_.0 Consider four different types of electromagnetic radiation: microwaves, infrared, visible light, and gamma rays. Arrange the types of radiation from the lowest to the highest frequency, and from the highest to the lowest energy. ) Lowest frequency Highest energy Highest frequency Lowest energy Answer Bank Answer Bank microwaves visible light gamma rays microwaves infrared gamma rays infrared visible light ' Consider four different types of electromagnetic radiation: microwaves, infrared, visible light, and gamma rays. Arrange the types of radiation from the shortest to the longest wavelength, and from the lowest to the highest energy. Shortest wavelength Lowest energy Longest wavelength Highest energy Answer Bank Answer Bank microwaves gamma rays infrared microwaves visible light infrared visible light Classify each statement about electromagnetic radiation as true or false. True False Ultraviolet radiation is lower in energy than infrared radiation. The speed of electromagnetic radiation varies with wavelength. Visible light has a lower frequency than infrared radiation. The light from the sun includes multiple types of electromagnetic radiation. Blue light has shorter wavelengths than red light. If the frequency of a wave increases by some factor, the wavelength of that wave decreases by the same factor. 3 The energy of a photon is related to its frequency through the following equation E = hv Where E is the energy, h is Planck's constant, and v is the frequency. Rearrange the equation to solve for v. y: A photon has an energy of 3 .45 x 10'19 J. What is the frequency of the photon? 3 The energy of a photon is related to its wavelength through the following equation hC E=l1 where E is the energy, [2 is Planck's constant, c is the speed of light, and A is the wavelength. Rearrange the equation to solve for 11. A photon has an energy of 4.63 x 10'19 J. What is the wavelength of the photon? Determine the frequency and energy for light with a wavelength of 717.2 nm. What is the color of light with a wavelength of 717.2 nm? Refer to the electromagnetic spectrum as needed. Determine the wavelength and energy for light with a frequency of 5.823 x 1014 s"1 . Ll What is the color of light with a frequency of 5.823 x 1014 s"1 ? Refer to the electromagnetic spectrum as needed. Determine the frequency and energy for yellow light with a wavelength of 578.2 nm. Determine the wavelength and frequency for light with energy of 253.6 kJ/mol. ... What is the color of light with energy of 253.6 kJ/mol? Refer to the electromagnetic spectrum as needed. I ' | green orange red yellow violet blue EM Spectrum Electromagnetic Spectrum Increasing wavelength Increasing energy 10-11 10-10 10-9 10 8 10-7 10 6 10-5 10 4 10-3 10-2 10-1 101 102 103 Wavelength (m) Gamma X rays Ultra- violet Infrared Microwaves Radio rays Frequency (s-1) 1020 1019 1018 1017 1016 1015 1014 1013 1012 1011 1010 109 108 107 106 105 104 Visible 400 500 600 700 750 nm @Sapling LearningWhen an electron in a hydrogen atom is in the n = 3 state, is it on average closer to, farther from, or the same distance to the nucleus than in the ground state? 0 the same 0 farther O closer Does it take more, less, or the same amount of energy to ionize a hydrogen atom (eject an electron) in the n = 3 state than one in which the electron is in the ground state? 0 the same - atom, classify the electron transitions according to whether they result in the absorption or emission ! Absorption Emission n=2ton=1, 'n=3ton=2] [n=3ton=5, 'n=1ton=3 Ignoring sign, which transition is associated with the greatest energy change? On=3ton=2 On=2ton=1 On=3ton=5 On=1ton=3 The Lyman series results from transitions of the electron in hydrogen in which the electron ends at the n = 1 energy level. Using the Rydberg formula for the Lyman series, calculate the wavelength 12.51 of the photon emitted in the transition '12 1 = I: nm from the n = 2 energy state. Give an answer in units of nanometers (nm). Identify the band of radiation from the electromagnetic spectrum to which the 212.,1 photon belongs. O infrared O visible light 0 ultraviolet 0 X-ray Using the Rydberg formula for the Lyman series, calculate the wavelength 114.,1 of the photon emitted in the transition it _ : nrn 4:1 from the n = 4 energy state. Give an answer in units of nanometers (11m). Identify the band of radiation from the electromagnetic spectrum to which the A461 photon belongs. O infrared O visible light 0 ultraviolet 0 Xray 9 Consider a hydrogen atom in the ground state. What is the energy of its electron? m II '1 Calculate the energy of a photon emitted when an electron in a hydrogen atom undergoes a transition from n = 4 to n = 1. energy emitted:Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level n = 3 to the level n = 1. #:11111 Calculate the frequency of the n = 6 line in the Lyman series of hydrogen. In what region of the electromagnetic spectrum is this line observed? G gamma 0 visible 0 infrared 0 Xray O ultraviolet 0 radio 0 microwave For each atom in its ground state, determine the number of electrons in each energy shell. If there are no electrons in an energy shell, enter a 0 for that shell. Na, energy shell 1: Na, energy shell 2: Na, energy shell 3: Na, energy shell 4: Al, energy shell 1: Al, energy shell 2: Al, energy shell 3: Al, energy shell 4: P, energy shell 1: P, energy shell 2:P, energy shell 3: P, energy shell 4: S, energy shell 1: S, energy shell 2: S, energy shell 3: S, energy shell 4: Ar, energy shell 1: Ar, energy shell 2: Ar, energy shell 3: Ar, energy shell 4:3 Enter the number of electrons in each energy level (shell) for each of the elements. If the energy level does not contain any electrons, enter a 0. It may help to refer to the periodic table. He: K: n = 1 n = 2 n = 3 n = 4 What is the neutral atom that has its first two energy levels filled, has 1 electron in its third energy level, and has no other electrons? Enter the name of the element, not the abbreviation. element name