Advertisements
Advertisements
Question
State the trends in the variation of electronegativity in groups and periods.
Advertisements
Solution
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
RELATED QUESTIONS
The group of elements in which the differentiating electron enters the anti penultimate shell of atoms are called ________.
Which of the following elements will have the highest electronegativity?
In the third period the first ionization potential is of the order.
Which one of the following is true about metallic character when we move from left to right in a period and top to bottom in a group?
What is the effective nuclear charge?
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"
Explain the periodic trend of ionisation potential.
Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium?
Explain the following, give an appropriate reason.
The electron affinity values of Be and Mg are almost zero and those of N (0.02 eV) and P (0.80 eV) are very low.
Explain the following, give an appropriate reason.
The formation of \[\ce{F^-_{(g)}}\] from \[\ce{F_{(g)}}\] is exothermic while that of \[\ce{O^2-_{(g)}}\] from \[\ce{O_{(g)}}\] is endothermic.
