Free Printable Midterm review

1.

What is the best classification for this substance?

a)

An element

b)

A compound

c)

A mixture

2.

What is the best classification of this substance? H₂SO₄

a)

An element

b)

A compound

c)

A mixture

3.

Does this image represent a chemical or physical change?

a)

Chemical change

b)

Physical change

4.

Does this image represent a chemical or a physical change?

a)

Chemical change

b)

Physical change

5.

What is an atom which has gained or last electrons called?

a)

isotope

b)

atom

c)

ion

d)

balanced

6.

On the Periodic Table each element increases by one _________

a)

electron

b)

proton

c)

neutron

d)

letter

7.

A row across the Periodic Table where each element has the same number of energy shells

a)

column

b)

family

c)

period

8.

In a family or column, the elements have similar properties because they all have the same number of

a)

protons

b)

neutrons

c)

valence electrons

d)

electrons

9.

What is the octet rule? How many valence electrons can the first three periods hold?

a)

8

b)

2

c)

2 8 8

d)

2 8 16

10.

Whether or not bonds form is due to the ?????

a)

valence electron configurations

b)

protons

c)

atomic mass

d)

chance

11.

The chemical bond formed when two atoms share electrons is call a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

electron bond

12.

How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?

a)

2

b)

4

c)

6

d)

8

13.

What is a valence electron?

a)

an electron that is found in the outermost shell of an atom

b)

an electron found in the innermost shell of an atom

c)

an electron found in the middle shell

d)

an electon found in the nucleus

14.

What is the number of valence electrons of Neon?

a)

6

b)

7

c)

8

d)

9

15.

What is the number of valence electrons of Oxygen?

a)

1

b)

2

c)

6

d)

8

16.

A ____________is the force that holds atoms together in a compound.

a)

Chemical Formula

b)

Chemical Reaction

c)

Chemical Bond

d)

Synthesis Reaction

17.

An ionic compound is held together by the _______--the force of attraction between opposite charges of the atoms.

a)

Covalent Bond

b)

Ionic Bond

c)

Synthetic Bond

d)

Molecular Bond

18.

A ________is the force of attraction between atoms sharing electrons.

a)

Synthetic Bond

b)

Ionic Bond

c)

Molecular Bond

d)

Covalent Bond

19.

What elements generally make an ionic bond ?

a)

Metal and nonmetal

b)

2 or more nonmetals

c)

2 or more metals

d)

2 elements

20.

What is the name of K₂S?

a)

Dipotassium sulfide

b)

Potassium sulfur

c)

Potassium sulfide

d)

Potassium (II) sulfide

21.

What is the formula for calcium chloride?

a)

CaCl

b)

CaCl₂

c)

Ca₂Cl

d)

CaCl₃

22.

What is the name for Fe₂S₃?

a)

Iron sulfide

b)

Diiron trisulfide

c)

Iron (II) sulfide

d)

Iron (III) sulfide

23.

What is the formula for Zinc oxide?

a)

ZnO

b)

ZnO₂

c)

Zn₂O

d)

Zn₂O₃

24.

What is the formula for iron (III) chloride?

a)

Fe₃Cl

b)

FeCl₃

c)

Fe₂Cl₃

d)

FeCl

25.

What is the name for Zn(ClO₄)₂?

a)

Zinc chlorate

b)

Zinc chlorite

c)

Zinc hypochlorite

d)

Zinc perchlorate

26.

What is the name of CaSO₃?

a)

Calcium sulfite

b)

Calcium sulfate

c)

Calcium acetate

d)

Calcium sulfur oxide

27.

What is the formula for potassium dichromate?

a)

K₂Cr₂O₅

b)

KCr₂O₇

c)

K₂Cr₂O₇

d)

K₂CrO₄

28.

What is the formula for ammonium nitrate?

a)

NH₃NO₂

b)

NH₄NO₂

c)

NH₃NO₃

d)

NH₄NO₃

29.

What is the name of P₄O₁₀?

a)

Phosphorus oxide

b)

Tetraphosphorus decoxide

c)

Quadraphosphorus decoxide

d)

Phosphorus decoxide

30.

What is the name of CO?

a)

Carbon oxide

b)

Monocarbon monoxide

c)

Carbon monoxide

d)

Carbon dioxide

31.

