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The Periodic Law

Total questions: 207

Worksheet time: 2hrs 29mins

Name
Class
Date
1.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
2.
A vertical column is called...
a)
group
b)
tower
c)
period
d)
crew
3.
The number at the bottom of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
chemical symbol
d)
element name
4.
The number at the top of each square on the periodic table is the ...
a)
atomic number
b)
atomic mass
c)
Chemical Symbol
d)
Element Name
5.
A rule that states that repeating chemical and physical properties of elements change periodically with the atomic number of the elements is the _________.
a)
periodic law
b)
alkaline-earth metals
c)
actinide
d)
group rule
6.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
7.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

8.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

9.

who discovered the first scientific and systematic periodic table

a)

Henry Mosley

b)

Dmitri Mendeleev

c)

John Dalton

d)

sir Isaac Newton

10.

Which one is correct about mendeleev's periodic law

a)

Properties of elements are periodic function of their atomic mass

b)

the physical and chemical properties of elements are periodic function of their atomic number.

c)

physical properties of elements are periodic function of their atomic weight.

d)

chemical properties of elements are periodic function of their atomic number.

11.

Which person was the first to organize the periodic table by atomic mass?

a)

J. Newlands

b)

Dmitri Mendeleev

c)

Lothar Meyer

12.

How are the elements arranged on the periodic table today?

a)

By atomic mass

b)

By number of electrons

c)

By atomic number

d)

By alphabetic order

13.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
14.
These are found on the Periodic Table.
a)
Compounds
b)
Elements
c)
Mixtures
15.

Who arranged the elements by increasing atomic number?

a)

John Newlands

b)

Lothar Meyer

c)

Dmitri Mendeleev

d)

Henry Moseley

16.

Who proposed the Law of Octaves?

a)

Lothar Meyer

b)

Henry Moseley

c)

John Newlands

d)

Dmitri Mendeleev

17.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
18.
As the Coulombic attraction in an atom increases, the energy needed to remove an electron: increases or decreases?
a)
increases
b)
decreases
19.
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
20.

Which element is not a metal?

a)

Hg

b)

Rh

c)

Al

d)

C

21.

What period and group is Chlorine (Cl)?

a)

Period 3, Group 14

b)

Period 3, Group 17

c)

Period 2, Group 17

d)

Period 2, Group 14

22.

What period and group is Arsenic (As)?

a)

Period 3, Group 14

b)

Period 3, Group 15

c)

Period 4, Group 15

d)

Period 4, Group 14

23.

The number of periods and groups in the

periodic table are______.

a)

6,16

b)

7,17

c)

8,18

d)

7,18

24.

Who organized the first periodic table?

a)

Mendeleev

b)

Moseley

c)

Mozart

d)

Lavosier

25.

Identify the period and group of the element that has the electron configuration 1s2 2s2 2p6 3s2 3p3.

a)

Period 2 group 12

b)

Period 3 group 11

c)

Period 3 group 13

d)

Period 3 group 15

26.

Which of the following would be found in Group 4?

a)

Silicon (Si)

b)

Titanium (Ti)

c)

Sodium (Na)

d)

Potassium (K)

27.

What is the electron configuration of the element in period 3, group 16?

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3d10 3p4

c)

1s2 2s2 2p6 3s2 3p4

d)

1s2 2s2 2p6 3s2 3p2

28.
Looking at atoms in the same group/family, what factor affects Coulombic attraction?
a)
number of protons
b)
distance from the nucleus
29.
Looking at atoms in the same valence energy level, what factor affects Coulombic attraction?
a)
number of protons
b)
distance from the nucleus
30.
Ionization energy is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
31.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
32.
As the Coulombic attraction increases the atomic radius: increases or decreases?
a)
increases
b)
decreases
33.
Which element has the smaller atomic radius: potassium (K) or bromine (Br)?
a)
potassium (K)
b)
bromine (Br)
34.
As the Coulombic attraction in an atom increases, the energy needed to remove an electron: increases or decreases?
a)
increases
b)
decreases
35.
Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?
a)
Aluminum (Al)
b)
Chlorine (Cl)
36.
As the Coulombic attraction of an atom increases, the electronegativity of the atom: increases or decreases?
a)
increases 
b)
decreases
37.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
38.
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
39.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
40.
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
41.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
42.
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
43.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
44.
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.
45.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
46.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
47.
A rule that states that repeating chemical and physical properties of elements change periodically with the atomic number of the elements is the _________.
a)
periodic law
b)
alkaline-earth metals
c)
actinide
d)
group rule
48.

