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Chemistry Final Exam

Total questions: 65

Worksheet time: 5hrs 25mins

Name
Class
Date
1.
While performing lab using acids and bases you accidentally splash acid all over your face.  What piece of safety equipment should you use immediately?
a)
fire blanket
b)
fire extinguisher
c)
eye wash station
d)
safety shower
2.

Which equipment heats liquids and some stir liquids?

a)

beaker

b)

graduated cylinder

c)

flask

d)

hot plate

3.

What does it mean when you see this lab safety symbol?

a)

working with glassware/chemicals

b)

wear goggles

c)

working with sharp objects

d)

working with electricity

e)

working with chemicals

4.

Which scientist's model is referred to as the Plum Pudding Model?

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

5.

Which scientist performed the Gold Foil Experiment??

a)

Democritus

b)

John Dalton

c)

Ernest Rutherford

d)

J.J. Thomson

e)

Niels Bohr

6.

Which subatomic particle has a positive charge?

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

7.

Which of the following represents protons on the periodic table?

a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
8.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
9.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)

Subtract the number of the atomic number from the mass number

d)
Add the mass number to the number of e-
10.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

11.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

12.

Oxygen has 6 valence electron. It will have a charge of _______.

a)

+1

b)

-1

c)

+2

d)

-2

13.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

14.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

15.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

16.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

17.

Elements that have the same number of energy levels are said to be in the same ______.

a)

group

b)

period

c)

family

d)

classification

18.
Which of the following is the most reactive group of metals? 
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Transition Metals
19.
What group on the Periodic Table contains the elements of the alkaline earth family?
a)
1
b)
2
c)
17
d)
18
20.
Gold (Au)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Earth Metal
d)
Heavy Metal
21.

As you move across the period, atoms tend to get _______ because the positively charged _______ pull the electrons closer to the nucleus.

a)

bigger,

electrons

b)

smaller,

protons

c)

smaller,

neutrons

d)

bigger,

protons

22.

Electronegativity is the measure of the ability of an atom in a compound to attract. _______.

a)

Electrons

b)

Protons

c)

Neutrons

23.

Which shows increasing electronegativity?

a)

F, Cl, Br, I

b)

Ba, Mg, Cl, F

c)

Cl, Si, Al, Na

d)

O, Se, K, Rb

24.

A substance that may have properties of both metals and nonmetals is called a --

a)

Metal

b)

Nonmetal

c)

Metalloid

25.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
26.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
27.

The maximum number of electrons that can be placed in the p subshell.

a)

2

b)

6

c)

10

d)

14

28.

Which is not true about the liquid state of matter?

a)

The liquid state has a definite volume and a definite shape.

b)

The liquid state takes on the shape of its container.

c)

The liquid state has a definite volume and an indefinite shape.

d)

The particles in a liquid can easily move past each other.

29.

Which process could cause a material to change state from gas to liquid?

a)

Adding heat

b)

Adding energy

c)

Removing particles

d)

Removing energy

30.

Oil and water are each homogeneous mixtures. What happens to them when they are mixed?

a)

They form a heterogeneous mixture.

b)

They form a pure substance.

c)

They form a phase.

31.
Frank has a paper clip. It has a mass of 9g and a volume of 3cm3. What is its density?
a)
3 g/cm3
b)
1/3 g/cm3
c)
27 g/cm3
d)
39 g/cm3
32.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
33.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
34.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
35.
How many electrons are needed in the outer energy levels of an atom to be stable?
a)
2
b)
4
c)
6
d)
8
36.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

37.

Formula for iron (II) carbonate

a)

FeCO3

b)

Fe2CO3

c)

FeCO2

d)

Fe2CO2

38.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
39.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
40.

In the equation, 2Mg + O2 ---> 2MgO, which are the reactants?

a)

Mg and O

b)

Mg and MgO

c)

MgO

d)

O and MgO

41.

Balance the following equation:

___ Mg+ ___ O2→___ MgO

a)

1, 1, 3

b)

2, 1, 2

c)

1, 2, 1

d)

2, 2, 2

42.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
43.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
44.

The substance being dissolved in a solution is the?

a)

solution

b)

solute

c)

solvent

d)

mixture

45.

If I dissolve carbon dioxide in water, what is the solvent?

a)

Carbon Dioxide

b)

There is no solvent

c)

Oxygen

d)

Water

46.

How does a solution become supersaturated?

a)

by pouring lots of solute in it then stirring.

b)

dissolve a little solute in it and stir.

c)

heat the solution to make it dissolve more solute and then cool it down.

d)

dissolve a small amount of solvent in it then heat it up.

47.

CaCl2

a)

Soluble

b)

Insoluble

48.

Mg(OH)2

a)

Soluble

b)

Insoluble

49.

Which is the correct net ionic equation for the reaction of:

AgNO3 (aq) + CaCl2 (aq) -> AgCl (s) + Ca(NO3)2 (aq)

a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
50.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
51.

What effect does increasing the surface area have on the rate of a chemical reaction?

a)

No effect on the reaction rate

b)

Decreases the reaction rate

c)

Increases the number of collisions

d)

Decreases the number of collisions

52.

What happens to the reaction rate when the temperature is increased?

a)

Increases due to more frequent collisions

b)

Remains the same

c)

Decreases due to lower kinetic energy

d)

Decreases due to fewer collisions

53.

2 NaClO3 (s) → 2NaCl (s) +3 O2 (g)

How many grams of O2 will be produced from 12.00 moles of NaClO3?

a)

256 g of O2

b)

576 g of O2

c)

288 g O2

d)

32 g O2

54.
What is the molar mass of (NH4)2CO3 ?
a)
144 g
b)
138 g
c)
96 g
d)
78 g
55.

Identify the limiting and excess reactants in the reaction shown.

a)

O2 is limiting and H2 is excess. 

b)

H2 is limiting and O2 is excess. 

c)

O2 is both limiting and excess.

d)

There is no limiting reactant. 

56.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
57.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
58.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
59.

Find the percentage composition of Mg in Mg3(PO4)2.


a)

27.48% Mg

b)

43.11% Mg

c)

16.00% Mg

d)

12.63% Mg

60.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

61.

What is the molecular formula of a compound that has an empirical formula of C4H4O. The molar mass of the molecular formula is 136 g/mol.

a)

C12H12O3

b)

C24H24O6

c)

C16H16O4

d)

C8H8O2

62.

A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?

a)

Mg4N3

b)

MgN2

c)

Mg3N2

d)

MgN

63.

What is the molarity of a solution prepared by dissolving 58.5 grams of NaCl in enough water to make 0.5 liters of solution? (Molar mass of NaCl = 58.5 g/mol)

a)

0.5 M

b)

1.0 M

c)

2.0 M

d)

4.0 M

64.

How many moles of solute are present in 250 mL of a 2.0 M solution?

a)

0.25 moles

b)

0.5 moles

c)

1.0 mole

d)

2.0 moles

65.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

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