Classification of Elements and Periodicity in Properties Test

Result

Classification of Elements and Periodicity in Properties Test - 6

Score
-
out of -
Rank
-
out of -

TIME Taken - -

SHARING IS CARING

If our Website helped you a little, then kindly spread our voice using Social Networks. Spread our word to your readers, friends, teachers, students & all those close ones who deserve to know what you know now.

Weekly Quiz Competition

Question 1
1 / -0

Ionization enthalpy increases across a period because

A
outermost electrons are held more and more tightly

B
outermost electrons are not held tightly

C
shielding is more effective

D
screening is more effective

Solution

Consider moving from lithium to fluorine across the second period, where successive electrons are added to orbitals in the same principal quantum level. The shielding of the nuclear charge by the inner core of electrons does not increase very much to compensate for the increased attraction of the electron to the nucleus. Thus, across a period, increasing nuclear charge outweighs the shielding. Consequently, the outermost electrons are held more and more tightly and the ionization enthalpy increases across a period.
Question 2
1 / -0

One of the following has ns¹ as its outermost electronic configuration

A
Transition elements

B
Alkaline earth metals

C
Alkali metals

D
Lanthanoids

Solution

The elements of Group 1 (alkali metals) which have ns¹ outermost electronic configuration belong to the s-Block Elements.
Question 3
1 / -0

The correct increasing order of radii of following species is ----?

A
I⁺ < I⁻ < I

B
I < I⁺ < I⁻

C
I⁻ < I⁺ < I

D
I⁺ < I < I⁻

Solution

It is because

(i) radius of anion ( anionic radius ) is greater , and
(ii) radius of cation ( cationic radius ) is lesser than that of its parent neutral atom.
Question 4
1 / -0

Amongst the following elements (whose electronic configurations are given below), the one having the highest ionization enthalpy is

A
[Ne] 3s²3p¹

B
[Ne]3s²3p³

C
[Ne]3s²3p²

D
[Ne]3d¹⁰4s²4p²
Question 5
1 / -0

To which block of elements in the periodic table 3d¹⁰4s² belongs?

A
p- Block

B
f- Block

C
s- Block

D
d- Block

Solution

d-block element have the general outermost electronic configuration as (n-1)d^1-10 ns^0-2.
Question 6
1 / -0

The ionisation enthalpy of lithium is 520 kJ/mol. How much enthalpy is needed to convert all atoms of Li to Li⁺ ions present in 7 mg of Li vapours?

A
74.3 kJ

B
520 kJ

C
520 J

D
780 J
Question 7
1 / -0

In the periodic table Electronegativity generally

A
increases across a period from left to right and decreases down a group

B
increases across a period from left to right and increases down a group

C
decreases across a period from left to right and decreases down a group

D
decreases across a period from left to right and increases down a group

Solution

The electronegativity value increases as the effective nuclear charge on the atomic nucleus increases. In a period moving from left to right, the electronegativity increases due to decrease in atomic radii resulting an increase in effective nuclear charge. Whereas, in a group moving from top to bottom, the electronegativity decreases because atomic radius increases due to subsequent addiiton of shells.
Question 8
1 / -0

Which of the following is a set of isoelectronic species (At. No. of Cs = 55, Br = 35)?

A
N^3-, F^-, Na⁺

B
Be, Al³⁺, Cl^-

C
Ca²⁺, Cs^₊, Br

D
Na⁺, Ca²⁺, Mg²⁺
Question 9
1 / -0

The elements with atomic numbers 9, 17, 35, 53 and 85 are all

A
noble gases

B
halogens

C
heavy metals

D
light metals
Question 10
1 / -0

Identify the correct order in which the ionic radii of the following ions increase:

I. F^-
II. Na⁺
III. N^3-

A
III, I, II

B
I, II, III

C
II, III, I

D
II, I, III

E
III, II, I
Question 11
1 / -0

The correct order of decreasing electronegativity values among the elements I - beryllium, II - oxygen, III - nitrogen and IV - magnesium is

A
II > III > I > IV

B
I > II > III > IV

C
III > IV > II > I

D
II > III > IV > I
Question 12
1 / -0

Consider the ions K⁺, S^2-, Cl^- and Ca²⁺. The radii of these ionic species follow which of the following orders?

