* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Semester 2 review questions
Chemical bond wikipedia , lookup
Chemical element wikipedia , lookup
Low-energy electron diffraction wikipedia , lookup
Condensed matter physics wikipedia , lookup
Photoredox catalysis wikipedia , lookup
Marcus theory wikipedia , lookup
Photoelectric effect wikipedia , lookup
Metastable inner-shell molecular state wikipedia , lookup
History of molecular theory wikipedia , lookup
Water splitting wikipedia , lookup
Abundance of the chemical elements wikipedia , lookup
IUPAC nomenclature of inorganic chemistry 2005 wikipedia , lookup
Rutherford backscattering spectrometry wikipedia , lookup
Electrochemistry wikipedia , lookup
Molecular orbital diagram wikipedia , lookup
Gas chromatography–mass spectrometry wikipedia , lookup
X-ray fluorescence wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Auger electron spectroscopy wikipedia , lookup
Stoichiometry wikipedia , lookup
Electronegativity wikipedia , lookup
Atomic orbital wikipedia , lookup
Electrolysis of water wikipedia , lookup
Light-dependent reactions wikipedia , lookup
Metallic bonding wikipedia , lookup
Hydrogen atom wikipedia , lookup
Periodic table wikipedia , lookup
History of chemistry wikipedia , lookup
Metalloprotein wikipedia , lookup
Chemistry: A Volatile History wikipedia , lookup
Photosynthetic reaction centre wikipedia , lookup
Degenerate matter wikipedia , lookup
Extended periodic table wikipedia , lookup
Name_______________ Chemistry I: Semester Review Questions – The Mole and Stoichiometry 1. How many particles of CO2 are present in 245 g of CO2? 2. How many liters of oxygen gas at STP are required to react with 65.3 g of aluminum in the production of aluminum oxide? 3. Copper reacts with silver nitrate to form silver and copper(II) nitrate. How many grams of copper are required to react with 50.0 mL of 8.0M AgNO3? 4. A substance is found to be composed of 70.58% Carbon, 5.93% Hydrogen, and 23.49% Oxygen. Find the empirical formula for the substance. Empirical Formula ____________________ 5. Given that the substance above has a molar mass of 204.24 g/mole, find the molecular formula of the substance. Show your work. Molecular formula: 6. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas. How many liters of 3.75 M HCl are needed to fully react with 165.53 g of zinc? 7. For ZnCl2, calculate the Percent Composition of each element. Data Table: The Reaction between Tin(II) Nitrate and Aluminum Mass of Empty Beaker Mass of beaker and Tin (II) Nitrate Trial 1 34.56 g 78.84 g Mass of Aluminum metal 6.45 g Mass of beaker and Tin (Sn) Metal after reaction 64.76 g 1. Balance the following Equation: _____ Sn(NO3)2 + _____ Al _____ Al(NO3)3 + _____ Sn 2. Determine the Mass of Aluminum metal and Tin(II) Nitrate used in this reaction. 3. Using the information from question (2) and the balanced equation, calculate the theoretical amount of Tin (Sn) that should have been produced from this reaction. (hint: determine the limiting reactant) Theoretical yield =_________________________, Limiting reactant = ______________ 4. Using the above data table, calculate the actual amount of Tin (Sn) produced from the reaction. 5. Using the information from questions 3 & 4, calculate the percent yield of Tin for the reaction. Based on your answer to #3 (the limiting reactant), find out how much of the excess reactant should be left at the end of the experiment. Chemistry I: Semester Review Questions – Electron Configuration NAME THE TERM DESCRIBED BY THE FOLLOWING DEFINITIONS: 1. A packet of light energy that carries a quantum of energy. 2. The state when all electrons of an atom are in the lowest possible energy levels. 3. When an electron jumps up to a higher energy level, the atom is in its ___. 4. The scientist who applied Einstein’s particle-wave theory to electrons. 