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What is Matter--REVIEW

Total questions: 74

Worksheet time: 52mins

Name
Class
Date
1.

Vaporization is the change from

a)

Liquid to Gas

b)

Solid to Liquid

c)

Gas to Solid

d)

Solid to Gas

2.

Change from Solid to Gas

a)

Condensation

b)

Melting

c)

Sublimation

d)

Boiling

3.

The fact that water floats in the solid state is know as

a)

Solid

b)

Freezing

c)

Boating

d)

Density Anomaly

4.

Change from gas to solid

a)

Sublimation

b)

Deposition

c)

Boiling

d)

Melting

5.

A substance with a HIGH specific heat capacity:

a)

Take a long time to heat up and cool down

b)

Never freezes

c)

Takes a short time to heat up and cool down

d)

Is always a solid

6.

What changes for a phase to go through a phase change?

a)

Temperature

b)

Altitude

c)

Location

d)

Energy

7.

Anything that takes up space and has mass

a)

Matter

b)

Energy

c)

Gravity

d)

Force

8.

Three basic states of matter

a)

Energy, Solids, Gases

b)

Solids, Gases, Plasma

c)

Solids, Gases, Liquids

d)

Solids, Liquids, Plasma

9.

Heterogeneous Mixture

a)

Particles are distributed non-uniformly (Chocolate chip cookie)

b)

Particles are distributed uniformly (Milk, coffee)

10.

Homogeneous Mixture

a)

Particles are distributed non-uniformly (Chocolate chip cookie)

b)

Particles are distributed uniformly (Milk, Coffee)

11.

Substance that is dissolved in solution.

a)

Solute

b)

Solvent

c)

Solution

d)

Substance

12.

Chemical substance that dissolves another chemical substance to form a solution.

a)

Solute

b)

Solvent

c)

Solution

d)

Substance

13.

Match the following

a)

Pure Substance

1.

One element or one compound.

b)

Mixture

2.

Two or more substances not combined.

c)

Element

3.

Contains only one kind of atom.

d)

Compound

4.

Contains two or more kinds of atoms.

14.
A pure substance containing only one kind of atom.
a)
element
b)
mixture
c)
compound
15.
Can only be separated by chemical means.
a)
element
b)
mixture
c)
compound
16.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
17.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
18.
The amount of mass in a specific volume
a)
density
b)
weight
c)
matter
d)
state
19.
The ability of a substance to be pounded or rolled into thin sheets
a)
State
b)
Ductility
c)
Malleability
d)
Thermal Conductivity
20.
The ability of a substance to be pulled into wires
a)
Malleability
b)
Flexibility
c)
State
d)
Ductility
21.
Physical or Chemical?  Water is nonflammable
a)
Physical
b)
Chemical
c)
Neither
22.
Physical or Chemical Property? If copper comes in contact with water, it will turn green.
a)
Physical
b)
Chemical
c)
Neither
23.
Physical or Chemical Property?  The temperature of boiling water is 100 degrees Celsius.
a)
Physical
b)
Chemical
c)
Neither
24.
Physical or Chemical Property?  The solid form of water is ice.
a)
Physical
b)
Chemical
c)
Neither
25.
Define a Physical Property
a)
A property of matter not involving in its manifestation a chemical change
b)
A property in which stops a chemical reaction from occuring.
c)
A property or behavior of a substance which undergoes a chemical change or reaction.
d)
A property which makes the object smell or taste different.
26.
Define a Chemical Property
a)
A property which depends on the objects size or matter.
b)
A property of matter not involving in its manifestation a chemical change
c)
A property or behavior of a substance which undergoes a chemical change or reaction.
d)
A property which makes the object smell or taste different.
27.
Boiling point,melting point, and density are some of an element's
a)
pure properties
b)
physical properties
c)
chemical properties
28.
A mixture that appears to be evenly mixed throughout:
a)
an atom
b)
a compound
c)
a homogeneous mixture
d)
a heterogeneous mixture
29.
 mixture that does NOT appear to be evenly mixed throughout:
a)
an atom
b)
a compound
c)
a homogeneous mixture
d)
a heterogeneous mixture
30.

What is the charge of an electron?

a)

-1

b)

0

c)

+1

31.

Which characteristic defines an atom as belonging to a particular element?

a)

atomic mass

b)

atomic number

c)

neutron count

d)

charge

32.

If Nitrogen (N) is Z=7, how many protons does an atom of it have?

a)

7

b)

not enough information

33.

Why do electrons repel other electrons?

a)

They hate each other

b)

They have the same electrical charge

c)

They have opposite electrical charge

34.

Which physicist claimed that electrons are quantized?

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

35.

Who claimed that electrons act like a wave?

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

36.

The claim that electrons act like a circular standing wave was made by...

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

37.

Which scientist claimed that the location of a particle is uncertain and therefore, unknown?

a)

Niels Bohr

b)

Louis de Broglie

c)

Werner Heisenberg

d)

Erwin Schrodinger

38.

