chem 106 quiz 2

Question 1

types of crystalline solids

Answer 1

molecular, ionic, atomic, network

Question 2

molecular solids examples

Answer 2

H2O, CO2

Question 3

ionic solids example

Answer 3

NaCl

Question 4

atomic solids examples

Answer 4

metals; Ar(s)

Question 5

network solids examples

Answer 5

diamond, graphite

Question 6

the melting point of ionic solids is (less than/equal to/greater than) molecular solids

Answer 6

greater than (b/c ionic bonds over IMFs)

Question 7

example of liquid solution with liquid solvent and gas solute

Answer 7

CO2(g) in H2O(l)

Question 8

example of liquid solution with liquid solvent and solid solute

Answer 8

NaCl(s) in H2O(l)

Question 9

example of liquid solution with liquid solvent and liquid solute

Answer 9

ethanol(l) in H2O(l)

Question 10

example of solid solution with solid solvent and solid solute

Answer 10

Iron(s) in Carbon(s) (steel)

Question 11

example of solid solution with solid solvent and liquid solute

Answer 11

Mercury(l) in Silver(s) (amalgam)

Question 12

example of solid solution with solid solvent and gas solute

Answer 12

H2(g) in Pd(s)

Question 13

what are the catalyst metals?

Answer 13

Ni, Pd, Pt

Question 14

solution form when

Answer 14

the attractive forces between solvent and solute are greater than the interactions between the solute and itself; “like dissolves like”

Question 15

oil and water do not mix because

Answer 15

oil is nonpolar and water is polar

Question 16

the ΔHsolution =

Answer 16

ΔHsolute + ΔHsolvent + ΔHmixture

Question 17

in the equation ΔHsolution = ΔHsolute + ΔHsolvent + ΔHmixture, what are the signs on each?

Answer 17

-, +, +, -

Question 18

Henry’s Law

Answer 18

Solubility,gas = k * P,gas

Question 19

solubility and pressure are (directly/inversely) related

Answer 19

directly

Question 20

Henry’s constant, k, has to do with

Answer 20

solubility and intermolecular forces (units will be solubility/pressure)

Question 21

Henry’s constant and solubility are (directly/inversely) related

Answer 21

directly

Question 22

polarizability

Answer 22

ability to form instantaneous dipoles

Question 23

why is CO2 soluble in H2O since it’s nonpolar?

Answer 23

it has a high polarizability

Question 24

polarizability increases with

Answer 24

size

Question 25

why do scuba divers have to pace themselves upon ascending?

Answer 25

N2 tries to bubble out of blood - too much in system because need more at higher pressure/the lower you go

Question 26

mass percent equation

Answer 26

mass solute / total mass

Question 27

parts per million equation

Answer 27

mass component / mass solution x 10^6

or mg/kg

Question 28

mole fraction

Answer 28

moles solute / total moles

Question 29

molarity

Answer 29

moles solute / volume solution

Question 30

molality

Answer 30

moles solute / mass solvent

Question 31

for a really concentrated solution, (molarity/molality) increases faster

Answer 31

molality

Question 32

temperature affects (molarity/molality)

Answer 32

molarity

Question 33

adding a solute to a solvent (lowers/raises) the vapor pressure of the solvent & why

Answer 33

lowers; the solute is blocking the vaporization (?)

Question 34

P,A = ?

Answer 34

(X,A)(P*,A) (mole fraction times vapor pressure of pure substance)

Question 35

vapor pressure of the solution decreases with (decreasing/increasing) mole fraction

Answer 35

decreasing

Question 36

lower vapor pressure leads to a (lower/higher) boiling point

Answer 36

lower

Question 37

alcohol by weight

Answer 37

g solute/g solvent ?