chapter7

Question 1

Any sample of matter is either a

Answer 1

pure substance or a mixture of pure substances.

Question 2

Suspension

Answer 2

a mixture i which particles of a material are more or less evenly dispersed throughout a liquid or gas.

Question 3

Colloid

Answer 3

a mixture consisting of tiny particles that are intermediate in size between those in solutions and those in suspensions, and that are suspended in a liquid, solid, or gas.

Question 4

emulsion

Answer 4

a colloid in which liquids that normally don’t mix are spread throughout each other.

Question 5

solution

Answer 5

is a homogenous mixture of two or more substances uniformly dispersed throughout a single phase.

Question 6

Solute

Answer 6

the substance that dissolves in the solvent.

Question 7

Solvent

Answer 7

the substance in which the solute dissolves.

Question 8

miscible

Answer 8

liquids mix to form solutions.
Miscible fluids may be separated by distillation, but only if the mixtures have different boiling points.

Ex. Alcohol and water are miscible with each other.

Question 9

Alloy

Answer 9

a solid or liquid mixture of two or more metals. Alloys aren’t chemically combined.

Question 10

Polar Compound

Answer 10

a molecule that has an uneven distribution of electrons. Ex. H2O.

Question 11

Dissolving depends on forces between particles

Answer 11

To dissolve an ionic substance, water molecules must except a force on the ions that is more attractive than the force between the ions in the crystal.

Question 12

Hydrogen Bonding

Answer 12

the intermolecular force occurring when a hydrogen atom that is bonded to a highly electronegative atom of on molecule is attracted to two unshared electrons of another molecule.

Question 13

Non-polar compound

Answer 13

a compound whose electrons are evenly distributed among its atoms.

Question 14

By kinetic theory of matter, solvent molecules collide and transfer energy to the solute molecule at the surface of the crystal.

Answer 14

This energy and the attractive forces between the solute and solvent molecules causes the surface of the crystal to dissolve.

Question 15

By the kinetic theory of matter, solutes dissolve faster when the solvent is hot —

Answer 15

cuz of faster moving molecules.

Question 16

Concentration

Answer 16

the amount of a particular substance in a given quantity of a mixture, solution, or ore.

Question 17

unsaturated solution

Answer 17

a solution that hasn’t reached the saturation point at given temperature & is able to dissolve additional solute

Question 18

Saturated solution

Answer 18

a solution that cannot dissolve any more solute under the given conditions.

Question 19

Supersaturated solution

Answer 19

a solution that holds more dissolved solute than it otherwise would at a given temperature.

Normally achieved by saturating the solution at a higher T and then letting it cool. It will hold all that solute. A single extra atom of the solute will cause the solute to precipitate, until the actual saturation point for the given T.

Question 20

Solute crystalizes out until

Answer 20

the solution reaches the new saturation point for the cooler temperature. i.e. until the new (lower) saturation point is reached at a lower temperature

Question 21

Molarity

Answer 21

the concentration of a solution in moles of dissolved solute per liter of solution.
Molarity = moles of solute/ liters of solution, or M = mol/L.