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Sloan [31]
3 years ago
15

Draw the best lewis structure for cl3-. what is the formal charge on the central cl atom?

Chemistry
1 answer:
shepuryov [24]3 years ago
3 0

Answer : The formal charge on central Cl atom is -1.

Explanation :

The given molecule is, Cl^-_3

First we have to determine the total number of valence electrons in, Cl^-_3

As we know, chlorine has 7 valence electrons.

Total number of valence electrons in Cl^-_3 = 3(7) + 1 = 22 electrons

Electrons used in bonding pair = 4

Electrons used as lone pair = 22 - 4 = 18

Now we have to calculate the formal charge on central Cl atom.

  • Formal charge = Number of valence electrons of a central atom - (2 × Number of lone pairs) - Number of bond pairs

Formal charge on central Cl atom = 7 - (2 × 3) -2 = -1

Therefore, the formal charge on central Cl atom is -1.

The lewis-dot structure of Cl^-_3 is shown below.

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8 0
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Please Answer! Help! Will Give Brainliest. Find Keq for a 3.0 L container with 1.2 moles of both NO2 and N2O4 initially and 0.38
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Answer:

Kc → 41.9

Explanation:

This is the equilibrium:

2NO₂(g) ⇌ N₂O₄(g)

So the expression for Kc will be:

Kc = [N₂O₄] / [NO₂]²

We prospose the situations:

Initially we have 1.2 moles of NO₂ and N₂O₄

X amount has reacted. As stoichiometry is 2:1, we have produced x/2 of the product during the reaction

Finally In equilibrium we have, 0.38 NO₂

                2NO₂(g)     ⇌       N₂O₄(g)

Initially        1.2                        1.2

React            x                         x/2

Eq         (1.2 - x) = 0.38          1.2 + x/2

As we have [NO₂] in the equilibrium, we can determine x (the amount that has reacted) to solve and determine, the [N₂O₄] in the equilibrium

1.2-0.38 = x → 0.82

1.2 + 0.82/2 = 2.02 → [N₂O₄]

For Kc, we need Molar concentration, so we have to divide [N₂O₄] and [NO₂] by the volume

[N₂O₄] → 2.02 mol/3L = 0.673 M

[NO₂] → 0.38 mol/3L = 0.127 M

Now we can replace the Kc expression:

Kc →  [N₂O₄] / [NO₂]² → 0.673 / 0.127² = 41.9

Remember that Kc has no UNITS

6 0
3 years ago
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