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Chemistry 1 Review

Total questions: 106

Worksheet time: 2hrs 21mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
2.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
3.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
4.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
5.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
6.

How many electrons can the p sublevel hold?

a)

14

b)

10

c)

2

d)

6

7.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

8.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
9.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
10.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
11.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
12.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
13.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
14.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
15.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
16.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
17.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
18.
Who came up with this model of an atom?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
19.
Which of the following scientist discovered the current model of the atom?
a)
Dalton
b)
Schrodinger.
c)
Thomson
d)
Dalton
20.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

21.

What is the atomic number of the atom pictured?

a)

9

b)

8

c)

18

d)

19

22.
Xenon (Xe)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
23.
Sodium (Na)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
24.
Calcium (Ca)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
25.
Radium (Ra)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
26.
Argon (Ar)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
27.
Potassium (K)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
28.
Gold (Au)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Earth Metal
d)
Heavy Metal
29.
Silver (Ag)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Metal
d)
Heavy Metal
30.

What name is given to the first of the bottom two rows on the periodic table?

a)

Lanthanide Series

b)

Actinide Series

31.

What name is given to the very bottom row on the periodic table?

a)

Lanthanide Series

b)

Actinide Series

32.

Back in the olden days in Europe, noblemen never mixed with the ordinary peasants. This is how the name Noble Gases derived. Why do the Noble Gases never mix or react with other elements?

a)

Because they already have full outer energy levels.

b)

Because gases don't react with other gases.

33.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
34.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
35.

The Atomic number is known as the _______

a)

Number of electrons in an atom

b)

Number of Protons in an atom

c)

Number of neutrons in an atom

d)

Number of Protons and electrons in an atom

36.

The formula used to calculate the number of neutrons is:

a)

Mass Number - Atomic Number

b)

Protons + Electrons

c)

Atomic Number - Mass Number

d)

Protons x2

37.

What does the C represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

chemical symbol

38.

What does the 6 represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

chemical symbol

39.

What does 12.011 represent?

a)

atomic mass

b)

atomic number

c)

element name

d)

chemical symbol

40.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
41.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

42.
What is the name of this element?
a)
Beryllium
b)
Boron
c)
Barium
d)
Bromine
43.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

44.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

45.
This is the correct dot diagram for nitrogen, group 15.
a)
true
b)
false
46.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
47.

Which of the following shows a correct Lewis dot structure?

a)
b)
c)
d)
48.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
49.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)
50.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
51.

What is the formula of this molecule?

a)

CH

b)

HC4

c)

CH4

d)

C4H4

52.

This could be the dot diagram of

a)

Si

b)

Br

c)

B

d)

S

53.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

54.

Is this the correct structure for CH2O?

a)

Yes

b)

No

55.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
56.

Is this an element or a compound? CaSO4CaSO_4  

a)

Element

b)

Compound

57.

What is the total number of atoms in this chemical formula? C8H3NaBr12C_8H_3NaBr_{12}  

a)

18

b)

12

c)

25

d)

24

58.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
59.
How many Magnesium are in 10MgCl2?
a)
10
b)
5
c)
20
60.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
61.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
2
c)
8
d)
24
62.
How many atoms are there TOTAL in:
H2SO4
a)
6
b)
5
c)
7
d)
3
63.
Number of N in (NH₄)₂CrO₄
a)
1
b)
2
c)
8
d)
16
64.
How many Sodium (Na) are in 6NaCl?
a)
1
b)
12
c)
6
65.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
66.

How many unique elements are in this chemical formula?

H2SO4H_2SO_4  

a)

1

b)

2

c)

3

d)

4

67.

How many unique elements are in this chemical formula? NaHCO3NaHCO_3  

a)

1

b)

2

c)

3

d)

4

68.

