If aluminum forms an ion.<\/p>\n\n\n\n
a) will it gain or lose electrons ?<\/p>\n\n\n\n
b) how many electrons will it gain or lose?<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n Correct Answers:<\/strong><\/p>\n\n\n\n a)<\/strong> Aluminum will lose<\/strong> electrons. Aluminum is a metal found in Group 13 (or IIIA) of the periodic table, with the atomic number 13. This means a neutral aluminum atom has 13 protons and 13 electrons. Its electron configuration is:<\/p>\n\n\n\n 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u00b9<\/strong><\/p>\n\n\n\n The electrons in the outermost shell (valence electrons) determine how an element reacts. For aluminum, the three electrons in the third energy level (3s\u00b2 3p\u00b9) are its valence electrons. These electrons are relatively loosely held and can be easily removed during chemical reactions.<\/p>\n\n\n\n Metals like aluminum tend to lose<\/strong> electrons rather than gain them because losing electrons allows them to achieve a more stable electron configuration \u2014 one that resembles the nearest noble gas. In aluminum’s case, losing its three valence electrons leaves it with the electron configuration of neon (1s\u00b2 2s\u00b2 2p\u2076), a stable noble gas with a full outer shell.<\/p>\n\n\n\n When aluminum loses three electrons, it forms a +3 ion (Al\u00b3\u207a)<\/strong>. This positively charged ion is more stable because it now has a full outer energy level. Since the aluminum atom lost electrons (which are negatively charged), the overall charge of the ion becomes positive.<\/p>\n\n\n\n This behavior is consistent across most metals. Metals lose electrons to form cations<\/strong> (positive ions), while nonmetals usually gain electrons to form anions<\/strong> (negative ions). For aluminum, forming a +3 cation is energetically favorable in chemical reactions such as bonding with nonmetals like oxygen or chlorine.<\/p>\n\n\n\n In summary, aluminum loses 3 electrons to form a stable Al\u00b3\u207a ion, aligning with its tendency as a metal to achieve a full outer shell by shedding valence electrons. This principle helps explain its behavior in ionic compounds such as aluminum oxide (Al\u2082O\u2083).<\/p>\n","protected":false},"excerpt":{"rendered":" If aluminum forms an ion. a) will it gain or lose electrons ? b) how many electrons will it gain or lose? The correct answer and explanation is : Correct Answers: a) Aluminum will lose electrons.b) Aluminum will lose 3 electrons. Explanation (Approx. 300 Words): Aluminum is a metal found in Group 13 (or IIIA) […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[],"tags":[],"class_list":["post-6191","post","type-post","status-publish","format-standard","hentry"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/6191","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=6191"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/6191\/revisions"}],"predecessor-version":[{"id":6192,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/6191\/revisions\/6192"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=6191"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=6191"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=6191"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
b)<\/strong> Aluminum will lose 3 electrons<\/strong>.<\/p>\n\n\n\n
\n\n\n\nExplanation (Approx. 300 Words):<\/h3>\n\n\n\n