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Hypothesis
a testable statement explaining your data and observations; may be little more than a hunch or guess based upon limited data.
Theory
a tested hypothesis that explains a body of facts; stood the test of time and is supported by a large amount of data.
Law
Observations generally accepted to be true and universal often taking the form of a mathematical equation.
Directly Proportional
two variables if increasing one value causes the other one to increase, or decreasing one value causes the other one to decrease
Indirectly Proportional
two variables if increasing one value causes the other to decrease, or decreasing one value causes the other to increase
Antoine Lavoisier
creator of the Law of Conservation of Mass
Joseph Proust
created the Law of Definite Composition
Atom
the smallest unit of matter; combine to form molecules
Molecule
consist of the same type of atoms or different types of atoms
Compounds
substances containing at least two different elements chemically combined in definite proportions
Mixtures
consist of more than one atom, element, or compound physically bound together
Solid
the state of any matter that has a definite shape and a definite volume
Liquid
the state of any matter that has a definite volume but an indefinite shape
Gas
the state of matter that has neither a definite shape nor a definite volume
Physical Properties
properties that can be observed or measured without altering the identity of the material
Chemical Properties
the ability of a substance to undergo a change that alters its identity
Extensive Physical Properties
depend on the amount of matter present and include mass, length, and volume
Intensive Physical Properties
do NOT depend on the amount of matter present and include melting point, boiling point, density, ductility, malleability, color, crystalline shape, refractive index, etc
Mole
an SI base unit and the measure of the amount of a substance (how many) not how much (mass)
Avogadro’s Number
the larger number a mole refers to; 6.02 × 10^23
Homogenous Mixture
mixture that is uniform throughout
Heterogeneous Mixture
mixture that is not uniform throughout
Solutions
-do not separate on standing
-cannot be separated by filtration
-do not scatter light
-ex: salt water, sugar water, brass, alloys, air, soda, etc
Colloids
-do not separate on standing
-cannot be separated by filtration
-scatter light, exhibit the Tyndall effect
-ex: butter, milk, cream, fog, smog, smoke, asphalt, inks, paints, glues
Suspensions
-settle out on standing
-can be separated by filtration
-may scatter light (usually do not) but are not transparent
-ex: mud, flour in water, sand in water, blood, and most aerosol sprays
Metals
-lustrous &good conductors
-relative high density
-high melting point
-ductile & malleable
-solid at room temp
-high tensile strength
-good reflectors
-crystalline structure
-easily lose electrons & form cations
-corrode easily
Nonmetals
-non lustrous and poor conductors
-brittle
-low density and melting point
-most are solid at room temp, some are gasses & Bromine is a liquid
-tend to gain electrons forming anions
Metalloids
-solid at room temp
-can be shiny or dull
-may be ductile or malleable
-semi conductors
-can act as a metal or nonmetal depending upon what they are reacting with in the chemical reaction
Kinetic Energy
the energy of an object in motion
Potential Energy
the energy of an object due to its position or composition
Law of Conservation of Energy
energy can neither be created nor destroyed in ordinary chemical or physical changes, but can be converted from one form to another
Reactants
substances that exist before the chemical change begins
Products
new substance or substances produced as a result of a chemical reaction
Exothermic
chemical reaction (or physical change) that releases heat
Endothermic
chemical reactions (or physical change) that absorb energy
Activation Energy
initial input of energy required to get a reaction going
Fahrenheit to Celcius
(F - 32)/1.8
Celcius to Kelvin
C + 273
Specific Heat
the amount of heat required to raise the temperature of 1g of a substance 1 degree C; it is an intensive physical property and varies for each substance
Joule
the SI unit of heat energy and all other forms of energy
calorie
non SI unit of energy defined as the amount of heat required to raise the temperature of 1 g of water one degree centigrade
Calorie (food)
= 1,000 cal