Correct Answer:<\/strong> Explanation:<\/strong> The complete electron configuration of chlorine is: However, when asked for the noble gas configuration<\/em>, we use the symbol of the noble gas that comes before<\/em> chlorine in the periodic table to represent the core electrons. In chlorine\u2019s case, that noble gas is neon, which has the electron configuration: This accounts for 10 electrons. The remaining 7 electrons (17 – 10 = 7) are then written as: So, the noble gas configuration of chlorine becomes: This configuration tells us several things. First, chlorine has its valence electrons in the third energy level (principal quantum number n = 3), specifically in the 3s and 3p orbitals. The 3p orbital has 5 electrons, just one short of being completely filled (which would be 3p\u2076). That\u2019s why chlorine is highly reactive\u2014it wants to gain one more electron to achieve a full outer shell, just like a noble gas.<\/p>\n\n\n\n By achieving a full valence shell (octet), chlorine becomes more stable. This is also why chlorine often forms -1 ions (Cl\u207b) in chemical reactions, especially when bonding with metals like sodium, forming ionic compounds such as sodium chloride (NaCl).<\/p>\n\n\n\n Using noble gas notation makes electron configurations shorter, easier to read, and focuses attention on the valence electrons, which are most important in chemical bonding and reactivity.<\/p>\n\n\n\n what is the correct noble gas configuration of chlorine The Correct Answer and Explanation is: Correct Answer:[Ne] 3s\u00b2 3p\u2075 Explanation:Chlorine is a chemical element with the atomic number 17, which means it has 17 electrons when in its neutral state. 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[Ne] 3s\u00b2 3p\u2075<\/p>\n\n\n\n
Chlorine is a chemical element with the atomic number 17, which means it has 17 electrons when in its neutral state. To write its electron configuration, we need to arrange these electrons into the appropriate energy levels or orbitals.<\/p>\n\n\n\n
1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2075<\/p>\n\n\n\n
1s\u00b2 2s\u00b2 2p\u2076<\/p>\n\n\n\n
3s\u00b2 3p\u2075<\/p>\n\n\n\n
[Ne] 3s\u00b2 3p\u2075<\/strong><\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-605.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"