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Grade 10Elite Chapter 8 Periodic Relationships Among the Element

Total questions: 136

Worksheet time: 2hrs 9mins

Name
Class
Date
1.

The atoms of elements belonging to the same group of periodic table have same number of_____.

a)

protons

b)

electrons

c)

neutrons

d)

electrons in outermost

2.

The atoms of elements belonging to the same group of periodic table have same number of_____.

a)

protons

b)

electrons

c)

neutrons

d)

electrons in outermost

3.

All the elements in a period in the periodic table have the same _______

a)

atomic number

b)

electronic configuration

c)

atomic weight

d)

valence shell

4.

All the members in a group of a long form of periodic table have the same ________.

a)

valency

b)

number of valence electrons

c)

chemical properties

d)

All of the above

5.

Which has the maximum atomic radius ?

a)

Al

b)

Si

c)

P

d)

Mg

6.

In modern periodic table, arrange the third row elements Na, Mg, Al and Si in the increasing order of their atomic size ______.

a)

Na > Mg > Al > Si

b)

Al > Si > Na > Mg

c)

Si > Al > Mg > Na

d)

Na > Al > Si > Mg

7.

In the third period of the periodic table, the element having smallest size is _____.

a)

Na

b)

Ar

c)

Cl

d)

Si

8.

In the periodic table, the metallic character of elements ______.

a)

decreases from left to right and down the group

b)

decreases from left to right and increases down the group

c)

increases from left to right and down the group

d)

increases from left to right and decreases down the group

9.

From top to bottom in a group of the periodic table electropositive character of the element ______.

a)

increases

b)

decreases

c)

remains unchanged

d)

changes irregularly

10.

Which of the following increases along the period ?

a)

Number of valence electrons

b)

Atomic size

c)

Electropositive character

d)

All of these

11.

The total number of elements found in 4th period of modern periodic table is _____.

a)

8

b)

18

c)

32

d)

12

12.

Which of the following element loses an electron most easily?

a)

Na

b)

Mg

c)

K

d)

Ca

13.

For 52X24 , number of electrons is _______.

a)

52

b)

24

c)

76

d)

28

14.

To complete the octate, outer most shell of Aluminium ______.

a)

looses two electrons

b)

gains three electrons

c)

looses three electrons

d)

shares four electrons

15.

Each of the following element forms univalent ions except _____

a)

Li

b)

Na

c)

Mg

d)

K

16.

The elements with atomic numbers 3, 11, 19, 37 and 55 are all termed as____.

a)

Noble metals

b)

Alkali metals

c)

Noble gases

d)

Alkaline Earth metals

17.

Why are the elements lithium, sodium and potassium called alkali metals ?

a)

Because they reacts with water to form alkali

b)

Because they form acidic oxides

c)

Because they are present in first group

d)

Because they are less reactive in nature

18.

Alkali metals in each period have ______.

a)

Smallest size

b)

Lowest I.E.

c)

Highest E.A

d)

Highest electronegativity

19.

Which of the following statements is not a correct statement about the trends when going from left to right across the periods of the periodic table ?

a)

The elements become less metallic in nature

b)

The number of valence electrons increases

c)

The atoms lose their electrons more easily

d)

The oxides become more acidic

20.

Considering the elements B, Al, Mg and K, the correct order of their metallic character is _____.

a)

B > Al > Mg > K

b)

AI > Mg > B > K

c)

Mg > Al > K > B

d)

K > Mg > Al > B

21.

Which of the following elements has maximum metallic character ?

a)

Li

b)

N

c)

Na

d)

P

22.

On moving left to right in a period, in the periodic table, metallic character _____.

a)

decrease

b)

increases

c)

remains same

d)

first increase, then decreases

23.

On moving from top to bottom in a group, in the periodic table, size of an atom______.

a)

increases

b)

decreases

c)

remains same

d)

first increases, then decreases

24.

On moving from top to bottom in a group, in the periodic table, valency ______.

a)

increase

b)

decreases

c)

remains same

d)

first increases, then decreases

25.
As the elements are considered from top to bottom of group 15 (V A),  which sequence in properties occurs? 
a)
metalloid→metal→nonmetal
b)
nonmetal→metalloid→metal
c)
metal→nonmetal→metalloid
d)
metal→metalloid→nonmetal
26.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

27.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

28.

Of the halogens, which has the smallest electronegativity?

a)

F

b)

Cl

c)

At

d)

Ne

29.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
30.
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)
31.
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
32.
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
33.
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. 
34.
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
35.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
36.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

37.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

38.

