Classification of Elements and Periodicity in Properties Test

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Classification of Elements and Periodicity in Properties Test - 50

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Weekly Quiz Competition

Question 1
1 / -0

Elements of which of the following group $$\left ( s \right )$$ of periodic table do not from hydrides.

A
group 7,8,9

B
group 13

C
group 15,16,17

D
group 14

Solution

The metals from group $$7,8,9$$ do not form hydrides and the element $$Cr$$,the only element in group $$6$$ which forms hydride.
Question 2
1 / -0

Which of the following is incorrect statement?

A
The electron affinity of Si is greater than that of phosphorous

B
Penetration power of p-orbital is more than s-orbital

C
Second ionisation energy of sodium is more than Mg.

D
The numerical value of electronegativity of an atom depends on its ionisation potential and electron affinity.

Solution

$$(B)$$ is the incorrect statement. Penetration of $$s$$-orbital is much more than $$p$$-orbital$$,$$ since $$s$$ is spherical in shape and get contracted more upon increasing $${Z}_{eff}.$$
Question 3
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Four elements $$P,\ Q,\ R,\ S$$ have atomic numbers $$Z-1,\ Z,\ Z+1$$ and $$Z+2$$ respectively. If $$Z$$ is 17, then bond between which pair of elements will be most ionic?

A
$$S$$ and $$Q$$

B
$$P$$ and $$R$$

C
$$S$$ and $$R$$

D
$$S$$ and $$P$$

Solution

Solution:- (A) $$S$$ and $$Q$$
Given:-
$$Z = 17$$
Therefore,
Atomic no. of $$P = Z - 1 = 16$$
Electronic configuration $$= 2, 8, 6$$
Atomic no. of $$Q = Z = 17$$
Electronic configuration $$= 2, 8, 7$$
Atomic no. of $$R = Z + 1 = 18$$
Electronic configuration $$= 2, 8, 8$$
Atomic no. of $$S = Z + 1 = 19$$
Electronic configuration $$= 2, 8, 1$$
The element $$P$$ belongs to oxygen family and requires $$2$$ electrons to complete it's octet.
The element $$Q$$ belongs to halogen family and requires only $$1$$ electron to complete its octet.
The element $$R$$ belongs to the inert gas family.
The element $$S$$ belongs to alkali metal family requires to lose $$1$$ electron to get its complete octet.
Hence the bond between $$S$$ and $$Q$$ will be most ionic.
Question 4
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Which of the following has the least electron affinity?

A
$$Na$$

B
$$Ca$$

C
$$K$$

D
$$F$$
Solution
- The electron affinity of an atom or molecule is defined as the amount of energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion.
- The less valence electrons an atom has, the least likely it will gain electrons. Electron affinity decreases down the groups and from right to left across the periods on the periodic table because the electrons are placed in a higher energy level far from the nucleus, thus a decrease from its pull.
- Considering the trends we find $$Na$$ will be having least electron affinity as $$Na$$ readily looses its electron to form stable $$Na^{+}$$.
Question 5
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Which of the following pair has electron deficient compounds?

A
$$B_2H_6, \ AlCl_3$$

B
$$C_2H_6, \ Al_2Cl_6$$

C
$$SF_2, \ Cl_2O$$

D
$$NaBH_4, \ ICl$$

Solution

(Refer to Image 1)
In Diborane structure, each Boron bonds with $$4$$ hydrogen atoms. But Boron valency is $$3$$. Each Boron gives $$3$$ valence electrons but for the $$4^{th}$$ bond, there is no electron from Boron side which makes it electron deficient.
(Refer to Image 2)
In $$AlCl_3$$, $$Al$$ atom bonds with $$3$$ $$Cl$$ atoms. But here it violates octet rule. There are no bonds or lone pairs, which makes the surrounding electron count $$8$$. It has only $$3$$ bonds which makes $$6$$ electrons. So, it is an electron deficient compound. So, both $$AlCl_3$$ and $$B_2H_6$$ are electron deficient compounds.
Question 6
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General electronic configuration of outermost and penultimate shell is $$\left( {n - 1} \right)\,\,{s^2}\,\,\left( {n - 1} \right){p^{6\,\,}}\left( {n - 1} \right)\,{d^x}\,\,n{s^2}$$. If $$n = 4$$ and $$x = 5$$ then number of protons in the nuleus will be :-

A
$$ > \,\,25$$

B
$$ < \,\,24$$

C
$$25$$

D
$$30$$

Solution

Given $$ n = 4 \times = 5 $$

So $$ \begin{matrix}(4-1)s^2 \\ 3s^2 \end{matrix}\begin{matrix} (4-1)p^6 \\ 3p^6 \end{matrix}\begin{matrix} (4-1)d^5 \\ 3d^5 \end{matrix}\begin{matrix} 4s^2 \\ 4s^2 \end{matrix} $$

Total electrons $$= 2 + 6 + 5 + 2 = 15$$

Electrons in 1st and 2nd orbit $$= 2 + 8 = 10$$

Total electrons $$= 10 + 15 = 25$$

No. of electrons $$=$$ no. of protons

So, total protons $$= 25$$
Question 7
1 / -0

Which of the following contains three centre and two electron bonds?

