AP CHEM: Summer Vocab

Absorbance

Light that does not pass through a solution A \= abc

Activation Energy

Minimum energy that needs to be added to a system in order for the chemical reaction to occur

Alpha Particle

He2+ 2 protons, mass number \= 4, 2+ charge Highly ionizing particle; Low energy

Anion

Negatively charge ion

Arrhenius Acid

Donates a H+ ion

Arrhenius Base

Donates a OH- ion

Atom

Smallest constituent unit of ordinary matter that has the properties of a chemical element

Average Atomic Mass

Average of all naturally occurring isotopes

Atomic Number

Number of protons; defines the atom

Beta Particle

-1 proton, mass number \=0; medium ionizing ability, medium energy

Boiling

Phase change from a liquid to a gas

Bronsted-Lowry Acid

Donates a proton, H+

Bronsted-Lowry Base

Accepts a proton, H+

Calorimetry

Means of measuring the heat gained/ lost by a system during a chemical reaction

Catalyst

Lowers the activation energy. Consumed in one step and produced in another

Cation

Positively charged ion

Chemical Equilibrium

Rate of the forward reaction equals the rate of the reverse reaction

Condensation

Phase change from a gas to a liquid

Conversion Factor

Allows for the conversion from one unit of measure to another

Covalent Bond

Bond formed by the sharing of electrons between atoms.

Deposition

Phase change from a gas to a solid

Dipole-Dipole

Permanent IMF between molecules caused by the permanent dipole moment within the polar molecules

Direct Relationship

Relationship between two variables where when one changes, the other changes in the same manner

Dissociate

To break into ions

Dissolve

To break into smaller pieces

Distillation

Process of separating liquids based on differences in boiling temperatures

Double Bond

Two shared pairs of electrons

Electrolyte

Dissociates into charged particles which are capable of conducting electricity

Electrolytic Cell

Redox reaction that is not spontaneous

Electron Affinity

Energy released when an atom/ion gains an electron

Electron

Negatively charged particle. Charge \= -1, Mass ~0amu. Located in the orbitals surrounding the nucleus

Electronegativity

The ability of an atom to attract electrons towards its nucleus

Empirical Formula

Lowest whole number ratio of atoms in a compound

Exothermic

Energy is released by the system

Filtrate

Liquid that passes through the filter paper

Filtration

Process of separating a precipitate from its aqueous solution

Formula Unit

Small whole-number ratio of ionically bonded atoms

Freezing

Phase change from a liquid to a solid

Galvanic / Voltaic Cell

Redox reaction that is spontaneous

Gamma Ray

0 protons, mass number \= 0, Low ionizing ability, high energy

Halogen

Elements in group 17. Form halides as ions. Have a 1- charge

Hydrogen Bonding

Strong dipole moment between molecules that results when H is bonded to F, O, or N within the molecule

Indirect relationship

Relationship between two variables where when one changes, the other changes in the opposite manner

Insoluble

Does not dissolve in water

Intermediate

Species produced in one step and consumed in another step

Intermolecular Forces, IMF

Attractive forces between molecules

Ion

Charged particle

Ionic Bond

Bond formed by the transfer of 1 or more electrons from the least electronegative atom to the more electronegative atom

Ionization Energy

Energy required to remove the outer electron from a gaseous atom

Kinetic Energy

Energy of motion, temperature is a measure of KE

Limiting Reactant

Reactant to runs out first thus limiting the amount of product that can be formed

London Dispersion Forces

Temporary IMF between molecules caused by the movement of electrons within the molecule

Lone Pair

Unbonded electrons

Mass Number

Mass of all protons and neutrons

Melting

Phase change from a solid to a liquid

Molar Mass

grams per 1 mol

Molarity

moles of solute per liter of solution

Molecular Formula

actual number of moles of each atom in a compound

Molecule

Covalently bonded atoms

Neutron

Neutral particle. No charge. Mass \= 1amu, Located in the nucleus

Noble Gas

Group 18 on the PT. Each has 8 valence electrons. Nonreactive

Orbital

Regions of probability where electrons are located. Each orbital can contain up to 2 electrons

Oxidation Number

A charge assigned to an atom that represents that charge it would have if it contained and ionic bond. Are written as charge value, +4, -6, +2

Oxidation

Process of losing electrons which increases the oxidation number

Percent Error

Absolute value (Theoretical - Experimental) / Theoretical) x 100%

Percent Yield

(Quantity produced / Theoretical Amount) x 100%

Precipitate

Solid matter that forms from the reaction of two aqueous solutions

Principle Energy Level

n, n\=1 is first energy level, n\=2 is secind energy level...Principle energy levels contain sublevels

Proton

Positively charged particle. Charge \= +1, Mass \= 1amu, Located in the nucleus

Reduction

Process of gaining electrons which reduces the oxidation number

Significant Figures

Those digits that carry meaning contributing to its precision

Single Bond

One shared pair of electrons

Soluble

Dissolves in water

Solute

The species that gets dissolved to form a solution

Solution

Solute and solvent

Solvent

The species that does the dissolving to form a solution

Specific Heat

Energy required to raise 1 gram of a substance 1C

Strong Acid

Dissociates 100% to produce H+

Strong Base

Dissociates 100% to produce OH-

Sublevel

s, p, d, and f. defines the shape

Sublimation

Phase change from a solid to a gas

Surroundings

This refers to everything outside of the system

System

This refers to the reaction

Transmittance

Light that passes through a solution and reaches the detector

Triple Bond

Three shared pairs of electrons

Valence electrons

Outer electrons which are available for bonding

Weak Acid or Base

Dissociates very little. Remains mostly in its molecular form

Molality

kg solute / Liter of Solvent

JJ Thomson

Discovered the e-

Goldstein

Discovered the P

Chadwick

Discovered the N

Rutherford

Theorized the nuclear model of the atom

Coulombic Attraction

Force of attraction as protons pull electrons inward

Ideal Gas Law

PV\=nRT

Enthalpy

Delta H - (endo/exo)

Entropy

Delta S - (disorder/order)

Gibbs Free Energy

Delta G - Energy available to do work

Hvap

Energy required to change 1 mol (l) to (g)

Hfus

energy required to change 1 mol (s) to (l)

Endothermic

Energy is gained by the system