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Unit 3 Test Review (Atomic Theory)

Total questions: 75

Worksheet time: 1hrs 14mins

Name
Class
Date
1.

Which subatomic particle determines the type of element the atom represents and is called the 'atomic number'?

a)

proton

b)

neutron

c)

electron

d)

boron

2.

How many neutrons are in the atom Potassium-39"?

a)

29

b)

19

c)

58

d)

20

3.

Atoms with the same number of protons, but a different number of neutrons are known as:

a)

ions

b)

mixtures

c)

isotopes

d)

compounds

4.
The atomic mass is equal to _.
a)
the number of protons only
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons, neutrons, and electrons.
5.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
6.

When an atom loses an electron, it becomes a

a)

Cation

b)

Anion

c)

neutral ion

d)

neutral atom

7.

An atom has 11 protons, 10 electrons, and 12 neutrons. What is the mass number of this element?

a)

12

b)

33

c)

11

d)

23

8.

An atom has 27 protons, 25 electrons, and 26 neutrons. What is atom's charge?

a)

+2

b)

+1

c)

0

d)

-1

e)

-2

9.

An atom has 11 protons, 10 electrons, and 12 neutrons. What element is this?

a)

Magnesium (Mg)

b)

Sodium (Na)

c)

Scandium (Sc)

d)

Vanadium (V)

10.
How many protons does this atom have?
a)
2.5
b)
6
c)
5
d)
10.811
11.

How many electrons are in this element if its electrically neutral?

a)

35

b)

45

c)

0

d)

80

12.

What is the symbol and charge of a Calcium ion?

a)

Ca1+

b)

Ca2+

c)

Ca1-

d)

Ca2-

13.

What is the symbol and charge of an Oxygen ion?

a)

O-3

b)

O-

c)

O2+

d)

O-2

14.

What is the symbol and charge of a Nitrogen ion?

a)

N-2

b)

N-4

c)

N3-

d)

N+2

15.

Which of the following tend to gain electrons when forming ions?

a)

metalloids

b)

metals

c)

nonmetals

d)

cations

16.

Acids give away

a)

H+ in water

b)

OH− in water

c)

Carbon in water

d)

None of these

17.

Bases generate this when added to water.

a)

H+

b)

OH−

c)

Neutrons

d)

Electrons

18.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
19.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
20.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
21.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
22.

What are the vertical columns on the periodic called?

a)

groups

b)

periods

c)

nonmetals

d)

metals

e)

metalloids

23.

Which element is similar to Mg?

a)

Ca

b)

B

c)

O

d)

Cl

24.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

25.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

26.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
27.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
28.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
29.
The name of P₄S₁₀ is
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
30.
The name of SO₃ compound is
a)
sulfate
b)
sulfur oxide
c)
sulfur trioxide
d)
monosulfur trioxide
31.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
32.

The chemical formula of Iron (III) bromide is

a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
33.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

34.

What is the name of AlF3AlF_3  ?

a)

aluminum fluorate

b)

monoaluminum trifluoride

c)

aluminum fluoride

d)

aluminum trifluoride

35.
HBr
a)
hydrogen bromine acid
b)
hydrobromide acid
c)
hydrobromic acid
d)

Bromic acid

36.
Name the following hydrate:  NaCl * 5H2O
a)

sodium chloride pentahydroxide

b)

sodium chlorate pentahydrate

c)
sodium chloride pentahydrate
d)

sodium chloride

37.
A compound is a hydrate when it...
a)
is composed of only hydrogen and oxygen
b)
is a state of water
c)

contains water in the ionic compound

d)
repels water from the compound
38.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfur tetraoxide

d)

Sodium sulfuroxide

39.

a three-dimensional geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions

a)

crystal lattice

b)

delocalized electrons

c)

electrolyte

d)

electron sea model

40.

The correct name for TiCl4TiCl_4  is:

a)

titanium (IV) chloride

b)

titanium tetrachloride

c)

titanium (II) chloride

d)

titanium (I) chloride

41.

Name the following compound: Na2CO3

a)

Disodium monocarbon trioxide

b)

Sodium carbonate

c)

Sodium carbide

d)

Disodium carbonate

42.

Rutherford's "gold-foil" experiment using alpha particle scattering concluded that

a)

the center of the atom is empty

b)

atomic mass is spread over the whole atom

c)

the center of the atom has a negative charge

d)

most of the atom is empty except for a very tiny nucleus

43.

All of the following are true about John Dalton's atomic theory EXCEPT ______.

a)

Everything is made up of atoms

b)

Atoms of different elements vary in size and shape.

c)

Atoms are composed of subatomic particles.

d)

Atoms combine to form Compounds in fixed ratios

44.

What did James Chadwick's irradiation of Beryllium foil discover?

a)

Atoms

b)

Electrons

c)

Protons

d)

Neutrons

45.