Which one is correct about mendeleev's periodic law

a)

Properties of elements are periodic function of their atomic mass

b)

the physical and chemical properties of elements are periodic function of their atomic number.

c)

physical properties of elements are periodic function of their atomic weight.

d)

chemical properties of elements are periodic function of their atomic number.

49.

Which person was the first to organize the periodic table by atomic mass?

a)

J. Newlands

b)

Dmitri Mendeleev

c)

Lothar Meyer

50.

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

51.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
52.

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

a)

8

b)

10

c)

2

d)

4

53.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
54.

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

55.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
56.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

57.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

58.

Which of the following is not a correct designation for a sublevel?

a)

zz

b)

p

c)

d

d)

f

59.
Which periodic table family could have electrons filling orbitals in the s-block?
a)
Alkaine Earth 
b)
Halogens
c)
Noble Gases
d)
Transition Metals
60.

How many electrons can the second shell have?

a)

Two

b)

Eight

c)

Five

d)

Three

61.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
62.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
63.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

64.

Elements in the same group have the same

a)

Properties

b)

Number of electrons

c)

Number of protons

d)

Nucleus

65.
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 neutrons
66.

Atomic number

a)

The number of protons in the nucleus of an atom

b)

a measure of the size of its atom

c)

formulated the first Periodic Law and created a farsighted version of the periodic table of elements that arranged elements by their properties and not atomic mass.

d)

Negatively charged particle that orbits the nucleus of an atom.

67.

Atomic Radii

a)

The number of protons in the nucleus of an atom

b)

a measure of the size of its atom

c)

formulated the first Periodic Law and created a farsighted version of the periodic table of elements that arranged elements by their properties and not atomic mass.

d)

Negatively charged particle that orbits the nucleus of an atom.

68.

Dmitri Mendeleev

a)

The number of protons in the nucleus of an atom

b)

a measure of the size of its atom

c)

formulated the first Periodic Law and created a farsighted version of the periodic table of elements that arranged elements by their properties and not atomic mass.

d)

Negatively charged particle that orbits the nucleus of an atom.

69.

Electron

a)

The number of protons in the nucleus of an atom

b)

a measure of the size of its atom

c)

formulated the first Periodic Law and created a farsighted version of the periodic table of elements that arranged elements by their properties and not atomic mass.

d)

Negatively charged particle that orbits the nucleus of an atom.

70.

Electron configuration

a)

the arrangement of electrons in an atom

b)

a measure of the ability of an atom in a chemical compound to attract electrons

c)

reformulated the periodic table based on atomic number better fitting the periodic law and pattern seen by scientists.

d)

the energy required to remove an electron from an atom or ion

71.

Electronegativity

a)

the arrangement of electrons in an atom

b)

a measure of the ability of an atom in a chemical compound to attract electrons

c)

reformulated the periodic table based on atomic number better fitting the periodic law and pattern seen by scientists.

d)

the energy required to remove an electron from an atom or ion

72.

Henry Moseley

a)

the arrangement of electrons in an atom

b)

a measure of the ability of an atom in a chemical compound to attract electrons

c)

reformulated the periodic table based on atomic number better fitting the periodic law and pattern seen by scientists.

d)

the energy required to remove an electron from an atom or ion

73.

Ionization Energy

a)

the arrangement of electrons in an atom

b)

a measure of the ability of an atom in a chemical compound to attract electrons

c)

reformulated the periodic table based on atomic number better fitting the periodic law and pattern seen by scientists.

d)

the energy required to remove an electron from an atom or ion

74.

