Question 1 Which of the following pairs are isoelectronic 2

Question 1 Which of the following pairs are isoelectronic? 2+. and K Ca 2+ O cl- and Ar2 O P3- and S O AI and B 3+

Solution

ANSWER (1) =(c) P^3- &S^2-

Isoelectronic refers to two atoms, ions or molecules that have the same electronic structure and same number of valence electrons.

Both have same electron configuration = 1s² 2s² 2p⁶ 3s² 3p⁶

Answer (2) = (a) Polar covalent

ANSWER (3)=(b) the nucleas is becoming more positive from left to right

the ionization energy is the energy required to remove the atom\'s nth electron, Trend-wise, ionization energy tends to increase while one progresses across a period because the greater number of protons (higher nuclear charge) attract the orbiting electrons more strongly, thereby increasing the energy required to remove one of the electrons.

ANSWER (4)=(a) Po

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.

Po has more electron than other atom. So valance electron keep away from the proton. so it experience less attraction compare to othar atom se, te, s. So electronegetivity decrease

ANSWER (5) = (b)

Flourine and oxygen placed side by side on periodic table. Oxygen have 16 proton & flourine have 17 Proton. Florine have More positive charge which is contract it. So florine is smaller than oxygen.

So option b is right.

ANSWER (6)

electon configuration of electron = 1s² 2s² 2p⁶ 3s² 3p¹

So Principle quantum number n = 3

Angular momentum quantum number l = 1 (For s(l=0), p(l=1),d(l=2)

Magnetic quantum number ml = -1, 0, 1 (Any one of them)

because lase electon in p orbital, So there are one electron so we take any one of them

Spin quantum number ms = +1/2 or -1/2