Question

1. in each of the following sets of atoms, which element would be expected to have the highest ionization energy?

a. cs, k, li
b. ba, sr, ca
c. i, br, cl
d. mg, si, s

Explanation:

Step1: Recall ionization - energy trend

Ionization energy increases across a period and decreases down a group in the periodic table.

Step2: Analyze part a

Cs, K, Li are in Group 1. Li is at the top - most, so it has the highest ionization energy among them as ionization energy decreases down a group.

Step3: Analyze part b

Ba, Sr, Ca are in Group 2. Ca is at the top - most, so it has the highest ionization energy among them as ionization energy decreases down a group.

Step4: Analyze part c

I, Br, Cl are in Group 17. Cl is at the top - most, so it has the highest ionization energy among them as ionization energy decreases down a group.

Step5: Analyze part d

Mg, Si, S are in Period 3. S is the right - most among them. Since ionization energy increases across a period, S has the highest ionization energy.

Answer:

a. Li
b. Ca
c. Cl
d. S