Question

Indicate the direction of polarity of each of the following covalent bonds by dragging the appropriate delta notation to each end of the bond.
please just write a + or - not the bonds. PLEASE HELP!!!!
C-O
O-Cl
O-F
C-N
Cl-C
S-H
S-Cl

Answer 1

(C-O) + - , (O-Cl) - - , (O-F) - - , (C-N) + - , (Cl-C) - + , (S-H) - + , (S-Cl) - +

Answer 2

The bond is said to be polar if there is difference in electronegativity between atoms of elements. Here, the more electronegative atom can attract bonding pair of electrons towards itself and gets partial negative charge. Partial positive charge is acquire by atom of less electronegative element. The direction of polarity will be from less electronegative to more electronegative atom.

C-O:

Here, oxygen(3.44) is more electronegative than carbon(2.55) thus, it can be represented as: $C^{\aa +}-O^{\aa -}$

O-Cl

Here, oxygen(3.44) is more electronegtive than chlorine(3.16) thus, it can be represneted as:

$O^{\aa -}-Cl^{\aa +}$

0-F

Here, fluorine(3.98) is more electronegative than oxygen(3.44) thus, it can be represented as:

$O^{\aa +}-F^{\aa -}$

C-N

Here, nitrogen(3.04) is more electronegative than carbon(2.55) thus, it can be represented as:

$C^{\aa +}-N^{\aa -}$

Cl-C

Here, chlorine(3.16) is more electronegative than carbon(2.55) thus, it can be represented as:

$Cl^{\aa -}-C^{\aa +}$

S-H

Here, sulfur(2.58) is more electronegative than hydrogen(2.20) thus, it can be represented as:

$S^{\aa -}-H^{\aa +}$

S-Cl

Here, chlorine(3.16) is more electronegative than sulfur(2.58) thus, it can be represented as:

$S^{\aa +}-Cl^{\aa -}$