What did Thomson's experiment with the Cathode Ray Tube discover?

a)

Atoms

b)

Neutrons

c)

Electrons

d)

Protons

46.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
47.
Ca +2  and  OH -
a)
Ca2OH
b)
CaOH2
c)
Ca(OH)2
d)
correct answer is not given
48.

The Law of Conservation of Mass says that matter can neither be __________ or __________.

a)

created; destroyed

b)

recycled; renewed

c)

subtracted; added

d)

joined; separated

49.

What did Millikan's oil droplet experiment tell us about the atom?

a)

Atom's have neutrons

b)

Atoms' have a nucleus

c)

Charge of an electron

d)

Charge of a proton

50.

How many electrons does the following particle have?

a)

42

b)

40

c)

20

d)

18

e)

22

51.

How many neutrons does the following particle have?

a)

42

b)

40

c)

20

d)

18

e)

22

52.

How many protons does the following particle have?

a)

42

b)

40

c)

20

d)

18

e)

22

53.

Which of the following is an Alkali Metal?

a)

Rb

b)

Ba

c)

Fe

d)

Al

54.

Which of the following is an Alkaline Earth Metal?

a)

Rb

b)

Ba

c)

Fe

d)

Al

55.

Which of the following is a Transition Metal?

a)

Rb

b)

Ba

c)

Fe

d)

Al

56.

Ions come together in Ionic compounds to make the overall charge:

a)

Neutral

b)

Postive

c)

Negative

57.

Which of the following shows an Acid reacting with a Base?

a)

4Fe + 3O2 → 2Fe2O3

b)

HNO3 + NaOH

→ NaNO3 + H2O

c)

HCl + K → KCl + H2

d)

Ca(OH)2 + NiCl2 → CaCl2 + Ni(OH)2

58.

What is different between the organic compounds: Hexane and Methane?

a)

The presence of double bonds

b)

The number of carbon atoms

c)

The number of hydrogen atoms

d)

The presence of functional groups

59.

What is different between the organic compounds Hexane and Hexene?

a)

The number of carbon atoms

b)
Hexane is a cyclic compound, while Hexene is a linear compound.
c)

The number of functional groups

d)

The type of bond between carbon atoms.

60.

What is a functional group in an organic hydrocarbon?

a)

A group of atoms that determines the number of carbons.

b)
A group of atoms that determines the shape of the molecule.
c)

A group of atoms that determines the presence of double bonds.

d)
A specific group of atoms that determines the chemical properties and reactivity of the molecule.
61.

Which of the following elements is not diatomic?

a)
oxygen
b)
nitrogen
c)
carbon
d)
hydrogen
62.

True or False: Hydrate compounds can have their water removed by heating and then can reabsorb the water back into its crystal lattice.

a)
False
b)
True
63.

True or False: Carbohydrates are a special type of Hydrate because they also give off water when heated.

a)
True
b)
False
64.

What is different between the compounds Sodium Chlorate vs Sodium Chlorite?

a)

The number of sodium atoms

b)

The number of chlorine atoms

c)

The number of oxygen atoms

d)

The charge of the ion

65.

True or False: The elemental oxygen in the air has a charge of -2.

a)
True
b)
False
66.

True or False: The elemental nitrogen in the air is neutral.

a)
True
b)
False
67.

True or False: Noble gases do not form chemical compounds.

a)
False
b)
True
68.

True or False: Carbon tends to form a charge of -4 in compounds.

a)
False
b)
True
69.

Which part of the periodic table would have elements that are similar?

a)

Vertical columns

 ↓

b)

Horizontal Rows

→

c)

Up and to the Right diagonal

↗ 

d)

Down and to the Right diagonal

↘

70.

True or False: Isotopes of the same element have identical chemical properties.

a)
True
b)
False
71.

True or False: Atoms and Ions of the same element have identical chemical properties.

a)
True
b)
False
72.

What type of bonding is found in molecular compounds?

a)
covalent bonding
b)

electrostatic bonding

c)
metallic bonding
d)
ionic bonding
73.

Which of the following is an Ionic compound?

a)

ZnS

b)

Zn + Ni

c)

SF6

d)

H2SO4

74.

What is the name of the following compound: H2SO4

a)

Sulfuric acid

b)

Hydrosulfuric acid

c)

Hydrogen Sulfate

d)

Hydrogen Sulfide

75.

Which of the following is illustrated by Joseph Proust’s Law of Definite Proportions?

a)

Helped explain why atoms of one element are different from atoms of another element.

b)

Showed the total mass of chemical reactants was equal to the mass of products in a chemical reaction.

c)

Elements always combine in the same relative mass quantities when forming compounds.

d)

All small particles can be found to randomly tumble under a microscope (even when in dilute solutions).

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