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Chemistry: 1st Semester Test

Total questions: 100

Worksheet time: 30hrs 13mins

Name
Class
Date
1.

A _____ property of water is that it is unreactive with oil.

a)

Physical

b)

Chemical

c)

Mixture

d)

Bonding

2.

_____ is an example of a physical change.

a)

Freezing

b)

Rusting

c)

Burning

d)

Digesting

3.

Substances have a definite volume and an indefinite shape in the _____ state.

a)

Gas

b)

Solid

c)

Liquid

d)

Molten

4.

Anything that has mass or volume is called _____.

a)

Temperature

b)

Matter

c)

Energy

d)

Work

5.

Phase changes are classified as _____ changes.

a)

Physical

b)

Chemical

c)

Homogenous

d)

Compound

6.

In the gas state, a substance will have a(n) _____ volume.

a)

Indefinite

b)

Definite

c)

Fixed

d)

Equal

7.

In a compound the elements are _____ together, whereas in a mixture the substances are blended together.

a)

Meshed

b)

Mixed

c)

Wired

d)

Bonded

8.

A taco is an example of a _____.

a)

Element

b)

Heterogeneous Mixture

c)

Compound

d)

Homogeneous Mixture

9.

copper (II) chloride (CuCl₂) is a _____

a)

Element

b)

Heterogeneous Mixture

c)

Compound

d)

Homogeneous Mixture

10.

water (H₂O) is a _____

a)

Element

b)

Heterogeneous Mixture

c)

Compound

d)

Homogeneous Mixture

11.

Trix® cereal is a _____

a)

Element

b)

Heterogeneous Mixture

c)

Compound

d)

Homogeneous Mixture

12.

potassium (K) is a _____

a)

Element

b)

Heterogeneous Mixture

c)

Compound

d)

Homogeneous Mixture

13.

Dissolving salt is a _____ change.

a)

Physical Change

b)

Chemical Change

14.

Boiling water is a _____

a)

Physical Change

b)

Chemical Change

15.

Digesting Taco Bell® is a _____

a)

Physical Change

b)

Chemical Change

16.

The name of the type of ion when electrons are lost (ion is positive) is _____.

a)

Lation

b)

Anion

c)

Onion

d)

Cation

17.

The atomic mass is measured in _____.

a)

Kilograms

b)
Grams
c)

Atomic mass units

d)
Pounds
18.

Electrons are found in the _____ around the nucleus.

a)
Electron cloud
b)
Proton field
c)
Neutron zone
d)
Photon belt
19.

Cations are formed by electrons being _____.

a)

Gained

b)

Lost

c)
Shared
d)
Transferred
20.

Like or same charges _____ each other.

a)
Repel
b)
Attract
c)
Neutralize
d)
Ignore
21.

An atom is said to be _____ when the number of protons equals the number of electrons.

a)
Neutral
b)
Positive
c)
Negative
d)
Charged
22.

_____ saw that particles in a gas were attracted to the positive plate of the cathode ray.

a)

Einstein

b)
Rutherford
c)
Bohr
d)

Thomson

23.

Atomic mass is an average of the elements _____.

a)

Molecules

b)

Isotopes

c)
Compounds
d)
Ions
24.

The group of elements that tend to gain electrons is _____.

a)

Metals

b)

Nonmetals

c)
Noble gases
d)
Metalloids
25.

_____ said that atoms of the same element are the same but atoms of different elements are different.

a)
Dalton
b)
Einstein
c)
Bohr
d)
Rutherford
26.

Isotopes have the same number of protons but have different number of _____.

a)

Protons

b)
Electrons
c)

Neutrons

d)
Atoms
27.

_____ said that an atom is mostly empty space.

a)

Thomson

b)
Einstein
c)
Bohr
d)

Rutherford

28.

The first scientist who thought about atoms was _____.

a)

Einstein

b)
Aristotle
c)
Newton
d)

Democritus

29.

The nucleus of an atom is _____

a)

Negatively charged and has a low density.

b)

Negatively charged and has a high density.

c)

Positively charged and has a low density.

d)

Positively charged and has a high density.

