Review for Regular/Pre AP Chemistry Final KHS

Transcription

1 Review for Regular/Pre AP Chemistry Final KHS Vocabulary Absorption Accurate Alkali metals Alkaline Earth Metals Alpha decay Alpha particle Alpha radiation Aqueous Atomic number Atomic Radius Average atomic mass Avogadro s number Balanced equation Beta decay Beta particle Beta radiation Boiling point Bond Cathode ray tube Chemical properties Chemical changes Chemistry Chromatography Composition Conductivity Conductor Covalent compound Dalton Ductile, Electrolyte Electron Electron configuration Electronegativity Electrons Elemental gas Empirical formula Endothermic Energy level Energy sub-level Exothermic Extensive property Fission Fusion Flammability Formula mass Formula unit Freezing point Frequency Fume Hood Gamma radiation g/mole Halogens Heisenberg Heterogeneous mixture Homogenous mixture Hydrogen bonding Insulator Intensive property Intermolecular forces Ion Ionic compound Ionization energy Kinetic Energy Kinetic Theory Law of Conservation of Mass Lewis dot structure London dispersion forces Malleable, Matter Mendeleev Metal/ nonmetal/metalloid Metallic bond Molar mass Mole Molecular formula Molecule Moseley Negative pole Neutral Neutrons Noble gases Orbital Oxidation number Oxidation state Percent composition Photon Physical properties Physical changes Polarity Polyatomic ion Positive pole Potential Energy Precise Product Protons Reactant Reactivity Rutherford Saturated Schrodinger Scientific Theory Solubility Soluble Solute Solvent Spectrometer Spectrum States of matter Supersaturated Surface area Thomson Transition metals Unsaturated Van der Waals Wavelength Yield 1

2 Answer the following questions. 1) What are fume hoods used for? 2) What safety equipment is needed for reactions involving high amounts of heat or possible explosion? 3) What safety precautions should you use with the chemical described in the MSDS below? 4) How should you dispose of left over HCl? 5) List 3 uses of science in the world today. 6) How can you prove or disprove a hypothesis? 7) Using standard lab equipment and acid, how can you determine if one piece of metal is more chemically reactive than another? How would you construct an experiment to test this? 8) The true value of a measurement is When three measurements are made they are recorded as 1.051, 1.052, and 1.053? Are the three measurements precise? Are they accurate? 9) Express in scientific notation. 10) Express the product of 561 and 1.2 using the correct number of significant digits. 11) Which of the graphs below show the relationship that would occur in container of gas on a hot day? On the graphs below, the y axis label should read volume. 12) If the predominant color of the light spectrum of a gas is violet what can you say about the magnitude of the wave s energy, wavelength and frequency? 13) List three possible pollution problems associated with nuclear power. 14) Chemistry is the study of matter and how it. This would help in any career field that dealt with 15) Alcohol has a lower freezing and boiling point than water. Knowing this, what fluids used in your car might benefit from mixing alcohol with it? 16) Iron rusting, food digesting, and wood burning are all examples of changes. 17) Light activates photosynthesis in plants which is a change. 18) How can you separate salt from salt water? 19) Draw a picture of what the particles of a mixture would look like if the mixture was composed of He gas, O 2 and NH 3. 20) Mendeleev s periodic table was based on. 21) Moseley s periodic table was based on. 22) Where do you find the transition metals? 2

