Name ______Answer Key______Period ______Date ______

Physical Science –2nd Semester – Final Exam Study Guide – (2012-2013)

  1. Physical Science Basics
  2. What tool(s) would you want to use to find the:
  3. Mass of an object? ______Triple Beam Balance______Basic SI Unit? _____g____
  4. Volume of an object? ______Graduated Cylinder or Ruler______Basic SI Unit? __L –or- cm³_
  5. Length of an object? ______Ruler or Meterstick______Basic SI Unit? ____m_____
  6. Density of an object? ______Triple Beam Balance & Ruler______Basic SI Unit?_g/L –or- g/cm³
  7. What is the formula for calculating density? ______Density = mass / volume or D=m/v______
  8. What is the density of a cube that is 15 g and has a volume of 3 cm3? __15g / 3cm³ = 5 g/cm³_____
  9. Compare the density of solid H2O to liquid H2O, and explain what observable effect this has.
    Solid water has a lower density than liquid water, and so solid water (ice) floats in liquid water!
  10. Chemistry Basics
  11. Element (def.) The building block of all matter; made up of only one type of atom
  12. Atom (def.) The smallest part of an element that still has the properties of that element
  13. Compound (def.) A substance made up of two or more DIFFERENT atoms bonded together
  14. Molecule (def.) A substance made up of two or more atoms bonded together
  15. Model of the Atom: Evolution of the Atomic Theory

Atoms are so small that many scientists throughout history have created _____models______to describe them.

Why have atomic theories changed over time? _____The advancement of new technologies______

Scientist / Year / Major Discovery/Contribution / Name of atomic model
John Dalton / (1) / The Atomic Theory: Provided evidence that atoms were the smallest thing in the universe; atoms of the same element were the same, while atoms of different elements were different / Billiard Ball Model
J.J. Thomson / (2) / Cathode Ray Gun:
Discovered the electron / Plum Pudding Model
Niels Bohr / (4) / Discovered that elements gave off light energy when electrons jumped from orbital to orbital / Bohr Model
Ernest Rutherford / (3) / Gold Foil Experiment: Discovered the dense, positively charged nucleus surrounded by empty space / Planetary Model
  1. Periodic Table
  2. The current periodic table is arranged by increasing ______Atomic Number______.
  3. Reading the Periodic Table
  4. An element’s ___Physical and chemical properties____ can be predicted from its location in the periodic table.
  5. The atomic number represents the number of ___protons____.
  6. The atomic mass represents the number of _____protons and neutrons in the nucleus____.
  7. The atomic symbol represents ____the name of the element______.
  8. The group/family number represents ____the number of valence electrons______.
  9. The row/period number represents _____the number of orbitals____.
  10. This group contains the most elements: ___Transition Metals____.
  11. MatchingWord Bank: Metalloid, transition element, metal, non-metal, group 18- noble gases, group, group 1

The most stable elements are found here. They are colorless tasteless gases that glow when an electrical current passes through them. / Group 18 – Noble Gases
Elements that share some properties with metals, and some with non-metals. / Metalloids
Column of elements in the periodic table that have similar physical or chemical properties. / Group
The most reactive elements in the periodic table, and are soft enough to be cut with a knife. / Group 1 – Alkali Metals
An element that has a shiny luster, is a good conductor of heat and electricity, is malleable and ductile. / Metal
Elements in groups 3-12 / Transition Metal
Element that is usually a gas or brittle, solid at room temperature, and does not conduct heat and electricity well. / Non-metal
  1. Parts of an Atom

Subatomic Particle / Charge / Location in the atom
Proton / Positive / Nucleus
Electron / Negative / Electron Cloud/Orbital
Neutron / Neutral / Nucleus
Nucleus / Positive / Center of Atom
The atom shows to the left has __7__ valence electrons.
This atom has __7__ electrons that would be involved in bonding.

