General Chemistry I
classifications of matter
• heterogeneous mixtures
• homogeneous mixtures (solutions)
• pure compounds
• pure elements
properties of matter
• physical
o extensive (mass, volume, …)
o intensive (density, color, …)
• chemical
o flammability, toxicity, …
metrix prefixes give powers of 10
mega (M) 106 kilo (K) 103
giga (G) 109
deci (d) 10-1
centi (c) 10-2
milli (m) 10-3
micro (µ) 10-6 nano (n) 10-9 pico (p) 10-12
units of measurement
• length (meter)
• volume (liter = cubic decimeter)
• time (seconds)
• mass (kilogram)
• temperature (oC, oF, K)
unit conversions
• 2.54 cm = 1 inch (exactly)
• 1mL = 1 cubic centimeter
K = oC + 273
• oC = 5/9 (oF -32)
• oF = 9/5 oC +32
Density =
mass
Volume
quality of data
• precision (nearness of results to one another)
• accuracy (nearness of a result to the truth)
errors in measurements
• random (reading a buret)
• systematic (balance is broken)
Review Sheet for Exam I
recording significant figures
• non-zero digits are significant
• interior zeros are significant
• zeros to the left not significant
• zeros to the right (need a decimal point
if significant)
following significant figures in a calculation
×,÷ same # as least significant data
-, +
same decimal place as the least
significant data
Periodic Table
• groups are columns
• periods are rows
element groups
• metals / non-metals
• alkali metals
• alkaline earth metals
• transition metals
• halogens
• noble gases
structure of atoms
• nucleus
o protons (+) (p)
o neutrons (0) (n)
o extremely dense
o all of the mass
• outer cloud
o electrons (-) (e)
o mass negligible
o determine charge
atomic number = # p
this gives identity of atom
atomic mass number = #p + #n
determines isotope
overall charge = #p - #e
19 −
F
atomic symbol (example 9
)
mass number
charge
atomic number SYMBOL
or
name-mass number ( fluorine-19)
atomic mass (amu)
based on carbon-12 = 12 amu
weighted average %abund for each element
The Mole
• 6.022 x 1023 items
• 12 grams of carbon-12 = mole of 12C
atoms
• periodic table gives molar masses of the
atoms in grams
Conversions:
• grams to moles (divide by molar mass)
• moles to grams (X by molar mass)
• moles to atoms (X by 6.022 x 1023)
Naming Ionic Compounds
• charge of ions is significant
• cation charge included in the name as a
roman numeral - if not obvious
• know polyatomic ions
Naming Covalent Compounds
• non-metal elements
• charge is not significant
• prefix used in name:
1=mono
2=di
3=tri
4=tetra
5=penta
6=hexa
7=hepta
8=octa
9=nona
10=deca
Polyatomic Ions:
acetate
carbonate
hydroxide
nitrite
nitrate
chromate
dichromate
phosphate
ammonium
hypochlorite
chlorite
chlorate
perchlorate
permanganate
sulfite
sulfate
cyanide
peroxide
CH3COOCO32OHNO2NO3CrO42Cr2O72PO43NH4+
ClOClO2ClO3ClO4MnO4SO32SO42CNO22-
(also the hydrogen additions to the above list)
Acids are formed by adding hydrogen to the
anions until a neutral charge exist. Examples:
sulfate  sulfuric acid H2SO4
nitrite  nitrous acid HNO2
Hydrated compounds are named by using a dot
and following the name with the number of
water molecules attached. Example:
copper (II) sulfate pentahydrate
CuSO4 • 5 H 2O