Solubility Rules: ID the 6 Rules to Memorize

Solubility Rules: ID the 6 rules to memorize

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Polyatomics:ID 19 anions & 1 cationAcids:

----HCl = hydrochloric

----H2SO4 = sulfuric

----HNO3 = nitric

----CH3COOH = acetic

----H3PO4 = phosphoric

----H2CO3 = carbonic

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Matter is

Substance isMixture is

Homogenous Mixture has ______composition throughout (solution)Heterogeneous Mixture does not

Physical Properties: observed or measured Chemical Properties: ability to undergo chemical change

Law of Conservation of Mass:

Extensive Properties: mass and volumeIntensive Properties: composition

Solid: definite shape, volume, not easily compressedLiquid: indefinite shape, definite volume, not easily compressed

Gas: indefinite shape, volume, easily compressed*Particles are always moving in S, L, G

Indications of Chemical Reaction:

Qualitative give descriptions, no numbersQuantitative number-based

Accuracy is how close to a single measurementPrecision is how close several measurements are together

Error = | – |% Error = |expt-accepted|/accepted * 100Percent Yield = expt/theoretical * 100

1 kilo(unit) = _____(unit)1 (unit) = ____milli1 (unit) = ____centimicro=106nano=109

K =C =H2O FP=273KBP=373KDensity = mass/volumeDensity of H2O = 1 g/mL

Sig Figs: For addition & subtraction use ______/ For Multiplication & Division use ______

Dalton’s Atomic Theory: 1) 2)

3)4)

Proton = pos., change = radioactivityNeutron = neutral, change = isotopeElectron = neg., change = ion

AMU = atomic mass unit = 1/12th Carbon 12 atom (average atomic mass appears on Periodic Table)

Electrons found in electron cloud, move around in orbital, movement creates electricity

Quantum Mechanical Model: atom has no definite shape, increase in # of electrons = increase in size & energy

Energy Levels (n) = 1,2,3,4,5,6,7 (rows on PT)Sublevels = s (max 2e-), p (max 6e-), d (max 10e-), f (max 14e-)

Aufbau Principle:Pauli Exclusion:

Hund’s Rule:

**Exceptions based on Aufbau principle; due to stable electron-electron interactions; now unstable______

Frequency = Speed of Light/Wave LengthSpeed of Light = 3.0 x 108 m/s or 3.0 x 1010 cm/s

Atomic Spectra Principles:1) Light is a form of energy called Electromagnetic Radiation

2) Waves have wavelength and frequency3) Electromagnetic Radiation includes broad spectrum of radiant E

4) Speed of wave = wavelength x frequency5) Energy is directly proportional to frequency; freq. & w.l. are inversely

*When you excite electrons you increase energy which is given off as heat and light = atomic spectra

Dmitri Mendeleev arranged elements by ATOMIC MASSHenry Moseley arranged by ATOMIC NUMBER

Periods are rows / energy levels (1-7)Groups are vertical columns (18); A = representative elements, B = transitions

Periodic Law states

Noble Gases – Alkali Metals –Alkaline Earth Metals –

Halogens –Transitions –Lanthanides (inner transition)Actinides (inner transition)

Atomic & Ionic Radii –Ionic Size –

Ionization Energy –Electronegativity –

*Flourine (F) has highest ______*Francium (Fr) has greatest ______& ______

Cations give up electrons (metals)Anions take electrons (nonmetals)

Molecular Compounds: composed of

Ionic Compounds: composed of

MonaryCmpd. – 1 element Binary Cmpd. – 2 elements Ternary Cmpd. – 3 elements Diatomics:

Prefixes: Endings: -ide = periodic table -ite/ate: polyatomic

Ionic bonding –

Ions bond to complete their Octet Rule (have full outer electron shell)Seen through Lewis Dot Diagram

Metallic bonding – a more specific type of ionic bonding

Salts – metal cation + halogen; most are solid at STP, in 3D pattern, conduct electricity as liquid, ductile & malleable

Law of Definite Properties – masses of elements are in SAME PROPORTIONS within same compound
Law of Multiple Proportions – can compare masses of same element between similar compounds via small #d ratios

Covalent bonding –

Nonbonding Sites: IA (1; 1 valence e), IVA (4; 4 valence e), VA (3; 5 valence e), VIA (2; 6 valence e), VIIA (1; 7 valence e)

Coordinate Covalent –Resonance –

Paramagnetism –Dimagnetism –

VSEPR Theory – valence shell electron pair repulsion theory; e- repel each other so bond angles adjust

Trigonal Planar =120 deg. Tetrahedral =109.5 deg. TrigonalBipyramidal =90 & 120 deg.Linear=180 deg. Bent =120 deg.

