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Unit 4 Review (Electrons and Periodic Trends)

Total questions: 105

Worksheet time: 4hrs 34mins

Name
Class
Date
1.
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
2.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)

Zinc (Zn)

b)

Copper (Cu)

c)

Nickel (Ni)

d)

Germanium (Ge)

3.

Write the configuration for Phosphorus (P)

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

d)

1s2 2s2 2p5 3s2 3p3

4.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
5.
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
6.

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

7.

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

8.

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

a)

8

b)

10

c)

2

d)

4

9.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
10.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
11.

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

12.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
13.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
14.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

15.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
16.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
17.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
18.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
19.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
20.

What is the electron configuration of Ca+2?

a)

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

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p6 4s4

d)

1s2 2s2 2p6 3s2 3p6 4s2 4p2

21.

The Ca+2 ion is isoelectronic with what -1 ion?

a)

F-1

b)

Cl-1

c)

Br-1

d)

K-1

e)

Ar-1

22.

Which of the following are isoelectronic with O-2 ion?

a)

Flourine

b)

Mg+1

c)

Flouride

d)

Nitride

e)

Neon

23.

1s2 2s2 2p6 is the electron configuration of which ION?

a)

Aluminum

b)

Chloride

c)

Beryllium

d)

Boron

e)

Neon

24.

What is the electron configuration of the Sc+2 ion? (Element #21).

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2 3p6 3d2

c)

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

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d2

25.

Which levels do electrons get removed from first, when they are lost?

a)

1st level

b)

outer levels

c)

valence shells

d)

s and p levels

e)

d levels

26.

What is the electron configuration of the Sn+3 ion? (element #50)

a)

1s2 2s1

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2

d)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p6 5d10

e)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10

27.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Pauli's Exclusion Principle

c)

Hund's Rule

d)

Heisenberg uncertainty principle

28.

What is incorrect about this orbital diagram?

a)

Both arrows in the filled 2p box should be pointing the same direction

b)

In the there should only be 1 arrow in the first 2p box and one in the 2nd 2p box

c)

There is nothing incorrect with this diagram

d)

All the arrows should be pointing the same direction.

29.

Which rule is violated in the following orbital diagrams?

a)

Hund's Rule

b)

Pauli's Exclusion Principle

c)

Aufbau Principle

30.

Which of the following is the electronic configuration for Mg2+ ion?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p2

d)

1s2 2s2 2p6 3s2

31.

What is meant by isolectronic?

a)

Group of atoms or ions have the same electronic configuration

b)

Group of atoms or ions have the same protonic configuration

c)

Group of atoms or ions have the same electrical properties

d)

Group of atoms or ions have the same electron charge

32.

What is the example of species that are isolectronic?

a)

Li+ and H+

b)

S2- and O2-

c)

Li+ and He

d)

F- and Cl-

33.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
34.
Write the electronic structure for Cu+1 ion
a)
[Ar]4s13d10
b)
[Ar]4s13d9
c)
[Ar]4s03d10
d)
[Ar]3d10
35.

Which scientist edited the Periodic Table and arranged elements in increased atomic number?

a)

Rutherford

b)

Dalton

c)

Mendeleev

d)

Moseley

36.

Which scientist created the Periodic Table and arranged elements in increasing atomic mass?

a)

Rutherford

b)

Thomson

c)

Mendeleev

d)

Moseley

37.

Elements in the same group or family have _____________.

a)

the same number of valence electrons and different properties.

b)

the same number of valence electrons and similar properties

c)

different number of valence electrons and similar properties.

d)

different number of valence electrons and different properties.

38.

What is the name of Group 1 elements?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Halogens

39.

What is the name of the elements that are unreactive and have a full octet?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Transition Metals

40.

The Halogen group has an oxidation number of -1. Why?

a)

The Halogen group will gain one electron, therefore have an oxidation number of -1.

b)

The Halogen group will lose one electron, therefore have an oxidation number of -1.

c)

The Halogen group will lose seven electrons, therefore have an oxidation number of -1.

41.

Where are metalloids located on the Periodic Table?

a)

In the s block.

b)

In the f block.

c)

In the d block.

d)

The elements that touch the staircase except aluminum.

42.

What is the trend for atomic radius (radii)?

a)

It increases left to right on the Periodic Table and decreases down a group.

b)

It decreases left to right on the Periodic Table and increases down a group.

c)

It increases left to right on the Periodic Table and increases down a group.

d)

It decreases right to left on the Periodic Table and decreases down a group.

43.

Why does the atomic radius decrease across a period?

a)

There are more protons in the nucleus that pull electrons closer.

b)

There are more electrons in the nucleus that pull protons closer.

c)

There are more protons in the nucleus that pull neutrons closer.

d)

There are more neutrons in the nucleus that pull protons closer.

44.

What does the atomic radius increase down a group?

a)

There are more electrons and energy levels.

b)

There are fewer electrons and energy levels.

c)

There are more protons that need more energy levels.

d)

There are more neutrons that need more energy levels.

45.

What element has the largest atomic radius?

a)

oxygen

b)

neon

c)

carbon

d)

sodium

46.

Which element has the smallest atomic radius?

a)

magnesium

b)

chlorine

c)

bromine

d)

argon

47.

What is the trend for ionization energy?

a)

Across a period (left to right) it increases and down a group it decreases.

b)

Across a period (left to right) it decreases and down a group it increases.

c)

Across a period (left to right) it decreases and down a group it decreases.

d)

Across a period (left to right) it increases and down a group it increases.

48.

