Classification of Elements & Periodicity in Properties Test 4

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Classification of Elements & Periodicity in Properties Test 4

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Question 1
1 / -0

f block of the Periodic Table consists of

A
The first two groups of the periodic table

B
halogens (Group 17) and the chalcogens (Group 16)

C
Groups 13 and 14 “Transition Elements”.

D
The two rows of elements at the bottom of the Periodic Table, called the Lanthanides, Ce(Z = 58) ñ Lu(Z = 71) and Actinoids

Solution

Lanthanides, Ce(Z = 58) ñ Lu(Z = 71) and Actinoids comprises of f block elements.
Question 2
1 / -0

The elements charecterised by the filling of 4 f-orbitals, are:

A
Alkali metals

B
Lanthanoids

C
Alkaline earth metals

D
Transition elements)

Solution

Elements characterized by the filling of 4f orbitals are lanthanides.
Question 3
1 / -0

14 elements after actinium is called

A
Lanthanides

B
Actinides

C
D-block elements

D
P block elements

Solution

The correct answer is Option B.
14 elements after actinium is called Actinides.
Question 4
1 / -0

An element belongs to Group 15 and third period of the periodic table. Its electronic configuration will be

A
1s²2s²2p⁶3s²3p³

B
1s²2s²2p³

C
1s²2s²2p⁴

D
1s²2s²2p⁶3s²3p²

Solution

group is 15 so total valence electrons will be 5 while period is 3rd so n value of valence shell will be 3.
Question 5
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It is now recognized that the ‘Modern Periodic Law’ is essentially the consequence of the

A
periodic variation in electronic configurations

B
periodic variations in the element lattice

C
periodic variation in chemical bonds

D
periodic variation in chemical properties

Solution

Modern periodic law is essentially the result of periodic variation and electronic configuration.
Question 6
1 / -0

Metalloids show the properties of

A
properties that are characteristic of both metals and viscous liquids

B
properties that are characteristic of both metals and plastics

C
properties that are characteristic of both metals and nonmetals

D
properties that are characteristic of both metals and gases

Solution

Metalloids shows both the properties of metals as well as non metals.
Question 7
1 / -0

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

A
coordinate radius

B
covalent radius

C
van der waals’radius

D
metallic radius

Solution

coordinate radius is not used for explaining atomic radius.
Question 8
1 / -0

Among the alkali metals cesium is the most reactive because

A
it has a single electron in the valence shell

B
the outermost electron is more loosely bound than the outermost electron of the other alkali metals

C
it is the heaviest alkali metal

D
its incomplete shell is nearest to the nucleus

Solution

Among the alkali metals cesium is the most reactive because the outermost electron is more loosely bound than the outermost electron of the other alkali metals.
Question 9
1 / -0

In which one of the given formulae of xenon compounds there are five α−bonds and three π-bonds in it?

A
XeF₃O₂

B
XeFO

C
XeF₂O₂

D
XeF₂O₃

Solution
Question 10
1 / -0

In the modern periodic table

A
The horizontal rows are called series and the vertical columns, groups.

B
The horizontal rows are called periods and the vertical columns, groups.

C
The horizontal rows are called groups and the vertical columns, periods

D
The horizontal rows are called periods and the vertical columns, series.

Solution

Horizontal rows are periods while vertical column are groups.
Question 11
1 / -0

Which of the following statements is false?

A
Alkali metals form covalent bonds with oxygen.

B
Alkali metals have relatively low first ionization energies

C
Alkali metals forms oxides that act as basic anhydrides.

D
Alkali metals usually have a +1 oxidation state

Solution

Alkali metals always form ionic bonds.
Question 12
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The order of Decreasing radius is

A
Van der Waals’radius > Metallic radius > Covalent radius

B
Covalent radius > Van der Waals’radius

C
Metallic radius > Van der Waals’radius > Covalent radius

D
Van der Waals’radius > Covalent radius > Metallic radius

Solution

vanderwaal radius > Metallic radius > Covalent radius.
Question 13
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For alkali metals, which one of the following trends is INCORRECT?

