CP Chemistry Unit 2 Test Review PDF

# CP Chemistry Unit 2 Test Review ## 1. Calculate the frequency emitted by a photon of light having a wavelength of 1.52 × 10^-7 m. C = λν 3.00 × 10⁸ m/s = 1.52 × 10^-7 m = 1.97 × 10¹⁵ Hz ## 2. Calculate the change in energy for a photon of light w...

# CP Chemistry Unit 2 Test Review ## 1. Calculate the frequency emitted by a photon of light having a wavelength of 1.52 × 10^-7 m. C = λν 3.00 × 10⁸ m/s = 1.52 × 10^-7 m = 1.97 × 10¹⁵ Hz ## 2. Calculate the change in energy for a photon of light with a frequency of 4.85 × 10¹⁴ Hz. E = hν 6.626 × 10^-34 J/Hz * 4.85 × 10¹⁴ Hz = 3.21 × 10^-19 J ## 3. Draw the electromagnetic spectrum from shortest wavelength to longest. Label the extremes with high or low energy, short or long wavelength, and high or low frequency. **lower energy** <---------- **radio waves** <--- **microwaves** <--- **infrared** <--- **visible light** <--- **ultraviolet** <--- **x-rays** <--- **gamma rays** ---------> **higher energy** **long wavelength** <-------- **short wavelength** ## 4. Fill in the blank with the appropriate term. * (higher, lower, longer, shorter)* * Red photons emit **lower** energy than yellow photons. * Blue light has a **higher** frequency than violet light. * Ultraviolet radiation emits **higher** energy than microwave radiation. * Gamma radiation has a **higher** frequency than x-rays. * Green light has a **longer** wavelength than violet light. ## 5. Provide descriptions for the following rules for electron filling.... * **Aufbau Principle** - fill energy levels from **low** -> **high energy.** * **Pauli Exclusion Principle** - same orbital, **opposite spin** * **Hund's Rule -** even distribution (in same sublevel) ## 6. Write Electron Configurations for the following elements. * **Strontium:** Sr 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² * **Gold:** Au 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s¹ 4f¹⁴ 5d¹⁰ * **Arsenic:** As 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p³ ## 7. Write the Noble Gas Configurations for the following elements. * **Iodine:** [Kr] 5s² 4d¹⁰ 5p⁵ * **Copper:** [Ar] 4s¹ 3d¹⁰ * **Californium:** [Rn] 7s² 5f¹⁰ ## 8. Complete the following table: | Isotope | Nuclear Symbol | Protons | Neutrons | Electrons | |---|---|---|---|---| | Cobalt-59 | ⁵⁹₂₇Co | 27 | 32 | 27 | | Selenium-79 | ⁷⁹₃₄Se | 34 | 45 | 34 | | Francium-223 | ²²³₈₇Fr | 87 | 136 | 87 | | Bromine-80 | ⁸⁰₃₅Br | 35 | 45 | 35 | ## 9. Fill in the following table about the subparticles of an atom * (proton, neutron, electron)*: | | Charge (+1, 0, or -1) | Mass (1 or 0) | Inside or Outside the Nucleus | |---|---|---|---| | Proton | +1 | 1 amu | Inside | | Neutron| 0 | 1 amu | Inside | | Electron | -1 | 0 | Outside | ## 10. Using the Bohr models below, explain how spectral lines are formed. Which one of the diagrams actually shows what causes colored light? * If an electron falls back to the ground state the electron releases energy photons in the form of colored light with specific wavelengths. <br> ## 11. Identify what elements are in the mixture below. * **Barium** * **Lithium** * **Helium** * **Hydrogen** <br> ## Test Studying Tips: Review your notes, textbook (page numbers on HW PKT), and review/practice HW PKT.