Classification of Elements and Periodicity in Properties Test

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Classification of Elements and Periodicity in Properties Test - 5

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Weekly Quiz Competition

Question 1
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The atomic numbers of vanadium (V), chromium (Cr), iron (Fe) and Cobalt (Co) are 23, 24, 26 and 27, respectively. Which one of these may be expected to have the highest second ionisation enthalpy?

A
V

B
Cr

C
Co

D
Fe
Question 2
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Electronic configuration of an element is:

A
The distribution of electrons into different atomic orbitals.

B
The distribution of electrons into magnetic states of an atom

C
The distribution of electrons into spin state of an atom

D
The distribution of electrons into azimuthal orbitals of an atom only

Solution

The electronic configuration of an atom, describes the arrangement of electrons in space around the nucleus. The electrons are distributed over different energy level. These energy levels are called the shell or orbits.
Question 3
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d-Block Elements are characterized by the

A
inner d orbitals are not filled

B
filling of outer d orbitals

C
absence of d orbital electrons

D
filling of inner d orbitals by electrons

Solution

d-Block elements also known as transition elements are characterized by the filling of inner d orbitals by electrons before the valence-shell s orbital.
Question 4
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If the valence shell electronic structure of an element is ns²np⁵, then the element will belong to the group of

A
alkali metals

B
halogens

C
alkaline earth metals

D
noble gases
Question 5
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Atomic number of element Unnilhexium is:

A
110

B
107

C
106

D
105

Solution

un=1 Nil=0 Hex=6 So 106=uninilhexium.
Question 6
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Which of the following statements is false?

A
Alkali metals form covalent bonds with oxygen.

B
Alkali metals usually have a +1 oxidation state

C
Alkali metals forms oxides that act as basic anhydrides.

D
Alkali metals have relatively low first ionization energies

Solution

The elements of Group 1 (alkali metals) have ns1 as outermost electronic configuration. They are all reactive metals with low ionization enthalpies. They lose the outermost electron readily to form 1+ ion. The compounds of the alkali, with the exception of those of lithium are predominantly ionic.
Question 7
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Which of the following statements is correct?

A
The ionic radius of a metal is same as its atomic radius.

B
The ionic radius of a metal is greater than its atomic radius.

C
The ionic radius of non-metal is less than its atomic radius.

D
The ionic radius of a metal is less than atomic radius of parent atom.
Question 8
1 / -0

According to IUPAC nomenclature for elements with Z greater than 100,the root 'sept' corresponds to the digit:

A
3

B
7

C
4

D
8

Solution
Question 9
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To which group of the periodic table does the element with electronic configuration 1s², 2s², 2p⁶, 3s², 3p⁶, 3d¹⁰, 4s², 4p⁶, 4d¹⁰, 5s², 5p³ belong?

A
13

B
12

C
15

D
17
Question 10
1 / -0

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

Which of the following orders of elements is correct in terms of decreasing ionization enthalpies?

A
Na > Li > H

B
H > Li > Na

C
Li > H > Na

D
Na > H > Li
Question 11
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Which of the following elements has the greatest tendency to lose electrons?

A
F

B
S

C
Fr

D
C
Question 12
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Directions: The following question has four choices out of which ONLY ONE is correct.

The element whose configuration is 1s², 2s², 2p⁶, 3s²is

A
a metal

B
a metalloid

C
an inert gas

D
a non-metal
Question 13
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Directions: The following question has four choices out of which ONLY ONE is correct.

The first four ionisation energy values of an element are 191, 578, 872 and 5962 kcal. The number of valence electrons in the element is

A
1

B
2

C
3

D
4
Question 14
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Which of the following elements is a metalloid?

A
Si

B
C

C
Bi

D
Sn
Question 15
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The elements with atomic numbers 4, 12, 20, 38 and 56 belong to the group of

A
alkali metals

B
alkaline earth metals

C
halogens

D
noble gases
Question 16
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Select the pair(s) showing diagonal relationship.

A
Li-Mg

B
Be-Al

C
B-Si

D
All of the above
Question 17
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The electronic configurations of four elements are given as follows.

(1) [Xe] 6s¹(2) [Xe] 4f¹⁴, 5d¹, 6s²(3) [Ar] 4s², 4p⁵(4) [Ar] 3d⁷, 4s²Which of the following statements about these elements is incorrect?

A
[Xe] 6s¹ is a strong reducing agent.

B
[Xe] 4f¹⁴, 5d¹, 6s² is a d-block element.

C
[Ar] 4s², 4p⁵ has high electron affinity.

D
[Ar] 3d⁷, 4s² shows variable oxidation state.
Question 18
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Which of the following ions has the highest value of ionic radius?

A
Li⁺

B
B³⁺

C
O^2-

D
F^-
Question 19
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Which of the following series of elements is correct in terms of increasing atomic radii?

