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Physical Science Mid-term Review Name _____________________ Review for Chemistry Final 1. Explain the steps in the scientific method. 2. Scientists use the metric system for measurement. What are the basic metric units for the following? Length – Volume Time Mass 3. List the values for 6 different prefixes. 4. All matter has both physical and chemical properties. Give 3 examples of physical properties. 5. What is a chemical property? Give an example. 6. Explain how to find the density of an object or a liquid. 7. A piece of wood has a mass of 2.0 grams and a volume of 6 cm3. What is the density of the wood? Will the wood float on top of water or sink? 8. Define the 4 phases of matter a) Draw a molecular interpretation of a solid changing to a liquid and then to a gas. b) How much heat energy is needed to boil a 10.0 g piece of ice that has a temperature of – 30.0°C 9. Matter can undergo physical and chemical changes. Give 3 examples of physical changes. 10. Give 3 examples of chemical changes. 11. Describe the 3 classes that matter can be divided into and give 3 examples of each. 12. The law of conservation of mass states that matter cannot be made or destroyed by ordinary chemical means. Explain what is meant by this statement. 13. Who is Democritus and what did he believe? How about the early Greeks? 14. John Dalton created an atomic theory in the early 1800’s. It has been slightly revised. Write down the 5 parts of the modern atomic theory. Include the names and models of 5 scientist. 15. Describe the 3 basic particles found in the atom? 16. Draw a picture of the modern day atom. 17. Describe an isotope and give two examples. 18. Describe an ion and give two examples. 19. Fill in the following table. Use a periodic table Remember: (atomic number = number of protons), (number of electrons = number of protons), (mass number = number of protons + number of neutrons.) Element Symbol Sodium Atomic # Mass # 11 23 Ar Aluminum 13 Ion Charge +1 # of protons # of neutrons 0 18 22 14 +3 27 32 127 Br 80 -1 # of electrons 25 53 36 20. Draw the Bohr diagrams for three of the elements in the above table. Change the third one into an anion or cation that would be most appropriate for that element. 21. Chemical bonds are forces that hold two or more atoms together. There are two types of chemical bonds: ionic bonds and covalent bonds. Explain the difference between the two bonds. 22. Name the groups on the Periodic Table and describe how to predict valence e- # & Oxidation # 23. Using e-dot diagrams show the bonding structure for the following compounds and molecules a. Aluminum and Chlorine b. Hydrogen and Oxygen c. Calcium and Phosphorus 24. Choose three metals and 2 non-metal element and 1 negative poly-atomic ion. Using those 6 ions create 9 different compounds list formulas and names. 25. Name the following formulas a. Ni(NO3)3 b. BaS c. NaC2H3O2 d. (NH4)3(PO4) e. FeP Study your notes know the major concepts and understand the connections between them. Physical Science Mid-term ANSWERS Name ______FSK____ Review for Chemistry Final 1. Explain the steps in the scientific method. 1) Define the Problem 2) Hypothesis 3) Experiment 4) Draw Conclusions (Theory/Law) 5) Publish (Report Results) 2. Scientists use the metric system for measurement. What are the basic metric units for the following? Length – Meter Volume - Liter Time - Second Mass - Kilogram 3. List the values for 6 different prefixes. Micro = 1/1,000,000; Deka – 10 ; milli- 1/1000; kilo 1000; centi 1/100; Mega – 1,000,000 4. All matter has both physical and chemical properties. Give 3 examples of physical properties. Color, Mass, Density, Temperature, volume, texture …. 