Chapter 7

Question 1

S orbital

Answer 1

1 orbital
Circular cloud

Question 2

P orbital

Answer 2

3 orbitals
Figure 8

Question 3

D orbital

Answer 3

5 orbitals
2 figure 8’s

Question 4

F orbital

Answer 4

7 orbitals
Complex form of a figure 8

Question 5

What makes an atom more paramagnetic?

Answer 5

It has more unpaired electrons

Question 6

Coulombic force of attraction

Answer 6

The force of attraction between the negative electrons in the shells, and the positive protons in the nucleus

Question 7

Effective nuclear charge

Answer 7

The charge that of the nucleus that an electron actually experiences

Question 8

Shielding electrons

Answer 8

Block the outer electrons of an atom from feeling the full nuclear charge

Question 9

Equation for effective nuclear charge:

Answer 9

Zeff= atomic # - # of shielding electrons

Question 10

Atomic radius trend

Answer 10

• Decreases across a group because atoms gain protons and electrons are pulled closer into the nucleus
• Increase down a group because the number of shells increase

Question 11

First ionization energy definition

Answer 11

The minimum amount of energy needed to remove one electron from an atom’s valence shell

Question 12

First ionization energy trend

Answer 12

• Increases across a period because there are more valence electrons
• Decreases down a group because there are more shells and as the valence electrons get farther from the nucleus, they are easier to remove

Question 13

First ionization energy anomalies

Answer 13

Groups 2 and 3: Group 3 atoms have a lower first ionization energy than group 2 because their electrons are in the p orbital and therefore slightly farther from the nucleus
Groups 15 and 16: Group 15 has all unpaired electrons so they are slightly harder to remove since there are less repelling forces in the atom

Question 14

Electronegativity definition

Answer 14

A measure of how much an atom attracts electrons to bind with it

Question 15

Electronegativity trend

Answer 15

• Increases across a period because there are more valence electrons that want to gain an electron
• Decrease down a group because the electrons get farther from the nucleus so it’s harder for the nucleus to pull in electrons

Question 16

Electron affinity defintion

Answer 16

The likelihood of an atom to gain an electron

Question 17

Electron affinity trend

Answer 17

• Increases across a period because there are more valence electrons that want to gain an electron
• Decrease down a group because the electrons get farther from the nucleus so it’s harder for the nucleus to pull in electrons

Question 18

Metal reactivity

Answer 18

Metals are typically oxidized (lose electrons)

Question 19

Metal reactivity trend

Answer 19

• Decreases across a period because there are more valence electrons making them harder to remove
• Increases down a group because there is more distance from the nucleus and therefore the electrons are easier to remove

Question 20

Non-metal reactivity

Answer 20

Non-metals are typically reduced (gain electrons)

Question 21

Non-metal reactivity trend

Answer 21

• Increases across a period because there are more valence electrons that are closer to having full shells
• Decreases down a group because as the electrons get farther from the nucleus, the nucleus has less of a pull

Question 22

Isoelectronic definition

Answer 22

Particles with the same number of electrons

Question 23

Hund’s rule

Answer 23

A single electron must be placed into each orbital before any pairing takes place

Question 24

Pauli exclusion principal

Answer 24

No more than 2 electrons in each orbital, electrons must have opposite spins

Question 25

Aufbau principal

Answer 25

Electrons must fill the lowest available orbitals before moving to the higher ones