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    • Resources >
      • Study Skills
      • Periodic Table
      • Common Ion Sheet
      • The Scientific Method
      • Doing Background Research
    • Introduction and Course Philosophy
    • Unit 1: Beginning Chemistry >
      • Lesson 1: The Atom >
        • What is an Atom?
        • The Structure of Atoms
        • The Periodic Table
        • Modeling Atoms
      • Lesson 2: Chemical Bonding >
        • Why Do Atoms Form Bonds?
        • Ionic Bonding
        • Covalent Bonding
        • Intermolecular Attraction
      • Lesson 3: Chemical Nomenclature >
        • Octet Rule
        • Ionic Compounds
        • Covalent Molecules
      • Lesson 4: Molecular Molecules >
        • Modeling Ionic Compounds
        • Modeling Covalent Molecules
      • Lesson 5: States of Matter >
        • States of Matter
        • Phase Changes
      • Lesson 6: Density >
        • What is Density?
        • Calculating Density
      • Lesson 7: Thermodynamics >
        • Temperature
        • Heat
        • Gas Laws
      • Lesson 8: Solution Chemistry >
        • Diffusion
        • Solutions and Molarity
        • Semi-Permeable Membranes
      • Lesson 9: Thermal Expansion >
        • Thermal Expansion
    • Unit 2: Earth Science >
      • Lesson 10: Earth at a Glance >
        • Perspective
        • Maps
      • Lesson 11: Layers of the Earth >
        • Layers of the Earth
      • Lesson 12: Plate Tectonics >
        • Plate Tectonics
      • Lesson 13: Rocks and Minerals >
        • Rocks and Minerals
      • Lesson 14: Particle Sorting >
        • Differentiation
        • Deposition of Sediment
      • Lesson 15: The Atmosphere >
        • Composition of the Atmosphere
        • Layers of the Atmosphere
        • Change Over Time
        • Atmospheric Disruption
    • Unit 3: The Cell >
      • Lesson 16: Life >
        • What is Life?
        • Structural Hierarchy of Living Things
      • Lesson 17: Biochemistry >
        • Intro to Biochemistry
        • Water
        • Micromolecules
        • Energy, Carbohydrates, Lipids
        • Protein and Nucleic Acid
      • Lesson 18: Cells >
        • What are Cells?
        • Microscopy
        • Plant and Animal Cells
      • Lesson 19: Membrane Transport >
        • A Special Environment
        • The Structure of Membranes
        • Membrane Transport
      • Lesson 20: Energy and Cell Respiration >
        • Energy in Biology
        • Energy Diagrams
        • Glycolysis and Anaerobic Respiration
        • Aerobic Cellular Respiration
      • Lesson 21: Photosynthesis >
        • Plants Get Energy From The Sun
        • Photosynthesis Process
        • Energy, Ecosystems, and the Environment
    • Unit 4: Anatomy and Physiology >
      • Lesson 22: The Human Body >
        • What Are Bodies Made Of?
        • What Do Bodies Do?
      • Lesson 23: The Nervous System >
        • The Nervous System
        • Neuronal Communication
        • The Central Nervous System
      • Lesson 24: The Endocrine System >
        • The Endocrine System
        • Hormones
        • Hormones, Puberty, and Reproduction
      • Lesson 25: The Integumentary System >
        • The Integumentary System
      • Lesson 26: The Musculoskeletal System >
        • The Skeletal System
        • The Muscular System
        • Anatomy Of The Musculoskeletal System
      • Lesson 27: The Cardiovascular System >
        • Blood and Blood Vessels
        • The Heart
      • Lesson 28: The Respiratory System >
        • The Respiratory System
      • Lesson 29: The Digestive System >
