Portfolio Page: Scientific Measurement

identify significant figures in measurements

_____ a. 0.050 ml

_____ b. 100. cm

_____ c. 30.0 g

_____ d. 5000 L

_____ e. 0.004 g

round answers to significant figures

__________ a. 28.993 (3)

__________ b. .00591 (4)

__________ c. .00591 (1)

__________ d. 10 (2)

__________ e. 1.0245 (3)

complete the chart

identify equivalent metric measurements with the same number of significant figures

measure quantities according to the limit of the instrument

__________ cm ___________ ml or cm3

T. O’Toole

leading zeros trailing

AND decimal

# sig figs scientific notation

- exponents are numbers smaller than 1 and larger than 0

Test: m, K, c, and cm3

VOLUME:1cm3 = 1ml

# sig figs convert

470 ml _______ ______ L.0050 Kg _______ _____ mg

30.0 cm3

_______ _____ L4.77 cm _______ _____ m5.0 g _______ _____ mg

Add an estimated

digit—even if it is a 0

How can I use measurement, the metric system, and scientific notation to explain if a 0 is significant?

report calculated answers to the correct number of significant figures

calculate percent errorThe volume of mouthwash is measured in a graduated cylinder. Mouthwash has alcohol

as an ingredient. Alcohol evaporates at close to room temperature. The mouthwash has been stored for a number of years. The measured volume was 362.0 ml and the package indicated the volume was 375 ml.

• What is the smallest graduation on the graduated cylinder that was used

• Calculate percent error

• Based on the sign of the percent error, what is the biggest source of error

How can I use factor label to convert quantities and solve problems?Morocco, shown at the St. Louis World’s Fair in 1904, measured 21.2 handsand weighed 2835 pounds If 1 hand measures 4.00 inches, how many meterstall was the horse? 1 meter = 3.28 feet

In one of the episodes of the TV program McGyver, a plane load of gold was being transported from the Soviet Union to the United States during World War II. The plane crashed in the Artic region and to prevent the "bad guys" from getting the gold the pilot and co-pilot transferred it to a cave by stacking the gold on a door of the crashed plane and pulling the gold on this "sled" to the cave. You were led to believe in the episode that they accomplished the move in one trip because the gold was neatly stacked on the "sled" in the cave. The neatly stacked gold measured about 1 meter on a side. Calculate the weight, in tons, of one cubic meter of gold. The density of gold is 19.3g/cm3

Jonathan Dorogy won a silver medal at the 2013 PIAA State Track and Field meet in the 100 meter dash with a time of 10.83 seconds. Convert this rate to miles per hour. There are 0.6214 miles in 1 km.

T. O’Toole

Addition & Subtraction Multiplication & Division

Express the sum of 7.68 m and 3.0 m using the correct number of significant figures:

Express the product of 4.0 x 10-2 m times 8.1 x 102 m using the correct number of significant figures:

only as far to the right as is common in all

total is least # of sig figs from all measurements

x100expected

expectedobserved

Portfolio Page: Matter and Its Changes

How can I use information about properties and indicators to justify whether a change is physical or chemical?

__________ granular texture

__________ length

__________ state of matter

__________ density

__________ reacts with acid

calculate density

How can I use specific heat to predict temperature change?calculate quantities related to specific heat

classify changes as physical or chemical

T. O’Toole

Intensive Extensive Chemical

What is the amount of heat required to increase the temperature of 100. grams of aluminum by 10.0 0C? The Cp is 0.21J/g 0C.

If 20.0 grams of gold is heated to 142.0˚C and then added to 30.0 grams of water at 20.0˚C the equilibrium temperature is 22.43˚C. Calculate the specific heat of gold. The specific heat of water is 4.18J/g˚C.