What is the formula for dichlorine heptoxide?

a)

Cl₂O₆

b)

Cl₂O₇

c)

ClO₅

d)

Cl₂O₉

32.

What is the name of HBr?

a)

Hydrobromic acid

b)

Bromic acid

c)

Hydrogen bromide

d)

Hydrobro acid

33.

What is the name of H₂SO₄?

a)

Hydrosulfuric acid

b)

Sulfuric acid

c)

Sulfurous acid

d)

Hydrogen Sulfate

34.

What is the formula for hydrochloric acid?

a)

HClO₃

b)

HClO₂

c)

H₂ClO₃

d)

HCl

35.

What is the name of NaOH?

a)

Sodium hydrogen oxide

b)

Sodium acid

c)

Sodium hydroxide

d)

Sodium oxalic acid

36.

What is the formula for calcium hydroxide?

a)

CaOH

b)

Ca(OH)₂

c)

Ca₂OH

d)

HCa

37.

Which would have more atoms?

a)

1 mole of Li

b)

1 mole of Au

c)

1 mole of Si

d)

None, all are equal

38.

What is the definition for Avogadro's number?

a)

number of grams per one mole of a substance

b)

whole number ratio that is a multiple of a chemical formula

c)

simplest, whole number ratio of a chemical formula

d)

6.02 x 10^23 particles per one mole of a substance

39.

Which represents the greatest mass of sulfur?

a)

1 gram of sulfur

b)

1 molecule of sulfur

c)

0.5 mole of sulfur

d)

6.02 x 10²³ atoms of sulfur

40.

How many moles are present in 32.3 grams of carbon dioxide (CO₂)?

a)

44.01 moles

b)

1421.52 moles

c)

32.3 moles

d)

0.73 moles

41.

What is the mass in grams of 5.90 mol C₈H_18?

a)

.0512 g

b)

19.4 g

c)

673 g

d)

389 g

42.

What is the mass of 2.50 mol of oxygen gas O₂?

a)

40 g

b)

80 g

c)

16 g

d)

32 g

43.

How many water molecules are in 5.2 moles of water?

a)

6.02 x 10²³

b)

5.2

c)

3.1304 x 10²⁴

d)

8.638 x 10^-24

44.

What is the definition of molar mass?

a)

number of grams per one mole of a substance

b)

whole number ratio that is a multiple of a chemical formula

c)

simplest, whole number ratio of a chemical formula

d)

6.02 x 10^23 particles per one mole of a substance

45.

Molar mass is in units of ________.

a)

grams

b)

grams/mole

c)

mole

d)

moles/gram

46.

Shivani measures out 6.0 moles of epsom salt (MgSO₄) to put in her bath. How many grams of MgSO₄ went in the bath?

a)

3.6 x 10²⁴ g

b)

720 g

c)

0.050 g

d)

20 g

47.

How would you set up the problem if you have a sample of 2.50 g of sodium (Na), how many moles of Na do you have?

a)

$2.50g\ Na\ \times\frac{22.99\ mol\ Na}{1\ g\ Na}=$

b)

$2.50\ g\ Na\ \times\frac{1\ mol\ Na}{22.99\ g\ Na}=$

c)

$2.50\ g\ Na\ \times\frac{22.99\ g\ Na}{1\ mol\ Na}=$

d)

$2.50\ g\ Na\ \times\frac{1\ g\ Na\ }{22.99\ mol\ Na}=$

48.

How would you set up the problem if you want to find the mass, in grams, of 0.55 moles of silicon?

a)

$0.55\ mol\ Si\ \times\ \frac{28.09\ g\ Si}{1\ mol\ Si}\ =\$

b)

$0.55\ mol\ Si\ \times\frac{1\ g\ Si\ }{28.09\ mol\ Si}=$

c)

$0.55\ mol\ Si\ \times\frac{28.09\ mol\ Si}{1\ g\ Si}=$

d)

$0.55\ mol\ Si\ \times\frac{1\ mol\ Si}{28.09\ g\ Si}=$

49.

If you're converting between grams and moles you need to use:

a)

1 mole = 6.022x10²³things

b)

the metric prefix chart

c)

molar mass

d)

the atomic number

50.

How many moles are in 16.94 g of water H2O?

a)

0.996 mol H₂O

b)

0.9401 mol H₂O

c)

305.3 mol H₂O

d)

1.063 mol H₂O

51.

