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Chemistry Semester 1 Review

Total questions: 84

Worksheet time: 1hrs 3mins

Name
Class
Date
1.
What is the atomic mass of Copper?
a)
63
b)
29
c)
34
d)
92
2.
How many electrons does Cu4+ have?
a)
29
b)
33
c)
25
d)
30
3.
How many electrons does S2- have?
a)
16
b)
18
c)
14
d)
12
4.
A proton is....
a)
A negatively charged subatomic particle
b)
A positively charged subatomic particle
c)
A neutrally charged subatomic particle
d)
The only subatomic particle located in the nucleus
5.
A neutron has a charge of
a)
+2
b)
No charge
c)
-1
d)
+1
6.
What does the atomic mass tell you?
a)
Basically,the number of electrons and protons
b)
The number of neutrons
c)
Basically, the number of protons and neutrons
d)
The number of protons.
7.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
8.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
9.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
10.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
11.
The first energy level can hold up to how many electrons?
a)
8
b)
4
c)
2
d)
5
12.

Do electrons contribute to the atomic mass of an atom?

a)

YES of course, they are there for a reason

b)

NO, they are useless to the atom

c)

No, their mass is too small to contribute to the mass

d)

YES, silly, they are the superstars of the atom

13.
The number of protons is equal to 
a)
the atomic number
b)
the number of neutrons
c)
the energy levels
d)
the periodic table groups
14.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

15.

which explanation of this notation is correct?

a)

12 is proton #

b)

6 tells you there are 6 neutrons

c)

6 tells you there are 6 protons

d)

12 is not a mass # here

16.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
17.

An ion is

a)

Also a compound

b)

An atom that has gained or lost an electron

c)

An atom that has only gained electrons

d)

An atom where the number of protons=electrons

18.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

19.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

20.

A Beryllium atom that has lost 2 electrons would look like

a)

Be2+

b)

B2-

c)

B2+

d)

Be2-

21.

The cation Rb+ has

a)

Had nothing happen to it

b)

Gained 1 electron

c)

Lost 1 electron

d)

Become negative

22.

Describe the anion S2-

a)

Silicon that gained 2 electrons

b)

Sulfide that gained 2 electrons

c)

Sulfur that gained 2 electrons

d)

Strontium that gained 2 electrons

23.

Which of the following is true of 1 mole of Carbon and 1 mole of Oxygen?

a)

Their molar masses are equal

b)

They have the same atomic mass

c)

They have the same number of subatomic particles

d)

They contain the same number of atoms

24.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

25.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

26.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

27.

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

28.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

29.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

30.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

31.

When naming ionic compounds with transition metals you need to include roman numerals to show the

a)

Charge of the nonmetal

b)

mass number

c)

Charge of the metal

d)

ionization energy of the metal

32.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

33.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

34.

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

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

35.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

36.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

37.

The number that tells you if an ion has lost or gained electrons

a)

atomic number

b)

oxidation number

c)

mass number

d)

electron number

38.

If I gain electrons I become

a)

Positive because I've added to my atom

b)

negative because I've added electrons

c)

same because i'm balanced

d)

equal because now I have electrons

39.

By looking at the formula of an ionic compound, we can determine the charge (oxidation state) of a transition metal.

a)

True

b)

False

40.

The overall charge of an ionic compound ...

a)

depends on the elements that are combined

b)

is always positive

c)

is always neutral

d)

is always negative

41.
Ionic Bonding involves...
a)
The transfer of protons
b)

The sharing of electrons

c)
The transfer of electrons
d)

The sharing of protons

42.

Which structure consists of a giant crystal lattice of cations and anions held together by strong electrostatic forces of attraction?

a)

ionic bonding

b)

covalent bonding

43.

Which of the following types of bonding results in materials which have the lowest melting and boiling points?

a)

ionic bonding

b)

covalent bonding

44.

An atom shares an electron with another atom in a

a)

covalent bond

b)

ionic bond

45.

If a molecule is said to be "polar," that means it

a)

has a charge (positive end and negative end)

b)

has no charge

c)

is a white bear

46.

Which two statements are correct about the figure shown?

a)

It is a covalent bond.

b)

Hydrogen atoms loss electrons and Carbon gains the atoms.

c)

It happens on metal and on another non-metal.

d)

The valence electrons are shared by both atoms.

47.

Check two general properties of a covalent bond.

a)

Hard

b)

Brittle/Soft

c)

Low melting point

d)

poor conductor of electricity when in solid state.

48.

Covalent bonds are formed between

a)

metals

b)

non-metals

c)

metal and non-metal

d)

metalloids

49.

When dissolved in water, the solution is a good conductor of electricity.

a)

ionic compounds

b)

molecular compounds

50.

Classify the following molecule.

a)

polar

b)

nonpolar

51.