_____ origami (folding)

_____ burning

_____ filtering

_____ evaporation

_____ combustion

_____ leaves changing color

_____ exploding fireworks

_____ grinding

_____ sanding

_____ explosion

Dental aprons are required for patients receiving X-rays. These aprons contain a standard 0.30 mm thickness. An adult apron is 58.5 cm x 66.0 cm. Calculate the mass of lead in an apron if the density of lead is

3cm

g 11.3

D

MV

MDV

V

MD

REMEMBER: convert mm to cm, watch significant figures!

identify indicators for chemical changes

How can I use information about properties and changes to predict classifications of matter?classify substances (elements, compounds, homogeneous mixtures, or heterogeneous mixtures)

T. O’Toole

_____ air _____ 14 kt gold _____ sand + iron filings

_____ cement _____ nail polish _____ hand sanitizer

_____ helium _____ Tide laundry soap _____ carbon dioxide

_____ steel _____ nitrogen _____ propane

_____ methane _____ lead _____ copper

_____ zinc _____ granite _____ Jell-O

_____ iron _____ water _____ oleic acid

Chemical Change: Adding Alka-Seltzer to Water

Indicator:

New Substance(s):

Chemical Change: Neutralizing an Acid (resulting combination gets hotter)

Indicator:

New Substance(s):

Chemical Change: Plants converting Carbon Dioxide into Oxygen

Indicator:

New Substance(s):

Chemical Change: Ripening Tomatoes (producing ethylene gas)

Indicator:

New Substance(s):

Chemical Change: Two Colorless Liquids are combined to form a Solid and a Liquid

Indicator:

New Substance(s):

Chemical Change: Instant Ice Pack

Indicator:

New Substance(s):

Indicators:*heat*light*gas

*precipitate

Portfolio Page: The Atom & The Mole

How can I justify the structure of the atom based on historical experimentation?

explain and demonstrate the principles in Dalton’s Atomic Theory1. Matter is composed of tiny, indivisible particles called atoms

2. Atoms of the same element are identical, and atoms of any one element are different from those of another element

3. Reactions occur when atoms are separated from one another, joined, or rearranged, but matter cannot be created or destroyed

4. Atoms of different elements can combine in whole number ratios to form compounds

summarize the experimentation that led to the nuclear model of the atom

summarize the Gold Foil Experiment and Rutherford’s Nuclear Model

RESULTS: CONCLUSIONS

1. 2.3.

hypothesis:

•Early philosophers including Aristotle thought the “elements” were earth, air, fire and water•Democritus reasoned that matter must be made of small particles that were indivisible and therefore named them atomos (Greek) indivisible

LoDP Both LoMP

Example

Q. Why is this statement incorrect?

A.

Q. Why is this statement incorrect?

A.

Law of Conservation of Mass

~1800-Dalton 1897-Thomson

discovers electron

Plum Pudding Model

T. O’Toole

Portfolio Page: The Atom & The Mole

How can I use a model to represent subatomic information from the Periodic Table?

determine the identity of an atom or ion using the number of subatomic particles and the periodic table

calculate the average atomic mass of atoms with isotopesThe lithium found in a hearing aid battery has two naturally occurring isotopes. Lithium-6 has a mass of 6.015121 amu and an abundance of 7.42%. Lithium-7 has a mass of 7.016003 amu and an abundance of 92.58%. Calculate the (average) atomic mass of lithium.

How can I use factor label to explain the mole?

T. O’Toole

9Fluorine

19.00

18Argon39.95

35Bromine79.90

20Calcium40.08

Z=A=protons=neutrons-=electrons=

Z=A=protons=neutrons-=electrons=

Z=A=protons=neutrons-=electrons=

Z=A=protons=neutrons-=electrons=

isotopes have different numbers of neutronsions have different numbers of electrons!!

fluorine atom

argon atom

calcium +2 ion

bromine -1 ion

symbol protons neutrons electrons mass charge

Si 0

26 0

I 54

31 +3

196.97 +1

calculate moles in 7.50 grams of CuSO4 calculate atoms in .900 moles of Al

calculate molecules in 20.50 grams of Ca(OH)2 calculate moles in 2.35x1036 molecules of CO2

E. Goldstein determines the

mass of 1 proton in grams

Portfolio Page: The Electron

Why is the Bohr Model of the atom incomplete?

How does electron configuration predict valence number?identify and describe the quantum numbers and all possible values

write electron configurations in order to determine electron dot diagrams and valence numbers

T. O’Toole

Bohr Model-electrons function like particles and could therefore only exist in orbitals of fixed energy. This is also called the Planetary Model or the Solar System Model. This model will work for the element Hydrogen as it contains only 1 proton and 1 electron and therefore there is no electron repulsion.

