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Chem II Unit 1 Review

Total questions: 95

Worksheet time: 1hrs 11mins

Name
Class
Date
1.

How many valence (outer) electrons does an Oxygen atom have?

a)

2

b)

6

c)

8

d)

16

2.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
3.

Name this element.

a)

Neon

b)

Magnesium

c)

Sodium

d)

Manganese

4.

If an atom of Sodium has a mass number of 23, it will have...

a)

23 protons

b)

11 neutrons

c)

12 protons

d)

12 neutrons

5.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
6.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
7.

Which subatomic particle has a positive charge and is found inside the nucleus?

a)

Electron

b)

Proton

c)

Neutron

d)

Nucleus

8.

Which subatomic particle has a neutral charge and is found inside the nucleus?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Nucleus

9.

Which scientist developed this model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

10.

What is the maximum number of electrons that can be found in the second shell (energy level)?

a)

2

b)

8

c)

18

11.

What is the maximum number of electrons that can be found in the first shell (energy level)?

a)

2

b)

8

c)

18

12.
An atom has an atomic number of 15 and a mass number of 31. How many protons are there in the atom?
a)
15
b)
31
c)
16
d)
47
13.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
14.
An element has three different isotopes. One has a mass of 35.00 amu; another has a mass of 36.00  amu; and another has a mass of 38.00  amu. What is the average atomic mass of this element?
a)
36.33 amu
b)
37.00 amu
c)
12.11 amu
d)
impossible to tell
15.
An element with 4.35% have a mass of 49.9461 amu, 83.79% have amass of 51.9405 amu, 9.50% have a mass of 52.9407 amu, and 2.36% have a mass of 53.9389amu.
a)
51.99 amu
b)
52.19 amu
c)
53.45 amu
d)
17.33 amu
16.

The​ (a)   of a wave is the distance between adjacent crests (or any two analogous points) and is measured in units such as meters, micrometers, or nanometers.

Choose from the below words
wavelength
frequency
17.

The ____________ is a characteristic of light that represents the number of cycles that pass through a stationary point in a given period of time (often measured in 1/s, s-1, or hertz (Hz))

a)

wavelength

b)

frequency

18.

Wavelength is ​ (a)   proportional to frequency.

Choose from the below words
inversely
directly
19.

True or False: In a vacuum, all forms of electromagnetic radiation travels at a constant speed of 3.00 x 108 m/s.

a)

True

b)

False

20.

As the frequency of an electromagnetic wave increases, the amount of energy in that wave

(a)  

Choose from the below words
increases.
decreases.
stays the same.
21.
Solve this problems using the equation: C = λ  x  ν
If an AM radio station broadcasts at 9.95 x 105 Hz, what is the wavelength of this radiation?
a)
6.59 x 10-28 m
b)
1.01 x 10-6 m
c)
3.32 x 10-3 m
d)
301 m
22.

Microwaves are used to cook food and transmit information. What is the wavelength of a microwave that has a frequency of 3.44 × 109 Hz?

For this problem, what formula do you use?

a)

c = λν

b)

E = hv

c)

λ = c/v

d)

v = c/λ

23.

Emission spectra (bright line spectra) are created when electrons move from ___.

a)

higher to lower energy levels.

b)

lower to higher energy levels.

c)

s orbitals to p orbitals.

d)

one atom to a different atom.

24.

The analysis of the way matter emits and absorbs radiation is called ___.

a)

astronomy

b)

chemistry

c)

spectroscopy

d)

atomic theory

25.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

26.

In which state does an electron have the least amount of energy?

a)

Excited state

b)

Ground state

c)

Orbital

d)

Bohr model

27.

The proper pair of the l value with the orbital shape.

a)

0; f

b)

3; p

c)

1; s

d)

2; d

28.

Match the type of orbital with the value of the angular momentum quantum number, l.

a)

s

1.

l = 0

b)

p

2.

l = 1

c)

d

3.

l = 2

d)

f

4.

l = 3

29.

Match the quantum number with its symbol.

a)

Principal Quantum Number

1.

n

b)

Angular momentum quantum number

2.

l

c)

Magnetic quantum number

3.

ml

d)

Spin quantum number

4.

ms

30.