        • The Digestive System
        • Nutrition
      • Lesson 30: The Excretory System >
        • The Excretory System
      • Lesson 31: The Immune System >
        • Disease and Infection
        • Immunity
    • Units 5-6 Coming Soon
  • Workbench
    • Unit 1 >
      • EIS >
        • Lesson 1: Atoms
        • Lesson 2: Chemical Bonding
        • Lesson 3: Chemical Nomenclature
        • Lesson 4: Molecular Models
        • Lesson 5: States of Matter
        • Lesson 6: Density
        • Lesson 7: Thermodynamics
        • Lesson 8: Solution Chemistry
        • Lesson 9: Thermal Expansion
      • Unit 1: Project
      • Unit 1: Exam Review
      • Unit 1: Exam
    • Unit 2 >
      • EIS >
        • Lesson 10: Earth at a Glance
        • Lesson 11: Layers of the Earth
        • Lesson 12: Plate Tectonics
        • Lesson 13: Rocks and Minerals
        • Lesson 14: Particle Sorting
        • Lesson 15: The Atmosphere
      • Unit 2: Project
      • Unit 2: Exam Review
      • Unit 2: Exam
    • Unit 3 >
      • EIS >
        • Lesson 16: Life
        • Lesson 17: Biochemsitry
        • Lesson 18: Cells
        • Lesson 19: Membrane Transport
        • Lesson 20: Energy and Cell Respiration
        • Lesson 21: Photosynthesis
      • Unit 3: Project
      • Unit 3: Exam Review
      • Unit 3: Exam
    • Unit 4 >
      • EIS >
        • 22: The Human Body
        • 23: The Nervous System
        • 24: The Endocrine System
        • 25: The Integumentary System
        • 26: The Musculoskeletal System
        • 27: The Cardiovascular System
        • 28: The Respiratory System
        • 29: The Digestive System
        • 30: The Excretory System
        • 31: The Immune System
      • Unit 4 Project
      • Unit 4 Exam Review
      • Unit 4 Exam
    • Units 5-6 Coming Soon
  • Donate
  • Home
  • About Us
  • Classroom
    • Resources >
      • Study Skills
      • Periodic Table
      • Common Ion Sheet
      • The Scientific Method
      • Doing Background Research
    • Introduction and Course Philosophy
    • Unit 1: Beginning Chemistry >
      • Lesson 1: The Atom >
        • What is an Atom?
        • The Structure of Atoms
        • The Periodic Table
        • Modeling Atoms
      • Lesson 2: Chemical Bonding >
        • Why Do Atoms Form Bonds?
        • Ionic Bonding
        • Covalent Bonding
        • Intermolecular Attraction
      • Lesson 3: Chemical Nomenclature >
        • Octet Rule
        • Ionic Compounds
        • Covalent Molecules
      • Lesson 4: Molecular Molecules >
        • Modeling Ionic Compounds
        • Modeling Covalent Molecules
      • Lesson 5: States of Matter >
        • States of Matter
        • Phase Changes
      • Lesson 6: Density >
        • What is Density?
        • Calculating Density
      • Lesson 7: Thermodynamics >
        • Temperature
        • Heat
        • Gas Laws
      • Lesson 8: Solution Chemistry >
        • Diffusion
        • Solutions and Molarity
        • Semi-Permeable Membranes
      • Lesson 9: Thermal Expansion >
        • Thermal Expansion
    • Unit 2: Earth Science >
      • Lesson 10: Earth at a Glance >
        • Perspective
        • Maps
      • Lesson 11: Layers of the Earth >
        • Layers of the Earth
      • Lesson 12: Plate Tectonics >
        • Plate Tectonics
      • Lesson 13: Rocks and Minerals >
        • Rocks and Minerals
      • Lesson 14: Particle Sorting >
        • Differentiation
        • Deposition of Sediment
      • Lesson 15: The Atmosphere >
        • Composition of the Atmosphere
        • Layers of the Atmosphere
        • Change Over Time