A
Ca²⁺ > K⁺ > Cl^- > S^2-

B
Cl^- > S^2- > K⁺ > Ca²⁺

C
Ca²⁺ > Cl^- > K > S^2-

D
S^2- > Cl^- > K⁺ > Ca²⁺
Question 13
1 / -0

The correct order of increasing radii of the elements Na, Rb, K and Mg is

A
Mg, Na, K, Rb

B
Mg, K, Na, Rb

C
Na, K, Rb, Mg

D
Na, Rb, K, Mg
Question 14
1 / -0

The correct order of increasing radii of the elements Na, Si, Al and P is

A
Si, Al, P, Na

B
Al, Si, P, Na

C
P, Si, Al, Na

D
Al, P, Si, Na
Question 15
1 / -0

The polarizing power of the anions N^3-, O^2- and F^-, follows the order

A
N^3- > O^2- > F^-

B
O^2-> N^3- > F^-

C
N^3- > F^-> O^2-

D
O^2- > F^- > N^3-
Question 16
1 / -0

Which of the following orders is not correct according to the property written against it?

A
Al³⁺ < Mg²⁺ < Na⁺ < F^- increasing ionic size

B
B < C < N < O  increasing first ionisation enthalpy

C
I < Br < F < Cl  increasing electron gain enthalpy (with negative sign)

D
Li < Na < K < Rb  increasing metallic radius
Question 17
1 / -0

The ionization enthalpy of nitrogen is more than that of oxygen because of

A
greater attraction of nucleus for the electron

B
extra stability of half filled p-orbitals

C
smaller size of nitrogen atom

D
more penetrating effect

Question 18

1 / -0

Column I	Column II
(a) He	(i) High negative electron gain enthalpy
(b) Cl	(ii) Most electropositive element
(c) Ca	(iii) Strongest reducing agent
(d) Li	(iv) Highest ionisation enthalpy

The correct match of the contents in column I with those in column II is

a - iii, b - i, c - ii, d - iv

a - iv, b - iii, c - ii, d - i

a - ii, b - iv, c - i, d - iii

a - iv, b - i, c - ii, d - iii

Question 19
1 / -0

Which of the following statements is/are correct?

A
1^st and 2^nd IEs of nitrogen are more than 1^st and 2^nd IEs of oxygen.

B
IE of oxygen is greater than IE of nitrogen.

C
IE₂ of oxygen is greater than IE₂ of nitrogen.

D
All of the above
Question 20
1 / -0

Which of the following isoelectronic ions has the lowest ionization energy?

A
K⁺

B
Ca²⁺

C
Cl⁻

D
S²⁻
Question 21
1 / -0

The correct order for the increase in atomic radii is

A
C< Br< I

B
I< Br< Br< F

C
F< C< I< Br

D
F< Cl < Br < I

Solution

In a group movig from top to bottom the number of shells increases. So the atomic size increases. Although the effective nuclear charge increases but its effect is negligible in comparison to the effect of increasing number of shells.
Question 22
1 / -0

The correct order for the decrease in atomic radii is

A
C< Li< Be< B

B
Li< Be< B< C

C
Li< Be< B< C

D
Be< B< C< Li

Solution

In a period moving from left to right, the effective nuclear charge increases because the next electron fills in the same shell. So the atomic size decreases.
Question 23
1 / -0

Choose one of the following in the increasing order of electron gain enthalpy

A
I < Br < F < Cl

B
F < Cl < Br < I

C
Cl < I < Br < F

D
Br < F < Cl < I

Solution

In general as the we move down the group electron gain enthalpy decreases; so the expected trend should be I < Br < Cl < F but in actual the order is I < Br < F < Cl . This is due to small size of F atom. The valence electrons of F atom provide strong repulsion to incoming electron, hence F has unexpectedly low electron affinity.
Question 24
1 / -0

The formation of oxide ion O^2- (g) requires first an exothermic and then an endothermic step as shown below:

O (g) + e^- O^- (g) H_o = - 142 kJ/mol
O^- + e^- O^2- (g) H_o = + 844 kJ/mol

This is because

A
oxygen is more electronegative

B
oxygen has high electron affinity

C
O^- will tend to resist the addition of another electron

D
O^- ion has comparatively larger size than oxygen atom
Question 25
1 / -0

Right order of increasing metallic character is:

A
P < Si < Be < Mg < Na.

B
Si < Be < Mg < Na < P

C
Si < Mg < Na < P < Be

D
Be < Mg < Na < P< Si

Solution

Elements of s block are more matallic than p block elements
Question 26
1 / -0

In which of the following pairs is the first atom or ion not larger than the second?

A
K, K⁺

B
S, O

C
Br, Br^-

D
N, O
Question 27
1 / -0

Which of the following electronic configurations corresponds to the element with the largest negative electron gain enthalpy?

