Question

however, as stated in the course outline, and in the orientation session, this quiz is not open book. you cannot access course material while you write the quiz. nor can you google your answers, work as a group, use a cheat sheet, etc. question 1 (1 point) what is the electron configuration for a sodium ion? $1s^{2}2s^{2}2p^{6}3s^{2}$ $1s^{2}2s^{2}2p^{6}$ $1s^{2}2s^{2}2p^{4}3s^{1}3p^{1}$ $1s^{2}2s^{2}2p^{6}3s^{1}$

Explanation:

Step1: Determine the atomic number of sodium

Sodium (Na) has an atomic number of 11. So, a neutral sodium atom has 11 electrons. The electron configuration of a neutral sodium atom is \(1s^{2}2s^{2}2p^{6}3s^{1}\).

Step2: Analyze the formation of sodium ion

A sodium ion (\(Na^{+}\)) is formed when a sodium atom loses one electron. It loses the electron from the outermost shell (the 3s orbital). So, the number of electrons in \(Na^{+}\) is \(11 - 1=10\).

Step3: Write the electron configuration of sodium ion

The electron configuration of an atom/ion with 10 electrons is \(1s^{2}2s^{2}2p^{6}\).

Answer:

\(1s^{2}2s^{2}2p^{6}\) (the second option)