5. What is a chemical property? Give an example. A chemical property is a description of how a substance reacts or relates to other substances. Ex: Flammable, reacts with acids, decomposes … 6. Explain how to find the density of an object or a liquid. D = mass/volume 7. A piece of wood has a mass of 2.0 grams and a volume of 6 cm3. What is the density of the wood? Will the wood float on top of water or sink? D = m/v = (2.0 g)/6cm3 = 0.33 g/cc it will float because its density is less then water’s 1.0 g/ml. 8. Define the 4 phases of matter Solid liquid gas plasma increased motion and energy a) Draw a molecular interpretation of a solid changing to a liquid and then to a gas. Continue to break more and more intermolecular bonds till there are none in a gas. b) How much heat energy is needed to boil a 10.0 g piece of ice that has a temperature of – 30.0°C 1) q = mCp∆T = (10.0 g)(4.184 J/g/C°)(30C) = J 2) q = mHf = (10.0g)(334J/g) = ___J 3) q = mCp∆T = (10.0 g)(4.184 J/g/C°)(100C) = J 4) q = mHv = (10.0g)(2260J/g) = ___J 9. Matter can undergo physical and chemical changes. Give 3 examples of physical changes. Folding paper, squeezing water out of a sponge, freezing gasoline in the tank. 10. Give 3 examples of chemical changes. Burning paper, pouring water on Sodium(explode), Eating a freezer pop. 11. Describe the 3 classes that matter can be divided into and give 3 examples of each. Element Lead, Compound Alcohol, Solution pen ink., Colloid Mayo, Suspension house Paint, Solid mixture Wood 12. The law of conservation of mass states that matter cannot be made or destroyed by ordinary chemical means. Explain what is meant by this statement. The mass you start with must be the same mass you finish with regardless of the type of change the matter endures. 13. Who is Democritus and what did he believe? How about the early Greeks? Coin the term “ATMOS” 1st to believe the concept of the atom. 14. John Dalton created an atomic theory in the early 1800’s. It has been slightly revised. Write down the 5 parts of the modern atomic theory. Include the names and models of 5 scientist. 1) All matter is made of atoms that are in constant motion. Dalton Billiard Ball 2) Atoms are indivisible Thompson Plum Pudding 3) Atoms from different elements are different. Rutherford Nuclear Model 4) Atoms from the same elements are the same Bohr Planetary Model 5) Law of Multiple Proportions. Heisenberg and Schrödinger Modern Day Model 15. Describe the 3 basic particles found in the atom? Proton Positive charge mass of 1 amu Electron Negative charge mass of 0 amu Neutron No charge mass of 1 amu 16. Draw a picture of the modern day atom. Should include, p.n.e, orbitals , energy levels, and nucleus 17. Describe an isotope and give two examples. Element with different # of N Carbon-14 and Deuterium (H-2) 18. Describe an ion and give two examples. Charged atom (different # e then P) Na+ Cation or Cl- anion 19. Fill in the following table. Use a periodic table Remember: (atomic number = number of protons), (number of electrons = number of protons), (mass number = number of protons + number of neutrons.) Element Ion Charge +1 # of protons # of neutrons # of electrons 11 12 0 18 22 +3 13 27 14 11 18 13 32 27 53 74 45 53 Symbol Atomic # Mass # Na 11 23 Argon Ar 18 Aluminum Al Co I 13 40 27 59 127 -1 Sodium Cobalt Iodine Bromine 27 53 35 Br 80 35 35 20. Draw the Bohr diagrams for three of the elements in the above table. Change the third one into an anion or cation that would be most appropriate for that element. Al +3 Draw 21. Chemical bonds are forces that hold two or more atoms together. There are two types of chemical bonds: ionic bonds and covalent bonds. Explain the difference between the two bonds. Ionic bonds transfer e- from cation to anion ::: Covalent bonds is a sharing of electrons between two atoms Ionic is metal to non-metal bonds ::: Covalent bond are between to non-metals 22. Name the groups on the Periodic Table and describe how to predict valence e- # & Oxidation # Outline of table with charges & e- listed. 23. Using e-dot diagrams show the bonding structure for the following compounds and molecules d. Aluminum and Chlorine AlCl3 e. Hydrogen and Oxygen H2O f. Calcium and Phosphorus Ca3P2 24. Choose three metals and 2 non-metal element and 1 negative poly-atomic ion. Using those 6 ions create 9 different compounds list formulas and names. Multiple Answers possible. 25. a. Ni(NO3)3 Nickle(III) Nitrate b. BaS Barium Sulfide c. NaC2H3O2 Sodium Acetate d. (NH4)3(PO4) e. FeP Ammonium Phosphate Iron(III) Phosphide