title":{"rendered":"For each of the following"},"content":{"rendered":"\n

For each of the following,<\/p>\n\n\n\n

a. Draw the lewis structure<\/p>\n\n\n\n

b. Indicate the molecular geometry<\/p>\n\n\n\n

c. Indicate the bond angles<\/p>\n\n\n\n

PCI3
IBr4-
SeF4
NH2-
SCN-
SnCl5-<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

1. PCl\u2083<\/strong><\/h3>\n\n\n\n

a. Lewis Structure:<\/strong>
P is the central atom with three Cl atoms bonded and one lone pair.<\/p>\n\n\n\n

   ..\n  :Cl:\n   |\n:Cl\u2013P\u2013Cl:\n   ..\n<\/code><\/pre>\n\n\n\n
b. Molecular Geometry:<\/strong> Trigonal pyramidal
c. Bond Angles:<\/strong> ~107\u00b0<\/p>\n\n\n\n
\n\n\n\n
2. IBr\u2084\u207b<\/strong><\/h3>\n\n\n\n
a. Lewis Structure:<\/strong>
Iodine is central with four Br atoms and two lone pairs.<\/p>\n\n\n\n
Br\u2013I\u2013Br  \n |     |  \nBr     Br  \n(with 2 lone pairs on I)\n\n<\/code><\/pre>\n\n\n\n
b. Molecular Geometry:<\/strong> Square planar
c. Bond Angles:<\/strong> 90\u00b0<\/p>\n\n\n\n
\n\n\n\n
3. SeF\u2084<\/strong><\/h3>\n\n\n\n
a. Lewis Structure:<\/strong>
Se has four bonded F atoms and one lone pair.<\/p>\n\n\n\n
    F\n     |\nF \u2013 Se \u2013 F  \n     |\n     F  \n(one lone pair on Se)\n\n<\/code><\/pre>\n\n\n\n
b. Molecular Geometry:<\/strong> See-saw
c. Bond Angles:<\/strong> ~101\u00b0 (equatorial), ~173\u00b0 (axial)<\/p>\n\n\n\n
\n\n\n\n
4. NH\u2082\u207b<\/strong><\/h3>\n\n\n\n
a. Lewis Structure:<\/strong>
N is central with two H atoms and two lone pairs.<\/p>\n\n\n\n
H\u2013N\u207b\u2013H  \n   ..\n   ..\n<\/code><\/pre>\n\n\n\n
b. Molecular Geometry:<\/strong> Bent
c. Bond Angles:<\/strong> ~104\u00b0<\/p>\n\n\n\n
\n\n\n\n
5. SCN\u207b<\/strong> (thiocyanate ion)<\/h3>\n\n\n\n
a. Lewis Structure:<\/strong>
Resonance structures exist:
S=C=N\u207b or \u207bS\u2013C\u2261N
(Linear structure overall)<\/p>\n\n\n\n
b. Molecular Geometry:<\/strong> Linear
c. Bond Angles:<\/strong> 180\u00b0<\/p>\n\n\n\n
\n\n\n\n
6. SnCl\u2085\u207b<\/strong><\/h3>\n\n\n\n
a. Lewis Structure:<\/strong>
Sn is central with five Cl atoms and one extra electron (negative charge).<\/p>\n\n\n\n
Trigonal bipyramidal with 5 Cl atoms around Sn\n<\/code><\/pre>\n\n\n\n
b. Molecular Geometry:<\/strong> Trigonal bipyramidal
c. Bond Angles:<\/strong> 90\u00b0, 120\u00b0, 180\u00b0<\/p>\n\n\n\n
\n\n\n\n
Explanation:<\/strong><\/h3>\n\n\n\n
The geometry and structure of a molecule depend on the Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>, which states that electron pairs around a central atom repel each other and arrange themselves to minimize this repulsion.<\/p>\n\n\n\n
PCl\u2083<\/strong> has three bonded atoms and one lone pair on phosphorus, making it AX\u2083E<\/strong> and resulting in a trigonal pyramidal<\/strong> shape, similar to ammonia, with bond angles slightly less than the tetrahedral angle due to lone pair repulsion.<\/p>\n\n\n\n
IBr\u2084\u207b<\/strong> has four bonded atoms and two lone pairs on iodine, giving an AX\u2084E\u2082<\/strong> system. The lone pairs occupy opposite positions in an octahedral arrangement, resulting in a square planar<\/strong> geometry with 90\u00b0 bond angles.<\/p>\n\n\n\n
SeF\u2084<\/strong> has four bonded atoms and one lone pair on selenium (AX\u2084E<\/strong>). This lone pair distorts the shape from trigonal bipyramidal to see-saw<\/strong>, affecting bond angles.<\/p>\n\n\n\n
NH\u2082\u207b<\/strong> has two bonded atoms and two lone pairs on nitrogen. Like water, it’s bent, with angles slightly less than 109.5\u00b0, about 104\u00b0<\/strong>, due to increased repulsion from lone pairs.<\/p>\n\n\n\n
SCN\u207b<\/strong> is a linear ion where resonance structures are possible, but all forms are AX\u2082<\/strong> with a linear<\/strong> geometry and 180\u00b0<\/strong> bond angles due to no lone pairs on the central carbon.<\/p>\n\n\n\n
SnCl\u2085\u207b<\/strong> forms a trigonal bipyramidal<\/strong> shape, common for five bonded pairs (AX\u2085), with a mix of 90\u00b0, 120\u00b0, and 180\u00b0 angles. Negative charge increases electron density but doesn\u2019t change geometry significantly.<\/p>\n\n\n\n
This analysis relies on electron domain geometry and hybridization (sp\u00b3, sp\u00b3d, etc.), critical for predicting molecular behavior, reactivity, and physical properties.<\/p>\n\n\n\n
\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
For each of the following, a. Draw the lewis structure b. Indicate the molecular geometry c. Indicate the bond angles PCI3IBr4-SeF4NH2-SCN-SnCl5- The Correct Answer and Explanation is: 1. PCl\u2083 a. Lewis Structure:P is the central atom with three Cl atoms bonded and one lone pair. b. Molecular Geometry: Trigonal pyramidalc. Bond Angles: ~107\u00b0 2. IBr\u2084\u207b […]<\/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-222261","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222261","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=222261"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222261\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=222261"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=222261"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=222261"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}