Chemistry, 25.11.2020 14:20 cecilysimpson7521

Draw the Lewis structure with the lowest formal charges for ClF2+ . Include nonzero formal charges and lone pair electrons in the structure.

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The Lewis structure is a representation that shows electrons' distribution around each of the atoms composing a molecule. In the attached files you will find the Lewis structure for ClF2+.

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The Lewis structure is a representation that shows electron pairs in bonds between the atoms that compose the molecule. It also shows the solitary electron pairs that remain for each atom.

Structure

There is always a central atom and terminal atoms.The central atom is surrounded by the terminal ones.The central atom forms many bonds with terminal atoms.When the molecule is composed of many atoms of the same element and a single atom of a different element, this last one is the central atom, and the others are terminal ones.Usually, hydrogen and oxygen atoms are terminal, and carbon atoms are central.Usually, the electropositive atoms are central, while the electronegative atoms are terminal.

Bonds

Bonds between atoms might be represented either as points or using a line. Two points equal a single line.A pair of electrons represent one single bond.Electrons pairs that are not involved in the bond are placed around the belonging atom.

Electrons

When adding the valence electrons of each atom we get the total number of electrons in the molecule. The valence value is the number of electrons placed in the last energetic level of the atom.

When drawing the Lewis structure of an ion, the entire structure is between square brackets, and the charge is written as an exponent in the upper right corner, outside the brackets.

So let us analyze the exposed example, ClF2+

1) Cl and F have 6 electron pairs and a single one. 7 electrons in total each.

2) Since there are two F and one Cl, then Cl is the central atom and F are the terminal ones.

3) Valence electrons: 7e⁻ F + 7e⁻ F + 7e⁻ Cl = 21 electrons

Since the ion has a possitive charge, there are 20 electrons.

4) Electron pairs:

Each F needs to form bonds with Cl. Each bond requires two electrons.

Since there are two bonds, four electrons are required.

The 16 remaining electrons must be placed as 8 solitary pairs. Each atom needs a maximum of 8 electrons.

Each F will get 3 pairs maximum to get the 8 e⁻.Cl will get 2 pairs to get the 8 e⁻.

5) The ion is between brackets, and the charge is written as an exponent in the upper right corner.

You will find the image in the attached files.

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You can learn more about the Lewis structure

link

Draw the Lewis structure with the lowest formal charges for ClF2+ . Include nonzero formal charges a

Answer from: xxnomr3cyxx

See explanation

Explanation:

The formal charge is obtained from;

Formal Charge = Valence electrons on atom - [number of bonds - lone pair electrons]

The correct structure of ClF2+ is the structure attached to this answer (image obtained from quora) in which the formal charge on fluorine is zero and the formal charge on chlorine is + 1. This is the correct structure because the chlorine is more electronegative than fluorine as expected.

Answer from: Quest

The answer options is d

Answer from: Quest

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Draw the Lewis structure with the lowest formal charges for ClF2+ . Include nonzero formal charges a...

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