Ch. 6 Periodic Trends

Front

What is ionization energy?

Back

The energy required to remove an electron from an atom in its gaseous state.

Front

Which element has a lower ionization energy: Calcium (Ca) or Scandium (Sc)?

Back

Calcium (Ca) has a lower ionization energy than Scandium (Sc).

Front

What happens to atomic size as you move down a group in the periodic table?

Back

Atomic size increases because atoms have more energy levels.

Front

What is the trend in ionization energy across a period?

Back

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

Front

What is electronegativity?

Back

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

Front

Which element has a higher electronegativity: Hydrogen (H) or Fluorine (F)?

Back

Fluorine (F) has a higher electronegativity than Hydrogen (H).

Front

What is the trend in atomic radius as you move across a period?

Back

Atomic radius decreases as you move from left to right across a period.

Front

What is the trend in ionic radius down a group?

Back

Ionic radius increases down a group due to the addition of energy levels.

Front

How does the number of protons affect ionization energy?

Back

As the number of protons increases, ionization energy generally increases due to greater nuclear charge.

Front

What is the relationship between ionization energy and electron affinity?

Back

Generally, elements with high ionization energy also have high electron affinity.