Chemistry Regents Review

Vocabulary flashcards based on Chemistry Regents review notes.

Tie back long hair

A safety measure to prevent interference or hazards during experiments.

Rinse and inform teacher

Standard procedure to follow when a liquid is spilled on the skin during a lab.

Proper chemical disposal

The act of disposing of chemical waste in correct containers.

Proton

Subatomic particle with a positive charge.

Neutron

Subatomic particle with a neutral charge.

Nucleus

The location of protons and neutrons.

Mass number

The sum of protons and neutrons in an atom.

Atomic number

The number of protons in an atom.

Isotopes

Atoms with the same number of protons but different numbers of neutrons.

Neutral atom

An atom with the same number of protons and electrons, resulting in an overall charge of zero.

Electron configuration

Shows location of electron in their shells.

Valence electrons

Electrons found in the outermost shell.

Excited electron

When electron moves from higher energy levels to lower energy levels and emits energy.

Transmutations

All Nuclear reactions are _.

Fusion

Light nuclei combine to form a heavy nucleus and a lot of energy.

Half-life

The length of time it takes for half the mass of a sample to decay.

Elements

Cannot be broken down by chemical means.

Compounds

Can be broken down by chemical means.

Diatomics

Two of the same atom bonded together.

Homogeneous mixtures

Even distribution of particles.

Heterogeneous mixtures

Not even throughout.

Chemical property

How substances react.

Chemical change

Results in the formation of a different substance.

Physical change

Do not form new compounds, commonly phase changes.

Deposition

Gas to solid phase change.

Sublimation

Solid to Gas phase change.

Thermal energy

Random motion of atoms and molecules.

Exothermic

Energy exits (is released).

Endothermic

Energy absorbed.

STP

Standard Temperature and Pressure.

Metals

Left of the staircase, are good conductors of heat, malleable.

Nonmetals

To the right of the staircase.

Metalloids

On the staircase.

Noble gases

Group 18 are stable because of their stable electron configuration, they are not reactive.

Electronegativity

Attraction for electrons in a chemical bond.

Synthesis

Two or more reactants combine to form one product.

Decomposition

One compound is broken down into two.

Single replacement

One element switches partners.

BARF

Bond BROKEN energy ABSORBED (endothermic), energy RELEASED bond FORMED (exothermic).

Ionic compound

metal and nonmetals or table E ions.

Covalent bond

Nonmetals.

SNAP

Molecule Polarity- symmetrical nonpolar, asymmetrical polar.

% Composition by mass

mass of part / mass of whole.

Empirical formula

Simplified formula.

Table G

Use when given a temperature and asking about a salt dissolved in water.

Table F

Insoluble compounds will not fully dissolve in water and will be in solid phase, soluble compounds will dissolve in water and be in aq phase.

PPM

(grams of solute / grams of solution) x 1,000,000.

Reaction rate

Increase temperature, increases reaction rate.

Activation energy

goes from the reactants to top of curve.

Entropy

gases have the highest, then liquid/aq and solids have the lowest.

Forward and reverse reaction are equal

At equilibrium the concentration of reactants and products remain constant because __.

Arrhenius theory

acids yield H+ ion and bases have an OH-.

BAAD

BASES ACCEPT H+ ACIDS DONATE H+.

Neutralization

Acid + base --> salt + water.

Titration

determines the concentration of unknown acids or bases.

Oxidation number

Single atom = 0, look on reference table or use algebra for atoms with multiple charges.

Redox

electrons are lost (electrons on right), Reduction: electrons are gained (electron on left).

Voltaic cell

chemical energy is converted to electrical energy spontaneously.

Electrolytic cell

electrical energy to chemical energy.

Organic compounds

must contain at least one carbon and one hydrogen.

Saturated hydrocarbons

have all single bonds.

Unsaturated compounds

compounds have double or triple bonds between carbons.

Isomers

have same number of C’s and H’s but are in a different structural arrangement.

Fermentation

sugar + enzyme --> ethanol (alcohol) + carbon dioxide.