In a crystal of salt there are electrons and

positive ions.
How does the net charge of the electrons
compare with the net charge of the ions?
1. Unable to determine
2. Sometimes the net charge of the negative
electrons is greater than the net charge of the
ions and sometimes it is less.
3. The net charge of the negative electrons
is less than the net charge of the ions.
4. The net charge of the negative electrons
is greater than the net charge of the ions.
5. The net charge of the negative electrons
has the same magnitude as the net charge of
the ions.

What holds the dang crystal together?

In a crystal of salt, the net charge of the electrons compared to the net charge of the ions can be determined by considering the nature of ionic bonding.

Salt (NaCl) is composed of sodium ions (Na+) and chloride ions (Cl-). The sodium ion has a positive charge because it has lost an electron, while the chloride ion has a negative charge because it has gained an electron.

The net charge of the negative electrons compared to the net charge of the ions can be explained by considering the overall charge neutrality of the crystal. In an ionic compound like salt, the total positive charge carried by the cations (positive ions) must be equal to the total negative charge carried by the anions (negative ions).

Since each sodium ion has a single positive charge (Na+), and each chloride ion has a single negative charge (Cl-), the net charge of the cations is equal in magnitude but opposite in sign to the net charge of the anions.

Therefore, the net charge of the negative electrons is equal in magnitude but opposite in sign to the net charge of the positive ions. In other words, the net charge of the negative electrons has the same magnitude as the net charge of the ions (option 5).

To summarize, considering the charge neutrality requirement of the crystal and the nature of ionic bonding, the correct answer is option 5 - the net charge of the negative electrons has the same magnitude as the net charge of the ions.