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Quiz 4 Review Chemistry

Total questions: 101

Worksheet time: 2hrs 9mins

Name
Class
Date
1.
The chemical compound of water is
a)
HO
b)
H2O
c)
H3O
d)
HO2
2.
Pure water has a
a)
Neutral pH 
b)
Negative pH
c)
Positive pH
d)
Both Negative and Positive pH
3.
A solvent is...
a)
substance into which the solute dissolves
b)
a compound being dissolved
c)
a substance that does not dissolve
d)
None of the above
4.
A Compound that is being dissolved is called a
a)
Solution
b)
Solute
c)
Solvent
d)
Suspension
5.
What is water made of?
a)
Water
b)
Liquid
c)
Hydrogen and oxygen
d)
Blue 
6.
Why can water have no net charge but have slight charges in different parts of the molecule?
a)
The oxygen end is slightly negative and the hydrogen end is slightly positive
b)
The hydrogen end is slightly negative and the oxygen end is slightly positive
c)
The hydrogen and oxygen ends change in polarity
d)
Because it is hydrophobic
7.
Attractions between water molecules are called
a)
Covalent bonds
b)
Ionic bonds
c)
Polar bonds
d)
Hydrogen bonds
8.
Which end of the water molecule has a slightly positive charge?
a)
the oxygen end
b)
the hydrogen end
c)
both ends are slightly positive
d)
neither end is positive
9.
Which types of compounds dissolve easily in water?
a)
Polar and Nonpolar
b)
Polar and Ionic
c)
Nonpolar and Ionic
d)
Covalent and Nonpolar
10.
molecule in which opposite ends have opposite electric charges
a)
cohesion
b)
polar molecule
c)
hydrogen bond
d)
solution
11.

What is an intermolecular force?

a)

Forces around molecules

b)

Gravity

c)

Forces between molecules

d)

Forces within a molecule like a covalent or ionic bond

12.

What type of solute-solvent combination is carbon dioxide in water?

a)

gas-liquid

b)

liquid-gas

c)

liquid-liquid

d)

cannot be determined

13.

A dissolved solute that does not form ions is

a)

a nonelectrolyte.

b)

a weak electrolyte.

c)

a strong electrolyte.

d)

insoluble.

14.

A solution that contains a large concentration of solute but can hold even more solute is

a)

unsaturated and dilute.

b)

saturated and dilute.

c)

unsaturated and concentrated.

d)

saturated and concentrated.

15.

It is the medium in which matter is dissolved.

a)

Solubility

b)

Solution

c)

Solvent

d)

Solute

16.

We have 3 cups of orange juice samples, based on the color which one is SATURATED?

a)

Cup A

b)

Cup B

c)

Cup C

d)

None of the Above

17.

We have 3 cups of orange juice samples, based on the color which one is SUPERSATURATED?

a)

Cup A

b)

Cup B

c)

Cup C

d)

None of the Above

18.

You make a Kool Aid drink using Kool Aid powder, sugar, & water & you notice your drink still has to much powder sitting at the bottom. What will happen if you add more water to the drink?

a)

decrease the solubility of your drink

b)

decrease the solubility rate of your drink

c)

increase the solubility rate of your drink

d)

increase the solubility of your drink

19.
What type of solution is holds more than the maximum amount of solute when it is rapidly heated & then cooled slowly producing crystals?
a)
unsaturated 
b)
saturated 
c)
supersaturated 
20.
When no more sugar will dissolve in a glass of water, the solution is...
a)
unsaturated
b)
saturated
c)
supersaturated
21.
Which salt is LEAST soluble at 0 ºC?
a)
K2Cr2O7
b)
KNO3
c)
 KClO3
d)
Ce2(SO4)3
22.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

23.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

24.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

25.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
26.
A nonelectrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
27.
When one of the parts of the solution is water we call it _________. 
a)
water stuff 
b)
water mixture 
c)
aqua-man
d)
aqueous 
28.
Solubility is a ________ property. 
a)
neat 
b)
chemical 
c)
physical 
d)
an organic 
29.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
30.

What happens when kinetic energy increases?

a)

Temperature increases.

b)

Temperature decreases.

c)

Temperature is not affected by kinetic energy.

31.

A liquid has _________ temperature than a solid.

a)

Higher

b)

Lower

32.

A gas has ________ kinetic energy than a liquid.

a)

more

b)

less

33.

A sample of a compound has a mass of 30 g and a specific heat of 0.258 J/g*K. If its temperature drops 40 K, how much heat was released? ( q=mcΔTq=mc\Delta T  )

a)

309.6 J

b)

-309.6 J

c)

465 J

d)

-465 J

34.

