Answer true or false.<\/p>\n\n\n\n
(a) The name of a binary ionic compound consists of the name of the positive ion followed by the name of the negative ion.<\/p>\n\n\n\n
(b) In naming binary ionic compounds, it is necessary to state the number of each ion present in the compound.<\/p>\n\n\n\n
(c) The formula of aluminum oxide is Al2 O3 .<\/p>\n\n\n\n
(d) Both copper(II) oxide and cupric oxide are acceptable names for CuO.<\/p>\n\n\n\n
(e) The systematic name for Fe2 O3 is iron(II) oxide.<\/p>\n\n\n\n
(f) The systematic name for FeCO3 is iron carbonate.<\/p>\n\n\n\n
(g) The systematic name for NaH2PO4 is sodium di- hydrogen phosphate.<\/p>\n\n\n\n
(h) The systematic name for K2HPO4 is dipotassium hydrogen phosphate.<\/p>\n\n\n\n
(i) The systematic name for Na2O is sodium oxide.<\/p>\n\n\n\n
(j) The systematic name for PCl3 is potassium chloride.<\/p>\n\n\n\n
(k) The formula of ammonium carbonate is NH4CO3.<\/p>\n\n\n\n
39.<\/p>\n\n\n\n
(a) A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9.<\/p>\n\n\n\n
(b) If the difference in electronegativity between two atoms is zero (they have identical electronegativ- ities), then the two atoms will not form a covalent bond.<\/p>\n\n\n\n
(c) A covalent bond formed by sharing two electrons is called a double bond.<\/p>\n\n\n\n
(d) In the hydrogen molecule (H2), the shared pair of electrons completes the valence shell of each hydrogen.<\/p>\n\n\n\n
(e) In the molecule CH4 , each hydrogen has an electron configuration like that of helium and carbon has an electron configuration like that of neon.<\/p>\n\n\n\n
(f) In a polar covalent bond, the more electronegative atom has a partial negative charge (\u00c3\u201a\u00c2\u00ad2) and the less electronegative atom has a partial positive charge (\u00c3\u201a\u00c2\u00ad1).<\/p>\n\n\n\n
(g) These bonds are arranged in order of increasing polarity CiH , NiH , OiH.<\/p>\n\n\n\n
(h) These bonds are arranged in order of increasing polarity HiF , HiCl , HiBr. (<\/p>\n\n\n\n
i) A polar bond has a dipole with the negative end located at the more electronegative atom.
(j) In a single bond, two atoms share one pair of electrons; in a double bond, they share two pairs of electrons; and in a triple bond, they share three pairs of electrons.<\/p>\n\n\n\n
(k) The Lewis structure for ethane, C2H6, must show eight valence electrons.<\/p>\n\n\n\n
(l) The Lewis structure for formaldehyde, CH2 O, must show 12 valence electrons.<\/p>\n\n\n\n
(m) The Lewis structure for the ammonium ion, NH4 1, must show nine valence electrons.<\/p>\n\n\n\n
(n) Atoms of third-period elements can hold more than eight electrons in their valence shells.<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n Here are the true or false answers, followed by a 300-word explanation:<\/p>\n\n\n\n (a) True<\/strong> (a) True<\/strong> \u2013 A covalent bond forms when the difference in electronegativity is less than 1.9. Ionic and covalent compounds follow distinct naming conventions and bonding rules. Binary ionic compounds consist of a metal cation<\/strong> and a nonmetal anion<\/strong>, with the cation name first<\/strong> and the anion name second<\/strong> (e.g., NaCl = sodium chloride<\/strong>). The charges must balance, but numbers of ions are not explicitly stated unless using a Roman numeral system for transition metals<\/strong> (e.g., Fe\u2082O\u2083 = iron(III) oxide<\/strong>).<\/p>\n\n\n\n Covalent bonds form when atoms share electrons<\/strong>. A polar covalent bond<\/strong> occurs when electronegativity differences<\/strong> create a dipole<\/strong> (e.g., H\u2013F<\/strong>). A nonpolar bond<\/strong> occurs when atoms have similar electronegativities<\/strong>, like O\u2082 or N\u2082<\/strong>.<\/p>\n\n\n\n The Lewis structures<\/strong> of molecules help visualize bonding and valence electrons. Some molecules follow the octet rule<\/strong> (8 valence electrons), but third-period elements<\/strong> (like sulfur or phosphorus) can have expanded octets<\/strong>, holding more than 8 electrons.<\/p>\n\n\n\n Understanding bonding, naming conventions, and valence electron arrangements is essential in chemistry to predict molecular properties, reactivity, and stability<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":" Answer true or false. (a) The name of a binary ionic compound consists of the name of the positive ion followed by the name of the negative ion. (b) In naming binary ionic compounds, it is necessary to state the number of each ion present in the compound. (c) The formula of aluminum oxide is […]<\/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-187262","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187262","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=187262"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187262\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187262"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187262"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187262"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Answers:<\/strong><\/h3>\n\n\n\n
Binary Ionic Compounds:<\/strong><\/h4>\n\n\n\n
(b) False<\/strong> \u2013 The number of each ion is not explicitly stated in the name, as ionic compounds naturally balance charges.
