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Andrew [12]
3 years ago
7

Compare and contrast the compounds CH4 and PH3 in terms of covalent bonding, molecular geometry (shape), and intermolecular forc

es. Which substance would experience a stronger attraction between its molecules, and why?
Chemistry
1 answer:
Pepsi [2]3 years ago
4 0
CH4 and PH3 are both covalent since they are composed both of non-metals.  
<span>
CH4 is non- polar because of </span> London forces and<span> has a geometry of tetrahedral  PH3 , on the other hand, is umbrella shaped polar and has dipole-dipole intermolecular force (IMF) . Since PH3 is polar, it has a stronger IMF </span>
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Determine the molecular formula for each of the following compounds from the
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The molecular formula for each of the following compound given the data is

  • C₂H₆
  • C₂H₂
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<h3>A. How to determine the molecular formula </h3>

We'll begin by calculating the empirical formula. This can be obtained as follow:

  • C = 80%
  • H = 20%
  • Empirical formula =?

Divide by their molar mass

C = 80 / 12 = 6.67

H = 20 / 1 = 20

Divide by the smallest

C = 6.67 / 6.67 = 1

H = 20 / 6.67 = 3

Thus, the empirical formula of the compound CH₃

Thus, the molecular formula of the compound can be obtained as follow

  • Empirical formula = CH₃
  • Molar mass of compound = 30 g/mol
  • Molecular formula =?

Molecular formula = empirical × n = mass number

[CH₃]n = 30

[12 + (3×1)]n = 30

15n = 30

Divide both side by 15

n = 30 / 15

n = 2

Molecular formula = [CH₃]n

Molecular formula = [CH₃]₂

Molecular formula = C₂H₆

Thus, the molecular formula of the compound is C₂H₆

<h3>B. How to determine the molecular formula </h3>

We'll begin by calculating the empirical formula. This can be obtained as follow:

  • C = 92.3%
  • H = 7.7%
  • Empirical formula =?

Divide by their molar mass

C = 92.3 / 12 = 7.7

H = 7.7 / 1 = 7.7

Divide by the smallest

C = 7.7 / 7.7 = 1

H = 7.7 / 7.7 = 1

Thus, the empirical formula of the compound CH

Thus, the molecular formula of the compound can be obtained as follow

  • Empirical formula = CH
  • Molar mass of compound = 26 g/mol
  • Molecular formula =?

Molecular formula = empirical × n = mass number

[CH]n = 26

[12 + 1]n = 26

13n = 26

Divide both side by 13

n = 26 / 13

n = 2

Molecular formula = [CH]n

Molecular formula = [CH]₂

Molecular formula = C₂H₂

Thus, the molecular formula of the compound is C₂H₂

<h3>C. How to determine the molecular formula </h3>

We'll begin by calculating the empirical formula. This can be obtained as follow:

  • C = 37.5%
  • H = 6.3%
  • Cl = 55.8%
  • Empirical formula =?

Divide by their molar mass

C = 37.5 / 12 = 3.125

H = 6.3 / 1 = 6.3

Cl = 55.8 / 35.5 = 1.572

Divide by the smallest

C = 3.125 / 1.572 = 2

H = 6.3 / 1.572 = 4

Cl = 1.572 / 1.572 = 1

Thus, the empirical formula of the compound C₂H₄Cl

Thus, the molecular formula of the compound can be obtained as follow

  • Empirical formula = C₂H₄Cl
  • Molar mass of compound = 127 g/mol
  • Molecular formula =?

Molecular formula = empirical × n = mass number

[C₂H₄Cl]n = 127

[(2×12) + (4×1) + 35.5]n = 127

63.5n = 127

Divide both side by 63.5

n = 127 / 63.5

n = 2

Molecular formula = [C₂H₄Cl]n

Molecular formula = [C₂H₄Cl]₂

Molecular formula = C₄H₈Cl₂

Thus, the molecular formula of the compound is C₄H₈Cl₂

Learn more about empirical formula:

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