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Science Final
Friday, June 10, 2016
The following is a guide to important terms & concepts discussed in Chemistry. There may be
things not specifically stated that are on the final. You need to review all past quizzes and
tests. Many questions will be pulled from those assessments.
How to study?
Review all past quizzes and tests (some ?’s will come directly from here).
Reread all your notes.
Familiarize yourself with all terms and concepts on the review guide.
Use the text as a resource for any material that is not understood.
Unit 1 Elements, Compounds, and Mixtures - Chapter 4
Define and give examples and properties of an element, compound, and mixture.
Properties- Metal, Non-metal, Malleable, Ductile, Reactivity
Symbol = Element
Formula = Compound
Ex: Element – Sodium
Symbol – Na
Physical - Malleable, Soft, Silvery Metal
Chemical – Highly reactive with water
What is a pure substance? Examples
Mixtures - Explain similarities and differences of solutions, suspensions, and colloids.
For example: Does it settle? Scatter light? Can it be filtered?
Mayo is a _________ Salt water is a _________Italian Salad Dressing is a ___________
Solutions- Dilute vs. Concentrated (Saturated)
Components - Solvent and solute
Know the factors that affect the rate of a solution.
Explain an isotope (C-12 compared with C-13)
Physical vs. Chemical Changes- Define and give examples of each.
Unit 2 Atoms Chapter 11
Parts of an atom - This includes location, charge, and relative mass
What does A.M.U. mean? This was developed based on?????
Greek word for atom is……………… meaning………………….
Proton, Neutron, & Electron – Must know mass, location, and charge of each.
Ex: Nucleus – center of the atom
Proton – found in the nucleus, positive charge, 1 AMU
Electron – found outside the nucleus, negative charge, 1/1600 AMU
Be able to briefly explain or identify the contributions of the following scientists to the atomic
theory: Democritus, Dalton, Thomson, Rutherford, Bohr and the Electron Cloud.
Be able to explain the difference between mass number and atomic mass
Unit 3 Periodic Table Chapter 12
Who developed the first table? How was it organized?
Identify how the modern table is organized and what information it contains
Ex: symbols, atomic number, atomic mass, group and………..
Describe the difference between a group and a row?
Know characteristics of metals, non-metals and metalloids
Label each group and know the main properties of each
For example: alkaline metals- highly reactive, never found uncombined, one valence
Solve atomic trivia
Where are the lanthanides and actinides placed? Why?
Unit 4 Chemical Reactions Chapter 14
What are the clues a chemical reaction may be taking place?
Define Chemical Reaction
Compare a chemical symbol, formula and chemical equation
Know the parts of a chemical equation
Be able to balance chemical equations
Law of Conservation of Mass
Explain the difference between a subscript and coefficient.
Describe the four types of chemical reactions
Synthesis, Decomposition, Single Replacement………………..
Identify and write examples of each
Exothermic and Endothermic reactions
Describe the factors that affect the rate of a reaction (temperature, surface area, etc.)
Explain activation energy with examples
How do a catalyst and inhibitor affect chemical reactions
Additional science vocabulary and concepts Chemical Compounds
What is a chemical bond?
What are valence electrons?
Be able to explain the OCTET RULE.
Safety Rules - What should you do several times before beginning a lab or activity?
Read the directions
Basic Metric Measurements
What is Length? Mass? Volume? Density? Temperature?
What is the measurement tool and basic unit of measure for each of the above?
For example - Length is measured with a ruler and the basic unit is the meter.
For example
Law vs. Theory
Scientific method
Labs and Demonstrations
Instant HOT/COLD Pack
Elephant’s Toothpaste
Solar Bag
*** There will be a few questions from the HEAT Unit (Chapter 10). Please review the study
guide online.