Orbital

a)

a region of an electron subshell where there is a high probability of finding electrons.

b)

a vertical column of elements in the periodic table; elements in the same group share chemical properties

c)

The physical and chemical properties of the elements are periodic functions of their atomic numbers

d)

a horizontal row of elements in the periodic table

75.

Periodic Group

a)

a region of an electron subshell where there is a high probability of finding electrons.

b)

a vertical column of elements in the periodic table; elements in the same group share chemical properties

c)

The physical and chemical properties of the elements are periodic functions of their atomic numbers

d)

a horizontal row of elements in the periodic table

76.

Periodic Law

a)

a region of an electron subshell where there is a high probability of finding electrons.

b)

a vertical column of elements in the periodic table; elements in the same group share chemical properties

c)

The physical and chemical properties of the elements are periodic functions of their atomic numbers

d)

a horizontal row of elements in the periodic table

77.

Periodic Period

a)

a region of an electron subshell where there is a high probability of finding electrons.

b)

a vertical column of elements in the periodic table; elements in the same group share chemical properties

c)

The physical and chemical properties of the elements are periodic functions of their atomic numbers

d)

a horizontal row of elements in the periodic table

78.

Periodic Properties

a)

recurring trends in physical and chemical characteristics of elements.

b)

an electron that is found in the outermost shell of an atom and that determines the atom’s chemical properties.

c)

The energy level at which electrons orbit the nucleus of an atom.

d)

a subdivision of electron shells. Broken into s,p,d,f subshells

79.

Which has the smaller Electronegativity?

a)

Cl

b)

Al

80.

Which has the larger Electronegativity?

a)

Carbon

b)

Nitrogen

81.

Which of the following will have a larger radius than Gallium (Ga)?

a)

Ge

b)

Al

c)

Mg

d)

Sr

82.

Which of these has the smallest atomic radius?

a)

K

b)

Rb

c)

Fr

d)

Cs

83.
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
84.

Which has the smaller ionization energy?

a)

P

b)

Mg

85.

Which has the highest ionization energy?

a)

Ca

b)

As

c)

Br

86.

Which would be the easiest to take an electron from?

a)

He

b)

F

c)

Ba

d)

Fr

87.

Which element would want to keep its electrons the most?

a)

O

b)

S

c)

Al

d)

Rb

88.

As you move to the right across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have more neutrons

c)

the atoms have more protons.

d)

the atoms have more electrons.

89.
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
90.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
91.
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
92.
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
93.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
94.
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.
95.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
96.
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
97.
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
98.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
99.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
100.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
101.
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
102.
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)
103.
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)
104.
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. 
105.
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.
106.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
107.
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
108.
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
109.
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
110.
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 
111.
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
112.

Which species has the larger radius?

a)

Cl

b)

Cl-

113.

Which species has the larger radius?

a)

Na

b)

Na+

114.

Which is larger... P or P3- ? … and why?

a)

P3- because it gains an energy level

b)

P3- due to extra electron repulsion

c)

P because it loses an energy level

d)

P because of extra electron repulsion

115.
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
116.
The more protons there are, the  ____ .
a)
Weaker the pull
b)
Smaller the electrons
c)
Stronger the pull
d)
The bigger the electrons
117.

Arrange these species in increasing order of size.

Cl- , Ca2+ , S2- , Ar , K+

a)

Ca2+ > K+ > Ar > Cl- > S2-

b)

S2- > Cl- > Ar > K+ > Ca2+

c)

Ca2+ < K+ < Ar < Cl- < S2-

d)

S2- < Cl- < Ar < K+ < Ca2+

118.

Which has the highest ionization energy?

a)

Arsenic

b)

Iron

c)

ZInc

d)

Cobalt

119.

Going down the group, the atomic radius of elements increases. Why is that so?

a)

the number of shell (n) increases

b)

Shielding effect increases

c)

Nucleus attraction towards valence electrons weaker

d)

All of the above

120.

