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HC U3 Practice Test Periodic Trends and Atomic Structure

Total questions: 200

Worksheet time: 5hrs 20mins

Name
Class
Date
1.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
2.
Which has the greater EN: 
N or C?
a)
C
b)
N
3.
Which has the greater EN: 
H or F?
a)
H
b)
F
4.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
5.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
6.
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)
7.
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
8.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
9.
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
10.
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.
11.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
12.
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. 
13.
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
14.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
15.
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.
16.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
17.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

18.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
19.
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 
20.
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
21.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
22.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
23.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

24.

What element is the most electronegative

a)

chlorine

b)

bromine

c)

iodine

d)

astatine

25.

What element is the LEAST electronegative

a)

cadmium (Cd)

b)

antimony (Sb)

c)

Zirconium (Zr)

d)

Strontium (Sr)

26.

What metal is most reactive

a)

lithium

b)

sodium

c)

potassium

d)

rubidium

27.

What non-metal is the most reactive

a)

iodine

b)

sulfur

c)

oxygen

d)

fluorine

28.
Which atom has the largest atomic radius?
a)
Potassium (K)
b)
Rubidium (Rb)
c)
Francium (Fr)
d)
Cesium (Cs)
29.
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
30.

How many peaks would be expected for a PES spectum for Calcium?

a)

2

b)

3

c)

4

d)

5

31.

Which of these elements would have the same number of PES peaks as Fluorine?

a)

Neon

b)

Beryllium

c)

Sodium

d)

Chlorine

32.

The PES spectrum below is for the element _______________.

a)

O

b)

Ne

c)

N

d)

F

33.

Examine the spectrum below. Where would you expect the 2p peak for F be if it were on the same spectrum?

a)

To the left of the peak at 3.04

b)

To the right of the peak at 3.04

c)

To the left of the peak at 1.31

d)

To the right of the peak at 1.31

34.

What does the 4th peak from the left represent?

a)

The 2s electrons

b)

The 3d electrons

c)

The 2p electrons

d)

The 3s electrons

35.

Which electrons would be easiest to remove according to the spectrum below?

a)

The ones in the peak at 151

b)

The ones in the peak at 7.9

c)

The ones in the peak at 1.09

d)

The ones in the peak at 0.58

36.

Which peak (or peaks) correspond to the valence electrons?

a)

The peak at 1

b)

The peaks at 1 and 2.05

c)

The peak at 239

d)

The peaks at 239 and 22.7

37.

How many valence electrons does the element pictured in the PES spectrum below have?

a)

1

b)

2

c)

3

d)

4

38.

Where would you expect the 2s peak for Sodium to fall relative to the presented spectrum of a different element below?

a)

Just to the left of the peak at 126

b)

Just to the right of the peak at 126

c)

Just to the left of the peak at 9.07

d)

Just to the right of the peak at 9.07

39.

Which peak (or peaks) correspond to valence electrons?

a)

The peak at 0.8

b)

The peaks at 0.8 and 1.36

c)

The peak at 19.3

d)

The peaks at 19.3 and 1.36

40.

Which element has the electron configuration 1s22s22p63s23p5?

a)

chlorine

b)

fluorine

c)

sulfur

d)

phosphorus

41.

How many peaks would you see for the PES graph for the element with an electron configuration of 1s22s22p63s1

a)

2

b)

3

c)

4

d)

5

42.

What is the electron configuration for this PES graph?

a)

1s22s22p63s23p2

b)

1s22s22p63s23p1

c)

1s22s22p63s23p3

d)

1s22s22p63s2

43.

Researchers from the planet Zorba have discovered an atom with the following electron structure (shown as a shell model). Sketch the photoelectron spectrum that the researchers analyzed to obtain this knowledge of atomic structure.

a)

1s32s12p63s3

b)

1s32s12p43s3

c)

1s22s22p63s23p1

d)

1s22s22p63s2

44.

For the highlighted group, what is charge of ion formed?

a)

1-

b)

2-

c)

1+

d)

2+

e)

3+

45.

For the highlighted group, what is charge of ion formed?

a)

1+

b)

1-

c)

2+

d)

2-

e)

3+

46.

For the highlighted group, what is charge of ion formed?

a)

1+

b)

1-

c)

2+

d)

2-

e)

3-

47.

For the highlighted group, what is charge of ion formed?

a)

1+

b)

2+

c)

1-

d)

2-

e)

3+

48.

