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Honors Chem Semester Review (Ch 1-5)

Total questions: 75

Worksheet time: 3hrs 1mins

Name
Class
Date
1.

The outside temperature is 290 C. What is the temperature in Kelvin?

a)

302 K

b)
290 K
c)
300 K
d)
310 K
2.

Choose the pure substance from the list:

a)

gatorade

b)

sea water

c)

fluorine

d)

smoothie

3.

Which one of the following is a chemical change?

a)

leaves changing color in the fall

b)

water freezing

c)

oil boiling

d)

ice melting

4.

Which one of the following is a chemical property?

a)

The boiling point of water is 100oC

b)

Potassium reacts explosively with water

c)

Water melts at 0oC

d)

Condensation forms on the outside of a glass

5.

Round the following number to 3 significant figures: 29,318

a)

29,300

b)

293

c)

293.00

d)

2.9318 x 105

6.

An object has a mass of 16.0 g and a volume of 3.81 mL. What is the density of the object in g/mL?

a)

3.199 g/mL

b)

0.199 g/mL

c)

60.96 g/mL

d)

4.20 g/mL

7.

An object has a density of 3.30 g/mL, and a mass of 22.4 g. What is the volume of this object?

a)

6.79 mL

b)

73.92 mL

c)

0.147 mL

d)

0.587 mL

8.

Convert and show your work with units: 3.56 miles to ft.

(1 mile = 5,280 feet)

a)

3.565280=6.74x10−4\frac{3.56}{5280}=6.74x10^{-4}

b)

3.56mi(1.0ft5280 mi)=18796.8 ft3.56mi\left(\frac{1.0ft}{5280\ mi}\right)=18796.8\ ft

c)

3.56mi(5280ft1.0 mi)=18796.8 ft3.56mi\left(\frac{5280ft}{1.0\ mi}\right)=18796.8\ ft

d)

5280ft3.56 mi=1483 ft\frac{5280ft}{3.56\ mi}=1483\ ft

9.

Correctly show your work to convert 153kg to mg using the factors in Table 1.3 of the textbook.

a)

153kg(1.0 g103 kg)(1.0mg10−3g)153kg\left(\frac{1.0\ g}{10^3\ kg}\right)\left(\frac{1.0mg}{10^{-3}g}\right)

b)

153kg(103g1.0 kg)(1.0 mg10−3g)153kg\left(\frac{10^3g}{1.0\ kg}\right)\left(\frac{1.0\ mg}{10^{-3}g}\right)

c)

153kg(103kg1.0 g)(1.0 g10−3mg)153kg\left(\frac{10^3kg}{1.0\ g}\right)\left(\frac{1.0\ g}{10^{-3}mg}\right)

d)

153kg(1.0 g103 kg)(10−3 mg1.0g)153kg\left(\frac{1.0\ g}{10^3\ kg}\right)\left(\frac{10^{-3}\ mg}{1.0^{ }g}\right)

10.

A metal cube has a volume of 3.25 mL, and a density of 7.85 g/mL. What is the mass of this metal cube?

a)

5.12 g

b)

0.414 g

c)

25.51 g

d)

2.42 g

11.

Select the three subatomic particles that make up atoms:

a)

protons

b)

photons

c)

neutrons

d)

electrons

12.

Protons have a ​ (a)   charge, electrons have a ​ (b)   charge, and neutrons are ​ (c)   .

Choose from the below words
positive
negative
neutral
13.

Two subatomic particles, ​ (a)   are in the nucleus of the atom, and ​ (b)   are in the volume of space surrounding the nucleus.

Choose from the below words
protons and neutrons
electrons
protons
neutrons
protons and electrons
electrons and neutrons
14.

A neutral lithium, Li, atom has how many protons and electrons?

a)

3 protons and 3 electrons

b)

3 protons and 2 electrons

c)

2 protons and 3 electrons

d)

2 protons and 2 electrons

15.

A neutral sodium, Na, atom, has ​ (a)   protons, and ​ (b)   electrons. When it loses 1 electron, it now has ​ (c)   electrons and a ​ (d)   charge.

Choose from the below words
11
10
+1
9
12
-1
+2
-2
16.

How many protons does a neutral nitrogen, N, atom have?

a)

7

b)

14

c)

12

d)

6

17.

This is an atom of hydrogen with a mass number of 1. Label the red and blue circles.

a)

neutron

b)

electron

c)

proton

d)

photon

e)

molecule

1
2
1)
2)
18.

Predict the charge that a Mg ion would have.

a)

+1

b)

+2

c)

-1

d)

-2

19.

Predict the charge that a F ion would have.

a)

+1

b)

+2

c)

-1

d)

-2

20.

Predict the charge that the Fe ion has in the following compound: FeO

a)

+3

b)

+4

c)

+1

d)

+2

21.