Classify the following molecule.

a)

polar

b)

nonpolar

52.
What type of reaction occurs between an element and a compound?
Zn + 2HCl --> ZnCl2 + H2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
53.
What kind of reaction is this:
2C3H7OH +9O2 -> 6CO2 + 8H2O
a)
Double Replacement
b)
Combustion
c)
Single Replacement
d)
Decomposition
54.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
55.
What kind of reaction is this:
2H2 + O2 --> 2H2O
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
56.
Students react baking soda & vinegar.
Which of the following would provide the evidence that the number of atoms present before a chemical reaction is equal to the number of atoms present after the chemical reaction?
a)
The mass of the plastic bag, baking soda, and vinegar before the reaction was equal to the mass after the reaction.
b)
Bubbles were produced during the reaction, which meant that a gas was being produced.
c)
The plastic bag did not change in any way, indicating that it was not involved in the reaction.
d)
The mass of the baking soda was exactly equal to the mass of the vinegar used to create the chemical reaction.
57.
What kind of reaction is this:
2H2O2 →2 H2O + O2
a)
Synthesis
b)
Decomposition
c)
Single Replacement 
d)
Combustion
58.
Suppose a reaction were to happen in an open container in a lab.  During the reaction, the scientist observes the chemicals bubble, and produce a gas.   During the analysis the scientist notices that the reactants weighed 20 g when he started, and the product weighed 18 g.  Explain what happened.  
a)
His chemical reaction defied the law of conservation of mass
b)
The product destroyed mass during the reaction
c)
The reactants created matter during the reaction
d)
The gas that was produced was not able to be weighed since the container was open.  
59.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
60.
If there are 4 H atoms on the reactant side, how many H atoms will be on the product side? 
a)
2
b)
4
c)
6
d)
You need more information to answer this question
61.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
62.
The reaction below is an example of?
AgNO3 + NaCl → AgCl + NaNO3
a)
Single Replacement
b)
Double Replacement
c)
Decomposition
d)
Combustion
63.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
64.

True or false - the number of moles should be the same on the reactants and products side.

a)

True

b)

False

65.

Which of these are subatomic particles

a)

Proton

b)

Neutron

c)

Electron

d)

Cell

e)

Organelle

66.

Identify which subatomic particles have a (non-neutral) charge

a)

Proton

b)

Neutron

c)

Electron

d)

None of these

67.

Identify which subatomic particles have a mass of 1 amu

a)

Proton

b)

Neutron

c)

Electron

d)

None of these

68.

Identify which subatomic particles would be found in the center/nucleus of the atom

a)

Proton

b)

Neutron

c)

Electron

d)

None of these

69.

Identify which subatomic particle determines an atom's identity

a)

Proton

b)

Neutron

c)

Electron

d)

None of these

70.

Identify which subatomic particle determines an atom's stability

a)

Proton

b)

Neutron

c)

Electron

d)

None of these

71.

Identify which subatomic particle determines an atom's reactivity

a)

Proton

b)

Neutron

c)

Electron

d)

None of these

72.

Identify which subatomic particle differs between isotopes of the same atom

a)

Protons

b)

Neutrons

c)

Electrons

d)

None of these

73.

Identify which subatomic particle differs between ions of the same atom

a)

Protons

b)

Neutrons

c)

Electrons

d)

None of these

74.

Identify which of the following is represented by 1.00794 in the symbol to the right

a)

Element Name

b)

Atomic number

c)

Atomic mass

d)

Atomic symbol

75.
Which is an electron?
a)
A
b)
B
c)
C
76.
What is found in the nucleus of atoms?
a)
Protons and electrons.
b)
Protons, neutrons, and electrons.
c)
Protons and neutrons.
d)
Neutrons and electrons.
77.

Match the following

a)

Atoms of the Same Element with a different charge

1.

Ion

b)

A positively charged atom

2.

Cation

c)

A negatively charged atom

3.

Anion

d)

Atoms of the same element with a different mass

4.

Isotope

e)

If I have questions

5.

I ask

78.

In Element Notation the element name is written followed by the...

a)

Atomic Number

b)

Mass Number

c)

Number of Electrons

d)

Charge

79.

In Symbol Notation the number on the top left of the symbol is the...

a)

Atomic Number

b)

Mass Number

c)

Number of Electrons

d)

Charge

80.

In Symbol Notation the number on the bottom left of the symbol is the...

a)

Atomic Number

b)

Mass Number

c)

Number of Neutrons

d)

Charge

81.

The mass of Atoms of the same element will always be the same

a)

True

b)

False

82.

The Number of Protons and Electrons will always be the same as the atomic number

a)

True

b)

False

83.

The Number of Protons and Electrons will always be the same as the atomic number in a Neutral atom

a)

True

b)

False

84.

Match the following

a)

Determines the identify of the atom

1.

Proton

b)

Determines the reactivity of the atom

2.

Electron

c)

Determines the stability of the atom

3.

Neutron

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