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A compound consists of 47.5% S and 52.5% Cl by mass. Draw the Lewis structure based on the empirical formula and comment on its deficiencies. Draw a more plausible structure with the 7. same ratio of S and Cl

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jufsanabriasa

Answer:

Look picture

Explanation:

The empirical formula is obtained with average of each atom by mass over Atomic weight, thus:

47,5% S ÷ 32,045 g/mol = 1,48 mol S

52,5% Cl ÷ 35,45 g/mol = 1,48 mol Cl

Thus, empirical formula is:

[tex]S_{1,48} Cl_{1,48}[/tex] ≡ SCl.

The Lewis structure for this SCl molecule is in the picture. You can see one unpaired electron in S. These unpaired electrons are very unstable doing SCl an improbable molecule.

The more pausible structure with the same S:Cl ratio is S₂Cl₂ (Look picture). In this molecule you don't have unpaired electrons doing this compound more stable (In fact, exist, and its name is Disulfur dichloride)

I hope it helps!

Ver imagen jufsanabriasa
sebassandin

Answer:

See explanation.

Explanation:

Hello,

In this case, one could identify the subscripts in the empirical formula, based on the given percentages as shown below:

[tex]n_S=\frac{47.5g}{32g/mol}=1.48 \\n_{Cl}=\frac{52.5g}{35.45g/mol}=1.48\\ S=\frac{1.48}{1.48} =1;Cl=\frac{1.48}{1.48} =1[/tex]

Thus, the empirical formula is:

[tex]SCl[/tex]

Nevertheless, such empirical formula does not respect the sulfur's octet, based on the first drawing on the attached picture (that is a deficiency), that is why a more plausible structure is based on the following formula:

[tex]S_2Cl_2[/tex]

Which actually respect the octet based on the second drawing on the attached picture.

Best regards.

Ver imagen sebassandin