A
F < Cl < Br

B
Li < K < Na

C
Ca < Mg < Be

D
N < As < P
Question 20
1 / -0

The ionisation energy of hydrogen atom is 13.6 eV. What will be the ionisation energy of He⁺?

A
13.6 eV

B
54.4 eV

C
122.4 eV

D
0 eV
Question 21
1 / -0

According to IUPAC nomenclature,element Ununnillium have an atomic number of:

A
109

B
111

C
108

D
110

Solution

un=1 nil=0 So 110 = ununnilium.
Question 22
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s-block elements comprise of

A
Group 4 (alkali metals) and Group 7 (alkaline earth metals)

B
Group 1 and Group 4

C
Group 3 and Group 2

D
Group 1 (alkali metals) and Group 2 (alkaline earth metals).

Solution

s-block contains two group of elements including alkali earth metal and alkaline earth metal.
Question 23
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Iron triad of elements also contains

A
cobalt and nickel

B
manganese and chromium

C
palladium and platinum

D
platinum and iridium
Question 24
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The third period (n = 3) begins at sodium with addition of first electron to

A
3p orbital

B
2s orbital

C
2p orbital

D
3s orbital

Solution

The electronic configuration of sodium is 1s² 2s² 2p⁶ 3s¹. The valence electron is in 3s orbital.
Question 25
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The screening effect of s orbital electron is

A
greater than that of p, but lesser than that of d and f electrons

B
lesser than that of p, d and f electrons

C
greater than that of p, d and f electrons

D
equal to that of p, d and f electrons
Question 26
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Diagonal relationship in the periodic table is shown by the elements of

A
first and second periods

B
second and third periods

C
third and fourth periods

D
None of these
Question 27
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Maximum number of electrons occupied by s,p and d orbitlas are:

A
2, 6 and 10

B
2, 8, 8

C
2, 10, 10

D
2, 2, 8

Solution

s-orbital ml=0, so it can accommodate 2 electron.
p-orbital has ml = -1,0,+1. It can accommodate 6 electrons.
d-orbital has ml = -2,-1,0,1,2.It can accommodate 10 electrons.
Question 28
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If we have an element with atomic number 115, then which of the following statements is correct about this element?

A
It will be an s-block element.

B
It will be a p-block element.

C
It will be a d-block element.

D
It will be an actinide.
Question 29
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From the ground state of electronic configuration of various electrons, which will have the highest second ionisation energy?

A
1s², 2s², 2p⁶, 3s²

B
1s², 2s², 2p⁶, 3s¹

C
1s², 2s², 2p⁶

D
1s², 2s², 2p⁵
Question 30
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Metalloids show the properties of

A
properties that are characteristic of both metals and plastics

B
properties that are characteristic of both metals and nonmetals.

C
properties that are characteristic of both metals and gases

D
properties that are characteristic of both metals and viscous liquids

Solution

A metalloid is any chemical element which has properties in between those of metals and nonmetals, or that has a mixture of them. Typical metalloids have a metallic appearance, but they are brittle and only fair conductors of electricity. Chemically, they behave mostly as nonmetals. They can form alloys with metals. Most of their other physical and chemical properties are intermediate in nature. The six commonly recognised metalloids are boron, silicon, germanium, arsenic, antimony, and tellurium.

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Classification of Elements and Periodicity in Properties Test - 5

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Classification of Elements and Periodicity in Properties Test - 5

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Question 1

V

Cr

Co

Fe

Question 2

The distribution of electrons into different atomic orbitals.

The distribution of electrons into magnetic states of an atom

The distribution of electrons into spin state of an atom

The distribution of electrons into azimuthal orbitals of an atom only

Solution

Question 3

inner d orbitals are not filled

filling of outer d orbitals

absence of d orbital electrons

filling of inner d orbitals by electrons

Solution

Question 4

alkali metals

halogens

alkaline earth metals

noble gases

Question 5

110

107

106

105

Solution

Question 6

Alkali metals form covalent bonds with oxygen.

Alkali metals usually have a +1 oxidation state

Alkali metals forms oxides that act as basic anhydrides.

Alkali metals have relatively low first ionization energies

Solution

Question 7

The ionic radius of a metal is same as its atomic radius.

The ionic radius of a metal is greater than its atomic radius.

The ionic radius of non-metal is less than its atomic radius.

The ionic radius of a metal is less than atomic radius of parent atom.

Question 8

3

7

4

8

Solution

Question 9

13

12

15

17

Question 10

Na > Li > H

H > Li > Na

Li > H > Na

Na > H > Li

Question 11

F

S

Fr

C

Question 12

a metal

a metalloid

an inert gas

a non-metal

Question 13

1

2

3

4

Question 14

Si

[Xe] 6s¹ is a strong reducing agent.

[Xe] 4f¹⁴, 5d¹, 6s² is a d-block element.

[Ar] 4s², 4p⁵ has high electron affinity.

[Ar] 3d⁷, 4s² shows variable oxidation state.

Li⁺

B³⁺

O^2-

F^-