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Chemistry Midterm Review

Total questions: 108

Worksheet time: 4hrs 44mins

Name
Class
Date
1.

This is a type of mixture where one substance dissolves into another

a)

Solution

b)

Miscibility

c)

Compound

d)

Solubility

2.
What type of mixture separates upon standing?
a)
Solution
b)
Alloy
c)
Colloid
d)
Suspension
3.

Two substances have been combined physically and appear the same throughout is called a.........

a)

A homogeneous mixture

b)

A heterogeneous mixture

c)

An element

d)

A compound

4.

Solutions has ______________ sized particles, colloids have _________________ sized particles, and suspensions have _________________________ sized particles.

a)

small, medium, large

b)

large, medium, small

c)

medium, small, large

d)

medium, large, small

5.

In the diagrams provided, the circles of different colors represent the atoms of different elements. Which diagram represents a mixture?

a)

I

b)

II

c)

III

d)

IV

6.

Which diagram represents an element?

a)

Diagram (a)

b)

Diagram (b)

c)

Diagram (c)

d)

None of the diagrams represent the parts of an element.

7.

What type of matter is shown in this particle diagram?

a)

Element

b)

Compound

c)

Mixture of Elements

d)

Mixture of Compounds

e)

Mixture of Elements and Compounds

8.
Which of the following could be separated by a physical change.
a)
A
b)
B
c)
C
9.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

10.
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 p+ from the mass number
d)
Add the mass number to the number of e-
11.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

12.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
13.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
14.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
15.

What does the number 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

16.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
17.
There are 4 different types of subshells (orbitals) s,p,d,f.
a)
true
b)
false
18.

Choose the s orbital

a)
b)
c)
d)
19.

Each p subshell contains _____ orbitals

a)

1

b)

3

c)

5

d)

7

20.

How many electrons can fit in one orbital?

a)

1

b)

2

c)

8

d)

18

21.

Choose the p orbital

a)
b)
c)
d)
22.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

23.

How many neutrons are in this isotope?

a)

20

b)

41

c)

61

d)

21

24.

How many electrons will be in the 1st shell, 2nd shell, 3rd shell, and or 4th shell? (electrons = 20)

a)

2, 8, 8, 3

b)

2, 8, 8, 0

c)

2, 8, 8, 1

d)

2, 8, 8, 2

25.

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

26.

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

27.

If an element has 3 valence electrons, what charge will likely form on its ion ?

a)

+3

b)

+5

c)

-3

d)

-5

28.

What is the total sum of oxidation numbers in the following compound Li3PO4?

a)

+2

b)

-1

c)

0

d)

+5

29.

What is the charge, or oxidation number, for elements in Group 2?

a)

-2

b)

+2

c)

-3

30.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
31.
Who proposed that the atom consists mostly of empty space?
a)
Bohr
b)
Dalton
c)
Rutherford
d)
Chadwick
32.
Which model suggested that: Atoms mostly consist of positively charged material with negatively charged particles (electrons) located throughout the positive material.
a)
Bohrs Model
b)
Plum Pudding Model 
c)
Democritus Model
d)
Our current model 
33.
What does the Bohr model suggest?
a)
Atoms are small, hard, indivisible objects. 
b)
That protons in the nucleus are attracted to electrons in the electron clouds. 
c)
That electrons travel around the nucleus of an atom in orbits or definite paths.
34.
What was James Chadwicks most notable discovery?
a)
The nucleus contains protons. 
b)
The nucleus contains neutrons.
c)
Electron are not fixed.
d)
Protons are positive.
35.

Which model of the atom is this?

a)

Billiard Ball

b)

Plum Pudding

c)

Planetary (Bohr)

d)

Electron Cloud

e)

Rutherford (nuclear)

36.

A chemical compound always has the same proportion of elements by mass


a)

Law of Definite Proportions

b)

Law of Multiple Proportions

c)

Definitive Law of Proportions

d)

Proportion Law

37.

What part of Dalton's atomic theory is wrong?

a)

Atoms cannot be subdivided

b)

All matter is composed of atoms

c)

Atoms are combined separated or rearranged in chemical reactions

d)

Atoms are identical in mass

38.

Which of the following is the ground-state configuration for the atoms of a transition element?

a)

1s22s22p53s23p54s23d3

b)

1s22s22p63s23p64s23d5

c)

1s22s22p62d103s24s23p5

d)

1s22s22p63s23p5

39.
In which of the following groups are the three species isoelectronic?
a)
S2¯, K+, Ca2+
b)
Sc, Ti, V2+
c)
O2¯, S2¯, Cl¯
d)
Mg2+, Ca2+, Sr2+
40.
Which of the following is the ground-state configuration of a negative ion of a halogen?
a)
1s22s22p53s23p5
b)
1s22s22p63s23p6
c)
1s22s22p62d103s23p6
d)
1s22s22p63s23p63d5
41.

