General Chemistry Principles & Modern Applications 9 th Edition Petrucci/Harwood/Herring/Madura Chapter 8 Electrons in Atoms Dr. Travis D. Fridgen Memorial University of Newfoundland © 2007 Pearson Education
Based on the diagram and equations below which of the following statements is true? 1. The energy of radio waves are greater than the energy of visible waves. 3. The energy of ultraviolet waves are greater than the energy of infrared waves. 4. The energy of gamma waves are smaller than the energy of X-Ray waves. 2. The greater the wavelength, the greater the energy of the light.
Based on the diagram and equations below which of the following statements is true? 1. The energy of radio waves are greater than the energy of visible waves. 3. The energy of ultraviolet waves are greater than the energy of infrared waves. 4. The energy of gamma waves are smaller than the energy of X-Ray waves. 2. The greater the wavelength, the greater the energy of the light.
Based on the diagram and the equation below which of the following statements is true? 1. The frequencies of radio waves are greater than the frequencies of visible waves. 2.The frequencies of ultraviolet waves are greater than the frequencies of infrared waves. 3. The frequencies of gamma waves are smaller than the frequencies of X-ray waves. 4. None of the above statements are true.
Based on the diagram and the equation below which of the following statements is true? 1. The frequencies of radio waves are greater than the frequencies of visible waves. 2.The frequencies of ultraviolet waves are greater than the frequencies of infrared waves. 3. The frequencies of gamma waves are smaller than the frequencies of X-ray waves. 4. None of the above statements are true.
To the right is a schematic of the apparatus used for photoelectric effect measurements where 0 is called the threshold frequency. True or false, if light of a higher frequency is shone on the metal a larger current will be measured? 1. True 2. False
1. True 2. False To the right is a schematic of the apparatus used for photoelectric effect measurements where 0 is called the threshold frequency. True or false, if light of a higher frequency is shone on the metal a larger current will be measured?
Without the use of a calculator, indicate which of the following transitions in the hydrogen atom results in the emission of light of the greatest energy? 1. n=4 to n=3 2. n=1 to n=2 3. n=3 to n=2 4. n=2 to n=1 5. n=1 to n=3
Without the use of a calculator, indicate which of the following transitions in the hydrogen atom results in the emission of light of the greatest energy? 1. n=4 to n=3 2. n=1 to n=2 3. n=3 to n=2 4. n=2 to n=1 5. n=1 to n=3
Without the use of a calculator, indicate which of the following transitions in the hydrogen atom results in the emission of light of the longest wavelength? 1. n=4 to n=3 2. n=1 to n=2 3. n=3 to n=2 4. n=2 to n=1 5. n=1 to n=3
Without the use of a calculator, indicate which of the following transitions in the hydrogen atom results in the emission of light of the longest wavelength? 1. n=4 to n=3 2. n=1 to n=2 3. n=3 to n=2 4. n=2 to n=1 5. n=1 to n=3
The best experimental evidence for the existence of discrete (quantized) energy levels in an atom comes from 1.Diffraction of electrons by crystals. 2. Dispersion of light by matter. 3. Atomic Line Spectra. 4. The Stern-Gerlach Experiment
The best experimental evidence for the existence of discrete (quantized) energy levels in an atom comes from 1.Diffraction of electrons by crystals. 2. Dispersion of light by matter. 3. Atomic Line Spectra. 4. The Stern-Gerlach Experiment
1. n=2, l = 0, m l = 0 2. n=3, l = 0, m l = 0 3. n=3, l = 1, m l = 1 4. n=3, l = 2, m l = n=3, l = 3, m l = -3 Which of the following orbital designations is impossible?
1. n=2, l = 0, m l = 0 2. n=3, l = 0, m l = 0 3. n=3, l = 1, m l = 1 4. n=3, l = 2, m l = n=3, l = 3, m l = -3 Which of the following orbital designations is impossible?
