Unit 7

Question 1

bHow to draw Lewis Dot Structures?

Answer 1

1. Identify the central atom (aka the atom we have one of).
2. If there is more than one, they will be next to eachother.
3. Draw the central atom in the center and the other atoms around it.
4. Add the valence electrons and bond to satisfy octet rule.

Question 2

Which atom(s) only need 2 valence electrons to be stable?

Answer 2

Hydrogen and Helium.

Question 3

Which atom(s) only need 6 valence electrons to be stable?

Answer 3

Aluminum and Boron.

Question 4

What does charges mean in the formula?

Answer 4

Signifies the amount of electrons gained or removed. Negative is gained and positive is removed.

Question 5

How must you draw the electrons?

Answer 5

Don’t leave two electrons separate, combine them.

Question 6

VSEPR Linear structure

Answer 6

Central atom is bonded twice with NO lone pairs. 180 degrees

Question 7

VSEPR Trigonal planar

Answer 7

Central atom is bonded three times with NO lone pairs. 120 degrees.

Question 8

VSEPR Tetrahedral

Answer 8

Central atom is bonded four times with NO lone pairs. 109.5 degrees bond angle

Question 9

VSEPR Bent

Answer 9

ONE lone pair = 120 degrees
TWO lone pairs = 109.5 degrees

Question 10

VSEPR Trigonal pyramidal

Answer 10

Central atom is bonded three times with ONE lone pair. 109.5 degrees.

Question 11

The three different types of bonds

Answer 11

Ionic
Polar covalent
Nonpolar covalent

Question 12

Polar covalent bonds

Answer 12

CAN contain a dipole.
Difference in electronegativity of the atoms is greater than 0.5 but less than 1.67.

Question 13

Nonpolar covalent bonds

Answer 13

Difference in electronegativity of the atoms is less than 0.5.

Question 14

Ionic bonds

Answer 14

Difference in electronegativity of the atoms is greater than 2.0.

Question 15

What symbol goes over the molecule with greater electronegativity?

Answer 15

-

Question 16

What symbol goes over the molecule with less electronegativity?

Answer 16

+

Question 17

Dipole

Answer 17

Caused by a difference in electronegativity where one part of the molecule becomes slightly negative and the other becomes slightly positive.

Question 18

Intramolecular forces

Answer 18

The two main categories of bonds that occur within a molecule. Covalent (Polar and nonpolar) and ionic bonds.

Question 19

Intermolecular forces

Answer 19

Affect the boiling point. The higher the IMF, the higher the boiling point. They determine whether a molecule will dissolve in a particular solvent. Polar molecules dissolve in polar solvents.

Question 20

Types of IMF

Answer 20

Dipole-Dipole. Strong
Hydrogen bonding (a type of dipole-dipole) Strongest
London Dispersion Forces (LDF) Weakest

Question 21

Dipole-Dipole

Answer 21

ONLY polar covalent molecules withe a dipole.
Molecules with a dipole can be attracted to other molecules with dipoles.
- 2nd strongest IMF

Question 22

Hydrogen bonding

Answer 22

ONLY polar covalent molecules withe a dipole.
This time molecules that bond hydrogen with F.O.N. (Fluorine, oxygen, nitrogen)
- Strongest IMF

Question 23

London Dispersion Forces (LDF)

Answer 23

Between molecules with NO DIPOLE and always (but no exclusively) nonpolar covalent molecules and sometimes polar covalent.
There are some attraction to other molecules, known as temporary dipoles.
- Higher mass, stronger dipole
- Weakest IMF