For the highlighted group, what is charge of ion formed?

a)

1-

b)

2-

c)

3-

d)

2+

e)

3+

49.

For the highlighted group, what is charge of ion formed?

a)

1-

b)

2-

c)

3-

d)

2+

e)

3+

50.
If an atom has 3 valence electrons, what charge will it have as an ion?
a)
+3
b)
-3
c)
+5
d)
-5
51.
If an atom gains 3 electrons, what charge will it have as an ion?
a)
+3
b)
-3
c)
+5
d)
-5
52.
How many valence electrons does a Sulfur atom have?
a)
2
b)
4
c)
6
d)
7
53.
If an element gains 2 electrons, what charge will it have when it becomes an ion?
a)
+2
b)
-2
c)
-6
d)
-6
54.
If an atom loses 2 valence electrons, what charge will it have as an ion?
a)
+2
b)
-2
c)
0
d)
+8
55.
What charge will a Beryllium ion have?
a)
+
b)
2+
c)
2-
d)
-
56.
anions are _____ ions.
a)
positive
b)
negative
c)
neutral
57.
What charge will a nitride ion have?
a)
3+
b)
2+
c)
2-
d)
3-
58.
How many valence electrons does magnesium have?
a)
1
b)
2
c)
12
d)
24
59.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
60.
Why are ions charged particles?
a)
The number of electrons does not equal the number of protons.
b)
The number of protons does not equal the number of neutrons.
c)
The number of neutrons does not equal the number of electrons.
d)
The electric charges of the electrons and protons cancel each other out.
61.

Negative ions are called ____________________.

a)

Cations

b)

Anions

c)

Negions

d)

Electrons

62.

The element "Na" tends to _________ when it becomes an ion.

a)

lose 1 electron

b)

gain 2 electrons

c)

lose 3 electrons

d)

gain 3 electrons

63.

Which noble gas does Aluminum want to have the same number of electrons as?

a)

He

b)

Ne

c)

Ar

d)

Kr

64.

When a neutral atom of oxygen becomes an ion it will ___________ to have the same number of electrons as __________ and have a charge of _______.

a)

gain 2e-, neon, 2+

b)

gain 2e-, neon, 2-

c)

lose 6e-, helium, 6-

d)

lose 6e-, helium, 6+

65.
A potassium ion has a charge of 1+. A sulfide ion has a charge of 2-. What is the chemical formula for potassium sulfide?
a)
CS
b)
KS
c)
K1 S
d)
K2 S
66.
How many elements make up this compound?
a)
6
b)
4
c)
2
d)
3
67.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
68.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
69.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
70.
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
71.
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.
72.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
73.

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.

74.
Which periodic group has the smallest atomic radius?
a)

Alkali metals (Group 1)

b)

Halogens (Group 17)

c)

Noble Gases (Group 18)

d)

Transition metals (middle of table)

75.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
76.
The more protons there are, the  ____ .
a)

Weaker the pull by the protons

b)
Smaller the electrons
c)

Stronger the pull by the protons

d)
The bigger the electrons
77.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
78.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
79.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
80.

Put the following in order of increasing ionization energy:Neon (Ne), Lithium (Li), Carbon (C)

a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon
81.

Put the following in order of increasing ionization energy: Sodium (Na), Oxygen (O), Boron (B)

a)
Sodium, Boron, Oxygen
b)
Oxygen, Boron, Sodium
c)
Sodium, Oxygen, Boron
d)
Oxygen, Sodium, Boron
82.
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
83.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
84.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

c)

antimony (Sb)

d)

Aluminum (Al)

85.

Which element has the lowest ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

c)

Fluorine (F)

d)

Bromine (Br)

86.
Which element has the greater ionization energy?
a)

Lead (Pb)

b)

Silicon (Si)

c)

Tin (Sn)

d)

Germanium (Ge)

87.
Which of these elements has the highest ionization energy?
a)
Lithium (Li)
b)
Potassium (K)
c)
Francium (Fr)
d)
Sodium (Na)
88.
Which of these elements has the lowest ionization energy?
a)
Oxygen (O)
b)
Boron (B)
c)
Carbon (C)
d)
Fluorine (F)
89.

Across a period, Ionization energy ____a____

Down a group, ionisation energy ____b_____

a)

a: increase

b: decrease

b)

a: increase

b: increase

c)

a: decrease

b: decrease

d)

a: decrease

b: increase

90.