What is the trend for electronegativity as you move left to right across a period and why?

a)

EN increases because the shielding effect increases causing the effective nuclear charge to decrease as you add more protons to the nucleus

b)

EN decreases because the shielding effect decreases causing the effective nuclear charge to increase as you add more protons to the nucleus

c)

EN increases because the effective nuclear charge increases as you add protons to the nucleus and increase the number of valence electrons in the outer shell

d)

EN decreases because the effective nuclear charge decreases as you reduce the number of protons in the nucleus and increase the number of valence electrons in the outer shell

121.

What is the trend for EN as you move down a group or family and why?

a)

EN increases because the number of energy levels decrease causing an increase in the shielding effect and a decrease in the effective nuclear charge.

b)

EN decreases because the number of energy levels increases causing an increase in the shielding effect and a decrease in the effective nuclear charge

c)

EN increases because the number of energy levels increases causing a decrease in the shielding effect and an increase in the effective nuclear charge

d)

EN decreases because the number of energy levels decrease causing a decrease in the shielding effect and a decrease in the effective nuclear charge.

122.

Which element has the greatest electronegativity?

a)

Si

b)

S

c)

Ar

d)

Na

123.

Which element has the lowest electronegativity?

a)

Sr

b)

Mg

c)

Ra

d)

Ca

124.

Which element has the least effective nuclear charge?

a)

N

b)

F

c)

Li

d)

Be

125.

Arrange the following elements in order by increasing electronegativity - Sn, Sr, I, Ag, Zr

a)

Sr, Zr, Ag, Sn, I

b)

Sr, Ag, Zr, I, Sn

c)

I, Sn, Ag, Zr, Sr

d)

Sn, I, Zr, Ag, Sr

126.

The trend for reactivity for metals is that the reactivity _______ as you go across the period and it _________ as you move down a group.

a)

increases, increases

b)

decreases, decreases

c)

does not change, decreases

d)

decreases, increases

127.

The trend for reactivity for nonmetals is that as you move across from left the right reactivity __________(except for noble gases) and as you move down a group the reactivity _________

a)

increases, increases

b)

decreases, decreases

c)

decreases, increases

d)

increases, decreases

128.

Which of the following nonmetals are the most reactive?

a)

Ge

b)

Kr

c)

Se

d)

Br

129.

Which of the following nonmetals are the most reactive?

a)

Po

b)

S

c)

Se

d)

O

130.

What is the most reactive nonmetal?

a)

I

b)

F

c)

N

d)

At

131.

What is the most reactive metal?

a)

Li

b)

Be

c)

Fr

d)

H

132.

Metals that are the most reactive have the following characteristics

a)

small atomic radius, high ionization energy, high electronegativity

b)

large atomic radius, high ionization energy, low electronegativity

c)

large atomic radius, low ionization energy, low electronegativity

d)

small atomic radius, low ionization energy, low electronegativity

133.

As you move down a group the effective nuclear charge ________ as the shielding effect _________

a)

decreases, increases

b)

decreases, decreases

c)

increases, increases

d)

increases, decreases

134.

The most reactive nonmetals have _____ valence electrons

a)

1

b)

2

c)

7

d)

8

135.

The most reactive metals have _____ valence electrons.

a)

1

b)

2

c)

7

d)

8

136.

Which element has an electronegativity of 4.0, the highest of all elements?

a)

H

b)

Fr

c)

He

d)

F

137.

Which element has an electronegativity of 0.7, the lowest of all the elements?

a)

H

b)

He

c)

F

d)

Fr

138.

Metals are electron _______ because they tend to _______ electrons in order to become stable like the noble gases.

a)

takers, lose

b)

takers, gain

c)

givers, gain

d)

givers, lose

139.

What has the greatest effect on electronegativity as you move across a period? (check all that are correct)

a)

shielding effect

b)

effective nuclear charge

c)

number of neutrons

d)

number of protons

e)

number of energy levels

140.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

141.

The distance between nucleus and outermost shell occupied electron

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

142.

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

143.

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

144.

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

145.

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

146.

Which element has higher electronegativity?

a)

Fluorine is higher than Oxygen

b)

Potassium is higher than Sodium

c)

Aluminium is higher than Boron

d)

Phosphorus is higher than Chlorine

147.

Which element has higher electronegativity?

a)

Fluorine is higher than Oxygen

b)

Potassium is higher than Sodium

c)

Aluminium is higher than Boron

d)

Phosphorus is higher than Chlorine

148.

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

149.

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

150.

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

151.

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

152.
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)
153.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
154.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
155.

Which color on the image of the periodic table corresponds with the halogens.

a)

red

b)

black

c)

blue

d)

orange

156.

Which color on the image of the periodic table corresponds with the lanthanides.

a)

red

b)

black

c)

blue

d)

orange

157.

Which color on the image of the periodic table corresponds with the transition metals.

a)

red

b)

black

c)

blue

d)

orange

158.

Which of the following are poor conductors of heat and electricity?

a)

metals

b)

metalloids

c)

nonmetals

d)

alkaline earth elements

159.

Which group on the periodic table is known as the alkaline earth metals?

a)

group 1A

b)

group 2A

c)

group 8A

d)

group 7A

160.

Halogens are good disinfectants. Which of the following is a halogen?

a)

N

b)

O

c)

Cl

d)

Fe

161.

Why do atomic numbers jump by 15 from left to right in the section of the periodic table shown above?

a)

The missing elements have not yet been discovered.

b)

The missing elements are all radioactive.

c)

The missing elements form the lathanide and actinide series, usually found below the periodic table.

d)

The missing elements do not exist.

162.

Why are both hydrogen and cesium s-block elements, when hydrogen has one electron and cesium has 55?

a)

All blocks contain at least one element from each period.

b)

Blocks of elements on the periodic table are based only on an element's valence electrons.

c)

The s-block includes only the most reactive elements.

d)

They have identical electron configurations.

163.

Atoms of elements in group 1 have ____________.

a)

one electron in their outermost energy level

b)

two electrons in their outermost energy level

c)

seven electrons in their outermost energy level

d)

eight electrons in their outermost energy level

164.

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

a)

s block

b)

p block

c)

d block

d)

f block

165.

What makes the d block wider than either the s block or the p block?

a)

The d sub-orbital can hold ten electrons, making the d block ten elements wide.

b)

The d block is the most researched area of the periodic table.

c)

The elements in the d block are more important than the elements in the rest of the table.

d)

The elements in the d block are all metals.

166.

Atoms with large ionization energy values are __________.

a)

more likely to form positive ions

b)

less likely to form positive ions

c)

most likely to lose their outer electrons

d)

lacking valence electrons lacking valence electrons

167.

Why are the ionic radii generally larger for group 15 than for group 17?

a)

Atoms in group 15 are larger than atoms in group 17.

b)

Atoms in group 15 have more protons than atoms in group 17

c)

Ions forming from group 15 atoms have a greater negative charge than ions forming from group 17 atoms.

d)

Atoms in group 15 are less likely to lose electrons than atoms in group 17.

168.

element Triads have similar properties; quantitative properties of middle element are the average of the other two in the triad; had lots of exceptions

a)

Meyer

b)

Mosley

c)

Mendeleev

d)

Dobereiner

169.

first to organize the elements by atomic mass; noticed patterns in every 8th element; law of octaves; left no gaps for future discovery; law of octaves did not work for larger elements

a)

Dobereiner

b)

Mendeleev

c)

Seaborg

d)

Newlands

170.

synthesized many elements past Uranium and reorganized the table by adding an f-block

a)

Seaborg

b)

Mosley

c)

Meyer

d)

Mendeleev

171.

organized elements by atomic number; modern periodic table; fixed some of inconsistencies from "best" of the historic periodic tables

a)

Meyer

b)

Mosley

c)

Newlands

d)

Mendeleev

172.

all have full valence shell; inert gases; "nonreactive"

a)

Halogens

b)

Actinides

c)

Metalloids

d)

Noble Gases

173.

Which element would have a larger atomic radius?

a)

tellurium, Te

b)

beryllium, Be

174.

Which of these shows the correct relationship for atomic and ionic radii?

a)

Ca < Ca2+

b)

N > N3-

c)

K > K+

d)

Fe2+ = Fe3+

175.

