English
Karnataka Board PUCPUC Science Class 11

Among the elements B,Al,C and Si, which element has the highest first ionisation enthalpy?

Advertisements
Advertisements

Question

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

Short/Brief Note
Advertisements

Solution

C has the highest ionization energy among the given elements as along the period ionization enthalpy increases whereas it decreases down the group.

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 32]

APPEARS IN

NCERT Exemplar Chemistry Exemplar [English] Class 11
Chapter 3 Classification of Elements and Periodicity in Properties
Multiple Choice Questions (Type - I) | Q 28.(i) | Page 32

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?


How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?


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?


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.


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 ______. 


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)


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×