Question

Which of the following ions are likely to form?
Mn3+
N3−
Zn4+
Li2+
K−

Answer 1

The  ions  that  are likely   to form   is N3-

Explanation

• Ion  are formed  when a  element  gain or lose electrons  in the  outermost energy  level .

• metal form  ion by losing  electrons  to which result to  forming a cation ( a positively charged ion) .

•  Nonmetal  form ion  by gaining electrons which  result to formation  of anion ( a negatively charged ion).

• nitrogen(N)   is in atomic number number   7 hence  has 2.5  electron configuration.  Nitrogen  gain 3  electron to  ion N3-

• Other  ions like MN3+  is not  likely to be formed since  Mn  loses  2  electron to form Mn2+  ion  . Li loses 1 electron to form Li+  ion.   K  is a metal  and it  loses 1 electron  to K+  ion.  Zn  is a  metal it loses  2 electrons to form Zn 2+  ion

Answer 2

The ion that is most likely to form is $\boxed{{{\text{N}}^{3-}}{\text{ ion}}}$.

Further explanation:

Octet rule:

Lewis structure for any atom or molecule depicts the valence electrons as dots around the element’s symbol present in the molecule along with the bonds that connect them. Every element tries to complete an octet except the hydrogen atom. Every element in the Lewis structure tries to attain eight electrons in its valence shell by transfer or share of electrons. This rule is known as the octet rule. It only applied on main s and p subshells and not applied on d and f subshells.

1. The electronic configuration of ${\text{M}}{{\text{n}}^{3+}}$ion,

$\left[{{\text{Ar}}}\right]3{d^4}$

Since ${\text{M}}{{\text{n}}^{3+}}$ion has no fully-filled d-orbital thus it is not most likely to form.

2. The electronic configuration of ${{\text{N}}^{3-}}$ ions,

$\left[{{\text{He}}}\right]2{s^2}2{p^6}$

Since ${{\text{N}}^{3-}}$ion has eight electrons in its valence shell and it is fully filled, therefore, it follows the octet rule, and it is most likely to form.

3. The electronic configuration of ${\text{Z}}{{\text{n}}^{4+}}$ion,$\left[{{\text{Ar}}}\right]3{d^8}$

The ${\text{Z}}{{\text{n}}^{4+}}$ion has no fully-filled d-orbital, and thus it is not most likely to form.

4. The electronic configuration of ${\text{L}}{{\text{i}}^{2+}}$ion,

$1{s^1}$

The ${\text{L}}{{\text{i}}^{2+}}$ has no fully-filled s-orbital, and also it does not follow octet rule. Thus it is not most likely to form.

5. The electronic configuration of ${{\text{K}}^-}$ion,

$\left[{{\text{Ar}}}\right]4{s^2}$

The ${{\text{K}}^-}$ion does not have eight electrons in its valence shell, and thus it is not most likely to form.

Learn more:

1. Determine the Lewis structure of butanal.: https://brainly.com/question/6215269

2. Determine the reason that causes water molecule a bent shape.:https://brainly.com/question/1979769

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Octet rule

Keywords: Periodic table, electronic configuration, Mn3+, N3−, Zn4+, Li2+, K, magnesium, potassium, lithium, nitrogen, zinc, and octet rule.