When an atom gains an electron, the size of atom

a)

will increase

b)

will decrease

c)

will not change

91.

When an atom loses an electron the size of atom

a)

will increase

b)

will decrease

c)

will not change

92.

Cations have atomic radii that are larger than their atomic radii.

a)

True

b)

False

93.

Anions have atomic radii that are larger than their ionic radii.

a)

True

b)

False

94.

Select the element with the largest atomic radius

a)

Potassium

b)

Scandium

c)

Gallium

d)

Arsenic

95.

Select the element most likely to lose an electron

a)

Magnesium

b)

Sulfur

c)

Barium

d)

Oxygen

96.

Select the sequence that correctly orders from smallest to largest atomic radius

a)

Sn, Y, Ru

b)

Cu, Ga, Br

c)

Al, S, Na

d)

F, N, Li

97.

Where on the periodic table can nonmetals be found?

a)

Top

b)

Bottom

c)

Left

d)

Right

98.

Select the element with the highest ionization energy

a)

Sodium

b)

Aluminum

c)

Phosphorous

d)

Chlorine

99.

Select the element Alkali Earth Metal found in Period 4

a)

Calcium

b)

Potassium

c)

Titantium

d)

Krypton

100.

Select the element with the largest atomic radius

a)

Cesium

b)

Lithium

c)

Hydrogen

d)

Potassium

101.

Select the element with the highest electronegativity

a)

Chlorine

b)

Silicon

c)

Argon

d)

Magnesium

102.

Select the sequence of increasing electronegativity.

a)

Sn, Ag, I

b)

I, Sn, Ag

c)

Ag, Sn, I

d)

Sn, I, Ag

103.

Select the element with the lowest ionization energy.

a)

Barium

b)

Beryllium

c)

Magnesium

d)

Strontium

104.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

105.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
106.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
107.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
108.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

109.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

110.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

111.

Atomic radius DECREASES when

a)

when you go across a row from right to left

b)

when you go down a group

c)

when you go across a row from left to right

d)

when you go across a group from left to right

112.

Ionization energy ________________ as you go DOWN a group

a)

increases

b)

decreases

113.

Which atom has smaller ionization energy

a)

strontium

b)

iodine

114.

According to the periodic table what element is in group 9 period 4?

a)

Hydrogen

b)

Magnesium

c)

Cobalt

d)

Sulfur

115.

According to the periodic table what element is in group 7 period 4?

a)

Hydrogen

b)

Manganese

c)

Plutonium

d)

Nitrogen

116.

According to the periodic table what element is in group 1 period 1?

a)

Hydrogen

b)

Manganese

c)

Oxygen

d)

Nitrogen

117.

How many valence electrons do group 16 elements have?

a)

2

b)

4

c)

6

d)

8

118.

How many valence electrons do group 1 elements have?

a)

1

b)

2

c)

3

d)

8

119.

Which of the following is not a metal?

a)

H

b)

K

c)

Cu

d)

Fe

120.

How do we identify metals on the periodic table?

a)

they are all on the right hand side

b)

They are to the left of the staircase line

c)

They are in group 18

d)

They are all in period 3

121.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

122.

I am a metal


I am in group 2


I am in period 6


I am…

a)

Mo

b)

Re

c)

S

d)

Ba

123.

I am a nonmetal


I am in period 2


I am in group 16/6A

a)

Ba

b)

Si

c)

Ba

d)

O

124.

What are the three main groups of the periodic table?

a)

groups

b)

metal

c)

nonmetals

d)

metalloids

e)

periods

125.

Is Ra a metal or nonmetal or metalloid?

a)

metal

b)

nonmetal

c)

metalloid

126.

Is Sulfur a metal or nonmetal or metalloid?

a)

metal

b)

nonmetal

c)

metalloid

127.

Outermost energy level of an atom.

a)

blocks

b)

valence electron

c)

electron configuration

d)

group no.

128.

The electron configuration of Na is _______.

a)

3s1

b)

2p1

c)

3s2

d)

2p4

129.

The least reactive element listed is __________.

a)

Hydrogen

b)

Magnesium

c)

Helium

d)

Calcium

130.

Nitrogen and phosphorus are

a)

Non metals

b)

Metals

c)

Metalloids

d)

None of the above

131.

