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U2: Periodic Table and Bonding Summative Review

Total questions: 118

Worksheet time: 4hrs 42mins

Name
Class
Date
1.

Area within red box

a)

Group 2

b)

Period 2

c)

Group 3

d)

Period 3

2.

Gradual wearing away of a metal due to chemical reactions with something in the environment

a)

acidity

b)

corrosion

c)

luster

d)

malleability

3.

Metals tend to _____ electrons to form _____ ions

(a)  

4.

Nonmetals tend to _____ electrons to form _____ ions

(a)  

5.

The Russion scientist ________ is credited with making the first periodic table.

a)

Chekov

b)

Mendeleev

c)

Stalin

d)

Einstein

6.

Located between the metals and the nonmetals

a)

inner transition metals

b)

metalloids/semi-metals

c)

alkali metals

d)

alkaline earth metals

7.

Able to be drawn into wire

a)

malleable

b)

corrosive

c)

ductile

d)

metalloid

8.

Platinum is in group _____ period _____

(a)  

9.

Metals tend to have a _________ luster

a)

dull

b)

red

c)

shiny

d)

ceramic

10.

Property?

a)

ductility

b)

luster

c)

conductivity

d)

malleability

11.

A family of elements is the same as a ______

a)

period

b)

group

c)

transition metal

d)

atom

12.

If an atom GAINS electrons, it forms a _____ ion

a)

positive

b)

negative

c)

neutral

13.

If an atom LOSES electrons, it forms a _____ ion

a)

positive

b)

negative

c)

neutral

14.

Which of the following has ONE valence electron?

a)

sodium

b)

magnesium

c)

aluminum

d)

helium

15.

Which element is the NONMETAL in group 1?

a)

hydrogen

b)

helium

c)

sodium

d)

potassium

16.

Which of the following is an ALKALINE EARTH METAL?

a)

lithium

b)

calcium

c)

aluminum

d)

silicon

17.

Calcium is in period ____

a)

2

b)

3

c)

4

d)

5

18.

Which element DOES NOT have 7 valence electrons?

a)

fluorine

b)

chlorine

c)

bromine

d)

neon

19.

Noble gas

a)

chlorine

b)

argon

c)

hydrogen

d)

oxygen

20.

How many valence electrons?

a)

1

b)

2

c)

8

d)

12

21.

Charge?

a)

-2

b)

0

c)

+2

d)

+12

22.

Next closest star to Earth after our sun

a)

Beetlegeuse

b)

Proxima Centauri

c)

Sirius

d)

Alpha Centauri

23.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
24.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
25.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
26.
These are found on the Periodic Table.
a)
Compounds
b)
Elements
c)
Mixtures
27.
What Periodic Table family is represented by the Lewis dot diagram?
a)
Halogens
b)
Alkali Metals
c)
Transition Metals
d)
Noble Gases
28.
What group on the Periodic Table contains the elements of the alkaline earth family?
a)
1
b)
2
c)
17
d)
18
29.
Gold (Au)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Earth Metal
d)
Heavy Metal
30.
Which element is not in the Alkali metal family?
a)
Li
b)
H
c)
Fr
d)
Cs 
31.
Argon (Ar)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
32.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
33.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
34.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
35.

The is family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

36.

This type of element is dull, brittle solids and gases, insulators, poor conductors of heat and electricity, as well as having low melting points.

a)

metals

b)

metalloids

c)

nonmetals

37.

Sulfur is a...

a)

metal

b)

nonmetal

c)

metalloid

38.
Which is an alkaline earth metal?
a)
Calcium
b)
Rubidium
c)
Carbon
d)
Iodine
39.

Which of the following element is an example of Halogen

a)

Sodium

b)

Magnesium

c)

Fluorine

d)

Carbon

40.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
41.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
42.
an atom with atomic number 6 would have how many protons 
a)
6
b)
12
c)
3
d)
cannot be determined 
43.
What is the atomic number for an element with three protons?
a)
2
b)
1
c)
3
d)
6
44.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
45.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
46.

What is an isotope?

a)

A charged atom

b)

Two atoms of the same element with different amounts of neutrons

c)

Two atoms of the same element with different amounts of protons

d)

A neutral atom

47.

Which two components of an atom contribute to the mass?

a)

Protons and neutrons

b)

Protons and electrons

c)

neutrons and electrons

48.

Which part of an atom is used to identify it?

a)

number of protons

b)

number of neutrons

c)

number of electrons

49.
I which location on the Periodic Table are nonmetals found?
a)
Location 1
b)
Location 2
c)
Location 3
d)
Location 4
50.
Which element would have similar properties to Sulfur?
a)
Nitrogen
b)
Oxygen
c)
Flourine
d)
Chlorine
51.
What do elements in group 1 have in common?
a)
Number of valence electrons 
b)
Melting point of the element
c)
Possible number of bonds formed
d)
Metallic characteristics of the element
52.
Which pair of elements have the same number of valence electrons?
a)
Lithium and Beryllium
b)
Magnesium and Sodium
c)
Lithium and Sodium
d)
Magnesium and Lithium
53.
Based on this table it can be concluded that
a)
Sodium is the most reactive
b)
strontium is the best conductor
c)
phosphorous is the least stable
d)
aluminum has the most protons
54.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
55.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
56.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
57.
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
58.