Which of the following is NOT a possible pair of quantum numbers?

a)

2p

b)

2d

c)

4p

d)

4f

31.

The maximum number of electrons with quantum numbers with n=3 and l=2 is

a)

2

b)

4

c)

6

d)

10

32.

For l = 0, tick the possible values of ml :

a)

-2

b)

-1

c)

0

d)

1

e)

2

33.

Match the quantum number with what it tells us.

a)

Principal Quantum Number

1.

which shell

b)

Angular momentum quantum number

2.

which shape

c)

Magnetic quantum number

3.

which orbital

d)

Spin quantum number

4.

spin up or spin down

34.

Match the quantum number what it tells us.

a)

which main energy level

1.

n

b)

what shape/type of subshell

2.

l

c)

which orbital in a subshell

3.

ml

d)

spin of the electron

4.

ms

35.

Which of the following is the (n) / principal quantum number of 3d10?

a)

1

b)

2

c)

3

d)

4

36.

Let's check your memory. What is the shape of the s configuration?

a)
b)
c)
d)
37.

Let's check your memory. What is the shape of the d configuration?

a)
b)
c)
d)
38.

Which of the following is the Angular (l) quantum number of 4f10

a)

0

b)

1

c)

2

d)

3

39.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of Na?

a)

2, 1, 0, -½

b)

2, 0, 0, -½

c)

3, 1, 1, +½

d)

3, 0, 0, +½

40.

How many electrons are in 1s2 2s2 2p4?

a)

5

b)

6

c)

8

d)

13

41.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

42.

What is the noble gas configuration for 1s2 2s2 2p6 3s2?

a)

[He] 3s2

b)

[Ne] 3s2

c)

[Ar] 3s2

d)

[Ar] 4s2

43.

What is the noble gas configuration for Cobalt?

a)

[Kr] 4s2 3d7

b)

[Kr] 4s2 4d7

c)

[Ar] 4s2 3d7

d)

[Ar] 4s2 4d7

44.

What element has the electron configuration 1s2 2s2 2p6 3s2 3p5?

a)

Chlorine

b)

Argon

c)

Fluorine

d)

Sulfur

e)

Bromine

45.

Match the following quantum numbers to the correct element.

a)

3, 1, 1, -1/2

1.

Ar

b)

2, 1, -1, +1/2

2.

B

c)

1, 0, 0, -1/2

3.

He

d)

5, 2, 2, -1/2

4.

Hg

46.

Which element has the quantum numbers n=4 l=2 ml= -1 ms= +1/2

a)

Rhodium

b)

Zirconium

c)
Lithium
d)
Titanium
47.

Which of the following transitions of an electron in a helium atom will emit a photon that has the highest frequency?

a)

n=7 to n=6

b)

n=6 to n=4

c)

n=3 to n=4

d)

n=2 to n=5

e)

n=1 to n=3

48.

Which of the following will have similar properties to 1s2 2s2 2p6 3s2 3p2?

a)

carbon

b)

calcium

c)

chlorine

d)

cesium

49.

What is the electron configuration for potassium?

a)

1s2 2s2 2p6 3s2 3p6 4s1

b)

1s2 2s2 2p6 3s2 3p6 4s2

c)

1s2 2s1 2p6 3s2 3p5 4s1

d)

1s2 2s2 2p6 3s1

50.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

51.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
52.

What is the noble gas notation electron for Sulfur?

a)

[Ne] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

53.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

54.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
55.

All orbitals of equal energy are occupied by one electron before any single orbital is occupied (paired) by a second electron.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund’s rule

d)

Core Notation

56.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
57.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
58.
According to the Aufbau Principle, which sublevel should starting filling with electrons before the 3p sublevel?
a)
3s
b)
2p
c)
4s
d)
4p
59.

Which of the following will have a larger radius than Zinc?

a)

Gallium

b)

Magnesium

c)

Aluminum

d)

Strontium

60.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon

b)

Antimony

c)

Neon

d)

Germanium

61.

Which of the following will have a lower ionization energy than Scandium (Sc)?

a)

Helium

b)

Calcium

c)

Titanium

d)

Magnesium

62.

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....

a)

decreases

b)

increases

c)

remains the same

d)

none of the above

63.