Heisenberg Uncertainty Principle- This begins to refute the Bohr Model. “It is impossible to determine both the speed and location of an electron.” The mere process shining a light on it to look for it causes it to move. The particle behavior of electrons is not supported.

Quantum Mechanical Model, Wave Mechanical Model, Electron Cloud-Erwin Schrodinger concludes that electrons are points, but their forces of repulsion cause them to behave like waves. There is no exact location for an electron. There is a region in space where there exists the probability of finding the electron. This region in space is an electron cloud. The physical boundaries of the cloud are solution sets to calculus equations combining area and energy.

Quantum Numbers

1. Principal 2.Angular Momentum 3. Magnetic 4. Spin

Description

Possible Values

Aufbau: electrons go in orbitals with the lowest energy first

define and explain atomic radius

atomic radius across a period:

effective nuclear charge:

atomic radius down a family:

define and explain ionic radius

ionic radius down a family:

ionic radius across the cations:

largest cation in a period/series:ionic radius across the anions:

largest anion in a period/series:

define and explain ionization energy

Be:B:Circle the last electron in each electron configuration & explain why the IE of B < IE Be

____________________________________Circle the 1A elements and describe IE down a family ______________________________

define and explain electronegativity

Electronegativity-ability to pull an electron in a bonding situationFluorine has the most EN because___________

____________________________________

____________________________________

define and explain reactivity of metals• Metals with a _________radius will easily

lose electrons• Metals that only need to lose __________

electron will be more reactive than other metals

• ________ is the most reactive METAL

define and explain reactivity of non-metals• Non-metals with a ________radius will easily

gain electrons• Non-metals that need to gain _________

electron will be more reactive than other non-metals

• __________ is the most reactive non-metal

T. O’Toole

How can atomic radius, ionization energy, and reactivity be evaluated using the Periodic Table?

Portfolio Page: Formulas

How do you decide the appropriate method to name a compound?

Why do formulas contain subscripts and/or parentheses?writing formulas

T. O’Toole

IONIC MOLECULAR

Sodium Hypochlorite Carbon Monoxide

Iron (II) sulfide Silicon Dioxide

Lithium Dichromate Diphosphorus Trioxide

Potassium Permanganate Carbon Tetrachloride

Calcium Hydroxide Sulfur Dioxide

Tin (IV) Oxide Nitrogen Triiodide

Ammonium Chloride Phosphorus Pentachloride

Aluminum Sulfite Phosphorus Trihydride

Silver Nitrate Dinitrogen Tetraoxide

name acids

How is math utilized to describe a chemical formula?mathematically determine the percent composition of compoundsCalculate the percent of each element in potassium chlorate

mathematically determine the empirical and molecular formulas of compounds

mathematically analyze hydrates

T. O’Toole

percent to massmass to moledivide by smallesttimes til whole

A compound has been analyzed and contains 70.0% iron and 30.0% oxygen. Calculate the empirical formula and name the compound.

What is the molecular formula for CH2O if the molecular molar mass is 90.0 g/mole?

Calculate the percent water in sodium carbonate deca-hydrate.

Determine the empirical formula of a hydrate that is 32.3% water and 67.7% iron (III) phosphate

potassium chlorine oxygen

Portfolio Page: Bonding

How can bonding be used to predict properties?

predict and describe bond character

T. O’Toole

Ionic Bonds have a __________ EN difference. One element (a ___________) will have a large EN and a __________ valence number meaning it will gain electrons. The other element (a ___________) will have a small EN and a __________ valence number meaning it will lose electrons. When you subtract, you will get a difference greater than 1.7. In the dog bone analogy, the Non-Metal will completely take the electron from the metal. The non-metal forms a _______ and the metal forms a _______. These opposite charges attract causing the ions to come close together in a strong attractive bond. These bonds are not-symmetrical or _________ because anions are ____________ than their neutral atoms and cations are ___________ than their neutral atoms.

Polar Covalent Bonds have a __________ EN difference. When you subtract the two EN values, you will get a difference greater than .3 and less than 1.7. Polar means _________ and Covalent means ____________. These shared electrons count for both element’s octet. The sharing is unequalresulting in a dipole—thelarger EN elementhas the electron _______ of the time and thus is partially ____________. In the dog bone analogy, thelarger EN (dog) will take the electron more of the time.