(c) True<\/strong> \u2013 The correct formula for aluminum oxide is Al\u2082O\u2083<\/strong>.
(d) True<\/strong> \u2013 Copper(II) oxide<\/strong> and cupric oxide<\/strong> both correctly name CuO.
(e) False<\/strong> \u2013 The systematic name for Fe\u2082O\u2083<\/strong> is iron(III) oxide<\/strong>, not iron(II) oxide.
(f) True<\/strong> \u2013 The correct name for FeCO\u2083<\/strong> is iron(II) carbonate<\/strong> (or simply iron carbonate).
(g) True<\/strong> \u2013 NaH\u2082PO\u2084<\/strong> is named sodium dihydrogen phosphate<\/strong>.
(h) True<\/strong> \u2013 K\u2082HPO\u2084<\/strong> is named dipotassium hydrogen phosphate<\/strong>.
(i) True<\/strong> \u2013 Na\u2082O<\/strong> is named sodium oxide<\/strong>.
(j) False<\/strong> \u2013 PCl\u2083<\/strong> is named phosphorus trichloride<\/strong>, not potassium chloride.
(k) False<\/strong> \u2013 The correct formula for ammonium carbonate is (NH\u2084)\u2082CO\u2083<\/strong>, not NH\u2084CO\u2083.<\/p>\n\n\n\n
\n\n\n\nCovalent Bonding:<\/strong><\/h4>\n\n\n\n
(b) False<\/strong> \u2013 Even if the difference is zero, the atoms can still form a nonpolar covalent bond<\/strong>.
(c) False<\/strong> \u2013 A covalent bond sharing two electrons is a single bond<\/strong>, not a double bond.
(d) True<\/strong> \u2013 In H\u2082<\/strong>, both hydrogen atoms achieve a full valence shell<\/strong> by sharing electrons.
(e) True<\/strong> \u2013 In CH\u2084<\/strong>, hydrogen attains the helium<\/strong> configuration, and carbon attains the neon<\/strong> configuration.
(f) True<\/strong> \u2013 In a polar covalent bond<\/strong>, the more electronegative atom<\/strong> gets a partial negative charge<\/strong>, and the less electronegative atom<\/strong> gets a partial positive charge<\/strong>.
(g) True<\/strong> \u2013 Polarity increases as C\u2013H < N\u2013H < O\u2013H<\/strong> due to electronegativity differences.
(h) True<\/strong> \u2013 Polarity increases as H\u2013I < H\u2013Br < H\u2013Cl < H\u2013F<\/strong>.
(i) True<\/strong> \u2013 A polar bond<\/strong> has a dipole moment<\/strong> where the negative end is at the more electronegative atom<\/strong>.
(j) True<\/strong> \u2013 Single bond = one pair<\/strong>, double bond = two pairs<\/strong>, triple bond = three pairs<\/strong> of electrons.
(k) False<\/strong> \u2013 C\u2082H\u2086<\/strong> must show 14 valence electrons<\/strong> (not 8).
(l) True<\/strong> \u2013 CH\u2082O<\/strong> must show 12 valence electrons<\/strong> (4 from carbon, 6 from oxygen, 2 from hydrogen).
(m) False<\/strong> \u2013 The ammonium ion (NH\u2084\u207a<\/strong>) has 8 valence electrons<\/strong>, not 9, due to the positive charge<\/strong>.
(n) True<\/strong> \u2013 Third-period elements<\/strong> like phosphorus and sulfur can have expanded octets<\/strong> (more than 8 electrons).<\/p>\n\n\n\n
\n\n\n\nExplanation:<\/strong><\/h3>\n\n\n\n