Chapter 7

Answer 1

Atomic and ionic radii decrease across a period from left to right due to increasing nuclear charge.

Answer 2

Atomic and ionic radii increase down a group from top to bottom due to the addition of electron shells.

Question 3

What are properties of metals?

Answer 3

Shiny luster, conduct heat and electricity, malleable and ductile, solids at room temperature (except mercury,) low ionization energies/form cations easily

Question 4

What is ionization energy?

Answer 4

The ionization energy is the minimum energy required to remove an electron from the ground state of a gaseous atom or ion.

Question 5

With each successive electron, does it get more or less difficult to remove the next electron?

Answer 5

It requires more energy to remove each successive electron. When all valence electrons have been removed, it takes a great deal more energy to remove the next electron (a core electron).

Question 6

What are the periodic trends in First ionization energy?

Answer 6

Generally increases across a period and generally decreases down a group.

Question 7

What factors influence ionization energy?

Answer 7

Smaller atoms have higher I values, I values depend on effective nuclear charge and average distance of the electron from the nucleus.

Question 8

What are the electron configurations of cations?

Answer 8

Cations: The electrons are lost from the highest energy level (n value).

Question 9

What are the electron configurations of anions?

Answer 9

The electron configurations are filled.

Question 10

What is electron affinity?

Answer 10

Electron affinity is the energy change accompanying the addition of an electron to a gaseous atom.

Question 11

What is the general trend in electron affinity?

Answer 11

Not much change in a group. Across a period, it generally increases.