3 23) Categorize the following as metal, transition metal, metalloid, or nonmetal: iron, silver, aluminum, chlorine, silicon, and zirconium. 24) High conductivity, low ionization energy, and low Electronegativity would most likely indicate a (metal/nonmetal). 25) Low conductivity, high ionization energy, and high Electronegativity would most likely indicate a (metal/nonmetal). 26) Look at the table below. Elements 2, 10, and 18 have the highest ionization energies. Why? 27) Explain this observation in terms of electrons. 28) What did J.J. Thomson observe that led him to believe that the electron had a negative charge? 29) When Ernst Rutherford performed the gold foil experiment, what did he discover about the structure of the atom? 30) What discoveries led to each of the following models of the atom; plum pudding, planetary, quantum mechanical? 31) A certain photon of light has a wavelength of 653 nm. What is the frequency of its light? 32) What is the atomic mass of Hafnium if 5.0% have a mass of g/mol, 19.0% have a mass of g/mol, 27% have a mass of g/mol, 14% have a mass of g/mol, and 35% have a mass of g/mol? 33) In the diagram below, tell to what A, B, and C refer. 34) Write the Lewis dot structure for potassium. 35) The element represented by 1s 2 2s 2 2p 6 3s 2 3p 5 is 36) Write the electron configuration for phosphorus. 37) Write the IUPAC name for NH 4 Br, Cu 3 (PO 4 ) 2, HF, and SO 2. 38) Write the chemical formula for potassium chloride, iron II sulfate, phosphoric acid, and trinitrogen disulfide. 39) Construct the electron dot formula for the compound formed from lithium and bromine. 40) Construct the electron dot formula for the compound carbon disulfide. 41) Metals tend to electrons to form ionic bonds. 42) A mole is represented by particles of a substance. 43) The molar mass of NaOH is: 44) If 28% of a sample is Iron-55, 20% is Iron-56 and 52% is Iron-57, the average atomic mass of a sample of Iron would be. 45) The number of moles represented by 1.51 x atoms of an element is moles. 46) How many sulfate ions would occur in 1.8 moles of CuSO 4? 47) How many moles are represented by 30.3g of Neon gas? 48) The number of Na 1+ ions necessary to make 4 moles of Na 3 PO 4 would be. 3

4 49) What is the percent of oxygen found in MgO? 50) If the percent of sodium in sodium oxide is 74%, what is the empirical formula for this compound? Balance each of the following equations: A) C 3 H 8 + O 2 CO 2 + H 2 O B) H 2 SO 4 + NaOH Na 2 SO 4 + H 2 O C) Cu + Pb(NO 3 ) 4 Cu(NO 3 ) 2 + Pb 51) Describe the relative molecular motion for each of the states of water listed below: ice, liquid water. steam. 52) What are the similarities and differences in the amount of kinetic energy found in the most common 3 states of matter? 53) What is the Kinetic Molecular Theory? 54) How is water unique, as compared to other molecular compounds such as CO 2? 55) What is polarity, and what effect does it have on the solubility of substances? 56) Based upon the graph at right; what mass of KNO 3 will dissolve in 100g of water at 30 o C? 57) What would be a possible temperature and mass of LiBr for an unsaturated solution? 58) If 30g of NaClO 3 is dissolving 100g of water at 50 o C, how much more can be dissolved to reach a saturated solution? 59) What are three ways to make rock salt dissolve into a cup of water faster and why does each of the actions you listed work? 60) If a compound is added to water, and the starting temperature of the water was 25 o C, predict a possible temperature at the end of the dissolution of the compound if it is Exothermic or Endothermic: 61) Compare and contrast the properties of ionic and covalent compounds. 62) How do the intermolecular forces holding a substance together change as the substance changes state? Problems: 1)Identify the type of reaction for each of the equations below: A) HBr + NaOH NaBr + H 2 O B) 2Cu +2 HNO 3 2CuNO 3 + H 2 C) 2Na + 2H 2 O 2NaOH + H 2 D) 3Mg(OH) 2 + 2H 3 PO 4 Mg 3 (PO 4 ) 2 + 6H 2 O 2) What is the density of methane (CH 4 ) at STP? 3) If the volume of a sample of methane is 32.7 ml at STP, what is the mass of that sample? 4) If the temperature of a sample of cold water is 41 º C, and a metal object with a temperature of 132 º C is added to it, what will happen to the temperature of the metal? What will happen to the temperature of the water? What can you predict about the final temperature of the system? 4

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