{"id":26980,"date":"2025-06-19T20:12:17","date_gmt":"2025-06-19T20:12:17","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=26980"},"modified":"2025-06-19T20:12:34","modified_gmt":"2025-06-19T20:12:34","slug":"u-woi-negative-charge-on-each-cr4-four-anions-each-net-charge-on-each-cr4-you-can-see-the-net-charge-will-only-be-zero-if-x-4","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/u-woi-negative-charge-on-each-cr4-four-anions-each-net-charge-on-each-cr4-you-can-see-the-net-charge-will-only-be-zero-if-x-4\/","title":{"rendered":"U Woi negative charge on each Cr4+ (four anions each) net charge on each Cr4+ You can see the net charge will only be zero if x = 4"},"content":{"rendered":"\n
U Woi negative charge on each Cr4+ (four anions each) net charge on each Cr4+ You can see the net charge will only be zero if x = 4. That is, the cation. Here is the completed table: ANSWER Ionic compound cation: NaCl, NaNH4F, NH4NO3, Ni(NO3)2, V3+ NO3, CrCl4 More Practice Ma<\/pre>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
To correctly analyze and determine the net charge and balance in an ionic compound, we must understand how charges between cations (positively charged ions) and anions (negatively charged ions) interact to produce a neutral compound. Let us focus on CrCl\u2084<\/strong> in your example.<\/p>\n\n\n\n
\n\n\n\n
Correct Answer:<\/strong><\/h3>\n\n\n\n
Compound:<\/strong> CrCl\u2084
Cation:<\/strong> Cr\u2074\u207a (Chromium ion with +4 charge)
Anions:<\/strong> 4 \u00d7 Cl\u207b (Chloride ions, each with a \u20131 charge)<\/p>\n\n\n\n
Net charge on Cr\u2074\u207a:<\/strong> +4
Total charge of anions:<\/strong> 4 \u00d7 (\u20131) = \u20134
Overall net charge of the compound:<\/strong> (+4) + (\u20134) = 0 \u2192 neutral compound<\/strong><\/p>\n\n\n\n
So, the net charge on each Cr\u2074\u207a ion is +4<\/strong>, and since each Cl\u207b has a \u20131 charge, four chloride ions are required to balance one Cr\u2074\u207a ion, resulting in a neutral ionic compound<\/strong>.<\/p>\n\n\n\n
\n\n\n\n
Explanation:<\/strong><\/h3>\n\n\n\n
In ionic compounds, atoms gain or lose electrons to form ions that combine in ratios that result in an overall neutral charge. The total positive charge from cations must equal the total negative charge from anions. This is the key principle behind the formation of stable ionic compounds.<\/p>\n\n\n\n
Take the compound CrCl\u2084<\/strong> as an example. Chromium (Cr) is a transition metal and can form multiple oxidation states. In CrCl\u2084, each chlorine (Cl) atom forms a Cl\u207b ion with a \u20131 charge. Since there are four Cl\u207b ions, the total negative charge is \u20134. For the compound to be neutral, the positive charge from the chromium cation must exactly offset this \u20134 charge.<\/p>\n\n\n\n
This means the chromium ion in CrCl\u2084 must have a charge of +4, making it a Cr\u2074\u207a<\/strong> ion. The charges now balance: +4 from Cr\u2074\u207a and \u20134 from four Cl\u207b ions result in a net charge of zero.<\/p>\n\n\n\n
This balance of charges is essential in naming and understanding ionic compounds. If the charges did not balance, the compound would not be stable or correctly formed. Thus, in CrCl\u2084, each Cr\u2074\u207a ion is balanced by four Cl\u207b ions to maintain electrical neutrality, which is the hallmark of a correctly formed ionic compound.<\/p>\n\n\n\n
\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
U Woi negative charge on each Cr4+ (four anions each) net charge on each Cr4+ You can see the net charge will only be zero if x = 4. That is, the cation. Here is the completed table: ANSWER Ionic compound cation: NaCl, NaNH4F, NH4NO3, Ni(NO3)2, V3+ NO3, CrCl4 More Practice Ma The Correct Answer […]<\/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-26980","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26980","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=26980"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26980\/revisions"}],"predecessor-version":[{"id":26983,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26980\/revisions\/26983"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=26980"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=26980"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=26980"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}