Chemistry Unit 1: Unit Conversions and Density + Measurements and Glassware + Matter and Mixtures

mass

g, mg, lbs, kg

volume

L, mL, oz, gal, cm3, ft3

temperature

ºF, ºC, K

time

sec, min, hrs, yrs, ms

nano

1×10^-9

micro

1×10^-6

milli

1×10^-3

centi

1×10^-2

deci

1×10^-1

deka

1×10¹

hecto

1×10²

kilo

1×10³

what number goes in front of the prefix

prefix gets the 1

density

matter per unit of space; mass/volume

beaker

poor measurements, good for mixing

erlenmeyer flask

poor measurements, good for mixing

watch glass + petri dish

large surface area, evaporating liquids

test tubes

small samples

graduated cylinder

good for measuring, bottom to top measurements

buret

good for measuring, top to bottom measurements

volumetric flask

measures 1 volume very accurately

volumetric pipet

measures 1 volume very accurately

significant figures conditions

leading zeros are never significant

trapped zeros are always significant

trailing zeros are only significant if a decimal is present

accuracy

how close you are to the true answer

precision

how close your measurements are to each other

random error

indeterminate error from estimating last digit; a problem during one trial

systematic error

determinate error occurs in the same direction fro each measurement; same problem for every trial

solids

fixed shape + volume

liquids

fixed volume

gases

takes shape + volume of container

element

simplest form of matter

compound

chemically bonded elements

homogeneous mixture

uniform parts (if you cut a piece out, the composition will be the same)

heterogeneous mixture

nonuniform parts (if you cut a little piece out, the composition will be varied)

chemical change

chemical composition changes

physical change

state/phase changes

distillation

separates based on boiling points

filtration

used to separate solids from liquids

chromatography

a mobile phase carries a mixture through a stationary phase