Chemistry Final Exam Review Topics Honor 2008-09

EnglishHonors ChemistryFinal Exam Review Guide

Chemistry Final Exam Review Guide Honors 2013-4

The final exam will assess the knowledge and skills you developed through the entire year (Unit 0-8) because the concepts and skills learned during the first semester are put in use in concepts developed in the second semester. This document provides you with a summary of the learning objectives that will be assessed in the final exam. Here are some items to study and review.

Learning Objectives from each unit
Unit Reviews (Unit 0-8)
Formative assessments in each unit
Unit tests (available to you during afterschool help sessions and the review day)
Worksheets and handouts
Lab reports and notes

Unit 0-1 Physical Properties of Matter – Simple Particle Model

1.Measurement:

Correct scale reading and uncertainty
Recognize the number of significant figures in a given measured value.
Round off calculated values to the appropriate number of significant figures.
Convert between quantities in metric units using dimensional analysis.
Correctly using scientific notation when appropriate.

2.Density:

Recognize density is a characteristic property of matter.
Identify substances using density
Interpret a Mass-Volume graph
Recognize density is a proportion between mass and volume and can be used as a factor label to convert between mass and volume.

Unit 2 Energy and States of Matter Part 1

1.States of matter

Describe the characteristics of solids, liquids and gases in terms of particles and their arrangement.
Use particle diagrams to account for motion and density differences.
Describe how the arrangement of particles changes during phase changes.

2.Energy and Kinetic Molecular Theory

Relate temperature to the kinetic energy (Ek) of particles in motion.
Explain, at the particle level, how a thermometer measures the temperature of the system.
Recognize the basic tenets of Kinetic Molecular Theory (KMT).

3.Gas behavior

Describe how a mercury barometer measures atmosphere pressure.
Determine the pressure of an enclosed gas from the manometer display.
Apply features of gas particles and the concept of pressure to explain observations.
Predict the effect of changing P, V, n or T on any of the other variables.
Explain (in terms of the collisions of particles) why the change has the effect you predicted.
Use factors to calculate the new P, V or T. Make a decision as to how the change affects the variable you are looking for. (PVnT table)

Unit 3 Energy and States of Matter Part 2

1.States of matter

Describe the characteristics of solids, liquids and gases in terms of particles arrangement and attractions

2.Energy storage and transfer

Define energy and describe ways of how energy is stored in a system and how energy is transferred between system and surroundings.
Draw and interpret energy bar diagrams to account for energy storage and transfer in all sorts of physical changes.

3.Heating/cooling curve

Identify what phase(s) is/are present in each portion of the curve.
Identify energy in which storage mode is changing for each portion of the curve.
Relate energy bar diagrams to any points along the curve.
Draw and interpret heating/cooling curve of a substance from the given melting and boiling temperatures.

4.Energy calculation

State the meaning of the heat of fusion (Hf) and heat of vaporization (Hv) for a given substance. Use these factors to relate the mass of a substance to the energy absorbed or released during a phase change. (at melting/boiling temperature)
State the meaning of the heat capacity (c) of a substance and use this factor to relate mass and temperature changes to the energy absorbed or released during a change in temperature (with no phase change).
Calculate total energy absorbed or released during a process involving both phase changes and temperature changes. (draw heating/cooling curve to help)

Unit 4 Describing Substances – Particles have internal structure

1.Representing types of substances

Distinguish mixtures from pure substances, elements from compounds, molecular compounds from ionic compounds, atoms from molecules based on the characteristics of each.
Recognize different types of substances in given particle diagrams.
State key ideas in Dalton’s atomic theory.
State the Law of definite composition and cite evidence to support that some pure substances are “compounded” of simpler particles in a definite ratio.
Apply Lavoisier’s law of mass conservation to determine percent mass composition of a compound from given mass data.
State Avogadro’s Hypothesis and use it to deduce the formulas of some compounds.

2.Periodic Table

Name elements from symbols and write symbols from names.
Recognize elements as metal, nonmetal, transition metal, and semimetals.
Recognize the family name for 4 groups: alkali metal, alkaline earth metal, halogens and noble gases.

Unit 5 “How Much” to “How Many” – Counting Particles Too Small to See

1.Relative mass, mole and molar mass

Determine relative masses of objects from experimental data and state the meaning.
Define one mole (using hydrogen, but know the modern definition by carbon-12).
Describe how molar mass of a substance is obtained from the relative mass (using hydrogen as reference).
Determine molar mass of a substance from the relative mass in the periodic table.
Relate Avogadro’s number to mole
Convert between mole, mass and number of particles of a given substance using factor labeling.

2.Empirical and Molecular Formulas

Determine the empirical formula of a substance from the given composition data.
Determine the molecular formula of a substance from the empirical formula and the given molar mass.

Unit 6 Internal structure of the atom

1.Atomic model

Describe a model of the atom that accounts for the fact that neutral particles can become either positively or negatively charged (Thomson’s plum pudding model).
Cite experimental evidence from J.J. Thomson’s experiments that supported his atomic model.

Apply the above atomic model to explain the observed interactions between the tapes, foil and paper in the Sticky Tape Lab.

2.Compounds

Cite observable evidence that distinguishes molecular compounds and ionic compounds.
Cite observable evidence for (+) charged metal ions and (-) charged nonmetal ions. Give atomic level explanations. (electrolysis of CuCl2 solution)
Differentiate atomic, molecular and ionic solids by their lattice structures. Relate the structures to their properties such as melting and boiling points.
Compare and contrast ionic and molecular compounds at atomic level and relate to their properties.
Write formulas of compounds from given names and name compounds from given formulas (a polyatomic ion chart will be provided).
Identify if a compound is molecular or ionic from its name or formula.

Unit 7 Representing Chemical Change – Chemical Reactions and Energy

1.Representing chemical reactions

Recognize that chemical changes involve rearranging atoms to form new substances.
Recognize that the total number of atoms does not change during a chemical reaction but the total number of molecules may. Give reasoning for both.
Balance a given reaction equation or write complete (including states of matter) balanced chemical equations from word descriptions of reactions.
Describe reactions both macroscopically (according to observations) and microscopically
Describe how a reaction proceeds at atomic level both in words and by particle diagrams. (electron transfer, spectator ion, molecules break down into atoms and recombine, etc.)
Cite observable evidence from lab experiments (nail lab) to support description of reaction process at atomic level.

2.Patterns of reactions

Describe characteristics of the five basic patterns in the way substances react and classify reactions based on these characteristics.
Predict reaction products for combustion, single and double replacement reactions.

3.Energy in chemical reactions

Recognize exo- or endothermic reactions based on observations.
Write the energy term on the correct side of the reaction equation and give reasoning.