The electronegativity difference in the bonds of CH4 is:

a)

0.4

b)

5.9

c)

-0.4

d)

1.7

39.

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

40.

Ionization energy trends is . . . .

a)

becomes greater up and to the right of the periodic table.

b)

becomes greater down and to the right of the periodic table.

c)

becomes greater up and to the left of the periodic table.

d)

becomes greater down and to the left of the periodic table.

41.

Electron affinity trends is . . . .

a)

generally increases across a period, and a trend of decreasing electron affinity going down groups would be expected.

b)

generally decreases across a period, and a trend of decreasing electron affinity going down groups would be expected.

c)

generally increases across a period, and a trend of increasing electron affinity going down groups would be expected.

d)

generally decreases across a period, and a trend of increasing electron affinity going down groups would be expected.

42.

Metallic character trends is . . . .

a)

decrease going across a period and tends to increase going down a group.

b)

increase going across a period and tends to increase going down a group.

c)

decrease going across a period and tends to decrease going down a group.

d)

increase going across a period and tends to decrease going down a group.

43.

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

44.

Which types of elements from anions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

45.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

46.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
47.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
48.

What is the term for the rows of periodic table?

a)

periods

b)

groups

c)

blocks

d)

configurations

e)

trends

49.

Who is the founder of current periodic table system?

a)

Dmitri Mendeleev

b)

Antonie Lavoisier

c)

John Dalton

d)

Erwin Schrodinger

e)

Johann Dobereiner

50.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
51.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
52.

Metallic character is based on...

a)

how shiny something is.

b)

the density of a material.

c)

an atom's ability to lose electrons.

d)

the ability to conduct electricity.

53.

This results in decreased attraction of electrons for the nucleus of an atom due to inner electrons blocking the attraction of valence electrons.

a)

Periodic Trends

b)

Shielding Effect

c)

Octet Rule

d)

Hund's Rule

54.

Which of the following is the best metal?

a)

Na

b)

K

c)

Mg

d)

Ca

55.

Which of the following is the best nonmetal?

a)

O

b)

F

c)

S

d)

Cl

56.

Which of the following is NOT a metal?

a)

Ca

b)

Cu

c)

Ge

d)

Zn

57.

Which of the following is a complete list of metalloids?

a)

B, Si, Ge, As, Sb

b)

B, Si, Ge, As, Sb, Te

c)

B, Si, Ge, As, Sb, Te, Po

d)

B, Si, Ge, As, Sb, Te. Po, At

58.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
59.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

60.
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
61.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
62.

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.

63.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
64.
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 
65.
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.
66.
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
67.
Put the following in order of increasing ionization energy:Sodium, Oxygen, Boron
a)
Sodium, Boron, Oxygen
b)
Oxygen, Boron, Sodium
c)
Sodium, Oxygen, Boron
d)
Oxygen, Sodium, Boron
68.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

69.
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
70.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
71.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
72.
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
73.
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.
74.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
75.
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 
76.
The more protons there are, the  ____ .
a)
Weaker the pull
b)
Smaller the electrons
c)
Stronger the pull
d)
The bigger the electrons
77.

Which element's atom is larger? Nitrogen or Phosphorus?

a)

Nitrogen

b)

Phosphorus

78.

As you move ______ a group, more energy levels are added, which increases the size of the atom

a)

down

b)

up

c)

diagonal

d)

away

79.

Within periods on the periodic table: Size decreases as you go down a group

a)

Flase

b)

True

80.

Which element's atom is the smallest?

a)

Rhodium

b)

Silver

c)

Cadmium

d)

Tin

81.

Which of these best explains the reasoning behind the trend that as you go across a period, size decreases?

a)

As you go across a period, more energy levels are added, which shrinks the atom.

b)

The added electrons in the nucleus give the atom a negative charge, which shrinks the atom.

c)

The added protons in the nucleus pull the electrons closer to them, which shrinks the atom.

d)

All of the above

82.

Which order is correct from largest to smallest atomic radius?

a)

Thallium, Indium, Gallium, Boron

b)

Boron, Thallium, Indium, Gallium

c)

Boron, Gallium, Indium, Thallium

d)

Thallium, Gallium, Indium, Boron

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.
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.
85.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
86.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
87.
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
88.
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.
89.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
90.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
91.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
92.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
93.
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
94.
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)
95.
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)
96.

Atomic size 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

97.

