Write an expression for the net change in charge if two electrons are added to each of six atoms in a group. Also, write an expression that represents removing two protons each from a group of six atoms.\u200b<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n To solve this, we need to express the net change in charge resulting from the addition of electrons and the removal of protons from a group of atoms. Here\u2019s how we can approach each part of the question:<\/p>\n\n\n\n Each electron carries a negative charge of ( -1 \\, e ) (where ( e ) is the elementary charge, approximately ( 1.602 \\times 10^{-19} ) coulombs). If two electrons are added to each of six atoms, the total change in charge can be expressed as:<\/p>\n\n\n\n [ Since two electrons are added to each atom, and there are six atoms in total, the total number of electrons added is:<\/p>\n\n\n\n [ The charge contributed by each of these 12 electrons is ( -1 \\, e ). Therefore, the total change in charge is:<\/p>\n\n\n\n [ Thus, the expression for the net change in charge from adding two electrons to each of six atoms is:<\/p>\n\n\n\n [ This means the charge of the group of atoms becomes more negative, with a total charge change of ( -12 \\, e ).<\/p>\n\n\n\n Each proton carries a positive charge of ( +1 \\, e ). If two protons are removed from each of six atoms, the total number of protons removed is:<\/p>\n\n\n\n [ Since each proton carries a positive charge of ( +1 \\, e ), the total change in charge is:<\/p>\n\n\n\n [ Thus, the expression for the net change in charge from removing two protons from each of six atoms is:<\/p>\n\n\n\n [ This means the group of atoms becomes more positive, with a total charge change of ( +12 \\, e ).<\/p>\n\n\n\n The change in charge of an atom depends on the type of particle added or removed. Electrons have a negative charge, so adding electrons makes the atom more negatively charged. Conversely, protons have a positive charge, so removing protons makes the atom more positively charged. In this problem:<\/p>\n\n\n\n These calculations rely on the fact that the number of electrons and protons determines the overall charge of an atom or a group of atoms.<\/p>\n","protected":false},"excerpt":{"rendered":" Write an expression for the net change in charge if two electrons are added to each of six atoms in a group. Also, write an expression that represents removing two protons each from a group of six atoms.\u200b The Correct Answer and Explanation is: To solve this, we need to express the net change in […]<\/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-167855","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167855","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=167855"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167855\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=167855"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=167855"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=167855"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}1. Net Change in Charge from Adding Electrons<\/strong><\/h3>\n\n\n\n
\\text{Net change in charge} = (\\text{number of electrons added}) \\times (\\text{charge of each electron})
]<\/p>\n\n\n\n
2 \\times 6 = 12 \\, \\text{electrons}
]<\/p>\n\n\n\n
\\text{Net change in charge} = 12 \\times (-1 \\, e) = -12 \\, e
]<\/p>\n\n\n\n
\\boxed{-12e}
]<\/p>\n\n\n\n2. Net Change in Charge from Removing Protons<\/strong><\/h3>\n\n\n\n
2 \\times 6 = 12 \\, \\text{protons}
]<\/p>\n\n\n\n
\\text{Net change in charge} = 12 \\times (+1 \\, e) = +12 \\, e
]<\/p>\n\n\n\n
\\boxed{+12e}
]<\/p>\n\n\n\nExplanation<\/h3>\n\n\n\n
\n