A
Hydration energy: Li > Na > K > Rb

B
Ionization energy: Li > Na > K > Rb

C
Atomic size: Li < Na < K < Rb

D
Density: Li < Na < K < Rb

Solution

Actual trend of density is Li < K < Na < Rb
Question 14
1 / -0

Dmitri Mendeleev (1834-1907) and the German chemist, Lothar Meyer (1830-1895) proposed arranging elements in

A
increasing order of their atomic weights

B
decreasing order of their atomic weights

C
decreasing order of their atomic numbers

D
increasing order of their atomic numbers

Solution

They arranged elements in increasing order of atomic weights.
Question 15
1 / -0

According to the recommendation of International Union of Pure and Applied Chemistry (IUPAC), the groups in the modern periodic table are numbered from

A
1 to 10

B
1 to 12

C
1 to 18

D
1 to 8

Solution

they are numbered from 1 to 18 1 is alkali metal group and 18 is noble gases.
Question 16
1 / -0

Ionization enthalpy increases across a period because

A
outermost electrons are held more and more tightly

B
screening is more effective

C
outermost electrons are not held tightly

D
shielding is more effective

Solution

as we move from left to right in a period atomic radii decreases and due to effective nuclear charge outermost electrons are held more closely to the nucleus.
Question 17
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Choose one of the following in th increasing order of bond length

A
F₂< N₂< Cl₂< O₂

B
Cl₂ < O₂ < N₂ < F₂

C
F₂ < Cl₂ < O₂ < N₂

D
N₂ < O₂ < F₂ < Cl₂

Solution

As the size increases bond length also increases.
Question 18
1 / -0

For the four successive transition elements (Cr, Mn, Fe and Co), the stability of + 2 oxidation state will be there in which of the following order? (At. nos. Cr = 24, Mn = 25, Fe = 26, Co = 27)

A
Fe > Mn > Co > Cr

B
Mn > Fe > Cr > Co

C
Cr > Mn > Co > Fe

D
Co > Mn > Fe > Cr

Solution

Mn has most stable +2 stable because Mn+2 had d5 configuration which is most stable.
Question 19
1 / -0

A transition metal ion exists in its highest oxidation state. It is expected to behave as

A
a chelating agent

B
a central metal in a coordination compound

C
an oxidising agent

D
a reducing agent

Solution

When a transition metal ion is in highest oxidation state it tends to lower its oxidation state by gaining electrons. thus it itself reduces and oxidizes the substance from which it accepts electron. So, it acts as oxidising agent.
Question 20
1 / -0

The sequence of ionic mobility in aqueous solution is

A
K⁺ > Na⁺ > Rb⁺ > Cs⁺

B
Cs⁺ > Rb⁺ > K⁺ >Na⁺

C
Rb⁺ > K⁺> Cs⁺ > Na⁺

D
Na⁺ > K⁺ >Rb⁺ >Cs⁺

Solution

Smaller the size of cation, higher will be the hydration and its effective size will increase and hence mobility in aqueous solution will decrease. Larger size ions have more ionic mobility due to less hydration. Thus the degree of hydration of M⁺ ions decreases from Li⁺ to Cs⁺. Consequently the radii of the hydrated ion decreases from Li⁺ to Cs⁺. Hence the ionic conductance of these hydrated ions increases from Li⁺ to Cs⁺
Question 21
1 / -0

In the periodic table Electronegativity generally

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

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

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

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

Solution

electronegativity increases on moving from left to right while decreases as we move down the group.
Question 22
1 / -0

Al(3+)

A
the same number of electrons (9 electrons).

B
isoelectronic species

C
the same number of electrons (8 electrons).

D
the same number of electrons (7 electrons).

