2nd Semester SURVIVAL CHEMISTRY

2nd Semester SURVIVAL CHEMISTRY
Lundquist

Survival chemistry The BARE minimum you must know to pass the SOL/Semester exam SOL is cumulative 60 questions Multiple choice 10 Technology enhanced questions 30 is all 400 correct NO partial credit

Unit 7: Stoichiometry Balancing Mole to mole Mass to mass Vol to vol

Survival information from Unit 7: Stoichiometry
BEFORE ANY STOICH Balance reactions Rxts = prod. Keep polyatomics together Save elemental for last If stuck, double.

Note Quiz Questions 1 2

Mole to Mole Ratio In a balanced equation coefficients: Can be read as molecules AND moles Can be used as a conversion

THE PROBLEM C3H8 + 5O2  3CO2 + 4 H2O
If a propane (C3H8) tank lost 48.6g of mass while running, what mass of water (H2O) was produced?

48.6𝑔 𝐶 3 𝐻 𝑔 𝑚𝑜𝑙 =1.1𝑚𝑜𝑙 𝐶 3 𝐻 8 Mass to mass Stoich Dimensional Analysis (TESTED!!) Proportion Steps 1.1𝑚𝑜𝑙 𝐶 3 𝐻 𝐻 2 𝑂 1 𝐶 3 𝐻 8 =4.42𝑚𝑜𝑙 𝐻 2 𝑂 48.6𝑔 𝐶 3 𝐻 8 𝑋𝑔 𝐻 2 𝑂 = 44𝑔 𝐶 3 𝐻 8 =1 𝐶 3 𝐻 8 72𝑔 𝐻 2 𝑂=4 𝐻 2 𝑂 4.42𝑚𝑜𝑙 𝐻 2 𝑂 18 𝑔 𝑚𝑜𝑙 =79.5𝑔 𝐻 2 𝑂 𝑔𝑟𝑎𝑚𝑠. 𝐶 3 𝐻 8 →𝑚𝑜𝑙. 𝐶 3 𝐻 8 →𝑚𝑜𝑙. 𝐻 2 O→𝑔𝑟𝑎𝑚𝑠. 𝐻 2 𝑂 𝑔𝑟𝑎𝑚𝑠. 𝐶 3 𝐻 8 →𝑚𝑜𝑙. 𝐶 3 𝐻 8 →𝑚𝑜𝑙. 𝐻 2 O→𝑔𝑟𝑎𝑚𝑠. 𝐻 2 𝑂 48.6𝑔 𝐶 3 𝐻 8 1𝑚𝑜𝑙 𝐶 3 𝐻 8 44𝑔 𝐶 3 𝐻 𝐻 2 𝑂 1 𝐶 3 𝐻 𝑔 𝐻 2 𝑂 1𝑚𝑜𝑙 𝐻 2 𝑂 = 79.5𝑔 𝐻 2 𝑂

Percent Yield % 𝑦𝑖𝑒𝑙𝑑 = Experimental Theoretical × % 𝑦𝑖𝑒𝑙𝑑 = 𝐺𝑖𝑣𝑒𝑛 𝑆𝑡𝑜𝑖𝑐ℎ ×100 How much you produced In a perfect world = 100% (it’s never 100% -- reality sucks)

Note Quiz Questions 9 A student performs the above reaction with 1.01g Al and excess silver nitrate. She captures 12.5 g of Ag. What is her percent yield? 3.19% 95.9% 103 % 186% 10 If her experiment was similar to the one you performed in class, what is a possible reason for her percent yield? The sample may still be wet She did not use enough silver nitrate The gram scales were not accurate She did not calculate her theoretical yield correctly

Unit 8.1: Thermochemistry
States of Matter Phase change Kinetic & Potential Energy

Survival information from Unit 8.1: Thermochemistry
Solid Gas Strongest attraction between molecules Definite shape & volume Form a lattice Vibrational movement only NO attraction between molecules NO shape or volume Compressible & expandable Constant movement

Liquids Strong attraction between molecules (not REALLY strong, but still a lot) Definite volume but no shape Constant movement Special Properties Surface tension Viscosity Capillary Action

Note Quiz Questions (Unit 8.1)
1.

