3.31. The first (ΔiH1) and the second (ΔiH2) ionization enthalpies (in kJ mol–1) and the (ΔegH) electron gain enthalpy (in kJ mol–1) of a few elements are given below:
Elements ΔH1 ΔH2 ΔegH
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 MX2 (X = halogen)
(f) The metal which can form a predominantly stable covalent halide of the formula MX (X = halogen)?
3.31. The first (ΔiH1) and the second (ΔiH2) ionization enthalpies (in kJ mol–1) and the (ΔegH) electron gain enthalpy (in kJ mol–1) of a few elements are given below:
Elements ΔH1 ΔH2 ΔegH
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 MX2 (X = halogen)
(f) The metal which can form a predominantly stable covalent halide of the formula MX (X = halogen)?
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1 Answer
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(a) The element V has the highest first ionization enthalpy (? iH1) and positive electron gain enthalpy (? egH) and hence it is the least reactive element. Since inert gases have positive? egH, therefore, the element-V must be an inert gas. The values of? iH1, ? iH2 and? egH match that of He.
(b) The element II which has the least first ionization enthalpy (? iH1) and a low negative electron gain enthalpy (? egH) is the most reactive metal. The values of ? iH1, ? iH2 and? egH match that of K (potassium).
(c) The element III which has high fi
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Among isoelectronic monoatomic species, size is inversely proportional to atomic number. Hence among isoelectronic species Na? , O²? , N³? , F? (having the nearest noble gas configuration);
Order of size is Na? < F? < O²? < N³?
N³? has least atomic number hence the largest size
Electron gain enthalpy increases with electro negativity chlorine has higher electron gain enthalpy than fluorine (exception)
In isoelectronic species nuclear charge can be approximated as
Nuclear charge ≈ z / no. of electrons
Al³? Mg²? Na? F? O²? N³?
Nuclear Charge: 13/10 12/10 11/10 9/10 8/10 7/10
Minimum nuclear charge is in N³? and maximum is in Al³?
So order should be
Al³? < Mg²? < Na? < F? < O²? < N³?
This is a Matching Type Questions as classified in NCERT Exemplar
i d + 48
ii a &n
This is a Matching Type Questions as classified in NCERT Exemplar
i ) b 1681 3374 – 328
ii ) a 419 3051 – 48
iii)
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