Non Polar Covalent Bonds have a __________ EN difference. This is because each element has a _____________ EN. When you subtract the two EN values, you will get a difference less than .3. Non Polar means _________ and Covalent means ____________. These shared electrons count for both element’s octet. The sharing is equal because neither element has sufficient EN to “win” the electron.

metal + non-metal

2 different non-metals or middle of periodic table

2 identical non-metals

EN difference

bond character

larger atom formula

H and O

Zn and S

O and O

metallic bonding

How can the geometry of a molecule be predicted?draw Lewis dot diagrams for single bonds to predict molecular geometry

How can the geometry of a molecule predict properties?predict and explain hydrogen bonding

draw Lewis dot diagrams for covalent compounds and ions

Example: H2CS

Example: sulfate ion with resonance

T. O’Toole

“Bond” between 2 adjacent molecules each containing H and N, O, or F. The hydrogen becomes partially positive because of its smaller EN and the N, O, or F become partially negative because of their large EN. These opposite charged ends attract adjacent molecules to each other making boiling points higher than you would expect.

1. Count valence electrons2. Required for octet (8 each or 2

for each H)3. Shared pairs= (#2-#1)/2

electrons in a pair4. Unshared pairs=(#1-electrons in

shared pairs)/2 electrons in a pair

5. Distribute unshared pairs as necessary

AB and AB2-linear AB3-trigonal planar AB4-tetrahedral

AB3E-trigonal pyramidal AB2E or AB2E2 -angular/bent AB5-trigonal bipyramidal

Portfolio Page: Reactions

How are the products of chemical changes predicted?

write equations in words and symbols for double replacement reactions

write equations in words and symbols for single replacement reactions

T. O’Toole

DiatomsH2, N2, O2, F2, Cl2, Br2, I2

FormatAB + CD AD + CB

Underline the cations—they switch

1. calcium hydroxide + lithium phosphate

2.

Precipitates and Net Ionic Equations• Write the equation in words and then symbols, circle the precipitatecobalt (II) chloride + lithium carbonate

• Write the total ionic equation and the net ionic equation for the reaction between calcium chloride and silver acetate

2 cations switch+ +

1. zinc metal is added to copper (II) sulfate

2.

• Write a single replacement reaction that contains exactly 2 diatoms

• Write a single replacement reaction that produces hydrogen gas

write equations in words and symbols for simple and complex synthesis reactions

complex synthesis - two binary compounds form 1 compound with a polyatomic ion

write equations in words and symbols for combustion reactions

C2H + O2 CO2 + H2O

C4H + O2 CO + H2O

write equations in words and symbols for decomposition reactions

Why are chemical equations balanced with coefficients, not changing subscripts?Balance H and O second to last and last!!If you end up with an even # of O on one side and an odd # of O on the other—DOUBLE!

T. O’Toole

C+ + A- CA

Cation MUST be first

Use Criss-Cross

magnesium is burned in air and combines with oxygen

sulfur is added to zinc and burned

reactant anion

SO2 SO3-2

SO3 SO4-2

N2O3 NO2-1

N2O5 NO3-1

P2O3 PO3-3

P2O5 PO4-3

lithium oxide is dissolved in water

iron (II) oxide is burned in diphosphorus pentoxide

write the equation for the synthesis of aluminum nitrite

CnH2n+2

1=meth 6=hex

2=eth 7=hept

3=prop 8=oct

4=but 9=non

5=pent 10=dec

CompleteCO2 + H2OIncompleteCO + H2O

reactant product product

C+A- C A

C+ClO3-1 C+Cl-1 02

C+CO3-2 C+O-2 CO2

C+OH-1 C+O-2 H2O

+ sodium iodide

aluminum chlorate

copper (II) carbonate

lithium hydroxide always use criss-cross for reactants and the pattern product

Portfolio Page: Stoichiometry

How can I use factor label to solve for quantities involved in chemical changes?use the mole ratio from a balanced chemical equation to solve for chemical quantities

Use the decomposition to the right to answer the following:1. If you decompose 2 moles of potassium chlorate, how many moles of oxygen will be produce?

2. If you decompose 4.57 moles of potassium chlorate, how many moles of potassium chloride will be produced?

3. Because we don’t have scales that measure moles, we should use grams. If you decompose 4.57 moles of potassium chlorate, how many grams of potassium chloride will be produced?

