Final Review Chapter 10

Question 0

The forces of attraction between molecules

Answer 0

Intermolecular force

Question 1

A force that tends to pull adjacent parts of a liquid’s surface together, thereby decreasing surface area to the smallest possible size

Answer 1

Surface tension

Question 2

Intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshaped pair of electrons of an electronegative atom in a nearby molecule

Answer 2

Hydrogen bonding

Question 3

What three elements does hydrogen have to be bonded to in order for hydrogen bonds to occur

Answer 3

Nitrogen
Oxygen
Fluorine

Question 4

Molecule created when the negative region in one polar molecule attracts the positive region in adjacent molecules

Answer 4

Dipole-dipole

Question 5

Intermolecular attractions resulting from the constant motions of electrons and the creation or instantaneous dipoles

Answer 5

London dispersion forces

Question 6

Explain London dispersion forces using you own words

Answer 6

Electrons go out their orbital giving the atom a momentary polarity, affecting the other molecules

Occurs with carbon dioxide and nitrogen

Question 7

Force of attraction within a molecule, holds the molecules together

Answer 7

Intramolecular forces

Question 8

Examples of intramolecular forces

Answer 8

Ionic,

Covalent, and metallic bonds

Question 9

What are the three types of intramolecular forces

Answer 9

Ionic bond, covalent bond, and metallic bond

Question 10

What are the three types of intermolecular forces

Answer 10

Hydrogen bonding, dipole dipole, and London dispersion forces

Question 11

Arrange the intermolecular and intramolecular forces from weakest to strongest

Answer 11

LDF, dipole dipole, hydrogen bonding, ionic covalent and metallic bonding

Question 12

What causes dipole dipole interactions

Answer 12

The cause of the dipole movement in a compound is due to the difference in the electron affinity of the atoms that are bonded in the compound

Question 13

Why is hydrogen bonding only possible with hydrogen

Answer 13

Hydrogen is the only element that has an exposed proton when an electron is lost
The exposure of the proton and the fact that the other element that the hydrogen is bonded to has a very high electron affinity, the compound ends up having a very strong dipole movement called hydrogen bonding

Question 14

What are the three possible elements that hydrogen atom must be attached to in order for the compound to contain hydrogen bond

Answer 14

Nitrogen
Oxygen
Fluorine

Question 15

How do London dispersion forces arise

Answer 15

Are created by a momentary polarity due to a valence electron moving out of its normal orbit

Question 16

For what type of molecules Are the London dispersion forces the only major intermolecular forces

Answer 16

Nonpolar molecules

Question 17

Are London dispersion forces relatively strong or relatively weak

Answer 17

They are the weakest force of attraction

Question 18

What causes surface tension

Answer 18

The forces of attraction from molecule molecule ( intermolecular force – hydrogen bonding ) are much stronger than the attraction for the objects that the liquid comes in contact with

Question 19

Why is ice less dense than water

Answer 19

The density of ice is less because when ice is formed the water molecules form rings that create more space between the molecules

Question 20

What is the reasoning behind chlorine being in a gaseous state bromine being in a liquid state and iodine being in a solid-state

Answer 20

London dispersion forces increase as the size of the atom increases. Since the size of the Adams increase from chlorine to bromine to iodine, forces of attraction are strong enough for the states to go from gaseous state, to liquid state to solid-state for the respective molecules