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Shielding Effect

Increase in n...

Question

Increase in nuclear charge of an atom decreases the tendency of the atom to loose electrons.

A

True

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B

False

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Solution

The correct option is A True
Ionization energies increase moving from left to right across a period (decreasing atomic radius).
So, increase in nuclear charge of an atom, increases ionisation potential and the tendency of the atom to loose electrons decreases.

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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. Nuclear charge of an atom is the negative charge on the nucleus of an atom.

Q. Assertion :Atomic size decreases in a period due to increase of atomic number. Reason: The nuclear charge is increasing and size of valence shell remains same as we move from left to right. Hence, in any period, the atomic size of the element decreases from left to right.

Q. Assertion :Atom with large atomic radii and low ionisation potential are more metallic in nature. Reason: Atom with large atomic radii and low ionisation potential have tendency to loose electron

Q. The electron affinity increases on moving from left to right along a period. Arrange the reasons in a proper sequence.
(a) The amount of energy released during the addition of an electrons increases from left to right along a period.
(b) Effective nuclear charge of the elements increases from left to right.
(c) The atomic size of the elements decreases from left to right.
(d) The tendency to gain electrons and form anion increases from left to right.

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