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Chemistry Semester 2 Cumulative Test

Total questions: 91

Worksheet time: 2hrs 11mins

Name
Class
Date
1.

Orbital

a)

a region in an atom where there is a high probability of finding electrons.

b)

an electron that is found in the outermost shell of an atom and that determines the atom’s chemical properties.

c)

The energy level at which electrons orbit the nucleus of an atom

d)

a subdivision of electron shells

2.

Valence Electron

a)

a region in an atom where there is a high probability of finding electrons.

b)

an electron that is found in the outermost shell of an atom and that determines the atom’s chemical properties.

c)

The energy level at which electrons orbit the nucleus of an atom

d)

a subdivision of electron shells

3.

Electron Shell

a)

a region in an atom where there is a high probability of finding electrons.

b)

an electron that is found in the outermost shell of an atom and that determines the atom’s chemical properties.

c)

The energy level at which electrons orbit the nucleus of an atom

d)

a subdivision of electron shells

4.

Electron Subshell

a)

a region in an atom where there is a high probability of finding electrons.

b)

an electron that is found in the outermost shell of an atom and that determines the atom’s chemical properties.

c)

The energy level at which electrons orbit the nucleus of an atom

d)

a subdivision of electron shells

5.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
6.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
7.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
8.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
9.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
10.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
11.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
12.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
13.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
14.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
15.
Identify this atom: 
a)
Lithium
b)
Chlorine
c)
Phosphorus 
d)
Fluorine
16.

Which of the following pictures represents energy shells around an atom (Chem 3.01 Lv 1)

a)
b)
c)
d)
17.

According to the energy shell model, an electron cannot reside at ___ in this figure?

a)

A

b)

B

c)

C

d)

D

18.

How can the energy shells around the nucleus be described?(Chem3.01 Lv2)

a)

They are all identical to each other just larger orbits

b)

Each energy shell has electrons at different energy levels

c)

That the shells get harder as you move away from the nucleus

d)

Energy shells or levels are a scientific myth

19.

Which electron would have the most energy? (Chem3.01 Lv3)

a)

An electron in energy shell 1

b)

An electron in energy shell 2

c)

An electron in energy shell 4

d)

An electron in energy shell 3

20.

Which of the following are correct about orbitals? (Chem3.01 Lv3)

a)

s type subshells have 1 orbital, p-type has 3 orbitals, d type has 5 orbitals, and f type has 7 orbitals.

b)

s type subshells have 7 orbitals, p-type has 5 orbitals, d type has 3 orbitals, and f type has 1 orbital.

c)

s type subshells have 1 orbital, p-type has 7 orbitals, d type has 5 orbitals, and f type has 3 orbitals.

d)

They all have the same number of orbitals.

21.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

22.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
23.
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
24.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
25.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
26.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
27.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
28.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
29.

What separates metals from non-metals on the periodic table?

a)

The stairstep

b)

oxygen

c)

the magic line

d)

sodium

30.

Metals are on the what side of the periodic table.

a)

Left

b)

Right

c)

Center

d)

They are not on the periodic table

31.

Non-Metals are on the what side of the periodic table.

a)

Left

b)

Right

c)

Center

d)

They are not on the periodic table

32.

The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to

a)

Mendeleev.

b)

Moseley.

c)

Bohr.

d)

Ramsay.

33.

Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing

a)

atomic number.

b)

density.

c)

reactivity.

d)

atomic mass.

34.

The octet rule sates that atoms are seeking to get how many valence electrons? (Chem4.01 Lv1)

a)

2

b)

4

c)

6

d)

8

35.

Atoms will _______ or _________ electrons to get the number of valence electrons to meet the octet rule (Chem4.01 Lv2)

a)

Gain, Lose

b)

Gain, Take

c)

Lose, Give up

d)

Lose all, Gain no

36.

How can you find the number of valence electrons? Check all the apply (Chem4.01 Lv2)

a)

Electron Configuration

b)

Group number on the periodic table

c)

Period Number on the periodic table

d)

Counting the total number of valence electrons

37.

Which of the following elements LOSES 1 electron in order to attain an octet? (Chem4.01 Lv3)

a)

potassium

b)

helium

c)

fluorine

d)

calcium

e)

boron

38.

