{"id":26358,"date":"2025-06-19T12:55:20","date_gmt":"2025-06-19T12:55:20","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=26358"},"modified":"2025-06-19T12:55:23","modified_gmt":"2025-06-19T12:55:23","slug":"draw-the-lewis-dot-structure-for-h","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/draw-the-lewis-dot-structure-for-h\/","title":{"rendered":"Draw the Lewis dot structure for H"},"content":{"rendered":"\n

Draw the Lewis dot structure for H?. Show the formal charge. 1b. Draw the Lewis dot structure for Sn2+. Show the formal charge. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. 1c. Draw the Lewis dot structure for K+. Show the formal charge. 1d. Draw the Lewis dot structure for Br?. Show the formal charge. 1e. ?Draw the Lewis dot structure for Se2?. Show the formal charge. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. 1f. Draw the Lewis dot structure for Sc3+. Show the formal charge. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom<\/p>\n\n\n\n

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

1a. Hydrogen atom (H\u00b7)<\/strong>
Lewis dot: H\u00b7<\/strong>
Formal charge: 0<\/strong><\/p>\n\n\n\n

Explanation:<\/strong>
Hydrogen has one valence electron. In its neutral atomic form, it is shown as a single dot next to the letter H. It forms one bond or gains one electron to reach the stable configuration of helium. Since it has the expected number of valence electrons, its formal charge is zero.<\/p>\n\n\n\n

\n\n\n\n

1b. Tin ion (Sn\u00b2\u207a)<\/strong>
Lewis dot: Sn\u00b2\u207a<\/strong> (no dots)
Formal charge: +2<\/strong><\/p>\n\n\n\n

Explanation:<\/strong>
Tin is in group 14 and normally has four valence electrons. In the Sn\u00b2\u207a ion, it has lost two electrons, so it is left with two fewer than its neutral valence count. Therefore, it is typically written without any dots and with a +2 charge to reflect the loss.<\/p>\n\n\n\n

\n\n\n\n

1c. Potassium ion (K\u207a)<\/strong>
Lewis dot: K\u207a<\/strong> (no dots)
Formal charge: +1<\/strong><\/p>\n\n\n\n

Explanation:<\/strong>
Potassium is an alkali metal with one valence electron. When it becomes a K\u207a ion, it loses that single electron, resulting in no valence electrons left to show. It is written as K with a +1 charge and no dots.<\/p>\n\n\n\n

\n\n\n\n

1d. Bromide ion (Br\u207b)<\/strong>
Lewis dot: :Br:\u207b<\/strong> (with 8 valence electrons arranged as 4 pairs)
Formal charge: \u20131<\/strong><\/p>\n\n\n\n

Explanation:<\/strong>
Bromine has seven valence electrons in its neutral state. When it gains one more electron to form Br\u207b, it reaches an octet with eight electrons, shown as four pairs around Br. The formal charge is \u20131.<\/p>\n\n\n\n

\n\n\n\n

1e. Selenide ion (Se\u00b2\u207b)<\/strong>
Lewis dot: :Se:\u00b2\u207b<\/strong> (8 valence electrons, four pairs)
Formal charge: \u20132<\/strong><\/p>\n\n\n\n

Explanation:<\/strong>
Selenium has six valence electrons. The Se\u00b2\u207b ion gains two more electrons, giving it a complete octet (8 electrons). These are shown as four pairs of dots. The formal charge is \u20132.<\/p>\n\n\n\n

\n\n\n\n

1f. Scandium ion (Sc\u00b3\u207a)<\/strong>
Lewis dot: Sc\u00b3\u207a<\/strong> (no dots)
Formal charge: +3<\/strong><\/p>\n\n\n\n

Explanation:<\/strong>
Scandium normally has three valence electrons. As Sc\u00b3\u207a, it has lost all three, so there are no electrons left to show. It is simply written with the +3 charge.<\/p>\n\n\n\n

\n\n\n\n

These dot structures are based on the number of valence electrons and how many are gained or lost during ion formation. Positive ions (cations) have fewer electrons than the neutral atom and usually show no dots, while negative ions (anions) have gained electrons and display full octets with dots.<\/p>\n\n\n\n

\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

Draw the Lewis dot structure for H?. Show the formal charge. 1b. Draw the Lewis dot structure for Sn2+. Show the formal charge. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. 1c. Draw the Lewis dot structure for K+. Show the formal charge. 1d. […]<\/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-26358","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26358","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=26358"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26358\/revisions"}],"predecessor-version":[{"id":26361,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/26358\/revisions\/26361"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=26358"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=26358"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=26358"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}