{"id":184807,"date":"2025-01-21T16:29:37","date_gmt":"2025-01-21T16:29:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184807"},"modified":"2025-01-21T16:29:39","modified_gmt":"2025-01-21T16:29:39","slug":"depict-the-electron-configuration-for-magnesium-ing-an-orbital-box-diagram-and-noble-gas-notation","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/21\/depict-the-electron-configuration-for-magnesium-ing-an-orbital-box-diagram-and-noble-gas-notation\/","title":{"rendered":"Depict the electron configuration for magnesium ing an orbital box diagram and noble gas notation"},"content":{"rendered":"\n

13. Depict the electron configuration for magnesium ing an orbital box diagram and noble gas notation. Give a complete set of four quantum numbers for each of the electrons beyond those of the preceding noble gas US-ir growth in poisonous. ce of the electron ments, and a town in resistant ial appli- gh zirco- th. and in world. re im- ron aird corro- may be tum numbers? In some “none.” In such cases, explain why “none” is the correct answer. (a) n = 3 (b) n = 3 and l = 2 (c) n = 4, l = 1, me = -1, and m\u00e2\u201a\u201a = (d) n = 5, l = 0, me = -1, ms = + \u00c2\u00bd +\u00c2\u00bd an. 13. Depict the electron configuration for magnesium ing an orbital box diagram and noble gas notation. Give a complete set of four quantum numbers for each of the electrons beyond those of the preceding noble gas. 14. Depict the electron configuration for phosphorus us ing an orbital box diagram and noble gas notation. Give one possible set of four quantum numbers for each of the electrons beyond those of the preceding noble gas. 15. Using an orbital box diagram and noble gas nota- tion, show the electron configuration of gallium, Ga. Give a set of quantum numbers for the highest-energy electron. 16. Using an orbital box diagram and noble gas notation, show the electron configuration of titanium. Give one possible set of four quantum numbers for each of the electrons beyond those of the preceding noble gas. gas nota ions. Ar Periodic Prop (See Section Screens 7.7- 23. Arrang size: A at Figu the ne 24. Arr ing si looki up th ho 25. Sele radi (a) 26. S larg (a) 27. Wh CO (a) (b<\/p>\n\n\n\n

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

13. Electron Configuration for Magnesium (Mg)<\/h3>\n\n\n\n
    \n
  1. Electron Configuration<\/strong>:<\/li>\n<\/ol>\n\n\n\n
      \n
    • Orbital box diagram:
      1s \u2191\u2193 2s \u2191\u2193 2p \u2191\u2193 \u2191\u2193 \u2191\u2193 3s \u2191\u2193<\/code><\/li>\n\n\n\n
    • Noble gas notation: [Ne] 3s\u00b2<\/strong><\/li>\n<\/ul>\n\n\n\n
        \n
      1. Quantum Numbers Beyond Noble Gas<\/strong>:<\/li>\n<\/ol>\n\n\n\n
          \n
        • Electrons beyond the preceding noble gas ([Ne]): 3s\u00b2\n
            \n
          • For 3s (1st electron): (n=3), (l=0), (m_l=0), (m_s=+\\frac{1}{2})<\/li>\n\n\n\n
          • For 3s (2nd electron): (n=3), (l=0), (m_l=0), (m_s=-\\frac{1}{2})<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
            \n\n\n\n