In covalent bonding, atoms ______________ electrons.

a)
share
b)
gain
c)
lose
d)
absorb
42.

When magnesium gets the same electron configuration as Ne it has a _______ charge.

a)
-2
b)
+2
c)
+1
d)
0
43.

Molecules with 5 atoms, like CH4, will have a ___________________ shape.

a)
tetrahedral
b)
linear
c)
planar
d)
octahedral
44.

The VSEPR theory stands for the ________________________________________ theory.

a)
Valence Shell Electron Pair Repulsion Model
b)
Valence Shell Electron Pair Attraction
c)
Valence Shell Electron Pair Repulsion Theory
d)
Valence Shell Electron Pair Repulsion
45.

Ar and Cl-1 have the same electron configuration, so they are ___________________ with each other.

a)
ionic
b)
isoelectronic
c)
covalent
d)
isotopes
46.

Ionic compounds will not conduct an electric current in the ___________ state.

a)
liquid
b)
gas
c)
aqueous
d)
solid
47.

___________________ is the only element in group 1 to bond covalently.

a)
Lithium
b)
Sodium
c)
Potassium
d)
Hydrogen
48.

The difference between the trigonal planar and pyramid shapes is that the ____________________ shape has an unshared pair of electrons on the central atom.

a)
trigonal planar
b)
linear
c)
tetrahedral
d)
trigonal pyramid
49.

In a ___________________ covalent bond, electrons are shared unequally.

a)
nonpolar
b)
polar
c)
ionic
d)
metallic
50.

Match the following

a)

CH4

1.

Tetrahedral

b)

SiS2

2.

Linear

c)

Br2

3.

Linear

d)

SeCl2

4.

Bent

e)

SbI3

5.

Pyramidal

51.

Organize these options into the right categories:

Categorize the following
Polar
Nonpolar
52.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

53.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
54.

Light is emitted when electrons ...

a)

return from high energy state to low energy state

b)

jump from low energy state to high energy state

c)

either of these

d)

none of these

55.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
56.

List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.

a)

Li<Na<C<O<F

b)

Na<Li<C<O<F

c)

F<O<C<Li<Na

d)

Na<Li<F<O<C

e)

Na<Li<C<F<O

57.
Which atom would require the most energy to remove an electron?
a)
F
b)
Cl
c)
Br
d)
I
58.

Which of the atoms pictured would have the lower ionization energy and why?

a)

Atom A because it it bigger

b)

Atom A because the outer electrons are not "held" as tightly as those in atom B

c)

Atom B because it is smaller

d)

Atom B because the outer electrons have a greater attraction for the nucleus.

59.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
60.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
61.

Mendeleev arranged the periodic table by ___.

a)

proton number

b)

atomic mass

c)

atomic number

d)

neutrons

62.

Identify the element: 4 valence electrons, 3 energy levels

a)

Si

b)

Ga

c)

Be

d)

Al

63.

What is the second ionization energy?

a)

energy to required to remove an electron.

b)

energy required to remove the 2nd electron.

c)

energy required to de-energize the 2nd electron.

d)

I don't know.

64.

Using electron configuration and your knowledge of ionization energy, which would you expect to have a higher second ionization energy: Na or Mg?

a)

Na

b)

Mg

c)

Both would be expected to have the same second ionization energy

d)

Cannot be determined

65.

Successive ionization energies for an element in Period 4 were determined experimentally and found to be: IE1=600 kJ/mol, IE2=1800 kJ/mol, IE3=2700 kJ/mol, IE4=11,600 kJ/mol and IE5=15,000 kJ/mol. What element is this?

a)

germanium

b)

selenium

c)

gallium

d)

silicon

e)

phosphorous

66.

Which is larger:

P or P-3 ?

a)

P because it is the neutral atom.

b)

P-3 because it lost 3 electrons.

c)

P-3 because it gained 3 electrons.

d)

They are the same size since they are both P.

67.

A sodium atom (Na) loses an electron to form a sodium ion (Na+1). Which statement is correct in regards to describing the ionic radius.

a)

The sodium ion (Na+1) has a larger radius than the neutral sodium atom (Na).

b)

The sodium ion (Na+1) has a smaller radius than the neutral sodium atom (Na).

c)

The sodium ion (Na+1) and the neutral sodium atom (Na) are the same size because they are both sodium.

d)

The sodium ion (Na+1) has twice the radius of the neutral sodium atom (Na).

68.

What is the name of the chemical with the formula: MgSO4 ?

a)

Magnesium sulfide

b)

Magnesium sulfur

c)

Magnesium sulfate

d)

Manganese sulfide

69.

