With Reference To The Alkali Metals In Group 1 [IA] And The Halogens In 17 [VIIA] Explain The Trend In Ionization Potential, Electron Affinity And Electronegativity On Moving Down The Groups In The Periodic Table.

	Alkali Metals Group 1 [IA]	Halogens Group 17 [VIIA]
Ionization Potential	On moving down the group both atomic size and nuclear charge increases but atomic size increase dominates over nuclear charge increase hence Ionization Potential decreases down the group. ∴ Li > Na > K > Rb > Cs	Similarly for Halogens too Ionization Potential decreases down the group. ∴ F > Cl > Br > I
Electron Affinity	On moving down the group, electron affinity decreases as atomic size increase dominates over nuclear charge increase hence the atom attracts the electrons with a lesser force. ∴ Li > Na > K > Rb > Cs	Here also electron affinity decreases in general on moving down the group but Fluorine is an exception here as it has lesser electron affinity than Chlorine due to its electronic configuration. ∴ F < Cl > Br > I
Electronegativity	Similar to electron affinity, electronegativity decreases on moving down the group. ∴ Li > Na > K > Rb > Cs	Electronegativity decreases on moving down the group. ∴ F > Cl > Br > I

Alkali Metals
Group 1 [IA]

Halogens
Group 17 [VIIA]

Ionization
Potential

On moving down the group both atomic size and nuclear charge increases but atomic size increase dominates over nuclear charge increase hence Ionization Potential decreases down the group.
∴ Li > Na > K > Rb > Cs

Similarly for Halogens too Ionization Potential decreases down the group.
∴ F > Cl > Br > I

Electron Affinity

On moving down the group, electron affinity decreases as atomic size increase dominates over nuclear charge increase hence the atom attracts the electrons with a lesser force.
∴ Li > Na > K > Rb > Cs

Here also electron affinity decreases in general on moving down the group but Fluorine is an exception here as it has lesser electron affinity than Chlorine due to its electronic configuration.
∴ F < Cl > Br > I

Electronegativity

Similar to electron affinity, electronegativity decreases on moving down the group.
∴ Li > Na > K > Rb > Cs

Electronegativity decreases on moving down the group.
∴ F > Cl > Br > I

X	Y
1: Element with atomic number 19	A: Group 18 [0 group]
2: Element with electronic configuration 2	B: Group 16 [VI A]
3: Element with a valency of -2	C: Group 1 [IA]
4: Element ‘P’ which loses 3 electrons to form a cation	D: Group 17 [VII A]
5: Element ‘Q’ in period-3 which has the highest electron affinity	E: Group 13 [III A]

1: Element with atomic number 19

A: Group 18 [0 group]

2: Element with electronic configuration 2

B: Group 16 [VI A]

3: Element with a valency of -2

C: Group 1 [IA]

4: Element ‘P’ which loses 3 electrons to form a cation

D: Group 17 [VII A]

5: Element ‘Q’ in period-3 which has the highest electron affinity

E: Group 13 [III A]

With reference to group 1 [IA] of the periodic table – fill in the blanks with the correct word:
The elements are …………… [light/heavy] …………… [metals/non metals] since their atomic size is …………… [large/small]. The energy binding the atoms is …………… [high/low] and hence the elements have …………… [high/low] melting points. The melting points of the elements …………… [increases/decreases] down the subgroup. The electropositive character …………… [increases/decreases] down the subgroup and the elements are strong …………… [reducing/oxidizing] agents. The element with electronic configuration 2, 8, 1 will have …………… [higher/lower] electron affinity and …………… [smaller/larger] atomic size than the element with electronic configuration 2, 1.

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Question

With reference to the alkali metals in Group 1 [IA] and the halogens in 17 [VIIA] explain the trend in ionization potential, electron affinity and electronegativity on moving down the groups in the periodic table.

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Question

With reference to the alkali metals in Group 1 [IA] and the halogens in 17 [VIIA] explain the trend in ionization potential, electron affinity and electronegativity on moving down the groups in the periodic table.

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