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Chem final review

Total questions: 72

Worksheet time: 1hrs 26mins

Name
Class
Date
1.

The molar volume of a gas at STP occupies _____________.

a)

22.4 L

b)

0˚C

c)

1 kiloPascal

d)

12 grams

2.

In a double replacement, ____________________

a)

The reactants are usually a metal and a nonmetal

b)

One of the reactants is often water

c)

The reactants are generally 2 ionic compounds in aqueous solutions

d)

Energy in the form of light or heat is often produced

3.

If 7.00 grams of nitrogen gas are contained in a 5.00 L flask at 4.62 kPa. What is the temperature of the gas?

a)

11.1 K

b)

1.00 K

c)

4.12 K

d)

9.07 K

4.

Which of the following statements is NOT true about what happens in all chemical reactions?

a)

The ways in which atoms are joined together change

b)

New atoms are formed as products

c)

The starting substances are called reactants

d)

The bonds of reactants are broken and new bonds of products are formed

5.

Chemical equations must be balanced to satisfy ____.

a)

The law of definite proportions

b)

The law of multiple proportions

c)

The law of conservation of mass

d)

Avogadro's principle

6.

What are the coefficients that will balance the skeleton equation below?

AlCl3 + NaOH → Al(OH)3 + NaCl

a)

1,3,1,3

b)

3,1,3,1

c)

1,1,1,3

d)

1,3,3,1

7.

How many moles of aluminum are needed to react completely with 1.2 mol of FeO?

2Al(s) + 3FeO(s) → 3Fe(s) + Al2O3(s)

a)

1.2 mol

b)

0.8 mol

c)

1.6 mol

d)

2.4 mol

8.

When an equation is used to calculate the amount of product that could form during a reaction, then the value obtained is called the ____.

a)

Actual yield

b)

Percent yield

c)

Minimum yield

d)

Theoretical yield

9.

The equation 2C3H7OH + 9O2 → 6CO2 + 8H2O is an example of which type of reaction?

a)

Combustion reaction

b)

Single replacement reaction

c)

Double replacement reaction

d)

Decomposition reaction

10.

How many significant figures would the product of the following numbers have: 202 x 20 x 40.121

a)

1

b)

2

c)

3

d)

4

e)

5

11.

How many significant figures are there in the number 0.0100?

a)

1

b)

2

c)

3

d)

4

e)

5

12.

How many feet are there in 120 meters? (1m = 100 cm, 1 inch = 2.54 cm, 12 inches = 1 foot)

a)

390 ft

b)

393 ft

c)

4716 ft

d)

394 ft

13.

Which target demonstrates high precision, but low accuracy?

a)

A

b)

B

c)

C

d)

D

14.

Which subatomic particle can be found inside the nucleus?

a)

electron

b)

proton

c)

neutron

d)

both proton and neutron

15.

If a nitrogen atom gained three electrons to have a full valence shell, what charge would it have?

a)

+3

b)

-3

c)

+1

d)

-1

16.

Which energy level would be occupied by electrons with the LEAST amount of energy?

a)

E1

b)

E2

c)

E3

d)

E4

17.

What is the symbol for this element?

a)

C

b)

Be

c)

N

d)

P

18.

How many UNPAIRED, or lone, electrons does the Lewis structure for Nitrogen have?

a)

1

b)

2

c)

3

d)

4

19.

What type of chemical bond does lithium chloride have?

a)

ionic

b)

covalent

c)

metallic

20.

What is the chemical formula for silver nitrate?

a)

Ag(NO3)2

b)

Ag2(NO3)

c)

AgNO3

d)

AgN

21.

How many valence electrons do elements in Group 17 of the periodic table have?

a)

1

b)

2

c)

3

d)

7

22.

Which is the correct formula and charge of nitrate?

a)

NO3+1

b)

NO3-1

c)

NO2-1

d)

NO2+1

23.

What is the molar mass of H2O?

a)

37.01

b)

18.02

c)

1.01

d)

16.00

24.

What is the molar mass of lithium carbonate?

a)

73.89

b)

54.23

25.

How many moles is 212 g of H2O?

a)

11

b)

12

c)

11.8

d)

11.76

26.

What is the mole to mole ratio of Mg to O2 , in the balanced equation of 2 Mg + O2 --> 2 MgO

a)

1 to 1

b)

2 to 1

c)

1 to 2

d)

2 to 2

27.

