Final Examination Review Packet 2008
Chemistry Level 1/2
Cheshire High School
Although
topics such as:
- Balancing chemical reaction
- Significant figures for multiplication and division
- Rules for rounding for addition and subtraction
- Naming compounds
- Writing formula equations from word equations
- The mole and molar mass
- Etc
Were
not directly covered the second half of the year, those topics are intimately interwoven into the fabric of chemistry and
serve as the backbone of the concepts covered following the midterm. As such,
knowledge of the above topics are quite important to review when studying for the final.
The
exam will cover in depth chapters 5, 12, 13, 14, 15, 16, 17, 18, 19 (pH and pOH), and for level 1 parts of chapter 20.
Note- for level 1 it is a cumulative final and all topics from the beginning
of the year will be covered- you should refer to the midterm study packet to help with the first half of the year.
Total
time for exam: 1 hour 55 minutes
- This time does not include the time required to distribute the materials.
General
advice for studying:
- There is a large quantity of material to study for the exam- do not wait till the last minute to study
- The most challenging part of the exam is recognizing which type of question you are dealing with. My best suggestion for you is to randomly take questions from different practice problem worksheets and
copy them to a separate sheet of paper (tonight or tomorrow night). Put that
sheet of paper aside and do not look upon it until you have studied for the exam. At
that point in time- since the problems are mixed- you should attempt to answer the questions.
If you do this right- you will be able to recognize problem type effectively.
Chapter 5:
- Major Topcis:
o
Development of the Periodic table
§ The
periodic law
§ Contributions
of Dobereiner, Newlands, Mendeleev, and Mosely
o
Reading the Periodic table
§ Why
elements in a group have similar properties
§ Metals,
non-metals, semimetals
§ Alkaline
metals, alkaline earth metals, halogens, noble gas
§ Noble
gas inner core and ionization energy
§ The
four blocks of the periodic tables
§ Periods
and series vs groups and families
o
Periodic Trends
§ Define
periodic trend
§ Five
basic periodic trends-
· Electronegativity
· Atomic radius
· Ionic radius
· Electron affinity
· Ionization
energy
§ Ionic
radii vs molecular radii
- Sample Calculations
o
How many elements are in the 2nd period?
o
Where are the non-metals located?
o
Why do elements in group 1A from 1+ ions?
o
Why does atomic radius decrease as you move from left to right across a
period?
o
Which element has a larger atomic radius- boron or magnesium
o
Which is bigger the Chlorine atom or the Chlorine ion
o
Why is a molecular radius smaller than the combined values of the individual
atoms involved in the bond?
Chapter
12 Thermochemistry
Vocabulary
of concern
- Heat capacity
- Specific heat
- Endothermic Reactions
- Exothermic Reactions
- Joule
- Temperature
- Calorimtery
- Tf
- Ti
- Thermochemistry
- Enthalpy
- Hess’s law
- Energy
- Calorie
Concepts
of concern
- Why do all chemical reactions involve changes energy?
- In terms of bonds- which has more energy stored in bonds (products or reactants) for exothermic reactions;
for endothermic reactions.
- When energy is found on the left side (reactants side) is the reaction endothermic or exothermic?
- Which sign is associated with the enthalpy of an exothermic reaction- is heat absorbed or released?
(Figure 12-5)
- What factors affect the amount of heat that a reaction absorbs or releases? (pg 385)
- How to apply Hess’s law
- The difference between heat and temperature
- Caloric theory vs. kinetic theory – who, what, and when?
Sample
Problems
1) How much heat
is absorbed if 13.92 g of nitrogen (N2) reacts with excess hydrogen according to the following equations?
H2 (g) + N2 (g) à NH3 (g)
DH = -92.22 kJ
2) If 28 kJ of heat are released according to the above equation, what mass of ammonia was produced?
3) From the following
enthalpy changes:
