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

Answer:

ANSWER

(a) Element 2 has a very low value of first ionization energy and a high value of second ionization energy. Hence, it is reactive alkali metal.

Its first ionization energy is lowest among the given elements.

(b) Element 4 has a second-highest value of first ionization energy among the given elements.

Hence, it is reactive non-metal.

(c) The element 1 has the highest value of first ionization energy among the given elements.

Hence, it is a noble gas

(d) Element 3 has the second-lowest value of first ionization energy among the given elements.

Hence, it forms a stable binary halide of the type AX

2

Hence, the correct sequence is 2413.