Chem Final

intramolecular

bonding within the molecule

ionic and covalent

solids, liquids, and gases do not

ionize

aqueous solutions, strong acids, and strong bases do

ionize

when formula writing make sure to write

states of matter

ionic and covalent are ____ than IMF

stronger

ionic

nm/m

transferred

covalent

nm/nm

shared

intermolecular forces

what relationship two molecules have with one another

types of intermolecular forces

london dispersion, dipole/dipole, hydrogen bonding

hydrogen bonding

nitrogen, oxygen and fluorine + hydrogen

boil/melt

cutting attraction

strongest

dipole/dipole

polar/polar

london dispersion

every molecule has london

depends on mass

mass> property

stronger the IFs, higher the

bp, mp, and viscosity

law of conservation of matter

mass cannot be created or destroyed

who came up with balancing equaltions

antoine lavoisier

Synthesis

N2 +3H2→ 2NH3

nitrogen reacts with hydrogen to produce ammonia

Decomposition

2H20→ 2H2 +O2

Water decomposes to produce hydrogen and oxygen

Single replacement

Zn + 2HCl → H2 + ZnCl2

Double replacement

Pb(NO3)2 +KI → PbI2 + KNO3

Complete Combustion

2HC + O2 → H20 +CO2

four states of matter

solid, liquid, gas, aqueous

pure liquid

H2O and Hg

diatomics

cannot exist by themselves

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

aq + aq → s + aq

occurs

aq + aq → aq + aq

does not occur

catalysts

speeds up reactions

not consumed

no power to start a reaction

activity series

determines if SR occurs

activity series rule

element that is by itself must be higher than what it is kicking out for reaction to occur

solubility table

to see if DR occurs

ioninc compounds

soluble

aq

insoluble

s

basic acid base neutralization

acid (ph=1) + base (pH=14)→ H20 (neutral, pH=7) + Ionic compound

step to balance ABNs

1. balance ionic compound

2. h

3. o

1 mol

molar mass

1 mole

6.022×10²³ molecules/atoms

Formula unit

ionic

stoich steps

1. write and balance equations

2. Label knowns and unknowns

3. use mass/mole conversions and mole-to-mole ratio

4. Look to see what units answer needs to be in

Limiting reagent steps

1. write/balance equation

2. label knowns and unknowns

3. take each reactant and calculate how much product will form. The reactant that yields less product is the limiting factor.

4. Do stoich to calculate what you need to do reaction

5. make sure you use lr lab value to calculate any product

percent yield equation

actual/theoretical x100

actual is the value

given

theoretical is the value found from

stoich

percent yields less than 100 means

you have lost product

percent yields over 100 could mean

product is wet or you have unreacted reactant

two components of a solution

solute and solvent

solute

gets dissolved (ionic)

solvent

dissolves solute

universal solvent

water

If the solute diappears, then you have a

homogeneous mixture

If some of the solute remains, then you have a

heterogeneous mixture (not a solution)

Equaltion for molarity

M= mol of solute/L of solution

The larger the molarity, the more

concentrated the solution (has a large amount of solute)

the smaller the molarity, the more

dilute the solution (has a smaller amount of solute

more dangerous to spill solutions with

higher molarity

If you have a concentrate solution then diluting the mixture will

reduce the molarity

dilution

add water to a solution to make it less concentrsated

purpose of dilution

save solute, make it safer for students

add acid

to water bc it will spit if you do it the other way

equation for dilution

m1v1=m2v2

When it asks what happens in a dilution say

pipette v1 value of m1 value in v2 flask, add water to mark

for soluble species we write an

(aq) meaning that we cannot see the solute

for insoluble species we write a

(s) meaning we can see the solute

what is a precipitate

chunking solid falls out of solution

precipitate reaction

aq + aq → s + aq

Electrolytes

compounds that are soluble in water and will conduct electricity as ions

water is

not a good conductor of electricity

strong electrolytes

soluble ionic compounds, strong acids, strong bases

bright light

HCl, NaHCO3

weak electrolytes

weak acids, weak bases, slightly soluble ionics and very few covalents

dim light

NH3

Nonelectrolytes

organic compounds and most covalents

h20 (deionized) and alcohol

dissociation=

pop=electrocute

what does it mean if an electrolyte is a s, l, or gas

no pop and double headed arrow

cannot pop

weak and non electrolytes

net ionics

1. write/balance equations and determine what is soluble and insoluble

2. split aq species into ions and keep isnoluble solids, gases, and liquids

3. cancel out spectator ions and reqrite equations

valence electrons

highest energy level

determine by looking at Roman numeral

Assymetrical things tend to be

polar

what doesnt hybridize

halogens and terminal atoms

have a hybridization of p

h hybridization

s

Symmetrical things tend to be

nonpolar

arrow on geometry

element comes forward

triple bonds

1 sigma, 2 pi

train tracks on geomtry

element goes behind

arrow for dipoles goes towards the

most electronegative element

+delta→ -delta

no pull/dipoles for

ionic and nonpolar covalent

label this

f orbitals are 4 and 5

what do you do if you have a d⁴ or d⁹

make them d⁵/d¹⁰ by moving an electron from s sublevel

how many boxes do s orbitals have

1

2e

how many boxes do p orbitals have

3

6e

how many boxes do d orbitals have

5

10e

how many boxes do f orbitals have

7

14e

stable sublevels

full spdf

half full pdf

empty spdf

para

at least one or more unpaired e

effects magnet

dia

all e are paired up

does not effect magnet

cation

loses electrons (+)

metals

anion

gains electrons (-)

nometals

group 1 charge

+1

group 2 charge

+2

group 13 charge

+3

Ag charge

+1

Zinc and Cd charge

+2

group 15 charge

-3

group 16

-2