Question

question 2. select the correct answers from the drop-down menu for each statement about ionization energy.
a) sodium (na) has a ▼ ionization energy compared to magnesium (mg).
b) fluorine (f) has a ▼ ionization energy compared to iodine (i).

Explanation:

Step1: Recall ionization energy trends

Ionization energy generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.

Step2: Analyze part (a)

Sodium (Na) and Magnesium (Mg) are in the same period (period 3). As we move from left to right across a period, ionization energy increases because the effective nuclear charge increases, holding the electrons more tightly. Na is to the left of Mg in period 3. So Na has a lower ionization energy than Mg.

Step3: Analyze part (b)

Fluorine (F) and Iodine (I) are in the same group (group 17, halogens). As we move down a group, ionization energy decreases because the electrons are in higher energy levels (larger atomic radius), so they are farther from the nucleus and easier to remove. F is above I in group 17. So F has a higher ionization energy than I.

Answer:

a) lower
b) higher