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Worksheets

jana

Total questions: 110

Worksheet time: 3hrs 43mins

Name
Class
Date
1.

Ionic bonds form between ---

a)

nonmetals.

b)

metals and nonmetals.

2.

Covalent bonds form between ---

a)

nonmetals.

b)

metals and metals

c)

metals and nonmetals

3.

What are valence electrons?

a)

sum of the protons and neutrons

b)

protons minus electrons

c)

electrons in the inner shells

d)

electrons in the outer shell

4.

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

a)

-1.

b)

-2.

c)

+1.

d)

+2.

5.

If an atom has 7 protons and 7 electrons, its electric charge is ---

a)

-7

b)

-14

c)

0

d)

+7

6.

Atoms form compounds to become more ---

a)

reactive

b)

stable

c)

explosive

d)

toxic

7.

A _______ is the force that holds atoms together in a compound.

a)

Chemical Formula

b)

Chemical Reaction

c)

Chemical Bond

d)

Synthesis Reaction

8.

Why do chemical bonds form?

a)

so the number of protons equals the number of electrons

b)

to fill the outermost electron level

c)

so an atom can become unstable

9.

An electron has a ___ charge.

a)

no charge

b)

positive

c)

negative

d)

it depends

10.

A proton has a ___ charge.

a)

positive

b)

negative

c)

no charge

d)

it depends

11.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

8

d)

10

12.

It is a chemical bond arises between the atoms of non-metals by sharing of each atom with electrons

a)

ionic bond

b)

Covalent bond

c)

Electric bond

d)

Magnetic bond

13.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

14.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
15.

Which of these is not a real bond in chemistry?

a)

James

b)

Ionic

c)

Covalent

d)

Metallic

16.
Ionic bonds are between...
a)
nonmetals and nonmetals
b)
carbon and oxygen
c)
metals and nonmentals
d)
hydrogen and chlorine
17.
Covalent bonds are between...
a)
two or more nonmetals
b)
sodium and chlorine
c)
metals and metals
d)
metals and nonmetals
18.
What is the name for an ion with a positive charge?
a)
cation
b)
anion
c)
onion
d)
union
19.
What is the name for an ion with a negative charge?
a)
cation
b)
anion
c)
onion
d)
union
20.
What kind of bond forms when atoms exchange electrons?
a)
ionic
b)
covalent
c)
artificial
d)
univalent
21.
If an atom loses two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
22.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
23.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

24.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

25.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
26.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
27.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
28.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
29.

Chemical bond is ...

a)

the physical mixing of two different atoms.

b)

the force that holds two atoms together

c)

the energy used up when two atoms combined.

d)

the temperature that changes the phase of matter.

30.

Which of the following atoms is most likely to bond with another atom?

a)
b)
c)
d)
31.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

32.

Which statement best describes the relationship between atoms & molecules.

a)

molecules are made of atoms that are chemically bonded together.

b)

atoms are made of molecules that are chemically bonded together.

c)

molecules are made of a mixture of atoms and compounds.

d)

atoms are made of protons, neutrons & electrons.

33.

symbol of sodium

a)

k

b)

Fe

c)

Na

d)

Ag

34.
A copper penny turning greenish after a few years is an example of ...
a)
Chemical Change
b)
Physical Change
35.
An explosion occurs ...
a)
Chemical Change
b)
Physical Change
36.
Is digesting your food a physical or chemical change?
a)
Physical
b)
Chemical
37.
Is a car using fuel a physical or chemical change?
a)
Physical
b)
Chemical
38.
The diagram below shows changes happening to water in a specially shaped bottle.
What changes did the water undergo?
a)
melting and then freezing
b)
freezing and then evaporation
c)
condensation and then melting
d)
evaporation and then condensation
39.

Identify what type of change happening in the picture below...

a)

Chemical Reaction

b)

Physical Change

c)

Change in State

d)

Change in appearance only

40.

Which of the following is a molecule?

a)

copper

b)

ferrum

c)

oxygen we inhale

d)

none of these

41.

The atomicity of water is

(a)  

42.

Which of the following is correct representation of carbon monoxide?

a)

Co

b)

cO

c)

none of these

d)

CO

43.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

44.

Which element has a lower electronegativity value?

a)

Calcium

b)

Barium

45.

Electronegativity (a)   as you go down a group.

46.

Electronegativity trends are the same as:

a)

Atomic radius trends

b)

Ionization energy trends

c)

Both of these

d)

None of these

47.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

48.

As you move across a period, the outer electrons are ________ to the nucleus, so the nucleus of the atom is ________ to attract electrons in a bond.

a)

closer, more able

b)

closer, less able

c)

further, less able

d)

further, more able

49.

Do noble gases have electronegativity values?

a)

yes

b)

no

50.

Why does electronegativity decrease as you go down a group?

a)

As you go down a group, the outer electrons are further away from the nucleus

b)

As you go down a group, the nucleus is less able to attract electrons in a bond

c)

Both of these

d)

None of these

51.

Which is the correct order of electronegativity from lowest to highest?

a)

Zinc, Nickel, Iron, Scandium

b)

Iron, Nickel, Zinc, Scandium

c)

Scandium, Iron, Nickel, Zinc

d)

Scandium, Iron, Zinc, Nickel

52.

Electronegativity is the ability of an atom to attract electrons in a physical bond.

a)

false

b)

true

53.

Sodium and Bromine will make a _____ bond

a)

Ionic

b)

Hydrogen

c)

Covalent

d)

Exploding

54.

