Question

1. electron configurations can be represented in an abbreviated form also known as the noble gas configuration for an element. what is the correct name and noble gas configuration for the element with the following configuration?

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p²

strontium - ar5s²4d¹⁰5p²
tin - kr5s²4d¹⁰5p²
zirconium - kr5s²4d¹⁰5p²
lead - xe5s²4d¹⁰5p²

Explanation:

• First, find the noble gas core. The electron configuration \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}\) is the electron configuration of \(Kr\) (krypton).
• The remaining part of the electron configuration is \(5s^{2}4d^{10}5p^{2}\).
• For tin (\(Sn\)), its atomic number is \(50\). The electron configuration of \(Kr\) has \(36\) electrons. Adding \(5s^{2}4d^{10}5p^{2}\) (\(2 + 10+ 2=14\) electrons) gives \(36 + 14=50\) electrons.
• Strontium (\(Sr\)) has an atomic number of \(38\). If we use \([Ar]\) as the core (\(18\) electrons), \(18+5s^{2}=20\) (incorrect as \(Sr\) has \(38\) electrons and its correct noble - gas configuration is \([Kr]5s^{2}\)).
• Zirconium (\(Zr\)) has an atomic number of \(40\). Its noble - gas configuration is \([Kr]5s^{2}4d^{2}\).
• Lead (\(Pb\)) has an atomic number of \(82\). Its noble - gas configuration is \([Xe]6s^{2}4f^{14}5d^{10}6p^{2}\).

Answer:

tin - \([Kr]5s^{2}4d^{10}5p^{2}\)