Step 1: Understanding the Question:
Match the given electron configurations for second-period elements ($n=2$) to their first ionization energy (IE) values. Step 2: Detailed Explanation:
First, identify the elements for $n=2$:
(A) $2s^2 2p^1$: Boron (B)
(B) $2s^2 2p^6$: Neon (Ne)
(C) $2s^2$: Beryllium (Be)
(D) $2s^2 2p^3$: Nitrogen (N)
General trend of IE in Period 2: Li < B < Be < C < O < N < F < Ne.
Exceptions to the trend:
- Be > B: Be has a fully filled $2s^2$ subshell, making it harder to remove an electron compared to B ($2s^2 2p^1$).
- N > O: N has a half-filled $2p^3$ subshell, which is more stable than O's $2p^4$.
Ordered list of IE for the given elements: B < Be < N < Ne.
Ordered list of given values (kJ/mol): 801 (Q) < 899 (S) < 1402 (R) < 2080 (P).
Matching:
(A) B $\rightarrow$ 801 (Q)
(C) Be $\rightarrow$ 899 (S)
(D) N $\rightarrow$ 1402 (R)
(B) Ne $\rightarrow$ 2080 (P) Step 3: Final Answer:
The matching is A-Q, B-P, C-S, D-R.