Krypton is located in group 18. It has __8__valence electrons, which is the most that any element can have.
Krypton’s atomic number is 36 and its atomic mass is 84. It has _36_ protons, _48_ neutrons, and _36_ electrons.

  1. Properties of Atoms Gaining or Losing Electrons
  2. An atom that has gained or lost an electron is called a(n) ___ion____
  3. Group (# and name) ___Group 1 – Alkali Metals____ loses electrons most easily.
  4. Group (# and name) ___Group 17 - Halogens___ gains electrons most easily.
  5. Elements in group 17 want to bond with elements in group _1 (Alkali Metals)_
  6. Elements in group 16 want to bond with elements in group _2 (Alkaline Earth Metals)_
  7. The charge becomes positive when what has happened? _atoms lose electrons_
  8. What do we call a positively charged ion? _cation_
  9. The charge becomes negative when what has happened? _an atom gains electron_
  10. What do we call a negatively charged ion? _anion_
  11. An ionic bond is an attraction between what charges? _Oppositely charged ions_
  12. DNA
  13. TRUE / False. All things, living and non-living are made up of atoms.
  14. Macromolecule (def.) _A large molecule made up of thousands of atoms_
  15. List the 5 elements that make up the DNA macromolecule: *REMEMBER TO “CHONP” 

1). _Carbon_; 2). _Hydrogen_; 3). _Oxygen_; 4). _Nitrogen_; 5). _Phosphorous_

  1. Chemical Bonding
  2. Ionic bond
  3. Metal/non-metal and metal/non-metal bonded together
  4. Protons/neutrons/electrons are shared/transferred
  5. Draw how Aluminum and Oxygen would ionically bond (using arrows).
  6. Covalent bond
  7. Metal/non-metal and metal/non-metal bonded together
  8. Protons/neutrons/electrons are shared/transferred
  9. Draw the structural and Lewis structure for Carbon tetrachloride.
  10. Classify the following compounds as ionic or covalent, then name them accordingly:
  11. KCl _Ionic_ _Potassium chloride__
  12. CO2_Covalent_ _Carbon dioxide_
  13. CaF2 _Ionic__ _Calcium fluoride_
  14. P2O5_Covalent_ _Diphosphorous pentoxide_
  1. Naming Chemical Formulas
  2. H2O is the molecular formula for _water_. The 2 means _2 atoms of hydrogen__; no number after the O indicates _there is only one atom of oxygen_.
  3. The molecular formula for oxygen gas is O2_.
  4. Oxygen is a diatomic molecule because _it is made up of 2 atoms_.
  5. C6H12O6 is the chemical formula for _sugar_.
  6. The chemical formula for methane is _CH4_.
  1. Physical and Chemical Properties and Changes
  2. Identify the following as either being a physical property or a chemical property:
  3. Flammability _Chemical property (Irreversible; DEF: the ability for something to catch on fire)_
  4. Melting point _Physical property (Reversible; DEF: the point at which something melts)_
  5. Color _Physical property (observe with the senses)_
  6. Name a property that would describe salt. _Small, white, crystalline, salty_; Name a property that would identify salt. _salty taste_
  7. A chemical/ physical change occurs when bonds are broken.
  8. A chemical / physical change occurs when no new substance is formed.
  9. Physical change (def.) _Occurs when one or more physical properties of a substance are changed, is reversible_
  10. Name 3 examples of a physical change:
  11. _melting_ 2. _dissolving_ 3. _boiling_
  12. Chemical change (def.) _An irreversible change that occurs when chemical bonds break and new bonds form, producing a new substance with new properties_
  13. Name examples of a chemical change:
  14. _Change in color_2. _Change in odor_3. _Production of light_ 4._Emission of a gas_

5. _Formation of precipitate_ 6. _Release energy (Exothermic)_ 7. _Absorb energy (Endothermic)_