Predict the charge that the Cu ion has in the following compound: CuCl2

a)

+3

b)

+4

c)

+1

d)

+2

22.

An atom has the following subatomic particles. Write the element symbol with atomic number, mass number, and charge:

30 protons

32 neutrons

28 electrons

a)

3062Zn2+_{30}^{62}Zn^{2+}

b)

3032Zn2+_{30}^{32}Zn^{2+}

c)

3062Zn2−_{30}^{62}Zn^{2-}

d)

3065Zn2+_{30}^{65}Zn^{2+}

e)

6230Zn2+_{62}^{30}Zn^{2+}

23.

Identify a cation

a)

An atom with a positive charge because it has gained one or more protons

b)

An atom with a negative charge because it has lost one or more protons

c)

An atom with a positive charge because it has lost one or more electrons

d)

An atom with a negative charge because it has gained one or more electrons

24.

Identify an anion

a)

An atom with a positive charge because it has gained one or more protons

b)

An atom with a negative charge because it has lost one or more protons

c)

An atom with a positive charge because it has lost one or more electrons

d)

An atom with a negative charge because it has gained one or more electrons

25.

Organize these elements according to group/family:

Categorize the following

K

Li

F

Br

S

Se

Sr

Be

alkali metals
halogens
chalcogens
alkaline earth metals
26.

What is the chemical formula for oxygen difluoride?

a)

OF2

b)

O2F

c)

FO

d)

OF

27.

What is the chemical formula for phosphorus pentabromide?

a)

PBr5

b)

PB5

c)

P5Br

d)

PBr6

28.

What is the name for As2O3?

a)

diarsenic trioxide

b)

arsenic oxide

c)

arsenic(III) oxide

d)

arsenic(II) oxide

29.

What is the name for MgBr2?

a)

magnesium bromide

b)

magnesium dibromide

c)

magnesium(II) bromide

d)

magnesium(I) dibromide

30.

What is the chemical formula for iron(III) nitrate?

a)

FeNO3

b)

Fe(NO3)3

c)

Fe3N

d)

FeN

e)

FeNO2

31.

This mass spectrometer graph represents the ​ (a)   isotopes of ​ (b)  

Choose from the below words
4
lead
1
2
3
5
bismuth
thallium
32.

This mass spectrometer graph represents the element ​ (a)   , and the most abundant isotope is about ​ (b)   of all the isotopes

Choose from the below words
chlorine
75%
70%
25%
80%
bromine
krypton
33.

An unknown element found on the dwarf planet, Pluto, exists as 3 isotopes. Using the following masses and natural abundances, calculate the average atomic mass of this element that is temporarily being called peeyew, Pu.

34Pu has a mass of 34.05 amu and a percent abundance of 81.37%

32Pu has a mass of 31.97 amu and a percent abundance of 7.91 %

35Pu has a mass of 34.99 amu and a percent abundance of 10.72%

a)

33.99 amu

b)

56.75 amu

c)

34.07 amu

d)

33.78 amu

e)

33.16 amu

34.

What is the molar mass of As2Pe3?

(Pe is a fictional element said to have been found on the dwarf planet Pluto)

(a)  

35.

What is the molar mass of CH2Zf2?

(Zaepfelium is a new element your teacher discovered)

(a)  

36.

In one breath, about 0.037 g of CO2 is exhaled. How many moles of CO2 is this?

a)

0.000841

b)

1.628

c)

1189.5

d)

2.23E22

e)

5.06E20

37.

How many moles is 35.8 g of OZf2?

(Zaepfelium is a new element your teacher discovered)

a)

0.558

b)

2295

c)

1.79

d)

2.16E25

e)

3.36E23

38.

Convert 25 g of As2Pe3 to moles.

(Peeyew is a fictional element found on the dwarf planet Pluto)

a)

0.0993

b)

6.29E3

c)

10.07

d)

1.51E25

e)

5.98E22

39.

How many grams of NaCl is 1.28 moles of NaCl?

a)

74.8

b)

0.0219

c)

45.66

d)

7.71E23

e)

1.32E22

40.

What is the empirical formula (simplest whole number ratio) for this compound?

82.2% N

17.8% H

a)

NH3

b)

NH2

c)

NH

d)

N2H

e)

N3H

41.

A compound has the empirical formula of C2H8N and a molar mass of 92 g/mol. What is the molecular formula of this compound?

a)

C2H8N

b)

C4H16N2

c)

CH4N

d)

C6H24N3

42.

A 1.25 L solution of CaCl2 has a Molarity of 0.901 M. How many grams of CaCl2 was used to make this solution?

a)

125 g

b)

1.41 g

c)

1.11 g

d)

100 g

e)

110 g

43.