Which of the following elements GAINS 1 electron in order to attain an octet? (Chem4.01 Lv3)

a)

potassium

b)

helium

c)

fluorine

d)

calcium

e)

boron

39.

Which of the following elements LOSES 2 electrons in order to attain an octet? (Chem4.01 Lv3)

a)

potassium

b)

helium

c)

fluorine

d)

calcium

e)

boron

40.

Which of the following elements GAINS 2 electrons in order to attain an octet? (Chem4.01 Lv3)

a)

aluminum

b)

helium

c)

nitrogen

d)

sulfur

e)

boron

41.

A covalent bond forms when atoms ___________ electrons. (Chem4.02 Lv1)

a)

gain

b)

increase

c)

share

d)

transfer

42.

Which type of bond has a transfer of an electron from one atom to another? (Chem4.02 Lv1)

a)

Polar Covalent

b)

Ionic

c)

Non-Polar Covalent

d)

Metallic

43.

A bond between a metal and a nonmetal is called a(n) (Chem4.02 Lv2)

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Transfer bond

44.

A bond between a nonmetal and a nonmetal is called a(n) (Chem4.02 Lv2)

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Transfer bond

45.

Which bond shares electrons evenly? (Chem4.02 Lv3)

a)

Non-polar Covalent

b)

Polar Covalent

c)

Ionic

46.

Which bond shares electrons unevenly?(Chem4.02 Lv3)

a)

Non-polar Covalent

b)

Polar Covalent

c)

Ionic

47.

What is the electronegativity difference between Chlorine and Sodium and what bond type do you predict will occur?(Chem4.02 Lv3)

a)

2.1, Ionic

b)

2.1, Non-Polar Covalent

c)

-2.1, Ionic

d)

2.1, Polar Covalent

48.

What is the electronegativity difference between Nitrogen and Florine and what bond type do you predict will occur?(Chem4.02 Lv3)

a)

1, Ionic

b)

1, Non-Polar Covalent

c)

-1, Ionic

d)

1, Polar Covalent

49.

What is the electronegativity difference between Phosphorus and Iodine and what bond type do you predict will occur?(Chem4.02 Lv3)

a)

0.4, Ionic

b)

0.4, Non-Polar Covalent

c)

-0.4, Ionic

d)

0.4, Polar Covalent

50.

Which of the following is a chemical formula? (Chem5.01 Lv1)

a)

Co

b)

C

c)

O-

d)

CO2

51.

The blue numbers in the the image represent what?(Chem5.01 Lv2)

a)

I don't know and don't want to try

b)

coefficients

c)

the number of atoms of that element

d)

the mass of each compound

52.

How many atoms are there TOTAL in: H₂SO₄? (Chem5.01 Lv2)

a)

6

b)

7

c)

3

d)

5

53.

How many Hydrogen atoms are in H₂O? (Chem5.01 Lv3)

a)

1

b)

2

c)

4

d)

Who Cares

54.

What is a cation's charge? (Chem5.04 Lv1)

a)

positive

b)

neutral

c)

negative

d)

depends on the element

55.

What is an anion's charge? (Chem5.04 Lv1)

a)

positive

b)

neutral

c)

negative

d)

depends on the element

56.

What usually form cations?(Chem5.04 Lv1)

a)

Metal

b)

Nonmetal

c)

Metalloid

d)

Semimetal

57.

What usually form anions?(Chem5.04 Lv1)

a)

Metal

b)

Nonmetal

c)

Metalloid

d)

Semimetal

58.

What is the chemical formula for a compound that has the name Sodium Chloride? (Chem5.02 Lv3)

a)

NaCl

b)

Na⁺ Cl⁻

c)

SoCh

d)

Table Salt

59.

What is the chemical formula for a compound that has the name Dihydrogen Monocarbide? (Chem5.02 Lv3)

a)

H2C

b)

H2C1

c)

HC2

d)

HC

60.

What is the chemical formula for a compound that has the name Berlyium Nitrate? (Chem5.02 Lv3)

a)

Be(NO3)2

b)

BeNO3

c)

Be2NO3

d)

BeNo

61.