        • Atmospheric Disruption
    • Unit 3: The Cell >
      • Lesson 16: Life >
        • What is Life?
        • Structural Hierarchy of Living Things
      • Lesson 17: Biochemistry >
        • Intro to Biochemistry
        • Water
        • Micromolecules
        • Energy, Carbohydrates, Lipids
        • Protein and Nucleic Acid
      • Lesson 18: Cells >
        • What are Cells?
        • Microscopy
        • Plant and Animal Cells
      • Lesson 19: Membrane Transport >
        • A Special Environment
        • The Structure of Membranes
        • Membrane Transport
      • Lesson 20: Energy and Cell Respiration >
        • Energy in Biology
        • Energy Diagrams
        • Glycolysis and Anaerobic Respiration
        • Aerobic Cellular Respiration
      • Lesson 21: Photosynthesis >
        • Plants Get Energy From The Sun
        • Photosynthesis Process
        • Energy, Ecosystems, and the Environment
    • Unit 4: Anatomy and Physiology >
      • Lesson 22: The Human Body >
        • What Are Bodies Made Of?
        • What Do Bodies Do?
      • Lesson 23: The Nervous System >
        • The Nervous System
        • Neuronal Communication
        • The Central Nervous System
      • Lesson 24: The Endocrine System >
        • The Endocrine System
        • Hormones
        • Hormones, Puberty, and Reproduction
      • Lesson 25: The Integumentary System >
        • The Integumentary System
      • Lesson 26: The Musculoskeletal System >
        • The Skeletal System
        • The Muscular System
        • Anatomy Of The Musculoskeletal System
      • Lesson 27: The Cardiovascular System >
        • Blood and Blood Vessels
        • The Heart
      • Lesson 28: The Respiratory System >
        • The Respiratory System
      • Lesson 29: The Digestive System >
        • The Digestive System
        • Nutrition
      • Lesson 30: The Excretory System >
        • The Excretory System
      • Lesson 31: The Immune System >
        • Disease and Infection
        • Immunity
    • Units 5-6 Coming Soon
  • Workbench
    • Unit 1 >
      • EIS >
        • Lesson 1: Atoms
        • Lesson 2: Chemical Bonding
        • Lesson 3: Chemical Nomenclature
        • Lesson 4: Molecular Models
        • Lesson 5: States of Matter
        • Lesson 6: Density
        • Lesson 7: Thermodynamics
        • Lesson 8: Solution Chemistry
        • Lesson 9: Thermal Expansion
      • Unit 1: Project
      • Unit 1: Exam Review
      • Unit 1: Exam
    • Unit 2 >
      • EIS >
        • Lesson 10: Earth at a Glance
        • Lesson 11: Layers of the Earth
        • Lesson 12: Plate Tectonics
        • Lesson 13: Rocks and Minerals
        • Lesson 14: Particle Sorting
        • Lesson 15: The Atmosphere
      • Unit 2: Project
      • Unit 2: Exam Review
      • Unit 2: Exam
    • Unit 3 >
      • EIS >
        • Lesson 16: Life
        • Lesson 17: Biochemsitry
        • Lesson 18: Cells
        • Lesson 19: Membrane Transport
        • Lesson 20: Energy and Cell Respiration
        • Lesson 21: Photosynthesis
      • Unit 3: Project
      • Unit 3: Exam Review
      • Unit 3: Exam
    • Unit 4 >
      • EIS >
        • 22: The Human Body
        • 23: The Nervous System
        • 24: The Endocrine System
        • 25: The Integumentary System
        • 26: The Musculoskeletal System
        • 27: The Cardiovascular System
        • 28: The Respiratory System
        • 29: The Digestive System
        • 30: The Excretory System
        • 31: The Immune System
      • Unit 4 Project
      • Unit 4 Exam Review
      • Unit 4 Exam
    • Units 5-6 Coming Soon
  • Donate

