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1.Properies Stotes of Motep
Sublimation
[Iefirnika shape and e derite No definite shape
Boiling/ Evaporation
wolume (^) and volume Melting
Molecues are lecie are iess Far apart
closey psckad casey packed
Solid (^) Liquid Gas rce i (^) tiractiC (^) tihan is sxrong ery^ less iti n.2. state
it is difficult to ompressed more Freezing Condensation Casily than solids
Easy to compress Compress
O'c 32° Deposition
212'F Matter 100C Water boils Water boils
Pure substance
98.6'F Normal body temperature Mixture 37"C Normal body temperature
.32°F Element Compound Homogeneous Heterogeneous
0°C Water^ freezes^ mxture^ mixture Water freezes
Celsius Therrmometer (^) Fahrenheit Thermometer
HOMOGENEOUS MIXTURES VERSUS PURE^ SUBSTANCE HETEROGENEOUS MIXTURESs VERSUS MIXTURE onogenous inixiures hava unifom
composilion
throughout he nmixt
tarogous miures
Pure substances are (^) Mixtures are made up
onpison yhuehay made of only one of several substauces
matter: hus the (^) that are not eomposition is the same throughout
chemically bonded
Komponenis arg
Chemical and (^) Chemical and
physical properties physical properties
ire constant (^) may varTY
Can be categorised as gas, liquid and
Categorised as homogencous and heterogeeneous
elerEenus
hwtures Have large
Pallicle sizes
sofid
Examples include sand and sugar, oil
Examples include Compments cannot be separated easily
ompoinents can be separated easily
pure water. llydroge gis. gold and water Viit www.pedina.com Visit ww.pedn
Chemical and Physical (^) Changes
Elements V. Compounds Chemical^ change:^ A^ Physical^ change:^ Matter
chemical reaction forms changes form but not
gOMPOUNDS (^) new products. (^) chemical identity.
wo or more elements nne be breeaA thatcombine chemically ple substancos MKAL
EMample Carban, wOVEeh Ntrogen, cold
anythtng on the penadlc
table
Examples: Water (H20), Carbon Dioxide (C02), DNA, Proteins, eto |Combustion Rotting Melting Shredding
Elements are madeup of atoms
'
Rusting Digestlon Blling Chopping
2. MATH AND QUANTITATIVE RELATIONSHIPS:
Significant Figures Rules Sig Figs and Calculations
Significant Figures can be done using a set of around S rules,
With a lot of complications for how to deal with zeroes. Not significant: Not significant: Signilicant Multiplication^ and^ Addition^ and all zeros between Division: round the nonzero numbers answer to the saime
zero for (^) zeros used only Subtraction:^ round^ the "cosmetic"* to locatc the (^) answer to the same purpose (^) decimal point number of significant number of decimal
figures as the least places as the value^ with
certain measurement the fewest
Significant Signilicant: all nonzero
a number to the right 2.^
x (^) 14.25 41.
zeros at the end of (^) 7.050+6.2 13. intcgers (^3) siyh
Volume
1 mL=1 cm*
of decimal point^3 Mass
1 lb 453.59 g
Length Time
1 mile 1.609 km 60 s^1 min
1 in 2.54 cm 1 ft 12 in 3 ft 1 yd
1L=1.06qts
1 gallon=3.78 L 1 fl oz = 29.57 mL
+1 lb = 16 oz 60 min 1hr
1 lb 7.00x10 grains^24 hr^1 day
1 grain = 64.8 mg
1 kg = 2.20 lbs
1 ton 2000 lbs 1 km 0.621 (^) miles *1Ka= \KD
365 days =1 year
10 yr^1 decade 1 fluidram = 3.72 mL 100 yr 1 century
1m 39.4in 2 pts^ 1qt
5280 ft = 1 mile
Energy 4.184J1 cal A1 kcal = 1000 cal = 1 food cal (Cal)
Sample Metric Relationships for length
where meter (m) is the base unit:
1 Mm 1,000,000 m 1 km 1000 m
Temperature
10 dm = 1m
T Tc + 273
Tr=(T32)
Tp = ()Tc 4+
100 cm =1m
1,000 mm =1 m
1,000,000 um = 1 m
1,000,000 nm = 1 m
Pressure
1 atm 760 mmHg 760 torr
Paricts
UMbPr
ol (^) o.02 X^1023