What is the name of the chemical compound with the formula of CO2? (Chem5.03 Lv3)

a)

Carbon Monoxide

b)

Monocarbon Oxide

c)

Carbon Dioxide

d)

Monocarbon Monoxide

62.

Chemical reaction (Chem7.01 Lv1)

a)

a process in which one or more substances, the reactants, are converted to one or more different substances, the products.

b)

A chemical dissolved in water to form a solution.

c)

the symbolic representation of a chemical reaction in the form of symbols and formulas.

d)

the numbers in front of the formulas in a chemical equation that gives the number of molecules (or atoms) involved in the reaction. Can also represent the number of moles of a chemical substance in a reaction.

63.

Which of the following is a type of chemical reaction? (Chem 7.01 Lv2)

a)

synthesis reaction

b)

react reaction

c)

decomposition reaction

d)

single-replacement reaction

e)

product reaction

64.

Which of the following is a type of chemical reaction? (Chem 7.01 Lv2)

a)

double-replacement reaction

b)

react reaction

c)

combustion reaction

d)

explosion reaction

e)

product reaction

65.

What type of chemical reaction is happening in this reaction:

AgNO₃(ag) + NaCl(aq) ---> NaNO₃(aq) + AgCl(s)?

(Chem 7.01 Lv3)

a)

synthesis reaction

b)

decomposition reaction

c)

single-replacement reaction

d)

double-replacement reaction

e)

combustion reaction

66.

What type of chemical reaction is happening in this reaction:

Cu(s) + 2AgNO₃(aq) ---> Cu(NO₃)₂(aq) + 2Ag(s)?

(Chem 7.01 Lv3)

a)

synthesis reaction

b)

decomposition reaction

c)

single-replacement reaction

d)

double-replacement reaction

e)

combustion reaction

67.

What type of chemical reaction is happening in this reaction:

C₃H₈(g) + 5O₂(g) ---> 3CO₂(g) + 4H₂O(g)?

(Chem 7.01 Lv3)

a)

synthesis reaction

b)

decomposition reaction

c)

single-replacement reaction

d)

double-replacement reaction

e)

combustion reaction

68.

What type of chemical reaction is happening in this reaction:

Na(s) + Cl(g) ---> NaCl(s)?

(Chem 7.01 Lv3)

a)

synthesis reaction

b)

decomposition reaction

c)

single-replacement reaction

d)

double-replacement reaction

e)

combustion reaction

69.

What type of chemical reaction is happening in this reaction:

2NaOH(s) ---> Na₂O(s)+H₂O(g)? (Chem 7.01 Lv 3)

a)

synthesis reaction

b)

decomposition reaction

c)

single-replacement reaction

d)

double-replacement reaction

e)

combustion reaction

70.

Reactant (Chem 7.02 Lv1)

a)

the resulting chemical compounds after a chemical reaction has taken place.

b)

the chemical compounds going into a chemical reaction.

c)

describes a certain event of the natural world, but it does not attempt to explain how or why the event occurs.

d)

a reaction in which one element is substituted for another element in a compound.

71.

Product (Chem 7.02 Lv1)

a)

the resulting chemical compounds after a chemical reaction has taken place.

b)

the chemical compounds going into a chemical reaction.

c)

describes a certain event of the natural world, but it does not attempt to explain how or why the event occurs.

d)

a reaction in which one element is substituted for another element in a compound.

72.

What side of the arrow in a chemical equation is the reactant located? (Chem 7.02 Lv2)

a)

Right

b)

Left

c)

Above arrow

d)

It is not part of a chemical equation

73.

What side of the arrow in a chemical equation is the product located? (Chem 7.02 Lv2)

a)

Right

b)

Left

c)

Above arrow

d)

It is not part of a chemical equation

74.

What does it mean when a chemical is aqueous? (Chem 7.02 Lv3)

a)

It has melted

b)

It does not dissolve in water

c)

It is dissolved in water

d)

It will only react in gas form

75.

What state of matter is HC₂H₃O₂ in for the chemical equation below?

