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In the series Sc (2 = 21) to Zn (Z=30), ...

In the series Sc (2 = 21) to Zn (Z=30), the enthalpy of atomisation of which element is least?

A

Sc

B

Mn

C

Cu

D

Zn

Text Solution

Verified by Experts

The correct Answer is:
D
In general, greater the number of unpaired electronis, greater is the number of bond and therefore, greater is the strength of these bonds, thus higher will be enthalpy of atomization.
Enthalpy of atomization first increases in a series (as unpaired electrons increases from 1 to 6), reaches to maxima and then decreases, and it is lowest for Zn, Cd, Hg (due to 0 unpaired electrons).
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In the series Sc (Z = 21) to Zn (Z = 30), the enthalpy of atomisation of zinc is the lowest, i.e., 126 kJ mol^(-1) . Why ?

In the series Sc (Z= 21) to Zn ( Z= 30) , the enthalpy of atomisation of zinc is the lowest , i.e., 126 kJ mol^(-1) . Why ?

Knowledge Check

  • Assertion : In the series Sc to Zn, the enthalpy of atomisation of zinc is the lowest. Reason : Zinc has greater number of unpaired electrons.

    A
    If both assertion and reason are true and reason is the correct explanation of assertion.
    B
    If both assertion and reason are true and reason not is the correct explanation of assertion.
    C
    If assertion is trun but reason is false.
    D
    If both assertion and reason are false.

  • Which of the following has the lowest enthalpy of atomisation ?

    A
    V
    B
    Ti
    C
    Ni
    D
    Zn

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    Read the given passage and answer the questions number 1 to 5 that follow : The lowest common oxidation state of transition metals is + 2. To form the M^(2+) ions from the gaseous atoms, the sum of the first and second ionisation enthalpy is required in addition to the enthsualpy of atomisation. The dominant term is the second ionisation enthalpy which shows unusually high values for Cr and Cu where M^(+) ions have the d^(5) and d^(10) configurations respectively. The value for Zn is correspondingly low as the ionisation causes the removal of 1s electron which results in the formation of stable d^(10) configuration. The trend in the third ionisation enthalpies is not complicated by the 4s orbital factor and shows the greater difficulty of removing an electron from the d^(5) (Mn^(2+)) and d^(10) (Zn^(2+)) ions. In general, the third ionisation enthalpies are quite high. Also, the high values for third ionisation enthalpies of copper, nickel and zinc indicate why it is difficult to obtain oxidation state greater than two for these elements. In the series Sc(Z = 21) to Zn(Z = 30), the enthalpy of atomisation of Zn is the lowest. Why?

    In the series Sc(Z=21) to Zn(Z=30) the enthalpy of atomisation of zinc is the lowest, i.e., 126 kJ mol^(-1) . Why?

    In 3d series (Sc to Zn), the enthalpy of atomization of Zn is low. Why ?

    In 3d series, the enthalpy of atomisation of zinc is the lowest Why?

    Assign reasons for the following : (i) The enthalpies of atomisation of transition elements are high. (ii) The transition metals and many of their compounds act as good catalyst. (iii) From element to element the actinoid contraction is greater than the lanthanoid contraction. (iv) The E^(@) value for the Mn^(3+)//Mn^(2+) couple is much more positive than that for Cr^(3+)//Cr^(2+) . (v) Scandium (Z = 21) does not exhibit variable oxidation states and yet it is regarded as transition element.

    In the 3d series (Sc = 21 to Zn = 30) : (i) Which elements shows maximum number of oxidation states ? (ii) Which elements shows only +3 oxidation state ? (iii) Which elements has the lowest enthalpy of atomization?

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