30.

Which of the following statements below is FALSE?

a)

Electrons have a negative charge

b)

Electrons have a mass of 1 amu

c)

The nucleus of an atom is positively charged

d)

The neutron is found in the nucleus of an atom

31.

An atom of an element with atomic number 48 and mass number 120 contains _____

a)

48 protons, 48 electrons, and 72 neutrons

b)

72 protons, 48 electrons, and 48 neutrons

c)

120 protons, 48 electrons, and 72 neutrons

d)

72 protons, 72 electrons, and 48 neutrons

32.

The number 13 in the name carbon-13 represents _____

a)

The atomic number

b)

The mass number

c)

The sum of protons and electrons

d)

None of these

33.

_____ is not true.

a)

Atoms of the same element can have different numbers of neutrons and be called isotopes

b)

The nucleus of an atom has a positive charge

c)

Atoms of isotopes of an element have different numbers of protons

d)

Atoms are mostly empty space

34.

Atoms that have the same number of electrons are _____ with each other.

a)
Isoelectronic
b)
Isotopic
c)
Isobaric
d)
Isomeric
35.

Electrons closest to the nucleus of an atom are _____ in energy.

a)
Lowest
b)
Highest
c)
Moderate
d)
Variable
36.

The 2nd energy level contains these sublevels: _____.

a)
s, p
b)
s, d
c)
p, d
d)
s, f
37.

The s sublevel resembles this type of motion (shape): _____.

a)

Spiral

b)
Cube
c)

Sphere

d)
Cylinder
38.

Elements lose or gain electrons to become like this group of elements: _____.

a)

Transition Metals

b)
Halogens
c)
Alkali metals
d)

Noble gases

39.

Electrons located in the outermost energy level of an atom are called:

a)

Outermost electrons

b)

Valence electrons

c)

Aufbau electrons

d)

Principle energy levels

e)

Variance electrons

40.

Calcium loses two electrons. What element is it isoelectronic with?

a)

Ar

b)

Ne

c)

Kr

d)

Ti

e)

Xe

41.

A f sublevel can hold a maximum of _____ electrons, with only _____ electrons in each orbital.

a)
2, 6
b)
6, 2
c)
2, 14
d)
14, 2
e)
10, 2
42.

The n=_____ shell is the lowest in energy that may contain p-orbitals.

a)
2
b)
3
c)
4
d)
5
e)
6
43.

How many electrons can be found in the first energy level?

a)

6

b)

3

c)

0

d)

1

e)

2

44.

Which of the following energy levels can only have an s and p orbital?

a)

3

b)

4

c)

1

d)

6

e)

2

45.

The elements in group 17 are called ___.

a)
Halogens
b)

Alkali Metals

c)

Alkaline Earth Metals

d)

Noble Gases

46.

Tendency for an atom to attract electrons when chemically bonded to another atom

a)

Ionization Energy

b)

Electronegativity

c)

Electron Energy

d)

Atomic Radii

47.

A term for metalloids that conduct electricity at high temperatures

a)

Insulators

b)

Conductors

c)

Semiconductors

d)

Semi-insulators

48.

Name for group 3-12 elements

a)
Transition metals
b)

Rare Earth Metals

c)

Alkaline Earth Metals

d)

Alkali Metals

49.

The present day Periodic Table is arranged in order of increasing ___.

a)

Atomic Reactivity

b)

Atomic Mass

c)

Atomic Radii

d)

Atomic Number

50.

The property of metals to be made into wire is called ___.

a)
Ductile
b)

Malleable

c)

Conductivity

d)

Reactivity

51.

Name for group 2 elements

a)
Alkaline earth metals
b)

Alkali Metals

c)

Transition Metals

d)

Rare Earth Metals

52.

A property of nonmetals is that they are ___.

a)
Brittle
b)

Lustrous (shiny)

c)

Hard

d)

Conductive

53.

The anion form of an atom is always ________ than its neutral form.

a)

Smaller

b)

Larger

c)

The same

d)

Crazier

e)

Unable to tell

54.

