overall? idfk

Element

cannot be made simpler, building block of matter. Includes diatomics, atoms, and even polyatomic

Compound

Pure substances that can be broken down by chemical means ie. NaCl

Atoms

Neutral particles

molecules

Smallest physical unit, always neutral eg. a molecule of H2O

elements of a chemical formula

subscripts (number of atoms), superscript (charge), coefficient (# compounds), balanced

accurate

results close to the actual number

precise

results close to each other

Physical properties

appearance, smell, feel, melting point, density, etc

chemical properties

how things react ex. Mg burns in air

wtf is a barometer or a manometer

google it bitch

Methods of separation

decanting, filtration, distillation, evaporation

diatomics

H O N F I Cl Br

Ammonium

NH4 +

Hydroxide

OH -

Nitrate

NO3 -

Sulfate

SO4 2-

Carbonate

CO3 2-

Phosphate

PO4 3-

Diatomic tool

NICK the BABY CAMEL ate and INCH CLAM and CREPES for SUPPER in PHOENIX

Practice naming

don’t procrastinate

What is the number of protons

constant, atomic #

How to find neutrons

Mass-Protons/atomic #

Single replacement reaction

compound breaks apart and combines with the other reactant which is typically an element

Double replacement reaction

Both reactants break apart and recombine into two new parts

Synthesis/combination reaction

Several reactants combine to form a single product

decomposition reaction

a compound breaks down bc of a chemical change

Combustion reaction

tends to make H2O+CO2, reaction w/ O2 that produces light and heat

Group I solubility

soluble

NO3 - solubility

soluble

NH4+

soluble

Famous Precipitates

BaSO4 (white), PbI2 (bright yellow), AgCl, AgBr, AgI (white to pale yellow)

Precipitate Reaction

AB + XY = XB + AY (two ionics make at least one non soluble product)

Which are almost always (always when not with an always soluble) insoluble?

OH- (hydroxide), CO3 2- (carbonate), C2O4 2- (oxalate), PO4 3- (phosphate), "heavy metals"

electron configuration

1s2 2s2 2p5 etc (in order spdf)

What are orbital diagrams

the up down arrow ones

Coulomb's law

the force of attraction or repulsion between two charged particles is directly proportional to the product of the charges and inversely proportional to the distance between them. F = (kq1q2)/dˆ2

As an electron moves away from the nucleus it's potential energy...

..increases

what is special about transition metal ions?

they lose electrons from the s sublevel before d

isometric

same electron configuration (K+, Cl-, S2-, Ar)

periodic groups are...

...columns, # of electrons in outer shell

periodic periods are...

...rows, # of shells

transition element properties

conductive, malleable, for ions with variety of positive charges, act as good catalysts, often form colored compounds, form variety of alloys

valence electrons

outermost electron ring (highest energy level)

core electrons

\n all non valence electrons

effective strength formula

proton # - # core electrons = strength of + on valence e-

electronegativity/electron affinity

how much an element will attract electrons. increases (+ charge increases) across the periodic table, and decreases (greater atomic radii) descending

ionization energy (IE)

energy required to remove an electron. increases across (+ charge increases) and decreases descending periodic table (more barriers)

Evaporation is endothermic or exothermic

endothermic, need to GIVE it heat

cation

positive, metal

anion

negative, non-metal

Order of IMFs (least to greatest)

Disperson, dipole-dipole, hydrogen

Trigonal pyramidal

4 e- pairs, 3 bonds, 1 lone pair

Tetrahedral

4 e- pairs, all bonds

Octahedral

6 e- pairs, all bonds, x,y,z

Trigonal planar

3 e- pairs, all bonds, flat

Linear

2 e- pairs, all bonds, a line

Bent

4 e- pairs, 2 bonds, 2 lone pairs, angle

Water's normal boiling point is 100˚C, why can water evaporate at 20˚C?

Because of random velocities of water molecules causing some to have a high enough kinetic energy to escape from the surface.

What havens to water vapor pressure in a container with ice melting at room temp?

Increases rapidly, then more slowly until reaching equilibrium

What happens to the rate of condensation?

Increases until it equals the rate of evaporation and then remains constant.

What are the affects of temp, IMFs, and molar mass on the vapor pressure of a substance?

Vapor pressure increases with an increase in temp and a decrease in strength of IMFs and molar mass.

When, in general, does a liquid begin to boil?

\n When the vapor pressure equals the outside pressure

Why does ice have a lower density than water>

**than water>**

**Because of the crystal structure formed by hydrogen bonds and its open structure.**

hydrogen bonds occur when hydrogen is bonded to which elements

F, O, N

kinetic molecular theory

gas molecules are in constant random motion, when they collide energy is not lost, do not attract each other, far apart, same temp, same average kinetic energy

kinetic energy formula

KE=1/2mvˆ 2

pressure and force formula

p=f/a

Formula for pressure, volume, and temp

pv/t = pv/t

Dalton's law of partial pressures

Since gas pressure depends on # of molecules not their mass or size, it is easy to see that each gas in a mixture contributes pressure according to the number of molecules present.

Graham's Law

small particles diffuse faster

˚ C to K

\+273

atm to mmHg

atm x 760

How do gasses exert pressure?

Tiny molecules colliding with every pinhead-sized area of any surface. # of collisions is identical, forces add up for exert a force on the whole surface, creating a uniform "pressure".

Which is larger: proportional more collisions or harder collisions

samsies

mole to liter (for gasses)

1 mol = 22.4L

molar mass

g/mol

particles / mol

6\.02x10ˆ 23

Relative atomic mass

average atomic mass of all isotopes based on how common they are: (mass(%)+mass(%))/100

percent composition by mass

mass/total mass

density=

m/v

molarity

mass of solute per solution: moles of solute/liters

Dilution rule

concentration 1(volume 1) = concentration 2(volume 2)

Ideal gas law

PV = nRT

When will something produce a smell

when it is polar

When something has a charge, the polarity is…

Not applicable

manometer gas pressure shit

if gas is lower than outside: atmosphere pressure - height (mm) = gas pressure (mmHg)

\
If gas is greater than out side side: atmosphere pressure + height (mm) = gas pressure (mmHg)

percent error

(|accepted-measured| x 100) / accepted

is phase change a physical or chemical change

physical