  1. Name 3 signs that a chemical change has occurred:
  2. _Burning_2. _Cooking_3. _Rusting_
  1. Balancing Chemical Equations
  2. _2_ H2 + ____ O2  _2_ H2O
  3. How does the Law of Conservation of Mass apply to the equation you balanced above? _Atoms are not created or destroyed in the reaction. You must have the same number of atoms in the beginning of the reaction as you do in the final product._
  4. What forms of energy could be transferred in a chemical reaction? _Radiant (Light)__Heat__(All others) _
  5. A change that gives off energy is called _Exothermic (think “EXit”)_ Ex. _Fireworks exploding_
  6. A change that absorbs energy is called _Endothermic (think “ENter”)_ Ex. _Baking cookies_
  7. True / False. Every chemical reaction involves a change in energy.
  1. Mixtures
  2. Heterogeneous (def.) _A mixture that is unevenly mixed; can see the different parts of the mixture_
  3. Name an example of a heterogeneous mixture: _Salad, concrete, M&M’s_
  4. Homogeneous (def.) _A mixture that is evenly mixed; looks like the same substance_
  5. Name an example of a homogeneous mixture: _Kool-Aid, Salt-water_
  6. Separating Mixtures: Name & give a brief description of the 5physical methods to separatemixtures:
  1. Magnetism _Separates objects with magnetic properties (those with Fe, Ni, Co)_
  2. Filtration _Separates substances based on size_
  3. Dissolving _Breaks down a substance and surrounds it_
  4. Evaporation _Separates dissolved solute from a solution (Anything from water!)_
  5. Chromatography _Separates different colored pigments and dyes based on filtration_
  6. Solutions
  7. Solute (def.) _The substance found in the lesser amount; the substance that IS dissolved_
  8. Solvent (def.) _The substance found in the greater amount; substance thatDOES the dissolving_
  9. Solubility (def.) _The ability for a substance to be dissolved_
  10. In Kool-Aid, identify the solute _Kool-Aid Powder_ and the solvent _Water_
  11. True / False. Typically there is more solute than solvent in a solution.
  12. True / False. Solutes and solvents can be solids, liquids, or gases.
  13. True / False. When a salt dissolves in water, each of its particles is surrounded by water molecules. This is why the freezing point of salt water is lower than the freezing point of fresh water.
  1. Acids and Bases
  2. Acidic solutionspH levels from _0_ to _6_; Taste _Sour_; Ex. _Lemon juice_
  3. What can a substance do if it has a warning of “corrosive”? _It can eat away at other materials_
  4. Basic solutionspH levels from _8_ to _14_; Taste _Bitter_; Ex. _Shampoo, soap, other cleaning supplies_
  5. Phase Changes
  6. The three main states of matter are: _Solid_ _Liquid_ _Gas_
  7. Draw the molecular arrangement of each:
  1. Label the Phase Change Diagram. Use arrows where necessary (phase transitions).

Solid (A) Liquid (C)

Gas(E) Solid and Liquid(B)

Liquid and Gas(D)Freezing (B)

Melting(B) Evaporating(D)

Condensing(D)