What is the element with the highest electronegativity value?

a)

helium

b)

cesium

c)

fluorine

d)

calcium

59.

How many electrons can occupy any p sublevel?

a)

six

b)

two

c)

no more than eight

d)

ten

60.

How many electrons can occupy any d sublevel?

a)

six

b)

two

c)

no more than eight

d)

ten

61.

Which element listed below has the smallest atomic radius?

a)

He

b)

Ba

c)

Cu

d)

Si

62.

Which of the following atoms would have the largest radius?

a)

chlorine

b)

silicon

c)

sodium

d)

argon

63.

Copper is a common metal. Which of the following properties does this metal most likely have?

a)

High conductivity, high malleability, and low luster

b)

Low conductivity, low malleability, and low luster

c)

High conductivity, high malleability, and high luster

d)

Low conductivity, high malleability, and high luster

64.
Which element is least likely to conduct heat and electricity? 
a)
O
b)
Si
c)
Po
d)
Ca
65.
How would this element be classified?
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Metamorphic
66.
Which element is a metalloid?
a)
Titanium
b)
Selenium
c)
Potassium
d)
Polonium
67.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
68.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
69.

Bonds formed by transferring electrons from one atom to another are

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

70.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

71.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

72.

A compound forms between a metal and a nonmetal. It is

a)

ionic

b)

metallic

c)

covalent

73.

Ionic compounds are held together by

a)

intermolecular forces

b)

electrostatic forces

c)

magnetic forces

d)

nuclear forces

74.

A compound that is a poor conductor and has low melting and boiling points is most likely

a)

ionic

b)

metallic

c)

covalent

75.

Which compound is held together by electrostatic forces?

a)

NO2

b)

CaSO4

c)

Aluminum

d)

P4O10

76.

Which compound would have a very low melting point?

a)

sodium chloride

b)

copper (II) sulfate

c)

sulfur dioxide

d)

aluminum

77.

Typically, atoms are more stable when they are

a)

bonded together

b)

apart from each other

78.

Which bond does this picture best represent?

a)

Metallic bond

b)

ionic bond

c)

covalent bond

d)

James Bond

79.

What do positive ions tend to do?

a)

lose electrons

b)

gain electrons

c)

lose protons

d)

gain protons

80.

What do negative ions tend to do?

a)

lose electrons

b)

gain electrons

c)

lose protons

d)

gain protons

81.

What happens when magnesium loses 2 electrons?

a)

It stabilizes to a net charge of 0

b)

It turns into an atom

c)

It becomes negatively charged

d)

It becomes positively charged

82.

Predict the bond between Mg and Cl

a)

covalent

b)

ionic

c)

metallic

d)

none of the above

83.

What category of element usually forms a positive ion?

a)

Metals

b)

Nonmetals

c)

metalloids

d)

Noble gases

84.

Which category of elements usually form negative ions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

85.

CaCl2 is an example of what type of bond?

a)

Covalent

b)

Metallic

c)

Ionic

86.

What is the first step to take when starting to draw a Lewis Dot Structure?

a)

Count the valence electrons for only one atom.

b)

Place dots around outside atoms.

c)

Count all the valence electrons in the molecule.

d)

Connect outside atoms to central atom through single bond.

87.

When writing a Lewis Dot Structure I notice that I have completed all the octets for every atom in the molecule, but still have remaining electrons. What should I do?

a)

Place additional electrons around the outside atoms.

b)

Place the additional electrons around the central atom.

c)

Form a double or triple bond

d)

Ignore the additional electrons left over.

88.

When drawing a Lewis Dot Structure I find that my central atom is not at a completed octet, but I am out of electrons. The central atom is in Group 13, what do I do?

a)

Leave the structure alone

b)

Place additional dots around the central atom

c)

Form a double or single bond

d)

Give up

89.

When drawing a Lewis Dot Structure, I notice that my central atom is not completed to a full octet, but I am out of electrons. My central atom is not Be or in Group 13, what do I do?

a)

Leave it alone

b)

Place additional dots around the central atom

c)

Form a double or triple bond

d)

Add additional atoms to the molecule

90.

What is the maximum number of electrons hydrogen can hold?

a)

1

b)

2

c)

4

d)

8

91.

When the central atom has more than 4 total electron pair bonded to it, its called?

a)

electron deficient

b)

expanded octet

c)

deficient octet

d)

This can't happen

92.

