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Chapter 20: Problem 13

Comment on the relationship (if any) between the charge on a molecule or ion and the sum of the partial charges on all the atoms in the species.

Short Answer

Expert verified
The sum of partial charges on all atoms in a species equals the total charge on that species. This balance is observed regardless of whether the total charge is neutral or not, and forms a fundamental aspect of molecular structures and bonding in chemistry.

Step by step solution

01

Understanding: Total Charge and Partial Charges

Total charge is the net charge of a molecule or ion. It is determined by the number of protons in the nucleus, minus the number of electrons surrounding the nucleus, considering any extra electrons gained (in the case of negative ions) or lost (in the case of positive ions). In comparison, a partial charge is a charge less than the full charge of an electron, represented by δ+ or δ−. It arises due to the unequal sharing of electrons in covalent bonds, where more electronegative atoms pull the shared electrons closer to them, causing them to have a partial negative charge δ− and leaving the other atom with a partial positive charge δ+.
02

Relationship: Total Charge and Partial Charges

The sum of the partial charges on all atoms in a molecule or ion always equals to the total charge of the molecule or ion. This is because all the charges in the system - whether they are full charges on ions or partial charges on atoms within a molecule - must be accounted for. In a system in equilibrium, the charges should balance out, meaning the sum of charges occurring due to differences in electronegativity (partial charges) should equal the total charge.
03

Example: Water Molecule

In a water molecule (H2O), there are partial positive charges on the hydrogen atoms and a partial negative charge on the oxygen atom. The sum of these partial charges equals the total charge on the water molecule, which is neutral (0). This illustrates that in a balanced molecule, the sum of partial charges equals the total charge.

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Most popular questions from this chapter

For any diatomic molecule \(\mathrm{A}-\mathrm{B}\), what is the following sum: \(\delta_{\mathrm{A}}+\delta_{\mathrm{B}}\) ?

a) Why does the oxygen atom in water have a negative partial charge? b) Why does the sulfur atom in dihydrogen sulfide have a negative partial charge? c) Why is the oxygen atom in \(\mathrm{H}_{2} \mathrm{O}\) more negatively charged than the sulfur atom in \(\mathrm{H}_{2} \mathrm{~S}\) ?

Compare the values of the partial charges on the nitrogen atom in ammonia and on the nitrogen atom in nitrogen trifluoride. Rationalize the positive and negative aspects of these charges.

When two different atoms share electrons, which atom (in terms of electronegativities) has the partial negative charge?

For HF, why is the partial negative charge on the fluorine atom, and why is the magnitude of the partial charge on fluorine equal to the magnitude of the partial charge on hydrogen?
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