P-block elements are those elements in which last electron enters in

a)

P ortibal

b)

S orbital

c)

d orbital

d)

None of the above

132.

Which block of elements are known as transition elements?

a)

p-block

b)

s-block

c)

d-block

d)

f-block

133.

Which of the blocks on the periodic table contains the most elements?

a)

s block

b)

p block

c)

d block

d)

f block

134.

What element has this electron configuration?

a)

hydrogen

b)

helium

c)

lithium

d)

beryllium

135.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

136.

What element has this electron configuration?

a)

helium

b)

lithium

c)

beryllium

d)

boron

137.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

138.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

139.

Which element is represented by this electron configuration?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

140.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

141.

Which of the following is the electron configuration for Fluorine

a)
b)
c)
d)
142.

Which of the following is the electron configuration for neon?

a)
b)
c)
d)
143.

Which of the following is the electron configuration for silicon?

a)
b)
c)
d)
144.

Which of the following is the orbital notation for oxygen?

a)
b)
c)
d)
145.
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
146.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
147.

What is the element?

a)

Neon

b)

Chlorine

c)

Aluminum

d)

Argon

148.

What is the element?

a)

sulfur

b)

chlorine

c)

phosphorus

d)

silicon

149.

Which is the electron configuration for beryllium?

a)
b)
c)
d)
150.

Choose the correct electron configuration for Beryllium (Be).

a)

1s1

b)

1s2 2s2

c)

1s2 2s2 2p1

151.

Choose the correct electron configuration for Chlorine (Cl).

a)

1s2 2s2 2p1

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 3p5

152.

Choose the correct electron configuration for Nickel (Ni).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

b)

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

c)

1s2 2s2 2p6 3s2 3p6 4s10

153.

Choose the correct electron configuration for Krypton (Kr).

a)

1s2 2s2 2p6 3s2 3p6 4s8 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p3

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p6

154.

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

a)

Ca+2

b)

Ca

c)

Mg

d)

Na

e)

Ar

155.

What is the configuration for Carbon?

a)

1s2 2p2

b)

1s2 2s2 2p2

c)

1s1 1s2 2s2 2p2

156.

1s2 2s2 is which element?

a)

Lithium

b)

Beryllium

c)

Helium

d)

Boron

157.

Iron (Fe) configuration is

a)

1s2 2s2 2p6 3s2 3p3

b)

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

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

d)

1s2 2s2 2p6 3s2 3p6 4s2 4d6

158.

Which element is 1s2 2s2 2p6 3s2 3p6 4s2 3d7?

a)

Cobalt

b)

Nickel

c)

Manganese

d)

Chromium

159.

Write the configuration for Oxygen

a)

1s2 2s2 1p4

b)

2s2 2p4

c)

1s2 2s2 3p4

d)

1s2 2s2 2p4

160.

Write the configuration for Phosphorus

a)

2s2 2p6 3s2 3p3

b)

1s2 2s3 2p6 3p3

c)

1s2 2s2 2p6 3s2 3p3

d)

1s2 2s2 2p5 3s2 3p3

161.

Which element is 1s2 2s2 2p6 3s2 3p6 4s1?

a)

Sodium (Na)

b)

Lithium (Li)

c)

Potassium (K)

d)

Calcium (Ca)

162.

Choose the correct configuration for Zinc

a)

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

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d9

c)

1s2 2s2 2p6 3s2 3p6 3s2 3d10

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

163.

Choose the correct element for 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

a)

Chlorine

b)

Bromine

c)

Krypton

d)

Sulfur

164.

Choose the correct configuration for Neon (Ne).

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6

d)

1s2 2s1 2p6

165.

How many peaks would be expected for a PES spectum for Calcium?

a)

2

b)

3

c)

4

d)

5

166.

Which of these elements would have the same number of PES peaks as Fluorine?

a)

Neon

b)

Beryllium

c)

Sodium

d)

Chlorine

167.

The PES spectrum below is for the element _______________.

a)

O

b)

Ne

c)

N

d)

F

168.

Examine the spectrum below. Where would you expect the 2p peak for F be if it were on the same spectrum?

a)

To the left of the peak at 3.04

b)

To the right of the peak at 3.04

c)

To the left of the peak at 1.31

d)

To the right of the peak at 1.31

169.

What does the 4th peak from the left represent?

a)

The 2s electrons

b)

The 3d electrons

c)

The 2p electrons

d)

The 3s electrons

170.

