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chemistry revision

Total questions: 219

Worksheet time: 5hrs 33mins

Name
Class
Date
1.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
2.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

3.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
4.

What will be the charge of a bromine ion?

a)

+7

b)

-7

c)

-1

d)

+1

5.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
6.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
7.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
8.

Ionic bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

Depends on the situation

9.

Covalent bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

It depends on the situation

10.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
11.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

12.
What type of bond forms when atoms share electrons?
a)
Ionic Bond
b)
Covalent Bond
c)
Metallic Bond
d)
Gold Bond Medicated Powder
13.

What is a covalent bond?

a)

A bond between atoms where electrons are shared.

b)

A bond between atoms where one atom gains an electron and another loses an electron.

c)

A bond where electrons dance in a 123 pattern.

d)

A bond between two atoms where they send each other special BFF messages.

14.

Hydrogen atoms come together to form a _________________

a)

Dancing bear

b)

Hydrogen molecule

c)

Carina molecule

d)

Artemis molecule

15.

An atom with 1 valence electron 'needs' a full shell, so it can either gain 7 electrons or lose 1. Which is more likely to occur?

a)

lose 1 electron

b)

gain 7 electrons

16.

What two types of atoms make a covalent bond?

a)

metal atom and metal atom

b)

metal atom and non metal non atom

c)

non metal atom and non metal atom

17.

When an atom loses an electron, it becomes a _________.

a)

noble gas

b)

anion

c)

cation

18.

How many valence electrons does hydrogen have?

a)

1

b)

2

c)

3

d)

4

19.

Low melting point and low solubility in water are general properties of ______________________ compounds

a)

ionic

b)

covalent

c)

all

20.

Where are the non-metals located on the periodic table?

a)

all over

b)

On the left side of the "staircase"

c)

On the right side of the "staircase"

21.

Which of the following describe ionic bonding?

a)

It involves the transfer of electrons

b)

It involves sharing of electrons.

c)

It involves transfer of protons.

d)

It involves sharing of protons.

22.

From the periodic table, which pair of elements can combine to form ionic bonds?

a)

Ca and O

b)

H and N

c)

H and Cl

d)

Xe and Fe

23.

Bond that is formed when electrons are equally shared.

a)

non polar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

metallic bond

24.

Which of the following pairs of atoms is most likely to form a covalent compound?

a)

Ba and Cl

b)

Na and O

c)

Mg and Br

d)

C and O

25.

What is the chemical formula of Sulfur Hexafluoride?

a)

S6F

b)

S6F6

c)

SF6

d)

6SF

26.

Which of the following is a correct lewis structure for carbon dioxide CO2?

a)
b)
c)
d)
27.

7. Covalent compounds:

a)

Share electrons

b)

Transfer electrons

c)

Neither

28.

8. What happens when an atom loses an electron?

a)

Neutral (no charge)

b)

Positive Charge

c)

Negative Charge

29.

9. What happens when an atom gains an electron?

a)

Neutral (no charge)

b)

Positive Charge

c)

Negative Charge

30.

12. What elements generally make an ionic bond?

a)

metal and nonmetal

b)

2 or more nonmetals

c)

metal

d)

none of the above

31.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
32.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
33.

What is a non-polar covalent bond?

a)

transfer of electrons

b)

is a bond where electrons are shifted to the more electronegative atom

c)

Sea of electrons

d)

is a bond where electrons are shared equally

34.
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
35.
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.
36.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
37.
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. 
38.

As you look down a group, electronegativity

a)

increases

b)

decreases

39.

As you look from left to right across a period, electronegativity

a)

increases

b)

decreases

40.
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
41.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

42.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

43.
Which has the greater EN: 
H or F?
a)
H
b)
F
44.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
45.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
46.
Rows on the period table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
47.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
48.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
49.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
50.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
51.
The number of valence electrons in an element affects the reactivity of that element. Which element listed has the fewest valence electrons?
a)
beryllium (Be)
b)
sodium (Na) 
c)
oxygen (O) 
d)
neon (Ne)
52.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
53.
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. 
54.
What is the name of Groups 18?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Halogens
d)
Noble Gases
55.
Where are the metals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
56.
Where are the nonmetals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
57.
In what state of matter are most of the nonmetals?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
58.
What does the atomic number of an atom represent?
a)
Number of neutrons in the atom
b)
Number of protons in the atom
c)
Number of electrons in the atom
d)
Number of shells in the atom
59.

How many PROTONS does Silicon have?

a)

14

b)

28

c)

42

60.

