Question

the complete electron configuration for na is 1s² 1 2 3 the complete electron configuration for na⁺¹ is 1s² 4 5 6 a. 1s⁰ b. 1s¹ c. 1s² d. 2s⁰ e. 2s¹ f. 2s² g. 2p⁰ h. 2p¹ i. 2p² j. 2p³ k. 2p⁴ l. 2p⁵ m. 2p⁶ n. 3s⁰ o. 3s¹ p. 3s² q. 3s³

Explanation:

Step1: Recall sodium's atomic number

Sodium (Na) has an atomic number of 11.

Step2: Write electron - configuration for Na

Electrons fill orbitals in the order 1s, 2s, 2p, 3s etc. The 1s orbital can hold 2 electrons, the 2s can hold 2, and the 2p can hold 6. For Na (11 electrons), the electron - configuration is $1s^{2}2s^{2}2p^{6}3s^{1}$. So for the first part: 1 is F ($2s^{2}$), 2 is M ($2p^{6}$), 3 is O ($3s^{1}$).

Step3: Consider $Na^{+}$

$Na^{+}$ has lost one electron (from the outermost shell). So it has 10 electrons. The electron - configuration for $Na^{+}$ is $1s^{2}2s^{2}2p^{6}$. So 4 is F ($2s^{2}$), 5 is M ($2p^{6}$), 6 is N ($3s^{0}$).

Answer:

1. F. $2s^{2}$
2. M. $2p^{6}$
3. O. $3s^{1}$
4. F. $2s^{2}$
5. M. $2p^{6}$
6. N. $3s^{0}$