Use the symbols δ^+and δ^-to show the direction of the polarity of the indicated bond in each of

Use the symbols δ^+and δ^-to show the direction of the...

Use the symbols $\delta^{+}$and $\delta^{-}$to show the direction of the polarity of the indicated bond in each of the following compounds: a. $\mathrm{HO}-\mathrm{H}$ c. $\mathrm{H}_{3} \mathrm{C}-\mathrm{NH}_{2}$ e. $\mathrm{HO}-\mathrm{Br}$ g. I-Cl b. $\mathrm{F}-\mathrm{Br}$ d. $\mathrm{H}_{3} \mathrm{C}-\mathrm{Cl}$ f. $\mathrm{H}_{3} \mathrm{C}-\mathrm{Li}$ h. $\mathrm{H}_{2} \mathrm{~N}-\mathrm{OH}$

Use the symbols $\delta^{+}$and $\delta^{-}$to show the direction of the polarity of the indicated bond in each of the following compounds:
a. $\mathrm{HO}-\mathrm{H}$
c. $\mathrm{H}_{3} \mathrm{C}-\mathrm{NH}_{2}$
e. $\mathrm{HO}-\mathrm{Br}$
g. I-Cl
b. $\mathrm{F}-\mathrm{Br}$
d. $\mathrm{H}_{3} \mathrm{C}-\mathrm{Cl}$
f. $\mathrm{H}_{3} \mathrm{C}-\mathrm{Li}$
h. $\mathrm{H}_{2} \mathrm{~N}-\mathrm{OH}$

Key Concepts

Partial Charge Notation

Partial charge notation, using the symbols ?+ and ??, is a conventional way to indicate the relative electron density on atoms within a bond. The ?+ symbol marks the electron-deficient side (less electronegative atom), while the ?? symbol marks the electron-rich side (more electronegative atom), helping to visualize the bond’s polarity.

Bond Polarity

Bond polarity arises when two bonded atoms have different electronegativities, causing one atom to attract the shared electrons more strongly. This results in a polar covalent bond where one end of the bond acquires a partial negative charge (??) and the other end a partial positive charge (?+).

Electronegativity

Electronegativity is a property of an atom that describes its ability to attract electrons toward itself when bonded to another atom. This concept is central to understanding how electrons are distributed in a bond, and differences in electronegativity between atoms lead to an uneven electron distribution.

Transcript

00:01 In this question we have been given several molecules and we need to just use the symbols delta plus and delta minus to show the direction of the polarity of the indicated bond right in each of the given compounds so first of all we need to know what are the signs representing so this sign delta positive represents the partial positive charge right the partial positive charge and delta negative represents the partial negative charge which means that the that the atom that has the higher electron density on itself would contain the delta negative charge and vice versa and we can say that delta positive would be contained by an atom that has the lower electron density on itself right so first of all we can say that we have the compound hoh and in this compound we have the bond oxy bond between oxygen and hydrogen now it is very much clear that from the periodic table the electrone negativity of hydrogen is given as 2 .1 while for oxygen it is 3 .5 which means that oxygen would tend to attract the bond pair of electrons towards itself due to which the electron density increases on the oxygen end and hence it contains the partial negative charge while hydrogen would contain the partial positive charge similarly we have the compound b that is f br now for floating the value of electronegenegativity is 4 .0 and for bromine the value of electronegativity is somewhere around 2 .8 right so we can say that since the higher electronegativity atom fluorine would tend to attract the bond pay towards itself, electro -negativity and we can say electron density would further increase on the fluorine end and that is why it would contain partial negative charge while bromine would contain partial positive charge.

01:44 So now using these two examples, we can clearly assume that the atom with more electronegativity or higher electromagnetic value would contain partial negative charge while the one that has the lower value of electronegativity would contain the partial positive charge...

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