college chemistry test 1

accuracy

how close a measurement is to the true amount

precision

agreement among several measurements of the same quantity, reproducible

10.1g, 10.1g, 10.2g, actual amount is 15g. Is the measurement accurate or precise.

Precise but not accurate

E

tetra, 10^12

G

giga, 10^9

M

mega, 10^6

k

kilo, 10³

h

hecta, 10²

da

decka, 10

d

deci, 10^-1

c

centi, 10-²

m

milli, 10^-3

u

micro, 10^-6

n

nano, 10^-9

p

pico, 10^12

dementional analysis

conversion factor, cancels out labels

how to find density

D=m/v

how to find volume

V=m/D

how to find mass

m=DxV

percent error formula

emperimental value / actual value x100

pure substance vs mixture

a mixture can be separated into pure substances where a pure substance cannot be broken down as easily.

what are pure substances

elements and compound

heterogenous

different parts can be easily seen

homogenous

parts of the mixture cannot be seen

Lavoisier

Law of conservation of mass

Proust

law of definite proportions

law of definite proportions states

compounds will always have the exact same proportions of elements by mass

dalton

law of multiple proportions

law of definite proportions states

elements will combine in whole number ratios

Daltons 4 postulates

1. all things are made up of tiny particles called atoms

2. atoms of elements are the same (incorrect because of ions)

3. chemical compounds involve the reorganization of atoms

4. chemical compounds form when different elements combine

Democratis

Atomost (atom)

Thomson

cathode ray tube

what did the cathode ray tube discover

the negative charge of the electron

Milikan

oil drop experiment

what did the oil drop experiment find

exact mass of an electron

what is the exact mass of an electron

9.11×10^-31

rutherford

gold foil experiment

what did the gold foil experiment find

dense center of the atom, nucleus

atomic radius

size of an atom

ionization energy

amount of energy required to remove and electron

electronegativity/affinity

force between atoms in a chemical bond

non metallic

gains electrons/nonmetals

metallic

loses electrons/metals

columbic attraction

force between 2 oppositely charged particles

ionic bonds

nonmetal and metal

cation and anion

ionic bonding

covalent bonding

nonmetal and nonmetal

7 diatomics

H, N, O, Cl, Br, F, I

acids with polyatomics ending in ite

ous

acids with polyatomics ending in ate

ic

how to find electrons

protons, +charge if negative, -charge is positive per

percent yield

actual/theoretic yeild

waters shape

bent, 104.5 degree angle

waters polarity

water is polar because of the unequal sharing of electrons

unique properties of water

the solids that get dissolved are salts, ionics break apart into oppositely charged particles, cation is attracted to the the oxygen, anionn is attracted to the hydrogens

definition of solute

the substance that gets dissolved

definition of solvent

the solution doing the dissolving

definition of solution

a homogenous mixture of two or more substances that were dissolved in the solvent, has two parts, solvent and solute