Two atoms with an electronegativity difference of 0. 4 form a bond that is.

Chemistry

1 answer:

stepan [7]2 years ago

8 0

Answer:

Nonpolar Covalent

Explanation:

There are 3 main types of bonds: Nonpolar covalent, polar covalent, and ionic. All of them have multiple aspects that set them apart from each other, but in this case, the electronegativity difference is the focus. Electronegativity difference is the difference in the electronegativity values of 2 atoms. For example, Nitrogen has an electronegativity value of 3.04 and Oxygen is 3.44, so their electronegativity difference is 0.4.

Electronegativity values that range from 0 to 0.4 are nonpolar covalent, 0.5 to 1.9 is polar covalent, and 2 and above is ionic. Since the difference in this question is 0.4, the bond must be nonpolar covalent.

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A solution made by dissolving 33 mg of insulin in 6.5 mL of water has an osmotic pressure of 15.5 mmHg at 25°C. Calculate the mo

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Explanation:

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$\pi=iMRT$

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$\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT$

where,

$\pi$ = osmotic pressure of the solution = 15.5 mmHg

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (insulin) = 33 mg = 0.033 g (Conversion factor: 1 g = 1000 mg)

Volume of solution = 6.5 mL

R = Gas constant = $62.364\text{ L.mmHg }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$15.5mmHg=1\times \frac{0.033\times 1000}{\text{Molar mass of insulin}\times 6.5}\times 62.364\text{ L.mmHg }mol^{-1}K^{-1}\times 298K\\\\\text{molar mass of insulin}=\frac{1\times 0.033\times 1000\times 62.364\times 298}{15.5\times 6.5}=6087.2g/mol$