Chapter 7

Question 1

DIPOLE

Answer 1

Electrons within a compound that are evenly distributed

Question 2

There are extreme cases of dipoles - within an ionic compound

Answer 2

Example: Sodium chloride

Question 3

Milder Form of Diple

Answer 3

Occurs with water - in which the oxygen atom of each water molecule pulls electrons away from hydrogen atoms

Question 4

Polar Molecule Dipole

Answer 4

Oxygen side of water molecule slightly negative - Hydrogen side is slightly positive

Question 5

Ion-Dipole Attractions

Answer 5

A positive sodium ion attracts the negative side of the water molecule – a negative chloride ion attracts the positive side of water molecule

Ion-Dipole Attractions can act collectively to disrupt ionic bonds

Attractions exerted by the water molecules break the ionic bonds and pull the ions away from one another

Question 6

What Dipole Attraction is much weaker than iconic bonds?

Answer 6

Ion-Dipole Attractions

Question 7

DIPOLE-DIPOLE ATTRACTIONS (Permanent Dipoles)

Answer 7

An attraction between two polar molecules.

Question 8

Hydrogen Bond

Answer 8

An unusually strong Dipole-Dipole attraction

Also of great importance in the chemistry of large molecules, such as DNA and proteins

N, O, and F interacting with it…
DNA
Permamiuir

Question 9

DIPOLE-INDUCED DIPOLE ATTRACTIONS

Answer 9

Electrons are distributed evenly, so there is no dipole.

Temporarily uneven distribution of electrons

The resulting attraction between the permanent dipole (water) and the induced dipole (oxygen)

Question 10

What is much weaker than dipole-dipole attractions?

Answer 10

Dipole-Induced Dipole Attractions, however they are strong enough to hold relatively small quantities of oxygen dissolved in water.

Question 11

INDUCED DIPOLE-INDUCED DIPOLES ATTRACTIONS (sometimes called dispersion forces)

Answer 11

Because of randomness of electron distribution, however, at any given moment the electrons in an atom or a nonpolar molecule may be bunched to one side.

Can induce a Dipole in a nonpolar molecule, a temporary Dipole can do the same thing.

Question 12

SOLUTION

Answer 12

Homogenous mixture consisting of a single phase.

Question 13

Liquid Phase (Solutions)

Answer 13

Sugar water

Question 14

SOLID SOLUTIONS

Answer 14

Example: Gemstones

Metal alloys, which are mixtures of different metallic elements

Question 15

GASEOUS SOLUTION

Answer 15

Example: the air we breathe

Question 16

SOLVENT/SOLUTE

Answer 16

The component present in the largest amount. (SOLVENT)

Any other components (solute)

Question 17

DISSOLVING

Answer 17

Process of a solute’s mixing with a solvent

Question 18

SATURATED SOLUTION

Answer 18

A solution in which no more solute can be dissolved

Question 19

UNSATURATED SOLUTION

Answer 19

A solution that has not reached the limit of solute that will dissolve

Question 20

CONCENTRATION

Answer 20

Amount of solute dissolved per amount of solution

Question 21

One MOLE

Answer 21

Any type of particle is equal to 6.02 x 10^23 particles

Chemical amount of a substance

Question 22

MOLARITY

Answer 22

The solutions concentration expressed in moles of solute per liter solution

MOLARITY = numbers of miles of solute/liters of solution

Question 23

SOLUBILITY

Answer 23

Solutes ability to dissolve in a solvent

Depends on attractions between the fundamental particles of the solute and solvent.

Depends on attractions of solute particles for one another and attractions of solvent particles for one another

SOLUBILITY increases with increasing temp because hot water molecules have greater kinetic energy

Question 24

SOLUBLE

Answer 24

If a solute has any appreciable solubility in a solvent

Question 25

INFINITELY SOLUBLE

Answer 25

A solute that has no practical point of saturation in a given solute

Question 26

INSOLUBLE

Answer 26

A material that does not dissolve in a solvent to any appreciable extent

Question 27

SOLUBILITY OF GASES

Answer 27

Solubilities of gases in liquids decrease with increasing temperature. This effect occurs because with an increase in temperature, the solvent molecules have more kinetic energy. The solute molecules are literally ejected by the high energy solvent molecules

Question 28

Why does soap work?

Answer 28

Soap works because soap molecules have both nonpolar and polar properties. Because most of a soap molecule is nonpolar, it attracts nonpolar grime molecules via induced Dipole- induced Dipole attractions