Question

The following elements represent third period of the periodic table [5] Na Mg Al Si P S Cl Answer the following. a. Which of these have the electronic configuration as 2,8,4? b.Which has the smallest size in the period? Why? c. Which of these have lowest ionization potential? d. Electronegativity increases across period. Justify e. Noble gases have zero electron affinity. Why? Plzzz give an appropriate answer. The correct answer wud be marked brainliest. DON'T SPAM.

Answer 1

Answer:

a. Silicon Si

b. Chlorine Cl

c. Sodium Na

d. Electronegativity increases across period because their effective nuclear charge increases.

e. Noble gases have zero electron affinity because their octet is completed and are inert gases.

Answer 2

Explanation:

a.Si has electronic configuration of (2,8,4)

b.Cl smallest size among these elements as atomic size decreases across a period from left to right due to increase in nuclear charge.

c. Na has the lowest IP among these elements as it has the least nuclear charge, so it readily loses electron form it's outermost shell

d. Electronegativity increases across a period as the nuclear charge increases which pulls the electrons towards the nucleus thus elements in group 17 accept electrons more readily and are more electronegative.