4. If you decompose 10.0 grams of potassium chlorate, how many grams of oxygen gas will be produced?

5. If you want to produce 5.00 grams of potassium chloride, how many grams of potassium chlorate will have to be decomposed? How many grams of oxygen will also be produced?

T. O’Toole

Unit of coefficient is MOLE2KClO3 2KCl + 3O2

this decomposition will produce 2 moles KCl and 3 moles O2

calculate quantities using molarity

molarity is used for liquids because liquids are measured in volumes, butthey also have a concentration term. You know there is more Kool-Aidmix in a darker solution than there is in a lighter solution. We don’tmeasure the amount of mix in teaspoons—but rather moles.

calculate quantities using limiting reactant

15.0 ml of .25M lead (II) nitrate to 5.00 grams of sodium iodide, how many moles of precipitate are formed?

If .020 grams of zinc are added to 10.0 ml of 3.0M hydrochloric acid, what is the maximum mass of gas that can be produced?

T. O’Toole

If 75.0 ml of 3.0 M sodium phosphate are added to copper (II) nitrate, how many grams of precipitate are formed?

If .0500 grams of magnesium react with hydrochloric acid, how many ml of 3.00 M acid are required?

It is unusual for a reaction to contain perfect amounts of reactants so that all reactants are completely consumed and 100% product formation is possible. Usually something runs out—and when it does the production of products is LIMITED!

1. Convert to moles2. Divide by coefficient3. LR is SMALLER!!!

Portfolio Page: Gas Calculations

explain the behavior of gases

calculate with gases at STP

bubbling through water, water displacement, over water

T. O’Toole

Kinetic Theory*All matter is made of tiny atoms and molecules that are in constant motion*This motion causes elastic collisions (no loss of energy)*The particles have mass but not volume*The particles have no attractive or repulsive forces for each other*Molecular motion is temperature dependent (theoretically then there is a temperature where motion stops i.e. Absolute Zero or 0 K)Real Gases do not conform to these behaviors and can be liquefied and solidified by changing temperatures & pressures

Pressure

Pressure-force of colliding particlesMore Particles = More Pressure

**High altitudes have less pressure because they have fewer particles

Avogadro’s LawEqual volumes of gases at the same temperature & pressure will have the same number of particles (but different mass)

STPSTP=standard pressure & standard temperature

There are equivalent standard pressures so that conversions can be made using factor label

1 atm = 760 torr = 760 mmHg= 101.3 kPa

1 atm and 0˚C

K= ???˚C + 273

1. If 100.0 grams of lithium are added to water, what volume of gas can be produced at STP?

2. If 250.0 ml of propane undergoes complete combustion, how many grams of water will be formed at STP?

Neither example incorporates limiting reactant—but that is possible!!

1 mole of any gas at STP

occupies 22.4 L

water PLUS gas

How can I use math to solve for variables relating to one gas?

How can I use math to solve for gas quantities involved in chemical changes?*These problems require both factor label (B/A) and Pv=nRT—the order depends on the given!!

T. O’Toole

+

NOTE: grams of a gas can be converted to moles using factor label and the periodic table. This calculation can be written as n=g/fw.

g= fw=

An aerosol can with a volume of 456 ml contains 3.40 grams of propane gas as the propellant. If the can is at room temperature (23.00C), what is the pressure in the can?

Calculate the mass of the air in a hot-air balloon that has a volume of 4.00 x 105 liters when the temperature of the gas is 30ºC and the pressure is 748 mmHg. The molar mass of air is 29.0 grams per mole.

The Dumas method was used to determine the formula weight of a volatile liquid. The empty test tube with a volume of 8.60 ml and foil cover had a mass of 7.5228 grams. A volatile liquid was placed in the test tube and covered with the foil. The system was placed in a 99.0˚C water bath where the liquid vaporized and then condensed. The system after the experiment massed 7.5387 grams. The pressure was 100.0 kPa. Calculate the formula weight of the volatile liquid.

Determine the mass of water required to react with 100.0 ml of diphosphorus pentoxide if the reaction takes place at 745 mmHg and 23.0˚C.

