Question

question 4. identify the element with the greatest ionization energy.
a) nitrogen (n), rubidium (rb), copper (cu)
b) tellurium (te), indium (in), chlorine (cl)

Explanation:

Step1: Recall Ionization Energy Trends

Ionization energy (IE) generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. This is because as we move across a period, the effective nuclear charge increases, pulling electrons closer, so more energy is needed to remove an electron. Down a group, electrons are in higher energy levels (larger atomic radius), so less energy is needed to remove them.

Step2: Analyze Part a) - N, Rb, Cu

• Nitrogen (N): Period 2, Group 15.
• Rubidium (Rb): Period 5, Group 1. Alkali metals have low IE (easiest to lose electrons).
• Copper (Cu): Period 4, Group 11 (transition metal).

Compare their positions: N is in a higher period (2 vs Rb's 5, Cu's 4) and further right in the period than Cu. So N has a higher effective nuclear charge and smaller atomic radius than Rb and Cu. Thus, N has the highest IE among N, Rb, Cu.

Step3: Analyze Part b) - Te, In, Cl

• Tellurium (Te): Period 5, Group 16.
• Indium (In): Period 5, Group 13.
• Chlorine (Cl): Period 3, Group 17.

Compare positions: Cl is in a lower period (3 vs Te and In's 5) and further right (Group 17 vs Te's 16, In's 13). So Cl has a higher effective nuclear charge and smaller atomic radius than Te and In. Thus, Cl has the highest IE among Te, In, Cl.

Answer:

a) Nitrogen (N)
b) Chlorine (Cl)