Match the correct ionization enthalpies and electron gain enthalpies of the following elements-List IList IIA- Most reactive non-metal1- - H1 -419- H2 -3051-egH - -48B- Most reactive metal2- - H1 -1681- H2 -3374-egH - -328C- Least reactive elements 3- - H1 -738- H2 -1451-egH -40D- Metal forming binary halide4- - H1 -3272- H2 -5251-egH - -48

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Standard XII

Chemistry

Uses of Alkali Metals

Match the cor...

Question

Match the correct ionization enthalpies and electron gain enthalpies of the following elements.

List I List II
A. Most reactive non-metal 1. $Δ H_{1} = 419, Δ H_{2} = 3051, Δ_{e g} H = - 48$
B. Most reactive metal 2. $Δ H_{1} = 1681, Δ H_{2} = 3374, Δ_{e g} H = - 328$
C. Least reactive elements
3. $Δ H_{1} = 738, Δ H_{2} = 1451, Δ_{e g} H = - 40$
D. Metal forming binary halide 4. $Δ H_{1} = 3272, Δ H_{2} = 5251, Δ_{e g} H = + 48$

A - 2; B - 1; C - 4; D - 3

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A - 3; B - 1; C - 4; D - 2

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A - 2; B - 4; C - 1; D -3

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A - 1; B - 2; C - 4; D -3

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Solution

The correct option is A A - 2; B - 1; C - 4; D - 3
The most reactive nonmetal is 2 as it has the highest negative electron gain enthalpy.

The most reactive metal is 1 as it has the least first ionisation enthalpy.

The least reactive element is 4 as it has high ionisation energy and positive electron gain enthalpy.

Metal forming binary halide is 3 as it as comparable successive ionisation energy.

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Similar questions

Q. The first (

Δ H_{1}

) and second (

Δ H_{2}

) ionisation enthalpies (in kJ

m o l^{- 1}

) and the (

Δ_{e g} H

) electron gain enthalpy (in kJ

m o l^{- 1}

) of a few elements are given below:
Elements

Δ_{1} H_{1}

Δ_{1} H_{2}

Δ_{e g} H

(A) P 520 7300 -60
(B) Q 419 3051 -48
(C) R 1681 3374 -328
(D) S 1008 1846 -295
(E) T 2372 5251 +48
(F) U 738 1451 -40
The most reactive metal is :

Match the corect ionisation enthalpies and electron gain enthalpies of the following elements.
$\begin{matrix} E l e m e n t s & △ H_{1} & △ H_{2} & △_{e g} H (i) & M o s t r e a c t i v e n o n m e t a l & A & 419 & 3051 & - 48 (i i) & M o s t r e a c t i v e m e t a l & B & 1681 & 3374 & - 328 (i i i) & L e a s t r e a c t i v e e l e m e n t & C & 738 & 1451 & - 40 (i v) & M e t a l f o r m i n g b i n a r y h a l i d e & D . & 2372 & 5251 & + 48 \end{matrix}$

Q. The first (

Δ H_{1}

) and second (

Δ H_{2}

) ionisation enthalpies (in

k J m o l^{- 1}

) and the electron gain enthalpy (

Δ_{e g} H

) (in

k J m o l^{- 1}

) of the elements I, II, III, IV and V are given below:

Element	$Δ_{1} H_{1}$	$Δ_{1} H_{2}$	$Δ_{e g} H$
I	520	7300	-60
II	419	3051	-48
II	1681	3374	-328
IV	1008	1846	-295
V	2372	5251	+48

The most reactive metal and the least reactive non-metal of these are respectively.

Q. The first (

Δ H_{1}

) and second (

Δ H_{2}

) ionisation enthalpies (in kJ

m o l^{- 1}

) and the (

Δ_{e g} H

) electron gain enthalpy (in kJ

m o l^{- 1}

) of a few elements are given below:
Elements

Δ_{1} H_{1}

Δ_{1} H_{2}

Δ_{e g} H

(A) P 520 7300 -60
(B) Q 419 3051 -48
(C) R 1681 3374 -328
(D) S 1008 1846 -295
(E) T 2372 5251 +48
(F) U 738 1451 -40
The most reactive metal is :

Q. The first

(Δ_{i} H_{1})

and the second

(Δ_{i} H_{2})

ionization enthalpies (in kJ mol

^{- 1}

) and the

(Δ_{e g} H)

electron gain enthalpy (in kJ mol

^{- 1}

) of a few elements are given below:

Elements	$Δ H_{1}$	$Δ H_{2}$	$Δ_{e g}$ H
I	520	7300	-60
II	419	3051	-48
III	1681	3374	-328
IV	1008	1846	-295
V	2372	5251	+48
VI	738	1451	-40

Which of the above elements is likely to be :
(a) the least reactive element,
(b) the most reactive metal,
(c) the most reactive non-metal,
(d) the least reactive non-metal,
(e) the metal which can form a stable binary halide of the formula MX

_{2}

(X=halogen) and
(f) the metal which can form a predominantly stable covalent halide of the formula MX (X=halogen)?

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List I	List II
A. Most reactive non-metal	1. $Δ H_{1} = 419, Δ H_{2} = 3051, Δ_{e g} H = - 48$
B. Most reactive metal	2. $Δ H_{1} = 1681, Δ H_{2} = 3374, Δ_{e g} H = - 328$
C. Least reactive elements	3. $Δ H_{1} = 738, Δ H_{2} = 1451, Δ_{e g} H = - 40$
D. Metal forming binary halide	4. $Δ H_{1} = 3272, Δ H_{2} = 5251, Δ_{e g} H = + 48$