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Semester 1 Physical Science Exam review This is not an assignment, it is a review of the vocabulary, concepts, and sample questions for the exam. I suggest that you split it into parts and use them to study for the exam. Vocabulary Chapter 1 Scientific Method Scientific method Observation Question Hypothesis Experiment Results Conclusion Variable Control Control group Controlled experiment Independent variable Dependent variable Metric system Prefix Deka Kilo Mega Giga Deci Centi Milli Micro Nano Scientific notation Dimensional Analysis\ Conversion factor Ch. 3 States of matter Kinetic energy Kinetic theory of matter Cohesion Liquids Viscosity Gas Plasma Pascal’s law Hydraulics Boyle’s law Pressure Celsius Kelvin Charle’s law Phase Condensation Freezing Melting Freezing point Melting point Evaporation Boiling Vaporization Sublimation Deposition Density Exothermic Endothermic Ch. 4 Atoms Continuous theory of matter Discontinuous theory of matter Tin oxide experiment Law of conservation of mass Law of definite proportions Law of multiple proportions Dalton’s atomic theory Crook Crook’s tube Thompson Rutherford Gold foil experiment Neils Bohr Quantum energy levels Electron cloud model Protons Neutrons Electrons Isotopes Gravity Electromagnetic force Strong force Weak force Quark Ch. 5 Periodic table Mendeleev Valence electrons Henry Moseley Families Period Luster Ductile Malleable Metals Nonmetals Metalloids Alkali metals Alkaline earth metals Transition metals Boron family Carbon family Nitrogen family Oxygen family Halogens Noble gasses Rare earth elements Atomic radius Ionization energy Electron affinity Electronegativity Chapter 6 Chemical Bonding Ion Ionic compounds Bohr model Crystal lattice Cation Anion Formula Chemical name Covalent bonds Lewis structure Molecule Network solid Polyatomic ions Metallic bond Polar Nonpolar Electronegativity Ch. 7 Chemical Reactions Chemical reaction Chemical equation Coefficient Mole Conversion factor Molar mass Synthesis Combustion Decomposition Single replacement Double replacement Exothermic Endothermic Reaction rate Surface area Catalyst Equilibrium Concepts Chapter 1 Scientific Method Know why you should know science Know the scientific method, be able to create your own, be able to list parts from an existing experiment Be able to explain the control in an experiment Be able to give the dependent and independent variables Know prefixes Know how scientific notation works Know how to use excel Be able to set up and use dimensional analysis Chapter 3 States of Matter Know what cohesion and kinetic energy have to do with the state of matter Be able to draw solids, liquids, and gasses at the atomic level Know how a gas moves Know pascals law Know how hydraulics work Know and be able to use the formulas for hydraulics Know and be able to use boyle’s law Know and be able to use charle’s law Know how to explain boyles and charles laws using the kinetic molecular theory Know how to explain what is going on at the atomic level in phase changes Know why the boiling point is lower at high altitudes Chapter 4 atoms Know what the Greeks thought of matter and how they differed Understand how the tin oxide experiment works Understand the law of conservation of mass Understand how the law of definite proportions and the law of multiple proportions work and be able to prove them with an example (I give the compound(s) and break them down, you give the ratio) Know the crook’s tube and what he put inside and what it proved Know what Thompson did with a crook’s tube and what he proved Know Thompson’s model of an atom Know Rutherford’s gold foil experiment Know Rutherford’s three conclusions and explain how he got them Know Dalton’s atomic theory, including what two are false and how he got them Know what happens to an atom according to the Bohr model when light is absorbed or released Be able to draw an atom using the electron cloud model Be able to find the number of electrons, protons, and neutrons in an atom Know the 4 forces that act in or on an atom Chapter 5 Periodic Table Know how Mendeleev organized the periodic table Know Mendeleev’s problems in the periodic table and how he solved them Know what Henry Moseley did with the periodic table Know the metals, nonmetals, and metalloids including their general properties Know the different parts of the periodic table including their general properties Know 3 uses of each family (aka three elements in the family and 1 use for each) Know how atomic radius is measured Know what happens to