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Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ The final will be comprehensive, covering chapters 1-18, with the focus on chapters 10 – 18. The following questions will be what you have to Be Able To do for the final. Complete the following questions. Where it says important topics, you do not have to write anything, just study those topics in those chapters. Chapter 1 Important topics: homogeneous mixture, heterogeneous mixture 1. Place a X in the box to indicate whether the following substance is an element or a compound Substance H2 MgCl2 Ne Cl2 NaC2H3O2 Element Compound 2. Place a X in the box to indicate whether the following element is a metal, nonmetal, or metalloid Element N2 Ca Si Co Metal Nonmetal Metalloid Chapter 2 Important topics: significant figures, directly proportional, inversely proportional 3. A chunk of wood has a mass of 258g and occupies 122 cm 3. What is the density of this wood? 4. The density of water is roughly 1.0g/mL at room temperature. Would the chunk of wood float or sink in water? Why? 5. Under certain conditions, oxygen gas (O2) has a density of 0.00134 g/mL. What is the volume occupied by 250.0 g of O2 under the same conditions? Chapter 3 Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ Important topics: law of conservation of mass, definition of atomic mass, definition of isotope, definition of ions 6. Fill in the table below to determine the number of protons, neutrons, and electrons. Nuclear Symbol Protons Neutrons Electrons 26 30 23 7. Fill in the table below Element Number of valence electrons Ionic charge K O Ca F N Al 8. Write the electron configuration for a. Na b. Mg+2 c. Cl-1 9. Fill in the electrons in the orbital diagram below for sulfur Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ Chapter 5 Important ideas: shielding, nuclear charge, definition of ionization energy, definition of electronegativity 10. Fill in the table below to identify the proper element Description Element symbol Alkali metal in period 3 Halogen in period 2 Any transition metal in period 5 Noble gas in period 4 Alkaline earth metal in period 6 11. Which element has… a. Higher atomic radius: F or I b. Lower atomic radius: Na or Cl c. Higher electronegativity: C or O d. Lower electronegativity: I or F Chapter 6 Important topics: octet rule, intermolecular forces (hydrogen bonding, dipole, dispersion) 12. Place a X in the box to indicate whether the following compound is ionic or covalent Compound Ionic Covalent CaCl2 NO2 AlBr3 CH4 NH4Cl 13. Draw the Lewis structure for CF4 14. Write the shape notation and determine the shape of the compound drawn above 15. Is the compound drawn above is polar or nonpolar? 16. What type of intermolecular force does a sample of CF4 have? 17. Draw the Lewis structure for the compound formed between Mg and Cl Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ Chapter 7 Important topics: naming rules for ionic compounds, covalent compounds, acids 18. Give the formulas for the following compounds a. iodine pentafluoride _____________________________ b. sulfurous acid __________________________________ c. aluminum sulfide _______________________________ d. acetic acid _____________________________________ e. cobalt (III) carbonate ____________________________ f. dinitrogen trioxide ________________________________ 19. Give the names for the following compounds g. P4S5 __________________________________ h. Mg(CH3COO)2 ___________________________________ i. H2CO3 __________________________________ j. Si2Br6 __________________________________ k. H3P _____________________________________ l. Ni(OH)2 ________________________________________ Chapter 8 Important topics: 5 types of reactions 20. Write the balanced chemical reaction with the states of matter given the following descriptions a. Ethane (C2H6) burns Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ b. Potassium chloride reacts c. Calcium and nitrogen react d. Magnesium metal is added to a solution of copper (II) chloride e. Solutions of barium nitrate and sodium sulfate are mixed together Chapter 9 Important topics: molar mass, mole ratio, theoretical yield, percent yield, limiting reactant 1. For the following reaction: 2 Al + 3 CuCl2 → 3 Cu + 2 AlCl3 a. How many moles of aluminum are needed to completely react with 0.00789 moles of copper (II) chloride? b. How many grams of aluminum are needed to completely react with 0.004365 moles of copper (II) chloride? c. How many moles of copper (II) chloride are needed to completely react with 0.25 grams of aluminum? Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ d. How many grams of copper (II) chloride are needed to completely react with 0.15 grams of aluminum? e. Which reactant is the limiting reactant if there are only 1.254 grams of aluminum and 6.348 grams of copper (II) chloride available for this reaction? f. What is the theoretical yield of copper when 1.254 grams of aluminum and 6.348 grams of copper (II) chloride react? g. When this reaction was carried out in the lab, 3.487 grams of product was obtained. What is the percent yield of this reaction? Chapter 10 Important topics: kinetic molecular theory, gas laws – Boyle, Charles, Gay-Lussac, combined, Dalton If the temperature is held constant in the diagram above, name the gas law being illustrated, and describe how the variables change. Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ In the above container, with a fixed volume, the temperature is increased from the first picture to the 2nd. 1. Describe the change in kinetic energy of the particles 2. Name the gas law and describe how another variable, in addition to temperature will change. The temperature of a 3.00 L sample of gas is changed from 5 to 25 oC. what will the volume of gas be at the new temperature if pressure is held constant? A student collects 350 mL of oxygen gas at a temperature of 24 oC and a pressure of 0.85 atm. How many moles of oxygen did the student collect? A gas occupies 13 liters at a pressure of 50 mm Hg. What is the volume when the pressure is increased to 75 mm Hg? 600.0 mL of air is at 20 oC. what is the volume at 60.0 oC? Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ A sample of oxygen is collected in a 175 mL container over water at 35 oC when the barometric pressure reading is 742.0 torr. What is the partial pressure of the dry gas? If a mixture of gases contains 3 gases - carbon dioxide with a partial pressure of 0.285 torr and nitrogen with a partial pressure of 593.525 torr and oxygen at partial pressure = ? find the partial pressure of oxygen. What is the density of silicon tetraflouride gas at 68 oC and pressure = 135 kPa? A gas sample at 47 oC and 1.03 atm occupies a volume of 2.2 L what volume would this gas occupy at 107 oC and 0.789 atm? What is the mass of 85.0 L of NO2 at STP? How many grams of calcium carbonate is needed to form 2.5 L of CO2 when calcium carbonate is decomposed (see chapter 8 decompostion if you need to figure out equation)? Chapter 12 Final BAT Name: ___________________________________________ Date: ____________________ Period: ___ Important topics: Particle behavior in liquids and solids, phase changes, molar heat of fusion, molar heat of vaporization, phase diagrams, equilibrium vapor pressure Describe the change in the particles and indicate if heat is added or removed when: a) b) c) d) A liquid changes to a vapor A liquid changes to a solid A vapor changes to a liquid Solid CO2 sublimes How is boiling different from evaporation? During the boiling process – describe what is happening to the particles and the temperature. Explain why glycerol boils at a higher temperature than water (in terms of the attractive forces between molecules) At a given temperature, different liquids have different equilibrium vapor pressures. Explain why this is true (in terms of attractive forces between molecules).