SAAT Chemistry Comprehensive Review Flashcards

Chemistry flashcards based on the SAAT material, focusing on vocabulary, definitions, and key scientific laws found in the lecture notes.

Analytical Chemistry

A branch of chemistry that studies the types and composition of substances.

Mass

A measure of the amount of matter that remains constant and is unaffected by gravity.

Intensive Property

A physical property that remains the same regardless of how much of a substance is present, such as density.

Ozone

A substance found in the stratosphere that absorbs harmful ultraviolet (UV) radiation; one molecule is formed by three oxygen atoms ($O_3$).

Scientific Method

A systematic approach to problem-solving that includes observation, hypothesis, experimentation, data collection, and conclusion.

Qualitative Data

Observations that describe physical characteristics such as color, smell, or taste.

Quantitative Data

Numerical information that measures properties like mass, volume, temperature, and pressure.

Sublimation

The phase change in which a solid changes directly into a gas without becoming a liquid.

Deposition

The process where a substance changes from a gas to a solid without passing through a liquid state.

Compound

A substance with a definite composition made of two or more different elements chemically combined.

Organic Chemistry

 The branch of chemistry that focuses on compounds containing carbon.

Plasma

A state of matter that is the primary component of stars and galaxies, characterized by indefinite shape and volume.

Atom

The smallest part of an element that retains the properties of that element.

Isotopes

Atoms of the same element that have the same number of protons but different numbers of neutrons.

Radioactive Decay

A spontaneous process in which unstable nuclei lose energy by emitting radiation.

Alpha Particle

A particle emitted during decay consisting of two protons and two neutrons ($^{4}_{2}He$).

Synthesis Reaction

A chemical reaction in which two or more substances react to form a single product.

Limiting Reactant

The substance that is completely consumed in a chemical reaction and determines the amount of products formed.

Stoichiometry

The study of the relationship between the amounts of reactants and products in a chemical reaction.

Avogadro's Number

The number of atoms or molecules in one mole of a substance, equal to $6.02 \times 10^{23}$.

Percent Yield

The ratio of actual yield to theoretical yield expressed as a percentage.

Wavelength

The shortest distance between two successive peaks or troughs of a wave.

Photon

A massless particle that carries a quantum of energy.

Heisenberg Uncertainty Principle

States that it is impossible to simultaneously determine both the position and velocity of an electron.

Valence Electrons

Electrons in the atom's outermost orbitals that determine its chemical properties and ability to bond.

Hund's Rule

States that electrons fill orbitals of equal energy singly first before pairing up.

Electronegativity

A measure of an atom's ability to attract bonding electrons.

Ionization Energy

The energy required to remove an electron from a gaseous atom.

Lattice Energy

The energy released when ions combine to form an ionic compound, increasing with higher charge and smaller atomic radius.

Diffusion

The movement of particles from an area of higher concentration to an area of lower concentration.

Viscosity

A measure of a liquid's resistance to flow.

Surface Tension

The result of strong cohesive forces that allow a liquid surface to resist an external force, such as a spider walking on water.

Dalton's Law

States that the total pressure of a gas mixture is equal to the sum of the partial pressures of all gases in the mixture.

Absolute Zero

The lowest possible temperature, equal to $0\,K$ or $-273^{\circ}C$.

Boyle's Law

States that at constant temperature, the volume of a gas is inversely proportional to its pressure ($P_1V_1 = P_2V_2$).

Charles' Law

States that at constant pressure, the volume of a gas is directly proportional to its Kelvin temperature ($\frac{V_1}{T_1} = \frac{V_2}{T_2}$).

Exothermic Reaction

A chemical change that releases energy to the surroundings, often in the form of heat.

Specific Heat

The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.

Activation Energy

The minimum amount of energy required for reacting particles to form an activated complex and initiate a reaction.

Catalyst

A substance that increases the rate of a chemical reaction by lowering the activation energy without being consumed.

Fractional Distillation

A method used to separate crude oil into simpler components based on their different boiling points.

Polymer

Large molecules made up of many repeating building blocks called monomers.

Tyndall Effect

The phenomenon where light is scattered by particles in a colloid or a fine suspension.

Molarity ($M$)

The number of moles of solute dissolved per liter of solution.

Molality ($m$)

The number of moles of solute per kilogram of solvent.

Buffer Solution

A solution that resists changes in pH when small amounts of an acid or base are added.

Oxidation

The process of losing electrons, resulting in an increase in the oxidation number.

Reduction

The process of gaining electrons, resulting in a decrease in the oxidation number.

Anode

The electrode where oxidation occurs in an electrochemical cell.

Cathode

The electrode where reduction occurs in an electrochemical cell.