Determine the volume of gas that can be collected by bubbling it through water if .05 grams of magnesium are added to 10.0 ml of .15M hydrochloric acid. The barometric pressure is 742 mmHg and the temperature is 28.0˚C.

LR

Portfolio Page: Gas Behavior

How do the three gas Laws represent the principles of Kinetic Theory?How can I use math to verify the principles of Kinetic Theory?

T. O’Toole

Boyle’s Law

Charles’ Law

Gay-Lussac’s Law

Combined Gas Law

When a tooth becomes infected the tissue fills with gas. While waiting to see the dentist, a person tried to relieve the pain by treating the area with moist heat. Will this help? Why or why not?

The gas inside an aerosol can is 5.9 atm at room temperature (22˚C). What is the pressure when the can is heated to 100˚C?

Explain how the contents of a small fire extinguisher can be used to put out a larger sized fire.

The volume of a gas is reduced from 200.0 ml to 50.0 ml when the pressure is changed TO 1.9 atm. What was the original pressure?

Explain why a can of pop explodes if left in the hot sun.

A balloon has a volume of 3.12 L at 22˚C. What is the volume outside on a 37˚C day?

An internal combustion engine in a car operates by injecting fuel vapor and air into a cylinder, compressing the gas with a piston, and igniting the pressurized gas. Suppose an engine cylinder has a volume of 420 ml when the gas is injected. The gas has a temperature of 32°C and a pressure of 92.0 kPa. At the time of firing, the cylinder volume has changed to 49.4 ml and the gas is at a temperature of 400.0°C. What is the pressure of the gas at that time?

Polar Solute & Solvent Non-Polar Solute & Solvent

draw the diagrams for water solvent dissolving the Na+ and Cl- ions

Explain how non-polar solutes are dissolved

Portfolio Page: Solutions

How can I use molecule polarity to predict an appropriate solvent?

How can I use solubility curves to explain solutions?

explain factors that affect the solubility of gas and solid solutes

T. O’Toole

solid soluteTemperature-

gas solute

Temperature-

Pressure (Henry’s Law)-

-define each term-identify an appropriate point

saturated-

unsaturated-

supersaturated-

use colored pencils

Specifically, how would you prepare a supersaturated solution with 150 grams of KNO3 dissolved in 100 grams of water at 60˚C?

__________ How many grams of solute can be dissolved in 100 grams of water at 20˚C?

__________At what temperature will 150 grams of solute in 100 grams of water be saturated?

If you have 190 grams of solute dissolved in 240 grams of water at 600C, is the solution

saturated, unsaturated, or supersaturated?

How can I use math to explain solution concentrations?calculate molarity and mass of solute required

calculate molality and mass of solute required

calculate percent mass and mass of solute

How can I use math to explain colligative properties?

T. O’Toole

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R

Calculate the molarity if 40.0 grams of potassium permanganate are dissolved in a 250 ml volumetric flask.

How would you prepare (what mass of solute is required) to prepare 500 ml of.15M copper (II) nitrate?

Calculate the molality if .75 grams of calcium hydroxide are added to 200 grams of water.

How would you prepare (what mass of solute is required) to prepare a .28m solution of potassium carbonate if 500 grams of water are available?.

ml solvent unknown

g (ml) solution unknown

Calculate the % if 0.059 grams of solute are dissolved in 10.0 grams of solvent.

Calculate the grams of solute required to prepare 150.0grams of a 7.5% solution.

Calculate the grams of solute required to prepare a 14% solution if 100 grams of water are available.

Volatile/Ionic Solutes • Formed from criss-cross• Fall apart into ions• CaCl2 #=3

Non-Volatile/Molecular Solutes• Not formed by criss-cross• #=1

Calculate the formula weight of an ionic solute (C2X) if 16.20 grams are added to 250.0 grams of water. The solution boils at 110.5˚C.

____ NaCl____CH3OH____Ca(OH)2

Calculate the new freezing point and the new boiling point of a solution containing 4.025 grams of sodium chloride dissolved in 100.0 grams of water. Kf=1.86˚C/m and Kb=.512˚C/m

Portfolio Page: Acids and Bases

T. O’Toole

How can I make connections to polarity, dissolving, and ionization?

