Question

1. drag and drop the electron configurations to the elements. refer to the periodic table.

1s²2s²2p⁶3s²3p⁵

1s²2s²2p³

1s²2s²2p⁶3s²3p¹

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

Explanation:

Step1: Calculate the number of electrons

For \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}\), sum the exponents: \(2 + 2+6 + 2+5=17\). Chlorine (\(Cl\)) has atomic number \(17\).

Step2: Calculate the number of electrons

For \(1s^{2}2s^{2}2p^{3}\), sum the exponents: \(2+2 + 3=7\). Nitrogen (\(N\)) has atomic number \(7\).

Step3: Calculate the number of electrons

For \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}\), sum the exponents: \(2+2+6 + 2+1=13\). Aluminium (\(Al\)) has atomic number \(13\).

Step4: Calculate the number of electrons

For \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}\), sum the exponents: \(2+2+6+2+6 + 2+10=30\). Zinc (\(Zn\)) has atomic number \(30\).

Answer:

\(1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}\) → \(Cl\); \(1s^{2}2s^{2}2p^{3}\) → \(N\); \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}\) → \(Al\); \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}\) → \(Zn\)