A
1s², 2s², 2p⁵

B
1s², 2s², 2p⁶

C
1s², 2s², 2p⁶, 3s², 3p⁵

D
1s², 2s², 2p⁶, 3s¹
Question 28
1 / -0

One of the following options is not used for explaining atomic radius

A
covalent radius

B
metallic radius

C
coordinate radius

D
van der waals’radius

Solution

The distance from centre of the nucleus to the outermost shell containing the electrons is called atomic radius. There are four types that are widely used: covalent radii, metallic radii, van der Waal's radii and ionic radii.
Question 29
1 / -0

For P^3-, S^2- and Cl^- ions, the increasing order of size is

A
Cl^-, S^2-, P^3-

B
P^3-, S^2-, Cl^-

C
S^2-, Cl^-, P^3-

D
S^2-, P^3-, Cl^-
Question 30
1 / -0

Directions: The following question has four choices out of which ONLY ONE is correct.

Which of the following processes requires the highest energy?

A
Al (g) Al⁺ (g) + e^-

B
Al²⁺ (g) Al³⁺ (g) + e^-

C
Al⁺ (g) Al²⁺ (g) + e^-

D
Energy required is the same in all the three processes.

User

Question Analysis

Correct -
Wrong -
Skipped -

My Perfomance

Score
-
out of -
Rank
-
out of -

Re-Attempt Weekly Quiz Competition

Classification of Elements and Periodicity in Properties Test - 6

Result

Classification of Elements and Periodicity in Properties Test - 6

Score

-

Rank

-

SHARING IS CARING

Question 1

outermost electrons are held more and more tightly

outermost electrons are not held tightly

shielding is more effective

screening is more effective

Solution

Question 2

Transition elements

Alkaline earth metals

Alkali metals

Lanthanoids

Solution

Question 3

I+ < I− < I

I < I+ < I−

I− < I+ < I

I+ < I < I−

Solution

Question 4

[Ne] 3s23p1

[Ne]3s23p3

[Ne]3s23p2

[Ne]3d104s24p2

Question 5

p- Block

f- Block

s- Block

d- Block

Solution

Question 6

74.3 kJ

520 kJ

520 J

780 J

Question 7

increases across a period from left to right and decreases down a group

increases across a period from left to right and increases down a group

decreases across a period from left to right and decreases down a group

decreases across a period from left to right and increases down a group

Solution

Question 8

N3-, F-, Na+

Be, Al3+, Cl-

Ca2+, Cs+, Br

Na+, Ca2+, Mg2+

Question 9

noble gases

halogens

heavy metals

light metals

Question 10

III, I, II

I, II, III

II, III, I

II, I, III

III, II, I

Question 11

II > III > I > IV

I > II > III > IV

III > IV > II > I

II > III > IV > I

Question 12

Ca2+ > K+ > Cl- > S2-

Cl - > S2- > K+ > Ca2+

Ca2+ > Cl- > K > S2-

S2- > Cl- > K+ > Ca2+

Question 13

Mg, Na, K, Rb

Mg, K, Na, Rb

Na, K, Rb, Mg

Na, Rb, K, Mg

Question 14

I⁺ < I⁻ < I

I < I⁺ < I⁻

I⁻ < I⁺ < I

I⁺ < I < I⁻

[Ne] 3s²3p¹

[Ne]3s²3p³

[Ne]3s²3p²

[Ne]3d¹⁰4s²4p²

N^3-, F^-, Na⁺

Be, Al³⁺, Cl^-

Ca²⁺, Cs^₊, Br

Na⁺, Ca²⁺, Mg²⁺

Ca²⁺ > K⁺ > Cl^- > S^2-

Cl^- > S^2- > K⁺ > Ca²⁺

Ca²⁺ > Cl^- > K > S^2-

S^2- > Cl^- > K⁺ > Ca²⁺

N^3- > O^2- > F^-

O^2-> N^3- > F^-

N^3- > F^-> O^2-

O^2- > F^- > N^3-

Al³⁺ < Mg²⁺ < Na⁺ < F^- increasing ionic size

1^st and 2^nd IEs of nitrogen are more than 1^st and 2^nd IEs of oxygen.

IE₂ of oxygen is greater than IE₂ of nitrogen.

K⁺

Ca²⁺

Cl⁻

S²⁻

O^- will tend to resist the addition of another electron

O^- ion has comparatively larger size than oxygen atom

K, K⁺

Br, Br^-

1s², 2s², 2p⁵