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Unit 4 - 6 Test Review

Total questions: 86

Worksheet time: 3hrs 45mins

Name
Class
Date
1.

What is the periodic trend for electronegativity across a period?

a)

Electronegativity remains constant

b)

Electronegativity decreases

c)

Electronegativity is not affected by the period

d)

Electronegativity increases

2.

Which element has the highest electronegativity?

a)

Chlorine

b)

Oxygen

c)

Fluorine

d)

Sodium

3.

What is the periodic trend for ionization energy down a group?

a)

increases

b)

remains constant

c)

decreases

d)

fluctuates

4.

Which element has the lowest ionization energy?

a)

oxygen

b)

lithium

c)

fluorine

d)

helium

5.

What is the periodic trend for atomic radius across a period?

a)

increases

b)

decreases

c)

remains constant

d)

fluctuates

6.

Which element has the smallest atomic radius?

a)

hydrogen

b)

oxygen

c)

helium

d)

nitrogen

7.

What is the periodic trend for electronegativity down a group?

a)

Electronegativity increases

b)

Electronegativity remains constant

c)

Electronegativity fluctuates

d)

Electronegativity decreases

8.

Which element has the largest atomic radius?

a)

Helium (He)

b)

Oxygen (O)

c)

Neon (Ne)

d)

Francium (Fr)

9.

What is the periodic trend for ionization energy across a period?

a)

The ionization energy increases from right to left across a period.

b)

The ionization energy generally increases across a period from left to right.

c)

The ionization energy remains constant across a period.

d)

The ionization energy generally decreases across a period from left to right.

10.

Which element has the highest ionization energy?

a)

helium

b)

nitrogen

c)

oxygen

d)

hydrogen

11.
Which of the following elements in the periodic table have the highest first ionization energies?
a)
transition elements
b)
alkaline earth metals
c)
alkali metals
d)
noble gas elements
12.
Which of the following elements has the smallest radius?
a)
Mg
b)
Al
c)
Si
d)
K
13.
Why do noble gases have the highest first ionization energies?
a)
The principal quantum number increases left to right across the periodic table.
b)
The effective nuclear charge is low.
c)
The electron affinity is zero.
d)
An electron is harder to remove from a noble gas due to it being tightly bound by the inner nucleus.
14.
Which of the elements listed have the largest ionization energy and highest electronegativity?
a)
F
b)
Cl
c)
Br
d)
I
15.
Which of the following electron configurations represents an element with the largest atomic radius?
a)
1s22s22p63s1
b)
1s22s22p63s23p64s2
c)
1s22s22p63s23p63d104s1
d)
1s22s22p63s23p2
16.

Elements in the same family have the same

a)

Atomic numbers

b)

Atomic masses

c)

Number of  valence electrons

17.

Valence electrons are ____________________

a)

Electrons in the nucleus

b)

Electrons found on the inner shell

c)

Electrons found on the outer shell

18.

Choose the set of elements that have the same number of valence electrons

a)

Chlorine, Fluorine, Oxygen

b)

Fluorine, Chlorine, Iodine

c)

Lithium, Magnesium, Potassium

19.

The electronegativity of an atom ________ across a row, and _________ down a column

a)

Decreases, Increases

b)

Increases,

Decreases

c)

Decreases,

Decreases

d)

Increases,

Increases

20.

The ability of an atom to attract electrons that are shared in a bond.

a)

First Ionization Energy

b)

Negative Electron Affinity

c)

Positive Electron Affinity

d)

Electronegativity

21.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
22.

Which has the larger radius?

a)

Na

b)

Na+1

23.

Which has the largest radius?

a)

I

b)

I-1

24.

True or False: Cations are larger than their parent atoms because cations will have more protons than their parent atoms.

a)

True

b)

False

25.

True or False: Anions are larger than their parent atoms. This is due to the fact anions have more electrons compared to their parent atoms, which causes their electron cloud to expand to minimize the electron repulsions.

a)

True

b)

False

26.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

27.

This is a Bohr Diagram of Nitrogen. Nitrogen has

(a)   electrons.

Choose from the below words
7

2

5

28.

This is a Bohr Diagram of Nitrogen. Nitrogen has

​ (a)   valence electrons.

Choose from the below words
7

2

15
5
29.

All elements want ​ (a)   valence electrons except for ​ (b)   who want ​ (c)   valence electrons.

