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Worksheets

2nd semester review

Total questions: 105

Worksheet time: 3hrs 46mins

Name
Class
Date
1.

Choose the correct electron configuration for Nickel (Ni).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s2 4d8

c)

1s2 2s2 2p6 3s2 3p6 4s10

d)

1s2 2s2 2p6 3s2 3p6 4s2 4p8

2.

What is the position of an element in the periodic table if its electron configuration is 1s2 2s2 2p6 3s2 3p5?

a)

Group 1A

b)

Group 2A

c)

Group 5A

d)

Group 7A

3.

What is the noble gas configuration for silicon?

a)

[Ne] 3s2 3p1

b)

[Ar] 4s1

c)

[Kr] 5s1

d)

[Ne] 3s2 3p2

4.

This orbital diagram represents which neutral element?

Hint: Each half arrow is an electron

a)

Nitrogen

b)

Oxygen

c)

Carbon

d)

Neon

5.

This orbital diagram represents which element?

Hint: Each half arrow is an electron

a)

Sodium

b)

Magnesium

c)

Aluminum

d)

Iron

6.

How many valence electrons are in Phosphorus?

Hint: Use the group # on the periodic table to tell you how many electrons it has on the outer orbital.

a)
15
b)
4
c)
5
d)
31
7.

Which of the following is a correct electron dot structure?

Hint: Use the group # it is in to figure out how many valence electrons it has.

a)

b)

c)

d)

8.

How many valence electrons does Tin (Sn) have?

Hint: Use the group # it is in to figure out how many valence electrons it has.

a)

8

b)

7

c)

5

d)

4

9.

What type of compound is this?

Ionic = metal & nonmetal

Covalent = nonmetal only

Metallic = metallic only

a)

Ionic

b)

Covalent

c)

Metallic

10.

What type of bonding happens between the atoms in this compound?

a)

Ionic bonding - electrons move from one atom to another

b)

Covalent bonding - electrons are shared between 2 atoms.

c)

Metallic bonding - electrons are released by all the atoms and they are free to move around.

11.

What type of bonding exists between the atoms in this compound?

a)

Ionic bonding - electrons move from one atom to another

b)

Covalent bonding - electrons are shared between 2 atoms.

c)

Metallic bonding - electrons are released by all the atoms and they are free to move around.

12.

What type of compound is this?

Ionic = metal & nonmetal

Covalent = nonmetal only

Metallic = metallic only

a)

Ionic

b)

Molecular

c)

Metallic

13.

How many atoms are there TOTAL in:
CH3CH2CH2OH

a)

7

b)

9

c)

12

d)

14

14.

How many atoms are in the compound: Al(OH)3

a)

3

b)

4

c)

6

d)

7

15.

Calculate the molar mass of Ba(C2H3O2)2

Hint: Molar mass is calculated by adding all the element masses using the periodic table.

a)

255.43 g = 1 mol

b)

237.43 g = 1 mol

c)

228.43 g = 1 mol

d)

196.43 g = 1 mol

16.

Calculate the molar mass of NH4NO2

Hint: Molar mass is calculated by adding all the element masses using the periodic table.

a)

50.06 g = 1 mol

b)

60.12 g = 1 mol

c)

64.06 g = 1 mol

d)

78.04 g = 1 mol

17.

What is the percent composition by mass of oxygen in the compound MgSO4?

a)

20%

b)

27%

c)

46%

d)

53%

18.

What is the percent by mass of magnesium in MgO?

a)

20%

b)

40%

c)

50%

d)

60%

19.

What is the empirical formula if you have a compound that is made up of 81.82% carbon and 18.18% hydrogen?

a)

C3H8

b)

CH4

c)

C2H2

d)

C4H10

20.

What is the empirical formula of a compound that has the molecular formula of C2H4?

Hint: Empirical formulas are just the most simplified version of the molecular formula.

a)

C2H3

b)

CH3

c)

C2H6

d)

C2H2

21.

Name the following compound: Li3P

Hint: Use your ion reference sheet and periodic table

a)

lithium phosphate

b)

lithium phosphide

c)

lithium phosphorus

d)

lithium phosphite

22.

What is the name of the compound Ni3N2?

Hint: Use your ion reference sheet and periodic table

a)

nickel (I) nitride

b)

nickel (II) nitride

c)

nickel (III) nitrite

d)

nickel (II) nitrate

23.

The chemical compound for sodium phosphite would be:

Hint: Use your ion reference sheet and periodic table

a)

Na3P

b)

Na2PO4

c)

Na3PO3

d)

Na(PO3)3

24.

Name the following ionic compound: Cr(NO2)3

Hint: Use your ion reference sheet and periodic table

a)

chromium nitrite

b)

chromium nitride

c)

chromium III nitride

d)

chromium III nitrite

25.

