Law of Conservation of Mass
In a chemical reaction, matter is neither created nor destroyed"Antoina Lavoisier; observations on combustion.
Homogenous vs. Heterogenous
Homogenous: a mixture that has the same composition throughout; must be separated by distillation (boiling the mixture so that the more volatile liquid vaporizes and is then recondensed into a separate flask. (koolaid)Heterogeneous: composition varies from one region to another; separate by filtration. (wet sand)
Extensive vs. Intensive
Extensive: the value depends on the quantity of matter; extensive properties cannot be used to identify what type of matter something isIntensive: value independent of the quantity of matter (density)
Volume equivalencies of a solid
1 m3 = 106 cm3 1 cm3 = 10-6 m3 = 0.000001 m3
Commonly measured liquid or gas volume
1 L is slightly larger than 1 quart1 L = 1 dm3 = 1000 mL = 103 mL 1 mL = 0.001 L = 10-3 L1 mL = 1 cm3
Common units and their equivalents: Length
1 kilometer (km) = 0.6214 mile (mi)1 meter (m) = 39.37 inches (in.)1 meter (m) = 1.094 yards (yd)1 foot (ft) = 30.48 centimeters (cm)1 inch (in.) = 2.54 centimeters (cm) exactly
Mass: common equivalents
1 kilogram (km) = 2.205 pounds (lb)1 pound (lb) = 453.59 grams (g)1 ounce (oz) = 28.35 grams (g)
Volume: Common Equivalents
1 liter (L) = 1000 milliliters (mL)1 liter (L) = 1000 cubic centimeters (cm3)1 liter (L) = 1.057 quarts (qt)1 U.S. gallon (gal) = 3.785 liters (L)
What did Leucippus and Democritus suggest?
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What did Plato and Aristotle suggest?
#NAME?
Law of Definite Proportions
Joseph Proust; All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements.
Law of Multiple Proportions
John Dalton-When two elements, (call them A and B), form two different compounds, the masses of B that combine with 1 g of A can be expressed as a ratio of small, whole numbers
Dalton's atomic theory
Dalton proposed a theory of matter based on it having indivisible particles (atoms) to explain these laws1.) Each element is composed of tiny, indestructible particles called atoms2.) All atoms of a given element has the same mass and other properties that distinguish them from atoms of other elements3.) Atoms combine in simple, whole-number ratios to form molecules of compounds4.) In a chemical reaction, atoms of one element cannot change into atoms of another element -they simply rearrange the way they are attached
Periodic Law
Mendeleev-When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically
Conversions between *F, *C, and K
*C=(*F-32)/1.8K=*C + 273.15
Density-water-mercury-ethanol-lead
Water = 1.00Mercury = 13.55Ethanol = 0.789Lead = 11.4
Ionic Bonds
Occur between metals and non-metals; involve the transfer of one atom to another
Rules for naming ionic compounds
If cation is:-metal with invariant charge = metal name-metal with variable charge = metal name(charge)-polyatomic ion = name of polyatomic ionIf anion is:-nonmetal = stem of nonmetal name + ide-polyatomic ion = name of polyatomic ion
Acetate
C2H3O2-
Carbonate
CO32-
Hydrogen carbonate (bicarbonate)
HCO3-
Hydroxide
OH-
Nitrite
NO2-
Nitrate
NO3-
Chromate
CrO42-
Dichromate
Cr2O72-
Phosphate
PO43-
Hydrogen Phosphate
HPO42-
Dihydrogen Phosphate
H2PO4-
Ammonium
NH4+
Hypochlorite
ClO-
Chlorite
ClO2-
Chlorate
ClO3-