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CP CHEM MIDTERM EXAM REVIEW 25-26

Total questions: 80

Worksheet time: 3hrs 32mins

Name
Class
Date
1.
What is the measurement using the correct number of sig. figs.?
a)
8.5mL
b)
8.50mL
c)
8.45mL
d)
8.4mL
2.
What is the measurement using the correct number of sig. figs.?
a)
39.5 mL
b)
40 mL
c)
39 mL
d)
40.0 mL
3.
What is the measurement using the correct number of sig. figs.?
a)
89cm
b)
88.9cm
c)
88.90cm
d)
88cm
4.

Match the following number with the correct amount of sig figs.

a)

1 sig fig

1.

500

b)

2 sig figs

2.

0.0025

c)

3 sig figs

3.

0.0600

d)

4 sig figs

4.

5689

e)

5 sig figs

5.

50,000.

5.
Which of the following measurements contains two significant figures?
a)
0.00400 L
b)
0.00404 L
c)
0.00044 L
d)
0.00440 L
6.
Which value has only 4 significant digits? 
a)
6.930
b)
0.450
c)
8450
d)
0.392
7.
Which measurement contains 3 sig figs?
a)
200 mL
b)
20.0 mL
c)
0.02 mL
d)
0.020mL
8.

Round 0.005478923 to 4 sig figs.

a)

0.005

b)

0.00548

c)

0.00547900

d)

0.005479

9.

Round 3,456,098 to 2 sig figs.

a)

3,500,000

b)

35

c)

3,400,000

d)

3,500,000.

e)

3,500

10.

What is the charge of a proton?

a)

Negative

b)

Positive

c)

Neutral

11.

What is the charge of a neutron?

a)

Negative

b)

Positive

c)

Neutral

12.

These are found in the nucleus and have a neutral charge.

a)

proton

b)

electron

c)

neutron

13.
These will determine what element an atom is. 
a)
number of neutrons
b)
number of electrons
c)
number of atoms 
d)
number of protons 
14.

How many protons does sulfur have?

a)

32

b)

16

c)

48

d)

12

15.
An atom of the element with atomic number 6 always has _____.
a)
six protons in its nucleus
b)
an atomic mass of six
c)
more than six neutrons
d)
six electron clouds
16.

Al+3

The +3 tell you the

a)

number of protons.

b)

atomic mass.

c)

charge of the atom.

17.

Cations have what charge?

a)

+

b)

-

18.

Valence electrons means..

a)

Electrons inside the atoms

b)

Electrons on the outer most energy level

c)

Electrons with no charge

d)

Electrons that are stable

19.

Element Chlorine [Cl] at group #17 have how many valence electrons?

a)

6

b)

7

c)

17

d)

5

20.

Cations will

a)

Lose electrons

b)

Gain electrons

21.

This isotope have how many neutrons?

a)

26

b)

12

c)

14

d)

16

22.

Which is true about the following chlorine atom?

a)

17 protons and 36 neutrons

b)

17 protons and 19 electrons

c)

17 protons and 19 neutrons

d)

36 protons and 17 neutrons

23.

Which is true of the following beryllium atom?

a)

4 protons and 9 neutrons

b)

5 neutrons and 4 electrons

c)

9 protons and 4 neutrons

d)

4 protons and 2 electrons

24.

The majority of an atom's mass comes from which particle(s)?

a)

Protons

b)

Protons + electrons

c)

Electrons

d)

Protons + neutrons

25.

Why are atoms electrically neutral?

a)

The neutrons balance out any charge.

b)

There are more neutrons than protons or electrons.

c)

Protons and electrons cancel each other out because they have opposite charges.

d)

Neutrons have no charge which makes the who atom neutral.

26.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
27.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
28.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
29.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

30.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
31.

A hydrogen atom is in a ground state when its electron:

a)

Remains at the lowest energy level.

b)

Has moved away from the atom to the ground.

c)

Is moving back and forth through the nucleus.

d)

Has stopped moving.

32.

When an electron in a hydrogen atom jumps from an orbit farther from the nucleus to an orbit closer to the nucleus, it:

a)

emits four photons, one for each of the color lines observed in the line spectrum of hydrogen

b)

emits a single photon with an energy equal to the energy difference of the two orbits

c)

emits a number of photons dependent on the number of energy levels jumped over

d)

none of the above

33.

If you view sunlight through a spectroscope you will see:

a)

You cannot look at sunlight through a spectroscope, it is too dangerous for your eyes

b)

An emission line spectrum of hydrogen

c)

An ultraviolet spectrum

d)

A continuous spectrum

34.

The general relationship between energy and wavelength of an electromagnetic wave can be described as:

a)

indirect

b)

constant

c)

disproportional

d)

direct

35.

Which of the following types of radiation has the highest frequency (look at the back of your periodic table)?

a)

ultraviolet rays

b)

microwaves

c)

X-rays

d)

infrared radiation

36.

How does an atom give up excessive energy when dropping from a higher energy state to a lower state?

a)

a photon

b)

a positron

c)

an electron is expelled.

d)

a neutron is expelled.

