Free Printable Chemical bonding review

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Worksheets

Chemical bonding review

Total questions: 46

Worksheet time: 31mins

Name

Class

Date

1.

According to the octet rule most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

2.

If electrons are shared unequally then the bond is....

a)

Non-polar covalent

b)

Ionic

c)

Non-polar ionic

d)

Polar covalent

3.

If electrons are shared equally then the bond is....

a)

Non-polar covalent

b)

Ionic

c)

Non-polar ionic

d)

Polar covalent

4.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

5.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

6.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

7.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

8.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

9.

Why is the molecule polar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

10.

Why is the molecule nonpolar?

a)

There are nonbonding pairs on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no nonbonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

11.

The cohesive forces between liquid molecules are responsible for this phenomenon.

Example: insects walking in water.

a)

Surface Tension

b)

Viscosity

c)

Capillarity

d)

Fluidity

12.

It is the ability of liquids to resist flowing. These kinds of liquids are thick.

Example: glue, condensed milk.

a)

Fluidity

b)

Viscosity

c)

Surface Tension

d)

Capillarity

13.

Identify the IMF exist in CH₄

a)

dipole-dipole forces

b)

london forces

c)

ion-dipole forces

d)

hydrogen bonding

14.

Identify the IMF exist in NH₃

a)

london dispersion forces

b)

ion-dipole forces

c)

dipole-dipole forces

d)

hydrogen bonding

15.

Identify the IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

16.

Which of the following has the lowest boiling point?

a)

PH₃

b)

H₂O

c)

SiH₄

d)

NH₃

17.

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.

18.

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

a)

chlorine, fluorine, and oxygen

b)

fluorine, oxygen, and sulfur

c)

fluorine, bromine, and oxygen

d)

fluorine, oxygen, and nitrogen

19.

What will be the state of the following molecule?

a)

gas

b)

liquid

c)

solid

20.

Type of intermolecular force present in I₂, Br₂, and Cl₂.

a)

dipole dipole

b)

H-bond

c)

dispersion

d)

metallic

21.

Which of the following will take the longest to evaporate?

a)

CH₃CH₂OH

b)

CH₃OH

c)

CH₃CH₃

22.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

23.

Which statement explains why Br₂is a liquid at STP and I₂ is a solid at STP?

a)

Molecules of Br₂ are polar, and molecules of I₂are nonpolar

b)

Molecules of Br₂ are nonpolar, and molecules of I₂ are polar

c)

Molecules of Br₂ have stronger intermolecular forces than molecules of I₂.

d)

Molecules of I₂ have stronger intermolecular forces than molecules of Br₂.

24.

Table salt (NaCl) can be dissolved in water due to what inter-molecular force of attraction?

a)

Ion-dipole

b)

dipole-dipole

c)

hydrogen bonding

d)

metallic bonding

25.

Higher IMF means (a) Viscosity.

26.

It is the measure of the tendency of material to change into the gaseous state.

a)

Boiling point

b)

vapor pressure

c)

specific heat

d)

viscosity

27.

It is the attractive forces that exist between molecules.

a)

Intramolecular force

b)

Metallic bond

c)

Intermolecular force

d)

Covalent bond

28.

A weak IMF will result in a

a)

high melting point

b)

high viscosity

c)

high surface tension

d)

low surface tension

29.

What is the electron geometry and molecular geometry of SO2?

a)

trigonal planar, bent

b)

tetrahedral, trigonal pyramidal

30.

Which container has the greatest Intermolecular Force between Molecules?

a)

red

b)

yellow

c)

blue

31.

In which situation does DISPERSION FORCES are strongest?

a)

If two molecules are of comparable size and shape, dispersion forces will likely determine its physical properties.

b)

If one molecule is much larger than another, dispersion forces will likely determine its physical properties.

c)

If negative ends of polar molecules are oriented to positively charged cations, dispersion forces will likely determine its physical properties.

d)

If positive ends of polar molecules are oriented to negatively charged anions, dispersion forces will likely determine its physical properties.

32.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

33.

Oil molecules are nonpolar. What kind of solvent is required to remove an oil stain?

a)

saturated

b)

unsaturated

c)

polar

d)

nonpolar

34.

When salt is dissolved in water, the water molecules pull apart the salt. The chlorine ions of salt are surrounded by water molecules. Why do the hydrogen sides of water molecules point at the chlorine ions?

a)

Water is polar and so are chlorine ions

b)

The hydrogen and chlorine have positive charges, so they attract.

c)

The hydrogen has a partial positive charge and the chlorine has a negative charge.

d)

Water is polar and chlorine ions are nonpolar

e)

The hydrogen has a partial negative charge and the chlorine has a positive charge.

35.

What is the ELECTRONIC geometry of the following?

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Trigonal Bipyramidal

36.

Which molecule would have this molecular geometry?

a)

BF₃

b)

CH₄

c)

PCl₅

d)

CO₂

37.

What molecule could this be?

a)

H₂O

b)

CCl₄

c)

PCl₅

d)

NaCl

38.

Who could this be?

a)

CO₂

b)

NH₃

c)

H₂S

d)

CH₄

39.

Who could this molecule be?

a)

CH₄

b)

CO₂

c)

PCl₅

d)

BF₃

40.

Who could this be?

a)

H₂O

b)

NH₃

c)

CO₂

d)

CH₄

41.

What is the molecular shape of a silicon dioxide molecule?

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

42.

What molecular geometry would PH₃have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

43.

What is the molecular geometry and bond angel for H₂O?

a)

tetrahedral, 109.5^o

b)

trigonal planar, 120^o

c)

bent, < 109.5^o

d)

trigonal pyramidal, < 109.5^o

44.

What is the molecular geometry for PCl₅

a)

tetrahedral

b)

octahedral

c)

trigonal bipyramidal

d)

T-Shape

45.

Choose the correct shape for this molecule:

a)

linear

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

46.

How is electron geometry different from molecular geometry?

a)

Electron geometry only takes electron domains into account while molecular places large emphasis on lone pairs

b)

Molecular geometry only takes electron domains into account while electron geometry places large emphasis on lone pairs

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