When water evaporates, the process is...

a)

endothermic

b)

exothermic

35.

When wood is burned in a campfire, the process is...

a)

endothermic

b)

exothermic

36.

For an exothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

37.

For an endothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

38.

In an exothermic reaction, heat is a...

a)

product

b)

reactant

39.

In an endothermic reaction, heat is a...

a)

product

b)

reactant

40.

If you touch an exothermic reaction, it will feel...

a)

hot

b)

cold

41.

If you touch an endothermic reaction, it will feel...

a)

hot

b)

cold

42.

The graph is showing an ____________ reaction.

a)

exothermic

b)

endothermic

43.

The graph is showing an _________ reaction

a)

endothermic

b)

exothermic

44.

If the system releases 150J of heat, how much heat does the surrounding absorb?

a)

-100J

b)

-50J

c)

150J

d)

100J

45.

If the reaction is endothermic, how does heat flow?

a)

System to surrounding

b)

Surrounding to system

46.

Heat will always flow from a ______ object to a ______ object.

a)

Cold to Warm

b)

Warm to Cold

c)

Cold to Cold

d)

Warm to Warm

47.

Below are the specific heats of different substances. Determine which substance will take the LONGEST to heat up.

a)

Silver: 0.22 J/gC

b)

Methanol: 2.14 J/gC

c)

Gold: 0.129 J/gC

d)

Milk: 3.89 J/gC

48.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
49.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
50.

Which of the following is NOT a factor affecting reaction rate?

a)

temperature

b)

catalysts

c)

concentration

d)

polarity

51.
Which of the following increase the reaction rate?
a)
less surface area
b)
lower temperature
c)
an inhibitor
d)
increased concentration
52.

In an exothermic reaction, heat is ...

a)

absorbed

b)

released

53.

In an endothermic reaction, heat is ,,,

a)

absorbed

b)

released

54.

What is activation energy?

a)

The maximum amount of energy used

b)

The minimum amount of energy required for a reaction to start

c)

The energy of the reactants

d)

The energy possessed by the products

55.

Which state of matter will react the SLOWEST?

a)

solid

b)

liquid

c)

gas

d)

the all react at the same rate

56.

The potential energy of the reactants is..?

a)

100 kJ

b)

250 kJ

c)

50 kJ

d)

200 kJ

57.

What is the potential energy of the products?

a)

100 kJ

b)

250 kJ

c)

50 kJ

d)

200 kJ

58.

What is the activation energy?

a)

100 kJ

b)

250 kJ

c)

50 kJ

d)

200 kJ

59.

What is the overall change in energy (ΔH)?

a)

100 kJ

b)

250 kJ

c)

50 kJ

d)

200 kJ

60.
What two factors govern whether a collision between reacting particles will be effective?
a)
orientation and potential energy 
b)
kinetic energy and temperature 
c)
kinetic energy and orientation 
d)
potential energy and kinetic energy 
61.
Which of the following factors increases only the effectiveness of collisions?
a)
temperature
b)
catalysts
c)
concentration
d)
particle size
62.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
63.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
64.
Grinding a seltzer tablet into powder increases the rate of reaction due to...
a)
increased concentration of reactants
b)
increased surface area
c)
increased speed of particles.
d)
better orientation of reactants
65.

A catalyst alters the rate of a chemical reaction by:

* Select all that apply.

a)

lowering the actvation energy

b)

making the orientation f molecules more favorable

c)

providing a surface on which the molecules react

d)

speeding up the reaction rate

66.

Which factors affect the rate of a reaction?

a)

polarity

b)

temperature

c)

presence of a catalyst

d)

concentration

e)

physical state

67.

TRUE OR FALSE:

Hydrogen bonds are very strong interactions between two atoms.

a)

True

b)

False

68.

Hydrogen Bonds typically occur between atoms of hydrogen involved in this type of bond:

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Nonpolar AND Polar Covalent

69.

Hydrogen bonds are VERY important in determining the many properties of this very important molecule

(a)  

70.

The Oxygen atoms in the molecule shown have this charge:

a)

Positive

b)

Partial Positive

c)

Negative

d)

Partial Negative

71.

The Hydrogen atoms in the molecule shown have this charge:

a)

Positive

b)

Partial Positive

c)

Negative

d)

Partial Negative

72.

Would the following compound dissolve or dissociate?

NaCl

a)

Dissolve

b)

Dissociate

73.

Would the following compound dissolve or dissociate?

CO2

a)

Dissolve

b)

Dissociate

74.

Would the following compound dissolve or dissociate?

