Practice Test: Chapter 7

Matching skip

Short Answer skip

1. radial probability distribution
   
2. electron spin
   
3. Hund's Rule
   
4. Why do atoms have a tendency towards the s orbital
   
5. Emission spectrum
   

Multiple Choice skip

1. atomic radius
   1. Decreases from left to right across a period. Increase effective nuclear charge, decreased shielding. Increases down a group. Increases in the orbital sizes in successive principal quantum levels
   2. Light scattered from a regular array of points or lines. Wavelengths of visible light are not all scattered in the same colors, but 'separate.' Works the best when spacing between the scattering points is about the same as the wavelength of the wave being diffracted
   3. Postulated energy can be gained of lost only in whole-number multiples of the quantity hv where h is a constant
   4. Certain characteristics of light that particulate matter, certain that particulate waves
2. ground state
   1. Decreases from left to right across a period. Increase effective nuclear charge, decreased shielding. Increases down a group. Increases in the orbital sizes in successive principal quantum levels
   2. Eistein's special theory of relativity. Energy has mass.
   3. Lowest possible energy state
   4. Atoms with more than one electron
   5. ms, Can only have 2 values. -1/2, 1/2
3. Why is the Bohr Model incorrect
   1. Only certain energies are allowed for the electron in the hydrogen atom. Energy Quantized
   2. nhv
   3. Only works for Hydrogen. Important historically, paved the way for later theories. Current theory of atomic structure has nothing to do with Bohr model. No circular orbits for electrons
   4. The electrons in the outermost principal quantum level of an atom
   5. h = 6.626x10^-34 Js
4. Diffraction
   1. Light scattered from a regular array of points or lines. Wavelengths of visible light are not all scattered in the same colors, but 'separate.' Works the best when spacing between the scattering points is about the same as the wavelength of the wave being diffracted
   2. Schrodinger equation does not account for electron repulsions. To solve, treat each electron as if it were moving in a field of charge that is the net result of the nuclear attraction and the average repulsions of all the other electrons
   3. Only works for Hydrogen. Important historically, paved the way for later theories. Current theory of atomic structure has nothing to do with Bohr model. No circular orbits for electrons
   4. Lowest possible energy state
   5. Only certain energies are allowed for the electron in the hydrogen atom. Energy Quantized
5. Max Plank
   1. Postulated energy can be gained of lost only in whole-number multiples of the quantity hv where h is a constant
   2. n, Integral values 1, 2, 3…, Dictates size and energy of orbital
   3. Ψ. Function of the coordinates x, y and z = Electrons position in space
   4. Created when light diffracts. Can only be explained in terms of waves
   5. Electrons are emitted from the surface of a metal when light strikes it. 1. Threshold frequency v0, electrons not emitted below it regardless of intensity. 2. Number of electrons increase with intensity of light, if frequency above threshold. 3. Kinetic energy of emitted electrons increases linearly with frequency of light. Minimum energy required to remove electron = E0 = hv0

True or False skip

1. 3 characteristics of electromagnetic radiation
   There is a fundamental limitation to just how precisely we can know both the position and momentum of a particle at a given time. The more accurately we know a particle's position, the less accurately we can know its momentum. Not necessary for large things, Vital for small, like electrons

   True   False

2. hertz
   Unit per second. 1/s. Frequency measurement. Hz

   True   False

3. core electrons
   Similar to electron bound to nucleus. Stationary, do not travel along. Limitations to standing waves. Always a node at each end, must be a whole number of half wavelengths in allowed motions. Only certain circular orbits have a circumference into which a whole number of wavelengths will 'fit'

   True   False

4. Standing wave
   Similar to electron bound to nucleus. Stationary, do not travel along. Limitations to standing waves. Always a node at each end, must be a whole number of half wavelengths in allowed motions. Only certain circular orbits have a circumference into which a whole number of wavelengths will 'fit'

   True   False

5. Hydrogen line spectrum
   Wave function corresponding to the lowest energy for hydrogen atom

   True   False