Chem Week 1-2 Flashcards
Mass
Kilogram (Kg)
Length
Meter (m)
Temperature
Kelvin (K)
Time
Second (s)
Electric current
Ampere (A)
Quantity of substance
mole (mol)
Speed
Distance/time (m/s)
Volume
Space (distance^3) m^3
Also L
1cm^3 = 1 mL
Density
Mass/volume = kg/m^3 or kg/mL
Energy
Joule (kgm^2/s^2)
Power
Watt (Joule/s)
deka
da, 1
Tera
T, 12
Giga
G, 9
Mega
M, 6
Kilo
k, 3
Hecto
h, 2
deci
d, -1
centi
c, -2
milli
m, -3
micro
mu, -6
nano
n, -9
pico
p, -12
femto
f, -15
temperature
measure of average kinetic energy of particles in a sample
compare Celsius and kelvin
Celsius: based on properties of water, boiling point 100, freezing point 0
Kelvin: based on proprieties of gas, no negative Kelvin temperature, C + 273.15
Accuracy
Proximity of measurement to true value of quantity
Precision
Proximity of several measurements to each other (small difference between measurements)
Uncertainty
Smallest measurable difference, determines limit of precision
What are sig figs?
Measured digits, number denote uncertainty
Element
Substances can’t be separated into simpler substances
Compounds
Groups of DIFFERENT elements
Atoms
Smallest unit of matter, building blocks of chemistry
Mixture
Composed of 2+ pure substances
Pure substance
Simplest forms of matter that can’t be separated into other kinds by physical means
Molecules
Two or more atoms connected by chemical bonds
Intensive properties
Properties that characterize pure substance (independent of amount)
Extensive properties
Dependent on amount of substance
Physical processes
Change that doesn’t alter chemical identities
Chemical reactions
Change into compounds with different chemical identities
Molecules
Groups of atoms
Chemical bonds
Forces!!!
Immiscible
Don’t dissolve into each other
Distillation
Separate via evaporation and condensation (works with different volatility)
Filtration
Filter!!
Chromatography
Separate substances in mixture
States of matter
Liquid solid gas
Sublimation
Solid to gas
Deposition
Gas to solid
Condensation
Gas to liquid
Vaporization
Liquid to gas
When does energy increase
Water melts/vaporizes
Where does energy go when water molecules freeze?
Released
What happens to energy of molecules of water as it melts or vaporizes?
Add energy
Energy
Ability to do work (exert force through a distance)
Work
W=fd
Potential energy
Stored energy (composition or position)
Kinetic energy
Energy of motion
KE=1/2mV^2
Heat
Amount of energy transferred bc of diff in temp
Heat moves ____ to ______
Hot to cold
Law of conservation of energy
Energy cannot be created nor destroyed (transformed!)
Diatomic molecules?
H, N, O, Fluorine (F) , Chlorine (Cl), Bromine (Br), Iodine (I)
Have No Fear of Ice Cold Beer :))