Advertisements
Advertisements
प्रश्न
Explain the following:
The reducing power of element increases down in the group while decreases in a period.
Advertisements
उत्तर
The reducing property depends on the ionisation potential and electron affinity of the elements. In a period, from left to right in a horizontal row of the periodic table, the atomic size decreases and the nuclear charge increases, so the electron affinity and ionisation energy both increase. Hence, the tendency to lose electrons decreases across the period from left to right and thus the reducing property also decreases across the period from left to right.
The electron affinity and ionisation potential decreases along the group from top to bottom. Hence, the tendency to lose electrons increases, and thus, the reducing property also increases along the group from top to bottom.
APPEARS IN
संबंधित प्रश्न
State the factors on which electron affinity depends ?
Electron affinity values generally _______ across the periods left to right and ______ down the group top to bottom.
Give reason:
Electronegativity of chorine is higher than Sulphur?
Arrange the following according to the instruction given in the bracket:
F, B, N, O (In the increasing order of electron affinity).
Fill in the blank
Noble gases have ______ electron affinity.
What is electron affinity?
The following questions refer to the Periodic Table.
Which of the elements has the greatest electron affinity among the halogens?
Neon shows zero electron affinity due to ______.
The electron affinity of an element X is greater than that of element Y.
How is the electronegativity of X likely to compare with that of Y?
The electron affinity of an element X is greater than that of element Y.
State whether X is likely to be placed to the left or to the right of Y in the periodic table.