Phase Changes Energy

2. 3.

Enthalpy (DH) Measure of the potential energy stored in a substance Related to heat Measured in Energy During phase change, the energy needed to conduct that phase change is called the Enthalpy of X or heat of X Endothermic +DH Energy (heat) is a reactant Exothermic -DH Energy (heat) is a product

4.

Potential Energy diagrams A graph of enthalpy of a reaction over time Prod – Rxts = DH +DH = endothermic (Prod higher) -DH = exothermic (rxts higher)

Potential energy Diagrams Catalysts – lower the activation energy by rearranging the reactants, or providing an alternative pathway.

5.

Kinetic Energy Energy of motion Measured by temperature Heat ‘em up speed ‘em up General rule of thumb: 10oC increase in temperature will double the speed of a reaction

CELSIUS (oC = K – 273) Based off the freezing point of water KELVIN (K = oC + 273) Based off the freezing point of matter

6.

Calculating the amount of energy added/removed from a system q is energy (J or cal) m is mass (g or mol) c is specific heat (determines the others) DT is the change in temperature (K or oC) DT=Tf-Ti 𝑞=𝑚𝑐𝛥𝑇 𝑞=𝑚𝑐( 𝑇 𝑓 − 𝑇 𝑖 𝐽=𝑔 ( 𝐽 𝑔 𝑜 𝐶 )𝑜𝐶

Note Quiz Questions (Unit 8)
7. 8.

Phase change Increase/decrease in POTENTIAL ENERGY Increase the potential of chemicals to react Molecules move more an more thus weakening their IMFs

Phase Change -DHvap= DHcond DHvap -DHsub= DHdep DHsub DHfus
-DHfus= DHsolid

9.

Heating / Cooling Curves Graph demonstrating the temperature of a substance as energy is added (heating) or removed (cooling) Slopes = kinetic energy q=mcDT Plateaus = potential energy q=mDH Add all the q values to find the overall energy added (+)/removed(-)

Heating / Cooling Curves

10.

Kinetic Molecular Theory
Unit 8.2: Gases Pressure Kinetic Molecular Theory Gas Laws Ideal Gas Law

Units of Pressure at sea level
760mmHg = 760torr = 101.3kPa = 1atm

Survival information from Unit 8.2: Gases
Vapor Pressure Substances on the surface that break from their IMFs to form a vapor When vapor pressure > atmospheric pressure a substance boils

Unit 8.2 Note quiz questions
1. 2.

3.

Phase change diagrams Always (s)  (l)  (g) Lines = phase change Triple point Pressure and temp that all 3 states of matter are present Critical point Temp and pressure at which a substance is behaves like a liquid and gas

4.

Kinetic Molecular Theory 6 parts Lots of small particles Mostly empty space No attractive forces Constant motion Elastic collisions Avg. Temp ≈ kinetic energy

Gas Laws Graham’s Law Small gases effuse faster

Gas Laws Dalton’s Law The pressure of a system of gasses is equal to the partial pressures of the gasses in it. 𝑃 𝑇 = 𝑃 1 + 𝑃 2 + 𝑃 𝑃 𝑎 = 𝑃 𝑇 𝑚𝑜 𝑙 𝑎 𝑚𝑜 𝑙 𝑇

5. 6.

Gas Laws The Combined Gas Law You must be in kelvin! Give you ALL the gas laws P1V1=P2V2 Boyles V1T2=V2T1 Charles LABEL YOUR VARIBALES!!! 𝑃 1 𝑉 1 𝑇 1 = 𝑃 2 𝑉 2 𝑇 2 𝑃 1 𝑉 1 𝑇 2 = 𝑃 2 𝑉 2 𝑇 1

7. 8.

