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Acetic Acid
HC2H3O2/C2H3OOH
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Oxidation of Copper
1+,2+
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Oxidation States of Iron
2+,3+
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Oxidation States of Mercury
1+,2+
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Oxidation states of Antimony
3+,5+
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Oxidation states of Chromium
2+,3+
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Oxidation states of Tin
2+, 4+
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Chemistry
The study of matter, its composition, and the changes it undergoes
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Major Divisons of Chemistry
- 1.Biochemistry- study of biological chemicals
- 2.Organic- carbon based compounds
- 3.Inorganic- all other elements
- 4.Physical- theory and concepts
- 5.analytical- methods of analysis
- 6.nuclear- radioactive materials
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Scientific Method
- 1.Apply logical, organized reason to any observation made
- 2.Form Hypothesis
- 3.Reject or confirm (trial&error) hypothesis through experiment
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Matter
anything that has mass and takes up space
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Mass
measure of the amount of matter that object contains
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Weight
the effect of gravity on matter
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Physical Properties
can be seen without changing the composition of material
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Intense
size doesn't matter
ex.color, ordor, density, melting point, boiling point, taste, feel, compressibility, magnetism, duetility, solubility, conductivity
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extensive
size does matter
ex.mass, length, etc.
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Chemical Properites
change in composition
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Physical changes in matter
composition isnt altered
- changes in state
- dissolving
- pulverizing
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chemical changes in matter
composition is altered
- rusting
- combustion
- fermentation
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Factors that aid chemical reactions
- 1.heat energy
- 2.light energy
- 3.electric energy
- 4.water
- 5.catalyst
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exothermic
energy is released (heat or light)
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endothermic
energy is absorbed (temp. drops)
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atoms
smallest unit of an element that has all the properties of the element
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molecule
smallest unit of a pure substance that has all the properties of that substance
may have one atom or more
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diatomic
molecule that contains two atoms
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homoatomic
two or more atoms of one element
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heteroatomic
contains at least 2 atoms of two or more elements
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mixture
a combination of two or more pure substances
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homogenous
uniform composition
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heterogenous
non-uniform composition
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element
cannot be converted to simplier form by a chemical reaction
ex.hydrogen, oxygen
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compound
two or more elements in a definite, reproducible way
ex.water
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data
measurements and observations that you make
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results
data obtained from experiments
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units
defines the quantities being measured
must have units
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1 liter=_______quarts
1.057
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1 meter=_______yards
1.094
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accuracy
how close to the true value
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procision
how close to each other
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Significant Figures
- leading zeros are not significant
- captive zeros are significant
- trailing zeros are significant
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Formula to find Fahrenheit
9/5C+32
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Formula to find Celsius
5/9(F-32)
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Formula for finding Kelvins
C+273.15
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Denisty formula
D=mass/volume
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Speific Gravity formula
SG=density of substance/ density of reference
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Solid or liquid reference is equal to?
1.00g/cm3
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gas reference is equal to?
1.29g/l
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Percentage Error Formula
(theoretical-experimental)/theoretical
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Symbols
used to represent each element
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formulas
used to represent compounds
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compound formula
consists of the symbol of the elements found on the compound
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nucleus
the protons and neutrons are tightly bound together to form the central portion of an atom
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Protons
- located in the nucleus
- charge of 1+
- mass of 1u
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Neutrons
- located in the nucleus
- no charge
- mass of 1u
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Electrons
- located outside the nucleus
- charge of 1-
- mass of 1/1836u
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Atomic Number of an atom
equal to the number of protons in the nucleus of the atom
represented by the symbol of Z
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Mass number of an atom
equal to the sum of the number of protons and neutrons in the nucleus of the atom
represented by the symbol A
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Isotopes
atoms that contain the same number of protons but a different numbe of neutrons
- they have the same atomic # but different mass #
- same #of electrons outside that nucleus
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relative masses
extremely small size of atoms and molecules make it inconvenient to use their actual masses
comparisons of actual masses
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atomic weight
the relative mass of an average atom of the element expressed in atomic mass unit
the number given at the bottom ofthe box containing the symbol of each element
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molecular weight
relative mass of a molecule in the atomic mass unit
obtained by adding together the atomic weigth of all the atoms in the molecule
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Formula for finding atomic weight of isotopes
(isotope percentage)(isotope mass)/ 100
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Mole is equal to______
the number of atoms in one mole is equal to Avogardro's Number
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Avogardro's Number
6.022x1023
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Percentage Composition
- Know the formula
- 2.Know the formula weight
- 3.divide the number of atoms by the formula weight
- ex.H3PO4=98.00
- H=3.03/98.00=3.09%
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