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Unit 3 Honors IPC Electrons and Periodic Table

Total questions: 92

Worksheet time: 2hrs 39mins

Name
Class
Date
1.

The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is

a)

3

b)

6

c)

8

d)

10

2.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

3.

What is the noble gas shorthand electron for Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p4

4.

What atom matches this electron configuration?

[Xe] 6s25d9

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

5.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

6.

Which of the following has the smallest atomic radius?

a)

K

b)

Na

c)

Li

d)

Cs

7.

How many valence electrons does Si contain? (click to see image)

a)

14

b)

28

c)

2

d)

4

8.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

0

9.

An orbital can at most hold how many electrons?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

10.

What is the highest occupied energy level?

a)

1

b)

2

c)

3

d)

4

11.

What is the highest occupied energy level?

a)

4

b)

5

c)

6

d)

7

12.

Which element is depicted from this orbital diagram

a)

Fluorine

b)

Neon

c)

Chlorine

d)

Argon

13.

Which is associated with more energy?

a)

2p

b)

2s

c)

3p

d)

1s

14.

This orbital diagram represents:

a)

C

b)

B

c)

N

d)

O

15.

How many electrons can an s sublevel hold?

a)

1

b)

2

c)

3

d)

4

16.

How many atomic orbitals are there in the p sublevel?

a)

2

b)

3

c)

4

d)

5

17.

How many atomic orbitals are there in the d sublevel?

a)

3

b)

4

c)

5

d)

6

18.

How many atomic orbitals are there in the f sublevel?

a)

4

b)

5

c)

6

d)

7

19.

Electrons fill energy levels and sublevels of _____ energy first.

a)

lower

b)

higher

20.

Which of the following is a p block element?

a)

Ca

b)

Ar

c)

Re

d)

Au

21.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
22.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
23.
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 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
24.
What is the electron configuration for Bromine (Br)
a)
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1
b)
1s2, 2s2, 2p4
c)
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p5
d)
1s2, 2s2, 2p6
25.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
26.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
27.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
28.
The Quantum Mechanical Model is the most recent atomic model.
a)
True
b)
False
29.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
30.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
31.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
32.
Which of the following does not exist?
a)
2d
b)
5f
c)
4d
d)
6p
33.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
34.
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.
35.
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 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
36.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
37.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
38.

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

a)

decreases, increases

b)

increases, increases

c)

increases, decreases

d)

stays the same, increases

39.

Atomic radius generally increases as we move __________.

a)

down a group and from right to left across a period

b)

up a group and from left to right across a period

c)

down a group and from left to right across a period

d)

up a group and from right to left across a period

40.

Vertical columns of elements (these are also known as a "family") - they also have the same number of valence electrons and are known as ________________.

a)

groups

b)

periods

c)

quadrants

d)

rows

41.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
42.

Which element would have the same number of energy levels or orbitals as Zinc?

a)

Cadmium

b)

Krypton

c)

Silver

d)

Tin

43.

Rank the following from lowest ioniziation energy to highest ionization energy: C, P, S, As

a)

As, S, P, C

b)

As, C, P, S

c)

P, S, As, C

d)

C, P, S, As

44.

Which has the greatest Electronegativity:

a)

Cl

b)

Al

c)

Br

d)

He

45.
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
46.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
47.
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
48.

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 and an increased charge

d)

the atoms have less electrons and an increased charge

49.

Electronegativity is...

a)

the ability of an atom to gain an electron

b)

the ability of an atom to lose electrons

c)

the energy required to remove an electron from a specific atom

d)

how easy it is to make friends.

50.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
51.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
52.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
53.

When an electron has its lowest possible energy, the atom is in its _______________

a)

Excited state

b)

transition state

c)

Highest energy state

d)

Ground state

54.
How many orbitals are available to hold electrons in the 4th energy level (n=4)?
a)
4
b)
8
c)
16
d)
32
55.
According to the Aufbau Principle, which sublevel should starting filling with electrons after 5s?
a)
6s
b)
5p
c)
4d
d)
3f
56.

If n = 3, what is the maximum number of electrons that can fit in this shell?

a)

2

b)

8

c)

18

d)

32

57.

Max Planck described packets of energy as

a)

electrons

b)

quanta

c)

ions

d)

protons

58.

An element with the ns2(n-1)d4 configuration would be in what group

a)

16

b)

6

c)

4

d)

unknown

59.

elements with the ns2np2 configuration would be in group

a)

4

b)

2

c)

14

d)

8

60.