Ionic compounds have ____ melting point temperatures.

a)

high

b)

low

c)

medium

d)

very low

26.

Ionic compounds are _______ at room temperature.

a)

gas

b)

liquid

c)

solid

d)

plasma

27.

Ionic compounds are good electrical conductors when _____.

a)

solids

b)

crystalline

c)

gaseous

d)

melted or in a solution

28.

Ionic compounds are _____.

a)

malleable

b)

ductile

c)

soft

d)

brittle

29.

Ionic compounds are brittle because when trying to hammer, stretch, or bend them ions with LIKE charges get lined up beside each other, and they ___ each other.

a)

strongly attract

b)

only mildly attract

c)

strongly repel

d)

only mildly repel

30.

Ionic compounds usually ​ (a)   dissolve in water.

Choose from the below words
can
cannot
31.

The reason that a sodium ion bonds with a chlorine ion is because

(two correct answers)

a)

Chlorine transfers an electron to Sodium

b)

the opposite charge forms a strong attraction

c)

small ions are attracted to large ions

d)

Sodium transfers an electron to Chlorine

32.

If I gain electrons by rubbing my shoes on a carpet, I will...

a)

become positive because I've added more particles to my body.

b)

become negative because I've added more negative charge to my body.

c)

become positive because I've added more positive charge to my body.

d)

stay neutral because I already had electrons, now I just have more.

33.

What do the dots represent for the oxygen atom?

a)

There are 6 valence electrons.

b)

There are 6 total electrons.

c)

Oxygen has atomic number of 6.

d)

Oxygen will give away 6 electrons in order to gain stability.

34.

Which is the only nonmetal that is able to bond with 4 different atoms?

a)

Oxygen

b)

Carbon

c)

Nitrogen

d)

Hydrogen

35.

Which Electron Dot Model correctly shows an O2 molecule?

a)

b)

c)

d)

36.

How many total atoms are present in a molecule of diphosphorus pentoxide?

Hint: The prefixes tell you the number of atoms of each element!

a)

2

b)

5

c)

7

d)

9

37.

Which of the following elements can form a triple covalent bond?

Hint: You would need to draw the dots it has and see how many dots are single and able to bond.

a)

Nitrogen

b)

Oxygen

c)

Chlorine

d)

Potassium

38.

The chemical name of SO3 is:

Hint: Molecular compounds use prefixes in their names.

However, you do not use "mono" on the first element.

a)

sulfate

b)

sulfur oxide

c)

sulfur trioxide

d)

monosulfur trioxide

39.

The chemical formula of dinitrogen tetroxide is:

a)

Ni₂O₄

b)

NiO

c)

N₂O₄

d)

NiO₂

40.

What is the correct name for NO?

Hint: Molecular compounds use prefixes in their names.

However, you do not use "mono" on the first element.

a)

Mononitrogen Monoxide

b)

Nitrogen Monoxide

c)

Mononitrogen Dioxide

d)

Nitrogen Oxide

41.

How many total electrons are shared between two atoms in a double bond?

a)

2

b)

4

c)

6

d)

8

42.
The number of bonds an element will form in a covalent compound will be equal to
a)

the number of valence electrons

b)

the amount of paired dots it has

c)

the amount of unpaired dots it has

d)

the group number

43.

Some are solids, some are liquids, and some are gases at room temperature.

Which type of compound is this?

a)

ionic compounds

b)

molecular compounds

44.

Which of the following substances will not dissolve in water?

a)

Salt

b)

Sugar

c)

Oil

d)

Baking Soda

45.

Water is polar. What does that mean?

a)

it is a molecule with opposite charges on opposite ends

b)

it is a molecule with no charge

c)

it is a molecule with identical charges on opposite ends

d)

it is a molecule with too many protons

46.

What are the intermolecular attractions called between two water molecules?

a)

Hydrogen Bonds

b)

Dispersion Forces

c)

Dipole-Dipole Forces

d)

Covalent Bonds

47.

Which part of a water molecule has a Positive Charge?

Hint: it's the atom that is less electronegative

a)

The Hydrogen

b)

The Oxygen

c)

The Top

d)

The Bottom

48.

Which formula represents a nonpolar molecule?

Nonpolar bonding has a electronegativity difference of 0.0 - 0.4

Polar bonding has an electronegativity difference of 0.5 - 1.9

a)

HBr

b)

H2S

c)

NH3

d)

PCl3

49.

Classify the following as having polar or nonpolar bonding: SF2

Nonpolar bonding has a electronegativity difference of 0.0 - 0.4

Polar bonding has an electronegativity difference of 0.5 - 1.9

a)

polar

b)

nonpolar

50.