HC₂H₃O₂(aq) + NaHCO₃(s) -----> CO₂(g) + H₂O(l) + NaC₂H₃O₂(aq)

(Chem 7.02 Lv3)

a)

Solid

b)

Liquid

c)

Gas

d)

Aqueous

76.

What state of matter is NaHCO₃ in for the chemical equation below?

HC₂H₃O₂(aq) + NaHCO₃(s) -----> CO₂(g) + H₂O(l) + NaC₂H₃O₂(aq)

(Chem 7.02 Lv3)

a)

Solid

b)

Liquid

c)

Gas

d)

Aqueous

77.

What state of matter is CO₂ in for the chemical equation below?

HC₂H₃O₂(aq) + NaHCO₃(s) -----> CO₂(g) + H₂O(l) + NaC₂H₃O₂(aq)

(Chem 7.02 Lv3)

a)

Solid

b)

Liquid

c)

Gas

d)

Aqueous

78.

What state of matter is H₂O in for the chemical equation below?

HC₂H₃O₂(aq) + NaHCO₃(s) -----> CO₂(g) + H₂O(l) + NaC₂H₃O₂(aq)

(Chem 7.02 Lv3)

a)

Solid

b)

Liquid

c)

Gas

d)

Aqueous

79.

What does the coefficient in front of the chemical compounds represent? (Chem 7.02 Lv3)

a)

Number of molecules

b)

Number of times the reaction need to happen

c)

Number of products

d)

Number of pounds of chemicals needed for the reaction

80.

What is one reason we need to balance chemical equations? (Chem 7.03 Lv2)

a)

Because the teacher told me so

b)

Because the conservation of mass tells us that matter coming out of the reaction needs to equal the matter going into the reaction

c)

Because we need to have even numbers to do math with the equation

d)

Because the conservation of mass tells us that matter can be destroyed and we need to account for the loss of mass

81.

In the flowing chemical equation explain how the law of conservation of mass followed?

C₆H₁₂O₆ + 6O₂ ---> 6CO₂ + 6H₂O

(Chem 7.03 Lv3)

a)

The coefficients account for the amount of matter going into the reaction and the amount of matter coming out of the reaction. Make sure they are the same.

b)

The subscripts account for the amount of matter going into the reaction.

c)

The coefficients allow for more mass to be created

d)

The coefficients allow for more mass to be lost

82.

Which of the following would represent a synthesis reaction involving Magnesium and Bromine? (Chem 7.04 Lv2)

a)

Mg + Br -----> MgBr₂

b)

MgBr₂ ------> Mg + Br

c)

Mg + NaBr ----> Na + MgBr₂

d)

MgBr₂ + NaCl -----> NaBr + MgCl₂

83.

Which of the following would represent a single displacement reaction involving Copper and Silver Nitrate? (Chem 7.04 Lv2)

a)

Cu + Ag -----> CuAg

b)

AgNO₃ ------> Cu+ Cl₃

c)

AgNO₃ + Cu ------> Ag + CuNO₃

d)

AgNO₃ + CuCl₂ -----> AgCl + CuNO₃

84.

Which of the following would represent a combustion reaction of C4H10? (Chem 7.04 Lv2)

a)

C₄H₁₀ -----> C₄ + H₁₀

b)

C + H -----> C₄H₁₀

c)

C₄H₁₀ + O₂ -----> CO₂ + H₂O

d)

C₄H₁₀ + O₂ -----> CH₂ + C₂O

85.

Which coefficients correctly balance the formula equation NH₄NO₂(s) -----> N₂(g) + H₂O(l)? (Chem 7.04 Lv3). The numbers are from left to right.

a)

1, 2, 2

b)

2 on just H2O

c)

2, 1, 1

d)

2, 2, 2

86.
How many Sodium (Na) are in 6NaCl?
a)
1
b)
12
c)
6
87.
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.
88.

Is the following equation balanced?...

4Al + 3O2 --> 2Al2O3

a)

Yes!

b)

No!

89.

Is the following equation balanced?

2C2H2 + O2 --> 4CO2 + 2H2O

a)

yes

b)

no

90.
Is the following equation balanced?
4Fe + 3O2 --> 2Fe2O3
a)
yes
b)
no
91.
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

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