            14. Electron Configuration for Phosphorus (P)<\/h3>\n\n\n\n
              \n
            1. Electron Configuration<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                \n
              • Orbital box diagram:
                1s \u2191\u2193 2s \u2191\u2193 2p \u2191\u2193 \u2191\u2193 \u2191\u2193 3s \u2191\u2193 3p \u2191 \u2191 \u2191<\/code><\/li>\n\n\n\n
              • Noble gas notation: [Ne] 3s\u00b2 3p\u00b3<\/strong><\/li>\n<\/ul>\n\n\n\n
                  \n
                1. Quantum Numbers Beyond Noble Gas<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                    \n
                  • Electrons beyond [Ne]: 3s\u00b2 3p\u00b3\n
                      \n
                    • 3s (1st electron): (n=3), (l=0), (m_l=0), (m_s=+\\frac{1}{2})<\/li>\n\n\n\n
                    • 3s (2nd electron): (n=3), (l=0), (m_l=0), (m_s=-\\frac{1}{2})<\/li>\n\n\n\n
                    • 3p (1st electron): (n=3), (l=1), (m_l=-1), (m_s=+\\frac{1}{2})<\/li>\n\n\n\n
                    • 3p (2nd electron): (n=3), (l=1), (m_l=0), (m_s=+\\frac{1}{2})<\/li>\n\n\n\n
                    • 3p (3rd electron): (n=3), (l=1), (m_l=+1), (m_s=+\\frac{1}{2})<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
                      \n\n\n\n

                      15. Electron Configuration for Gallium (Ga)<\/h3>\n\n\n\n
                        \n
                      1. Electron Configuration<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                          \n
                        • Orbital box diagram:
                          [Ar] 4s \u2191\u2193 3d \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 4p \u2191<\/code><\/li>\n\n\n\n
                        • Noble gas notation: [Ar] 3d\u00b9\u2070 4s\u00b2 4p\u00b9<\/strong><\/li>\n<\/ul>\n\n\n\n
                            \n
                          1. Quantum Numbers for Highest-Energy Electron<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                              \n
                            • 4p\u00b9: (n=4), (l=1), (m_l=-1), (m_s=+\\frac{1}{2})<\/li>\n<\/ul>\n\n\n\n
                              \n\n\n\n

                              16. Electron Configuration for Titanium (Ti)<\/h3>\n\n\n\n
                                \n
                              1. Electron Configuration<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                                  \n
                                • Orbital box diagram:
                                  [Ar] 4s \u2191\u2193 3d \u2191 \u2191<\/code><\/li>\n\n\n\n
                                • Noble gas notation: [Ar] 3d\u00b2 4s\u00b2<\/strong><\/li>\n<\/ul>\n\n\n\n
                                    \n
                                  1. Quantum Numbers Beyond Noble Gas<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                                      \n
                                    • 4s\u00b2:\n
                                        \n
                                      • 4s (1st electron): (n=4), (l=0), (m_l=0), (m_s=+\\frac{1}{2})<\/li>\n\n\n\n
                                      • 4s (2nd electron): (n=4), (l=0), (m_l=0), (m_s=-\\frac{1}{2})<\/li>\n<\/ul>\n<\/li>\n\n\n\n
                                      • 3d\u00b2:\n
                                          \n
                                        • 3d (1st electron): (n=3), (l=2), (m_l=-2), (m_s=+\\frac{1}{2})<\/li>\n\n\n\n
                                        • 3d (2nd electron): (n=3), (l=2), (m_l=-1), (m_s=+\\frac{1}{2})<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
                                          \n\n\n\n

                                          Answers to Quantum Number Questions<\/h3>\n\n\n\n
                                            \n
                                          • (a) (n=3): Valid; quantum number (n) defines the shell and is an integer >0.<\/li>\n\n\n\n
                                          • (b) (n=3), (l=2): Valid; (l=2) corresponds to a d orbital ((0 \\leq l < n)).<\/li>\n\n\n\n
                                          • (c) (n=4), (l=1), (m_l=-1), (m_s=): Invalid; (m_s) must be (+\\frac{1}{2}) or (-\\frac{1}{2}).<\/li>\n\n\n\n
                                          • (d) (n=5), (l=0), (m_l=-1), (m_s=+\\frac{1}{2}): Invalid; (m_l) must be 0 when (l=0).<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

                                            13. Depict the electron configuration for magnesium ing an orbital box diagram and noble gas notation. Give a complete set of four quantum numbers for each of the electrons beyond those of the preceding noble gas US-ir growth in poisonous. ce of the electron ments, and a town in resistant ial appli- gh zirco- th. […]<\/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-184807","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184807","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=184807"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184807\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184807"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184807"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184807"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}