Which of the following elements is most likely to have similar properties to those of sodium (Na)?

a)

Magnesium (Mg)

b)

Sulfur (S)

c)

Francium (Fr)

d)

Titanium (Ti)

61.

In which group would an element that is not reactive most likely be located?

a)

1

b)

2

c)

16

d)

18

62.

In which group would an element that is very reactive most likely be located?

a)

1

b)

5

c)

15

d)

18

63.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

64.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
65.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

66.
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
67.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
68.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
69.

What happens to the atomic numbers as you move from left to right on the periodic table?

a)

Increase

b)

Decrease

c)

Stay the same

d)

Nothing

70.

Which of the following elements is most likely to have similar properties to those of sodium (Na)?

a)

Magnesium (Mg)

b)

Sulfur (S)

c)

Francium (Fr)

d)

Titanium (Ti)

71.

Which element is most likely to have six valence electrons?

a)

Barium (Ba)

b)

Carbon (C)

c)

Oxygen (O)

d)

Americium (Am)

72.

Which element is located in period 4 and group 5?

a)

Vanadium (V)

b)

Zirconium (Zr)

c)

Niobium (Nb)

d)

Titanium (Ti)

73.

In which group would an element that is very reactive most likely be located?

a)

1

b)

5

c)

15

d)

18

74.
Is this a metal, nonmetal or metalloid?
a)
Metal
b)
Nonmetal
c)
Metalloid
75.
Which of these elements has an electron structure most similar to that of element X?
a)
1
b)
2
c)
3
d)
4
76.

Group 3 elements have ____ electrons in their outermost shell.

a)

1

b)

2

c)

3

d)

4

77.

The valence electrons of an atom do not experience the full attractive force of protons in the atom’s nucleus due to the presence of inner core electrons. The reduction in nuclear charge experienced by valence electrons due to inner core electrons is called the 

a)

ionization energy effect.

b)

nuclear charge effect.

c)

periodic law effect.

d)

shielding effect.

78.

Which of the following correctly completes the statement:

Cations are always _____ than the parent atom and anions are always _____ than the parent atom.    

a)

smaller; smaller

b)

larger; smaller

c)

smaller; larger

d)

larger; larger    

79.

Which characteristic is not a periodic trend?

a)

atomic radius

b)

electron affinity

c)

ionization energies

d)

number of elements in a group

80.

Which pair of words correctly completes the statement?

Alkali metals are highly ___ since they ___ easily to form ions.

a)

nonreactive; lose 1 electron

b)

nonreactive; lose 2 electrons

c)

reactive; lose 1 electron

d)

reactive; gain 1 electron

81.

In the periodic table hydrogen is placed in Group 1A and helium is placed in Group 8A. The most likely reason for this is: 

a)

Hydrogen has one outer shell electron and helium has a full outer shell of electrons.

b)

Hydrogen has one outer shell electron and helium has 8 electrons in its outer shell.

c)

Hydrogen and helium are both metals.

d)

Hydrogen and helium are both gases.

82.

The metallic character of elements _____ across a period. Metals are good conductors of ______.

a)

increases; electricity

b)

decreases; heat

c)

decreases; metalloids

d)

remains the same; luster

83.

Which of the following correctly completes the statement:

Cations are always _____ than the parent atom and anions are always _____ than the parent atom.    

a)

smaller; smaller

b)

larger; smaller

c)

smaller; larger

d)

larger; larger    

84.

Based on their definitions, electron affinity could be considered the opposite of

a)

shielding effect.

b)

ionization energy.

c)

nonmetallic character.

d)

effective nuclear charge.

85.

Which arrangement of the following Period 5 elements, from left to right, orders them with respect to their atomic size, from smallest to largest?

a)

Rb; Sr; In; Sb; Te

b)

In; Rb; Sb; Sr; Te

c)

Te; Sb; In; Sr; Rb

d)

In; Sb; Te; Rb; Sr

86.

Which pair of words correctly completes the statement?

Alkali metals are highly ___ since they ___ easily to form ions.

a)

nonreactive; lose 1 electron

b)

nonreactive; lose 2 electrons

c)

reactive; lose 1 electron

d)

reactive; gain 1 electron

87.

Select the element most likely to gain an electron

a)

Bromine

b)

Fluorine

c)

Chlorine

d)

Iodine

88.

Select the element with the largest atomic radius

a)

Potassium

b)

Scandium

c)

Gallium

d)

Arsenic

89.

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

90.

