Chapter 2 - 3

Question 1

How many possibilities or shapes does each atomic orbital have?

Answer 1

s - 1
p - 3
d - 5
f - 7

Question 2

How do you find the maximum amount of electrons an orbital can hold?

Answer 2

Knowing that each can hold up two 2 electrons, simply multiply by the maximum number of shapes.

Question 3

What does the azimuthal quantum number determine?

Answer 3

what kind of orbital the atom is in

s - 0
p - 1
d - 2
f - 3

Question 4

Hund’s Rule

Answer 4

Electrons will not pair up to occupy the same orbital

Question 5

Aufbau Principle

Answer 5

electrons will fill the lowest energy orbital first

Question 6

In general, valence electrons are the outer values of an atom’s electron configuration, while the core are on the inside. What is one exception to this rule?

Answer 6

d shell electrons are considered valence electrons

Question 7

What atoms are the exceptions to the electron configuration rules?

Answer 7

chromium, copper, molybdenum, gold, and silver

Question 8

Paramagnetic includes _____ electrons which are ______ to magnets.

Diamagnetic includes _______ electrons which are ____ to magnets.

Answer 8

paramagnetic - unpaired, attracted

diamagnetic - paired, repel

Question 9

T/F - The photoelectric effect is observed when a metal is hit with photons to release energy.

Answer 9

False - when a metal is hit with energy, it will emit an electron.

Question 10

Heisenberg Uncertainty Principle

Answer 10

It is impossible to determine a subatomic particle’s location and its momentum with perfect accuracy

Question 11

When ionic compounds form, the metal will give its electron to the nonmetal and become _____, while the nonmetal will become ____.

Answer 11

cation, anion

Question 12

Lattice energy

Answer 12

the energy needed to separate an ionic compound’s cations and anions

Question 13

In order to have a large lattice energy, there needs to be a ___ bond distance and ____ charge

Answer 13

short, large

Question 14

What is the formula for formal charge?

Answer 14

FC = (valence electrons) - (number of dots) - (number of lines)

Question 15

T/F? Because pi bonds are found in both double and triple bonds, these are stronger than sigma bonds, which are found in single bonds.

Answer 15

FALSE - sigma bonds are actually stronger than pi!

Question 16

In regards to bond order, an AVERAGE length that is longer is typically:

a) stronger
b) weaker
c) cannot be determined without data

Answer 16

A

Question 17

List the hybridization for the following number of “things” around a central atom - 2, 3, 4, 5, 6

Answer 17

2 - sp
3 - sp2
4 - sp3
5 - sp3d
6 - sp3d2