Chemistry Final PHS

Matter

Anything that has mass and takes up space

Phases of Matter

Chemical Properties (properties of matter as it exist)

Chemical vs. Physical (chem-molecules change, phys-molecules dont change)

Chemical Properties (properties that we see as the molecules change)

Substance

Something with the same thing throughout

Element

Cannot be broken down, smallest atom

Compound

Combinations of one or more elements (no longer has characteristics of original element)

Mixture

Combinations of one or more substances

Solution

Are Homogenous mixtures

Metals (elements)

Copper, Silver, gold malleable, best with electricity conduction

Non metals(elements)

Exist in all three forms; solid, gas, liquid. Not malleable, heat poorly, no electricity.

Temperature- 3 Scales

1) Celcius

2) Fahrenheit

3) Kelvin

Atoms, Molecules, and Ions

All these combined give matter

Atom

Smallest unit of an element (extremely small)

Molecule

Smallest substance of an element (ex..H2O)

Metalloids

Some properties of both metals & non metals

Ion

Atoms or group of atoms that has acquired either a (+) or (-) charge

Isotopes

Atom from the same element with different number of neutrons

Cations

Positive charged ion (lose e-)

Anions

Negative charged ion (gain e-)

Acids

starts with H+

electronegativity

increases up and right

ionization energy

Energy required to split the electron from ion or atom

Anion single replacement

one anion replace anion

Cation single replacement

cation replace cation

double replacement

pos and neg ions of 2 ionic compound change places

combustion

oxygen combine with compound, release heat

synthesis

2 or more element or ompou nd combine, form more complex substance

decomposition

complex molecule break down, opposite of synthesis

limiting reactant

Number that limits the products or outcomes

excess reactant

leftovers aft er an reaction

theoretical yield

Largest amound of product made in chem reaction

percent yield

Percent ratio of the theoredical yield

heat

form of energy, high temp to lower

temperature

measure average kinetic energy

specific heat capacity

Amount of energy to change object’s temp

Kinetic energy

energy by motion

potential energy

energy by position

Boiling point

liquid to gas

condensation

gas to liquid

melting point

solid to liquid

freezing point

liquid to solid

entropy

Randomness

thermal equilibrium

2 substance reach equal temp

enthalpy

energy exchanged through chemical reaction

latent heat

phase change where the temp stays the same

heat of fusion

latent heat during melting point

heat of vaporization

latent heat during boiling point

endothermic

absorbs surrounding energy

Products are higher than reactants on the graph

cold

Exothermic

Release energy to the surroundings

Products are lower than reactants on the graph

hot

Homogenous mixture

Mixed well

Heterogeneous mixture

Doesn’t mix well

Covalent Bond

Share electron pair between 2 atoms

Ionic bond

Pos metal with neg non metal

Solute

Solid of solution

Solvent

liquid of solution

Solution

Solute plus Solvent

Polar

likes water

nonpolar

doesn’t like water

Molarity

Moles of solute / Liter solution

Concentration

How much substance is mixed with the solvent

Parts Per Million

Very small concentration

Concentrated solution

More solute than solvent

Diluted solution

More solvent than solute

Arrhenius acids

relesea H+

Arrhenius bases

Release OH-

Conjugate acid

Formed when base gets H+

Conjugate base

Formed when base loses H+

pH

Measure of acidity

Oxyacid

Acid with polyatomic anion, has oxygen

Binary Acid

No oxygen, 2 elements

Equilibrium shift

increase or decrease in molarity due to changes

Titration

Methods to find molarity, of the unkown acid or base

Titrant

Acid or base with known concentration

Analyte

Acid or base with unknown concentration

Equivalent point

Mol of H+ is equal to mol of OH-

Neutrialized

Le Chatelier’s principle

Equilibrium will adjust to shifts