Chemistry
Semester 1 Exam Study Guide
Exam Details:
 ~ 50% Multiple Choice, ~ 50% Short Answer
 Total of ~ 80 points
 Bring your calculator, pencil and eraser
 You will be given a periodic table and polyatomic ions list
Studying Tips:
1. Know what you are being tested on – collect all the material you’ve received during the term and use it
when studying. This includes quizzes, tests, assignments, homework questions, worksheets and notes.
2. Study in the best place for you – choose a quiet place where you won’t be distracted and turn off your phone,
computer and TV.
3. Take a break and have a snack – study for short periods of time and take frequent breaks (study for 20 min.,
take a 10 min. break).
4. Start studying early and often, then you won't be in a hurry and cramming the night before.
5. Redo questions from the homework, quizzes, assignments and tests – test yourself by answering questions
from previous work and then correcting it. Can you answer the questions without looking up the answers?
6. Memorize, memorize, memorize – if you don’t know the vocabulary or key concepts, you won’t be able to
discuss the material.
These are your Objectives. They are the topics that your exam will test you on. When making your study notes and
while studying, be sure to cover these topics fully and be able to describe each one in detail.
Unit 1 Introduction to Chemistry and Scientific Measurement
Ch. 1 and 3
1. Understand what the study of chemistry entails and the importance of it.
2. Explain how pure chemistry and applied chemistry are related.
3. Discuss the impact that chemists have on the world today.
4. Describe how Lavoisier helped to transform chemistry.
5. Identify and demonstrate the steps and methods that scientists often use to solve problems.
6. State the differences between a scientific theory and a scientific law and provide examples.
7. Discuss the roles of collaboration and communication in the scientific community.
8. Demonstrate use of scientific notation and explain why it is useful.
9. Understand the importance of accuracy and precision.
10. Identify the source and the amount of uncertainty in measurements by calculating percent error.
11. Understand the importance of, and how to determine, significant figures in measurements and calculations.
12. Name the prefixes used in SI, what multiple of ten each represents, and the symbols for length, volume, mass,
time, temperature, amount of substance, and energy and convert measurements among related SI units, using
dimensional analysis.
13. Perform calculations involving density and explain why a change in temperature affects a substance’s density.
Matter
Chemistry
Pure chemistry
Applied chemistry
Technology
Scientific method
Observation
Hypothesis
Experiment
Manipulated/independent variable
Responding/dependent variable
Theory
Scientific law
Measurement
Scientific Notation
Accepted Value
Experimental Value
Percent Error
Significant Figures
International System of Units (SI)
Absolute Zero
Unit 2: Matter and Atomic Theory
Ch. 2 Matter and Change, Ch. 4 Atomic Structure, Ch. 5 Electrons in Atoms
1.
Classify matter according to its composition and distinguish among elements, compounds, homogeneous
mixtures, and heterogeneous mixtures.
2.
Distinguish among the three main states of matter.
3.
Classify changes and properties as physical or chemical.
4.
Describe how to recognize a chemical change.
5.
Explain how Democritus described atoms and explain Dalton’s Atomic Theory.
6.
Describe subatomic and subnuclear particles and the overall structure of an atom.
7.
Understand and use atomic numbers and mass numbers to distinguish elements.
8.
Explain the role of isotopes in determining the atomic mass of an element and calculate average atomic mass.
9.
Describe the Bohr atomic model and the role of electron energy levels, which lead to the current quantum
mechanical model.
Substance
Physical property
Solid
Liquid
Gas
Vapor
Mixture
Heterogeneous mixture
Homogeneous mixture
Solution
Phase
Element
Compound
Chemical change
Chemical property
Chemical reaction
Reactant
Product
Precipitate
Atom
Atomic Theory
Electrons
Protons
Neutrons
Quarks
Nucleus
Atomic number
Mass number
Isotopes
Atomic mass unit
(AMU)
Energy levels
Quantum mechanical
model
Electron cloud
Unit 3: The Periodic Table
Chapters 4 – Atomic Structure and 6 – The Periodic Table
1. Describe early attempts at classifying elements, including Mendeleev’s periodic table of the elements.
2. State the periodic law.
3. Identify and state the properties, including physical state, of metals, metalloids, and non-metals.
4. Distinguish between the terms groups or families and periods.
5. Relate the position of any main group element in the periodic table to its number of valence electrons and
predict its relative properties.
6. Define the term ion and state ions formed by elements in groups 1, 2, 13, 14, 15, 16, and 17.
7. Define cation and anion.
8. Explain the periodic trends in atomic radius, ionization energy, ionic size, and electronegativity.
Periodic table
Period
Group/family
Periodic law
Metals
Luster
Nonmetals
Metalloids
Electron Configuration
Atomic radius
Shielding effect
Cation
Anion
Ionization energy
Electronegativity
Unit 4: Chemical Bonding
Chapter 7 – Ionic and Metallic Bonding, Chapter 8 – Covalent Bonding, Chapter 9 – Chemical Names and
Formulas
1. Determine the number of valence electrons in an atom by its position in the periodic table.
2. Determine ionic charges based on relative ionization values and the octet rule.
3. Predict ionic bonds between atoms and the properties of those compounds formed.
4. Describe metallic bonds, how they lead to the formation of alloys, and the importance of alloys.
5. Predict covalent bonds between atoms and the properties of those compounds formed.
6. Explain and determine single, double, and triple bonds.
7. Identify the relative polarity of bonds based on electronegativity values.
8. Explain and predict hydrogen bonds.
9. Deduce the formula and state the name of binary ionic compounds.
10. Deduce the formula and state the name of ionic compounds with polyatomic ions.
11. Deduce the formula and state the name of binary covalent compounds.
Valence electron
Electron Dot Structure
Octet rule
Ionic compounds
Ionic bonds
Metallic bonds
Alloys
Covalent bond
Molecule
Single covalent bond
Unshared pair
Double covalent bond
Triple covalent bond
Polyatomic ion
Nonpolar covalent bond
Polar covalent bond
Polar bond
Polar molecule
Dipole
Hydrogen bonds
Polyatomic ion
Binary compound
Unit 5: Chemical Quantities and Reactions
Chapter 10 – Chemical Quantities, Chapter 11 – Chemical Reactions, Ch. 12 Stoichiometry
1.
Demonstrate the three methods for measuring the amount of a substance – count, mass, and volume.
2.
Understand the concept of a mole and what it represents.
3.
Convert between the mass of a substance, the number of moles that mass contains, and the number of
particles in that mass.
4.
Calculate the volume of a gas at STP.
5.
Demonstrate how chemical equations describe chemical reactions.
6.
Illustrate how to balance chemical reactions by changing coefficients.
7.
State and describe the five general types of reactions.
8.
Given the equation of a reaction, classify the reaction as one of the general types.
9.
Interpret balanced chemical equations and understand all the information present in them.
10. Perform mole-mole, mass-mass, mass-particles, volume-volume, and other stoichiometry calculations.
11. Determine the amount of product produced in a chemical reaction when taking into consideration a limiting
reagent.
12. Determine the percent yield of a chemical reaction.
Mole (noun)
Mol (unit)
Avogadro’s Number
Molar Mass (g/mol)
STP
Molar Volume (22.4L/mol)
Reactants
Products
Word equation
Chemical Equation
Coefficient
Combination / Synthesis Reaction
Decomposition Reaction
Single-replacement / displacement Reaction
Activity Series
Double-replacement / displacement Reaction
Combustion Reaction
Mole Ratio
Limiting Reagent
Excess Reagent
Theoretical Yield
Actual Yield
Percent Yield