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Periodic Table Practice

Total questions: 192

Worksheet time: 4hrs 50mins

Name
Class
Date
1.

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

a)

Rutherford

b)

Dalton

c)

Mendeleev

d)

Moseley

2.

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

a)

Rutherford

b)

Thomson

c)

Mendeleev

d)

Moseley

3.

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.

4.

Which class of elements are malleable, ductile, shiny when clean and polished, good conductors of heat and electricity, and reacts with acids to form hydrogen gas?

a)

metals

b)

nonmetals

c)

metalloids

d)

ions

5.

What is the name of Group 1 elements?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Halogens

6.

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

7.

What is an atom or bonded group of atoms that has a positive or negative charge?

a)

ion

b)

atom

c)

metal

d)

nonmetal

8.

What is the term of an atom that will lose electron(s) and have a positive change?

a)

cation

b)

anion

c)

electronegativity

d)

ionic radius

9.

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.

10.

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.

11.

Which element has the smallest atomic radius?

a)

magnesium

b)

chlorine

c)

bromine

d)

argon

12.

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.

13.

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.

14.

Which element has the highest ionization energy?

a)

oxygen

b)

sulfur

c)

silicon

d)

potassium

15.

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

16.

Which element has the largest electronegativity?

a)

barium

b)

oxygen

c)

iron

d)

lithium

17.

Mendeleev was the first person to arrange the elements into a table. How did he arrange the rows?

a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
18.

Which of the following will have similar properties?

a)

O, S, Se

b)

O, F, Ne

c)

N, Ne, Na

d)

H, K, P

19.

Moseley arranged what we know as the "modern periodic table". How did he arrange it?

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

20.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
21.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
22.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
23.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

24.

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

25.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
26.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
27.

Name this group: These metals contain familiar metals such as gold, iron, and copper.

a)
b)
c)
d)
28.

Find an element with similar chemical properties to Barium (Ba).

a)

Ca an Ra, because they are in the same group and have similar chemical properties.

b)

Cs and La, b/c they are in the same period number.

c)

Ca and Y, b/c they are 90 degree angle and have similiar properties.

29.
a)
Same group
b)
Same period
30.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
31.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
32.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
33.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
34.

What do the periods (rows) represent?

a)

an additional energy level

b)

an additional proton

c)

an additional group

d)

an additional electron

35.

Put the groups of the periodic table in order from group 1A to group 8A (18).

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

1)
2)
3)
4)
36.

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

37.

Match the following

a)

lithium

1.

2 energy levels

b)

helium

2.

1 energy level

c)

aluminum

3.

3 energy levels

d)

bromine

4.

4 energy levels

e)

strontium

5.

5 energy levels

38.

Mendeleev & Moseley both organized the columns (groups) by...

a)

mass

b)

number

c)

symbol

d)

properties

39.

Element symbols have _____ capital letter(s).

a)

1

b)

2

c)

3

d)

4

40.

Compound formulas have ____ capital letter(s).

a)

1

b)

2

c)

3

d)

more than 1

41.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

42.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

43.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

44.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

45.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

46.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

47.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

48.
___________ is the only metal that is a liquid at room temperature.
a)
Platinum
b)
Water
c)
Tin
d)
Mercury
49.
__________ would have some characteristics of metals and some characteristics of nonmetals.
a)
Gold
b)
Sodium
c)
Arsenic
d)
Bismuth
50.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

51.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

52.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

53.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

54.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

55.

Elements that have the same number of energy levels are said to be in the same ______.

a)

group

b)

period

c)

family

d)

classification

56.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

57.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

58.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

59.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

60.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

61.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

62.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

63.
__________ would have some characteristics of metals and some characteristics of nonmetals.
a)
Gold
b)
Sodium
c)
Arsenic
d)
Bismuth
64.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

65.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

66.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

67.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

68.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

69.

