if we go from lithium to fluorine in the second period, there would be a decrease in
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Explanation:
On moving from Li to F in the second period,
-atomic radius decreases due to increase in effective nuclear charge.
-electronegativity increases the ability to pull electron pair increases across the period.
- Nonmetallic property increases across the period and decreses down the group and ionization potential increases because it takes more energy to knock out the electron from the outer shell of the atomas we go left to right ina period.
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Answer:
As we go from Li to F, atomic radius of the atoms will DECREASE. This means the increased nuclear charge has a greater force of attraction on the electrons, drawing them closer to the nucleus, hence causing a decrease in atomic radius.
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