Base -will ionize in water to produce OH- ions-sometimes water produces the OH- ions

like the case of NH3 + H2O NH4+ + OH-

-bases are electrolytes (conduct electricity)

How can I make connections to nomenclature?

identify properties of acids and bases

Acids:

Bases:

Acid-will ionize in water to produce H+ ions-these H+ ions attach to water H3O

+

-acids are electrolytes (conduct electricity)

ACID and BASE strength is directly proportional to % ionization

strong electrolytes are strong acids/bases

Draw 5 molecules of a weak acid using the generic formula HA.

How many of the molecules would ionize if the acid had been a strong one? _______

acetic acidbinary or ternary

hydrochloric acidbinary or ternary

nitrous acidbinary or ternary

H3Pbinary or ternary

H2Sbinary or ternary

H2SO3

binary or ternary

acid base

phenolphthalein

litmus

How can I make connections to reactions?

How can I use math to explain pH?

T. O’Toole

+

R

Acid + Metal: Single Replacement

Always Produces:

Write the balanced equation for nitric acid added to copper to produce a blue liquid

Acid + Carbonate or Bicarbonate: 3 products

Always Produces:

Write the balanced chemical equation for acetic acid added to sodium carbonate

Acid + Base (Neutralization): Double Replacement

Always Produces:

Write the balanced chemical equation for titrating hydrochloric acid with calcium hydroxide

Calculate the molarity of acid if 25.72 ml of .15M sodium hydroxide was used to neutralize (titrate) a 25.0 ml sample of sulfuric acid.

Acid Anhydride (Non-Metallic Oxide)

Base Anhydride (Metallic Oxide)

pH pOH [H3O+] [OH-] A or B

8.2

3.72x10-4

Kw=1x10-14

Kw=[H3O+][OH-]

pH + pOH=14

Portfolio Page: Redox Reactions

define oxidation and reduction

What connections exist between valence number and oxidation number?

How can I justify inserting coefficients from the half-reactions?How can I predict which chemical changes are Red-Ox?

T. O’Toole

Oxidation

Oxidation:• Loss of electrons• Increase in oxidation number

Na0 Na+1 +1e-

Remember: Losing negatively charged e- makes the element positive

Reduction

Reduction:• Gain of electrons• Reduction in oxidation number

1e- + Cl0 Cl-1

Remember: Gaining negatively charged e- makes the element negative

___Fe2O3 + ___CO ___Fe + ___CO2Redox because:

Oxidation including electrons lost

Reduction including electrons gained

___KMnO4 + ___H2C2O4 + ___H2SO4 ___MnSO4 + __K2SO4 + ___CO2 + ___H2ORedox because:

Oxidation including electrons lost

Reduction including electrons gained

Portfolio Page: Nuclear Chemistry

trace the discovery of radioactivity and isotopes

define the types of radiation

How can I write nuclear decay equations?

T. O’Toole

Henri Becquerel (1896)- discovered that uranium salts produced images on photographic plates in the absence of sunlight.

Marie Curie- purified the uranium ore to discover Polonium and Radium which were each capable of emitting particles and energy spontaneously to make their nuclei more stable.

Alpha decayUranium-238 begins its 14 step decay chain by emitting an alpha particle. This chain is completed in approximately 4.5 billion years (half-life).

Beta decayCarbon-14 decays in one step that requires 5730 years.

Gamma decaySometimes the high-energy radiation of gamma rays are emitted alongside alpha decay and beta decay. This is the second step in the decay of Uranium 238 (check your answer above).

How can I use math to explain the half-life of isotopes?

T. O’Toole

+

Calculate the amount remaining

1. The half-life of polonium-210 is 138.4 days. How many mg will remain after 415.2 days if you start with 2.0 mg?

2. Chromium-48 has a half-life of about 24 hours. If the initial activity in a sample is 3000, what is the activity after 60 hours?

Calculate the half –life 1. How much time would elapse for the radioactivity of C-14 in a piece of wood to drop from 14 counts per minute to 8 counts per minute if the half-life is 5730 years?

2. Bismuth-218 decayed from 3.0 grams to .375 grams in 1 hour. What is the half-life of this isotope?

3. The gamma rays from cobalt-60 are commonly used to irradiate food so as to kill harmful bacteria such as E. coli. Calculate the half-life of this isotope if after 1384 days the activity decreased from 3773 counts to 2292 counts.