What is an orbital?

a)

Chewing gum

b)

The path the sun takes around the moon

c)

A 3D area outside the nucleus where electrons are found

d)

The electron cloud

39.

All of the following are orbitals EXCEPT:

a)

f

b)

p

c)

d

d)

r

e)

s

40.

How is an orbital is defined in the quantum mechanical model of the atom?

a)

circular path traveled by a proton around an orbital

b)

circular path traveled by an electron around an orbital

c)

region of the most probable proton location

d)

region of the most probable electron location

41.

How many atomic orbitals are in the f level?

a)

7

b)

14

c)

5

d)

10

42.

How many atomic orbitals are in the p level?

a)

3

b)

6

c)

5

d)

10

43.

How many electrons can the d-sublevel hold?

a)

2

b)

6

c)

5

d)

10

44.

How many electrons can an s orbital hold?

a)

2

b)

1

c)

3

d)

6

45.

Which groups on the periodic table represent the s-block of elements?

a)

Groups 1-2

b)

Groups 3-12

c)

Groups 13-18

d)

Inner Transition Metals

46.

Which groups on the periodic table represent the d-block of elements?

a)

Groups 1-2

b)

Groups 3-12

c)

Groups 13-18

d)

Inner Transition Metals

47.

Which groups on the periodic table represent the d-block of elements?

a)

Groups 1-2

b)

Groups 3-12

c)

Groups 13-18

d)

Inner Transition Metals

48.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
49.

Which subshell letter corresponds to a spherical orbital?

a)

s

b)

p

c)

d

d)

f

e)

not enough information

50.

Which statement is true about "p" orbitals?

a)

A subshell that contains three "p" orbitals.

b)

These orbitals are shaped like dumbbells.

c)

A 3p orbital has a higher energy than a 2p orbital.

d)

All of these statements are true

51.

A principle that states that each electron

occupies the lowest energy orbital available.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund’s rule

52.

What does Hund's rule state?

a)

An orbital can contain two electrons only if the electrons have opposite spins.

b)

An orbital can contain two electrons only if all other orbitals at that sublevel are empty.

c)

An orbital can contain two electrons only if the electrons have different energy levels.

d)

An orbital can contain two electrons only if all other orbitals in that sublevel contain at least one electron.

53.

The filling of which orbital is represented by the transition metals in period 4?

a)

3d

b)

3s

c)

2s

d)

2p

54.

According to the Pauli exclusion principle, when can two electrons occupy the same orbital?

a)

only if there is no place else to put them

b)

only if they have the same spin

c)

only if they have opposite spins

d)

only if they are alike in all their properties

55.

Which orbital is displayed correctly?

a)

A

b)

B

c)

C

d)

D

56.

Does this orbital diagram follow the Pauli-Exclusion Principle?

a)

YES

b)

NO

57.

What is the maximum number of electrons that an s orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

58.

How many electrons can the third energy level hold?

a)

2

b)

18

c)
8
d)
0
59.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
60.

Which electron configuration rule describes how every electron configuration after helium starts with 1s2?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

61.

____: the three dimensional region in an atom where electrons are located.

a)

Atom

b)

Nucleus

c)

Atomic Orbital

d)

Electron Configuration

62.

Which orbital has the greatest amount of energy?

a)

4p

b)

4f

c)

4s

d)

4d

63.

Which orbital is a clover shape?

a)

s

b)

d

c)

d

d)

f

64.

What is the electron configuration of sodium?

a)

1s2 2s2 2p6 4s1

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p6 3s3

d)

1s2 2s2 2p6 3s2

65.

What is the electron configuration of magnesium?

a)

1s2 2s2 2p6 3s3

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p5 3s2

d)

1s2 2s2 2p6 3s2

66.

What is the shape of the p orbital?

a)

Spherical shape

b)

Dumbbell shape

c)

Cubic shape

d)

Tetrahedral shape

67.

What are quantum numbers used to describe?

a)

Molecules in a compound.

b)

Neutrons in an atom.

c)

Protons in a nucleus.

d)

Electrons in an atom

68.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

69.

Which of the following units is represented simply by a letter?

a)

orbital

b)

energy level

c)

sublevel

d)

quantum number

70.

Lateral overlap of p-orbitals leads to the formation of

a)

(a) pi-bond

b)

(b) Metallic bond

c)

(c) sigma -bond

d)

(d) lonic bond

71.

This overlapping leads to form

a)

sigma bond

b)

pi-bond

c)

ionic bond

d)

None of these

72.

This type of overlapping is

a)

s-p overlapping perpendicular to the axis

b)

s-p overlapping along the axis

c)

P-P overlapping along the axis

d)

P-P overlapping perpendicular to the axis

73.

This type of overlapping is a

a)

s-p overlapping along the axis

b)

s-s overlapping perpenticular to axis

c)

s-s overlapping along the axis

d)

p-p overlapping along the axis

74.

in the diagram, which overlapping forms sigma bond?

a)

s-s overlapping along the axis

b)

p-p overlapping perpendicular to the axis

c)

s-p overlapping along the axis

d)

both s-s and s-p overlapping along the axis

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