5. The theory that it is impossible to know both the position and speed of an electron simultaneously. 6. The theory that no two electrons in an atom can share the same 4 quantum numbers. 7. The theory that electrons fill the lowest energy orbitals first. 8. The theory that, within a sublevel, electrons prefer to occupy their own orbital. 9. A term describing the outermost electrons in an atom. 10. A positively charged ion is called a(n) ___. A negatively charged ion is called a(n) ___. 11. The most stable type of electron configuration. 12. A three-dimensional region in space where an electron is likely to exist. DRAW ORBITAL DIAGRAMS (boxes) FOR THE FOLLOWING ELEMENTS AND GIVE THE FOUR QUANTUM NUMBERS FOR THE LAST ELECTRON: 13. Mg 14. Si 15. Ti WRITE LONGHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS: 16. N 17. K 18. Cr WRITE SHORTHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS: 19. Sb 20. Bi 21. Tc 22. Ge Chemistry I: Periodic Trends Semester Review Questions Answer the following questions. (Correct any false statements). 1. ____________________ was a Russian chemist who arranged the known elements in vertical columns in order of increasing mass and noticed a pattern in physical and chemical properties. 2. ____________________ was a British physicist who determined the atomic number (number of protons in the nucleus)of the atoms of elements and then arranged the elements according to their atomic number. 3. _____(T/F) The modern periodic table arranges the elements in order of increasing atomic number. 4. ___________________ are the horizontal rows of the periodic table. 5. __________________ or ___________________ are the vertical columns of the periodic table. 6. _____(T/F) The elements in a period have similar chemical and physical properties. 7. _____(T/F) The characteristic properties of the elements in a group change from period to period. 8. Circle the element below that would most similar in chemical and physical properties as calcium: potassium iron (Fe) bromine (Br) beryllium sodium 9. Underline the element above that would be most different from calcium. 10. Label the following diagram with s, p, d, and f and then match the characteristics listed below with the letters s, p, d and f. _____ contains the noble (inert) gases _____ contains the alkali metals _____ contains most of the nonmetals _____ contains the transition metals _____ contains the alkaline earth metals _____ contains the lanthanide and actinide series (inner transition elements) _____ Representative elements (2 blocks) _____ group 1, 2 and helium _____ 13, 14, 15, 16, 17 and 18 11. State the periodic law: Answer the following questions by filling in the blank. 1. __________ Determine the number of valence electrons in the following element: [Ne]3s23p2 2. __________ How many valence electrons does column 13 contain? 3. __________Determine the number of valence electrons in the following element: [Ar]4s23d104p5 4. __________What is the valence electron configuration for any element in group 2? 5. __________ What energy level are Bromine’s valence electrons in? 6. Period:__________ Given the following configuration: [Ar]4s23d104p2; what period and block is the last valence electron found in? Block:___________ 7. ___________The electron configuration for an element is: [Ar]4s23d104p5 What family does it belong to? Fill in the blank with the correct choice, (A, B, or C) from the given list. A. Increase B. Decrease C. Stay the same 8_____ As you move left to right in a period, atomic size will… 9_____ As you move up a group, 1st ionization energy will… 10_____ As you move from Iodine to Fluorine, electronegativity will… 11_____ As you move from Scandium to Zinc, shielding will… 12_____ As you move down a group, atomic size will… 13_____ The size of a positive ion compared to the neutral atom will… 14_____ As you move from Sodium to Cesium, shielding will… 15_____ The size of a negative ion compared to the neutral atom will… 16_____ As you move from right to left in a period, 1st ionization energy will… 17_____ As you move left and down, electronegativity will… Use the Ionization Energies listed in the data table below to answer the following questions. Element 1st 2nd 3rd 4th 5th 6th Xq 650 1320 2745 12756 ----18__________ What is the value of the third ionization energy? 