Test Review Material

3U Study Guide for upcoming tests

Test #2 Chapters 4, 5, 6 with Nomenclature and Balancing
Test Thursday March 24
The following items will be found on this test

Simple nomenclature → make sure you both a periodic table and oxyacid chart
Balancing simple equations
Determining # of moles given a formula weight and the reverse problem
Working with Avogadro’s Number; grams ↔ moles ↔ number of molecules/atoms
Determining relative isotopic abundance
Trends in the periodic table
Bonding types; covalent, polar covalent, and ionic. Electronegativity and its use
Determining the % composition given the formula
Determining the Empirical formula given the % composition
Given a formula weight and a % composition, calculate the true formula

Test Review for Chapter Seven
Test Monday April 11

Make sure you can convert grams to moles and the reverse.
There is one question that asks you to use Avogadro's number.
Make sure you know what a double and single displacement reaction is.
Don't forget to balance equations.
Be careful and read questions carefully for units when working with a stiochiometric question.
Make sure you can handle the percentage yield question both ways, both finding percentage yield and if given percentage yoild calculate the mass of produce produced.
The standard limiting reagent question and one that asks you to just determine the limiting reagent.
Have a look at questions 9, 11, 17,
And that's all she wrote , folks!

Test Review for Chapter Nine
Test Monday April 25, May 9

Completing reactions using work equations

Completing reactions using formula then balancing the equation see page 340

Find the concentration of a solution given mass and volume; units in mol/L

Find the required number of grams required to make a given concentration at a fixed volume

Finding the final concentration of a solution when two solutions of given concentration and volume are mised together

Finding the mass of a precipitate formed when two solutions are mixed. In this type of problem a balanced equation is needed for mole ratios. A double displacement reaction usually occurs.

Finding the mass or percentage by mass of a soluble salt dissolved in water by precipitating either the cation or anion of this salt. The mass of sample taken and mass of precipitate are usually given. Problem is writen as an experimental investigation

Variation on the above may be used, such as find volume instead of mass in a solution.

Test Review for Acids Bases Chapter 10
Test May 19

Test format: true and false, multiple choice, short written answers, and problems

The two theories of acids and bases: Arrhenius and Bronsted-Lowry theories

Make sure you know the following terms or situations

conjugate acid base pair

The hydronium ion

An amphoteric substance

indiactor with examples

end point and equivalence point

pH and pOH and what the number mean

strong and weak acid or base, how to tell them apart

How to calculate the pH of a solution given the hydrogen ion concentration and
how to determie the concentration of a solution given the pH

Make sure you know your indicator colours

Be able to write balanced equations for neutralization reaction

Be able to solve a titration question to determine an unknown concentration. With this unknown concentration be able to convert it into a mole or mass value

Be able to determine the volume of a titrant (concentration given) required to neutralize a given concentration of acid or base

Be able to determine the amount of a concentrated acid (or baes) need to make a solution of required concentration. Similar to last chapter.

Test Review for Gas Laws Chapter 11 & 12
Test May 26

Test format: true and false, multiple choice, short written answers, and problems

Know your gas laws as statements

Boyle's Law

Charles' Law

Gay-Lussac's Law

Dalton's Law of Partial Pressure

Law of Combining Volumes Gay-Lussac's second law

Avogadro's hypothesis

Ideal Gas Law

Make sure you know equations that relate to all of the above and the combined Gas Law equation

Be able to solve questions using Gas Law equations

Using the Ideal Gas Law equation (an equation of state) PV = nRT to solve questions
Know what molar volume and molar mass are in relation to this equation

Kinetic Molecular Theory; know the postulates that where given to you as a note
especially the KMT of pressure

You did two assignments; make sure you know what these assignments taught you

Know how to convert Celcius to Kelvin and back again and never solve Gas Law problems in Celcius

Macro properties of a gas

STP and ASTP

Know your constants

8.314 L·kPa/K·mol the Gas Law constant

22.4 L/mol the volume of 1 mol at STP

101.3 kPa STP pressure

O^o C or 273 K STP temperature

Working with the balanced equation: Gas Law stiochiometry, use the matrix set-up you were taught
Are the conditions at STP? if so use 22.4 L/mol in the data row
Conditions not at STP? solve for the number of moles then use PV = nRT to find the require volume

Test Review for Organic Hydrocarbons and Calorimetry Chapter 13 & 14
Test June 2

Know the first ten hydrocarbon prefix names for the alkanes (single bonds) alkenes (double bonds) and alkynes (triple bonds)

Know the substituent add-on groups, probably the first four will be sufficient
methyl, ethyl, propyl, and its buddy isopropyl and butyl and its buddy tert-butyl

What does cyclo- means and how is it used in drawing organic compounds

Be able to sketch formula given names; know what the number mean

Be able to write names give a diagram of a hydrocarbon

Know what "di..." means in naming compounds

Cis and trans isomers

Combustion of hydrocarbons: complete and incomplete combustion

Thermodynamics: types of thermochemical reactions (equations)

endothermic

exothermic

bond energy making and breaking bonds and the potential energy diagram (graph)

know what a calorimeter is and what it collects

Measuring energy changes : Calorimetry

Thermal energy and heat

Heat flow and the measurement of heat changes

Principle of Heat Exchange

Calorimetry: the collection of heat produced in a reaction

Energy equation Q = mΔtc, this is a heat transfer equation

Be able to work with this equation and remember that heat produced by a reaction is absorbed by the calorimeter (usually a mass of water)

know what the number 4.184 J/g·^oC means and what it can only be used for. Celcius can be used because we are dealing with Δt not an actual temperature value

Be aware that each substance hast its own specific heat capacity

Be aware that a calorimeter will have a heat capacity not a specific heat capacity

It may seem like a lot here but there isn't