Select the group that is the most reactive metals

a)

Transition Metals

b)

Alkali Earth Metals

c)

Alkali Metals

d)

Halogens

91.

Select the element Alkali Earth Metal found in Period 4

a)

Calcium

b)

Potassium

c)

Titantium

d)

Krypton

92.

Select the element with the largest atomic radius

a)

Cesium

b)

Lithium

c)

Hydrogen

d)

Potassium

93.

Select the element with the highest electronegativity

a)

Chlorine

b)

Silicon

c)

Argon

d)

Magnesium

94.

Select the element that is a nonmetal

a)

Copper

b)

Lead

c)

Hydrogen

d)

Sodium

95.

What element is found in Group 5 period 4?

a)

Zirconium

b)

Magnesium

c)

Strontium

d)

Vanadium

96.

Select all elements that are metals

a)

Thallium

b)

Hydrogen

c)

Sulfur

d)

Argon

e)

Chromium

97.

Select the element with the lowest ionization energy.

a)

Barium

b)

Beryllium

c)

Magnesium

d)

Strontium

98.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

99.

Which element is most likely to lose an electron?

a)

Zinc

b)

Arsenic

c)

Bromine

d)

Potassium

100.

The periodic table is arranged by ______

a)

Atomic Mass

b)

Number of Electrons

c)

Atomic Number

d)

Atomic Weight

101.

The period number of an element corresponds to...

a)

The number of electrons

b)

The number of valence electrons

c)

The number of energy levels

d)

The number of protons

102.

The term valence electron refers to…

a)

The total number of electrons in an atom

b)

The electrons in the first energy level

c)

The electrons in the outermost energy level

d)

Electrons that are found in the nucleus

103.

The group number of an element corresponds to...

a)

The number of electrons

b)

The number of valence electrons

c)

The number of energy levels

d)

The number of protons

104.

Elements in Group 6 of the periodic table would have how many valence electrons?

a)

2

b)

6

c)

8

d)

Unable to tell from the given information

105.

Elements located in groups 7 & 8 tend to be classified as ________________

a)

Non-Metals

b)

Metalloids

c)

Metals

d)

Noble Gases

106.

Use the picture at right to answer the question.  Given the Lewis Dot structure, which of the following elements could the unknown (X) represent?

 X⋅X\cdot  

a)

B

b)

C

c)

K

d)

Ca

107.

Which element is located in Group 3, Period 2?

a)

Magnesium

b)

Lithium

c)

Helium

d)

Boron

108.

What is the correct electron configuration for the element Oxygen?

a)

1s2 1p4

b)

1s22s2 2p4

c)

1s22s2 2p6

d)

1s22s2 2p6

109.

Which element has the electron configuration 6s1 ?

a)

Rb

b)

Tl

c)

He

d)

Cs

110.

Which element will have the largest atomic radius?

a)

Ne

b)

Li

c)

Cs

d)

Rn

111.

Which element will have the smallest ionization energy?

a)

Ne

b)

Li

c)

Cs

d)

Rn

112.

How many dots will be needed when drawing the Lewis dot diagram for the element carbon?

a)

6

b)

4

c)

2

d)

Like, a ton, dude.

113.

What happens to the atomic numbers as you move from left to right on the periodic table?

a)

Increase

b)

Decrease

c)

Stay the same

d)

Nothing

114.

Which of the following elements is most likely to have similar properties to those of sodium (Na)?

a)

Magnesium (Mg)

b)

Sulfur (S)

c)

Francium (Fr)

d)

Titanium (Ti)

115.

If an element has 117 protons which group will it be in on the periodic table?

a)

1

b)

7

c)

11

d)

17

116.

Which element is located in group 3?

a)

Yttrium (Y)

b)

Carbon (C)

c)

Sodium (Na)

d)

Lithium (Li)

117.

Which element is located in period 4?

a)

Zirconium (Zr)

b)

Silicon (Si)

c)

Beryllium (Be)

d)

Iron (Fe)

118.

Which element is most likely to have six valence electrons?

a)

Barium (Ba)

b)

Carbon (C)

c)

Oxygen (O)

d)

Americium (Am)

119.

Which element is most likely to have three electron energy levels?

a)

Argon (Ar)

b)

Lithium (Li)

c)

Boron (B)

d)

Europium (Eu)

120.

Which element is most likely to have six electrons in its 4th energy level?

a)

Oxygen (O)

b)

Selenium (Se)

c)

Krypton (Kr)

d)

Potassium (K)

121.

In which group would an element that is not reactive most likely be located?

a)

1

b)

2

c)

16

d)

18

122.

