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Bonding Test Review Quizzizz

Total questions: 62

Worksheet time: 1hrs 5mins

Name
Class
Date
1.

______ molecules are found in nature as pairs of two atoms of the same type covalently bonded together.

a)

Diatomic

b)

Monatomic

c)

Polyatomic

d)

Network

2.

Which of the following types of elements can exist in monatomic form?

a)

alkali metals

b)

transition metals

c)

halogens

d)

noble gases

3.
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
4.
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
5.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
6.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
7.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

8.
A _________________ is composed of symbols and subscripts indicating the number of atoms of an element in a compound.
a)
Chemical Equation
b)
Chemical Reaction
c)
Synthesis Reaction
d)
Chemical Notation
9.

How many electrons do most elements want to have in their outer shell to be stable?

(a)  

10.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

11.
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.
12.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

13.

Examine the image: How many bonds are formed looking at the model of the compound? And also indetify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

14.

August 2015 #39: What is the number of pairs of electrons shared in a molecule of N2?

a)

1

b)

2

c)

3

d)

6

15.

June 2004 #13: Compared to the physical and chemical properties of the compound NO2, the compound N2O has

a)

Different physical properties and different chemical properties

b)

Different physical properties and the same chemical properties

c)

The same physical properties and different chemical properties

d)

The same physical properties and the same chemical properties

16.

August 2016 #8: Which formula represents a polar molecule?

a)

O2

b)

CO2

c)

NH3

d)

CH4

17.

June 2017 #12: Which substance has nonpolar covalent bonds?

a)

Cl2

b)

SO3

c)

SiO2

d)

CCl4

18.

If an atom loses 2 electrons what charge will it have?

a)

+2

b)

-2

c)

+1

d)

-1

19.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
20.

In a compound of MgCl2, the subscript 2 indicates that

a)

there are 2 magnesium ions for each ion of chlorine.

b)

the chloride ion is twice the size of the magnesium ion.

c)

there are 2 chloride ions for each magnesium ion.

d)

chlorine has a charge of 2.

21.

Which of the following is a typical property of an ionic compound?

a)

low melting point

b)

poor conductor of electric current when melted

c)

tendency to shatter when struck

d)

all choices are properties of ionic compounds

22.

In the name carbon dioxide, the prefix of the second word indicates that a molecule of carbon dioxide contains

a)

two carbon atoms.

b)

two oxygen atoms.

c)

a polyatomic ion.

d)

an ionic bond.

23.

What is the basis of a metallic bond?

a)

the attraction between neutral metal atoms

b)

the neutralization of protons by electrons

c)

the attraction of oppositely charged ions

d)

the attraction of metal ions to mobile electrons

24.

The particles responsible for chemical bonding are

a)

protons.

b)

cations.

c)

electrons.

d)

valence electrons.

25.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

26.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
27.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
28.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
29.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

30.

What is the name of the three-dimensional pattern that forms when ions bond?

a)

a crystal lattice

b)

a chemical compound

c)

an ionic bond

d)

a crystal lettuce

31.

The melting points of covalent molecules are:

a)

very high

b)

high

c)

medium

d)

low

32.

Giant structures with high melting and boiling points but only conduct electricity when molten or dissolved in a solution.

a)

Covalent

b)

Metallic

c)

Ionic

33.
Limestone is a naturally occuring form of calcium carbonate. The correct formula for calcium carbonate is:
a)
CaCO3
b)
Ca2(CO3)2
c)
Ca3CO
d)
Ca2CO2
34.
Provide the IUPAC name for NH4NO3.
a)
ammonium nitrogen trioxide
b)
nitrogen hydride nitrate
c)
ammonium nitrate
d)
ammonium (IV) nitrate
35.
Which of the following statements explains why the bond between hydrogen chloride is polar covalent?
a)
Chlorine has a greater atomic mass than hydrogen
b)
Chlorine has a greater electronegativity than hydrogen
c)
Chlorine has a higher ionization energy than hydrogen
d)
Chlorine has a greater number of valence electrons than hydrogen
36.
Which statement best compares the properties of ionic and metallic substances?
a)
The bonds of metallic substances are composed of delocalized electrons, the bonds of ionic compounds are composed of transferred electrons
b)
The bonds of metallic substances are composed of isolated electrons, the bonds of ionic substances are composed of shared electrons
c)
Metallic and ionic substances both have high melting points due to crystalline structure
d)
Metallic substances insulate heat and electricity, ionic compounds conduct heat and electricity
37.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
38.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
39.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
40.

According to the diagram below, how many bonds will this atom be able to make?

a)
1
b)
2
c)
3
d)
4
41.

Which shows the right valence electrons?

a)

A

b)

B

c)

C

d)

D

42.

Calculating the difference in electronegativity can always help determine_________?

a)

the # of valence electrons

b)

the polarity of a molecule

c)

the type of bond

d)

the geometry of a molecule

43.

Which of the following ordered pairs of elements has the highest difference in electronegativity?

a)

Li and Be

b)

Li and F

c)

O and F

d)

F and F

44.

The electrons in a POLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

45.

What is the difference in electronegativity for HBr?

a)

0.7

b)

1.9

c)

2.0

d)

2.8

46.

HBr has a difference in electronegativity of 0.7. Based on the table, what kind of bond is HF?

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

47.

 H2OH_2O  has a difference in electronegativity of 1.4. Based on the table, what kind of bond is 

 H2OH_2O ? 

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

48.

Which of the following diatomic molecules can be formed with a double covalent bond?

a)

N2

b)

O2

c)

F2

d)

C2

49.

If the difference in electronegativity between two bonding atoms is less than 1.7 but greater than .03 the bond is

a)

ionic

b)

polar covalent

c)

metallic

d)

nonpolar covalent

50.

The shape is?

a)

linear

b)

planar

c)

pyramidal

d)

tetrahedron

51.

The shape is?

a)

tetrahedron

b)

planar

c)

pyramidal

d)

linear

52.

The shape is?

a)

bent

b)

linear

c)

pyramidal

d)

planar

53.
What is the name of this shape?
a)
Linear
b)
Trigonal Planar
c)
Tetrahedral
d)
Trigonal Bipyramidal
54.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
55.
Define the term allotropes
a)
Atoms with same proton number but different number of neutrons
b)
Atoms with same proton number but different mass number
c)
Atoms in different arrangement in structure
d)
Atoms in different arrangement and different physical form
56.
Gp 4, Diamond (C) and Silicon (S) has highest melting point due to
a)
Strong covalent bonds between carbon atoms
b)
All carbon atoms are covalently bonded
c)
Strong covalent bonds in a macromolecular structure
d)
Carbon atom covalently bonded in a macromolecular structure
57.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
58.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

59.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
60.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

61.

Examples of an intermolecular force include

a)

london disperson

b)

hydrogen bonding

c)

dipole dipole

d)

all of the above

62.

For hydrogen bonding to occur, a molecule must have a hydrogen bonded to

a)

carbon

b)

another hydrogen

c)

Fluorine, Chlorine or Oxygen

d)

Fluorine, Nitrogen or Oxygen

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