Classification of Elements & Periodicity in Properties Test 15

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Classification of Elements & Periodicity in Properties Test 15

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Weekly Quiz Competition

Question 1
1 / -0

Why do noble gases have positive electron gain enthalpy?

A
It is difficult to add an electron due to small size

B
It is difficult to add an electron due to high electronegativity

C
It is difficult to add an electron due to stable configuration

D
It is difficult to add an electron due to high electron affinity

Solution

Due to stable configuration they do not accept an electron and hence they have positive electron gain enthalpy.
Question 2
1 / -0

As we move from left to right, the electronegativity increases. An atom which is highly electronegative has

A
large size

B
low electron affinity

C
high ionisation enthalpy

D
low chemical reactivity

Solution

It is difficult to remove an electron from a highly electronegative element.
Question 3
1 / -0

Study the given diagram and fill up the blanks with appropriate choice.

A
a

B
b

C
c

D
d

Solution

Ionisation enthalpy, electron gain enthalpy and electronegativity increases in a period from left to right while atomic radius decreases.
Question 4
1 / -0

Fill in the blanks with the appropriate option.
The ability of an atom to attract shared electrons to itself is called (i). It is generally measured on the (ii) scale. An arbitrary value of (iii) is assigned to fluorine (have greatest ability to attract electrons). It generally (iv) across a period and (v) down a group.

A
a

B
b

C
c

D
d

Solution

Electronegativity is measured on Pauling scale. Fluorine, the most electronegative element is given the value 4.0. Electronegativity increases from left to right across a period while decreases down a group.
Question 5
1 / -0

In which of the following, the order is not in accordance with the property mentioned.

A
Li < Na < K < Rb - Atomic radius

B
F > N > O > C - Ionisation enthalpy

C
Si < P < S < Cl - Electronegativity

D
F < CI < Br < I - Electronegativity

Solution

Electronegativity decreases down the group.
Question 6
1 / -0

Choose the incorrect statement.

A
Chemical reactivity tends to be high in group 1 metals, lower in elements in middle and increases to maximum in the group 17

B
Halogens have very high negative electron gain enthalpy

C
Noble gases have large positive electron gain enthalpy

D
Decrease in electronegativities across a period is accompanied by an increase in non-metallic properties

Solution

Electronegativity increases across a period.
Question 7
1 / -0

In the periodic table, the maximum chemical reactivity is at the extreme left (alkali metals) and extreme right (halogens). Which properties of these two groups are responsible for this?

A
Least ionisation enthalpy on the left and highest negative electron gain enthalpy on the right

B
Non-metallic character on the left and metallic character on the right

C
High atomic radii on the left and small atomic radii on the right

D
Highest electronegativity on the left and least electronegativity oh the right

Solution

Elements on the left side have lowest ionisation enthalpy due to which they can very easily lose electrons while the elements onthe right can accept electrons easily as they show highest negative electron gain enthalpy.
Question 8
1 / -0

An element X has atomic number 19. What will be the formula of its oxide?

A
X₂O

B
XO

C
XO₂

D
X₂O₃

Solution

Element X has atomic number 19. Its valency will be one. Hence, the formula ofits oxide will be X₂O.
Z = 19; 1s²2s²2p⁶3s²3p⁶4s¹
Question 9
1 / -0

An element 'P' has atomic number 56. What will be the formula of its halide?

A
PX

B
PX₂

C
PX₃

D
P₂X₃

Solution

Z = 56; [Xe] 6s²
Formula of halide is PX₂.
Question 10
1 / -0

Predict the formula of stable compound formed by an element with atomic number 114 and fluorine.

A
AF₃

B
AF₂

C
AF

D
AF₄

Solution

Atomic number 114 will fall into carbon family, hence it will be tetravalent. So, formula with F will be AF₄.
Question 11
1 / -0

Predict the formula of a compound formed by aluminium and sulphur.

