Question

A certain main-group element exhibits the following successive ionization energies in kJ/mol:IE1 = 100; IE2 = 2200; IE3 = 3300; IE4 = 4100; IE5 = 5200Select the false statement about this element below.A) This is likely a Group 1A elementB) If this element is given a symbol "J", it would form an ionic compound with oxygen such as J2OC) This element is typically found as a free element rather than in compoundsD) If this element was in period 3 of the period table, it would be sodium E) This element is a metal

Answer 1

Answer:

The option C is the false statement

Explanation:

Ionization energy is the energy needed to completely pull out an electron from the valence electron of a gaseous atom.

The given values of ionization energy (kJmol⁻) for a main group element is: IE₁ = 100; IE₂ = 2200; IE₃ = 3300; IE₄ = 4100; IE₅ = 5200

Since first ionization energy is very low and the difference between the first and the second ionization energy for the given element is very high.

Therefore, the given chemical element is most likely an alkali metal belonging to the group IA of the periodic table.

As the alkali metals react with oxygen to form oxides. So, the given element (J) can react with oxygen to form oxide of the formula J₂O.

Since the given element has low first ionization energy, thus it is reactive. Therefore, the given element can not exist as a free element.

If the given chemical element belongs to the period 3 of the periodic table, then it is should be the group IA alkali metal, sodium.

Therefore, option C is the false statement.