Chem Semester 2 Exam

aq

Dissolved in water.

Solid forms

Precipitate

Subscript

Indicates the number of atoms of a species.

dbl replacement reaction

A reaction where the cation and anion of two reactants switch places to form two new products

Activity Series

Check to see if a single replacement reaction will occur.

Solubility Table

Check for solid product (precipitate) in a double replacement reaction

S

Soluble

N.R.

No Reaction

Balancing Species Order

Polyatomics, Metals, Non-metals, Hydrogen, Oxygen

Electrolyte

A substance that creates a flow of electrons (usually from ions) when in aqueous solution; includes salts, acids, and bases.

Limiting Reagent

The reactant that is totally consumed when the chemical reaction is complete.

Percent Yield

Actual Yield/Theoretical Yield * 100

Empirical Formula

The simplest whole number ratio of atoms in a compound.

Molecular Formula

The actual number of atoms of each element in a molecule.

Exothermic Reaction

A reaction that releases heat from the system to the surroundings.

Endothermic Reaction

A reaction that absorbs heat from the surroundings to the system.

Kinetic Energy

Energy of motion

Potential Energy

Stored energy

Intermolecular Forces

Forces of attraction between molecules.

Triple Point

The temperature and pressure at which the solid, liquid, and vapor phases of a substance coexist in equilibrium.

Boyle's Law

The volume of a gas is inversely proportional to its pressure (at constant temperature).

Charles's Law

The volume of a gas is directly proportional to its absolute temperature (at constant pressure).

Gay-Lussac's Law

The pressure of a gas is directly proportional to its absolute temperature (at constant volume).

Valence Electrons in Covalent Bonds

Shared so the molecule becomes stable.

Polar Covalent Molecule

Unequal sharing of electrons, resulting in dipoles.

Non-Polar Covalent Molecule

Equal sharing of electrons.

Like Dissolves Like

Polar substances dissolve in polar substances, and nonpolar substances dissolve in nonpolar substances.

Solution

A homogeneous mixture composed of a solvent and a solute.

Miscible

Two liquids that dissolve in each other.

Immiscible

Two liquids that do not dissolve in each other.

Supersaturated Solution

A solution in which the saturation point has been exceeded, but no precipitate (solid) is present.

Net Ionic Equation

A chemical equation that only shows the ions and molecules directly involved in the reaction.

Strong Electrolytes

Completely dissociate in aqueous solutions.

Neutralization Reaction

Reaction between a strong acid and strong base to produce water and a salt.

Bronsted-Lowry Acid

H+ donor (proton donor).

Bronsted-Lowry Base

H+ acceptor (proton acceptor).

Equivalence Point

The point in a titration where moles of H+ equals moles of OH-.