Here are the Lewis dot structures and explanations for AgCl<\/strong> and Co(NO\u2083)\u2082<\/strong>.<\/p>\n\n\n\n AgCl (Silver chloride):<\/strong><\/p>\n\n\n\n Ag is a metal and forms a +1 ion (Ag\u207a), while Cl is a halogen that forms a -1 ion (Cl\u207b). The bonding in AgCl is ionic<\/strong>, not covalent, so the Lewis structure is represented by showing ions with their charges and valence electrons.<\/p>\n\n\n\n Structure:<\/strong><\/p>\n\n\n\n Ag\u207a\u2003\u2003\u2003\u2003:Cl:\u207b Chloride ion (Cl\u207b) has 8 valence electrons in total. It gains one electron from Ag to complete its octet. Silver loses one electron, becoming Ag\u207a.<\/p>\n\n\n\n Co(NO\u2083)\u2082 (Cobalt(II) nitrate):<\/strong><\/p>\n\n\n\n Cobalt(II) nitrate consists of a Co\u00b2\u207a ion and two NO\u2083\u207b (nitrate) ions. Each nitrate ion contains one nitrogen atom bonded to three oxygen atoms. One of the bonds is a double bond while the other two are single bonds with negative charges delocalized across the oxygen atoms. The structure is stabilized through resonance.<\/p>\n\n\n\n Structure (simplified representation):<\/strong><\/p>\n\n\n\n [O=N\u207a\u2013O\u207b] Each nitrate ion looks like this, with resonance between the three oxygen atoms. The nitrogen is at the center forming one double bond and two single bonds with oxygens. Due to resonance, each N\u2013O bond has a bond order of approximately 1.33.<\/p>\n\n\n\n Cobalt exists as Co\u00b2\u207a and is ionically bonded to two NO\u2083\u207b ions. The overall compound is neutral.<\/p>\n\n\n\n AgCl is a simple ionic compound formed from a transition metal, silver (Ag), and a halogen, chlorine (Cl). Silver readily loses one electron to form a stable Ag\u207a ion. Chlorine, with seven valence electrons, gains this electron to complete its octet and becomes Cl\u207b. Since AgCl is ionic, the Lewis dot structure is best represented by showing Ag\u207a without electrons and Cl\u207b surrounded by eight electrons, indicating a full valence shell. The strong electrostatic attraction between these ions holds them together in a crystal lattice in solid form.<\/p>\n\n\n\n Co(NO\u2083)\u2082 is a more complex ionic compound. Cobalt in this compound has a +2 oxidation state, so it forms the Co\u00b2\u207a cation. The nitrate ion (NO\u2083\u207b) is a polyatomic ion consisting of one nitrogen atom covalently bonded to three oxygen atoms. One of these bonds is a double bond while the other two are single bonds with extra electrons, making the oxygens negatively charged. However, the negative charge is delocalized through resonance, making all N\u2013O bonds equivalent in length and strength. Each nitrate carries a -1 charge, and with two nitrate ions, the total negative charge is -2, balancing the +2 charge of cobalt.<\/p>\n\n\n\n The bond between cobalt and nitrate is ionic, as cobalt loses electrons to form a cation and each nitrate ion gains one electron. The nitrate ions themselves contain covalent bonds internally, but the overall attraction between Co\u00b2\u207a and NO\u2083\u207b is ionic. Lewis structures help illustrate the ionic and covalent character in such mixed compounds and are essential for understanding electron arrangement and reactivity<\/p>\n\n\n\n <\/p>\n\n\n\n .<\/p>\n\n\n\n Draw a Lewis dot structure for AgCl and Co(NO3)2. The Correct Answer and Explanation is: Here are the Lewis dot structures and explanations for AgCl and Co(NO\u2083)\u2082. Lewis Dot Structure for AgCl AgCl (Silver chloride): Ag is a metal and forms a +1 ion (Ag\u207a), while Cl is a halogen that forms a -1 ion […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-39754","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39754","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=39754"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39754\/revisions"}],"predecessor-version":[{"id":39764,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39754\/revisions\/39764"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=39754"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=39754"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=39754"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nLewis Dot Structure for AgCl<\/strong><\/h3>\n\n\n\n
\u2003\u2003\u2003\u2003\u2003\u2003(6 lone pair electrons around Cl)<\/p>\n\n\n\n
\n\n\n\nLewis Dot Structure for Co(NO\u2083)\u2082<\/strong><\/h3>\n\n\n\n
\u2003\u2003\u2003|
\u2003\u2003\u2003O\u207b<\/p>\n\n\n\n
\n\n\n\nExplanation<\/strong><\/h3>\n\n\n\n
![\"\"](\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1185.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"