Which of these elements has a greater ionization energy?

a)

magnesium, Mg

b)

barium, Ba

176.

Which of these elements has a higher ionization energy?

a)

potassium, K

b)

germanium, Ge

177.

Which of these elements will have the higher electronegativity?

a)

oxygen, O

b)

polonium, Po

178.

Which of these elements will have the higher electronegativity?

a)

nitrogen, N

b)

beryllium, Be

179.

Which ion will have a greater radius?

a)

Sr2+

b)

Mg2+

180.

Which ion will have a greater radius?

a)

Al3+

b)

Na+

181.

Which atom's valence electrons will experience the greater Coulombic attraction to the nucleus?

a)

aluminum, Al

b)

chlorine, Cl

182.

Which atom's valence electrons will experience the greater Coulombic attraction to the nucleus?

a)

helium, He

b)

krypton, Kr

183.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
184.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
185.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
186.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
187.
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)
188.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
189.
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.
190.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
191.
Put the following in order of increasing ionization energy:Neon, Lithium, Carbon
a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon
192.
Which of the following elements has the largest atomic radius, vanadium or iron?
a)
vanadium
b)
iron
193.

Where is there a big jump of ionization energy increase for the element Silicon(Si)?

a)

between 1 and 2

b)

between 6 and 7

c)

between 7 and 8

d)

between 4 and 5

194.

Why is there a large jump in ionization energy 1 and 2 for Lithium?

a)

the valence electrons are harder to lose than core electrons

b)

the valence electrons are easier to lose than core electrons

195.

 After the atom is ionized, it then requires more energy to remove a second electron because the second electron is nearer the nucleus.

a)
False
b)
True
196.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

197.

Select ALL that explain the ionization energy trend within groups

a)

electrons are closer to the nucleus

b)

their is a weak pull between electrons from the nucleus, making them easily moveable

c)

feel more of a pull from nucleus, making them harder to move

d)

electrons are further from the nucleus

198.

Select ALL that explain the ionization energy trend within periods

a)

electrons are closer to the nucleus

b)

their is a weak pull between electrons from the nucleus, making them easily moveable

c)

feel more of a pull from nucleus, making them harder to move

d)

electrons are further from the nucleus

199.
Which of the following is true for alkaline earth metals as their atomic number increases?
a)
The atomic radius decreases.
b)
Ionization energy decreases.
c)
The number of valence electrons increases.
d)
The Coulombic attraction increases.
200.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
201.

What makes a valence electron less attracted to the nucleus?

a)

less distance between the nucleus and having less protons

b)

less distance between the nucleus and having more protons

c)

more distance between the nucleus and having less protons

d)

more distance between the nucleus and having more protons

202.
The bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?
a)
They are in the same period with W being furthest left.
b)
They are in the same period with W being furthest right.
c)
They are in the same group with W being furthest to the bottom.
d)
They are in a diagonal line with W being at the bottom right.
203.
The more protons there are, the  ____ .
a)
Weaker the pull
b)
Smaller the electrons
c)
Stronger the pull
d)
The bigger the electrons
204.

Beryllium has higher first ionization energy than Boron because ___________________

a)

the first electron is removed from partially filled orbital

b)

the first electron is removed from half filled orbital

c)

the first electron is removed from completely filled 2s orbital

d)

Be has smaller atomic radius

205.

What are/is the factors that influence the ionisation energy? (you may click more than one)

a)

Atomic Size

b)

Effective Nuclear Charge

c)

Shielding effect

d)

Orbital stability

206.

Choose the arrangement that shows increasing first IE in Period 2:

a)

Boron < Carbon < Nitrogen

b)

Nitrogen < Carbon < Boron

c)

Boron < Nitrogen < Carbon

d)

Carbon < Nitrogen < Boron

207.

Choose the arrangement that shows increasing first IE in Period 3:

a)

Aluminium < Phosphorus < Silicon

b)

Aluminium < Silicon < Phosphorus

c)

Silicon < Aluminium< Phosphorus

d)

Silicon < Phosphorus< Aluminium