Advanced Chem - Unit 2 Review Part 4: Periodic Table & Periodic Trends

Front

What is the most important factor affecting the attraction between the outermost electrons and the nucleus?

Back

The distance between the nucleus and outermost electrons.

Front

What happens to the atomic radius of group 1 elements as you move from top to bottom?

Back

Each successive element has a larger atomic radius and higher shielding effect.

Front

What is ionization energy?

Back

The energy required to remove an electron from a specific atom.

Front

Which element has a higher ionization energy than arsenic (As, #33)?

Back

Neon (Ne, #10).

Front

Why does chlorine (Cl) have the highest electronegativity in Period 3?

Back

Cl has the most protons and the same number of energy levels.

Front

What is the trend in ionization energy across a period in the periodic table?

Back

Ionization energy generally increases from left to right across a period.

Front

What is the trend in atomic radius down a group in the periodic table?

Back

Atomic radius generally increases as you move down a group.

Front

Define electronegativity.

Back

Electronegativity is a measure of the ability of an atom to attract electrons in a chemical bond.

Front

What is the relationship between nuclear charge and atomic size?

Back

As nuclear charge increases, atomic size generally decreases due to increased attraction between the nucleus and electrons.

Front

What is shielding effect?

Back

The shielding effect is the reduction in effective nuclear charge on the electron cloud, due to the presence of other electrons.