Lab 3.1: Properties of Ionic and Covalent Compounds

1. Ionic compounds generally have a high melting point, dissolve in water, and conduct electricity.
2. Covalent substances generally have a low melting point, don't dissolve in water, and don't conduct electricity.
3. Ionic bonds form from a metal and a non metal. The electrons are transferred.
4. Covalent bonds form from two non metals. The electrons are shared.
5. Covalent bonds don't conduct electricity because the electrons are fixed in one place and can't move freely.
6. When in solid form, ionic substances electrons can't move freely. Dissolving them separates the ions and allows them to move around.
Enrichment: When athletes sweat, they lose electrolytes. These electrolytes are needed to perform muscle function. The most commonly used electrolytes are dissolved metal salts. Some electrolytes used are Potassium, sodium, and chloride.

Lab 3.1: Modeling Molecules

1. I think the bond between ions is stronger than the bond between molecules because most ionic bonds have a higher melting point. Ionic bonds are also electrically attracted to each other, while molecules are not.

2.When you melt something, it's a physical change. Physical changes don't rearrange the atoms, chemical changes do. Therefore if you melted HCl molecules, they would not seperate.


3. When ionic substances are melted, the molecules are free to move around and create a charge.

4. Molecular substances do not create a charge because molecules have a neutral charge.

 Enrichment:
                    A polar molecule is a molecule with a bond from having two atoms with opposite charges. Water is a polar molecule.