How many unique elements are in C6H12O6?

a)

1

b)

2

c)

3

d)

4

69.
What do we call a substance consisting of a single atom?
a)
coefficient
b)
element
c)
compound
d)
molecule
70.
What do we call a chemical substance made up of 2 or more different types atoms bonded together?
a)
formula
b)
atom
c)
subscript
d)
compound
71.
A recipe for a chemical substance is called a ________ _________.
a)
coefficent
b)
chemical formula
c)
Oxygen
d)
atom
72.
H2O2← ?
This number tells the number of atoms present.
a)
coefficient
b)
molecule
c)
subscript
d)
atom
73.
→2H2O
This number tells how many molecules are in a chemical equation.
a)
coefficient
b)
subscript
c)
compound
d)
element
74.

What element is this?

a)

Boron

b)

Carbon

c)

Nitrogen

d)

Lithium

75.

What element is this?

a)

Helium

b)

Oxygen

c)

Sodium

d)

Phosphorous

76.
What is the name of the group that never reacts--ever ever they are stable with a full outermost ring!!!
a)
noble gases
b)
transition
c)
halogens
d)
borons
77.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

78.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

79.

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

80.
How many total electrons does O-2 (an oxide ion) have?
a)
8
b)
10
c)
6
d)
18
81.
How many total electrons does Mg+2 (a magnesium ion) have?
a)
10
b)
12
c)
14
d)
22
82.
Lowest energy state of an atom
a)
Ground
b)
Excited
83.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
84.
Which is a possible excited state electron configuration for Silicon?
a)
2-8-4
b)
1-9-4
c)
2-8-8
d)
2-8-3-1
85.

What is a possible excited state electron configuration of Ne?

a)

2-8-8

b)

2-7-1

c)

2-8

d)

2-7

86.

Which shows the right valence electrons?

a)

A

b)

B

c)

C

d)

D

87.

Which shows the right valence electrons?

a)

A

b)

B

c)

C

d)

D

88.

The positive ions tend to _____________ electrons.

a)

lose

b)

gain

89.

The negative ions tend to _____________ electrons.

a)

lose

b)

gain

90.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
91.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
92.

Where are metals located on the periodic table?

a)

Blue

b)

Orange

c)

Yellow

d)

Red

93.

What does the 6 represent?

a)

Atomic mass

b)

Atomic number

c)

Isotope

d)

Atomic Symbol

94.

Looking at the periodic table, when the alkali metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

95.

Looking at the periodic table, when the alkaline earth metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

96.

Looking at the periodic table, when the halogens form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

97.

The elements that do not ordinarily form compounds are

a)

elements in the carbon family

b)

metals

c)

halogens

d)

noble gases

98.
The core of an atom where most of the mass of an atom exists; contains protons and neutrons
a)
nucleus
b)
electron shell
c)
proton
d)
electron
99.

Which group of elements shares characteristics with both metals and nonmetals?

a)

salts

b)

metalloids

c)

halogens

d)

lanthanides

100.

Salts

a)

Ionic Bond

b)

Covalent Bond

101.
Absorption of energy by an electron results in 
a)
it moving from the ground to an excited state
b)
it moving from an excited to the ground state
c)
the emission of a photon
d)
it moving from an excited to the ground state and the emission of a photon
102.

What form of energy is emitted when an excited electron returns to the ground state?

a)

Photon (light)

b)

Heat

c)

Kinetic

d)

Potential

103.
What are electrons in the outermost energy level called?
a)
valence electrons
b)
bonus electrons
c)
protons
d)
orbitals
104.

When Li and Cl bond to form LiCl, this is known as an

a)

Ionic Bond

b)

Hydrogen Bond

c)

Salt Bond

d)

Flame Bond

105.

When Na and Cl bond to form NaCl, this is known as an

a)

Ionic Bond

b)

Hydrogen Bond

c)

Salt Bond

d)

Flame Bond

106.

When K and Cl bond to form KCl, this is known as an

a)

Ionic Bond

b)

Hydrogen Bond

c)

Salt Bond

d)

Flame Bond

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