The mutual sharing of one or more pairs of electrons between two atoms.

a)

Covalent

b)

Ionic

55.

 

This type of bonding can be described as "I give, I get"

a)

Covalent

b)

my mom

c)

Ionic

d)

Friendship

56.

Why do all bonds form?

a)

filling the outermost energy level

b)

to win

c)

to make other atoms unstable

d)

to be famous

57.

What two types of atoms make a covalent bond?

a)

2 Metal

b)

2 Ionic

c)

1 nonmetal 1 metal

d)

2 Nonmetal

58.

 

NaCl

a)

metallic

b)

covalent

c)

Ionic

59.

Hydrogen and Chlorine will from a ____ bond

a)

Unique

b)

bestie

c)

Covalent

d)

Ionic

60.

Beryllium and sulfur will form a ____ bond

a)

Covalent

b)

Metallic

c)

Ionic

d)

Unique

61.

In ionic bonds, metals tend to?

a)

Keep their electrons

b)

Gain valence electrons

c)

Lose valence electrons

d)

None of these answers are correct

62.

MgO for a _____ Bond.

a)

Ionic

b)

Metallic

c)

Covalent

63.

What type of bond involves the sharing of electrons between atoms?

a)

Covalent

b)

Ionic

c)

Best friend bonds

64.

Why don't noble gases form bonds?

a)

They all have a full octet

b)

Noble gases do form bonds

c)

They only bond when with eachother

d)

none of these answers are correct

65.

 

This type of bonding can be described as a "cooperation"

a)

Diverse

b)

Ionic

c)

Covalent

66.

Water, H2O

a)

Ionic

b)

Covalent

c)

Water

67.

When metals bond with non-metals they form what type of bonds

a)

Ionic

b)

Covalent

68.

An ionic compound forms between a ______

a)

2 nonmetals

b)

metal and nonmetal

c)

2 metals

d)

noble gasses

69.

Type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound.

a)

Ionic

b)

Covalent

70.

CH4 (Methane) is an example of a(n) ______ bond.

a)

metallic

b)

covalent

c)

Ionic

71.
Elements are made of 
a)
many types of atoms 
b)
the periodic table
c)
one type of atom 
d)
molecules 
72.
All matter is made of 
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
73.
Two or more atoms chemically bonded together are called a
a)
atom
b)
element
c)
molecule
d)
mixture
74.

Which subatomic particles are much smaller than the others and have a negative charge?

a)

protons

b)

neutrons

c)

electrons

75.
How many Protons are in one atom of Lithium?
a)
3
b)
6
c)
7
d)
6.941
76.

H₂O is a compound molecule.

a)

TRUE

b)

FALSE

77.

O2 is a compound molecule.

a)

TRUE

b)

FALSE

78.

Group of atoms bonded together

a)

Mixture

b)

Compouns

c)

Atom

d)

Molecules

79.

What is Covalent Bonding?

a)

Bonding that is the result of two nonmetals sharing electrons

b)

Bonding between two metals

c)

Bonding that is the result of a nonmetal and a metal exchanging electrons

d)

Bonding between more than two elements

80.

Which particle is responsible for bonding?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Nucleus

81.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

82.

Potassium Chloride is...

a)

Ionic

b)

Covalent

83.

Water (H2O) is...

a)

Ionic

b)

Covalent

84.

Ammonium (NH4) is...

a)

Ionic

b)

Covalent

85.
Share electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
86.
Gain or lose electrons
a)
Ionic Bonds
b)
Covalent Bonds
c)
Both bonds
d)
Neither bond
87.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
88.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
89.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
90.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
91.
In the correct Lewis structure for CH4, how many unshared electron pairs surround the carbon?
a)
2
b)
8
c)
0
d)
4
92.
In CO2, how many UNSHARED pairs of electrons does each oxygen have?
a)
2
b)
1
c)
4
d)
6
93.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
94.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
95.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
96.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
97.
This is a correct dot diagram for nitrogen (N)
a)
true
b)
false
98.
An atom that loses electrons in an ionic bond becomes a ________ charged ion.
a)
Negatively
b)
Positively
99.
An atom that loses electrons in an ionic bond becomes a ________ charged ion.
a)
Negatively
b)
Positively
100.
Ba +3 and  Cl-
a)
Ba3Cl
b)
Ba3Cl3
c)
BaCl3
d)
BaCl
101.
Fe +3  and  S -2
a)
Fe3S2
b)
FeS
c)
S3Fe2
d)
Fe2S3
102.
Ag +  and  Br -
a)
AgBr
b)
BrAg
c)
Ag2Br2
d)
Br2Ag2
103.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
104.
Li+ and P3- create...
a)
Li3P
b)
LiP3
c)
LiP
d)
Li2P
105.
What is the NAME of....
Na2S
a)
sodium (II) sulfide
b)
sodium sulfide
c)
disodium sulfide
d)
sodium sulfur
106.

Name this compound: KF

a)

Potassium fluoride

b)

Potassium fluorite

c)

Fluorine potasside

d)

Potassium fluorate

107.

Write the formula for barium + nitrogen

a)

Ba2N3

b)

Ba3N2

c)

BaN

d)

BaN3

108.
When naming ionic compounds, the cation is always named first and the anion is always named second.
a)
False
b)
True
109.

Which of the following is an ionic compound:

a)

CH4

b)

I2

c)

LiBr2

d)

CO

110.
What is the FORMULA for...
calcium arsenide
a)
Ca3As2
b)
CaAs2
c)
Ca3As
d)
Ca3Ar2

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