37.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

38.

Which color has the highest frequency?

a)

green

b)

blue

c)

red

d)

yellow

39.

Which color has the longest waves?

a)

red

b)

orange

c)

yellow

d)

green

40.

Frequency of light is ___ proportional to wavelength.

a)

directly

b)

inversely

41.

The only type of electromagnetic waves you can see are

a)

infrared waves

b)

ultraviolet waves

c)

visible light waves

42.

When wavelength increases...

a)

energy decreases

b)

energy increases

43.

the distance between peaks of adjacent electromagnetic waves is called:

a)

wavelength

b)

frequency

c)

energy

d)

amplitude

44.

An _____ is the smallest unit of an element that maintains the chemical identity of that element.

a)

Atom

b)

Element

c)

Matter

d)

Particle

45.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

46.
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
47.
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.
48.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
49.
The more protons there are, the  ____ .
a)
Weaker the pull
b)
Smaller the electrons
c)
Stronger the pull
d)
The bigger the electrons
50.

What is a cation?

a)

A negative ion formed from the gaining of electrons.

b)

A positive ion formed from the gaining of electrons.

c)

A negative ion formed from the loss of electrons.

d)

A positive ion formed from the loss of electrons.

51.

What is an anion?

a)

A negative ion formed from the gaining of electrons.

b)

A positive ion formed from the gaining of electrons.

c)

A negative ion formed from the loss of electrons.

d)

A positive ion formed from the loss of electrons.

52.

Which is larger:

P or P-3 ?

a)

P because it is the neutral atom.

b)

P-3 because it lost 3 electrons.

c)

P-3 because it gained 3 electrons.

d)

They are the same size since they are both P.

53.

A sodium atom (Na) loses an electron to form a sodium ion (Na+1). Which statement is correct in regards to describing the ionic radius.

a)

The sodium ion (Na+1) has a larger radius than the neutral sodium atom (Na).

b)

The sodium ion (Na+1) has a smaller radius than the neutral sodium atom (Na).

c)

The sodium ion (Na+1) and the neutral sodium atom (Na) are the same size because they are both sodium.

d)

The sodium ion (Na+1) has twice the radius of the neutral sodium atom (Na).

54.

Which is the smaller atom: Mg or Mg+2?

a)

Mg because it gains an energy level since it gains 2 electrons.

b)

Mg due to extra electron repulsion created by gaining 2 electrons.

c)

Mg+2 because of extra electron repulsion created by gaining 2 electrons.

d)

Mg+2 because it loses an energy level since it loses 2 electrons.

55.
Coulombic Attraction is the attraction between __________ charged particles.
a)
same 
b)
oppositely
c)
two positively
d)
two negatively
56.
An example of Coulombic Attraction in an atom is between
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
protons and protons
57.
As the distance between protons and electrons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is not affected
58.

In a larger atom, the attractive force between the valence electrons and the nucleus

a)

remains the same

b)

is larger

c)

is smaller

d)

is not affected

59.

Select the element that has the strongest Coulombic attraction.

a)

O

b)

F

c)

N

d)

C

60.

Select the element that has the strongest Coulombic attraction.

a)

O

b)

S

c)

Se

d)

Te

61.
As you go down a group, the amount of shielding....
a)
increases
b)
decreases
c)
stays the same
62.
As you go across a period, the amount of shielding...
a)
Increases
b)
decreases
c)
stays the same
63.
What does the symbol -10e represent
a)
alpha
b)
beta
c)
gamma
d)
the zero element
64.
What is the symbol for an alpha particle?
a)
42He
b)
0-1e
c)
0+1 e
d)
10n
65.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
66.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
67.

Complete the nuclear reaction

85209At = ___ + 24He

a)

83205Bi

b)

86209Rn

c)

81207Tl

d)

85208At

68.
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
69.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
70.
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
71.
Solve this equation for alpha decay.
20985At = ___ + 42He
a)
20583Bi
b)
20986Rn
c)
20781Tl
d)
20885At
72.
Which of the following nuclear emissions involves the release of a particle with no mass and a charge of +1?
a)
proton
b)
beta
c)
positron
d)
alpha
73.
Which of the following nuclear emissions has the greatest penetrating power?
a)
alpha
b)
gamma
c)
beta
d)
positron
74.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
decay
d)
gamma radiation
75.
Where does fusion occur naturally?
a)
Underwater
b)
All around us
c)
In the radioactive waste
d)
On the sun
76.
Which of the following is true about nuclear fusion?
a)
It is easy to implement.
b)
It produces less energy than nuclear fission.
c)
It produces more energy than nuclear fission.
d)
It has the ability to occur easily in everyday life.
77.
Takes two small nuclei and combines them into a larger nucleus
a)
fission
b)
fusion
78.

Which reaction represents fusion?

a)
b)
c)
d)
79.

Which reaction represents fission?

a)
b)
c)
d)
80.

Match the following

a)
1.

Beta

b)
2.

Alpha

c)
3.

Neutron

d)
4.

Gamma

e)
5.

Positron

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