CHM 110 Final Exam Review F22 (2)

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Chem 110 F22 Dr. Pfirman Final Exam Review Packet Name:____________________________________________________________ Section 1: Conversions 1. Express the following numbers in proper scientific notation. 93,000,000 ________________ 22.47 ________________ 0.0000529 ________________ 2. Express the following numbers in decimal form. 2.38029 x 10 2 ________________ 1.375 x 10 - 3 ________________ 1.09674 x 10 4 ________________ 3. Calculate the following conversions and use the correct number of significant figures. 2.24 cm = ___________________ in 2.24 L = ___________________ mL 10.0 mol H 2 O = _________________ g H 2 O 10.0 molecules H 2 O = _______________ moles H 2 O 1

Chem 110 F22 Dr. Pfirman 2 lbs = __________ kg 1.200 x 10 5 g CO 2 = _________________ moles CO 2 0.00100 ft = _______________ in 5.00 g sulfuric acid = ___________________ molecules Sulfuric acid 2.000 atm = __________________ mm Hg = __________________ torr 32.0 moles potassium carbonate = _____________________ g potassium carbonate Section 3: Accuracy and Precision 8. Classify the following sets of measurements as accurate, precise, both, or neither. (a) Checking for consistency in the weight of chocolate chip cookies: 17.27 g, 13.05 g, 19.46 g, 16.92 g (b) Testing the volume of a batch of 25-mL pipettes: 27.02 mL, 26.99 mL, 26.97 mL, 27.01 mL (c) Determining the purity of gold: 99.9999%, 99.9998%, 99.9998%, 99.9999% 2

Chem 110 F22 Dr. Pfirman Section 4: Chemical and Physical Properties and Changes 9. Label each of the following changes as physical or chemical: (a) condensation of steam (b) burning of gasoline (c) souring of milk (d) dissolving of sugar in water (e) melting of gold (f) coal burning (g) ice melting (h) mixing chocolate syrup with milk (i) explosion of a firecracker (j) rusting of metal chair in the rain Section 5: Ions, Isotopes, and Electron Configurations 12. Naturally occurring silver has two isotopes. Isotope A has a relative mass of 106.9051 and an abundance of 51.82%. Isotope B has a relative mass of 108.9047. Calculate the atomic mass of silver from these data. 3

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Chem 110 F22 Dr. Pfirman 13. Use the periodic table to find the numbers of protons, neutrons, and electrons for the following atoms or ions. Name of Element Element Symbol Mass Number Atomic Number Protons Neutrons Electrons Copper 29 35 Tc 98 43 Pb +4 207 Thallium 204 81 H +1 0 Carbon 12 14. Cobalt–60 and iodine–131 are radioactive isotopes commonly used in nuclear medicine. How many protons, neutrons, and electrons are in atoms of these isotopes? Write the complete electron configuration for each isotope. 15. Write BOTH the expected full electron configuration, AND the actual full electron configuration. a. Cu b. Cr 16. Write the abbreviated electron configurations (noble gas configuration) AND state how many valence shell electrons the atom has. a. Mn b. Be 4

Chem 110 F22 Dr. Pfirman Section 6: Periodic Trends 17. Which has the largest atomic radius in each pair? a. K Ge b. Eu Pm c. Ge Pb d. Bi Ni 18. Which has the largest ionization energy of each pair? a. Sn Pb b. Be B 19. Which has the highest electron affinity of each pair? a. F Cl b. Rb Sb c. Hg Pb Section 7: Quantum Theory and Advanced Bonding Theory 20. Write the set of quantum numbers for the 8 th electron of O. Write out the electron configuration and orbital-filling diagram FIRST, and circle the eighth electron to fill in the orbitals of O. 21. How many electrons fit into: a. one orbital? b. the p-subshell? c. the valence shell of a noble gas? 5

Chem 110 F22 Dr. Pfirman 22. Write a set of quantum numbers for each of the electrons with an n of 3 in a P atom. 23. For the molecules below: a. label each bond as either σ or π. b. label the hybridization for each non-H atom c. label the formal charge for each non-H atom 6 n l m l m s

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Chem 110 F22 Dr. Pfirman Section 8: Lewis Structures and Molecular Geometry Molecule Lewis Structure AND Bond Angles Electron Geometry Molecular Geometry Hybrid- ization on Central atom Formal Charge on Central atom Polar? ClO 3 - SF 6 PF 5 SO 4 -2 SF 4 7