Which of the following sets of quantum numbers is not matched with the orbital designation. 1. n=1, l = 0: a 1s orbital 2. n=2, l = 0: a 2p orbital 3. n=3, l = 0: a 3s orbital 4. n=3, l = 1: a 3p orbital 5. n=3, l = 2: a 3d orbital
Which of the following sets of quantum numbers is not matched with the orbital designation. 1. n=1, l = 0: a 1s orbital 2. n=2, l = 0: a 2p orbital 3. n=3, l = 0: a 3s orbital 4. n=3, l = 1: a 3p orbital 5. n=3, l = 2: a 3d orbital
Hydrogen atom Many electron atom In the hydrogen atom, the orbitals in a given shell are degenerate. For multiple electron atoms what is the main reason for the splitting of, say, the 2s and 2p orbital energies? 1. Higher nuclear charge. 2.The greater distance of the electrons from the nucleus. 3. Penetration of the nucleus by the 2s electron. 4. The presence of an angular node for the 2p orbital.
Hydrogen atom Many electron atom In the hydrogen atom, the orbitals in a given shell are degenerate. For multiple electron atoms what is the main reason for the splitting of, say, the 2s and 2p orbital energies? 1. Higher nuclear charge. 2.The greater distance of the electrons from the nucleus. 3. Penetration of the nucleus by the 2s electron. 4. The presence of an angular node for the 2p orbital.
Below are radial probability distributions for the 1s, 2s, 2p, 3s and 3p orbitals in random order. Which one is the radial probability distribution for the 3s orbital?
Below are radial probability distributions for the 1s, 2s, 2p, 3s and 3p orbitals in random order. Which one is the radial probability distribution for the 3s orbital?
Below are radial probability distributions for the 2s, 2p, 3s, 3p and 3d orbitals in random order. Which one is the radial probability distribution for the 3d orbital?
Below are radial probability distributions for the 2s, 2p, 3s, 3p and 3d orbitals in random order. Which one is the radial probability distribution for the 3d orbital?
Which of numbers in the periodic table below corresponds to the group of elements in which the 2p orbitals are being filled.
Which of numbers in the periodic table below corresponds to the group of elements in which the 4d orbitals are being filled
Which of the following is the condensed electron configuration for chlorine? 3. [Ne]3s 2 3p 6 2. [Ne]3s 2 3p 5 1. [Ne]3p 7 4. [Ne]3s 2 3d 5 5. [Ne]3s 2 3p 3 3d 2 Cl 2 (g) Cl 2 (l)
Which of the following is the condensed electron configuration for chlorine? 3. [Ne]3s 2 3p 6 2. [Ne]3s 2 3p 5 1. [Ne]3p 7 4. [Ne]3s 2 3d 5 5. [Ne]3s 2 3p 3 3d 2 Cl 2 (g) Cl 2 (l)
Which of the following is the condensed electron configuration for bismuth? [Xe] accounts for 54 electrons. 1. [Xe]6s 2 4f 14 5d 10 6p 3 2. [Xe]6s 2 6f 14 6d 10 6p 3 3. [Xe]5s 2 4f 14 4d 10 5p 3 4. [Xe]6s 2 4f 12 4d 10 6p 5 5. [Xe]5s 2 4f 12 4d 10 5p 5
Which of the following is the condensed electron configuration for bismuth? [Xe] accounts for 54 electrons. 1. [Xe]6s 2 4f 14 5d 10 6p 3 2. [Xe]6s 2 6f 14 6d 10 6p 3 3. [Xe]5s 2 4f 14 4d 10 5p 3 4. [Xe]6s 2 4f 12 4d 10 6p 5 5. [Xe]5s 2 4f 12 4d 10 5p 5
Which of the following is the condensed electron configuration for copper? [Xe] accounts for 54 electrons. 1. [Ar]3s 2 3d 9 2. [Ar]4s 2 2d 9 3. [Ar]3s 1 4d [Ar]4s 1 4d [Ar]4s 1 3d 10
Which of the following is the condensed electron configuration for copper? [Xe] accounts for 54 electrons. 1. [Ar]3s 2 3d 9 2. [Ar]4s 2 2d 9 3. [Ar]3s 1 4d [Ar]4s 1 4d [Ar]4s 1 3d 10