CHEMISTRY I - HONORS MIDTERM REVIEW* *Test may cover other topics not included on this review, yet have been covered throughout the semester.

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1 Name Period CHEMISTRY I - HONORS MIDTERM REVIEW* *Test may cover other topics not included on this review, yet have been covered throughout the semester. Chapter 2 Measurement & Calculations Describe the purpose of the scientific method Distinguish between qualitative and quantitative measurements Describe the differences between the hypotheses, theories and models Distinguish between a quantity, unit, and a standard measurement Name & use SI units for length, mass, time, volume & density Distinguish between mass & weight Perform density calculations Distinguish between accuracy and precision Determine the number of significant figures in measurements & perform operations Convert measurements into scientific notation Distinguish between inversely and directly proportional relationships Scientific measurement System Hypothesis Theory Model Accuracy Precision Percentage error Significant figures Scientific notation Directly proportional

2 Indirectly proportional Chapter 1 Matter and Change Distinguish between physical properties and chemical properties of matter Classify changes of matter as physical or chemical Explain gas, liquid & solid states in terms of particles Explain how conservation of matter applies to changes of matter Distinguish between a mixture & a pure substance Mass Matter Atom Element Compound Extensive properties Intensive properties Physical properties Physical change Change of state Solid Liquid Gas Plasma

3 Chapter 3 Atoms: the Building Blocks of Matter Explain the Conservation of Mass, the Law of Definite Proportions, & Law of Multiple Proportions Summarize the 5 essential points of Dalton's atomic theory Summarize the properties of the cathode ray tube that led to the discovery of the electron Summarize the experiment carried out be Rutherford that led to the discovery of the nucleus List the properties of the proton, neutron, electron Define the atom Explain what isotopes are Define atomic number & mass number, describe how they apply to isotopes Avogadro s number, molar mass and conversions between the two Law of Conservation Mass Law of Definite Proportions Law of Multiple Proportions Atom Nuclear forces Atomic number Isotope Mass number Nuclide Atomic mass unit Average atomic mass Molar mass Avogadro s number

4 Chapter 21 Nuclear Chemistry Explain what a nuclide is, and describe the different ways nuclides can be represented. Define and relate the terms mass defect and nuclear binding energy. Explain the relationship between nucleon number and stability of nuclei. Explain why nuclear reactions occur and know how to balance a nuclear equation. Define and relate the terms radioactive decay and nuclear radiation. Describe the different types of radioactive decay and their effects on the nucleus. Define the term half-life, and explain how it relates to the stability of a nucleus. Define and relate the terms decay series, parent nuclide, and daughter nuclide. Explain how artificial radioactive nuclides are made, and discuss their significance. Compare the penetrating ability and shielding requirements of alpha particles, beta particles, and gamma rays. Describe three devices used in radiation detection. Discuss applications of radioactive nuclides. Define nuclear fission, chain reaction, and nuclear fusion, and distinguish between them. Explain how a fission reaction is used to generate power. Discuss the possible benefits and the current difficulty of controlling fusion reactions. Mass defect Nuclear binding energy radioactive decay nuclear radiation half-life decay series parent nuclide daughter nuclide

5 Nuclear fission Chain reaction Nuclear fusion Chapter 4 Arrangement of Electrons Explain the mathematical relationship among the speed, wavelength & frequency of electromagnetic radiation Discuss the dual wave-particle nature of light Discuss the significance of the photoelectric effect & line-emission spectrum Describe the Bohr model of the hydrogen atom Discuss the development of the quantum model of the atom Explain the Heisenberg Uncertainty Principle List the 4 quantum numbers & describe their significance Relate the number of sublevels to an atom s energy levels, orbitals per sub-level List the total number of electrons needed to fully occupy each energy level State Aufbau principle, the Pauli Exclusion Principle, & Hund s Rule Describe electron configurations using, orbital notation, electron configuration or noble-gas notation Electromagnetic radiation Electromagnetic spectrum Wavelength Frequency Photoelectric effect Quantum Photon Ground state Excited state Line-emission spectrum Continous spectrum

6 Heisenberg Uncertainty Principle Quantum theory Orbital Quantum number Principle quantum number Angular momentum quantum number Magnetic quantum number Spin quantum number Electron configuration Aufbau Principle Pauli Exclusion Principle Hund s Rule Noble-gas Noble-gas configuration

7 Chapter 5 The Periodic Law Describe the roles of Medeleev and Moseley in the development of the periodic table Describe the modern periodic table Explain how periodic law can be used to predict physical and chemical properties Describe how elements belonging to a group are interrelated Locate and name the four blocks of the periodic table Discuss the relationship between group configurations and group numbers Describe the locations in the periodic table and the general properties of the alkalai metals, the alkaline earth metals, the halogens, and the noble gases Define and compare the periodic trends atomic radii, ionization energy, electron affinity & electronegativity Define valance electrons and state how many are present in each main group element Compare the periodic trends of the d-block elements with those of the main block elements Periodic law Periodic table Lanthanide Actinide Alkalai metal Alkaline earth metal Transition metal Main group elements