Elements that have the same number of energy levels are said to be in the same ______.

a)

group

b)

period

c)

family

d)

classification

70.
How many "valance electrons" are in chlorine?
a)
7
b)
2
c)
17
d)
8
71.
How many Protons does Bromine have?
a)
45
b)
79.904
c)
80
d)
35
72.
How many Neutrons does Bromine have?
a)
35
b)
80
c)
45
d)
79.905
73.
A particle with a negative charge inside of an element is called
a)
isotope
b)
neutron
c)
proton
d)
electron
74.
Does this carbon have the correct amount of electrons?
a)
Yes
b)
No, it needs one more
c)
No, it needs two more
d)
No, it needs three more
75.
Nitrogen has 5 valence electrons
a)
True
b)
False, it has 7
c)
False, it has 14
d)
False, it has 7.01
76.
An isotope has...
a)
the same number of protons but different number of electrons
b)
same number of protons but different number of neutrons
c)
same number of electrons and neutrons
d)
same number of electrons, protons, and neutrons
77.
Elements that are gases, brittle, and not conductive are
a)
Metals
b)
Metalloids
c)
Transition Metals
d)
Non-metals
78.
Not non-metals or metals but somewhere in between
a)
noble gases
b)
isotopes
c)
metalloids
d)
ions
79.
Is this Lewis Dot Structure correct
a)
Yes
b)
No, chlorine has 6 valence
c)
No, chlorine has 8 valence
d)
No, chlorine has 17 electrons
80.
How many electrons are in the following chlorine atom?
a)
7
b)
8
c)
17
d)
13
81.
What is titanium's atomic mass?
a)
47.867
b)
22
c)
26
d)
49
82.
The atomic mass of Boron is 10.81, which means Boron has..
a)
5 electrons and 6 protons, each weigh 1 amu
b)
5 neutrons and 6 electrons, each weigh 1 amu
c)
6 neutrons and 5 protons, each weigh 1 amu
d)
10.81 protons each weighing around 1 amu
83.

I am usually a good conductor and shiny/lustrous

a)

Metal

b)

Metalloid

c)

Non-metal

84.

I am usually a gas, and at the very right side of the periodic table of elements

a)

Metal

b)

Metalloid

c)

Non-metal

85.

I am Chlorine many electrons to I need to be complete?

a)

8

b)

7

c)

1

d)

0

86.

Potassium has 1 valence electron, would it rather gain 7 electrons or lose its one valence electron to complete its energy level?

a)

lose 1 electron

b)

gain 1 electron

c)

lose 7 electrons

d)

gain 7 electrons

87.

Lewis Dot Structure shows us the..

a)

Energy Levels of electrons

b)

Valence electrons

c)

number of protons

d)

total number of electrons

88.
Which of the following is an Alkali Metal? 
a)
Magnesium
b)
Chromium
c)
Sodium
d)
Fluorine 
89.
Which of the following is an Alkaline Earth Metal? 
a)
Calcium
b)
Lithium
c)
Phosphorus
d)
Copper 
90.
Which of the following is a transition metal? 
a)
Iron
b)
Oxygen
c)
Neon
d)
Barium
91.
Which of the following is a Halogen? 
a)
Bromine
b)
Rubidium
c)
Argon
d)
Beryllium
92.
Which of the following is a Noble Gas? 
a)
Krypton
b)
Chlorine
c)
Radium
d)
Gallium
93.
Which of the following is the most reactive group of metals? 
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Transition Metals
94.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
95.
Which of the following groups is inert? 
a)
Alkali
b)
Transition Metals
c)
Halogens
d)
Noble Gas
96.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
97.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
98.

Match the following term to its description

a)

ion

1.

different number of electrons

b)

isotope

2.

different number of neutrons

c)

different element

3.

different number of protons

99.

Name of Elements in found in group 2

a)

alkali metals

b)

alkali earth metals

c)

transition metals

d)

noble gases

e)

halogens

100.

________ created the first periodic table.

a)

Moseley

b)

Mendeleev

c)

Newton

d)

Dewey

101.

Ionization energy is needed to ___________ valence electrons

a)

remove

b)

add

c)

create

d)

destroy

102.

On the current periodic table, elements are arranged by ------

a)

increasing atomic mass

b)

increasing atomic number

c)

decreasing atomic mass

d)

decreasing atomic number

103.

Name of Elements in found in group 17

a)

alkali metals

b)

alkali earth metals

c)

transition metals

d)

noble gases

e)

halogens

104.

Which element has the highest electronegativity and most ionization energy?

a)

F

b)

Fe

c)

Fr

d)

Fl

105.

Name of Elements in found in the d block

a)

inner transition metals

b)

alkali earth metals

c)

transition metals

d)

noble gases

e)

halogens

106.

Which element has the largest atomic size?

a)

F

b)

Fe

c)

Fr

d)

Fl

107.

Location of protons and neutrons in atom

a)

nucleus

b)

electron cloud

c)

both of these

d)

neither of these

108.