What is ionization energy?

a)

The energy required to remove an electron from a neutral atom of an element.

b)

The energy change that occurs when an electron is acquired by a neutral atom.

c)

The measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

d)

How close an atom is to its neighboring atom.

49.

Which element has the highest ionization energy?

a)

oxygen

b)

sulfur

c)

silicon

d)

potassium

50.

What is the ability of an atom in a chemical compound to attract electrons from another atom in the compound?

a)

ionization energy

b)

electronegativity

c)

atomic radius

d)

electron affinity

51.

Which element has the largest electronegativity?

a)

barium

b)

oxygen

c)

iron

d)

lithium

52.

Which family is the most reactive Non-Metals

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Transition Metals (Group 3-12)

d)

Halogens (Group 17)

e)

Noble Gases (Group 18)

53.

As you move down a group on 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

54.

Which atom has the largest atomic radius?

a)

potassium (K)

b)

rubidium (Rb)

c)

francium (Fr)

d)

cesium (Cs)

55.

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

a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
56.
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.
57.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Alkaline Earth Metals

d)

Transition Metal Family

58.
Is silicon a metal, nonmetal or metalloid?
a)
Metal
b)
NonMetal
c)
Metalloid
59.

How many valence electrons does Beryllium (4Be) have?

a)

5

b)

1

c)

2

d)

8

60.

How many valence electrons does Silicon (14Si) have?

a)

4

b)

8

c)

3

d)

1

61.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

62.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
63.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
64.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
65.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
66.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
67.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
68.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
69.
Light behaves like both a particle and a ______.
a)
Mass
b)
Wave
c)
Current
70.
What particles make up light?
a)
Photons
b)
Neutrons
c)
Protons
71.
Which of the following types of radiation has the shortest wavelength and the highest frequency?
a)
Radio Waves
b)
Infrared
c)
Visible
d)
X-Rays
72.

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

a)

high, low

b)

high, high

c)

low, high

d)

low, low

73.

The frequency of violet light is 7.5x1014 Hz. What is its wavelength?

a)

4.0x10-7 m

b)

4.0x107 m

c)

2.25x1023m

d)

2.25x1023 Hz

74.

Red light has a wavelength of 675 x 10-9 m. What is its frequency?

a)

2.03x1011 m

b)

4.44x1014 Hz

c)

4.44x1014 nm

d)

2.03x1011 Hz

75.
As the wavelength of light increases
a)
the frequency increases.
b)
the speed of light increases.
c)
the energy decreases.
d)
the intensity increases.
76.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
77.
What is the wavelength for a quantum of light with energy of 7.56x10-19J? (λ=hc/E) 
a)
2.62x10-7m
b)
2.62x107m
c)
2.64x10-45m
d)
2.64x1045m
78.
The energy for a quantum of light is 2.84x10-19J. What is the wavelength. (λ=hc/E)
a)
6.97x10-45m
b)
6.97x1045m
c)
6.97x10-7m
d)
6.97x107m
79.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
80.

Which element in Period 6 has the lowest ionization energy?

a)

Rn

b)

Cs

c)

Os

d)

Tm

81.

Which of the following would be the ion formed by Gallium (Ga)?

a)

Ga+

b)

Ga+3

c)

Ga-3

d)

Ga-

82.

Which of the following would be the ion formed by sulfur (S)?

a)

S-

b)

S-2

c)

S+

d)

S+2

83.
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 
84.

Which is larger, P or P-3?

a)

P

b)

P-3

c)

both are same size

85.

Which is larger, Na or Na+?

a)

Na

b)

Na+

c)

They are the same size.

86.

Which is smaller, O or O2-?

a)

O

b)

O2-

c)

They are the same size.

87.

Which is smaller, Al or Al3+?

a)

Al

b)

Al3+

c)

They are the same size.

88.

Which types of elements form cations?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

89.

Which types of elements form anions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

90.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

91.

How many electrons would a Calcium ion gain/lose?

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

92.

What is the symbol for the most stable ion of Sulfur?

a)

S-2

b)

S+2

c)

S-8

d)

S+6

93.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

94.
As you go down a group, the amount of shielding....
a)
increases
b)
decreases
c)
stays the same
95.
As you go across a period, the amount of shielding...
a)
Increases
b)
decreases
c)
stays the same
96.
What is EFFECTIVE nuclear charge
a)
The charge that actually matters
b)
The sharge of an element
c)
The charge felt by the valence electrons
d)
The charge felt by the inner orbital electrons
97.
As you move down a group, the effective nuclear charge....
a)
increase
b)
decreases
c)
stays the same
98.
As you move across a period, the effective nuclear charge...
a)
increases
b)
decreases
c)
stays the same
99.
Which of the following elements has the most "shielding" electrons?
a)
Nitrogen
b)
Phosphorus
c)
Arsenic
d)
Bismuth
100.
Which of the following elements has the most "shielding" electrons?
a)
Neon
b)
flourine
c)
oxygen
d)
They have the same
101.
What are the sublevels that make up the n=1 energy level?
a)
s
b)
s, p
c)
s, p, d
d)
s, p, d, f
102.
What are the sublevels that make up the n=2 energy level?
a)
s
b)
s, p
c)
s, p, d
d)
s, p, d, f
103.
What are the sublevels that make up the n=3 energy level?
a)
s
b)
s, p
c)
s, p, d
d)
s, p, d, f
104.
What are the sublevels that make up the n=4 energy level?
a)
s
b)
s, p
c)
s, p, d
d)
s, p, d, f
105.
Ions from the halogen group form what oxidation state?
a)
+1
b)
-1
c)
-7
d)
+7

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