Honors Chemistry Quick Notes Review

Comprehensive vocabulary flashcards covering Experimental Design, Atomic Structure, Nuclear Chemistry, Chemical Bonding, Stoichiometry, Gases, Solutions, Acid-Base Chemistry, and Thermochemistry.

Independent Variable

The one and only factor that is changed in an experiment, graphed on the x-axis.

Dependent Variable

The factor that is measured or observed in an experiment and responds to the change in the independent variable; graphed on the y-axis.

Constants

All the factors that stay the same in an experiment.

Source Bias Indicators

A source may be biased if it is heavily opinionated, relies on unsubstantiated claims, presents highly selected facts, or has an unidentifiable author.

Atomic Number

The number of protons in an atom, which uniquely identifies an element.

Mass Number

$$\text{protons} + \text{neutrons}$$

Charge Formula

$$\text{protons} - \text{electrons}$$

Neutron ($n^{0}$)

A subatomic particle located in the nucleus with a mass of $1 \text{ atomic mass unit (AMU)}$ and a neutral charge.

Proton ($p^{+}$)

A subatomic particle located in the nucleus with a mass of $1 \text{ AMU}$ and a positive charge.

Electron ($e^{-}$)

A subatomic particle located in energy levels within the electron cloud with a negative charge.

Ground State

The state of lowest energy for an electron.

Excited State

A state reached when electrons absorb energy and jump to a higher energy level.

Photon

A particle of light emitted when an electron returns to its ground state from an excited state.

Atomic Emission Spectra

The unique pattern of light given off by an element when given energy, used to identify elements in a mixture.

Electromagnetic Radiation: Speed of Light Formula

$c = f(\lambda)$, where $c$ is speed of light ($\text{nm/s}$), $f$ is frequency ($\text{Hertz}$), and $\lambda$ is wavelength ($\text{nm}$).

Electromagnetic Radiation: Energy Formula

$E = h(f)$, where $E$ is energy ($\text{J}$), $f$ is frequency ($\text{Hertz}$), and $h$ is Planck’s Constant ($6.62 \times 10^{-34}$).

Sublimation

Phase change directly from a solid to a gas.

Deposition

Phase change directly from a gas to a solid.

Alpha Radiation

A stream of particles made of a Helium nucleus ($2$ protons and $2$ neutrons) with a charge of $+2$.

Beta Radiation

A stream of electrons with a charge of $-1$.

Gamma Radiation

High-energy photons with a charge of $0$.

Nuclear Reaction Conservation

In a nuclear equation, mass and charge are conserved, meaning the total mass and charge of reactants equals that of the products.

Half-life

The amount of time it takes for half of a radioactive isotope to decay.

Fission

The splitting of larger nuclei into $2$ or more smaller nuclei; utilized in nuclear power plants.

Fusion

The joining of $2$ or more smaller nuclei into $1$ larger nucleus; occurs in the sun and stars and produces more energy than fission.

Ionic Compound

Compounds composed of cations and anions, usually a metal and a nonmetal, held together by the transfer of electrons.

Covalent Compound

A neutral group of atoms, usually two or more nonmetals, held together by the sharing of electrons.

VSEPR (Molecular Shape)

Theory stating that the shape of a molecule depends on the repulsions of valence electrons as they try to minimize repulsion by moving as far apart as possible.

Synthesis Reaction

A chemical reaction where two or more substances combine to form a single product ($A + B \rightarrow AB$).

Decomposition Reaction

A chemical reaction where a single reactant breaks down into two or more products ($AB \rightarrow A + B$).

Combustion Reaction

A reaction where a hydrocarbon reacts with oxygen to produce carbon dioxide and water ($C_{x}H_{y} + O_{2} \rightarrow CO_{2} + H_{2}O$).

Soluble

A compound that dissolves in a solvent, labeled as $(aq)$ for aqueous.

Insoluble

A compound that does not dissolve in a solvent, labeled as $(s)$ for solid.

Metal Activity Series

A chart listing metals in order of reactivity; a solid metal will replace a lesser reactive ion if it is higher on the chart.

Limiting Reactant

The reactant that produces the lesser amount of product and runs out first in a chemical reaction.

Mole (mol)

A unit used to measure amount of substance; one mole is equal to $6.02 \times 10^{23}$ particles.

Molar Mass

The mass of $1 \text{ mole}$ of a substance.

Collision Theory

Theory stating that reactions occur when particles collide with enough energy and the correct orientation to break bonds.

Kinetic Molecular Theory

Explains gas behavior based on particles being in constant, random motion and having negligible energy loss during collisions.

Boyle’s Law

States that pressure and volume have an indirect relationship; as pressure increases, volume decreases.

Charles’ Law

States that volume and temperature have a direct relationship; as volume increases, temperature increases.

Gay-Lussac’s Law

States that pressure and temperature have a direct relationship; as pressure increases, temperature increases.

Solute

The minor part of a solution that gets dissolved.

Solvent

The major part of a solution that does the dissolving.

Molarity

A measure of concentration defined as the amount of solute in moles per volume of solution in liters ($L$).

Saturated Solution

A solution containing the maximum amount of solute dissolved; located on the line of a solubility graph.

Acid Properties

Donates an $H^{+}$, tastes sour, turns litmus red, is corrosive, and has a pH less than $7$.

Base Properties

Donates an $OH^{-}$, tastes bitter, turns litmus blue, feels slippery, and has a pH greater than $7$.

Neutralization Reaction

The reaction of an acid and a base to form water and a salt ($Acid + Base \rightarrow Salt + H_{2}O$).

Specific Heat Capacity (c)

The amount of energy required to raise the temperature of $1 \, \text{g}$ of a substance by $1 \, ^{\circ}\text{C}$. Formula: $q = mc\Delta T$.

Endothermic Reaction

A reaction that absorbs energy from the surroundings in the form of heat; heat is a reactant and $\Delta H$ is positive.

Exothermic Reaction

A reaction that releases energy into the surroundings in the form of heat; heat is a product and $\Delta H$ is negative.

Triple Point

The point on a phase diagram where all three phases (solid, liquid, gas) exist at once.

Equilibrium

A state in which forward and reverse reactions proceed at equal rates and amounts of reactants/products remain unchanging.

Le Chatelier’s Principle

States that if a stress (change in amount or temperature) is applied to a system at equilibrium, the reaction shifts to oppose that shift.

Conduction

Heat transfer between adjacent molecules.

Convection

Heat transfer involving the movement of a hot fluid.

Radiation

Heat transfer via the emission of electromagnetic rays.