The valence electrons for an element with ns2np4 would be

a)

2

b)

4

c)

8

d)

6

61.
This is the most complete and current model of the atom. It consists of 61 elementary particles. Electrons are located in complex orbitals.
a)
The "Quantum Mechanical Model" of the atom
b)
The "Rutherford Model" of the atom
c)
The "Plum Pudding Model" of the atom
d)
The "Solar System Model" of the atom
62.

The Bohr model depicts

a)

the atom as a small positively charged nucleus surrounded by electrons.

b)

paired and unpaired valence electrons in an atom.

c)

covalent bonds.

d)

valence electrons.

63.

When drawing a Lewis Structure, how do you determine the number of valence electrons?

a)

Atomic Number

b)

Mass Number

c)

Atomic Mass Unit

d)

By the column the element is found

64.

The Lewis Structure is also known as

a)

a Bohr Model.

b)

an electron dot diagram.

c)

valence electron drawings.

d)

a planetary model.

65.

One important difference between Bohr's model and the modern on is that electrons in the modern model are

a)

moving in fixed orbits around the nucleus

b)

moving in an electron cloud

c)

moving in a random motion around the nucleus

d)

not moving

66.

This model added on to previous models by showing electrons existed at certain "energy levels". However it does not accurately show what those levels look like.

a)

The "Bohr Model" of the atom

b)

The "Rutherford Model" of the atom

c)

The "Plumb Pudding Model" of the atom

d)

The "Quantum Mechanical Model" of the atom

67.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

68.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

69.

With each higher energy level, the electrons are

a)

lower in energy

b)

more stable

c)

weaker

d)

farther from the nucleus

70.

The difference between an orbit and an orbital is:

a)

an orbit is a set path, but an orbital has no dimension

b)

an orbital is a set path, but an orbit cannot be defined

c)

an orbit is a set path, but an orbital is a 3-dimensional region in which electrons may be found with high probability

d)

there is no difference when it comes to electron configurations

71.

Properly pair the l-value is with the orbital shape.

a)

0; f

b)

1; s

c)

3; p

d)

2; d

72.

If l equals 2 then what are the ml values.

a)

-1, 0, 1

b)

2, 1, 0, -1, -2

c)

-2, -1, 0, 1, 2

d)

0, 1, 2, 3

73.

n=3. l=2. ml = -1. ms = +1/2

What electron is this?

a)

3p2

b)

3s1

c)

3d2

d)

3f4

74.

What does the n quantum number represent?

a)

spin

b)

shape

c)

number of orbitals

d)

energy level

75.

Which of the following sub levels correspond to n=3 l=2

a)

2p

b)

3s

c)

3p

d)

3d

e)

3f

76.

In a theoretical g sub-shell which would be next after f, how many electrons would it hold?

a)

20

b)

18

c)

24

d)

36

77.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

78.

The line emission spectrum shown happens when

a)

Electrons transition from lower to higher energy levels.

b)

Electrons transition from higher to lower energy levels.

c)

Electrons exist in fixed energy states.

79.

Atoms emit light when...

a)

electrons move down to lower energy levels

b)

electrons move up to higher energy levels

c)

electrons move in circular orbits around the nucleus

d)

electrons crash into the nucleus

80.

Why do the spectra of individual elements only have certain bands of colors?

a)

they don't have enough electrons

b)

not all of the electrons are changing energy levels

c)

electrons are only allowed to have certain energies

d)

some electrons are moving up levels while some are moving down

81.

Which color has the highest energy?

a)

red

b)

yellow

c)

green

d)

violet

82.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
83.
Why are line emission spectra of elements called "atomic fingerprints"?
a)
They are all the same
b)
They are all unique
c)
They are all similar
d)
They all contain colored light
84.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

85.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

86.
What gases are in the unknown mixture?
a)
Gas B & Gas D
b)
Gas C & Gas B
c)
Gas A & Gas D
d)
Gas D & Gas C
87.
The parallel lines represents...
a)
energy levels of the atom
b)
energy levels of the electrons
c)
energy levels of the photons
d)
energy levels of the nucleus
88.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
89.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

90.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

91.

Each element produces its own pattern of emission spectra lines because each element has its own distinct

a)

Speed of light

b)

Electron configuration

c)

Number of neutrons

d)

None of these

92.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

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