Advertisements
Advertisements
प्रश्न
State the trends in the variation of electronegativity in groups and periods.
Advertisements
उत्तर
1. Variation of electronegativity in a group: The electronegativity decreases down a group. As we move down a group, the atomic radius increases, and the nuclear attractive force on the valence electron decreases. Hence electronegativity decreases in a group.
Variation of electronegativity along with I group
2. Variation of electron negativity in a period: The electronegativity increases across a period from left to right. Since the atomic radius decreases in a period, the attraction between the valence electron and the nucleus increases. Hence the tendency to attract shared pair of electrons increases. Therefore, electronegativity increases in a period.
Variation of electronegativity along with II group
APPEARS IN
संबंधित प्रश्न
Which one of the following arrangements represent the correct order of least negative to most negative electron gain enthalpy
Which of the following is the second most electronegative element?
IE1 and IE2 of Mg are 179 and 348 kcal mol−1 respectively. The energy required for the reaction \[\ce{Mg -> Mg^2+ + 2e^-}\] is
How does electron affinity change when we move from left to right in a period in the periodic table?
Is the definition given below for ionisation enthalpy is correct?
"Ionisation enthalpy is defined as the energy required to remove the most loosely bound electron from the valence shell of an atom"
Magnesium loses electrons successively to form Mg+, Mg2+ and Mg3+ ions. Which step will have the highest ionisation energy and why?
How would you explain the fact that the second ionisation potential is always higher than the first ionisation potential?
Explain the Pauling method for the determination of ionic radius.
Explain the following, give an appropriate reason.
Ionisation potential of N is greater than that of O
Briefly give the basis for Pauling's scale of electronegativity.
