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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Solution

(a) The element V is the least reactive element as it has highest value of first ionization energy and positive electron gain enthalpy.
(b) The metal II is the most reactive metal. It has very low value of first ionization energy.
(c) The element III is the most reactive non metal. Its electron gain enthalpy is most negative.
(d) The element IV is the least reactive non metal as it has least negative electron gain enthalpy among the non metals.
(e) The metal VI can form a stable binary halide of the formula $M X_{2}$ as it has lowest value of second ionization enthalpy.
(f) The metal I can form a stable $M X$ halide

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Similar questions

The first (Δ_iH1) and the second (Δ_iH) ionization enthalpies (in kJ mol^–1) and the (Δ_egH) electron gain enthalpy (in kJ mol^–1) of a few elements are given below:

Elements	Δ_iH	Δ_iH	Δ_egH
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.

(d) the least reactive non-metal.

(e) the metal which can form a stable binary halide of the formula MX₂, (X=halogen).

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

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.

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. $Δ H_{1} = 3272, Δ H_{2} = 5251, Δ_{e g} H = + 48$

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

The first

Δ_{i} H_{1}

and second

Δ_{i} H_{2}

ionisation enthalpies in kJ mol

^{- 1}

and the

Δ_{e q} H

electron gain enthalpy in kJ mol

^{- 1}

of a few elements are given below :

	Elements	$Δ_{i} H_{1}$	$Δ_{i} H_{2}$	$Δ_{e g} H$
(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 least reactive element is :

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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