Unit 1: Chemistry Exam Review

How to Study For and Exam

If you've never had to really study for an exam before, it can sometimes feel like a little bit of a daunting process. It's still your responsibility to learn, but, hopefully, you've already done most of the initial learning! The next step—the one you should be taking now—is to practice your recall by making sure you understand the most important ideas listed below. This video will also give you some suggestions on how to prepare for an exam:

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Most Important

  • Know the different ways that atoms and molecules are modeled, especially the Bohr model and Lewis structures.
  • Know how to use the Periodic Table.
  • Understand the basic principles of chemical bonding.
  • Understand that molecules are in constant motion, that this results in collisions and interactions, and that molecules move faster at higher temperatures.
  • Understand the behaviors of solids, liquids, and gases, including how this relates to density and intermolecular interactions.
    • Topics relevant to solids: Thermal Expansion
    • Topics relevant to liquids: Diffusion and Osmosis
    • Topics relevant to gases: Gas Laws
    • Topics relevant to all 3: Intermolecular Interactions and Density

Atoms

You should know how to:
  • Find the number of protons, neutrons, and electrons in an element, based off of the information in the Periodic Table.
  • Write an atomic symbol, based off of the information in the Periodic Table.
  • Draw a Bohr model, based off of the information in the Periodic Table.

You should understand:
  • What atoms are, what matter is, and how they are related.
  • That atoms are made up of protons, neutrons, and electrons, which have these traits:
    • ​​Protons: Positively charged, located in the nucleus, have a mass of about 1 amu, and change the atom so much that it becomes a new element.
    • Neutrons: Not charged, located in the nucleus, have a mass of about 1 amu, and change the radioactive stability of an atom (its isotope)
    • Electrons: Negatively charged, orbit the nucleus, have negligible mass, and changes the chemical reactivity of the atom
  • That our best model of the atom is more advanced than the one we use most in this class (the Bohr model), and that models can get replaced over time as scientific understanding becomes more advanced.
    • Other models are the Plum Pudding Model (which was debunked and replaced by the Bohr model) and the Electron Cloud Model (which is our current best model)
  • Where to find an element's atomic name, atomic symbol, atomic number, and atomic mass on the Periodic Table, and how atomic number and atomic mass​ relate to the number of protons, neutrons, and electrons.

Chemical Bonding

You should know how to:
  • Determine how many valence electrons an atom/ion has, based off of the information in the Periodic Table.
  • Determine the charge on a cation or an anion, based off of the information in the Periodic Table and your Polyatomic Ion sheet, and figure out how many of each ion will bond in an ionic bond so that the charges add up to zero.
  • Determine whether two elements will form an ionic bond or a covalent bond.

You should understand:
  • That atoms must collide (bump together) in order to form chemical bonds.
  • That atoms will continue to react until they become most stable.
  • How the concept of stability, the octet rule, and the number of valence electrons relate to one another.
  • That all of the atoms you will be working with (except hydrogen and helium) follow the octet rule. This means that they "want" to have 8 electrons in their valence shell. Hydrogen and helium want 2. (The always-true rule is that atoms “want” to look like noble gases).
  • That ionic bonds involve a positively-charged metal cation donating electrons to a negatively-charged nonmetal anion, which are then held together by electrostatic forces, or “opposites attract.”
  • That atoms share electrons in a covalent bond, due to wave overlap of electron orbitals.
  • That covalent bonds form between two nonmetals.
  • That electronegative elements will pull electron density toward them and out of a bond, making that portion of the molecule relatively more negative.
  • The relative strengths of ionic bonds, hydrogen bonding, dipole-dipole interactions, and London dispersion forces, and how this relates to whether a charge/dipole is permanent, temporary, complete, or partial.
  • Which forces are most commonly found in solids, liquids, and gasses, and how that relates to the strength of the interaction. 

Chemical Nomenclature

You should know how to:
  • Write the long-form name of an ionic compound, if you’re given the chemical formula.
  • Write the chemical formula of an ionic compound, if you’re given the formula. This requires you to be able to find the charge of the component ions and figure out how many of each ion is needed to make the total charge add up to zero.
  • Do both of these things for ionic compounds involving a polyatomic ion. You will be allowed to use your Polyatomic Ion sheet on the exam.
  • Write the long-form name of a covalent molecule, given the molecular formula. This requires you to know the standard greek prefixes for numbers.
  • Write the molecular formula of a covalent molecule, given the long-form name.

