Question

1. explain are all compounds molecules? why or why not? 4. compare ionic bonds and covalent bonds. 5. explain how the number of electrons in an energy level affects bond formation. 6. beryllium has four protons in its nucleus. how many neutrons are in beryllium - 9? explain how you calculated your answer.

Explanation:

3.

Not all compounds are molecules. Compounds are substances made of two or more elements. Molecules are formed by covalent - bonding. Ionic compounds, held together by ionic bonds, are not molecules. For example, sodium chloride (NaCl) is a compound but not a molecule as it exists as a crystal - lattice of ions.

Ionic bonds form when one atom donates electrons to another, creating ions that attract each other. Covalent bonds form when atoms share electrons. Ionic compounds often form crystals and have high melting points, while covalent compounds can be gases, liquids or solids with lower melting and boiling points in general.

Atoms aim for a stable electron configuration, often with a full outer energy level. If an energy level is not full, atoms can gain, lose or share electrons to achieve stability, forming bonds. For example, atoms with 1 - 3 valence electrons may lose them, while those with 5 - 7 may gain electrons to fill their outer shell.

Answer:

No, because some compounds like ionic compounds are not held together by covalent bonds to form molecules.

4.