Identify the correct statements from the following.
(a) An element with low ionization potential has high electropositivity and hence give out electrons easily.
(b) Due to decrease in ionization energy, in a group, the oxidizing property decreases.
(c) Electronegativity decreases along a period due to increase in nuclear charge and increase in atomic size.
(d) Due to increase in electron affinity the reducing property increases along a period.

a only

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b and c

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a and c

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c and d

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Solution

The correct option is C a only
Group I elements have low ionization energies because the loss of an electron forms a stable octet.
It becomes harder to remove an electron as the atomic radius decreases because the electrons are generally closer to the nucleus, which is also more positively charged.
Electronegativity increases along the period with an increase in the nuclear charge. Thus Fluorine has the highest electronegativity which is at the right-hand side of the periodic table.

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Similar questions

Q. Identify the correct alternative from the following set of properties that increase down the group.
(a) Atomic radius
(b) Ionization potential
(c) Electron affinity
(d) Electropositivity
(e) Oxidizing property
(f) Reducing property

Q. Which of the following sequence of explanation is appropriate for explaining the reason for the periodicity of reducing property in a period or group?
(a) Tendency to undergo oxidation decreases in a period and increases in a group.
(b) In a period ionization energy increases and in a group it decreases.
(c) In a period the atomic size decreases and in a group it increases.
(d) The elements present in the left side of the periodic table have strong reducing property.

Q. The amount of energy released when an atom in the gaseous state accepts an electron to form an anion. factor which affect electron affinity are: atomic size and Nuclear charge. As atomic radii increases, electron affinity increase. As nuclear charge increase, electron affinity increase. it decrease down a group and increases across a period. Explain.

Q. Consider the following statements with reference to the periodic table of chemical elements
(a) Ionization potential gradually decreases along a period.
(b) In a group of elements, electron affinity decreases as the atomic weight increases.
(c) In a given period, electro-negativity decreases as the atomic number increases.
Which of these statements(s) is/are correct?

Parts (a) to (e) refer to changes in the properties of elements on moving from left to right across a period of Periodic Table. For each property, choose the correct answer.

(a) The non-metallic character of the elements :

(i) decreases, (ii) increases,

(iii) remains the same, (iv) depends on the period

(b) The electronegativity :

(i) depends on the number of valence electrons,

(ii) remains the same,

(iii) decreases,

(iv) increases.

(i) goes up and down (ii) decreases

(iii) increases (iv) remains the same

(d) The atomic size :

(i) decreases,

(ii) increases,

(iii) remains the same ,

(iv) sometimes increases and sometimes decreases.

(e) The electron affinity of the elements in groups 1 to 7 :

(i) goes up and then down.

(ii) decreases and then increases,

(iii) increases,

(iv) decreases.

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