Question

Use periodic trends to select the atom in each pair with the higher first ionization energy:

a) Mg
b) P
c) As
d) Sb

Answer 1

The atom with the higher first ionization energy can be determined by comparing their positions in the periodic table. Magnesium (Mg) has a higher first ionization energy compared to Aluminum (Al). Phosphorus (P) has a higher first ionization energy compared to Sulfur (S). Arsenic (As) has a higher first ionization energy compared to Selenium (Se). Antimony (Sb) has a higher first ionization energy compared to Tin (Sn).

Step-by-step explanation:

The first ionization energy is the energy required to remove one electron from a neutral atom. It tends to increase across a period from left to right, and decrease down a group from top to bottom. In the given pairs, the atom with the higher first ionization energy can be determined by comparing their positions in the periodic table.

Based on periodic trends:

- Magnesium (Mg) has a higher first ionization energy compared to Aluminum (Al).

- Phosphorus (P) has a higher first ionization energy compared to Sulfur (S).

- Arsenic (As) has a higher first ionization energy compared to Selenium (Se).

- Antimony (Sb) has a higher first ionization energy compared to Tin (Sn).