General Chemistry Lecture Review

These flashcards cover key vocabulary terms and definitions from the lecture on general chemistry, focusing on the concepts of atomic structure, types of bonds, and properties of water.

Intramolecular Bonds

Bonds that occur within a molecule, including ionic and covalent bonds.

Ionic Bond

A type of bond formed when a metal donates an electron to a nonmetal, resulting in charged ions (cations and anions). Example: Sodium Chloride (NaCl).

Covalent Bond

A type of bond formed when two nonmetals share electrons to balance their valence shells. Example: Water (H2O).

Hydrogen Bond

A weak bond that occurs between a hydrogen atom and a nonmetal atom, owing to electrostatic forces.

Octet Rule

The principle that atoms are most stable when they have eight electrons in their valence shell.

Isomer

Compounds with the same chemical formula but different structural arrangements.

Cation

A positively charged ion formed when an atom loses one or more electrons.

Anion

A negatively charged ion formed when an atom gains one or more electrons.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Functional Groups

Specific groups of atoms within molecules responsible for the characteristic chemical reactions of those molecules.

Polar Covalent Bond

A covalent bond where electrons are shared unequally, leading to partial positive and negative charges.

Universal Solvent

A term used to describe water, which can dissolve many substances due to its polar nature.

Hydrogen Ion (H+)

A positively charged ion formed when a hydrogen atom loses its electron.

Hydroxide Ion (OH-)

A negatively charged ion consisting of one oxygen atom and one hydrogen atom.

Isotope

Atoms of the same element with different numbers of neutrons, which can be radioactive.

Lewis Dot Structure

A diagram that shows the bonding between atoms and the lone pairs of electrons in a molecule.