chemistry boi i am finna rock this final bra

chem final chem final chem final chem final

pure substances - elements and compounds

pure substances cannot be broken down to a smaller parts.

1. elements

on the dang periodic table

2. compounds

made of 2 or more elements

what type of atom diagram is this

bohr’s diagram

atomic number means…

amount of electrons and protons (# of electrons = # of protons)

atomic mass is…

how many grams is in a mol of that element/compound

atomic mass - protons =

number of neutrons

ions are…

atoms that lost or gained an ion

cations

positively charged - electron is removed

these ions got oxidized

happens to metals

LEO

anions

negatively charged ions - gained an electron

these ions get reduced

happens to non-metals

GER

LEO says what

he sais GER

reducing agents

metals (cations)

oxidizing agents

non-metals (anions)

naming cations

name + ion

calcium ion

naming anions

name + ____ide + ion

sulfide ion

what is this

bohr’s ion diagram

make sure to add how many ions gained/removed

alkali metals

group 1

very reactive

shiny, soft, malleable, reactive

alkali earth metals

reactive but not as reactive as alkali

group 2

soft, shiny, and silver but not as reactive

halogens

group 17

very reactive non-metals

create salts with group 1

noble gases

non reactive and stable

group 18

diatomic

hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, bromine

Have No Fear Of Ice Cold Beer

ionic compounds

complete transfer of ions

cation and anion

molecular compounds

two non-metals

share electrons (covalent bond)

polyatomic molecules

sulfur - EIGHTTTTTTT

phosphorus - four

ionic hydrates

# of waters and then hydrate

sodium carbonate pentahydrate

electronegativity

the ability to attract electrons

non-metals have higher electronegativity because they need electrons, while metals have lower ones because they need to get rid of theirs.

intramolecular bond

bond within an atom

the bond between hydrogen atoms and oxygen atoms

intermolecular bonds

bonds outside of atom

the bond between 1 water atom and another water atom

types of intramolecular bonds in the context of electronegativity

ionic bond - a difference of 1.7 or more

polar covalent bond - a difference of less than 1.7

covalent bond - no difference/very low - maximum of 0.4 difference

ion compounds create

crystal lattices

they create very high melting/boiling points

electrons want to be as ___________ from each other as ________

far possibe

wat dat

linear bond

example - CN

number of bonds

how many thing can connect to it

wat dat

bent

examole - water

wat dat

trigonal planar

4 atoms

example - double bond and 2 bonds

wat dat

pyramidal

4 atoms with a lone pair

examole - NH3

watdat

tetrahedral

5 atoms

no lonepair possible

example - CH4

most repelling thing ever

lonepair

what type of compound is non polar all the time

hydrocarbons

strongest to weakest intermolecular forces

ionic bonding

hydrogen bonding

dipole dipole

london dispersion forces

london dispersion forces

a temporary dipole effect caused by the movement of electrons. The force of LDFS increases the larger a compound is. This force is there for all molecules.

Dipole-dipole forces

present in polar covalent bonds

caused by difference in electronegativity - there’s 2 sides; one slightly negative, one side slightly positive.

The greater the difference in electronegativity, the stronger the force

H-bonding

caused by an oxygen, nitrogen, or fluorine atom being bonded to a hydrogen

idk why

has a large effect on physical properites

Oh No Fred

the higher the boiling point,

the stronger the intermolecular forces are.

isoelectronic

same size (number of electrons and protons), but different intermolecular forces.

what di polar things dissolve in

polar things

like dissolves…

like

compounds with h bonding dissolves

compounds with H bonding

what will dissolve in water

polar and (ideally) h bonded things

water still dissolves just polar things with no h bond

network covalent

carbon ions

electrolytes vs non electrolytic

electrolytes disperse ions with charges into water after being dissolves

non electrolytes: disperse neutral particle

what happens when a soluble compound gets dissolved in water

it breaks into its elements

nacl → na + cl

this is electrolytic

insoluble ionic compounds

maintain the same compound but just becomes aqueous

AgCl(s) → AgCl(aq)

dissociation

when something breaks into its ions

1 cation and 1 anion

this happens to ionic compounds and bases

what is ionization

when the neutral covalent bond forms an ion in water

this happens to ACIDS (hydrogen = non-metal, the other one is also a non metal)

bases and solubility

bases are basic and are made of a metal and a hydroxide

look at the chart for the solubility

high solubility - dissociate into major entities

low solubilities - stay the same but becomes aqueous

adic and solubility

strong acids ionize completely and become their ions

weak acids just become aqueous

electrolyte solutions

all ionic compounds, acids, and bases

what are the solutions that are not electrolytic

elements (except for oxygen and halogens), and molecular compounds

molecular compounds and solubility

high solubility (polar) would just become aqueous

CHO(l) → CHO(aq)

low solubility (non polar) would stay the exact same

CH(g)→CH(g)

what are the soluble elements

oxygen and halogens

arrhenius’ acids

acids start with H or end with COOH

turn litmus red

arrehnius bases

ionic compounds that have the hydroxide ion

turns litmus blue

arrhenius neutral substance

H+ and OH- (H2O)

endothermic and exothermic

endothermic = absorb energy

exothermic = release energy

breaking bonds

requires energy

(endothermic)

forming new bonds

releases energy

(exothermic)

solubility test =

look for things that make precipitate

dilution question

c1v1=c2v2

misability

misability = polar

immisability = non polar

misability is when a liquid can mix and become one uniform textre

example of immisability: water+oil (different layers)

revised arrhenius’ definitions

there are hydronium ions present

pH calculation

-log[H+]

negative log the CONCENTRATION

[ ]

concentration

pH sigdigs

only digits after the decimal place matter

124.1 has a sig dig count of 1

ph concentration calculation

10 to the power of NEGATIVE pH

pOH calculation

-log[OH-]

pOH concentration calculation

10 to the power of NEGATIVE pOH

pH + pOH

= 14

[H+] x [OH-] =

10 to the power of negative 14

boyle’s law

p1v1=p2v2

charle’s law

direct relationship between volume and temperature if pressure stays the same

v1/t1=v2/t2

combined gas law

p1v1t2=p2v2t1

percent yield

actual yield/theoretical yield x 100 = percent yield

avogadro’s theory about gas

just use r/g

equal volumes of gas at the same temperature and pressure = same number of molecules in all of them

when doing the dissociation equation, you already get all the ratios out of the way which makes this law possible

how to act most like an ideal gas

high temperatures

low pressure (don’t want them colliding because of attraction that wouldmess things up)

PV=nRT

ok

equivalence point

when the concentration reaches the same amount of [H+] and [OH-]

endpoint

when the thing changes color

non ionic

normal

total equation

shows all the major entities - dissociated elements will be shown as such, and unchanged will also be there

net ionic

same as total except the spectators (same as before) are removed from the equation

>99%

quantitative, what is expected in a stoic question

steps to a stoic

1. balanced chemical reaction

2. calculate mols of given

3. r/g

4. solve