In which group would an element that is a gas most likely be located?

a)

1

b)

3

c)

12

d)

18

123.

Which of the following elements is most likely a poor conductor of electricity?

a)

Beryllium (Be)

b)

Gold (Au)

c)

Phosphorus (P)

d)

Copper (Cu)

124.

What is the atomic mass of an element with 16 protons, 13 neutrons, and 16 electrons?

a)

13 amu

b)

16 amu

c)

29 amu

d)

45 amu

125.

How many neutrons are located in the nucleus of an atom that has 12 protons, 12 electrons, and an atomic mass of 28 amu?

a)

12

b)

16

c)

28

d)

40

126.

The distance between nucleus and outermost shell occupied electron

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

127.

The energy it takes to remove one electron from an atom

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

128.

The tendency of an atom to attract a shared pair of electrons

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

129.

The amount of energy released when an electron is added to a neutral atom to form a negative ion

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

130.

The degree of oxidation (loss of electrons) of an atom in a chemical compound

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

131.

Which element has higher ionization energy?

a)

Chlorine is higher than Sodium

b)

Phosphorus is higher than Nitrogen

c)

Silicon is higher than Carbon

d)

Magnesium is higher than Aluminium

132.

Which element has lower ionization energy?

a)

Chlorine is lower than Sodium

b)

Phosphorus is lower than Nitrogen

c)

Carbon is lower than Silicon

d)

Aluminium is lower than Magnesium

133.

Which element has higher electron affinity?

a)

Bromine is higher than Calsium

b)

Chlorine is higher than Fluorine

c)

Magnesium is higher than Beryllium

d)

Sodium is higher than Aluminium

134.

Which element has lower electron affinity?

a)

Bromine is lower than Calsium

b)

Chlorine is lower than Fluorine

c)

Berylliumis lower than Magnesium

d)

Aluminium is lower than Sodium

135.

Which element is more metallic?

a)

Sodium is more metallic than Aluminium

b)

Fluorine is more metallic than Beryllium

c)

Potassium is more metallic than Lithium

d)

Chlorine is more metallic than Silicon

136.

Which element is less metallic?

a)

Sodium is less metallic than Aluminium

b)

Beryllium is less metallic than Fluorine

c)

Lithium is less metallic than Potassium

d)

Chlorine is less metallic than Silicon

137.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
138.
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
139.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
140.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
141.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
142.
What type of elements touch the zigzag line?
a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Solids

143.
Where are the nonmetals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
144.
What does the atomic number of an atom represent?
a)
Number of neutrons in the atom
b)
Number of protons in the atom
c)
Number of electrons in the atom
d)
Number of shells in the atom
145.

How many NEUTRONS does an atom of Chlorine have?

a)

17

b)

18

c)

19

d)

35

146.

Where on the periodic table can nonmetals be found?

a)

Top

b)

Bottom

c)

Left

d)

Right

147.

Select the element Alkali Earth Metal found in Period 4

a)

Calcium

b)

Potassium

c)

Titantium

d)

Krypton

148.

Select the element that is a metalloid

a)

Gallium

b)

Boron

c)

Oxygen

d)

Magnesium

149.

Select the element that has 3 valence electrons

a)

Calcium

b)

Sodium

c)

Aluminum

d)

Sulfur

150.

Select the element that is a nonmetal

a)

Copper

b)

Lead

c)

Hydrogen

d)

Sodium

151.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

152.

Definition of ionization energy is

a)

The energy required to remove an electron

b)

The energy required to add an electron

c)

The ability to attract an electron

d)

The distance from the nucleus to the outermost electron

153.

Which of the following elements will most likely form cations?

a)

Oxygen

b)

Iodine

c)

Magnesium

d)

Sulfur

154.

Which of the following scientist is credited arranging the periodic table according to Atomic Mass?

a)

Mendeleev

b)

Dalton

c)

Ramsay

d)

Seaborg

155.

According to the Octet Rule, to achieve stability atoms attempt to fill the outer S and P orbitals. How many electrons are required to accomplish this?

a)

2

b)

4

c)

6

d)

8

156.

Which of the following Groups on the Periodic Table has the lowest Electronegativity?

a)

Group 1

b)

Group 2

c)

Group 16

d)

Group 17

157.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
158.
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.
159.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
160.
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)
161.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
162.
Is this a metal, nonmetal or metalloid?
a)
Metal
b)
Nonmetal
c)
Metalloid
163.
Atomic Radius is...
a)
the relative size of the atom's nucleus
b)
the relative size of the atom's electron cloud
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
164.