A
Al₂S₂

B
Al₃S₂

C
Al₂S₃

D
AIS

Solution

Al - 3e^- → Al³⁺, S + 2e^- → S^2-
The formula for its sulphide is AI₂S₃.
Question 12
1 / -0

There are many elements in the periodic table which exhibit variable valency. This is a particular characteristic of

A
Representative elements

B
Transition elements

C
Noble gases

D
Non-metals

Solution

Transition elements show variable valency due to the presence of vacant d-orbitals.
Question 13
1 / -0

Predict the formulae of the binary compounds formed by combination of the following pairs of elements:
(i) Magnesium and nitrogen
(ii) Silicon and oxygen

A
MgN₂, SiO₂

B
Mg₃N₂, SiO₂

C
Mg₂N₃, Si₂O₃

D
MgN, SiO₂
Question 14
1 / -0

The first element of the groups 1 and 2 are different from other members of the respective groups. Their behaviour is more similar to the second element of the following groups. What is this relationship known as?

A
Anomalous relationship

B
Periodic relationship

C
Diagonal relationship

D
Chemical relationship

Solution

The relation between 1^st element of a group and 2^nd element of the next group is called diagonal relationship.
Question 15
1 / -0

The main reason for showing anomalous properties of the first member of a group in s or p-block is

A
Maximum chemical reactivity

B
Maximum electronegativity and different configurations

C
Small size, large charge/radius ratio

D
Tendency to form multiple bonds

Solution

Due to small size, large charge/radius ratio and high electronegativity, the first elementshows anomalous behaviour.
Question 16
1 / -0

When we go from left to right in a period,

A
The basic nature of the oxides increases

B
The basic nature of the oxides decreases

C
There is no regular trend in the nature of oxides

D
Oxides of only first two groups are basic in nature

Solution

The basic nature of the oxides decreases from left to right in a period, e.g., in third period.
Question 17
1 / -0

Which of the following oxides is neutral in nature?

A
SrO

B
Al₂O₃

C
CO₂

D
CO

Solution

CO isa neutral oxide. SrO isa basic oxide. AI₂O₃ is an amphoteric oxide while CO₂ is an acidic oxide.
Question 18
1 / -0

What is the common property of the oxides CO, NO and N₂O?

A
All are acidic oxides

B
All are basic oxides

C
All are neutral oxides

D
All are amphoteric oxides

Solution

CO, NO and N₂O are neutral oxides.
Question 19
1 / -0

The correct order of acidic character of oxides in third period of periodic table is

A
SiO₂ < P₄O₁₀ < SO₃ < CI₂O₇

B
Cl₂O₇ < SO₃ < P₄O₁₀ < SiO₂

C
SO₃ < CI₂O₂ < P₄O₁₀ < SiO₂

D
SiO₂ < CI₂O₇ < P₄O₁₀ < SO₃

Solution

Acidic character of oxides increases as we move from left to right in a period.
Question 20
1 / -0

Which of the following sets of oxides is amphoteric in nature?

A
AI₂O₃, As₂O₃, ZnO

B
CO, NO, N₂O

C
SO₃, SO₂, CI₂O₇

D
Na₂O, MgO, BaO

Solution

AI₂O₃, As₂O₃ and ZnO are amphoteric in nature.
Question 21
1 / -0

(A), (B) and (C) are elements in the third short period. Oxide of (A) is ionic, that of (B). is amphoteric and of (C) a giant molecule. (A), (B) and (C) have atomic number in the order ;

A
(A) < (B) < (C)

B
(C) < (B) < (A)

C
(A) < (C) < (B)

D
(B) < (A) < (C)

Solution

A, B and C are magnesium, aluminium and sillicon. Magnesium forms ionic oxide, (MgO) aluminium forms amphoteric oxide, (AI₂O₃) and silicon forms a giant molecule (SiO₂).
Question 22
1 / -0

What is common between given cations and anions, O2^-, F^-, Na⁺, Mg²⁺, Al³⁺?