You should memorize:
  • The chemical formulas for the common elements water, ammonia, methane, and ozone.
  • Which elements are only found in nature as diatomic elements.

You should understand:
  • The concepts covered in “Chemical Bonding.”

Molecular Models

You should know how to:
  • Draw Lewis dot structures for single atoms/ions.
  • Model ionic compounds using Lewis dot structures, by showing how valence electrons get transferred and how the resulting charged ions are held together by electrostatic interactions.
  • How to draw Lewis dot structures for covalently bonded molecules, with single bonds, double bonds, and triple bonds.

You should understand:
  • The concepts covered in “Chemical Bonding.”

States of Matter

You should memorise:
  • The names of the phase changes between solids, liquids, and gases:
    • Solid to liquid: melting, or fusion
    • Liquid to gas: vaporization, or boiling
    • Gas to liquid: condensation
    • Liquid to solid: freezing

You should understand:
  • That molecules are closest together and bound by the strongest intermolecular forces in solids. Solids have definite shape and volume.
  • That molecules are medium-close together and bound by medium-strong intermolecular forces in liquids. Liquids have definite volume, but not shape.
  • That molecules are far apart and bound by weak or no intermolecular forces in gases. Gases have neither definite volume nor shape.
  • That substances can transition between solid, liquid, and gas depending on external factors, especially temperature and pressure. Higher temperature means more movement and more gas-like properties, and more pressure means less space between molecules and more solid-like properties.
  • The concept of heat and how it relates to kinetic energy of molecules.
  • How adding heat relates to phase changes: as particles move more, they can “escape” their intermolecular interactions and go from solid to liquid to gas.
  • How we graph heat changes: as we add heat, solids get warmer; then, all the energy goes into melting them into liquids, so the temperature doesn’t change; then liquids get warmer; then, all the energy goes into boiling the liquid, so the temperature doesn’t change; then, gases get warmer.

Density

You should know how to:
  • Calculate density from a known mass and volume.
  • Identify an unknown material by calculating density and comparing it to a list of known densities.

You should memorize:
  • The formula for calculating density, d = m/v.

You should understand:
  • The basic definition of density, which is the amount of mass (weight) we can fit into a certain volume. Molecules are more crowded in more dense objects. Molecules are less crowded in less dense objects.
  • How the concept of density relates to whether something will sink or float.
  • How the density of solids, liquids, and gases relate to each other both as a general rule and in the exception case, water.
  • That density is a physical property of matter, meaning it does not change based on the amount of a substance that we have, and will be constant for the same material (e.g., aluminum will always have a certain density, gold will always have a certain density, etc.)

Thermodynamics

You should know how to:
  • Identify whether a reaction is exothermic, endothermic, or isothermic, depending on the change in temperature of the system and surroundings.

You should understand:
  • That molecules are in constant motion.
  • How temperature relates to the kinetic energy of molecules.
  • The difference between heat (the transfer of energy) and temperature (average kinetic energy)
  • How gases behave in perfectly flexible containers:
    • As we add more gas to a container, the volume will go up
    • As we increase the temperature of the gas, the volume will go up
  • How gases behave in perfectly rigid containers:
    • As we add more gas to a container, the pressure will go up
    • As we increase the temperature of a gas, the pressure will go up

Solubility and Diffusion

You should know how to:
  • Determine the direction of movement of solutes or water across a semipermeable membrane in a U-tube, both when solutes are allowed across and when they aren’t.

You should understand:
  • That, in the process of diffusion, molecules naturally move down their concentration gradients from areas of high concentration to low concentration, until they reach equilibrium, which is a state of balance where there is no net change.
  • How the speed of diffusion changes based on how much molecules are moving (such as when the temperature increases)
  • What diffusion and osmosis are, how they are the same, how they are different, and why osmosis would occur instead of diffusion.
  • The direction of water movement during osmosis and how this relates to solute concentration.

Thermal Expansion

You should understand:
  • That solids, liquids, and gases all expand when heated and contract when cooled.
  • The importance of expansion gaps and expansion joints in engineering.
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