As you move from left to right on the periodic table, the number of valence electrons.......

a)

Increases

b)

Decreases

c)

Remains the same

98.

As you move down a group on the periodic table, the number of valence electrons....

a)

Increases

b)

Decreases

c)

Remains the same

99.

Which of the following would be most similar to Phosphorus? (select all that apply)

a)

Nitrogen

b)

Sulfur

c)

Silicon

d)

Germanium

e)

Antimony

100.

An electron that resides in the outermost energy level of an atom

a)

periodic trend

b)

electron shell

c)

ionic radius

d)

valence electron

101.

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

102.

The period that an element is in on the periodic table, tells you what?

a)

Number of protons

b)

Number of electrons

c)

Number of valence electrons

d)

Number of energy levels

103.

When across a period, the atomic size decreases so the first IE ___________.

a)

increases

b)

decreases

c)

constant

d)

i am not sure

104.

When going down a group, the atomic size increases so the first IE __________.

a)

increases

b)

decreases

c)

constant

d)

I am not sure

105.

Factors affecting the ionisation energy:

a)

Atomic radius

b)

Effective nuclear charge

c)

Shielding effect

d)

All of the above

106.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
107.
Which element has the greater ionization energy?
a)
Lead
b)
Silicon
108.
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
109.
Put the following in order of increasing ionization energy:Sodium, Oxygen, Boron
a)
Sodium, Boron, Oxygen
b)
Oxygen, Boron, Sodium
c)
Sodium, Oxygen, Boron
d)
Oxygen, Sodium, Boron
110.

In general ionization energy ____ as you go down a group,

and ____ as you go across the periodic table.

a)

decreases, decreases

b)

decreases, increases

c)

increases, decreases

d)

increases, increases

111.
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
112.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
113.

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)

114.

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)

115.

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

116.

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

a)

atom

b)

ion

c)

cation

d)

anion

117.

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

a)

cation

b)

anion

c)

electron

d)

ion

118.
Define electron affinity.
a)
The energy it takes to add an electron to an atom.
b)
The energy it takes to remove an electron from an atom.
119.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
120.

Which has the highest ionization energy?

a)

Arsenic

b)

Iron

c)

ZInc

d)

Cobalt

121.

Which has a lower ionization energy?

a)

Lithium

b)

Cesium

c)

Sodium

122.

Explain why ionization energy decreases as you go down a group.

a)

Outer electrons are further away from the nucleus you go down a group

b)

Electrons feel less pull from the nucleus as you go down a group

c)

Electrons are easier to remove as you go down a group

d)

All of the above

123.

Which of the following lists the atoms in order of increasing Ionization energy?

a)

calcium, iron, copper

b)

copper, iron, calcium

c)

calcium, copper, iron

d)

iron, copper, calcium

124.

Which element has the lowest electron affinity?

a)

Na

b)

K

c)

Rb

d)

Ar

125.

Which element has the highest electron affinity?

a)

Oxygen

b)

Sulfur

c)

Gallium

d)

He

126.

What group contains elements with 7 valence electrons

a)

Noble Gasses

b)

Alkali Earth Metals

c)

Halogens

d)

Transition Metals

127.

Which element is most likely to lose an electron?

a)

Zinc

b)

Arsenic

c)

Bromine

d)

Potassium

128.

Which of these will have the highest electron affinity: Na, Al, Mg, or S?

a)

Na

b)

Al

c)

Mg

d)

S

129.

Which of these has the electron affinity: I, Cl, Br, At

a)

I

b)

Cl

c)

Br

d)

At

130.

Which of these has the lowest electron affinity: Cl, As, K, or Cs?

a)

Cl

b)

As

c)

K

d)

Cs

131.

Which of these has the lowest electron affinity: Ge, As, Se, or Br?

a)

Ge

b)

As

c)

Se

d)

Br

132.

Which of the following has the lowest electron affinity: Sb, Sr, Ag, I

a)

Sb

b)

Sr

c)

Ag

d)

I

133.

Which one of these has the highest ionization energy: Ba, Mg, Ca, or Sr?

a)

Ba

b)

Mg

c)

Ca

d)

Sr

134.

Which of these has the highest ionization energy: P, Bi, Sb, or As?

a)

P

b)

Bi

c)

Sb

d)

As

135.

Which one of these has the highest electron affinity: Li, Al, C, or O?

a)

Li

b)

Al

c)

C

d)

O

136.

True or False: The Periodic trend for first ionization energy and electron affinity Is the same.

a)

True

b)

False

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