What is wrong with or ambiguous about the phrase "four molecules of NaCl"

I really don't understand my textbook says in the back that it is an ionic compound so I guess that its not really a molecule then I don't understand...

NaCl is an ionic compound. It is a solid made up of Na^+ and Cl^- interlaced into a three dimensional crystal lattice; thus there is no NaCl molecule as such. We write the formula as NaCl because that is the simplest empirical formula but it really is NaxClx because the Na^+ and Cl^- are repeating in all three dimensions. It is not possible to obtain four "molecules" of NaCl (or one or sixteen or any other number). It IS possible to obtain four formula weights of NaCl and there are many chemists in the world that don't like to use the terms molecular weight, molecular mass, or molar mass when talking about ionic crystals for the very reason that these don't exist as molecules. Those chemists prefer to use the term formula weight or formula mass. So the formula weight of NaCl is about 58.5 and that gets around the problem of NaCl not existing as a true molecule. CO2 is not an ionic compound and it does exist as a molecule. We can weigh a mole of molecules of CO2 (about 44 grams) or we can weigh a formula weight of NaCl (about 58.5 grams).

Very good

Ah, the wonders of chemistry! Let me break it down for you in my own bot-tastic way. So, the phrase "four molecules of NaCl" might sound a bit confusing because NaCl, or sodium chloride, is indeed an ionic compound, not a molecule.

You see, molecules are formed when atoms share electrons, creating covalent bonds. But in the case of ionic compounds like NaCl, the atoms don't share electrons, they give them away. Sodium (Na) gives away an electron to chlorine (Cl) to form an ionic bond, resulting in charged ions (Na+ and Cl-).

So, technically speaking, we wouldn't refer to NaCl as "molecules" since it lacks covalent bonds. It's more accurate to say "four units" or "four formula units" of NaCl.

Remember, chemistry can sometimes be an amusing enigma. Keep up the good work, and don't hesitate to ask if you have any more questions!

The phrase "four molecules of NaCl" is ambiguous and can be misleading. Here's why:

1. Ionic compound: Sodium chloride (NaCl) is indeed an ionic compound, not a molecule. In an ionic compound, such as NaCl, the atoms are held together by ionic bonds, where positively and negatively charged ions attract each other.

2. Definition of a molecule: A molecule is a group of atoms that are chemically bonded together. Molecules can be formed by covalent bonds, where atoms share electrons, or by metallic bonds.

3. Structure of NaCl: In NaCl, one sodium ion (Na+) and one chlorine ion (Cl-) are held together by an ionic bond. This forms a crystal lattice structure. So, NaCl does not consist of individual molecules like covalent compounds do.

Therefore, it would be more accurate to refer to "four formula units of NaCl" rather than "four molecules of NaCl" to describe the amount of sodium chloride.

The phrase "four molecules of NaCl" is technically incorrect or ambiguous because NaCl is not composed of discrete molecules. Instead, it is an ionic compound made up of individual sodium ions (Na+) and chloride ions (Cl-), arranged in a repeating lattice structure.

In an ionic compound, like NaCl, the atoms are held together by strong electrostatic forces, not covalent bonds as found in molecules. This results in the formation of a crystal lattice rather than distinct molecules.

To understand why NaCl is not a molecule, let's break it down.

First, let's consider the sodium (Na) atom. Sodium has one electron in its outermost shell, and it is energetically favorable for it to lose this electron to achieve a stable electron configuration. When sodium loses an electron, it forms a positively charged sodium ion (Na+).

Next, we have the chlorine (Cl) atom. Chlorine has seven electrons in its outermost shell, and it can gain one electron to complete its octet and achieve a stable electron configuration. When chlorine gains an electron, it forms a negatively charged chloride ion (Cl-).

In the case of NaCl, the positively charged sodium ions (Na+) and negatively charged chloride ions (Cl-) are attracted to each other, forming an ionic bond. This electrostatic attraction holds the ions together in a solid crystal lattice structure.

So, instead of referring to "four molecules of NaCl," it would be more accurate to say "four formula units of NaCl" or "four ionic compounds of NaCl." This clarifies that NaCl is not a discrete molecule but rather a compound composed of ions arranged in a crystalline lattice structure.