Calculate the electronegative differences (see table on the last page) for the a

Question

Calculate the electronegative differences (see table on the last page) for the atoms in the following bonds and determine which of the atoms carries a larger share of negative charge of the bonding electrons. a. CH b. HF a. Calculate the electronegative difference of the atoms in the (polar) CO bond. b. Would you expect CO_2 to be a polar or non-polar molecule? Explain your answer. Why is water almost never 100 % pure? Water and methane have similar molar masses (water: 18 g/mol, methane 16 g/mol), yet methane is a gas at room temperature and water is a liquid. Why does water to retain its liquid state at higher temperatures compared to methane?

Explanation / Answer

(13) According Pauling's scale,

electro negativity of C = 2.5, H = 2.1, O = 3.5 and F = 4.0

(a) In C - H bond since the carbon is more electro negative than hydrogen, the bond pair of electrons are crried larger share by Carbon.

Difference in electronegativity of C-H bond = 2.5 - 2.1 = 0.4

(b) In H - F bond since the fluorine is more electro negative than hydrogen, the bond pair of electrons are crried larger share by Fluorine

Difference in electronegativity of H-F bond = 4.0 - 2.1 = 1.9

(14) (a) Difference in electronegativity of CO bond = 3.5 - 2.5 = 1.0

(b) CO2 molecule is in linear shape.

O=C=O

in C=O bond, O is more electronegative than C, so the bondpair of electrons are more effectively attracted by O. But the both oxygen atoms are at opposite sides, and net polarity gets cancelled. Hence the CO2 molecule is non polar.

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