Which element does not belong in Group 1?

a)

Li

b)

Fr

c)

H

d)

K

e)

Na

109.

Match the following term to its description

a)

atomic mass

1.

sum of protons + neutrons

b)

atomic number

2.

# of protons only

c)

proton

3.

has a positive charge

d)

electron

4.

has a negative charge

e)

neutron

5.

has neutral (no) charge

110.

On the first periodic table, elements were arranged by ------

a)

increasing atomic mass

b)

increasing atomic number

c)

decreasing atomic mass

d)

decreasing atomic number

111.
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
112.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
113.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
114.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
115.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
116.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
117.
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.
118.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
119.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
120.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
121.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
122.
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. 
123.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
124.
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
125.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
126.
Which has the greater EN: 
N or C?
a)
C
b)
N
127.
Which has the greater EN: 
H or F?
a)
H
b)
F
128.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
129.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
130.
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)
131.
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
132.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
133.
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
134.
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.
135.
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.
136.
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. 
137.
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
138.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
139.
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.
140.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
141.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

142.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
143.
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 
144.
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
145.
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
146.
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
147.
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.
148.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
149.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
150.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
151.
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
152.
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)
153.
Which of the following will have a higher ionization energy than arsenic (As)?
a)
Gallium (Ga)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
154.
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. 
155.
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.
156.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
157.
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
158.
The electronegativity of Cl is the highest in Period 2.  Why?
a)
Cl is the largest and has the greatest effective nuclear charge
b)
Cl is the smallest and has the lowest effective nuclear charge
c)
Cl is the largest and has the lowest effective nuclear charge
d)
Cl is the smallest and has the greatest effective nuclear charge
159.
What term is used to describe "an atom's tendency to attract electrons to itself when is is chemically combined with another element"
a)
electronation
b)
electron affinity
c)
electronegativity
d)
electrolysis
160.
What term is used to describe "The energy required to remove an electron from gaseous atoms"
a)
excitation energy
b)
ionization energy
c)
polarization energy
d)
electrolytic energy 
161.
What term is used to describe "A measure of the size of an atom"
a)
chemical reactivity
b)
atomic radius
c)
energy levels
d)
orbit
162.
Which element has the greater ionization energy?
a)
Magnesium
b)
Phosphorus
163.
Put the following in order of increasing ionization energy:Strontium, Aluminum, Indium
a)
Strontium, Indium, Aluminum
b)
Strontium, Aluminum, Indium
c)
Indium, Aluminum, Strontium
d)
Aluminum, Indium, Strontium
164.
Put the following in order of increasing ionization energy:Cobalt, Tungsten, Ruthenium
a)
Tungsten, Ruthenium, Cobalt
b)
Cobalt, Tungsten, Ruthenium
c)
Ruthenium, Cobalt, Tungsten
d)
Cobalt, Ruthenium, Tungsten
165.
Put these in increasing order of atomic radii:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
166.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
167.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
168.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
169.
Rank the following elements by increasing atomic radius:
carbon, aluminum, oxygen, phosphorus.
Not sure? check out page 151 in your textbook
a)
O, C, P, Al
b)
Al, P, C, O
c)
O,P, C, Al
d)
O, P, Al, C
170.
The general trend of metal ion size is that they decrease in size as you move from ______ to ______ on the PT.
a)
Right to left
b)
Left to right
c)
Diagonally
d)
Top to bottom
171.
The general trend of non-metal ion size is that they increase in size as you move from ______ to ______ on the PT.
a)
Left to right
b)
Bottom to top
c)
Top to bottom
172.
What element is the MOST reactive metal on the PT?
a)
Cu
b)
Mn
c)
F
d)
Fr
173.
Which element is a metalloid?
a)
S
b)
Br
c)
As
d)
Au
174.
Alkali metals are characterized by their...
a)
Formation of +2 charges
b)
High levels of reactivity
c)
Low melting points
d)
valence electrons in the "p" block
175.
Noble gases are characterized by...
a)
High reactivity
b)
Being solid at room temperature
c)
Low ionization energy
d)
Full valence shell of electrons
176.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
177.
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
178.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
179.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
180.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
181.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

182.

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)

183.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

184.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

185.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

186.

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

187.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

188.

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

189.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

190.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

191.

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

a)

group or family

b)

period

c)

periodic law

d)

octet rule

192.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium

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