the atomic radius as you go down or across the periodic table Know why the atomic radius changes Know what happens to the ionization energy as you go down or across the periodic table Know why the ionization energy changes Know what happens to the electron affinity as you go down or across the periodic table Know why electron affinity changes Know what happens to the electronegativity as you go down or across the periodic table Know why electronegativity changes Ch. 6 Chemical Bonding Be able to draw ionic bonds using the bohr model Be able to draw a crystal lattice Given a chemical name be able to write a formula Given a formula be able to write a chemical name Be able to draw covalent bonds using the bohr model Be able to draw Lewis structures of single and double bonded molecules Know what metallic bonds are Be able to draw Lewis structures of polyatomic ions Chapter 7 Chemical Reactions Know how to balance equations Be able to convert from masses to moles Be able to convert from moles of one substance to moles of another substance Be able to convert from moles to masses Be able to tell if a reaction is synthesis, decomposition, combustion, single replacement, or double replacement Know the difference between exothermic and endothermic reactions Know what can change a reaction rate Know what chemical equilibrium is and what can change it Review Questions for the test on Scientific Method 1. Why should you know science, list at least three reasons. 2. Using the scientific method, write your own experiment (different than one we used in class or you did before) include all steps of the scientific method. 3. In your experiment above what is your control group? 4. In your experiment above, what is your dependent and independent variable? 5. What is the function of a control group? 6. Why is the metric system is better than the standard system. 7. I have 2 hairs stacked on top of each other to be used in a CSI forensic scan that blonde hair is 8.9x10-4 m high and the brunet hair is 2.2x10-4 m high. How high is my stack of hairs. Put your answer in scientific notation. 8. We have developed lasers that are so precise they can write your name on a single piece of hair. If your name is 6.2 micrometers express this size as a decimal. 9. A blood cell is .00004 m. Write this number in words and in scientific notation. 10. I have a small stack of papers that are 8.7x10-5 m tall. If I take one off that is 2.1x10-5 meters tall, how tall is the stack? 11. I have 3.83 x 107 grams of water in my pool, express this number in number format and in words. 12. If density = Mass/ Volume, what is the density of belly button lint that is 6.7x10-8 grams and has a volume of 4.9x10-2 cubic meters? 13. Watching strong men in the park tearing phone books in half in the park one day (June 23, 1998), I came up with a theory that the bigger the man the bigger the phone book he can tear in half. Matt weighs 97 pounds and can only tear a Where’s Waldo book (15 pages) in half. Waldo (weighing in at 210 lbs) can tear To Kill a mockingbird in half (the book, not the bird) (527 pages). Franz (at weighing 252 lbs) can tear a Harry Potter book in half (645 pages). Haans (302 lbs.) can tear Mein Komph (1043 pages). Make a table that shows this data.14. 14. What is one mistake in the experiment above that makes me a bad scientist? 15. 16. Knowing that distance = speed x time, if a lightning bolt travels at 3.7x106 meters per second for 1.7x10-1 seconds, how far from earth did the lightning bolt begin? 17. The largest hot cross bun was made by staff at Pegrums Bakery in the UK. The bun weighed 94.35 lbs and had a diameter of 4 ft 3 in. What was its weight in grams? 18. The human bladder can hold up to 2 cups of urine. (for those of you that need to go to the bathroom all the time) How many liters is this? Review questions for test on Ch. 3 1. What is the kinetic theory of matter? 2. What are the two definitions of a gas? 3. What makes air pressure on the atomic level? 4. What is pascal’s law? 5. The hydraulics on a high-low have a small piston with 3 cm2 and a large piston with 21 cm2. If the motor pushes with 524 lbs of force, how many tons can it lift? If the small piston moves 172 cm how far will the load rise? 6. A garbage compactor has a hydraulic unit set up with a large piston that is 12 inches across (and square) and a small piston is 1 inch in diameter (and round). If the motor can push on the small piston with 20 pounds of pressure how much pressure is compacting the garbage? 