English
Karnataka Board PUCPUC Science Class 11

Explain the deviation in ionisation enthalpy of some elements from the general trend by using the given figure.

Advertisements
Advertisements

Question

Explain the deviation in ionisation enthalpy of some elements from the general trend by using the given figure.

Short/Brief Note
Advertisements

Solution

The deviation in the ionization enthalpy of some elements from the general trend can be explained by the points as given below:-

(i) The fully filled and half-filled orbital provide extra stability due to the symmetry.

(ii) The effective nuclear charge.

(iii) The \[\ce{e- - e-}\] repulsion which lead to instability.

shaalaa.com
  Is there an error in this question or solution?
Chapter 3: Classification of Elements and Periodicity in Properties - Multiple Choice Questions (Type - I) [Page 33]

APPEARS IN

NCERT Exemplar Chemistry Exemplar [English] Class 11
Chapter 3 Classification of Elements and Periodicity in Properties
Multiple Choice Questions (Type - I) | Q 38 | Page 33

RELATED QUESTIONS

Energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.
Hint: Apply the idea of mole concept to derive the answer.


Among the second period elements the actual ionization enthalpies are in the

order Li < B < Be < C < O < N < F < Ne.

Explain why O has lower ΔiH than N and F?


What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?


The first ionization enthalpy values (in kJmol–1) of group 13 elements are:-

B Al Ga In Tl
801 577 579 558 589

How would you explain this deviation from the general trend?


Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.


Which one of the following statements is incorrect in relation to ionization enthalpy?


Those elements impart colour to the flame on heating in it, the atoms of which require low energy for the ionisation (i.e., absorb energy in the visible region of spectrum). The elements of which of the following groups will impart colour to the flame?

(i) 2

(ii) 13

(iii) 1

(iv) 17


Nitrogen has positive electron gain enthalpy whereas oxygen has negative. However, oxygen has lower ionisation enthalpy than nitrogen. Explain.


Arrange the elements \[\ce{N, P, O}\] and \[\ce{S}\] in the order of increasing first ionisation enthalpy. Give reason for the arrangement assigned.


Explain the following:

Ionisation enthalpy decrease in a group from top to bottom?


Define ionisation enthalpy. Discuss the factors affecting ionisation enthalpy of the elements and its trends in the periodic table.


Discuss and compare the trend in ionisation enthalpy of the elements of group1 with those of group17 elements.


In general, the property (magnitudes only) that shows an opposite trend in comparison to other properties across a period is ______. 


Consider the elements Mg, Al, S, P and Si, the correct increasing order of their first ionization enthalpy is ______.


For the gaseous reaction, \[\ce{K_{(g)} + F_{(g)} -> K^+_{ (g)} + F^-_{ (g)}}\], ΔH was calculated to be 19 kcal/mol under conditions where the cations and anions were prevented by electrostatic separation from combining with each other. The ionisation energy of K is 4.3 eV. The electron affinity of F is ______. (in eV)


`"A"_0/2` atoms of X(g) are converted into X+(g) by absorbing energy E1. `"A"_0/2` ions of X+(g) are converted into X(g) with release of energy E2. Hence ionization energy and electron affinity of X(g) are ______.


Which of the following atoms has the highest first ionization energy?


Arrange the following elements in increasing order of first ionization enthalpy:

Li, Be, B, C, N

Choose the correct answer from the options given below:


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×