NaOH

a)

Dissolve

b)

Dissociate

75.

Would the following compound dissolve or dissociate?

BaCl2

a)

Dissolve

b)

Dissociate

76.

Would the following compound dissolve or dissociate?

Br2

a)

Dissolve

b)

Dissociate

77.

Would the following compound dissolve or dissociate?

KClO3

a)

Dissolve

b)

Dissociate

78.

Would the following compound dissolve or dissociate?

C6H12O6

a)

Dissolve

b)

Dissociate

79.

Would the following compound dissolve or dissociate?

SO2

a)

Dissolve

b)

Dissociate

80.

Would the following compound dissolve or dissociate?

Li3N

a)

Dissolve

b)

Dissociate

81.

Would the following compound dissolve or dissociate?

KOH

a)

Dissolve

b)

Dissociate

82.

What is the process in which a solute breaks down into ions or atoms during dissolving?

a)

solvation

b)

dissolution

c)

dissociation

d)

condensation

83.

Which of the following substances dissociates into 3 ions when dissolved in water?

a)

CO2

b)

LiCl

c)

CuCl2

d)

H2O

84.

Which of the following substances dissociates into 2 ions when dissolved in water?

a)

CO2

b)

LiCl

c)

CuCl2

d)

CO

85.

____________ is the process whereby particles of a solvent completely surround the particles of a solute, disperse them throughout the solvent particles, and hold them in solution.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

86.

What attracts the negative ions of salt during dissociation?

a)

Negative ends of water

b)

Positive ends of water

c)

Neutral ends of water

d)

Positive ions of salt

87.

What is the final outcome of the dissociation process?

a)

All ions are combined

b)

All ions are separated

c)

All ions are dissolved

d)

All ions are evaporated

88.

Which part of water attracts positive ions of salt?

a)

Hydrogen ends

b)

Oxygen ends

c)

Neutral ends

d)

Both ends

89.

What is the initial step in the dissociation of ionic compounds?

a)

Heating the solution

b)

Attracting ions with water

c)

Evaporating the solution

d)

Mixing the solution

90.

What type of compounds are electrolytes?

a)

Covalent compounds

b)

Ionic compounds

c)

Metallic compounds

d)

Organic compounds

91.

Which of the following is NOT a factor that affects the rate of dissolving?

a)

Solute size

b)

Solvent temperature

c)

Stirring the solution

d)

Color of the solute

92.
Which solution would be least likely to carry an electric current?
a)
NaCl
b)
HCl
c)
C6H12O6
d)
CsI
93.

A dissolved solute that does not form ions is

a)

a nonelectroyte

b)

a weak electrolyte

c)

a strong electrolyte

d)

insoluble

94.

Table salt (NaCl) dissolves into water because...

a)

table salt is ionic and water is ionic

b)

table salt is ionic and water is polar.

c)

table salt is nonpolar and water is nonpolar too.

d)

table salt is ionic and water is nonpolar.

95.

Select the dissociation equation for LiOH and show the physical states of all species involved.

a)

LiOH(aq) --> Li+(s) + OH-(s)

b)

LiOH(s) --> Li+(aq) + OH- (aq)

c)

LiOH(s) --> Li+(aq) + O2(aq) + H2(aq)

d)

LiOH(s) --> Li+(aq) + O22-(aq) + H2+(aq)

96.

Select the dissociation equation for ZnCl2 and show the physical states of all species involved.

a)

ZnCl2(s) --> Zn2+(aq) + Cl-(aq)

b)

ZnCl2(s) --> Zn+(aq) + 2Cl-(aq)

c)

ZnCl2(s) --> Zn2+(aq) + 2Cl-(aq)

d)

ZnCl2(s) --> Zn+(aq) + Cl-(aq)

97.

Ice is ________ than water

a)

Heavier

b)

Lighter

98.

If you put an ice cube into a glass of water, the ice will ______.

a)

Float

b)

Sink

c)

Submerge

99.
What word describes when water is attracted to other substances?
a)
cohesion
b)
adhesion
c)
capillary action
d)
surface tension
100.

When water and other liquids stick together to form drops or thin films called ________________.

a)

adhesion

b)

capillary action

c)

cohesion

d)

surface tension

101.
Why does ice float?
a)
As water freezes, it expands and its density decreases.
b)
As water freezes, it takes up more hydrogen from the atmosphere, causing it to have a greater buoyancy.
c)
As water freezes, air becomes trapped between the hydrogen bonds of water molecules.
d)
As water freezes, it takes up more oxygen from the atmosphere, causing it to have a greater buoyancy.

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