Basic Concept of Chemistry Part 3

Observe that only electrons participate in bonding, as shown by lithium's shell structure; outer-shell electrons drive bonding, while noble gases with full outer shells remain stable and unreactive.

Explore how atoms achieve a complete outer shell like noble gases through electron transfer, forming ions and ionic bonds, driven by octet stability, as shown by sodium and chlorine.

Metals give away electrons to form positive ions, while nonmetals gain electrons to form negative ions, achieving noble gas configurations for stability; these oppositely charged ions attract and bond.

Chlorine and oxygen, non-metals, gain electrons to complete their octets and form negative ions, while metals like sodium and magnesium lose electrons to form positive ions, creating ionic bonds.

Explain how ionic bonding forms a giant ionic structure with strong attractions that yield high melting and boiling points, brittleness, and solubility in water due to polarity.

Ionic compounds conduct electricity when ions are present and free to move; solid-state ions cannot move, but in molten or aqueous form they move, enabling conduction.

Shows how covalent bonding forms by sharing electrons in methane, water, and carbon dioxide, enabling octets and stability.

Explore giant covalent macromolecules, such as diamond and graphite, formed by strong covalent bonds in three-dimensional and hexagonal carbon networks, and the silicon dioxide network with silicon–oxygen bonding.

Form a diamond macromolecule in a 3d covalent network, with each carbon forming four bonds. Yields high melting points, high density, and not volatile or soluble, except graphite conductivity.

Identify simple covalent molecules as small, volatile compounds with low melting and boiling points and low density. Note that weak intermolecular forces connect iodine molecules, while covalent bonds are strong.