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AlekseyPX
3 years ago
14

Draw a lewis structure for hccl3. Show all unshared pairs and the formal charges

Chemistry
1 answer:
klasskru [66]3 years ago
6 0

Explanation :

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.

The given molecule is, HCCl_3

Carbon has '4' valence electrons, hydrogen has '1' valence electron and chlorine has '7' valence electrons.

Therefore, the total number of valence electrons in HCCl_3 = 1(1) + 1(4) + 3(7) = 26

According to electron-dot structure, there are 8 number of bonding electrons and 18 number of non-bonding electrons.

The electron-dot structure of HCCl_3 is shown below.

Now we have to calculate the formal charges on carbon, hydrogen and chlorine.

Formula for formal charge :

\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}

\text{Formal charge on carbon}=4-0-\frac{8}{2}=0

\text{Formal charge on hydrogen}=1-0-\frac{2}{2}=0

\text{Formal charge on chlorine}=7-0-\frac{2}{2}=0

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A 5.32 g mixture contains both lithium fluoride, LiF, and potassium fluoride, KF. If the mixture contains 3.12 g fluorine, what
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Answer:

The mass of KF in the mixture is 2.77 gms.

Explanation:

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Total weight of mixture (LiF+KF)=5.32gms

Let, mass of KF in the mixture = x gms

⟹ mass of LiF in mixture =(5.32-x)gms.

We know that :

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Thus, moles of KF=x/58

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Thus,

moles of F in KF=moles of KF=x/58 ---(1)

moles of F in LiF =moles of LiF= (5.32-x)/26---(2)

From (1) & (2),

Total moles of Fluorine

=(x/58)+((5.32-x)/26)

Hence,

total weight of Fluorine in sample = moles*Atomic weight

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Now, solving the equation for x,

26x +(5.32*58)-58x

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Answer: 3.59

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3.59058 to 3 significant figures:

First three digits = 3.59

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