Classify NH3 in terms of polarity.

Nonpolar bonding has a electronegativity difference of 0.0 - 0.4

Polar bonding has an electronegativity difference of 0.5 - 1.9

a)

polar

b)

nonpolar

51.

Classify CH4 as having polar or nonpolar bonding.

Nonpolar bonding has a electronegativity difference of 0.0 - 0.4

Polar bonding has an electronegativity difference of 0.5 - 1.9

a)

polar

b)

nonpolar

52.

The strongest intermolecular attractions for this compound is

a)

Dipole-dipole

b)

London dispersion

c)

Hydrogen bonds

d)

dipole-induced dipole attractions

53.

Which molecule has the strongest intermolecular forces?

Hint: dispersion is the weakest, dipole-dipole is middle, and hydrogen bonding is strongest

a)

H-F

b)

H-Cl

c)

Br-Br

d)

Cl-I

54.

Type of intermolecular force present in I2, Br2, and Cl2.

Hint: these molecules are all non-polar

a)

dipole-dipole

b)

hydrogen bonding

c)

dispersion

55.

Which of the following molecules can attract to other molecules with dispersion and dipole-dipole, but not hydrogen bonding?

a)
b)
c)
d)
56.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
57.

List the 3 intermolecular forces from strongest to weakest.

a)

Hydrogen Bond, London Dispersion, Dipole-dipole

b)

London Dispersion, Dipole-dipole,

Hydrogen Bond

c)

Hydrogen Bond, Dipole-dipole, London Dispersion

d)

Dipole-dipole, Hydrogen Bond, London Dispersion

58.

Which of the following forces are found between two NONPOLAR molecules?

a)

Dispersion Forces

b)

Dipole-dipole interactions

c)

Hydrogen bonding

59.

What shape does this molecule have?

a)

trigonal planar

b)

tetrahedral

c)

bent

d)

linear

60.

What is the name of this molecule shape?

a)

tetrahedral

b)

octahedral

c)

trigonal pyramidal

d)

bent

61.

What is the name of this molecule shape?

a)

trigonal pyramidal

b)

trigonal planar

c)

bent

d)

tetrahedral

62.

Metallic bonds form because metals

a)

"want" to give up valence electrons

b)

always share valence electrons

c)

have many valence electrons

d)

always gain valence electrons

63.

Metals are used to make electric wires mainly because of which two properties?

a)

are ductile

b)

are shiny

c)

have free moving electrons

d)

They have a high melting point

64.

What are some benefits of metal alloys, such as steel, bronze, and brass? (choose all that apply)

a)

they can be stronger than pure metal

b)

they may not rust/corrode as easily

c)

they don't have electrons

d)

they form covalent bonds

65.

What is the formula for phosphorous acid?

Hint: "Sprite is delicious"

a)

H3PO4

b)

H2PO4

c)

H3P

d)

H3PO3

66.

What is the formula for nitric acid?

Hint: "I ate something icky"

a)

HNO2

b)

HNO3

c)

HNO4

d)

H2NO3

67.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

68.

What kind of compound is H2CO3?

a)

molecular

b)

covalent

c)

base

d)

acid

69.

Name the following base

Al(OH)3

a)

Aluminum monohydroxide

b)

Aluminum hydroxide

c)

Monoaluminum trihydroxide

d)

Aluminum Trioxide

70.

Write the formula of the following compound.

Iron(III) hydroxide.

a)

Fe(OH)3

b)

Fe(OH)2

c)

Fe OH3

71.

Balance this equation.
_CF4 + _Br2 --> _CBr4 + _F2

a)

2,1,2,1

b)

1,2,2,1

c)

1,2,1,2

d)

2,2,2,2

72.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
73.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__FeCl3 + __Ca(OH)2 --> __Fe(OH)3 + __CaCl2
a)
4,3--> 2,1
b)
3,2 --> 3,1
c)
2,3 --> 2,2
d)
2,3 --> 2,3
74.

2 Al + 3 CuCl2 ----> 3 Cu + 2 AlCl3

a)

combustion

b)

synthesis

c)

double replacement

d)

single replacement

75.

C3H8 + 5 O2 ---> 3 CO2 + 4 H2O

a)

single replacement

b)

double replacement

c)

combustion

d)

decomposition

76.

AgNO3 + NaCl ---> AgCl + NaNO3

a)

double replacement

b)

single replacement

c)

combustion

d)

decompostion

77.

2 MgO ----> 2 Mg + O2

a)

synthesis

b)

single replacement

c)

combustion

d)

decomposition

78.