Remember these relationships Pressure & Volume INVERSE Volume & Temp DIRECT

Gas Laws The Ideal Gas Law R Is a constant (the ideal gas constant) IT WILL BE GIVEN TO YOU 𝐿·𝑎𝑡𝑚 𝑚𝑜𝑙·𝐾 NOT A FORMULA

9. 10. R = 𝐿·𝑎𝑡𝑚 𝑚𝑜𝑙·𝐾

Unit 9: Solutions Definitions Solubility Curves Molarity & Dilutions

Survival information from Unit 9: Solutions
Homogeneous Cannot be filtered Transparent Can be separated by evaporating the solvent

Solvent = what you have more of Solute = what you have less of Solvent determines the state of matter

All about attraction!

Unit 9 Note Quiz Questions
1.

Solubility Like dissolves like Polar compounds dissolve polar compounds Non-polar compounds dissolve non-polar compounds

2.

Factors that affect Solubility Temperature Effects solid solubility mainly Direct relationship with solubility Pressure Effects gaseous solubility mainly Solubility increases as pressure around the solute increases Surface Area Solids can be crushed to increase collisions

Solubility curves Graph assumes a 100g sample of water, if you had 200g just double the values Different phases dissolve differently Solids Higher solubility at higher temp. (+) slopes Gases Higher solubility at lower temps (-) slopes

Solubility curves Saturated – on the line Unsaturated – below the line Supersaturated – above the line Excess is precipitate Solid falls out of solution To calculate: find how much you are over on the Y-axis and subtract till you get to the line

9.1 Note Quiz 3. 4.

Molarity Concentration – how much stuff do you have in a set space You are usually given grams so you have to convert You are usually given milliliters so you have to convert 𝑀= 𝑚𝑜 𝑙 𝑠𝑜𝑙𝑢𝑡𝑒 𝐿 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛

Making solutions

9.2 Note Quiz Questions 5. 6. 7.

Dilutions Adding the solvent to lower the concentration of the solute. The amount of solute (mols) remains unchanged LOWERS concentration (M) 𝑀 1 𝑉 1 = 𝑀 2 𝑉 2

Performing Dilutions

9.2 Note Quiz Questions 8. 9. 10.

Unit 10: Equilibrium Collision Theory

Survival information from Unit 10: Equilibrium
Collision Theory Reactions only occur if reactants collide

Rates of reactions Rate = change in concentration of a reactant or product per unit time determined experimentally Appearance of Prod Concentration of rxts Change in temp.

Factors that effect reaction rates
Notes p. 1 Factors that effect reaction rates GENERALLY: 10oC increase doubles speed Nature of Reactants Concentrations Surface Area Temperature Catalysts

Note Quiz Questions (Unit 10)
1. 2.

When the rate of the forward reaction is equal to the rate of the reverse reaction Dynamic – constantly in motion Will stay the same FOREVER unless something changes

Note Quiz Questions Unit 10 (Unit 10.1)
3. 4. 5.

Le Châtelier’s Principle Factors that shift equilibrium A system at equilibrium will stay at equilibrium circumstances that shift equilibrium Concentrations of Prod/rxts Surface Area Temperature Catalysts – affects both the forward and reverse reaction equally

Le Châtelier’s Principle Predict the shift Remember the table on cinder blocks Predict changes Get the table to lie flat again. Reactant Products

What would happen if more N2 (g) was added?

What would happen if H2 (g) was removed?

7. 6. 8. 2SO2 + O2  2SO3

+ 92 𝑘𝐽 𝑚𝑜𝑙 REMEMBER Temp. can be added to the reaction
+ 92 𝑘𝐽 𝑚𝑜𝑙 REMEMBER Temp. can be added to the reaction DH > 0 it is a reactant DH < 0 it is a product What would happen if the reaction was heated?

7. Cooling the equilibrium mixture

REMEMBER for pressure follow the volume
Vol increase go to the side with more gas Vol decreases go to the side with less gas What would happen if the pressure increased?

8. 9. 10.

Unit 11: Acid Base Chemistry & RedOx Reactions
Naming Acids Acid Base theory pH & pOH Oxidation and Reduction

Writing the name from the formula Name as an Ionic compound Change based on ending “-ate””-ic acid” “-ite””-ous acid” “-ide””hydro-”ROOT “-ic” H2SO4 Hydrogen Sulfate Sulfuric Acid H2SO3 Hydrogen Sulfite Sulfurous Acid H2S Hydrogen Sulfide Hydrosulfuric Acid

Writing the formula from the name Determine the anion “-ate””-ic acid” “-ite””-ous acid” “-ide””hydro-”ROOT “-ic” The charge is the number of hydrogens Chloric Acid Chlorate ClO3- HClO3 Chlorous Acid Chlorite ClO2- HClO2 Hydrochloric Acid Chloride Cl- HCl

1.