8 Halogens Atomic radius Ion Ionization Ionization energy Electron affinity Cation Anion Valence electrons Electronegativity Chemistry Midterm review random extra questions *Test may cover other topics not included on this review, yet have been covered throughout the semester. 1. What are the two main branches of science? And how do they relate to each other? 2. What is the difference between scientific law and scientific theory? Which can be changed or replaced and when can this happen? 3. Describe the relationship between science and technology? 4. What is the first step in the scientific method? 5. When are scientific models used? Give 2 examples. 6. How do scientists test a hypothesis? 7. Explain why no experiment should be called a failure? 8. What is the difference between an SI base unit and a derived unit? 9. What are the 3 types of graphs used? And when are each of them used? 10. Explain in your own words the difference between accuracy and precision? 11. Copy table 1, table 2, table 3 on page 16. (your SI base Units and the prefixes) 12. What is the rule for significant figures for adding/subtracting? And multiplying/dividing? 13. Convert 3.5 sec to milliseconds. 14. Convert 40 cm to m. 15. Convert 1.5 kg to g. 16. Convert 24 ml to L. 17. Write the following in scientific notation a m b. 60,200 mg c L 18. Write the measurements in long form. (take out of scientific notation) a. 4.5 x 10 3 g b x 10 8 cm c x 10 6 km 19. Perform the calculations and write the answer with the correct number of significant figures. a m x 40.3 m

9 b cm x 6.70 cm x cm c. 3.5 g g d L / 1.3 L e g 2.3 g 20. How many significant figures are in the following numbers: a. 45 b. 640 c d Explain the relationship between matter, atoms, and elements. 22. Which is the most abundant element on Earth? 23. What are the two types of pure substances? 24. Sketch a flow chart with these words: Matter, Mixtures, Pure Substances, Elements, Compounds, Homogeneous Mixture, and Heterogeneous Mixture. 25. Compare and contrast mixtures and pure substances. Give an example of each. 26. Describe the differences between physical and chemical properties. List some of these properties and explain why they are important. 27. How are mixtures separated? Give 3 examples. 28. Are changes of state physical or chemical changes? Why? 29. Which is easily reversible, physical or chemical change? Why? 30. List 3 clues that indicate a chemical change has occurred? 31. Is Density a physical or chemical property? Why? 32. Identify whether the following is an element or compound: a. H2O b. Fe c. K d. C6H12O6 33. In question above, how many Oxygen atoms are in 1a? 1d? 34. Calculate the following Density calculations: 35. A piece of tin has a mass of g and a volume of 2.26 cm 3. What is the density of the tin? 36. A piece of titanium metal has a mass of 67.5 g and volume of 15 cm 3. What is the density of the titanium? 37. The density of a piece of brass is 8.4 g/cm 3. If the mass of the brass is 510g, find the volume of the brass. 38. Identify whether the following is a chemical or physical property: a. Flammability b. Freezing point c. Boiling point d. Density e. Reactivity with air f. Color g. Identify whether the following is a physical or chemical change: h. Change of color i. Dissolving sugar in water j. Producing a gas k. Evaporation l. Rusting Iron m. Burning paper n. Fruit rotting

10 39. Describe how temperature relates to kinetic energy. If the temp. goes up or down what happens to kinetic energy? 40. Name several factors that determine the speed of the atoms and molecules of a particular substance. 41. What are the four states of matter? Describe them each in terms of having definite shape and definite volume. 42. Compare the viscosity of milk and honey. 43. Explain how differences in fluid pressure create buoyant force on an object. 44. Explain how gases differ from solids and liquids. List at least 4 properties of gases. 45. What causes the pressure exerted by gas molecules on their container? 46. Pick on of the gas laws and give one real life example. 47. Predict what will happen to a can of coke left in a hot car all day and explain your reasoning. 48. State whether energy is released or absorbed in the following: a. freezing b. boiling c. melting d. sublimation 49. State Boyle s Law Formula and apply it in the following problems: 50. A sample of Argon Gas occupies a volume of 2.8 L at 1.3 atm. What will its volume be at 1.3 atm? L of Hydrogen at 7.1 atm pressure is used to fill a balloon at a final pressure of 1.15 atm. What is its final volume? 52. Explain Dalton s atomic theory. 53. State the charge, mass, and location of each part of an atom according to the modern periodic table. 54. Do atoms have an electrical charge? Why or why not? 55. What were the differences between Bohr s model with the modern model of the atom? 56. What is the order of the periodic table based on? 57. How are the electrons of an element related to the arrangement of the periodic table? 58. What do valence electrons predict? 59. What group # are the alkali metals and alkaline earth metals located? And list 2 characterictics of each. 60. Where are the semiconductors located on the periodic table? List several characteristics of them. 61. Do Noble Gases exist as a molecule or a single element? And why? 62. What makes noble gases extremely stable and inert? 63. Do metals tend to lose or gain electrons? Why? 64. Do nonmetals tend to lose or gain electrons? Why? 65. Where are the transition metals located? 66. In the following problems, how many protons, electrons and neutrons are there: a. Carbon 14 b. Nitrogen 15 c. Sulfur 35 d Cl e. 15 7N 67. Name the element AND the group that the following elements belong to. a. K b. Ti c. Cl

11 d. Ne e. Mg f. Si 68. How many moles are present if you have 56.0 grams of BaBr2? 69. How many grams are present if you have 1.12 E23 atoms of Au? 70. How many grams are present if you have 4.50 moles of KCl? 71. How many molecules are present if you have 6.70 moles of Al2O3? 72. How many grams are present if you have 4.56 E23 molecules of NaOH? 73. How many grams are equal to 12.0 moles of H2? 74. How many moles are equal to 3.50 grams of BaBr2? 75. How many moles are equal to 6.02 E24 molecules of Ca3(PO4)2?