C101 Final Exam Vocabulary Review

Comprehensive vocabulary flashcards covering basic chemistry principles, atomic structure, bonding, reactions, thermochemistry, and electrochemistry based on the final exam topic list.

Physical Change

A change in matter that does not result in a new substance, such as a change in state or appearance.

Chemical Change

A change that results in the formation of one or more new substances with different properties.

Density

The ratio of mass to volume, often used in calculations where $D = \frac{m}{v}$.

Metric Conversions

The system of units involving prefixes such as kilo- ($10^3$), centi- ($10^{-2}$), and milli- ($10^{-3}$).

Alkali Metals

The family of elements found in Group 1 of the periodic table.

Alkaline Earth Metals

The family of elements found in Group 2 of the periodic table.

Valence Electrons

The electrons located in the outermost shell of an atom, determined by the group number (1-2, 13-18) on the periodic table.

Ionic Bonds

Chemical bonds formed through the electrostatic attraction between cations and anions.

Covalent Bonds

Chemical bonds formed by the sharing of electron pairs between atoms.

VSEPR

Valence Shell Electron Pair Repulsion theory used to determine the molecular shape based on electron geometry.

Intermolecular Forces

The forces of attraction between molecules in a pure sample that determine physical properties.

Solubility Rules

A set of guidelines used to predict whether a salt will dissolve in water or form a precipitate.

Endothermic

A process or reaction that absorbs energy from its surroundings.

Exothermic

A process or reaction that releases energy into its surroundings.

Specific Heat Capacity

The amount of energy required to raise the temperature of a substance, used in the formula q = mc\text{\Delta}T.

Ideal Gas Law

The mathematical relationship between pressure, volume, moles, and temperature defined as $PV = nRT$.

Combined Gas Law

The relationship used to calculate changes in gas properties, expressed in the transcript as $\frac{P_1 V_1}{P_2 V_2} = \frac{n_1 T_1}{n_2 T_2}$.

Oxidation

The loss of electrons by a chemical species, resulting in an increase in oxidation number.

Reduction

The gain of electrons by a chemical species, resulting in a decrease in oxidation number.

Molarity

A measure of solution concentration defined as the number of moles of solute per liter ($L$) of solution.

Brønsted-Lowry Definition

A theory that identifies acids as proton ($H^+$) donors and bases as proton acceptors.

Isotopes

Atoms of the same element that have the same number of protons (atomic number) but different numbers of neutrons (mass number), often represented in $\text{}^A_Z X$ format.

Limiting Reactant

The reactant in a chemical reaction that is completely consumed first, limiting the amount of product that can be formed.

Anode

The electrode in a voltaic cell where oxidation occurs.

Cathode

The electrode in a voltaic cell where reduction occurs.