Question

which among the following is the smallest size N³-,O²-,F-,Na-​

Answer 1

Explanation:

F- . BECAUSE AS WE MOVE ALONG A PERIOD ,THE SIZE OF ATOM GOES ON DECREASING.

Answer 2

11th/Chemistry

Classification of Elements and periodicity in properties.

Answer :

★ Cation is smaller and anion is larger than the parent atom of the element.

★ Atoms or ions having same number of electrons but different nuclear charge are called isoelectronic species.

For example, N(-3), O(-2), F(-), Na(+), Mg(+2), Al(+3)

• In isoelectronic ions, the size decreases if Z/e increases, i.e.; greater the nuclear charge, smaller is the size of the ion.
• Thus, the cation with the greater positive charge will have a smaller radius and the anion with negative charge will have the larger radius$.$

⧪ N(-3) : Z/e = -3/10 = -0.3

⧪ O(-2) : Z/e = -2/10 = -0.2

⧪ F(-) : Z/e = -1/10 = -0.1

⧪ Na(+) : Z/e = +1/10 = +0.1

Order of size :

• Na(+) < F(-) < O(-2) < N(-3)

Hence, Na(+) has the smallest size among the given ions.