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प्रश्न
Explain the following:
The reducing power of element increases down in the group while decreases in a period.
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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.
संबंधित प्रश्न
Element X is a metal with a valency 2, Y is 3 non- metal with a valency 3.
1) Write an equation to show how Y from an ion.
2) If Y is a diatomic gas, write an equation for the direct combination of X and Y to form a compound.
Choose the correct answer from the options given below:
If an element A belongs to Period 3 and Group II, then it will have
A. 3 shells and 2 valence electrons
B. 2 shells and 3 valence electrons
C. 3 shells and 3 valence electrons
D. 2 shells and 2 valence electrons
The energy released when an electron is added to a neutral gaseous isolated atom to form a negatively charged iron.
Arrange the elements of second period in increasing order of their electron affinity. Name the elements which do not follow the trend in this period.
State the factors on which electron affinity depends ?
Give reason:
Electronegativity of chorine is higher than Sulphur?
Choose the correct answer:
Among the period 2 elements the one which has high electron affinity is
In a period, increase in electron affinity increases ______.
Among period 2 elements A, B, C and D, the one which has highest electron affinity is ______.
