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Electron Configuration and Periodic Table Test Review

Total questions: 47

Worksheet time: 2hrs 34mins

Name
Class
Date
1.

Which electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

2.
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
3.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
4.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

5.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

6.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
7.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

8.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
9.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
10.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

11.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
12.

Cations are _______ that form ____________ ions and __________ electrons.

a)

nonmetals, positive, lose

b)

nonmetals, negative, gain

c)

metals, positive, gain

d)

metals, positive, lose

13.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
14.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
15.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
16.

Which of the following orbitals has the most energy

a)

4s

b)

4p

c)

4d

d)

4f

17.

What is the noble gas configuration for Cobalt (Co)?

a)

[Ne] 3s2 3p5

b)

[Kr] 5s2 4d3

c)

[Ar] 4s2 3d7

d)

[Ar] 3d7

18.

Which of the following orbital diagram's breaks Hund's rule and Pauli exclusion principle?

a)
b)
c)
19.
Which periodic table family could have electrons filling orbitals in the s-block?
a)
Alkaine Earth 
b)
Halogens
c)
Noble Gases
d)
Transition Metals
20.
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.
21.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
22.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
23.
What was Dmitri Mendeleev's greatest contribution to the history of the periodic table?
a)
He arranged all of the known elements by their atomic number
b)
He realised that there was a pattern of reactivity which repeated every 8 elements
c)
He predicted the existence (and properties) of new elements
d)
He identified the "law of triads" which became the groups
24.
The periodic table is organized by the number of ______ in each element's nucleus
a)
neutrons
b)
protons
c)
electrons
d)
atoms
25.
Who arranged the first periodic table.
a)
Mosely
b)
Einstein
c)
Mendeleev
d)
Bohr
26.
What property did Menedleev use to organize his first periodic table?
a)
atomic number
b)
atomic mass
c)
alphabetical order
d)
chemical properties
27.
Why did scientists need/want to organize the elements?
a)
Scientists like things organized
b)
make it easier to understand the elements
c)
have one list of the known elements.
d)
none of the above
28.
Why were there blank spaces left in Mendeleev's periodic table?                                              
a)
He didn't know what to put there.
b)
 Undiscovered elements not yet known.
c)
Multiple elements could have fit
d)
He forgot to add the elements in.
29.

In the modern periodic table elements are arranged by increasing:

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

30.

The bigger the amplitude, the ________ energy carried by the wave.

a)

more

b)

less

31.

The less the frequency, the ________ energy carried by the wave.

a)

more

b)

less

32.
High frequency waves have _________ wavelength.
a)
varying
b)
high
c)
the same
d)
low
33.

A wave with a large wavelength will have a ______ frequency and _____ energy

a)

high, low

b)

high, high

c)

low, high

d)

low, low

34.
The distance from one point to the next corresponding point on a wave is called the ________________.
a)
waveform
b)
peak
c)
amplitude
d)
wavelength
35.

The number of waves that pass a fixed point in a given amount of time is...

a)

frequency

b)

wave speed

c)

amplitude

d)

wavelength

36.
Put the visible light colors in order from longest wavelength to shortest wavelength
a)
Violet, Blue, Green, Orange, Yellow, Red
b)
Red, Yellow, Green, Orange, Violet, Blue
c)
Red, Orange, Yellow, Green, Blue, Violet
d)
Blue, Violet, Green, Yellow, Orange, Red
37.

Select the correct order of waves on the Electromagnetic Spectrum from longest to shortest wavelength.

a)

Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma

b)

Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio

c)

Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio

d)

Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma

38.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
39.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
40.
Electronegativity is...
a)
how good an atom is at attracting electrons
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. 
41.
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
42.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
43.

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

44.

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

45.
Which of the following pairs of elements have similar properties
a)
Barium and Calcium
b)
Sodium and Magnesium
c)
Nickel and Copper
d)
Lithium and Helium 
46.
Which of the following electron configurations represents the most chemically stable atom?
a)
[Ne] 3s1
b)
[Ne] 3s2 3p3
c)
[Ne] 3s2 3p6
d)
[Ar] 4s2 3d6
47.
Which is larger:
P or P-3
a)
P
b)
P-3
c)
both are same size

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