Ch. 5 - Electron Configuration and Periodic Trends

Question 1

What does the spin magnetic quantum number describe?

Answer 1

The direction of the spin of the electron. (m_s)

Question 2

What are the allowed values for m_s?

Answer 2

1/2 or -1/2.

Question 3

When is a substance diamagnetic?

Answer 3

When all the electrons are paired, they are repelled by magnetic fields.

Question 4

When is a substance paramagnetic?

Answer 4

When one or more electron is unpaired, they are attracted to magnetic fields.

Question 5

What is the Pauli exclusion principle?

Answer 5

Only two electrons with opposite spin direction may occupy each orbital.

Question 6

How many electrons can an s subshell have?

Answer 6

2

Question 7

How many electrons can a p subshell have?

Answer 7

6

Question 8

How many electrons can a d subshell have?

Answer 8

10

Question 9

How many electrons can an f subshell have?

Answer 9

14

Question 10

What is Hund’s Rule?

Answer 10

Assign one electron to each orbital then go back and add a second electron once all orbitals are half full.

Question 11

[!] What is the effective nuclear charge?

Answer 11

The amount of positive charge felt by an electron in a given orbital. (Z_eff)

Question 12

What is the periodic trend of effective nuclear charge?

Answer 12

Effective nuclear charge increases with atomic number.

Question 13

What is the covalent radius?

Answer 13

Half the distance between the nuclei of two identical atoms joined by a single covalent bond.

Question 14

What is the metallic radius?

Answer 14

Half the distance between the two nuclear of two adjacent atoms in the crystalline solid metal.

Question 15

What is the van der Waals radius?

Answer 15

Half the distance between the nuclei of two adjacent atoms in a solid sample of noble gas.

Question 16

What is the periodic trend of atomic radius?

Answer 16

Atomic radius increases from top to bottom and from right to left on the periodic table.

Question 17

What is first ionization energy?

Answer 17

The energy that must be absorbed in order to remove a valence electron from a neutral atom in the gas phase. (E_i)

Question 18

What is the periodic trend of the first ionization energy?

Answer 18

First ionization energy increases from bottom to top and from left to right on the periodic table.

Question 19

What is second ionization energy?

Answer 19

The energy that must be absorbed to remove a valence electron from a cation (+1) in the gas phase. (E_i2)

Question 20

What is electron affinity?

Answer 20

The energy released when a neutral atom in the gas phase acquired an extra electron in the lowest energy orbital available. (E_ea)

Question 21

What is the periodic trend of electron affinity?

Answer 21

Electron affinity increases from bottom to top and from left to right on the periodic table.

Question 22

What is electronegativity?

Answer 22

The ability of an element to hold onto its own electrons and attract electrons from other elements. (χ)

Question 23

What is the periodic trend of electronegativity?

Answer 23

Electronegativity increases from bottom to top and from left to right on the periodic table.