7. I have a piston at 11 atm and 9 ml. I let the piston up until there is 101.325 kPa of pressure (normal air pressure). What is my new volume in cm3? 8. Explain how Boyles law works with the kinetic molecular theory. 9. You are now a multimillionaire trying to circumnavigate the earth by hot air balloon. On earth the pressure is 101.325 kpa and your balloon is holding 300 cubic meters of air. At 30,000 feet the air will be only .25atm. You built your balloon to hold 1250 cubic meters of air. Will your balloon hold, making you the first person to complete such a feat or will your balloon rip sending you plummeting to the earth. 10. My rubber duckey in bath water (30 degrees C.) holds 15 cm3 of air. When the bath water turns cold (21 degrees C.) how much air will my rubber duckey hold? Assume that I put a cork in my duckey when it was in the warm water. 11. You are filling paintball cartridges to make your paintball gun shoot as far and as fast as possible. The side of the cartridge says to not fill it over 150 ml or it will blow up in your face. If you fill it with 100 ml of CO2 at 10 degrees Celsius, how much can you let it warm up (in C) until it blows? 12. Explain how Charles law works with the kinetic theory of matter. 13. What is a phase change? 14. list the three states of matter, and tell what the name of the phase change for each is, for example the phase change between a solid changing to a liquid is melting. 15. Why does the temperature of a compound stop changing when it is going through a phase change? (critical thinking) 16. What is an endothermic change, give an example in real life. 17. What is an exothermic change, give an example in real life. 18. How is boiling and vaporization different? 19. What is sublimation, how about deposition? 20. What is going on at the atomic level when a liquid turns into a gas? 21. How is boiling different than evaporation? 22. Can you make water hotter than 100 C? If so, how? 23. Liquid is forming on the outside of my glass containing ice water right now, what is this process called and what is going on at the atomic level. Is this process an exothermic or endothermic process? 24. .I have .84g of carbon dioxide in a 50 ml container at 105 kPa. If I release pressure (by making my volume bigger) until the gas is 25 kPa what is the density of my gas? 25. Why does sweating cool you down? Chapter 4 Review Questions 1. What were the two theories that the Greeks came up with and how are they different? 2. What three experiments led to the discovery of electrons, describe each. 3. Dalton said that atoms can not be divided, created, or destroyed, explain why he was wrong. 4. Dalton said that all atoms are identical in size, mass, and other properties. Explain why he was wrong. 5. What are isotopes and give one use of them. 6. What was JJ Thompson’s model of matter and how did he come up with it? 7. Why did Rutherford conclude that atoms are made of mostly empty space? 8. What are quantum energy levels? 9. What happens to the electrons when energy is added to an atom according to Neils Bohr? 10. If your shirt is red, describe how the atoms in your shirt make it that way? 11. How many protons, neutrons, and electrons are in a fluorine atom? 12. How many protons, neutrons and electrons are in Oxygen- 18 (Oxygen-18 is an isotope of oxygen with an atomic mass of 18)? 13. How many protons, neutrons and electrons are in K? 14. Draw a boron atom, include orbitals and electron placement according to the electron cloud model. 15. Draw a Cl atom, include orbitals and electron placement according to the electron cloud model. 16. Deuterium is a H-2 isotope (hydrogen with an atomic mass of 2), how many protons, electrons and neutrons are in deuterium? 17. List and describe the four forces that act in or on atoms. 18. Draw calcium using the electron cloud model. \ Review Question on Chapter 5 Periodic Table 1. Who created the first periodic table and what two criteria did he use to do it? 2. Who came along and fixed the periodic table, how did he do it? 3. How many electrons does the oxygen family want to gain or lose to become stable? 4. What are the general properties of the nonmetals? 5. Aluminum wants to lose how many electrons? 6. How did Mendeleev know where to leave spaces in his periodic table? 7. Explain how the atomic mass of an element is affected by the distribution of its isotopes in nature. 8. Does all the elements in a family have identical, or just similar properties, why? 9. Give me your best hypothesis on why it was difficult to find the Noble Gasses. 10. Give three elements and uses that are in the transition metals family. 