A 1.25 L solution of CaCl2 has a Molarity of 0.901 M. How many moles of CaCl2 was used to make this solution?

a)

125 mol

b)

1.41 mol

c)

1.13 mol

d)

100 mol

e)

110 mol

44.

A solution was made with 0.118 mols of an ionic compound dissolved in enough water to make 400 mL. What is the Molarity (mol/L) of this solution?

a)

0.295 M

b)

0.047 M

c)

3.39 M

d)

0.370 M

45.

MgCl2 → Mg2+ + 2Cl-

If you had 1 mole of MgCl2 completely dissolve in water according to the reaction above, how many moles of Mg2+ ions would be in solution?

a)

1

b)

2

c)

3

d)

4

e)

5

46.

K2SO4 → 2K+ + SO42-

If you had 2 moles of K2SO4 completely dissolve in water according to the reaction above, how many moles of K+ ions would be in the solution?

(a)  

47.

K2SO4 completely dissolves in water. Writing the charges on the ions in parenthesis, write the dissolution reaction below:

​ (a)   → ​ (b)   + ​ (c)  

Choose from the below words
K2SO4
2K(+)
SO4(2-)
K(2+)
SO4(-)
2SO4(-)
KSO4
K(+)
2SO4(2-)
48.

Balance the chemical reaction:

​ ​​ (a)   Al + ​ ​ (b)   NiBr2 → ​ (c)   AlBr3 + ​ (d)   Ni

What type of reaction is the above reaction?

​ (e)  

Choose from the below words
4
5
Combustion
Double Replacement
Synthesis
Single Replacement
Decomposition
2
3
1
49.

Balance the chemical reaction:

​ ​​ (a)   Al + ​​ (b)   O2 → ​ (c)   Al2O3

What type of reaction is the above reaction?

​ (d)  

Choose from the below words
4
5
Combustion
Double Replacement
Synthesis
Single Replacement
Decomposition
2
1
3
50.

Balance the chemical reaction:

​ (a)   ​C3H8 + ​ (b)   O2 → ​ (c)   CO2 + ​ ​ (d)   H2O

What type of reaction is the above reaction?


(e)  

Choose from the below words
4
6
Combustion
Double Replacement
Synthesis
Single Replacement
1
2
5
3
51.

Write the following word equation as a balanced chemical reaction:

Aluminum fluoride plus chlorine yields aluminum chloride plum fluorine.

a)

AlF3 + Cl2 → AlCl3 + F2

b)

2 AlF3 + 3 Cl2 → 2 AlCl3 + 3 F2

c)

AlF3 + 3 Cl → AlCl3 + 3 F

d)

AlF + Cl → AlCl + F

e)

2 AlF + Cl2 → 2 AlCl + F2

52.

Which type of reaction is:

4 (NH4)3PO4 + 3 Pb(NO3)4 → 12 NH4NO3 + Pb3(PO4)4

a)
Synthesis
b)
Decomposition
c)

Single Replacement

d)

Double Replacement

e)

Combustion

53.

2 H2 + O2 → 2 H2O

When 1 mole of O2 reacts, how many moles of water are produced?

a)

3

b)

2

c)

1

d)

6

e)

1.5

54.

2 H2 + O2 → 2 H2O

When 15.0 grams H2 reacts, how many moles of water are produced?

a)

7.44

b)

15

c)

134

d)

30.24

e)

3.72

55.

2 KClO3 → 2 KCl + 3 O2

When 25.0 grams of KClO3 decomposes, how many moles of O2 are produced?

The molar mass of KClO3 is 122.5 g/mol

a)

0.306

b)

0.204

c)

0.408

d)

0.612

e)

9.79

56.

N2 + 3 H2 → 2 NH3

If there are 6.0 moles of N2 and 15.0 moles of H2, which one is the limiting reactant (runs out first)?

a)

H2

b)

N2

c)

NH3

d)

Neither, they both run out at the same time

57.

Predict the products for the following Single Replacement reaction:

(You must have neutral products, but don't worry about balancing the whole reaction)

I2 + NaF → ​ (a)  

Choose from the below words
NaI + F2
NaI2 + F
NaI2 + F2
NaI + F
58.

Predict the products for the following Single Replacement reaction:

(You must have neutral products, but don't worry about balancing the whole reaction)

Ca + LiF → ​ (a)  

Choose from the below words
CaF2 + Li
CaF + Li
CaF + Li2
CaF2 + Li2
59.

What are the two products for this Double Replacement Reaction?

(You must have neutral products, but don't worry about balancing the whole reaction)

CaSO4 + Na3PO4 → ? + ?

a)

Ca3(PO4)2

b)

CaPO4

c)

Na2SO4

d)

Na3SO4

e)

Ca3P2

60.

What are the two products for this Double Replacement Reaction?