How many moles are present in 32.3 grams of carbon dioxide?

a)

44.01 moles

b)

1.15 moles

c)

1.36 moles

d)

0.73 moles

52.

What is the molar mass of Al₂(SO₄)₃?

a)

75 g

b)

342 g

c)

79 g

d)

27 g

53.

How many grams are there in 0.500 mol iron (III) oxide Fe2O3?

a)

319.2 g

b)

79.9 g

c)

398.8 g

d)

99.7 g

54.

Choose the correct shape for this molecule:

a)

linear

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

55.

*

a)

trigonal pyramid

b)

linear

c)

bent

d)

angular

56.

*

a)

linear

b)

trigonal planar

c)

trigonal pyramid

d)

bent of angular

57.

SiCl₄has what shape?

a)

square planar

b)

square pyramidal

c)

tetrahedral

d)

octahedral

58.

What is the shape of H₂O?

a)

linear

b)

tetrahedral

c)

bent

d)

trigonal pyramidal

59.

According to the octet rule most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

60.

What is the molecular geometry of CO₂?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Linear

61.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

62.

This is a correct dot diagram for fluorine (F)

a)

true

b)

false

63.

This is a correct dot diagram for oxygen (O)

a)

true

b)

false

64.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

65.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

66.

Choose the correct shape for this molecule:

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Trigonal planar

67.

What is the correct shape of CHCl₃?

a)

Bent

b)

Trigonal pyramidal

c)

Tetrahedral

d)

Trigonal planar

68.

Choose the correct shape for this molecule:

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal pyramidal

69.

Bent

a)

b)

c)

d)

70.

Linear

a)

b)

c)

d)

71.

Angular

a)

b)

c)

d)

72.

Trigonal Pyramidal

a)

b)

c)

d)

73.

What is the molecules molecular geometry name?

a)

Bent 1

b)

Bent 2

c)

Trigonal Pyramidal

d)

Trigonal Planar

74.

How many bonded pairs are present?

a)

1

b)

2

c)

3

d)

4

75.

How many bonded pairs are present?

a)

1

b)

2

c)

3

d)

4

76.

How many bonded pairs are present?

a)

1

b)

2

c)

3

d)

4

77.

How many lone pairs are present?

a)

1

b)

2

c)

3

d)

4

78.

How many lone pairs are present?

a)

1

b)

2

c)

3

d)

4

e)

NONE

79.

How many lone pairs are present?

a)

1

b)

2

c)

3

d)

4

e)

NONE

80.

What is the hybridization of the molecule shown?

a)

sp

b)

sp²

c)

sp³

81.

The bond angle in the molecular geometry shown is about....

a)

180^o

b)

120⁰

c)

109⁰

82.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

83.

What elements have zero electronegativity?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

84.

Electronegativity (a) as you go down a group.

85.

As you move across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have less mass

c)

the atoms have more protons.

d)

the atoms have less electrons.

86.

As you move down the periodic table atoms get bigger. This is because ____________.

a)

The atoms have more mass.

b)

The atoms have more protons.

c)

The atoms have more energy levels

d)

The atoms have more nuetrons

87.

Which one has the largest radius?

a)

Lithium (Li, atomic #3)

b)

Boron (B, atomic #5)

c)

Neon (Ne, atomic #10)

d)

Nitrogen (N, atomic #7)

88.

Which of the following elements would be smaller: indium or gallium?

a)

indium

b)

gallium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

89.

Which species has the larger radius?

a)

Cl

b)

^Cl-

90.

Which species has the larger radius?

a)

Na

b)

Na⁺

91.

CH₄ is

a)

polar

b)

non-polar

92.

NH₃ is

a)

polar

b)

non-polar

93.

Is the following molecule polar or non-polar?

a)

polar

b)

non-polar

94.

Non-polar molecules can have polar covalent bonds.

a)

True

b)

False

95.

More electronegative atoms in covalent compounds are likely to have:

a)

Partial positive charge

b)

Partial negative charge

96.

SO₂ is

a)

polar

b)

non-polar

97.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

98.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

99.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

100.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

101.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

102.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

103.

A diatomic molecule like O₂ is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

104.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

Midterm review

Total questions: 104

Worksheet time: 4hrs 30mins

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