11. Why are the transition metals called the transition metals 12. Give three elements in the alkaline earth metals family and a specific use of each. 13. What are the general properties of the halogen family? 14. What are three elements and their uses that are found in the nitrogen family? 15. What is electronegativity? What happens to electronegativity as you go across the periodic table? Why? 16. What is electron affinity? What happens to electron affinity as you go down the periodic table? Why? 17. What is ionization energy? What happens to ionization energy as you go across the periodic table? Why? 18. What is atomic radius? What happens to atomic radius as you go across the periodic table? Why? 19. What happens to atomic radius as you go down the periodic table? Why? 20. What are the properties of a metalloid? 21. Benjamin Franklin found that you can take electrons from a rod when you rub it with a wool cloth. What type of rod would you get more electrons from, a rod made of silicon or a rod made of carbon? Why? 22. What halogen would be a better electron acceptor (better at getting electrons) Chlorine or Bromine. (a better electron acceptor is more reactive, FYI) 23. In table salt (NaCl) what atom is going to get the electrons while in a bond? 24. Determine the average atomic mass for carbon given the following information: The abundance of Carbon – 12 is 98.90% with a mass of 12.000 amu. The abundance of carbon- 13 is 1.1% with a mass of 13.03335 amu. Review Questions for Ch. 6 Bonding 1. What is an ionic bond? High school definition, not kindergarten. 2. Draw the bohr model for sodium phosphide. 3. Draw lithium bromide in a crystal lattice. 4. Draw Magnesium Oxide in a crystal lattice 5. Name the following formulas a. MgCl2 b. Au2S3 6. Write the formula for the following compounds a. Iron (III) Bromide b. Aluminum Sulfide 7. Correct and rewrite the following formulas a. Be2F4 b. Na2Br 8. What does it mean to be polar? (hint: use page 168) 9. Draw the bohr model for CH3OH covalently bonded (this one is a toughy, not for the faint of heart!!) 10. Draw the bohr model of methane CH4 covalently bonded. 11. How is a covalent bond different than an ionic bond? 12. Draw a lewis structure for dichloromethane, CH2Cl2. 13. Draw the lewis structure for O2. 14. Draw the lewis structure for C2H5COOH 15. How are crystal lattices and network solids different, how are they the same? 16. What is a polyatomic ion. 17. Draw C2O42- in a Lewis structure 18. Draw Acetate C2H3O2- in a Lewis structure 19. Describe a metallic bond. 20. How is a cation different than an anion? Review Questions on Ch. 7 Chemical reactions 1. 1. What steps should I do when balancing a chemical reaction? 2. Balance the following reaction: sodium and water react to make sodium hydroxide (NaOH) and hydrogen. (this is used to make drain-o) 3. Balance the following reaction: C4H12 + O2 CO2 + H2O 4. Balance the following reaction: H2PO4 + Cl2 HCl + PO4 5. Why is it important to balance chemical reactions? 6. Write a balanced equation for the reactants and products in a match. Phosphorus (P)reacts with potassium chlorate (KClO3)to make potassium chloride (KCl)and phosphorus (V) oxide. (P2O5) 7. Balance the following reaction: Fluorine and aluminum bromide react to produce bromine gas and aluminum fluoride. 8. What does one mole of aluminum oxide weigh? 9. The reaction that causes cake batter to rise involves the production of CO2 from NaHCO3 (baking powder). How many liters of CO2 gas will be created when 15.0g NaHCO3 are heated? The density of CO2 is 1.997 g/L 2NaHCO3 H2O + Na2CO3 + CO2 9. When potassium hits water it creates potassium oxide and hydrogen gas an makes a large explosion (bigger than the one we did in class with sodium and water) If I toss 3 grams of potassium into water, how many grams of hydrogen gas will it make? H2O + K KOH + H2 10. How are double replacement reactions different than single replacement reactions? 11. Is the following reaction a synthesis, decomposition, single replacement, double replacement, or combustion reaction? Ca + H2O Ca(OH)2 + H2 12. Is the following reaction a synthesis, decomposition, single replacement, double replacement, or combustion reaction? 13. Is the following reaction a synthesis, decomposition, single replacement, double replacement, or combustion reaction? H2 + Cl2 HCl 14. Is the following reaction a synthesis, decomposition, single replacement, double replacement, or combustion reaction? KClO3 KCl + O2 14. Why does raising the temperature of a reaction increase the reaction rate? 15. What is chemical equilibrium?