Question

G. Which of the following pairs is NOT
isoelectronic ?
a. Na+ and Na
b. Mg2+ and Ne
c. A13+ and B3+
d. p3- and N3-​

Answer 1

Answer: The correct options are, (a), (c) and (d)

Explanation:

Isoelectronic atoms : It is defined as the atoms which have same number of electrons.

In the calculation, the positive charge is subtracted from the total number of electrons and negative charge is added to the total number of electrons.

For the given options:

Option a:  $Na^+\text{ and }Na$

For $Na^+$

Number of electrons in Na are 11

Number of electrons in Na ion = $[11-1]=10$

For $Na$

Number of electrons in Na are 11

Thus, they are not isoelectronic.

Option b:  $Mg^{2+}\text{ and }Ne$

For $Mg^{2+}$

Number of electrons in Mg are 12

Number of electrons in Mg ion = $[12-2]=10$

For $Ne$

Number of electrons in Ne are 10

Thus, they are isoelectronic.

Option c:  $Al^{3+}\text{ and }B^{3+}$

For $Al^{3+}$

Number of electrons in Al are 13

Number of electrons in Al ion = $[13-3]=10$

For $B^{3+}$

Number of electrons in B are 5

Number of electrons in B ion = $[5-3]=2$

Thus, they are not isoelectronic.

Option d:  $P^{3-}\text{ and }N^{3-}$

For $P^{3-}$

Number of electrons in P are 15

Number of electrons in P ion = $[15+3]=18$

For $N^{3-}$

Number of electrons in N are 7

Number of electrons in N ion = $[7+3]=10$

Thus, they are not isoelectronic.

Hence, the correct options are, (a), (c) and (d)

Answer 2

a. Na+ and Na are NOT isoelectronic.

Isoelectronic species:

• Isoelectronic species are two atoms, ions, or molecules that have the same electronic structure and the same amount of valence electrons.
• The term "same electric" or "equal charge" refers to these two atoms, ions, or molecules.
• The chemical characteristics of isoelectronic chemical species are often identical.
• Isoelectronic entities have the same number of electrons as elements or ions.
• For example, $O^{-2}$, $F^{-}$, and $Mg^{+2}$ each contains ten electrons.
• To get the isoelectronic pairings, just add the number of electrons in each atom in the species as well as the species charge (if present). -
• If the number of electrons in each species is equal, they are said to be isoelectronic pairs.

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