(You must have neutral products, but don't worry about balancing the whole reaction)

SrS + K3PO4 → ? + ?

a)

Sr3(PO4)2

b)

SrPO4

c)

K2S

d)

K3S

e)

Sr3P2

61.

Organize these compounds as either solid (s) or aqueous (aq)

Categorize the following

CaCO3

SrF2

Ca(OH)2

Pb(CH3CO2)2

Solid (s)
Aqueous (aq)
62.

Which one is the solid precipitate?

CaCl2 + 2 AgNO3 → Ca(NO3)2 + 2 AgCl

a)

CaCl2

b)

AgNO3

c)

Ca(NO3)2

d)

AgCl

e)

No precipitate is formed

63.

What is the net ionic equation for the following molecular equation?

CaCl2 + 2 AgNO3 → Ca(NO3)2 + 2 AgCl

a)

Ca2+ + 2 Cl-→ CaCl2

b)

Ag+ + NO3-→ AgNO3

c)

Ca2+ + 2 NO3- → Ca(NO3)2

d)

Ag+ + Cl- → AgCl

e)

CaCl2 + 2 AgNO3 → Ca(NO3)2 + 2 AgCl

64.

What is the net ionic equation for the following molecular equation?

SrBr2 + Pb(NO3)2 → Sr(NO3)2 + PbBr2

a)

Sr2+ + 2 Br- → SrBr2

b)

Pb2+ + 2 NO3- → Pb(NO3)2

c)

Sr2+ + 2 NO3- → Sr(NO3)2

d)

Pb2+ + 2 Br- → PbBr2

e)

SrBr2 + Pb(NO3)2 → Sr(NO3)2 + PbBr2

65.

N2 + 3 H2 --> 2 NH3

When 50.0 grams of N2 completely reacted, only 45.0 grams of NH3 was actually produced. What is the percent yield of NH3?

a)

74.1%

b)

90.0%

c)

82.4%

d)

34.0%

e)

28.3%

66.

Calculate the amount of heat in joules that 35.2 g of liquid water would need to absorb to increase in temperature by 10.0oC.

a)

1470 J

b)

1820 J

c)

737 J

d)

656 J

67.

A sample of CO2(g) increases in temperature from 50.0oC to 75.0oC by absorbing 4722 J. What is the mass of this sample of CO2?

a)

221 g

b)

1.38 x 105 g

c)

161 g

d)

4.15x 105 g

68.

A 70.0 g piece of metal at 80.0 °C is placed in 100 g of water at 22.0 °C contained in a calorimeter. The metal and water come to the same temperature at 24.6 °C.

What is the specific heat of the metal?

a)

0.28

b)

1087

c)

860

d)

  • - 860

e)

0.47

69.

  1. When 0.35 mols of N2 reacts, 63.21 kJ of heat is absorbed.

  2. Calculate ΔH in kJ/mol for the reaction:

  3. N2(g) + O2(g) → 2 NO(g)

a)

  • + 180.6 kJ

b)

- 180.6 kJ

c)

+ 2.26 kJ

d)

- 2.26 kJ

70.

  1. 2 H2O(l) + O2(g) → 2 H2O2(l) Δ\Delta H = + 196 kJ

  2. When 2 moles of O2 react according to the above thermochemical reaction, how much heat energy is absorbed?

a)

+ 392 kJ

b)

- 392 kJ

c)

+ 196 kJ

d)

- 98 kJ

e)

+ 98 kJ

71.

  1. Calculate ΔH° for the process

(i) Sb(s) + 5/2 Cl2(g) → SbCl5(s) ΔH° = ?

from the following information:

(ii) Sb(s) + 3/2 Cl2(g) → SbCl3(s) ΔH° = −314 kJ

(iii) SbCl3(s) + Cl2(g) → SbCl5(s) ΔH° = −80 kJ

a)

  • - 394 kJ

b)

- 234 kJ

c)

- 314 kJ

d)

- 80 kJ

72.

When 2.0 moles of carbon monoxide combusts according to the reaction on this chart, how many kJ of energy is released?

a)

566

b)

283

c)

10

d)

141.5

73.

When a sample of sulfur combusts according to the reaction written on this chart, 742 kJ of energy was released. How many moles of sulfur combusted?

a)

2.5

b)

1.5

c)

0.40

d)

2.2 x 105

74.

When a sample of methanol combusts according to the reaction written on this chart, 3478 kJ of energy is released. How many moles of methanol combusted?

a)

4.79

b)

2.86

c)

0.209

d)

2.53 x 106

75.

  1. N2(g)  +  3 H2(g) → 2 NH3(g) ΔH = -91.8 kJ

    When 1.75 moles of NH3 is produced according to the above thermochemical reaction, how much heat energy is released?

a)

+ 80.3 kJ

b)

- 80.3 kJ

c)

- 160.65 kJ

d)

- 45.9 kJ

e)

+ 45.9 kJ

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