Rank the following in order of increasing reactivity: Ge, K, Br, Ca (lowest to highest reactivity)

a)

Ge, K, Br, Ca

b)

K, Br, Ge, Ca

c)

Br, Ge, Ca, K

d)

Br, Ca, Ge, K

165.

The metals are located

a)

to the left of the stair step.

b)

to the right of the stair step.

c)

on and around the stair step.

166.

The metalloids are located

a)

to the left of the stair step.

b)

to the right of the stair step.

c)

on and around the stair step.

167.

Metals are MOSTLY _____ at room temperature.

a)

solid

b)

liquid

c)

gas

168.

Nonmetals are MOSTLY _____ at room temperature.

a)

solid

b)

liquid

c)

gas

169.

Which of the following is a metal?

a)

Calcium (Ca)

b)

Neon (Ne)

c)

Oxygen (O)

d)

Sulfur (S)

170.

Chlorine is what state of matter?

a)

solid

b)

liquid

c)

gas

171.

Nitrogen is a

a)

metal.

b)

nonmetal.

c)

metalloid.

172.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
173.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
174.
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)
175.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
176.

Most noble gases have _______ valence electrons.

a)

1

b)

2

c)

7

d)

8

177.
What is the oxidation number for Flourine (F)?
a)
+1 
b)
-1
c)
17
d)
7
178.

Rank the following in order of increasing reactivity: Ge, K, Br, Ca (lowest to highest reactivity)

a)

Ge, K, Br, Ca

b)

K, Br, Ge, Ca

c)

Br, Ge, Ca, K

d)

Br, Ca, Ge, K

179.

Group 2 on the Periodic Table contains the _____________________________. The oxidation number of these elements is _________________.

a)

alkali metals, -2

b)

alkaline earth metals, +2

c)

halogens, +1

d)

noble gases, -3

180.

The statement that an electron occupies the lowest available energy orbital is

a)

Hund's Rule

b)

AUfbau principle

c)

Bohr's law

d)

The Pauli Exclusion principle

181.

Which of the following rules requires that each of the p orbitals at a particular energy level receive one electron before any of them can have two electrons?

a)

the Pauli exclusion principle

b)

Aufbau principle

c)

Hund's rule

d)

The quantum rule

182.

The atomic sublevel with the next highest energy after 4p is

a)

4d

b)

4f

c)

5s

d)

5p

183.

In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?

a)

4s2, 3d1

b)

3d3

c)

4s3

d)

4s2 4p1

184.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
185.

What charge do electrons have?

a)

Positive

b)

Neutral

c)

Negative

186.

Which two particles are contained in the nucleus of an atom?

a)

Protons and Neutrons

b)

Protons and Electrons

c)

Electrons and Neutrons

187.
How many neutrons does a sodium atom have? (Use the image to help you)
a)
23
b)
11
c)
12
d)
34
188.
The atomic number of an element that has 9 protons, 9 electrons, and 10 neutrons is _____.
a)
9
b)
10
c)
19
d)
28
189.

The electronic configuration of 17Cl is

a)

2,8,8,1

b)

2,8,6

c)

2,8,8

d)

2,8,7

190.

Which of the following is the electronic Configuration of Sodium 11Na

a)

2,8

b)

2,8,1

c)

2,1,8

d)

8,1,2

191.

Which one of the following does not represent the electronic configuration of an atom in its ground state?

a)

1s2 2s2 2p3

b)

1s2 2s2 2p4

c)

1s2 2s2 2p6 3s1

d)

1s2 2s2 2p6 3d1

192.

Which one of the following is the electronic structure of a metal with a maximum oxidation state of +3?

a)

1s2 2s2 2p6 3s1

b)

1s2 2s2 2p6 3s2 3p4

c)

1s2 2s2 2p6 3s2 3p1

d)

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

193.

The vanadium atom (atomic number 23) in its ground state has the electronic configuration:

a)

1s2 2s2 2p6 3s2 3p6 3d3 4s2

b)

1s2 2s2 2p6 3s2 3p6 3d2 4s3

c)

1s2 2s2 2p6 3s2 3p6 3d1 4s2 4p2

d)

1s2 2s2 2p6 3s2 3p6 3d2 4s2 4p1

194.

The electron configuration of an atom is 1s22s22p61s^22s^22p^6 The number of electrons in the atom is 

a)

3

b)

5

c)

6

d)

10

195.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Pauli's Exclusion Principle

c)

Hund's Rule

d)

Heisenberg uncertainty principle

196.

