snc2d vocab

Standard Reduction Potential

Measure of how easily a substance gains electrons (is reduced).

Single displacement

A reaction where a more reactive element replaces a less reactive element in a compound.

Double displacement

A reaction where two ionic compounds exchange ions to form two new compounds.

Reactants

The starting substances in a chemical reaction.

Products

The substances formed in a chemical reaction.

Skeleton Equation

An unbalanced chemical equation showing only the reactants and products.

Balanced Equation

A chemical equation with the same number of each type of atom on both sides using coefficients.

Synthesis Reaction

A reaction where two or more reactants combine to form one product.

Decomposition Reaction

A reaction where one compound breaks into two or more simpler substances.

Ionization Energy

The energy required to remove an electron from an atom.

Activity Series

A ranking of metals by reactivity used to predict single displacement reactions.

Saturation threshold

The point where a system reaches its limit before a major change occurs (assignment term).

Precipitate

An insoluble solid formed during a chemical reaction in solution.

Complete Combustion

A reaction where a fuel burns with sufficient oxygen to produce carbon dioxide and water.

Incomplete Combustion

A reaction where a fuel burns with limited oxygen to produce carbon monoxide and/or carbon (soot) along with water.

Limiting Reactant

The reactant that is completely used up first and stops the reaction.

Catalyst

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

Exothermic

A reaction that releases energy to the surroundings.

Endothermic

A reaction that absorbs energy from the surroundings.

Fluoride (Anion)

F⁻

Chloride (Anion)

Cl⁻

Bromide (Anion)

Br⁻

Iodide (Anion)

I⁻

Hydroxide (Anion)

OH⁻

Nitrate (Anion)

NO₃⁻

Nitrite (Anion)

NO₂⁻

Hydrogen carbonate (Bicarbonate) (Anion)

HCO₃⁻

Acetate (Anion)

CH₃COO⁻

Oxide (Anion)

O²⁻

Sulfide (Anion)

S²⁻

Carbonate (Anion)

CO₃²⁻

Sulfate (Anion)

SO₄²⁻

Sulfite (Anion)

SO₃²⁻

Chromate (Anion)

CrO₄²⁻

Dichromate (Anion)

Cr₂O₇²⁻

Phosphate (Anion)

PO₄³⁻

Hydrogen (Cation)

H⁺

Lithium (Cation)

Li⁺

Sodium (Cation)

Na⁺

Potassium (Cation)

K⁺

Silver (Cation)

Ag⁺

Ammonium (Cation)

NH₄⁺

Magnesium (Cation)

Mg²⁺

Calcium (Cation)

Ca²⁺

Zinc (Cation)

Zn²⁺

Copper(II) (Cation)

Cu²⁺

Iron(II) (Cation)

Fe²⁺

Iron(III) (Cation)

Fe³⁺

Aluminum (Cation)

Al³⁺

Lead(II) (Cation)

Pb²⁺

Observe

To carefully notice and record what happens during an experiment.

Simultaneously

Happening at the same time.

Depleted

Completely used up.

Consumption

The use or use up of a substance during a reaction.

Aqueous (aq)

Dissolved in water.

Soluble

Able to dissolve in water.

Insoluble

Unable to dissolve in water.

Dissolve

To mix completely into a solvent and form a solution.

Oxidation

The loss of electrons.

Reduction

The gain of electrons.

Oxidizing agent

A substance that causes another substance to lose electrons and is itself reduced.

Reducing agent

A substance that causes another substance to gain electrons and is itself oxidized.

Electron transfer

The movement of electrons from one atom or ion to another.

Valence electrons

The electrons in the outermost shell of an atom that participate in bonding.

Bond formation

The process of atoms joining together by forming chemical bonds.

Bond breaking

The process of chemical bonds being broken during a reaction.

Activation energy

The minimum energy required for a reaction to begin.

Collision theory

The theory that reactions occur when particles collide with enough energy and the correct orientation.

Concentration

The amount of solute dissolved in a given volume of solution.

Moles

The SI unit used to measure the amount of substance (6.022 × 10²³ particles).

Coefficient

A number placed before a chemical formula showing how many molecules or formula units are present.

Subscript

A small number in a chemical formula showing the number of atoms of an element in one molecule or formula unit.

State symbol

A symbol indicating the physical state of a substance such as (s)

Conservation of mass

Mass is neither created nor destroyed during a chemical reaction.

Law of Conservation of Mass

The total mass of reactants equals the total mass of products in a chemical reaction.

Rearranged

Atoms are reorganized into new substances during a chemical reaction.

Neutral compound

A compound with no overall electric charge.

Ionic compound

A compound made of positive and negative ions held together by ionic bonds.

Covalent compound

A compound formed when atoms share electrons.

Polyatomic ion

A charged group of two or more covalently bonded atoms that acts as a single ion.

Rust

occuring in the presence of oxygen and water and is made worse by electrolytes such as salt.

Corrosion

The breakdown of a metal as it reacts with chemicals in the environment.

tissue

a collection of similar cells that perform a particular, but limited, function

organ

a structure composed of different tissues working together to perform a complex body function

organ system

a system of one or more organs and structures that work together to perform a major vital body function such as digestion or reproduction

Cell Theory

a theory that all living things are made up of one or more cells, that cells are the basic unit of life, and that all cells come from pre-existing cells