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Unit 2 Learning Checkpoint 1 Review

Total questions: 44

Worksheet time: 1hrs 9mins

Name
Class
Date
1.

What is a characteristic of a gas?

a)

Fixed shape and volume

b)

Particles are close together

c)

Particles are compressible

d)

Particles vibrate in place

2.

What is the primary difference between atoms and molecules?

a)

Atoms are larger than molecules.

b)

Atoms are single units, while molecules are combinations of atoms.

c)

Molecules are single units, while atoms are combinations of molecules.

d)

Atoms and molecules are the same.

3.

What is the main difference between elements and compounds?

a)

Elements are mixtures

b)

Compounds are made of one type of atom

c)

Elements cannot be broken down by ordinary means

d)

Compounds are always solid

4.

What are the two types of mixtures?

a)

Solid and liquid

b)

Chemical and physical

c)

Heterogeneous and homogeneous

d)

Simple and complex

5.

Which of the following is NOT a characteristic of mixtures?

a)

Can be separated by physical means

b)

Identities of substances are retained

c)

Always have a uniform composition

d)

Are physical combinations

6.

What type of bond is primarily responsible for holding the atoms together within a molecule?

a)

Intermolecular attraction

b)

Intramolecular attraction

c)

Ionic bond

d)

Hydrogen bond

7.

Which of these samples shown best represents an element?

a)

A

b)

B

c)

C

d)

D

8.

In the diagrams provided, the circles of different colors represent the atoms of different elements. Which diagram represents a mixture?

a)

I

b)

II

c)

III

d)

IV

9.

Which of the following represents a compound?

a)

Diagram (a)

b)

Diagram (b)

c)

Diagram (c)

d)

All of the diagrams represent the parts of a compound.

10.

Which diagram represents an element?

a)

Diagram (a)

b)

Diagram (b)

c)

Diagram (c)

d)

None of the diagrams represent the parts of an element.

11.

What type of matter is shown in this particle diagram?

a)

Element

b)

Compound

c)

Mixture of Elements

d)

Mixture of Compounds

e)

Mixture of Elements and Compounds

12.

What type of matter is shown in this particle diagram?

a)

Element

b)

Compound

c)

Mixture of Elements

d)

Mixture of Compounds

e)

Mixture of Elements and Compounds

13.

What type of matter is shown in this particle diagram?

a)

Element

b)

Compound

c)

Mixture of Elements

d)

Mixture of Compounds

e)

Mixture of Elements and Compounds

14.

What type of matter is shown in this particle diagram?

a)

Element

b)

Compound

c)

Mixture of Elements

d)

Mixture of Compounds

e)

Mixture of Elements and Compounds

15.
What type of mixture is this?
a)
homogenous mixture
b)
chemical
c)
heterogeneous mixture 
d)
solid mix
16.

What type of mixture does this diagram represent?

a)

Homogeneous, because there are layers.

b)

Heterogeneous, because there are layers.

c)

Homogenous, because the contents are mixed evenly.

d)

Heterogenous, because the contents are mixed evenly.

17.

What does this image of a gas chromatography chart show?

a)

The sample contains more carbon dioxide than methane.

b)

The sample contains more nitrogen than methane.

c)

The peaks represent different elements.

d)

The Hydrogen sample interacted the most with the substance in the column.

18.

Which two statements about the chromatogram is true?

a)

Chromatography separate compounds

b)

The highest peak has the greatest concentration.

c)

The samllest peak has the greatest concentration.

d)

Chromotography separates mixtures

19.
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.
20.

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

a)

higher

b)

lower

21.

Water and ammonia molecules are roughly the same size and the same mass but ammonia boils at -28°F and water boils at 212°F. What can we conclude about the intermolecular forces between water and ammonia?

a)

Water has stronger intermolecular forces

b)

Ammonia has stronger intermolecular forces

c)

The intermolecular forces are the same strength

d)

Not enough information is given

22.

The melting points and boiling points of substances can lead to inferences about the intermolecular attraction of the atoms of these substances because higher melting and boiling points indicate that

a)

the atomic mass of the substances is smaller.

b)

the substances produce exothermic reactions.

c)

atomic radii increases heat is added.

d)

more energy is needed to separate molecules.

23.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
24.

Intramolecular forces are the forces

a)

within molecules

b)

between molecules

25.

What kind of force is the arrow pointing to?

a)

Intramolecular Force

b)

Intermolecular Force

26.

What kind of force is the arrow pointing to?

a)

Intramolecular force

b)

Intermolecular force

27.

Which factor influences the strength of London dispersion forces?

a)

Molecular size

b)

Molecular bonds

c)

Molecular polarity

28.

What is the relationship between molecule size and force?

a)

Smaller molecule

1.

weak forces

b)

Bigger molecule

2.

strong forces

c)

Medium-sized molecule

3.

moderate forces

29.

Rank the following substances with their boiling points in order of strongest forces from strongest to weakest.

a)

H2O - 100oC

b)

C7H16- 98.4oC

c)

C3H8 - 56oC

d)

CH4 - 40.2oC

1)
2)
3)
4)
30.

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

a)

higher

b)

lower

31.
What type of forces will the following molecule have?
a)
dispersion forces
b)
dipoles
c)
hydrogen bonding
32.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

33.

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

34.

Which is the stronger intermolecular force present in NH3?

a)

London dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

35.

Which sample has hydrogen bonding?

a)

H2S

b)

CH4

c)

NH3

d)

HI

36.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

37.

Which one has the highest boiling point?

a)

BeCl2

b)

CO2

c)

SF4

d)

NH4

38.

Which of the following will have the highest melting point.

a)

naphthalene, C8H10

b)

SiO2

c)

methane CH4

d)

 C2H5OH

39.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
40.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
41.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
42.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
43.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
44.

Which of the following atoms would have the largest radius?

a)

chlorine

b)

silicon

c)

sodium

d)

argon

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