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VARVARA [1.3K]
3 years ago
9

Which of the following pairs of elements would form the covalent bond with the largest dipole moment? View Available Hint(s) Whi

ch of the following pairs of elements would form the covalent bond with the largest dipole moment?
a.Ge and O
b.H and P
c.In and F
d.B and N
Chemistry
1 answer:
LekaFEV [45]3 years ago
6 0

Answer:

In-F bond has the largest dipole moment.

Explanation:

Given the electronegativities:

Ge= 2.01

O= 3.44

H= 2.20

P= 2.19

In= 1.78

F= 3.98

B= 2.04

N= 3.04

The bond between Ge and O has an electronegativity difference:

ED= 3.44 - 2.01= 1.43

The bond between H and P has an electronegativity difference:

ED= 2.20 - 2.19= 0.01

The bond between In and F has an electronegativity difference:

ED= 3.98 - 1.78= 2.20

The bond between B and N has an electronegativity difference:

ED= 3.04 - 2.04= 1.00

As In-F bond has the largest electronegativity difference, this is the covalent bond with the largest dipole moment.

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. Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:
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Explanation:

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b) Equation of the reaction;

HgO -> Hg + O2

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c) Equation of the reaction;

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3 years ago
Calculate ∆G ◦ r for the decomposition of mercury(II) oxide 2 HgO(s) → 2 Hg(ℓ) + O2(g) ∆H◦ f −90.83 − − (kJ · mol−1 ) ∆S ◦ m 70.
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Answer:

4. +117,1 kJ/mol

Explanation:

ΔG of a reaction is:

ΔGr = ΔHr - TΔSr <em>(1)</em>

For the reaction:

2 HgO(s) → 2 Hg(l) + O₂(g)

ΔHr: 2ΔHf Hg(l) + ΔHf O₂(g) - 2ΔHf HgO(s)

As ΔHf of Hg(l) and ΔHf O₂(g) are 0:

ΔHr: - 2ΔHf HgO(s) = <u><em>181,66 kJ/mol</em></u>

<u><em /></u>

In the same way ΔSr is:

ΔSr= 2ΔS° Hg(l) + ΔS° O₂(g) - 2ΔS° HgO(s)

ΔSr= 2* 76,02J/Kmol + 205,14 J/Kmol - 2*70,19 J/Kmol

ΔSr= 216,8 J/Kmol = <em><u>0,216 kJ/Kmol</u></em>

Thus, ΔGr at 298K is:

ΔGr = 181,66 kJ/mol - 298K*0,216kJ/Kmol

ΔGr = +117,3 kJ/mol ≈ <em>4. +117,1 kJ/mol</em>

<em></em>

I hope it helps!

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