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Chemistry 1st Semester Review Units 4-6

Total questions: 69

Worksheet time: 46mins

Name
Class
Date
1.
Which process involves the joining of small nuclei?
a)
Beta decay
b)
Alpha decay
c)
Nuclear fission
d)
Nuclear fusion
2.
Which process involves the splitting of large nuclei?
a)
Beta decay
b)
Alpha decay
c)
Nuclear fission
d)
Nuclear fusion
3.
The time taken for half of an amount of radioactive atoms to decay.
a)
Nuclear fusion
b)
Full-life
c)
Dead time
d)
Half-life
4.
The nuclear process occurring at a nuclear power plant.
a)
Nuclear fusion
b)
Nuclear fission
c)
Combustion
d)
Multiplication
5.
Arrange in order of increasing ability to penetrate matter.
a)
Beta, gamma, alpha
b)
Alpha, gamma, beta
c)
Gamma, beta, alpha
d)
Alpha, beta, gamma
6.
What do these symbols represent?
a)
alpha particle
b)
beta particle
c)
neutron
d)
gamma ray
7.
How many neutrons are in this isotope of Uranium?
a)
235
b)
92
c)
327
d)
143
8.
How are these isotopes different?
a)
Different atomic numbers
b)
Different number of protons
c)
Different number of neutrons
d)
Different number of electrons
9.
What process is modeled by the equation?
a)
alpha decay
b)
beta decay
c)
fission
d)
fusion
10.
What process is modeled with this equation?
a)
alpha decay
b)
beta decay
c)
fission
d)
fusion
11.
What is the mass number of at isotope that has 20 protons, 21 neutrons and 18 electrons?
a)
18
b)
20
c)
21
d)
41
12.
What is one problem with using nuclear fission as an energy source?
a)
finding radioactive elements that have longer half-lives
b)
finding ways of storing radioactive wastes
c)
finding compounds to cool heated water
d)
finding non-radioactive elements for reactors
13.
What type of nuclear equation is this?
a)
fusion
b)
fission
c)
alpha
d)
beta
14.
What sort of shield will block gamma rays?
a)
skin
b)
paper
c)
aluminum
d)
thick lead
15.
What happens to the atomic number during alpha decay?
a)
The atomic number decreases by 4
b)
The atomic number increases by 1
c)
The atomic number decreases by 2.
d)
The atomic number stays the same.
16.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
17.
If the half-life of uranium-232 is 70 years, how many half-lives will it take for 10 g of it to be reduced to 1.25 g?
a)
1 half-life
b)
2 half-lives
c)
3 half-lives
d)
4 half-lives
18.

What % of the parent isotope remains after 2 Half Lives?

a)

50%

b)

25%

c)

12.5%

d)

6.25%

19.

What is the Half life of this isotope?

a)

5 seconds

b)

10 seconds

c)

15 seconds

d)

20 seconds

20.

Which of the following are imporant uses of nuclear technology at this time?

a)

Produce Electricity

b)

Medical Treatments

c)

Military Uses

d)

All of the above

21.

Which of the following is not an important consideration when trying to find a location to store nuclear waste?

a)

The area is very dry

b)

The area is far from where people live

c)

The area should be at the bottom of the ocean

d)

The area must be geologically stable

22.

Which particle is missing in this equation:

23994Pu ==> 42He + ____

a)

24396Cm

b)

23592U

c)

0-1e-

d)

23995Am

23.

Light is emitted when electrons

a)

move from one atom to another.

b)

collide with one another, releasing energy.

c)

move from a lower energy level to a higher energy level.

d)

move from a higher energy level to a lower energy level.

24.

Flame tests can be used to identify an element. Each element emits characteristic waves of light when it is heated in a flame. What describes how the light is produced?

a)

Protons in the ground state lose energy and give off light.

b)

Protons in the ground state gain energy and are emitted from the nucleus, giving off light.

c)

Electrons in the ground state lose energy and move to an excited state, giving off light.

d)

Electrons in the ground state gain energy, move to an excited state, and give off light when they return to the ground state.

25.

The atomic number of aluminum is 13. What is the correct designation of the electron configuration of aluminum?

a)

1s21p62s22p1

b)

1s22s22p63s3

c)

1s22s22p62d3

d)

1s22s22p63s23p1

26.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

27.

What element has the following electron configuration? [Ar] 4s23d104p3

a)
As
b)
P
c)
Se
d)
Ga
28.

What type of orbital does this image represent?

a)

S

b)

P

c)

D

d)

F

29.

What type of orbital does this image represent?

a)

S

b)

P

c)

D

d)

F

30.