Bond Polarity – polar = unequal pulling, nonpolar = equal pullingBond Dissociation Energy – energy to break bond (kJ)

Intermolecular Attractions – Ionic > Hydrogen > Dipole > DispersionVan der Waals –

Dispersion Forces –Dipole Interactions –

Hydrogen Bonds –

Avogadro’s Number = 6.02 x 1023 representative particles

THE MOLE ROAD:

Moles  Grams =Moles  Rep. Particles =Moles  Volume @ STP =

Grams  Moles =Rep. Particles  Moles =Volume @ STP  Moles =

Percent Composition: 1. Determine MM of each compound 2. Determine % of each element in compound

Percentage  Formula: 1. Assume % = grams2. Convert grams to moles of each element

3. Divide all mole values by smallest mole value to get “multiplier” for each element

Empirical  Molecular:1. Find Empirical Formula MM 2. MF mm/EF mm = multiplier

**Know how to balance equations

Types of Reactions: 4 base and 2 special = 6 totalReactants  Products

1. Synthesis –2. Decomposition –

3. Single Replacement –4. Double Replacement –

5. Acid-Base – 6. Combustion – 2 types; only thing that changes is hydrocarbon

COMPLETE: Hydrocarbon +INCOMPLETE: Hydrocarbon +

Solubility Constants and Rules

1-H2O is always a liquid2-Gases are anything that says “gas”, diatomics, noble gases

3-Solids are all metals except Hg4-Acids & Bases are always aqueous

Net Ionic Equations – 1. Break apartaq compounds2. Eliminate spectator ions3. Rewrite and balance

Stoichiometric Calculation Steps
1.Change GIVEN/HAVE into moles (reactants)
2. Convert HAVE of first reactant into NEED of second reactant via mole to mole ratio from balanced equation
HAVE > NEED =HAVE < NEED =
3. Take the moles of LR and convert to moles of the specified product then change moles of product into grams
This is the THEORETICAL YIELD
4. Determine Percent Yield(Actual Yield/Theoretical Yield) * 100
------Molarity – tells concentration of ions in an aqueous solution M =

Kinetic Energy – tiny particles are in constant motion; particle movement affected by volume, pressure, temperature
Evaporation = LGVaporization = LGCondensation = GL

Sublimation =Glass =

Plasma = [ex: Aurora Borealis – the Northern Lights]

To speed up kinetic energy = get faster movement = heat it upMeasures entropy (measure of randomness)
To slow down = become stationary = solidificationFor gases, collisions are elastic

Pressure: atm, kPa, mmHg, Tprr [1 atm = 101.3 kPa = 760 mmHg] result of collisions, no collisions in a vacuum

Temperature: Celsius, Fahrenheit, Kelvin; incr. temp = incr KEVolume: mL or L

Overall Relationship: only 2 change at a time; P&V are inversely proportional; T changes in same direction but ½ rate

Avogadro’s Hypothesis:

Real vs. Ideal Gases: ideal is hypothetical

Boyle’s Law:Charles’ Law:

Combined Gas Law:Dalton’s Partial Pressure:

Ideal Gas Law: P = pressure [atm (R=0.0821) or kPa (R=8.31)] V= volume n = molesT = Kelvin

**Know Exothermic and Endothermic Reaction Graphs

Energy transferred through the form of HEAT – determined by changes in temp
Exothermic = ∆H is ______, heat ______the systemEndothermic = ∆H is______, heat ______the system

Calorimeter – device that contains the heat within a unit, includes a lid and insulated holding device (Styrofoam cup)

Q = C x M x ∆Tq =M =∆T =

C = specific heat constant – 4.18 joules for water, 1 calorie for water

∆Hfus = molar heat of fusion∆Hsolid = molar heat of solidification∆Hvap = molar heat of vaporization
∆Hcond = molar heat of condensation∆Hsoln = molar heat of solution

**Know heat to mole ratio**Know Hess’s Law of Summation

Arrhenius (looks): Acid = H+ or H3O+; Base = OH- Bronsted-Lowry (behaves): Acid = Donates H+;Base = Accepts H+

Acids - # of Hs indicate strength of acid; more Hs means it can ionize more than once
HCl = monoprotic ionize onceH2SO4 = diprotic ionize twiceH3PO4 = triprotic ionize thrice

Bases - # of OHs tell solubility of base in water; more OHs means less soluble

pH = -log [H+]pOH = -log [OH-]pH + pOH = 14[H+][OH-] = 1 x 10-14

Neutralization Reactions – Acid + Base  H2O + SaltTitration – process of neutralizing an acid or base

Saturated –Unsaturated –Supersaturated –

**Solubility Graph!!!