Solution

They are isoelectronic species with same number of electrons. Higher is the atomic number, higher will be the effective nuclear charge, lower will be the size.
Question 23
1 / -0

Generally, the first ionization energy increases along a period. But there are some exceptions. One which is NOT an exception is ______.

A
Na and Mg

B
Mg and Al

C
N and O

D
Be and B

Solution

Na and Mg are not an exception.
Question 24
1 / -0

Which of the following will have the most negative electron gain enthalpy and which one the least negative? P, S, Cl, F.

A
Cl, P

B
P,Cl

C
P,S

D
none

Solution

Cl just need one more electrons to get fully filled electronic configuration so it has most negative electron gain enthalpy while P has d3 configuration which is already stable so it cannot accept one electron extra easily so have large positive electron gain enthalpy.
Question 25
1 / -0

For Atomic numbers greater than 100 IUPAC has made recommendation that until a new element ‘s discovery is proved, and its name is officially recognized, a systematic nomenclature be derived directly from the atomic number of the element using the numerical roots for 0 and numbers 1-9. The name 'sept' in this scheme corresponds to the digit

A
3

B
8

C
4

D
7.0

Solution

sept is for 7.

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Classification of Elements & Periodicity in Properties Test 4

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Question 1

The first two groups of the periodic table

halogens (Group 17) and the chalcogens (Group 16)

Groups 13 and 14 “Transition Elements”.

The two rows of elements at the bottom of the Periodic Table, called the Lanthanides, Ce(Z = 58) ñ Lu(Z = 71) and Actinoids

Solution

Question 2

Alkali metals

Lanthanoids

Alkaline earth metals

Transition elements)

Solution

Question 3

Lanthanides

Actinides

D-block elements

P block elements

Solution

Question 4

1s22s22p63s23p3

1s22s22p3

1s22s22p4

1s22s22p63s23p2

Solution

Question 5

periodic variation in electronic configurations

periodic variations in the element lattice

periodic variation in chemical bonds

periodic variation in chemical properties

Solution

Question 6

properties that are characteristic of both metals and viscous liquids

properties that are characteristic of both metals and plastics

properties that are characteristic of both metals and nonmetals

properties that are characteristic of both metals and gases

Solution

Question 7

coordinate radius

covalent radius

van der waals’radius

metallic radius

Solution

Question 8

it has a single electron in the valence shell

the outermost electron is more loosely bound than the outermost electron of the other alkali metals

it is the heaviest alkali metal

its incomplete shell is nearest to the nucleus

Solution

Question 9

XeF3O2

XeFO

XeF2O2

XeF2O3

Solution

Question 10

The horizontal rows are called series and the vertical columns, groups.

The horizontal rows are called periods and the vertical columns, groups.

The horizontal rows are called groups and the vertical columns, periods

The horizontal rows are called periods and the vertical columns, series.

Solution

Question 11

Alkali metals form covalent bonds with oxygen.

Alkali metals have relatively low first ionization energies

Alkali metals forms oxides that act as basic anhydrides.

Alkali metals usually have a +1 oxidation state

Solution

Question 12

Van der Waals’radius > Metallic radius > Covalent radius

Covalent radius > Van der Waals’radius

Metallic radius > Van der Waals’radius > Covalent radius

Van der Waals’radius > Covalent radius > Metallic radius

Solution

1s²2s²2p⁶3s²3p³

1s²2s²2p³

1s²2s²2p⁴

1s²2s²2p⁶3s²3p²

XeF₃O₂

XeF₂O₂

XeF₂O₃

F₂< N₂< Cl₂< O₂

Cl₂ < O₂ < N₂ < F₂

F₂ < Cl₂ < O₂ < N₂

N₂ < O₂ < F₂ < Cl₂

K⁺ > Na⁺ > Rb⁺ > Cs⁺

Cs⁺ > Rb⁺ > K⁺ >Na⁺

Rb⁺ > K⁺> Cs⁺ > Na⁺

Na⁺ > K⁺ >Rb⁺ >Cs⁺