What is the name for Li2O ?

a)

Lithium oxygen

b)

Lithide oxide

c)

Dilithium oxide

d)

Lithium oxide

70.

What is the formula for an ionic compound made from aluminum and oxygen?

a)

Al3O2

b)

AlO

c)

Al2O3

d)

O3Al2

71.

What is the correct formula for a compound named Lithium sulfide ?

a)

Li2S

b)

LiS

c)

Li2SO4

d)

LiSO4

72.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
73.
Name the compound using appropriate rules:
FeCl3
a)
Chloride Iron
b)
Iron III Chloride
c)
Chloride III Iron
d)
I have no clue
74.

What is the name of the following formula: Cu3N

a)

copper nitride

b)

copper (iii) nitride

c)

copper (i) nitride

d)

copper (iii) nitrogen (i)

75.
An ionic compound made of copper (Cu2+) and oxygen would be named
a)
copper oxygen.
b)
copper oxide.
c)
dicopper oxide.
d)
copper(II) oxide.
76.

What is the formula for tin (II) nitride?

(a)  

77.
chloric acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
78.
Select the name for the following acid: H2S
a)
Hydrosulfuric acid
b)
Sulfuric acid
c)
Sulfurous
79.
CH3COOH
a)
Acetic acid
b)
Ethanoic acid
c)
Acenous acid
d)
Hydroacetic acid
80.

H3PO4H_3PO_4

a)

hydrophsophorus acid

b)

phosphoric acid

c)

hydrogen phosphorous

d)

phosphori hydroxide

81.
There are __?__ significant digits in the number 0.00076
a)
2
b)
4
c)
5
d)
6
82.
There are __?__ significant digits in the number 90,000.00
a)
1
b)
2
c)
5
d)
7
83.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
84.

How many significant digits are there in "8.20 x 104"?

a)

1

b)

2

c)

3

d)

4

85.

Subtract and round to the appropriate number of significant digits. 65.76−11.365.76-11.3  

a)

54.46

b)

54.4

c)

54.5

d)

54

86.
Which of the following is the answer for the problem with the correct number of significant digits?
23.91 x 12.861 = 307.50651
a)
308
b)
307.51
c)
307.5
d)
307
87.
Which of the following is the answer for the problem with the correct number of significant digits?
65 ÷ 10.01= 6.4935064
a)
7.0
b)
6.5
c)
6.494
d)
6.0
88.
Multiply:
(9.4 x 106)(3.2 x 105)
a)
30.08 x 1011
b)
3.8 x 101
c)
3.008 x 1012
d)
2.9375 x 101
89.
Which of the following is correct scientific notation?
a)
20.35 x 104
b)
.2035 x 104
c)
2035 4
d)
2.035 x104
90.

Pure gold has a density of 19.32 g/cm3. How large would a piece of gold be if it had a mass of 318.97 g?

a)

6,163 cm3

b)

16.51 cm3

c)

0.6057 cm3

d)

299.7 cm3

91.

0.02 moles of potassium atoms has a mass of

a)

5.11 g

b)

39.098 g

c)

0.782 g

d)

6.022 x 1023 g

92.

If you are given 500g of Ag3PO4, how many moles does your sample contain?

a)

418.58 mol

b)

0.02 mol

c)

1.19 mol

d)

5.32 mol

93.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

94.

How many atoms would be contained in 454 grams of iron (Fe)?

a)

6.02 x 1023 atoms

b)

8.14 atoms

c)

4.90 x 1024 atoms

d)

55.85 x 1023 atoms

95.

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

96.
How many moles are 2.85 x 1018 atoms of iron?
a)
4.73 x 10-6 moles
b)
1.72 x 1042 moles
c)
1.72 x 10-42 moles
d)
4.73 x 106 moles
97.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
98.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

99.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
100.

What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?

a)

CH2O

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

101.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)

C3H9O3

102.

Conducts electricity when dissolved in water:

a)

ionic

b)

covalent

c)

metallic

d)

none of these

103.

Very low melting points:

a)

ionic

b)

covalent

c)

metallic

d)

none of these

104.

Never dissolves in water:

a)

ionic

b)

covalent

c)

metallic

d)

none of these

105.

Forms formula units:

a)

ionic

b)

covalent

c)

metallic

d)

none of these

106.

Brittle solids:

a)

ionic

b)

covalent

c)

metallic

d)

none of these

107.

Mostly liquids, gases or low melting point solids:

a)

ionic

b)

covalent

c)

metallic

d)

none of these

108.

Bonds with the greatest electronegativity difference:

a)

ionic

b)

covalent

c)

metallic

d)

none of these

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