Oxygen (O) atoms will combine with Hydrogen atoms to form water molecules (H2O). Which statement explains the process through which these molecules are formed?

a)

two oxygen atoms share some of their protons with Hydrogen atoms

b)

2 hydrogen atoms share their valence electrons with one oxygen atom

c)

protons are transferred from one oxygen atom to the other oxygen atom

d)

electrons are transferred from one hydrogen atom to the other oxygen atom

93.

When an atom of sodium and an atom of fluorine combine to form a salt compound, sodium fluoride is formed through an ionic bond. Which statement correctly describes the behavior of the valence electron in the ionic bond?

a)

an electron from the fluorine atom moves to the sodium atom forming 2 ions

b)

an electron from the sodium atom moves to the fluorine atom forming 2 ions

c)

an electron from the fluorine atom is shared with the sodium atom forming a sodium ion

d)

an electron from the fluorine atom is shared with the sodium atom forming a fluorine ion

94.

Aluminum oxide, Al2O3, is produced by combining Al3+ and O2- particles.  What type of compound has been formed?

a)

ionic

b)

metallic

c)

covalent

d)

molecular

95.

An ionic bond typically forms between certain types of elements.  Which pair of elements will form an ionic compound?

a)

N and O

b)

K and Cl

c)

Na and Cu

d)

Li and Mg

96.

 Iron oxides, such as rust, form when iron metal reacts with oxygen in the air. What are the chemical symbols for the two elements found in iron oxide?

a)

I and O

b)

Ir and O

c)

Fe and O

d)

Pb and O

97.

Which part of a sodium atom is transferred when an ionic bond is formed with another atom?

a)

proton

b)

neutron

c)

electron

d)

outer electron

98.

How many elements are in the compound shown in the image?

a)

2

b)

3

c)

4

d)

5

99.

How many atoms are in the compound shown in the image?

a)

2

b)

3

c)

4

d)

5

100.

The compound name formed from the elements calcium and chlorine is known as

a)

calcite

b)

chlorine calcide

c)

calcium chlorate

d)

calcium chloride

101.

The chemical structure for carbon dioxide is CO2.  Carbon dioxide is most likely a/an

a)

element

b)

diatomic gas

c)

ionic compound

d)

covalent compound

102.

Oxygen gas is essential to most living things. Its chemical formula is O2. What is oxygen and what type of bond holds the 2 oxygen atoms together? Select two choices.

a)

ion

b)

element

c)

compound

d)

covalent bond

e)

mixture

103.

Ions (formed when ionic bonds are made) tend to form by _______. (Select two answers)

a)

Gaining electrons to become stable and fill their outer energy level

b)

Losing electrons to become stable and dropping to the full energy level below

c)

Gaining electrons to match the electron patterns of other atoms

d)

Losing electrons to match the electron patterns of other alkali metals

e)

Gaining electrons to match the electron patterns of halogens

104.

Select two answers that are correct about the compound show in the particle diagram shown:

a)

When fluorine and carbon combine, they form an ionic bond.

b)

When fluorine and carbon combine, they form a covalent bond.

c)

The name for the compound is carbon fluoride

d)

The name for the compound is monocarbon tetrafluoride.

e)

The name for the compound is carbon tetrafluoride.

105.

Read the following passage to answer the question below. 


Element Z is a soft powdery solid with poor conductivity. It bonds with fluorine to form a product with the formula ZF6 which is a colorless, odorless gas. The Lewis Dot structure for Element Z is shown to the right.

a)

Element Z must be oxygen because the product is a gas and it matches the Lewis Dot structure.

b)

Element Z must be sulfur because of the description of the element and it matches the Lewis Dot structure.

c)

Element Z must be sodium because it is a metal that can bond with fluorine.

d)

Element Z must be chlorine because it is also halogen and has the same number of electrons as fluorine.

106.

Analyze the periodic table below showing unknown elements. Select the elements that would combine to make a binary ionic compound?

a)

Element B would combine with Element A

b)

Element B would combine with Element E

c)

Element C would combine with Element D

d)

Element G would combine with Element A

107.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
108.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

109.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
110.
Write the correct formula for an ionic compound formed from S2- and Rb1+.
a)
SRb2
b)
SRb
c)
Rb2S
d)
RbS2
111.

What will be the charge of a bromine ion?

a)

+7

b)

-7

c)

-1

d)

+1

112.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
113.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
114.
Which of the following is an example of an IONIC COMPOUND?
a)
NaCl
b)
H2O
c)
CO2
d)
NO
115.
a)

A

b)

B

c)

C

d)

D

116.
a)

A

b)

B

c)

C

d)

D

117.
a)

A

b)

B

c)

C

d)

D

118.

Which compound is formed by ionic bonding?

a)

CF4

b)

CuBr2

c)

N2O4

d)

P4O10

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