In the balanced equation of 2 Mg + O2 --> 2 MgO, if 25.30 g of Mg reacted, how many moles of O2 reacted?

a)

0.5204

b)

0.7021

c)

2.308

d)

0.702

e)

0.52

28.
An isotope has a different number of
a)
electrons
b)
neutrons
c)
protons
d)
positrons
29.
The average atomic mass for silicon will be closest to...
a)
Si-28 (92% abundance)
b)
Si-29 (5% abundance)
c)
Si-30 (3% abundance)
30.
The Law of Conservation of Mass is not always followed with nuclear reactions.
a)
True
b)
False
31.
Which of the following is an example of nuclear fusion? 
a)
A plutonium atom is used to start a chain reaction that detonates a nuclear weapon 
b)
A uranium atom is split apart into lighter elements
c)
 Two hydrogen atoms are combined to form a helium atom
d)
Two hydrogen atoms bond with an oxygen atom to form a water molecule 
32.
Which type of nuclear radiation is being emitted here along with Rn
a)
alpha
b)
beta
c)
gamma
d)
none
33.

Calculate ΔT\Delta T  when a substance goes from 10*C to 75*C

a)

-65*C

b)

75*C

c)

10*C

d)

65*C

34.

Calculate A 50g sample is heated with 500 joules of energy and has a 10*C temperature change. Calculate it’s specific heat.

a)

1 j/g*C

b)

250000 j/g*C

c)

500 j/g*C

d)

10 j/g*C

35.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

36.

What does q stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

37.

A solid is a state of matter that has a(n)

a)

indefinite volume and indefinite shape

b)

definite volume and a definite shape

c)

definite volume and an indefinite shape

d)

indefinite volume and a definite shape

38.
In which state of matter are particles packed tightly together in fixed positions?
a)
gas 
b)
solid
c)
liquid
d)
plasma
39.
Particles of a liquid
a)
are tightly packed together and stay in a fixed position
b)
have no viscosity
c)
decrease in volume with increasing temperature
d)
are free to move in a container but are in close contact with one another
40.
In which state of matter do particles spread apart and fill all the space available to them? 
a)
crystal
b)
liquid
c)
gas
d)
solid
41.
The change from a  liquid to solid, or the reverse of melting, is called
a)
condensation
b)
boiling
c)
sublimation
d)
freezing
42.

In which state of matter are the particles least able to move?

a)

A

b)

B

c)

C

43.

Which of these three states represents a liquid?

a)

A

b)

B

c)

C

44.
How many significant figures does the following number have?
0.00345
a)
6
b)
5
c)
3
d)
Ambiguous: 3,4,5, or 6
45.
How many significant figures does the following number have: 0.00204
a)
6
b)
4
c)
3
d)
2
46.

How many significant figures does the following number have?1.2500 x 10310^3  

a)
5
b)
3
c)

Ambiguous: 3 or 5

d)

7

47.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
48.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
49.
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
50.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
51.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
52.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
53.

How many grams are in 7.8 moles of NaCl?

a)

476 grams

b)

460 grams

c)

452 grams

d)

462 grams

54.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
55.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
 
1 Mg +  2 HCl --> 1 MgCl2  +  1 H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
56.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
57.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

58.

Look at this picture of Argon off the periodic table. Which of the following is true for this element?

a)

18 protons

b)

40 protons

c)

22 protons

d)

21.9 protons

59.

The atomic mass of an atom is equal to

a)

number of protons plus number of neutrons

b)

number of protons plus number of electrons

c)

number of electrons plus the number of neutrons

60.
The term "neutral" means
a)
having only a little bit of charge
b)
having a positive charge
c)
having a negative charge
d)
having no charge at all
61.
What is true about an atom?
a)
Most of the space in an atom is taken up by the nucleus
b)
Atoms are mostly empty space
c)
Atoms have no mass
d)
Electrons have much more mass that protons or neutrons.
62.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
63.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

64.

What is the light that you can see called?

a)

observatory light

b)

ultraviolet light

c)

visible light

d)

infrared light

65.

Diagram below shows

a)

Emission spectrum

b)

Absorption spectrum

c)

Line absorption spectrum

66.
The _______________ determines the color of visible light. 
a)
wavelength
b)
speed
c)
amplitude
d)
light
67.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
68.
When talking about energy levels in an atom, what is an "excited state"?
a)
The highest energy state of an atom.
b)
Any level higher than the ground state.
c)
The lowest energy state of an atom.
d)
When an atom loses an electron
69.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

70.
The parallel lines represents...
a)
energy levels of the atom
b)
energy levels of the electrons
c)
energy levels of the photons
d)
energy levels of the nucleus
71.
The blue section of the wave is measuring _________________.
a)
wavelength
b)
crest
c)
trough
d)
amplitude 
72.

Which scientist is credited with the discovery of atomic energy levels?

a)

Bohr

b)

Thomson

c)

Rutherford

d)

Bunsen

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