Which electrons would be ejected with the most kinetic energy according to the spectrum below?

a)

The ones in the peak at 151

b)

The ones in the peak at 7.9

c)

The ones in the peak at 1.09

d)

The ones in the peak at 0.58

171.

Which peak (or peaks) correspond to the valence electrons?

a)

The peak at 1

b)

The peaks at 1 and 2.05

c)

The peak at 239

d)

The peaks at 239 and 22.7

172.

How many valence electrons does the element pictured in the PES spectrum below have?

a)

1

b)

2

c)

3

d)

4

173.

Where would you expect the 2s peak for Sodium to fall relative to the presented spectrum of a different element below?

a)

Just to the left of the peak at 126

b)

Just to the right of the peak at 126

c)

Just to the left of the peak at 9.07

d)

Just to the right of the peak at 9.07

174.

Which peak (or peaks) correspond to valence electrons?

a)

The peak at 0.8

b)

The peaks at 0.8 and 1.36

c)

The peak at 19.3

d)

The peaks at 19.3 and 1.36

175.

Atomic radius _________ across a period because of the increasing number of _________ in the atom.

a)

Increases, energy levels

b)

Increases, electrons

c)

Decreases, electrons

d)

Decreases, protons

e)

Increases, protons

176.

Atomic radius _________ down a group because of the increasing number of _________ in the atom.

a)

Increases, energy levels

b)

Increases, electrons

c)

Decreases, electrons

d)

Decreases, protons

e)

Increases, protons

177.
Coulombic Attraction is the attraction between __________ charged particles.
a)
same 
b)
oppositely
c)
two positively
d)
two negatively
178.
An example of Coulombic Attraction in an atom is between
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
protons and protons
179.
As the distance between protons and electrons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is not affected
180.
If distance remains the same, as the number of protons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is divided by 1/2
181.
What are the two variables that affect Coulombic Attraction?
a)
Distance  and number of protons
b)
Number of neutrons and number of protons
c)
Number of neutrons and number of electrons
d)
solids or liquids
182.

Looking at atoms in the same group/family (column), what factor most greatly affects Coulombic attraction?

a)

number of protons

b)

distance from the nucleus

c)

moles of atoms

d)

number of neutrons

183.

What is the trend in Coulombic attraction going down a group?

a)

Coulombic attraction increases moving down a group.

b)

Coulombic attraction decreases moving down a group.

184.

What is the trend in Coulombic attraction moving from left to right across a period?

a)

Coulombic attraction increases moving from left to right across a period.

b)

Coulombic attraction decreases moving from left to right across a period.

185.

Select the element that has the strongest Coulombic attraction.

a)

O

b)

S

c)

Se

d)

Te

186.

Select the element that has the strongest Coulombic attraction.

a)

O

b)

F

c)

N

d)

C

187.

Select the element that has the strongest Coulombic attraction.

a)

Fe

b)

Mn

c)

Zn

d)

Sc

188.

Select the element that has the strongest Coulombic attraction.

a)

Li

b)

Na

c)

Rb

d)

Cs

189.

What are the two variables that affect Coulombic Attraction?

a)

Distance and number of protons

b)

Number of neutrons and number of protons

c)

Number of neutrons and number of electrons

d)

Distance and number of neutrons

190.

What is the trend in Coulombic attraction moving from left to right across a period?

a)

Coulombic attraction increases moving from left to right across a period.

b)

Coulombic attraction decreases moving from left to right across a period.

c)

No trend can be observed.

d)

The trend depends upon which period is being observed.

191.

What is the trend in Coulombic attraction going down a group?

a)

Coulombic attraction increases moving down a group.

b)

Coulombic attraction decreases moving down a group.

c)

No trend can be observed.

d)

The trend depends upon which group is being observed.

192.

Which of the following will have similar properties?

a)

O, S, Se

b)

O, F, Ne

c)

N, Ne, Na

d)

H, K, P

193.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
194.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
195.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

196.

Elements in the same group have : (2 correct answers)

a)

Similar chemical properties

b)

Similar names

c)

Same number of outer (valence) electrons)

d)

The same number of protons

197.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
198.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
199.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
200.

Match the following elements to the group they belong to.

a)

sodium

1.

alkali metal

b)

calcium

2.

alkaline earth metal

c)

chlorine

3.

halogen

d)

argon

4.

noble gas

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