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

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

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

Explain why Be has higher ΔiH than B?


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


Among the elements \[\ce{B, Al, C}\] and \[\ce{Si}\], which element has the highest first ionisation enthalpy? 


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


Explain the following:

Ionisation enthalpy decrease in a group from top to bottom?


Assertion (A): Generally, ionisation enthalpy increases from left to right in a period.

Reason (R): When successive electrons are added to the orbitals in the same principal quantum level, the shielding effect of inner core of electrons does not increase very much to compensate for the increased attraction of the electron to the nucleus.


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 ______. 


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)


The decreasing order of the second ionization potential of K, Ca and Ba is ______.


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×