19__________ How many valence electrons does element Xq have? Give the name for the following compounds 23. BaSO3 29. AgNO3 24. (NH4)3PO4 30. Fe2O3 25. MgSO4 31. HClO 26. CaO 32. N2O3 27. H3PO4 33. HF 28. MnO 34. NaHCO3 WRITE FORMULAS FOR THE FOLLOWING COMPOUNDS: 35. hydrobromic acid 42. diphosphorus pentoxide 36. chromium(III) carbonate 43. sulfurous acid 37. magnesium sulfide 44. lead(II) nitrate 38. iodine trichloride 45. dihydrogen monoxide 39. lithium hydride 46. sodium oxalate 40. ammonium hydroxide 47. perchloric acid 41. calcium chloride 48. chlorous acid Chemistry I: Covlent bonding Semester Review Questions For each of the following molecules, draw the Lewis Diagram. MOLECULE 1. OF2 2. CO32- 3. CI4 LEWIS DIAGRAM Chemistry I: Gas law Semester Review Questions FOR EACH OF THE FOLLOWING, NAME THE GAS LAW AND SOLVE THE PROBLEM: 1. Hydrogen is collected over water at 0.975 atm and 28C. What is the partial pressure of H2? Water has a partial pressure of .0349 atm. 2. How many moles of chloroform, CHCl3, are required to fill a 253-mL flask at 100.0C and 940 torr? 3. You want the pressure inside a bottle to be 75.0 kPa at 23C. At what temperature in Celsius should you seal the bottle when the pressure is 1.12 atm? 4. A diver’s lungs hold about 20.0 L of air underwater at a pressure of 875 mm Hg. Assuming he holds his breath and his lungs don’t burst, what will be the volume of air in his lungs at standard pressure on the water’s surface? 5. What pressure is required to compress a gas that occupies 6500 L at 25C and 1.0 atm to a volume of 40.0 L at 18C? 6. When a canning jar is sealed at 100C the pressure inside is 101.3 kPa. What is the pressure inside the jar when it cools to room temperature, about 21C? 7. CO2 gas is collected over water at 100.3 kPa and 19C. Find the pressure of the dry gas. Water has a partial pressure of 2.23 KPa. 8. What is the temperature of a 0.00893 mol sample of neon gas that has a volume of 302 mL and a pressure of 0.941 atm? 9. A gas occupies 4.78 L at 78.1 kPa and 25C. What will the volume be at 0.975 atm and 15C? 10. A shampoo bottle contains 443 mL of air at 65C. What is its volume when it cools to 22C? 11. A balloon is filled with helium to a volume of 12.5 liters at 25C and 101 kPa. How many grams of helium are in the balloon? 12. Three gases are inside a room. If the total pressure of the gases is 1.01 atm and Hydrogen has a pressure of 0.25 atm, Nitrogen has a pressure of 0.45 atm, and Oxygen is the only other gas in the container, what is the pressure of the oxygen in the container? 13. Ammonia and Nitrogen gases are placed in the same room. Which gas will diffuse faster and how many times faster will it be then the other gas? SOLVE THE FOLLOWING GAS STOICHIOMETRY PROBLEMS: 14. What volume of chlorine is required to produce 25.4 g of copper(II) chloride at 18C and 2.13 atm? Cu + Cl2 CuCl2 15. At 778 mm Hg and 25C, how many grams of zinc are required to produce 25.2 liters of hydrogen gas? __Zn + __HCl __ZnCl2 + __H2 16. If 5.45 g of potassium chlorate decompose, how many liters of oxygen gas are given off at 1.58 atm and 32C? 2KClO3 2KCl + 3O2 17. When aluminum is burned in 15.0 L of oxygen at 97.3 kPa and 21C, how many grams of aluminum oxide are formed? 4Al + 3O2 2Al2O3 18. If 12.8 g of CaCO3 decomposes at 38C and 0.96 atm, how many dm3 of CO2 are formed in addition to CaO? CaCO3 CaO + CO2 REMEMBER: 1cm 3 = 1 mL & 1 dm3 = 1 L Laws: P1V1 P2V2 T1 T2 Ptotal = P1 + P2 + … PV = nRT R = 0.0821 atm L mol K or R = 8.314 KPa L mol K