Choose from the below words
8
Hydrogen and Helium
2
group 18
noble gasses
7
1
transition metals
30.
This is a correct dot diagram for oxygen, group 16.
a)
true
b)
false
31.
This is the correct dot diagram for sodium, group 1
a)
true
b)
false
32.
This could be the dot diagram of
a)
Mg, group 2.
b)
Cl, group 17.
c)
C, group 14.
d)
O, group 16.
33.
What does an atom's group number help us determine?
a)
Number of protons
b)
Number of electrons
c)
Number of valence electrons
d)
Number of shells
34.
What is the name of the group that never reacts/is stable with the last energy level full!!!
a)
noble gases
b)
transition
c)
halogens
d)
borons
35.
How many electrons should Nitrogen, group 15, have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
36.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
37.

Ionic bonds form between ---

a)

nonmetals.

b)

metals and nonmetals.

38.

Covalent bonds form between ---

a)

nonmetals.

b)

metals and metals

c)

metals and nonmetals

39.

Atoms that gain an electron have an electric charge of ---

a)

-1.

b)

-2.

c)

+1.

d)

+2.

40.

Atoms form compounds to become more ---

a)

reactive

b)

stable

c)

explosive

d)

toxic

41.

Atoms gain lose, gain, or ______electrons to get a stable outer energy level.

a)

share

b)

split

c)

create

d)

destroy

42.

An atom with a different number of electrons than it should have (more or less) is called an ---

a)

isotope

b)

valence electron

c)

ion

d)

octet

43.

Which of the following is NOT a covalent bond?

a)

K2S

b)

H2O

c)

I2

d)

CO2

44.

Which of the following is NOT an ionic bond?

a)

NH3

b)

KCl

c)

K3N

d)

NaCl

45.

An electron has a ___ charge.

a)

no charge

b)

positive

c)

negative

d)

it depends

46.

Beryllium and sulfur will form a ______ bond

a)

ionic

b)

covalent

c)

metalloid

47.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

48.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

49.

What is the correct name for the compound PCl3?

a)

phosphorus chloride

b)

chlorine phosphide

c)

trichloride phosphorus

d)

phosphorus trichloride

50.

What is the correct name for the compound SO3?

a)

Sulfate

b)

Sulfite

c)

Sulfur (II) Oxide

d)

sulfur trioxide

51.

What is the correct name for the compound N2O?

a)

nitrogen dioxide

b)

dinitrogen monoxide

c)

nitrogen oxide

d)

dinitrogen oxide

52.

What is the correct name for the compound P2O5?

a)

diphosphorus pentoxide

b)

diphosphorus oxide

c)

pentaphosphorus oxide

d)

phosphorus oxide

53.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
54.
What's the formula for chlorine dioxide
a)
ClO2
b)
CLO
c)
ClO3
d)
HClO2
55.

Name the following covalent compound.

NO

a)

Mononitrogen Oxide

b)

Nitrogen monoxide

c)

Nitrogen Oxide

56.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

57.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

58.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

59.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

60.

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

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

61.

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

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

62.

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

63.

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

64.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

65.

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

66.
What is the Law of Conservation of Mass?
a)
It states that no matter can be created or destroyed.
b)
It states that no energy can be created or destroyed.
c)
It states that matter can be created or destroyed.
d)
It states that no sound can be created or destroyed.
67.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number in front of a chemical formula.
c)
The number in between the chemical symbols.
d)
The number behind a chemical formula.
68.
What is the part of the chemical equation in green called? 
Fe + S --> FeS
a)
products
b)
reactants
c)
yield
d)
chemical formula
69.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
70.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
71.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
72.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
73.
Is the following equation balanced?
2C2H2 + 5O2 --> 4CO2 + 2H2O
a)
yes
b)
no
74.
What are the smaller numbers that you CANNOT change in a chemical equation? 
a)
Coefficient
b)
Products
c)
Reactants
d)
Subscript
75.
What are the larger numbers that you CAN CHANGE in a chemical equation? 
a)
Coefficient 
b)
Products
c)
Reactants
d)
Subscripts
76.

Balance the following equation:

___ SeCl6+ ___ O2→___ SeO2+____Cl2

a)

1, 1, 1, 3

b)

2, 1, 2, 1

c)

1, 2, 1, 2

d)

2, 2, 2, 4

77.

Balance the following equation:

___ Mg+ ___ O2→___ MgO

a)

1, 1, 3

b)

2, 1, 2

c)

1, 2, 1

d)

2, 2, 2

78.

Identify the type of chemical reaction (a)  

Choose from the below words
Synthesis
Decomposition
Single replacement
Double replacement
Combustion
79.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

80.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

81.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
82.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

83.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

84.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

85.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

86.

What is the general reaction scheme for a decomposition reaction?

a)

A + B --> AB

b)

AB --> A + B

c)

A + CD --> C + AD

d)

AB + CD --> CB + AD

e)

CxHy+O2 −> CO2+H2OC_xH_y+O_2\ ->\ CO_2+H_2O

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