A
All have same ionic radii

B
All are isoelectronic species having 10 electrons

C
All of them belong to the third period

D
The nature of oxides of all the ions is basic
Question 23
1 / -0

Which of the following is arranged in order of increasing metallic character?

A
P < Si < Na < Be < Mg

B
Be < Mg < P < Na < Si

C
Si < Be > Mg < Na < P

D
P < Si < Be < Mg < Na

Solution

Metallic character increases down a group and decreases along a period as we move from leftto right. Hence, the order of increasing metallic character is :
P < Si < Be < Mg < Na
Question 24
1 / -0

Which is the most electropositive element?

A
Na

B
Cu

C
Cs

D
Ca

Solution

The element that belongs to group 1 is the most electropositive. Electropositive character increases down the group.
Question 25
1 / -0

Among the elements with atomic numbers 9, 12, 16 and 36 which is highly electropositive?

A
Element with atomic number 9

B
Element \vith atomic number 12

C
Element with atomic number 16

D
Element with atomic number 36

Solution

Z=9; 1s22s22p5
Z= 12; 1s²2s²2p⁶3s²
Z =16; 1s² 2s² 2p⁶ 3s² 3p⁴
Z = 36: 1s²2s² 2p⁶ 3s² 3p⁶3d¹⁰ 4s²4p⁶
Electropositivity decreases along the period while it increases going down the group.

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Classification of Elements & Periodicity in Properties Test 15

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Classification of Elements & Periodicity in Properties Test 15

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Question 1

It is difficult to add an electron due to small size

It is difficult to add an electron due to high electronegativity

It is difficult to add an electron due to stable configuration

It is difficult to add an electron due to high electron affinity

Solution

Question 2

large size

low electron affinity

high ionisation enthalpy

low chemical reactivity

Solution

Question 3

a

b

c

d

Solution

Question 4

a

b

c

d

Solution

Question 5

Li < Na < K < Rb - Atomic radius

F > N > O > C - Ionisation enthalpy

Si < P < S < Cl - Electronegativity

F < CI < Br < I - Electronegativity

Solution

Question 6

Chemical reactivity tends to be high in group 1 metals, lower in elements in middle and increases to maximum in the group 17

Halogens have very high negative electron gain enthalpy

Noble gases have large positive electron gain enthalpy

Decrease in electronegativities across a period is accompanied by an increase in non-metallic properties

Solution

Question 7

Least ionisation enthalpy on the left and highest negative electron gain enthalpy on the right

Non-metallic character on the left and metallic character on the right

High atomic radii on the left and small atomic radii on the right

Highest electronegativity on the left and least electronegativity oh the right

Solution

Question 8

X2O

XO

XO2

X2O3

Solution

Question 9

PX

PX2

PX3

P2X3

Solution

Question 10

AF3

AF2

AF

AF4

Solution

Question 11

Al2S2

Al3S2

Al2S3

AIS

Solution

Question 12

Representative elements

Transition elements

Noble gases

Non-metals

Solution

X₂O

XO₂

X₂O₃

PX₂

PX₃

P₂X₃

AF₃

AF₂

AF₄

Al₂S₂

Al₃S₂

Al₂S₃

MgN₂, SiO₂

Mg₃N₂, SiO₂

Mg₂N₃, Si₂O₃

MgN, SiO₂

Al₂O₃

CO₂

SiO₂ < P₄O₁₀ < SO₃ < CI₂O₇

Cl₂O₇ < SO₃ < P₄O₁₀ < SiO₂

SO₃ < CI₂O₂ < P₄O₁₀ < SiO₂

SiO₂ < CI₂O₇ < P₄O₁₀ < SO₃

AI₂O₃, As₂O₃, ZnO

CO, NO, N₂O

SO₃, SO₂, CI₂O₇

Na₂O, MgO, BaO