Classification of Elements and Periodicity in Properties Test

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Classification of Elements and Periodicity in Properties Test - 11

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Weekly Quiz Competition

Question 1
1 / -0

The tenth elements in the periodic table resembles with the

A
First period

B
Second period

C
Fourth group

D
Ninth group

Solution

Each period consists of a series of elements whose atom have the same principal quantum no. (n) of the outer most shell i.e. In second period n = 2, this shell has four orbitals (one 2s and three 2p) which can have eight electrons, hence second period contains 8 elements from atomic no. 3 to 10.
Question 2
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Who developed the long form of periodic table

A
Lothar Meyer

B
Niels Bohr

C
Mendeleev

D
Moseley

Solution

Niels Bohr developed the long form of periodic table on the basis of Mosley’s principle.
Question 3
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In the periodic table, the element with atomic number 16 will be placed in the group

A
Third

B
Fourth

C
Fifth

D
Sixth

Solution

\(16-1s^22s^22p^63s^23p^4\) there are 6e− in outer most shell therefore its group is \(VI^{th}A\).
Question 4
1 / -0

Which of the following is the atomic number of a metal?

A
32

B
34

C
36

D
38

Solution

38 is the atomic no. of strontium (Sr) which is s-block element and all the elements of s-block are metals.
Question 5
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Which is smallest in size?

A
\(O^{2-}\)

B
\(C^{4-}\)

C
\(F^-\)

D
\(N^{3-}\)

Solution

As the nuclear charge per electron is maximum in \(F^-\). Therefore it is smallest in size.
Question 6
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Which of the following property displays progressive increase down a group in the Bohr’s periodic table?

A
Electronegativity

B
Electron affinity

C
Ionization potential

D
Size of the atom

Solution

In completely filled shell inter atomic repulsion is more so have greater size.
Question 7
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Which has the maximum atomic radius?

A
Al

B
Si

C
P

D
Mg

Solution

Mg, as we move across the period atomic radius decreases.
Question 8
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Which one of the following is the smallest in size?

A
\(N^{3-}\)

B
\(O^{2-}\)

C
\(F^-\)

D
\(Na^+\)

Solution

\(Na^+ <F^-<O^{2-} <N^{3-}\)All are isoelectronic, effective number charge is highest for \(Na^+\) so it has smallest size.
Question 9
1 / -0

In halogens, with the increase of atomic number which habit is found

A
Habit to loose electrons decreases

B
Habit to loose electrons decreases

C
Ionization potential decreases

D
In \(MX_2 \)(M= metal and X= halogen), covalent properties decreases.

Solution

Ionization potential decreases. Since, atomic size increases.
Question 10
1 / -0

How many ionization energies can carbon have

A
1

B
2

C
4

D
6

Solution

The energy required to remove an electron from outermost orbit of an isolated gaseous atom is called I.E. Now carbon has 4e− in outermost shell. Thus it has 4 ionization energies.
Question 11
1 / -0

Which of the following has least ionization potential?

A
Li

B
Cs

C
Cl

D
I

Solution

Li and \(A_2B_3\) belong to Ist group but Cs has larger size, hence low nuclear attraction force, thus low ionization energy.
Question 12
1 / -0

The solubilities of carbonates decreases down the magnesium group due to a decrease in

A
Lattice energies of solids

B
Hydration energies of cations

C
Inter-ionic attraction

D
Entropy of solution formation

Solution

Due to decrease in hydration energy of cation and lattice energy remains almost unchanged.
Question 13
1 / -0

In third row of periodic table from Na to Cl

A
Electronegativity increases

B
Electronegativity decreases

C
Ionization energy decreases

D
Atomic volume increases

Solution

Electronegativity increases since the size decreases.
Question 14
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Which element has the lowest electronegativity?

A
Li

B
F

C
Fe

D
Cl

Solution

\(Li_3 - 1s^22s^1 \)donates \(1e^-\) easily.
Question 15
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Strongest acid is

A
\(Al_2O_3\)

B
\(MgO\)

C
\(Na_2O\)

D
\(CaO\)

Solution

The basic nature of oxide decreases across the period as metallic character decreases. Therefore acidic nature of oxide increases.
Question 16
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The electronic configuration of an element is. The atomic number and the group number of the element 'X' which is just below the above element in the periodic table are respectively

A
23 and 5

B
23 and 15

C
33 and 15

D
33 and 5

Solution

Atomic number of the given element =15; atomic number of element 'X' will be 18 + 15 =33; group no. of ′X′= 10 + 5 (valence electrons) = 15, period = 4th.
Question 17
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Which of the following have high electron affinity?

A
F

B
Cl

C
N

D
O

Solution

The electron affinities of some of the elements of second period (i.e., N, O, F etc.) are however, lower than the corresponding elements (i.e., P, S, Cl, etc.) of the third period. This is due to the reason that the elements of second period have the smallest atomic size amongst the elements in their respective groups.

As a result, there is considerable electron-electron repulsion within the atom itself and hence the additional electron is not accepted with the same ease as is the case with the remaining elements in the same group.
Question 18
1 / -0

Which has highest melting point?

A
\(LiCl\)

B
\(BeCl_2\)

C
\(BCl_3\)

D
\(CCl_4\)

Solution

In \(BeCl_2\) has the highest melting point due to ionic bond.
Question 19
1 / -0

The elements with zero electron affinity are

A
Boron and Carbon

B
Beryllium and Helium

C
Lithium and Sodium

D
Fluorine and Chlorine

Solution

Fully filled electronic configuration.
Question 20
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The set of three elements having successive atomic numbers and having the ionization energies of 2372, 520 and 890 kJ per mol is:

A
H, He, Li

B
He, Li, Be

C
Li, Be, B

D
B, C, N

Solution

He (Z = 2) is a noble gas and has highest I.E. The I.E. of Be (Z = 4) is more than that of Li (Z=3)

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Classification of Elements and Periodicity in Properties Test - 11

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Classification of Elements and Periodicity in Properties Test - 11

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Question 1

First period

Second period

Fourth group

Ninth group

Solution

Question 2

Lothar Meyer

Niels Bohr

Mendeleev

Moseley

Solution

Question 3

Third

Fourth

Fifth

Sixth

Solution

Question 4

32

34

36

38

Solution

Question 5

\(O^{2-}\)

\(C^{4-}\)

\(F^-\)

\(N^{3-}\)

Solution

Question 6

Electronegativity

Electron affinity

Ionization potential

Size of the atom

Solution

Question 7

Al

Si

P

Mg

Solution

Question 8

\(N^{3-}\)

\(O^{2-}\)

\(F^-\)

\(Na^+\)

Solution

Question 9

Habit to loose electrons decreases

Habit to loose electrons decreases

Ionization potential decreases

In \(MX_2 \)(M= metal and X= halogen), covalent properties decreases.

Solution

Question 10

1

2

4

6

Solution

Question 11

Li

Cs

Cl

I

Solution

Question 12

Lattice energies of solids

Hydration energies of cations

Inter-ionic attraction

Entropy of solution formation

Solution