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

a)

Aufbau Principle

b)

Hund’s Rule

c)

Pauli's Exclusion Principle

d)

Core Notation

197.

Which electron configuration belongs to Chlorine (Cl)?

a)

 1s22s22p63p51s^22s^22p^63p^5  

b)

 1s22s22p63s23p71s^22s^22p^63s^23p^7  

c)

 1s22s22p63s23p61s^22s^22p^63s^23p^6  

d)

 1s22s22p63s13p71s^22s^22p^63s^13p^7  

198.

What atom matches this electron configuration?

 1s22s22p63s23p64s23d101s^22s^22p^63s^23p^64s^23d^{10}  

a)

Zinc

b)

Nickel

c)

Copper

d)

Germanium

199.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

d)

Heisenberg uncertainty principle

200.

What is incorrect about this orbital diagram?

a)

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

b)

There is nothing incorrect with this diagram

c)

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

d)

All the arrows should be pointing the same direction.

201.

Which rule is violated in the following orbital diagrams?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli's Exclusion Principle

202.

Which rule is violated in the following orbital diagrams?

a)

Aufbau Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

203.

Chemists can identify the composition of some unknown salts by conducting a flame test. When potassium salts are heated in a flame, a purple color is observed.


This is due to the movement of electrons between energy levels. What is the electron configuration of a potassium atom at ground state?

a)

1s2; 2s2; 2p6; 3s2; 3p6; 4d1

b)

1s2; 2s2; 2p6; 3s2;3p6; 3d1

c)

1s2; 2s2; 2d6; 3s2; 3d6; 4s1

d)

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

204.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
205.

Which one of the following is the electronic configuration of the bromine atom?

a)

1s22s22p63s23p63d104s14p6

b)

1s22s22p63s23p63d104s24p7

c)

1s22s22p63s23p63d104s24p5

d)

1s22s22p63s23p63d104s24p6

206.

The vanadium atom (atomic number 23) in its ground state has the electronic configuration:

a)

1s2 2s2 2p6 3s2 3p6 3d3 4s2

b)

1s2 2s2 2p6 3s2 3p6 3d2 4s3

c)

1s2 2s2 2p6 3s2 3p6 3d1 4s2 4p2

d)

1s2 2s2 2p6 3s2 3p6 3d2 4s2 4p1

207.

An atom with a charge of 2- will have...

a)

2 more electrons than protons

b)

2 more neutrons than electrons

c)

2 more protons than electrons

d)

2 electrons less than protons

208.

Electronic configuration of boron

a)

1s2 3s2 2p1

b)

1s2 2s2 2p1

c)

1s2 2s5 2p1

d)

1s1 2s2 2p2

209.

Electronic configuration of Neon

a)

1s1 2s2 2p7

b)

2s2 2p2 2p6

c)

1s4 2s4 2p2

d)

1s2 2s2 2p6

210.

Which one of the following is the electronic configuration of the bromine ?

a)

A. [Ar]4s23d104p5

b)

B. 1s22s22p63s23p5

c)

C. 1s22s22p63s23p64s24p5

d)

D. [Ar]3s23d103p5

211.

What is the electron configuration of a copper atom?

a)

A. 1s22s22p63s23p63d9

b)

B. 1s22s22p63s23p64s13d10

c)

C. 1s22s22p63s23p64s23d9

d)

D. 1s22s22p63s23p64s23d10

212.

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

213.

Which one of the following contains no unpaired electrons in the ground state?

a)

Be

b)

F

c)

Si

d)

N

214.

What is the electron configuration of a copper atom (Z= 29)?

a)

A. 1s22s22p63s23p63d9

b)

B. 1s22s22p63s23p64s13d10

c)

C. 1s22s22p63s23p64s23d9

d)

D. 1s22s22p63s23p64s23d10

215.

Which of the following is the electronic configuration for Mg2+ ion? (Z=12)

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p2

d)

1s2 2s2 2p6 3s2

216.
FIND THE ELECTRONIC CONFIGURATION OF Cl (At no = 17)
a)
2,8,7
b)
2,8,8
c)
2,8,6
d)
2,8
217.
Ar (18)
a)
2,8,7
b)
2,8,8
c)
2,8,6
d)
2,8,5
218.
Mg (12)
a)
2,8,2
b)
2,8,6
c)
2,6
d)
2,7
219.
N (7)
a)
2,2
b)
2,3
c)
2,4
d)
2,5