Chem 110 F22 Dr. Pfirman Section 9: Electromagnetic Radiation 24. Heated lithium atoms emit photons of light with an energy of 2.961 10 –19 J. a. Calculate the frequency and wavelength of one of these photons. b. What is the total energy in 1 mole of these photons? c. What is the color of the emitted light? 25. The eyes of certain reptiles pass a single visual signal to the brain when the visual receptors are struck by photons of a wavelength of 850 nm. If a total energy of 3.15 x 10 –14 J is required to trip the signal, what is the minimum number of photons that must strike the receptor? 26. An FM radio station found at 103.1 on the FM dial broadcasts at a frequency of 1.031 10 8 s –1 (103.1 MHz). What is the wavelength of these radio waves in meters? 8

Chem 110 F22 Dr. Pfirman 27. FM–95, an FM radio station, broadcasts at a frequency of 9.51 10 7 s –1 (95.1 MHz). What is the wavelength of these radio waves in meters? Section 11: Chemical Reactions and Concentration 28. What is the molarity of a solution formed by dissolving 18.0 g of sodium nitrate in enough water to form 250.0 mL of solution? 29. How many grams of sodium chloride are there in 30.0 mL of a 1.2 M solution of sodium chloride? 30. What is the concentration of the MgCl 2 solution that results when 0.250 L of a 0.766-M solution is allowed to evaporate until the volume is reduced to 0.205 L? 9

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Chem 110 F22 Dr. Pfirman 31. a. Write and balance the full molecular reaction (use solubility rules to determine which compounds will have the designation aq or s ) according to the written description: Barium nitrate reacts with ammonium phosphate to produce barium phospate and ammonium nitrate. b. Write the full ionic equation. c. Write the net ionic equation. 32. a. Finish and balance the molecular equation. NaCl( aq ) + AgNO 3 ( aq ) ⟶ b. Write the full ionic equation. c. Write the net ionic equation 33. Determine and label all the oxidation charges, and state what species are oxidized, reduced, oxidizing agents, and reducing agents. H 2 ( g ) + Cl 2 ( g ) ⟶ 2HCl( g ) 10

Chem 110 F22 Dr. Pfirman 34. Consider this question: What is the mass of solute in 200.0 L of a 1.556- M solution of KBr? 35. A large piece of jewelry has a mass of 132.6 g. A graduated cylinder initially contains 48.6 mL water. When the jewelry is submerged in the graduated cylinder, the total volume increases to 61.2 mL. (a) Determine the density of this piece of jewelry. (b) Assuming that the jewelry is made from only one substance, what substance is it likely to be? Section 12: Random Assortment 36. Name the following compounds: Name Formula Tetracarbon nonoxide Carbonic acid Mg(OH) 2 FeCO 3 Copper (I) sulfate hexahydrate Beryllium chloride (NH 4 ) 2 SO 4 Iron (III) cyanide CF 4 MgO 2 Sn 3 (PO 4 ) 4 11

Chem 110 F22 Dr. Pfirman 37. Draw the following Lewis structures, and all possible resonance forms of each. (a) selenium dioxide (b) nitrate ion (c) nitric acid (d) benzene, C 6 H 6 38. Match the hybridization with the appropriate electron geometry. a. sp 1. Trigonal bipyramidal b. sp 2 2. Linear c. sp 3 3. Tetrahedral d. sp 3 d 4. Octahedral e. sp 3 d 2 5. Trigonal planar 12

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Chem 110 F22 Dr. Pfirman 39. List the three subatomic particles and their charges. 40. Atoms of the same element that differ in mass are called __________________. 41. An Iodine (I) ion has a charge of -1. What is the: Mass number? Atomic number? Protons? Neutrons? Electrons? 42. What quantity of heat (in J) is necessary to raise 3.00 L of water (d=1.00 g/mL) from 22.0°C to 63.0°C? 43. Calculate the enthalpy change, ΔH rxn °, for the following reaction: P 4 O 10 (s) + 6 PCl 5 (g) → 10 Cl 3 PO (g) Given: ΔH rxn ° (kJ) 1) P 4 + 6 Cl 2 → 4 PCl 3 - 1225.6 2) P 4 + 5 O 2 → P 4 O 10 - 2967.3 3) PCl 3 + Cl 2 → PCl 5 - 84.2 4) PCl 3 + 1/2 O 2 → Cl 3 PO - 285.7 13

Chem 110 F22 Dr. Pfirman 44. If 1.13 x 104 J of heat is added to a water sample and the temperature rises from 88.0 ºC to its boiling point, what mass of water is in the sample? 45 . The specific heat capacity of gold is 0.128 J/g ºC. How much heat would be needed to warm 250.0 grams of gold from 25.0 ºC to 100.0 ºC? 42. 14