  1. The average kinetic energy of the particles of a substance going through a phase transition can be described as (circle all that apply): increasing / decreasing / staying the same.
  2. Compare the amount of kinetic energy (motion) of the particles in a solid to a gas._Atoms of a gas have more kinetic energy than the atoms in a solid_
  1. Types of Energy
  2. Energy (def.) _The ability to do work or to cause change_
  3. What does it mean if something has potential energy? _Energy is stored in an object_
  4. Example: _A stretched rubber band, a roller coaster on top of a hill_
  5. When does an object possess kinetic energy? _An object in motion_
  6. Example: _A roller coaster moving down a hill_
  7. Chemical PE (def.) _Energy stored in chemical bonds, that can only be released during a chemical reaction_
  8. Example: _Fossil fuels (natural gas, coal, oil), food, batteries_
  1. Energy Transformations
  2. The law of conservation of energy states that when one form of energy is converted into another, _energy cannot be created or destroyed_
  3. True / False. Most forms of energy cannot be converted into other forms.
  4. Natural gas (_Chemical_ energy) heats(_Thermal_ energy) water.
  5. Batteries (_Chemical_ energy) are used to turn on a flashlight (_Radiant (light)_ energy).
  6. You rub your hands together (_Mechanical_energy) on a cold day and friction is created to produce heat (_Thermal_ energy).
  7. A microwave(_Radiant_ energy) in a house turns on because of energy produced in a nuclear power plantfrom an atom’s nucleus (_Nuclear_ energy)?
  8. Alight bulb [visible light](_Radiant_ energy) turns on because of turning on the light switch (_Mechanical_ energy)?
  9. Fossil fuels (_Chemical_ energy)are burned, which is called combustion, and heat (_Thermal_energy) is released.
  10. A spinning turbine (_Mechanical_energy) produces usable energy to power homes (_Electrical_ energy).
  1. Sources of Energy
  2. Identify the following as being renewable or non-renewable:

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  1. Biomass _ Renewable_
  2. Coal _Non-Renewable_
  3. Petroleum _Non-Renewable_
  4. Wind _ Renewable_
  5. Solar _ Renewable_
  6. Nuclear_Non-Renewable_
  7. Hydroelectric _ Renewable_
  8. Geothermal _Renewable_

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  1. What part of the water cycle would not be possible without solar energy? _The Sun_
  2. Nuclear Energy
  3. Energy stored in _the nucleus of an atom_
  4. Nuclear Fission (def.) _When two or more smaller atoms fuse together_
  5. Nuclear Fusion (def.) _When a large atom splits into two or more atoms_
  6. True / False. Fusion releases 3-4 times more energy than fission.
  7. True / False. Only nuclear energy is produced in a nuclear reaction, not light or heat.
  1. Heat Transfer
  2. Conduction (def.) the transfer of heat energy between substances that are touching
  3. Example: molecule to molecule
  4. Convection (def.) the cyclical motion of molecules in a gas or liquid caused by the transfer of heat through a surface
  5. Example: Hot Air Balloon
  6. Radiation (def.) Electromagnetic waves travel through space and transfer heat energy.
  7. Example: Microwave
  8. Temperature (def.) The measure of the amount of kinetic energy in a substance.
  9. The scale to measure the amount of KE in the atoms of a substance: Celsius
  10. Heat (def.) is the transfer of energy from an object with high molecular K.E., to an object with low molecular K.E.
  11. Heat moves from a hotter object to a coolerobject.
  12. Insulator (def.)A substance that prevents or slows the flow of heat energy.
  13. Example: Rubber
  14. Conductor (def.) substances that allow electrons to move freely across the surface of their atoms
  15. Example: _Metals_
  1. Electricity
  2. Static Electricity (def.) _The build-up of charges on an object._
  3. Static Discharge (def.) _Spark or shock; the loss of static electricity as electric charges move off an object in an attempt to become neutrally charged._
  4. A _switch_turns a circuit on and off by opening or closing.
  5. _Series_ circuits have one path, while _parallel_ circuits have more than one path.
  6. Circuits A C are _Series_
  7. Circuits B E are_Parallel_
  8. Electric currents always flow from the:
    Negative to Positive
  9. In a series circuit: finish the saying

“when one light bulb goes out…

they’ll all go out.”

  1. In a series circuit: Adding another bulb will _add resistance and make the lights dimmer_
  2. True / False. In a parallel circuit, the current from each bulb has its own path.
  3. An electric current will always follow the path _of least resistance_.
  1. Magnetism
  2. Magnetism (def.) the force of attraction or repulsion of magnetic material.
  3. Magnetism in a physical / chemical property.
  4. Poles that attract are _opposite_; Poles that repel are _similar_
  5. The region around the magnet is known as the magnetic field. The closer these lines are together, the stronger the magnetic field.
  6. True / False. A magnet is capable of producing an electric current.

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