Name: ______Date: ______Period: ______

Unit 5 Test Study Guide

Nuclear & Quantum Chemistry

Nuclear Equations

Write nuclear equations for the following scenarios:

  1. Alpha emission by plutonium-239, one of the substances formed in nuclear power plants.
  1. Beta decay by sodium-24, used to detect blood clots
  1. Oxygen-15 undergoes positron emission, used to assess the efficiency of the lungs.
  1. Copper-64 goes through electron capture, used to diagnose lung disease.
  1. A radioactive isotope is bombarded with an alpha particle to produce Polonium-84.
  1. A silver-117 undergoesthree beta emissions before it reaches a stable nuclide. What is the final product?

Complete the following nuclear equations and identify which type of nuclear decay it is.

  1. Sr Y + ____This is ______.
  1. F O + ____This is ______.
  1. Rn Po + ____This is ______.
  1. F + _____ OThis is ______.
  1. U He + ____This is ______.
  1. Xe  + _____This is positron emission.
  1. Sr + e  ____This is ______.

Radioactivity & Half-Lives

  1. One of the radioactive nuclides formed in nuclear power plants is hydrogen-3, called tritium, which has a half-life of 12.26 years. How long before a sample decreases to 1/8 of its original amount?
  1. Uranium-238 is one of the radioactive nuclides sometimes found in soil. It has a half-life of 454 years. What percentage of a sample is left after 2270 years?
  1. Cesium-133, which is used in radiation therapy, has a half-life of 30 years. What was the size of the original sample if after 120 years you now have 16.0 grams?
  2. Phosphorus-32, which is used for leukemia therapy, has decayed to 1/16th of its original amount in 42.9 days. What is the half-life of phosphorous-32?
  1. Iodine has a half-life of 8.07 days. Assuming you start with 90.5 grams, how much of the sample (in mg) would you have left after 24.21 days?

Bohr Model Diagrams

In the Bohr model diagrams show below, indicate the number of protons (p) and neutrons (n) in the nucleus of each atom. Write the number of electrons (e) on each energy level. Not all energy levels will be used for every element.

19.(a.)silicon-30(b.)calcium-41

Electromagnetic Spectrum

20.List the seven colors of the visible spectrum from shortest to longest wavelength.

______

21.What is the wavelength range of visible light? ______nm to ______nm.

22.Draw your interpretation of a long wavelength (above the time frame) and a short wavelength (below the time frame). Indicate which has higher frequency and higher energy.

23.(a) Which has a longer wavelength, orange or blue? ______

(b) Which has a lower frequency, green or red? ______

(c) Which has more energy, indigo or yellow? ______

Quantum Mechanics

Explain each of the following rules or terms associated with quantum mechanics.

24.Hund’s Rule______

25.Aufbau Principle______

26.Pauli Exclusion Principle______

27.Heisenberg’s Uncertainty Principle______

28.orbital______

29.identify the three (of the four) quantum numbers______

Orbital Diagrams

Draw the orbital diagrams (boxes and arrows) for each of the following elements.

30.silicon

31.zinc

Electron Configuration

32.Identify the element described by each electron configuration.

(a.)1s22s22p63s2______

(b.)1s22s22p63s23p64s23d104p65s24d3______

(c.)1s22s22p63s23p64s23d8______

(d.)[Kr] 5s24d6______

(e.)[Ar]4s23d104p4______

Electron Configuration Continued

33.Write the full electron configuration for the following atoms/ions (do NOT use the Noble Gas shortcut method).

(a.)P______

(b.)Y______

(c.)Ca+2______

(d.)Br-______

34.Write the Noble Gas (shortcut) electron configuration for each of the following.

(a.)Te______

(b.)Sb______

(c.)Bi______

Relating Bohr’s Diagram and Electron Configurations to the Quantum Numbers

35.Which quantum number tells you the main energy level? ______

36.In the atom, 1s22s22p4 – what is the highest every level that holds an electron? ______

37.How many orbitals are in the p-sublevel? ______How many electrons? ______

38.How many orbitals are in the d-sublevel? ______How many electrons? ______

39.Which quantum mechanical principle states that (choose from Pauli Exclusion Principle, Aufbau Principle, and Hund’s Rule):

(a) electrons will fill orbitals from lowest to highest energy? ______

(b) no two electrons can have the same set of quantum numbers? ______

(c) electrons will avoid pairing in an orbital if an orbital of equal energy is available? (the sharing rule) ______

40.How many electrons can be accommodated in each of the following:

(a) one d orbital ______

(b) a set of f orbitals ______(d) the 7s orbital ______

(c) the n = 4 shell ______(e) one p orbital ______

Important Vocabulary & Concepts to review

Define the following words

Trajectory______quantum ______entail ______valence electrons ______frequency ______

Wavelength ______

Explain the following concepts (you can use words and pictures)

  1. Nuclear decay
  1. Radioactivity
  1. Radioactive particle
  1. Half-Life
  1. Fission
  1. Fusion
  1. Electron orbital diagram
  1. Electron configuration
  1. Bohr model of the atom
  1. The relationship between wavelength, frequency and energy
  1. The relationship between energy levels, sublevels and orbitals
  1. The relationship between an element’s electron configuration & its position on the periodic table