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Ch. 4/5 Review

Total questions: 48

Worksheet time: 2hrs 44mins

Name
Class
Date
1.

Proposed the quantum mechanical model of the atom

a)

Sir J.J. Thomson

b)

Erwin Schrodinger

c)

Neils Bohr

d)

John Dalton

2.

Discovered neutrons

a)

Ernest Rutherford

b)

Robert Millikan

c)

Democritus

d)

Sir James Chadwick

3.

Performed oil droplet experiment

a)

Robert Millikan

b)

Eugen Goldstein

c)

Neils Bohr

d)

Sir J.J Thomson

4.

Discovered protons

a)

Sir James Chadwick

b)

Eugene Goldstein

c)

Erwin Schrodinger

d)

Robert Millikan

5.

Discovered electrons

a)

Neils Bohr

b)

Democritus

c)

Sir J.J Thomson

d)

Ernest Rutherford

6.

Proposed discrete energy levels for electrons

a)

Neils Bohr

b)

Sir James Chadwick

c)

John Dalton

d)

Robert Millikan

7.

Developed glass tubes containing gas at low pressure with charged particles

a)

Sir James Chadwick

b)

William Crookes

c)

John Dalton

d)

Democritus

8.

Proposed the plum pudding model (chocolate chip cookie model)

a)

Democritus

b)

William Crookes

c)

John Dalton

d)

Sir J.J. Thomson

9.

Suggested the existence of indivisible, indestructible particles

a)

Democritus

b)

William Crookes

c)

John Dalton

d)

Erwin Schrodinger

10.

Proposed atomic theory based on experimental evidence

4 lines
11.

Determined accurate values for the charge and mass of an electron

a)

Neils Bohr

b)

Eugen Goldstein

c)

Robert Millikan

d)

Sir J.J. Thomson

12.

Discovered the nucleus of an atom

a)

Sir James Chadwick

b)

William Crookes

c)

Ernest Rutherford

d)

Eugen Goldstein

13.

Performed experiment in which alpha particles were fired at extremely thin gold foil

a)

Democritus

b)

Eugen Rutherford

c)

William Crookes

d)

Erwin Schrodinger

14.

Performed transmutation experiment changing beryllium atoms into carbon atoms

a)

Neils Bohr

b)

Sir James Chadwick

c)

Democritus

d)

Sir J.J. Thomson

15.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
16.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
17.
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
18.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
19.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
20.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
21.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
22.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
23.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

24.
There are 4 different types of subshells (orbitals) s,p,d,f.
a)
true
b)
false
25.
What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
26.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
27.

Which type of orbital has the lowest energy?

a)

p orbital

b)

d orbital

c)

s orbital

d)

f orbital

28.

Atoms with the same atomic number but having different numbers of neutrons

a)

atomic mass unit

b)

atomic mass

c)

atomic number

d)

isotope

29.

You get the number of electrons in an atom from the ______________.

a)

Mass number

b)

Atomic mass

c)

Atomic number

d)

Atomic mass unit

30.

The number of protons and neutrons make up the ________________.

a)

Atomic mass unit

b)

Atomic mass

c)

Atomic number

d)

Mass number

31.

The number of protons in an atom comes from the _____________.

a)

Atomic mass unit

b)

Atomic mass

c)

Atomic number

d)

Mass number

32.

The weighted average of the atomic masses of the isotopes of an element is called _________________.

a)

Atomic mass unit

b)

Atomic mass

c)

Atomic number

d)

Mass number

33.

1/12 the mass of a carbon-12 atom is how we got a(n) ______________.

a)

Atomic mass unit

b)

Atomic mass

c)

Atomic number

d)

Mass number

34.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

35.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
36.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
37.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
38.

The 1st energy level can hold a maximum of ____ electrons

a)

2

b)

4

c)

6

d)

8

39.

The 2nd energy level can hold a maximum of ____ electrons.

a)

2

b)

4

c)

6

d)

8

40.

The 3rd energy level can hold ____ electrons.

a)

8

b)

16

c)

18

d)

24

41.

The 4th energy level can hold ____ electrons.

a)

20

b)

24

c)

32

d)

40

42.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

43.

Which of the following is the orbital notation for oxygen?

a)
b)
c)
d)
44.

How many electron pairs are in an atom of neon?

a)

2

b)

5

c)

10

d)

4

45.

How many electron pairs are in an atom of sulfur?

a)

3

b)

5

c)

7

d)

9

46.

Calculate the average atomic mass of silver.

a)

106.38649amu

b)

111.91896amu

c)

107.8677amu

d)

121

47.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
48.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.

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