A
1)(BeH2)2

B
(2) LiAlH4

C
3) (BeCl2)2

D
4) Li2C2

Solution

A three-center two-electron bond is an electron-deficient chemical bond where three atoms share two electrons. The combination of three atomic orbitals form three molecular orbitals: one bonding, one non-bonding, and one anti-bonding. The two electrons go into the bonding orbital, resulting in a net bonding effect and constituting a chemical bond among all three atoms. In many common bonds of this type, the bonding orbital is shifted towards two of the three atoms instead of being spread equally among all three.
Question 8
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Which of the following group bear maximum number of elements?

A
$$ 3^{rd} $$ group

B
$$ 2^{nd} $$ group

C
$$ 18^{th} $$ group

D
$$ 13^{th} $$ group

Solution

Since the third group contains $$d$$-block as well as $$f$$-block elements also which are much more than any group elements .
Question 9
1 / -0

Which of the following order is correct?

A
$$S (E.A.) < O(E.A.)$$

B
$$Hg (I.E.) < Cd (I.E.)$$

C
$$P(I.E.)> S (I.E.)$$

D
Both (B) and (C) are correct
Question 10
1 / -0

In period $$2$$, element $$'A'$$ is to the right of element $$'B'$$.Compare the following properties of A and B.

A
The element $$'A'$$ would probably have a______[smaller/larger] atomic size than $$'B'$$.

B
The element $$'A'$$ would probably have a______[lower/higher] ionisation potential than 'A'.

C
The element $$'A'$$ would have______[lesser/higher] electron affinity than $$'B'$$.

D
Nuclear charge of element $$'B'$$ would be _______[less/,more] than element $$'A'$$.

E
If an element $$'C'$$ had a low electronegativity and ionisation potential it would have more tendency to________[gain/lose] eletrons.

Solution

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Classification of Elements and Periodicity in Properties Test - 50

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Classification of Elements and Periodicity in Properties Test - 50

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Question 1

group 7,8,9

group 13

group 15,16,17

group 14

Solution

Question 2

The electron affinity of Si is greater than that of phosphorous

Penetration power of p-orbital is more than s-orbital

Second ionisation energy of sodium is more than Mg.

The numerical value of electronegativity of an atom depends on its ionisation potential and electron affinity.

Solution

Question 3

$$S$$ and $$Q$$

$$P$$ and $$R$$

$$S$$ and $$R$$

$$S$$ and $$P$$

Solution

Question 4

$$Na$$

$$Ca$$

$$K$$

$$F$$

Solution

Question 5

$$B_2H_6, \ AlCl_3$$

$$C_2H_6, \ Al_2Cl_6$$

$$SF_2, \ Cl_2O$$

$$NaBH_4, \ ICl$$

Solution

Question 6

$$ > \,\,25$$

$$ < \,\,24$$

$$25$$

$$30$$

Solution

Question 7

1)(BeH2)2

(2) LiAlH4

3) (BeCl2)2

4) Li2C2

Solution

Question 8

$$ 3^{rd} $$ group

$$ 2^{nd} $$ group

$$ 18^{th} $$ group

$$ 13^{th} $$ group

Solution

Question 9

$$S (E.A.) < O(E.A.)$$

$$Hg (I.E.) < Cd (I.E.)$$

$$P(I.E.)> S (I.E.)$$

Both (B) and (C) are correct

Question 10

The element $$'A'$$ would probably have a______[smaller/larger] atomic size than $$'B'$$.

The element $$'A'$$ would probably have a______[lower/higher] ionisation potential than 'A'.

The element $$'A'$$ would have______[lesser/higher] electron affinity than $$'B'$$.

Nuclear charge of element $$'B'$$ would be _______[less/,more] than element $$'A'$$.

If an element $$'C'$$ had a low electronegativity and ionisation potential it would have more tendency to________[gain/lose] eletrons.

Solution

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