When the first electron gain enthalpy ( ΔH eg ) of oxygen is - 141 kJ / mol , its second electron gain enthalpy is:

Almost the same as that of the first

Negative, but less negative than the first

A more negative value than the first

In general, the properties that decrease and increase down a group in the periodic table, respectively, are :

Electronegativity and atomic radius

Atomic radius and electronegativity

Electronegativity and electron gain enthalpy

Electron gain enthalpy and electronegativity

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Assertion : The atomic radii of the elements of the oxygen family are smaller than the atomic radii of the corresponding elements of the nitrogen family.
Reason : The members of the oxygen family are more electronegative and thus have lower values of nuclear charge than those of the nitrogen family.

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Important Questions on Classification of Elements and Periodicity in Properties

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 3>Q 7

Assertion: Fluorine has a less negative electron gain enthalpy than chlorine.
Reason: There is relative greater effectiveness of

2 p -

electrons in the small

F

atom to repel the additional electron entering the atom than to

3 p -

electrons in the larger

Cl

atom.

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 3>Q 8

Assertion:

Li

and

Mg

shows diagonal relationship.
Reason:

Li

and

Mg

are diagonal to each other in the periodic table

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 4>Q 1

Assertion: First ionisation energy for nitrogen is lower than oxygen.
Reason: Across a period effective nuclear charge decreases.

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 4>Q 2

Consider the following statements:
I. The radius of an anion is larger than that of the parent atom.
II. The ionization energy generally increases with increasing the atomic number in a period.
III. The electronegativity of an element is the tendency of an isolated atom to attract an electron. Which of the above statements is/are correct?

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 4>Q 3

Which of the order for ionization energy is correct?

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 4>Q 5

Following table shows the successive molar ionization energy

(k J m o l^{- 1})

of five elements A to E.

Element	Ionisation energy $(k J m o l^{- 1})$
Element	$1^{s t}$	$2^{n d}$	$3^{r d}$	$4^{t h}$
A	2080	4000	6100	9400
B	500	4600	6900	9500
C	740	1500	7700	10500
D	580	1800	2700	11600
E	420	3100	4400	5900

Which two elements are most likely to be in the same group of the periodic table?

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 4>Q 6

Arrange the elements

Se, Cl

and

S

in the increasing order of ionisation energy :

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Alpha Question Bank for Medical: Chemistry>Chapter 12 - Classification of Elements and Periodicity in Properties>Exercise 4>Q 7

Which of the following does not represent the correct order of the properties indicated?

Important Questions on Classification of Elements and Periodicity in Properties

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