Which of the following molecules has a geometry described as trigonal planar? A) CHF3 B) BF3 D) OF2 30) E) SiH4 C) PF3 31) After drawing the Lewis dot structure for SBr2, determine the number of single bonds, 31) double bonds, and lone pairs on the central atom.A) 2,0,2 B) 2, 0,1 C) 2,0,0 32) Which of the following compounds is a strong electrolyte? A) H20 B) CH40 C) NaF D) 0, 2,0 E) 1,1,0 32) D) CH4 E) 02 33) 33) Identify the major ionic species present in an aqueous solution of Na2CO3. A) Naz, C2, 03 B) Na+, CO32- C) Naz, CO32 D) Na, C, 02- E) Nat, 04, 032- 34) What mass of C6H1206 (glucose) is needed to prepare 450. ml. of a 0.650 M solution 34) of glucose in water? A) 293 g B) 0.692 g C) 52.7 g D) 0.293 g E) 125 g 35) What mass of K2CO3 is needed to prepare 200. mL of a solution having a potassium 35) ion concentration of 0.150 M A) 4.15 g B) 1.49 g C) 13.8 g D) 2.07 g E) 10.4 g 36) A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution. H2O 36) is the A) solution B) ionic compound C) solute D) solid El solvent 37) What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution? A) 2.5 B) 1.5 C) 3.5 D) None of the above E14.4<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n Answer: B) BF\u2083<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Other molecules:<\/p>\n\n\n\n Answer: A) 2 single bonds, 0 double bonds, 2 lone pairs<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Answer: C) NaF<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Answer: B) Na\u207a, CO\u2083\u00b2\u207b<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Answer: C) 52.7 g<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Answer: A) 4.15 g<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Answer: E) Solvent<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Answer: A) 2.5 M<\/strong><\/p>\n\n\n\n Explanation<\/strong>: Which of the following molecules has a geometry described as trigonal planar? A) CHF3 B) BF3 D) OF2 30) E) SiH4 C) PF3 31) After drawing the Lewis dot structure for SBr2, determine the number of single bonds, 31) double bonds, and lone pairs on the central atom.A) 2,0,2 B) 2, 0,1 C) 2,0,0 32) […]<\/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-184435","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184435","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=184435"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184435\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184435"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184435"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184435"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Solutions to the Questions:<\/h3>\n\n\n\n
1. Which molecule has a trigonal planar geometry?<\/strong><\/h4>\n\n\n\n
The geometry of a molecule depends on its central atom and the surrounding atoms. Boron trifluoride (BF\u2083) has a central boron atom surrounded by three fluorine atoms. Boron has three valence electrons and forms three single bonds with fluorine, leaving no lone pairs on boron. According to VSEPR theory, the molecule adopts a trigonal planar geometry to minimize electron pair repulsion, with bond angles of 120\u00b0.<\/p>\n\n\n\n\n
\n\n\n\n2. Lewis structure for SBr\u2082: How many single bonds, double bonds, and lone pairs on sulfur?<\/strong><\/h4>\n\n\n\n
Sulfur is the central atom in SBr\u2082. It forms two single bonds with two bromine atoms. Sulfur has six valence electrons, so after bonding with bromine (which contributes two electrons), four electrons remain as two lone pairs on sulfur. There are no double bonds.<\/p>\n\n\n\n
\n\n\n\n3. Which compound is a strong electrolyte?<\/strong><\/h4>\n\n\n\n
A strong electrolyte dissociates completely into ions in water. Sodium fluoride (NaF) is an ionic compound and dissociates into Na\u207a and F\u207b in water, making it a strong electrolyte. Water (H\u2082O) and methanol (CH\u2084O) are covalent and do not dissociate significantly, while O\u2082 and CH\u2084 are non-electrolytes.<\/p>\n\n\n\n
\n\n\n\n4. Major ionic species in an aqueous solution of Na\u2082CO\u2083?<\/strong><\/h4>\n\n\n\n
Sodium carbonate (Na\u2082CO\u2083) dissociates completely in water into two sodium ions (Na\u207a) and one carbonate ion (CO\u2083\u00b2\u207b).<\/p>\n\n\n\n
\n\n\n\n5. Mass of glucose to prepare 450 mL of 0.650 M solution?<\/strong><\/h4>\n\n\n\n
Moles of glucose = ( M \\times V = 0.650 \\times 0.450 = 0.2925 \\, \\text{mol} )
Molar mass of glucose (C\u2086H\u2081\u2082O\u2086) = 180 g\/mol
Mass = ( 0.2925 \\, \\text{mol} \\times 180 \\, \\text{g\/mol} = 52.7 \\, \\text{g} )<\/p>\n\n\n\n
\n\n\n\n6. Mass of K\u2082CO\u2083 to prepare 200 mL solution with 0.150 M K\u207a concentration?<\/strong><\/h4>\n\n\n\n
For K\u207a concentration of 0.150 M, K\u2082CO\u2083 concentration is ( \\frac{0.150}{2} = 0.075 \\, \\text{M} ).
Moles of K\u2082CO\u2083 = ( 0.075 \\times 0.200 = 0.015 \\, \\text{mol} )
Molar mass of K\u2082CO\u2083 = 138 g\/mol
Mass = ( 0.015 \\, \\text{mol} \\times 138 \\, \\text{g\/mol} = 4.15 \\, \\text{g} )<\/p>\n\n\n\n
\n\n\n\n7. In the KCl solution, what is H\u2082O?<\/strong><\/h4>\n\n\n\n
The solvent is the substance in which the solute dissolves. In this case, water (H\u2082O) is the solvent, and KCl is the solute.<\/p>\n\n\n\n
\n\n\n\n8. Molarity of solution with 5.0 moles of solute in 2.00 liters?<\/strong><\/h4>\n\n\n\n
Molarity = ( \\frac{\\text{Moles of solute}}{\\text{Volume of solution in liters}} )
Molarity = ( \\frac{5.0}{2.00} = 2.5 \\, \\text{M} ).<\/p>\n","protected":false},"excerpt":{"rendered":"