Question

1. explain why atomic radius decreases as you move from left to right across a period. 3. explain the trend for electronegativity as you move from left to right across a period. make sure to explain why this trend occurs.

Explanation:

2.

As you move from left - to - right across a period, the number of protons in the nucleus increases, leading to a greater nuclear charge. The electrons are added to the same energy level. The increased nuclear charge pulls the electrons closer to the nucleus, thus decreasing the atomic radius.

Electronegativity increases from left to right across a period. This is because as the number of protons in the nucleus increases (greater nuclear charge) and electrons are added to the same energy level, the nucleus has a greater ability to attract bonding electrons. The effective nuclear charge experienced by the outermost electrons increases, making the atom more likely to attract electrons in a chemical bond.

Answer:

The atomic radius decreases from left to right across a period because the increasing nuclear charge (more protons) pulls the electrons in the same energy level closer to the nucleus.

3.