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Chemistry 111 Exam 2 Study Guide

by: Bailey Wilhoit

Chemistry 111 Exam 2 Study Guide Chem 111

Marketplace > University of South Carolina - Columbia > Chemistry > Chem 111 > Chemistry 111 Exam 2 Study Guide
Bailey Wilhoit


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About this Document

This study guide covers chapters 6, 7, and 8.
Study Guide
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This 4 page Study Guide was uploaded by Bailey Wilhoit on Sunday October 16, 2016. The Study Guide belongs to Chem 111 at University of South Carolina - Columbia taught by Stefik in Fall 2016. Since its upload, it has received 38 views. For similar materials see Chemsitry in Chemistry at University of South Carolina - Columbia.


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Date Created: 10/16/16
Chemistry Study Guide Exam 2 Chapters 6, 7, & 8 1. What is the equation for Ideal Gas Law? 2. What are the four assumptions of the Kinetic Molecular Theory? 3. Express the pressure of a. 356 torr in atm b. 3.2 atm in torr c. 3760 Pa in atm 4. Convert the following temperatutes into Kelvin. a. 50℃ b. 230℃ c. -30℃ 5. A sample of gas occupies 135 mL at 22.5℃; with a the pressure at 200 torr. What is the pressure of the gas sample when it is placed in a 300 mL flask at standard temperature? 6. A 4.53 L sample of neon at 3.22 atm of pressure is added to a 10.0 L cylinder containing Argon. If the pressure in the cylinder is 6.98 after the neon is added, what was the pressure of argon in the cylinder? 7. What volume of ammonia is produced from the reaction of 3 L of hydrogen gas with 3 L nitrogen gas? What volume of the reactants will remain after the reaction ends? Assume all volumes are measured at the same pressure and temperature. 8. What is the density of He gas at 10.00 atm at standard temperature? 9. What volume of oxygen gas (L) at 30℃ and 0.993 atm reacts with excess hydrogen to produce 4.22 g water? 10. Calculate the pressure (atm) of 1.55 mol nitrogen at 530℃ in a 3.23 L container using ideal gas law and van der waals equation. 11. Why are there more lines observed in the emission spectra of hydrogen and other elements than are found in their absorption spectra? 12. How does the electron spin quantum number affect the energy of the electron in the hydrogen atom? 13. The strongest emission from excited-state Pb atoms has a wavelength of 405.8 nm. What is the frequency of this light? What region on the light spectrum is this found? 14. Calculate the wavelength, energy in one photon (in J), and energy of 1 mol of photons (in kJ) for cadmium with a threshold frequency of 9.83 x 10​14Hz. 15. What is the wavelength of an electron that is moving at a velocity of 2.9 x 10​ m/s? 16. Give the notation for each of the following subshells. a. n= 6, l=1 b. n=4, l=2 c. n= 3, l=0 17. How many subshells are present in the n=4 shell? How many orbitals in the 3d subshell? 18. Give the number of unpaired electrons present and the highest occupied subshell in the ground state of a. Arsenic b. Fluorine c. Carbon d. Helium e. Iron 19. Give the maximum number of electrons that can occupy each shell/subshell: a. 3d b. 5s c. 3p d. 4d 20. The speed of sound waves in the air is 344 m/s and the frequency of middle C is 512 Hz. What is the wavelength of this soundwave? 21. What are the electron configurations and orbital diagrams of the following elements? a. Be b. B c. Ne d. Rb e. C f. F 22. Define isoelectronic series. What are the symbols for four species that are isoelectronic. 23. What is ionization energy? 24. Write the electron configurations for the following elements. a. P b. Sr c. As d. Ba e. Bi f. U g. Xe 25. Using abbreviated notation, write the ground-state electron configuration for each element. a. S​2- 2+ b. Rh​ c. Co​ 3+ 2+ d. Ge​ e. Br​- 26. What neutral atoms are isoelectronic with the following ions? 2- a. O​ b. Ni​3+ c. In​+ 4+ d. Pb​ 27. Which species is larger? + a. Na or Na​ b. O​ or F​ - c. Na or Mg d. Li or Na 28. Which species has a higher ionization energy? a. N or F b. Mg​ 2+or Na​+ c. K or Si 29. How do you determine electron affinity? 30. Write the equation for the reaction of sodium and a. Oxygen b. Chlorine c. Nitrogen d. Water


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