Which area on this periodic table represents the D sublevel?

a)

A

b)

B

c)

C

d)

D

31.

Which area on this periodic table represents the P sublevel?

a)

A

b)

B

c)

C

d)

D

32.

Which area on this periodic table represents the S sublevel?

a)

A

b)

B

c)

C

d)

D

33.
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.
34.

Which of the following is written correctly?

a)

A

b)

B

c)

C

d)

D

35.

Which shows the correct orbital diagram for Cobalt?

a)
b)
c)
d)
36.

What element's orbital notation is pictured here?

a)

Ar

b)

Br

c)

Cu

d)

Cl

37.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

38.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
39.

How many valence electrons does Tin (Sn) have?

a)

8

b)

7

c)

5

d)

4

40.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

41.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
42.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
43.

Which term best describes the behavior of electrons?

a)

Waves

b)

Particles

c)

Both waves and particles

44.

Atoms of elements that are in the same group have the same number of

a)

protons.

b)

neutrons.

c)

valence electrons.

d)

protons and neutrons.

45.

Which of the following elements is an alkali metal?

a)

calcium

b)

magnesium

c)

mercury

d)

sodium

46.

How was Mendeleev's periodic table arranged?

a)

by increasing atomic mass

b)

by decreasing atomic mass

c)

by increasing atomic number

d)

by decreasing atomic number

47.

Each column of the periodic table is

a)

an element.

b)

a group.

c)

an isotope.

d)

a period.

48.

Elements in an elemental family have similar

a)

atomic symbols.

b)

atomic sizes.

c)

atomic weights.

d)

chemical properties.

49.

The order of elements in the modern periodic table is based on an element's

a)

atomic number.

b)

name.

c)

chemical symbol.

d)

atomic mass.

50.

Which statement about the alkali metals is correct?

a)

They are located in the left-most column of the periodic table.

b)

They are extremely nonreactive.

c)

They are usually gases.

d)

They form negative ions with a 1- charge.

51.

Metals tend to be

a)

gases.

b)

dull.

c)

brittle.

d)

good conductors.

52.

Which group is very stable due to the fact that they have a full outermost energy level?

a)

alkali metals

b)

halogens

c)

alkaline-earth metals

d)

noble gases

53.

Which of the following is a property of group 18 elements?

a)

malleable

b)

brittleness

c)

high electrical conductivity

d)

unlikely to react with other elements

54.

Based on its location on the periodic table, which of these elements most likely has physical and chemical properties most similar to boron (B)?

a)

magnesium (Mg)

b)

aluminum (Al)

c)

neon (Ne)

d)

chlorine (Cl)

55.

Which of the following groups on the Periodic Table is likely to form positively charged ions (or cations)?

a)

group 1

b)

group 14

c)

group 17

d)

group 18

56.

Which of the following elements would most likely be a shiny, gray-colored solid at room temperature, conduct electricity, and dent when hit with a hammer?

a)

argon (Ar)

b)

chlorine (Cl)

c)

sulfur (S)

d)

aluminum (Al)

57.

Alkali metals are extremely reactive because they

a)

have every small atomic masses.

b)

are not solid at room temperature.

c)

have one valence electron that is easily removed to form a positive ion.

d)

have two valence electrons that form compounds with calcium and magnesium.

58.

Which scientist is given credit for the arrangement of elements on the modern periodic table?

a)

Moseley

b)

Mendeleev

c)

Bohr

d)

Rutherford

59.

In the image, which column are the halogens located?

a)

A

b)

B

c)

C

d)

D

60.

In the image, which column are the alkali metals located?

a)

A

b)

B

c)

C

d)

D

61.

In the image, which column are the noble gases located?

a)

A

b)

B

c)

C

d)

D

62.

In the image, which column are the alkaline Earth metals located?

a)

A

b)

B

c)

C

d)

D

63.

What is the name of the group of elements which are not pictured in the image?

a)

Metalloids

b)

Transition Metals

c)

Chalcogens

d)

Carbonates

64.

Which column represents elements whose electron configuration ends with s2?

a)

A

b)

B

c)

C

d)

D

65.

Reactivity in a group will generally decrease as you go down a group?

a)

True

b)

False

66.

The electronegativity of halogens is higher than transition metals?

a)

True

b)

False

67.

A sodium ion is smaller than a sodium atom?

a)

True

b)

False

68.

Which diagram correctly shows the trend for electronegativity?

a)

A

b)

B

c)

C

d)

D

69.

Which diagram correctly shows the trend for atomic radius?

a)

A

b)

B

c)

C

d)

D

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