Question

The first ($IE_{1}$) and second ($IE_{2}$) ionisation energies (kJ/mol) of a new element designated by Roman numerals are shown below: S.N. (i) (ii) (iii) (iv) $IE_{1}$ 2372 520 900 1680 $IE_{2}$ 5251 7320 1760 3380 Which of these elements is likely to be (a) a reactive metal, (b) a reactive non-metal, (c) a noble gas, (d) a metal that forms a binary halide of the formula, AX₂?

Answer 1

"The "amount of energy" required to removal of an electrons form an isolated gaseous atoms are called ionization energy.

(a) Element (ii) is a most reactive metal because it has lowest first ionization energy.

(b) Element (i) is a "most reactive" "non-metal" because it has highest first ionization energy.

(c) Element (iv) is a Nobel gas because it has very less variation in between firs ionization and second ionization energy.

(d) Element (iii) is a forms binary halides because it has lowest second ionization energy."

Answer 2

Explanation:

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