What are the correct products for this acid base reaction HBr + Mg(OH)2 →

Hint: This is an acid base reaction that follows the pattern of double replacement.

a)

HMg + Br(OH)2

b)

H2O + MgBr2

c)

H2O + Mg2Br

d)

MgO2 + H2Br

79.

4 Fe + 3O2 ---> 2 Fe2O3

a)

decomposition

b)

combustion

c)

synthesis

d)

single replacement

80.
All of the following are indicators of a chemical reaction except one.  Which one is NOT an indicator that a chemical reaction has taken place?
a)
he production of heat or light
b)
a color change
c)
the production of gas bubbles
d)

a solid substance dissolving in a liquid

81.
Which of the following symbols is not a correct indication of the phase of a substance in a reaction? 
a)
(s)=solid
b)
(g)=grams
c)
(l)=liquid
d)
(aq)= aqueous
82.

In what state is this substance?

a)

solid precipitate

b)

dissolved in water

c)

released as a gas

d)

liquid

83.
The substances listed on the right side of a chemical equation are the
a)
Yields
b)
Reactants
c)
Products
d)
Precipitates
84.

Translate the word equation below.

Sulfur Trioxide reacts with Water to form Sulfuric Acid (H2SO4).

a)

SO3 + H2O → H2SO4SO_3\ +\ H_2O\ \rightarrow\ H_2SO_4

b)

SO → HO + HSOSO\ \rightarrow\ HO\ +\ HSO

c)

SO2 + H2O → H2SO4SO_2\ +\ H_2O\ \rightarrow\ H_2SO_4

d)

SO → H2O + H2SO4SO\ \rightarrow\ H_2O\ +\ H_2SO_4

85.

Translate the word equation below:

Nitrogen gas reacts with Hydrogen gas to form Nitrogen trihydride gas

a)

N  → H + NH3N\ \ \rightarrow\ H\ +\ NH_3

b)

N2 + H2 → NH3N_2\ +\ H_2\ \rightarrow\ NH_3

c)

N + H → NH3N\ +\ H\ \rightarrow\ NH_3

d)

N2 → H2 + NH3N_2\ \rightarrow\ H_2\ +\ NH_3

86.

Which is the correct chemical equation for the following: Solid Zn reacts with silver (I) chloride to produce Zinc (II) chloride and silver metal

a)

Zn + AgCl → ZnCl2 + Ag

b)

ZnCl2 + Ag → Zn + AgCl

c)

ZnCl2 + Ag2 → Zn + AgCl

d)

Zn2Cl + Ag → Zn + AgCl

87.

Which is the correct chemical equation for the following: Barium Chloride combined with sodium sulfide yields barium sulfide and sodium chloride

a)

BaCl + NaS → BaS+ NaCl

b)

BaCl2 + Na2S → BaS+ NaCl

c)

BaS+ NaCl → BaCl + NaS

d)

BaCl2 + Na2S → BaS+ NaCl2

88.

Magnesium can be burned in oxygen to produce solid magnesium oxide.

a)

Mg(s) + O2(g)→ MgO(s)

b)

Mg(s) + O(g) → MgO(s)

c)

Mg(s) + CO2(g) → MgO(s) + C(s)

d)

Mg(s) + O2(g) → Mg2O2(s)

89.
How many water molecules are in 5.2 moles of water?
a)

7.3 x 1025

b)

3.3 x 1022

c)

3.1 x 1024

d)

8.6 x 1024

90.

What is the mass of 2.5 mole of oxygen gas O2?

a)

40. g

b)

80. g

c)

16 g

d)

32 g

91.

Calculate the number of atoms in 0.0340 g Zn.

a)

5.20 x 10-4 atoms Zn

b)

3.13 x 1023 atoms Zn

c)

3.13 x 1020 atoms Zn

d)

2.05 x 1022 atoms Zn

92.

You have 3.5 L of H2 at STP. How many moles of gas are there?

a)

22.4 mol

b)

22.4 L

c)

0.16 mol

d)

0.16 L

93.

2H2  +   O2  →  2H2O How many moles of oxygen are consumed if 8 moles H2 react completely?

a)
2
b)
4
c)
6
d)
8
94.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
95.
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
96.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
97.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
98.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

99.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
100.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
101.

How many liters 0.110 M nitric acid can be prepared by diluting 5.00 mL of 15.3 M stock solution?

a)

1530 mL

b)

1.53 L

c)

0.0654L

d)

0.153 L

102.

A solution is made by dissolving 0.50 mole of NaCl in enough water to give a final volume of 400.0 mL. What is the molarity of the solution?

a)

0.10 M

b)

0.40 M

c)

1.25 M

d)

2.33 M

103.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
104.
The ___ is the thing being dissolved
a)
solute
b)
solvent
105.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL

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