As you move down the periodic table atoms get bigger. This is because ____________.

a)

the atoms have more mass

b)

the atoms have more energy levels

c)

the atoms have more protons

d)

the atoms have more neutrons

64.

As you move across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass

b)

the atoms have more protons

c)

the atoms have less mass

d)

the atoms have less electrons

65.

Electronegativity is

a)

the ability of an atom to attract/accept electrons

b)

the energy required to move an electron from a specific atom

c)

the ability of an atom to lose electrons

d)

how easy it is to make friends

66.

Ionization energy is

a)

the energy required to add an electron to a specific atom

b)

the energy required to shield the outer electrons from the nucleus

c)

how much energy it takes to remove an electron from an atom

d)

a measure of the ability of an atom to attract electrons

67.

The atom with the largest atomic radius in Group 18 is

a)

Argon

b)

Krypton

c)

Helium

d)

Radon

68.

Metals have the largest

a)

atomic radius and electronegativity

b)

atomic radius only

c)

electronegativity and ionization energy

d)

ionization energy and atomic radius

69.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period and increases down a group.

b)

Ionization energy increases across a period and increases down a group.

c)

Electronegativity decreases across a period and decreases down a group

d)

Ionic radius increases across a period and increases down a group.

70.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)

decreases, increases

b)

increases, decreases

c)

increases, increases

d)

stays the same, increases

71.

Vertical columns of elements (families) on the periodic table with similar properties

a)

groups

b)

quadrants

c)

periods

d)

rows

72.

Which has the greater electronegativity Cl or Al?

a)
Cl
b)
Al
73.
How are elements on the periodic table arranged by?
a)
in alphabetic order
b)
simular physical & chemical properties
c)
their symbols
d)
Just simular physical properties
74.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

75.

Which scientist is given credit for discovering the electron?

a)

Bohr

b)

Dalton

c)

Thomson

d)

Rutherford

76.

Who discovered that electrons travel in specific orbits around the nucleus?

a)

Bohr

b)

Schrodinger

c)

Democritus

d)

Rutherford

77.

Who was the first person to say that matter was made of atoms, and these atoms could not be created or destroyed?

a)

Dalton

b)

Democritus

c)

Rutherford

d)

Thomson

78.

Whose model of the atom is known as the "plum pudding" model (aka the "chocolate chip cookie" model)?

a)

Rutherford

b)

Schrodinger

c)

Dalton

d)

Thomson

79.

Whose gold foil experiment led to his conclusion that the nucleus of an atom contained protons?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

80.

Who developed the idea that electrons are found in a cloud?

a)

Bohr

b)

Dalton

c)

Schrodinger

d)

Rutherford

81.

Whose model of the atom is represented in the image?

a)

Thomson

b)

Bohr

c)

Dalton

d)

Rutherford

82.

Whose model is the most modern interpretation of an atom?

a)

Dalton

b)

Democritus

c)

Rutherford

d)

Schrodinger

83.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
84.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
85.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
86.
Because atoms are neutral, the number of protons will be equal to the number of __________ in an atom.
a)
Positrons
b)
Neutrons
c)
Electrons
d)
Nuclei
87.

How many quarks make up a proton?

a)

1

b)

2

c)

3

88.

Previously science believed protons and neutrons to be indivisible. We now know protons to be made of

a)

atomeons

b)

nucleons

c)

quarks

d)

atomeons, nucleons, and quarks

89.

Where are valence electrons located in an atom?

a)

On the outermost energy level

b)

On the innermost energy level

c)

In the nucleus

90.

What rule states that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons?

a)

Valence Electron Rule

b)

Octet Rule

c)

Energy Level Rules

d)

All of the above

91.

What is a charged atom known as?

a)

Electron

b)

Proton

c)

Ion

d)

Neutron

92.

What is a positive ion called?

(a)  
Choose from the below words
anion
cation
isotope
covalent
93.

What is a negative ion called?

(a)  
Choose from the below words
anion
cation
covalent
isotope
94.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
95.

One of the outermost electrons in a calcium atom in the ground state can be described by which of the following sets of four quantum numbers?

a)

4, 1, 1, 1/2

b)

4, 0, 0, -1/2

c)

4, 0, 1, -1/2

d)

4, 1, 0, -1/2

e)

4, 2, 0, -1/2

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