The cation form of an atom is always ________ than its neutral form.

a)

Energy

b)

Larger

c)

The same

d)

Identical

e)

Smaller

55.

The ____ of an atom is found by measuring the distance between the nuclei of two like atoms and halving that distance.

a)

Electronegativity

b)

Atomic size

c)

Ionic Size

d)

Ionization Energy

e)

None of these

56.

A triple covalent bond shares ________ electrons between atoms.

a)

five

b)

four

c)

three

d)

six

e)

two

57.

Which of the following sets of atoms can be joined by a covalent bond? Please circle the most correct answer. Write your answer on the given lines.

a)

S and F

b)

Mg and Na

c)

Li and Cl

d)

Be and F

e)

Na and Cl

58.

Why do atoms form ionic and covalent bonds?

a)

to attain a noble-gas electron configuration

b)

to become ions and attract each other

c)

to become more polar

d)

to increase their atomic numbers

e)

None of these

59.

Which of the following elements does not want to have eight valence electrons?

a)

magnesium

b)

oxygen

c)

fluorine

d)

hydrogen

e)

nitrogen

60.

An ionic compound is _______.

a)

composed of anions and cations

b)

held together by ionic bonds

c)

Composed of metals and non-metals

d)

all of the above

61.

Ionic compounds are normally in which physical state at room temperature?

a)

gas

b)

solid

c)

liquid

d)

plasma

e)

all of the above

62.

Which is NOT a characteristic of most ionic compounds?

a)

they have low melting points

b)

they are composed of metallic and non-metallic elements

c)

they are likely to conduct an electric current

d)

they are solids

e)

none of the above

63.

Why do atoms share electrons in covalent bonds?

a)

to become ions and attract each other

b)

to increase their atomic numbers

c)

to attain a noble-gas electron configuration

d)

to become more polar

64.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
5
65.
If a sulfur atom has 16 protons, 16 electrons, and 16 neutrons, its atomic mass is:
a)
16
b)
32
c)
48
66.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
67.
How is carbon-12 different from carbon-14?
a)
They have a different number of protons
b)
they have a different number of electrons
c)
they have a different number of neutrons
68.
If neutral copper atom (atomic number 29) becomes an ion that has a charge of 2+, how many electrons does the resulting ion have?
a)
27
b)
28
c)
29
d)
31
69.

What does the atomic number identify?

a)

The number of neutrons of a given atom.

b)

The number of protons of a given atom.

c)

The number of neutrons and protons of a given atom.

d)

The number of electrons of a given atom.

70.

How many neutrons are in the isotope Carbon-14

a)

6

b)

8

c)

14

d)

12

71.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
72.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
73.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
74.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
75.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
76.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
77.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
78.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

79.

How many neutrons does this Neon atom have?

a)

21

b)

11

c)

10

d)

12

80.

What is the mass number of this Neon atom?

a)

10

b)

11

c)

21

d)

20

81.

What type of atom is this?

a)

Neutral atom

b)

Cation

c)

Anion

d)

Isotope

82.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
83.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
84.
An element has three different isotopes. One has a mass of 35.00 amu; another has a mass of 36.00  amu; and another has a mass of 38.00  amu. What is the average atomic mass of this element?
a)
36.33 amu
b)
37.00 amu
c)
12.11 amu
d)
impossible to tell
85.
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
86.
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.
87.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
88.
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
89.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
90.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
91.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
92.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

93.

According to the diagram below, how many bonds will this atom be able to make?

a)
1
b)
2
c)
3
d)
4
94.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
95.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
96.

What type of bond is formed by the transfer of electrons from one atom to another?

a)

Covalent bond

b)

Metallic bond

c)

Ionic bond

d)

Hydrogen bond

97.

Which particle is responsible for bonding?

a)

Electrons

b)

Protons

c)

Nucleus

d)

Neutrons

98.

Examine the image: How many bonds are formed looking at the model of the compound? And also indetify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

99.

Ionic bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

Depends on the situation

100.

Covalent bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

It depends on the situation

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