Survival information from Unit 11: Acids & Bases
Conducts electricity corrosive. taste sour. React with metals to produce H2 gas. Indicators: Litmus = Red Phenophaline = clear bromothymol blue = yellow

Conducts electricity caustic taste bitter. Indicators: Litmus = blue Phenophaline = pink bromothymol blue = blue

Note Quiz Questions Unit 11
2.

Definitions of an acid Arrhenius Acids add H+ Start with H in their formulas Bases Add OH- End with OH in their formulas

Definitions of an acid Brønsted–Lowry Model Acids donate H+ Bases Accept H+ Creates conjugate pairs Con. Acid = add a H+ Con. Base = remove a H+

BRØNSTED–LOWRY CONJUGATE PAIRS

Note Quiz Questions 11.2 3. a. c. b. d.

0.1 The pH scale Think of it as how many zeros in front of the amount Acid pH < 7 (lots of H) Base pH > 7 (few H) The further from 7 the more acidic/basic

Note Quiz Questions 11.2 4.

Note Quiz Questions 11.2 5. 6.

The pH scale 14=𝑝𝐻+𝑝𝑂𝐻 𝑝𝑋=−log(𝑋

Note Quiz Questions 11 7.

Neutralization a reaction in which an acid and a base react in aqueous solution to produce a salt and water. double replacement reaction

Titrations Procedure to find the concentration of an unknown When they neutralize each other molacid=molbase (Macid)(Vacid)( # of H+) = (Mbase)(Vbase)( # of OH-)

Reduction Oxidation Gain electrons Lose electrons

Note Quiz Questions 11.3 9. a. c. b. d.

Oxidation Numbers Rules AKA Charge Be on the lookout for “-ide”s (those are ions) Assigned by a set of rules Biggies: 1 cap. letter = 0 (zero) O (oxygen) = -2 F = -1 The oxidation number of an ion is it’s charge The oxidation number for an atom in its elemental form is always zero, unless it has a charge The oxidation number of all Group 1A metals = +1 Oxygen is -2 (unless H2O2 then -1) The oxidation number of fluorine (F) is always -1. The sum of the oxidation numbers of all atoms (or ions) in a neutral compound = 0; in an ion = charge of the ion

Oxidation Numbers Give the ox. # for each element N2 NF3 CO2 NO3- HNO2 H2Cr2O7

Unit 12: Organic Chemistry
Definitions BASIC naming Polymers

Survival information from Unit 12: Organic Chemistry
What is Organic Chemistry Study of carbon based compounds EXCEPT: Carbonides (X4C) Carbonates (X2CO3) Carbon oxides (CO2)

Named by the number of carbons Prefixes Me Eat Peanut Butter How they attach to each other Single bond – “-ane” Double bond – “-ene” Triple bond – “-yne” Nomenclature

Nomenclature Named based off of the number of carbons in the LONGEST chain 1 = meth- 2 = eth- 3 = prop- 4 = but- 5 = pent- 6 = hex- 7 = hept- 8 = oct- 9 = non- 10 = dec- Remember: Me Eat Peanut Butter

Alkanes Alkenes & Alkynes Saturated End in “-ane” ALL single bonds Unsaturated End in “-ene” or “-yne” Double or triple bonds

Polymers LONG chains of carbons Made small sub-units called monomers

Uses of Polymers EVERYTHING Natural Polymers Proteins, cellulose, DNA Synthetic Polymers Teflon, Nylon, PVC, plastics

SOL SOON!!! 60 questions Approximately 40 correct is a 400.
The SOL 60 questions >40Multiple choice & < 15 TEIs (??) Approximately 40 correct is a 400. Approximately 51 correct is a 500 YOU CAN DO IT!!

2nd Semester SURVIVAL CHEMISTRY

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