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Chemistry Review

Total questions: 75

Worksheet time: 2hrs 5mins

Name
Class
Date
1.

What below is NOT considered matter?

a)

Carbon atoms

b)

Light

c)

Bacteria

d)

Air

2.

Matter is anything that.....

a)

Has mass and takes up space

b)

Has mass and is visible

c)

Takes up space and has energy

d)

Has energy and is visible

3.

What is the best classification for this substance?

a)

An element

b)

A compound

c)

A mixture

d)

An atom

4.

Does this particle view show an element or a compound?

a)

element

b)

compound

5.

How many different TYPES of ATOMS are in this image?

a)

1

b)

2

c)

3

d)

4

6.

How many TOTAL MOLECULES are in this image?

a)

4

b)

5

c)

15

d)

20

7.
Subatomic particle with a charge of 0
a)
neutron
b)
proton
c)
electron
d)
quark
8.
These will determine what element an atom is. 
a)
number of neutrons
b)
number of electrons
c)
number of atoms 
d)
number of protons 
9.

The number 16 for the element sulfur is the

a)

ionic number

b)

isotope

c)

atomic mass

d)

atomic number

10.

How many protons does sulfur have?

a)

32

b)

16

c)

48

d)

12

11.

How many electrons does sulfur have

a)

16

b)

32

c)

48

d)

12

12.
What is the atomic mass of "F"
a)
9
b)
18
c)
17
d)
19
13.

In a neutral atom, the number of protons is equal to the number of ____________.

a)

energy levels

b)

neutrons

c)

neurons

d)

electrons

14.

Which of the following is not a subatomic particle? 

a)
the nucleus 
b)

a proton

c)

an electron

d)

a neutron

15.

How many neutrons does potassium K contain? (click to see image)

a)
19
b)
39
c)
20
d)

58

16.

How many electrons does an Iodine atom have?

a)

53

b)

126

c)

73

d)

179

17.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

18.

The center of an atom is known as the

a)

nucleus

b)

electron cloud

c)

neutron cloud

d)

mass circle

19.
These particles have a mass of 1 amu
a)
protons and neutrons
b)
protons and electrons
c)
neutrons and electrons
20.
Protons have this type of charge
a)
positive
b)
negative
c)
neutral - no charge
21.
A particle that orbits around the nucleus is a(n)...
a)
Proton
b)
Neutron
c)
Electron
d)
Quark
22.

What does the nucleus of an atom contain?

a)

Electrons and neutrons

b)

Protons and neutrons

c)

Neutrinos and positrons

d)

Electrons and megatrons

23.
The two areas of an atom are the 
a)
nucleus and electron cloud
b)
proton cloud and nucleus
c)
inside and outside
d)
mass and volume
24.

How many atoms are in this molecule?

a)

1

b)

2

c)

3

d)

4

25.
The mass of one proton is greater than the mass of one...
a)
neutron
b)
electron
26.
Which letter represents a neutron?
a)
A
b)
B
c)
C
d)
D
27.
Which letter represents an electron?
a)
A
b)
B
c)
C
d)
D
28.
What is an atom mostly made up of?
a)
protons
b)
electrons
c)
empty space
d)
neutrons
29.

What is the mass number for an atom that has 3 protons, 5 neutrons, and 3 electrons?

a)

3

b)

5

c)

8

d)

6

30.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
31.

How many neutrons in Carbon-14?

a)
6
b)
7
c)
14
d)
8
32.

What is the name of an isotope of magnesium that has 12 protons and 13 neutrons

a)

Magnesium-12

b)

Magnesium-13

c)

Magnesium-25

d)

Magnesium-24.305

33.

Isotopes are atoms of the same element that have a different masses due to having different numbers of _

a)

Protons

b)

Neutrons

c)

Electrons

d)

Masses

34.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
35.
Electrons are not factored into atomic mass because:
a)
They are so small their mass is negligible
b)
They're not in the nucleus
c)
They're too big
d)
They move so quickly their mass is zero
36.
The nucleus of an atom can be described as:
a)
spacious and negatively charged
b)
dense and positively charged
c)
spacious and positively charged
d)
dense and negatively charged
37.

The number of protons is equal to the number of electrons for an atom. This means an atom is-

a)

electrically neutral

b)

electrically positive

c)

electrically negative

38.

Which part of the atomic theory did JJ Thomson prove?

a)

there are electrons

b)

electrons are in energy levels

c)

there is a nucleus

d)

cathode ray tube

39.

How many electrons can the d sublevel (the d orbitals) hold?

a)

14

b)

10

c)

2

d)

6

40.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
41.

Each orbital can hold how many electrons?

a)

5

b)

4

c)

8

d)

2

42.

In an electron configuration, what follows 4s?

a)

4p

b)

3d

c)

4s

d)

2f

43.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
44.

What is the noble gas configuration for beryllium (symbol Be)?

a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
45.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
46.

Line emission spectra is produced from atoms when

a)

electrons release energy as they move to their excited state.

b)

electrons absorb energy as they move to their excited state.

c)

electrons release energy as they return to the ground state.

d)

electrons absorb energy as they return to the ground state.

47.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
48.

A ground state electron is

a)

freshly crushed into a fine powder.

b)

in the highest possible energy level.

c)

in the lowest possible energy level.

d)

constantly emitting light.

49.

The line with the shortest wavelength (in other words the greatest energy) is produced in the hydrogen spectrum when electron moves

a)

from n=2 to n=1

b)

from n=4 to n=1

c)

from n=3 to n=1

d)

from n=4 to n=3

50.

How many electron energy levels does this element have?

a)

1

b)

2

c)

3

d)

0

51.

How many valence electrons does this atom have?

a)
2
b)
3
c)
5
d)
10
52.

Which Bohr model represents Neon?

a)
b)
c)
d)
53.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
54.

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

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

55.

How many electrons are in 1s2 2s2 2p4?

a)

5

b)

6

c)

8

d)

13

56.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

57.

What is the name of group number 1 on the periodic table?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

58.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

59.

A row on the Periodic Table of Elements is called

a)

family

b)

period

c)

row

d)

isotope

60.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

61.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

62.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

63.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

64.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

65.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

66.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
67.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
68.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
69.
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
70.
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.
71.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
72.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
73.

The 3 types of chemical bonds are ________, ________, and ______. (Choose 3)

a)

ionic

b)

valence

c)

covalent

d)

metallic

e)

atomic

74.

A bond between two nonmetal atoms is a __________ bond.

a)

ionic

b)

nuclear

c)

metallic

d)

covalent

75.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2

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