In J. J. Thompson’s experiment depicted in Figures 1.10 and 1.11, assume that the electrons are initially traveling at a speed of
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Chapter 1 Solutions
OWLv2 for Oxtoby/Gillis/Butler's Principles of Modern Chemistry, 8th Edition, [Instant Access], 1 term (6 months)
- Look up the van der Waals constants, b, for H2, N2, O2, and Cl2. Based on the periodic table, predict atomic radii for H, N, O, and Cl. Use these values to explain the sizes of the b constants.arrow_forwardDoes the main emission line for SrCl2 have a longer or shorter wavelength than that of the yellow line from NaCI?arrow_forwardW 4. (a) A laser emits light that has a frequency of 4.69 X 10¹4 s¹. What is the energy of one photon of this radiation? V (b) If the laser emits a pulse containing 5.0 X 1017 photons of this radiation, what is the total energy of that pulse? (c) If the laser emits 1.3 X 10-2 J of energy during a pulse, how many photons are emitted?arrow_forward
- What is the energy of photon that causes a hydrogen atom to undergo a transition from n-1→ n=2? State your answer in electronvolts (eV) (without units) to three significant figures. Note: 1 eV= 1.602 x 10-19 J.arrow_forward(A) A photon has a wavelength of 599 nm. Calculate the energy of the photon in joules. Enter your answer in scientific notation. (b) what is the wave length (in nm) of radiation that has an energy content of 9.53 x 103 kJ/mol? (B part 2) in which region of the electromagnetic spectrum is this radiation found? (c) what are the possible values for ml when the principal quantum number (n) is 2 and the angular momentum quantum number is 0?arrow_forwardWhen a hydrogen atom absorbs a photon of electromagnetic radiation (EMR), the internal energy of the atom increases and one or more electrons may be energized into an excited state. The release of this extra energy as the excited state electron transitions back to a lower energy state results in the emission of a photon. These energy changes are responsible for the emission spectrum of hydrogen (shown below) and are described by the Bohr equation. delta?=−2.178×10−18 J(1?2final−1?2initial)ΔE=−2.178×10−18 J(1nfinal2−1ninitial2) *refer to attached image before proceeding* To ionize a hydrogen atom (forming a hydrogen ion), requires that the energy absorbed is sufficient to send the energized electron an infinite distance away from the nucleus (as shown by the ionization line in the image above). In other words, nfinal is equal to infinity. Calculate the energy required to ionize a ground state hydrogen atom. Report your answer in kilojoules. delta E= ____kJ What is the longest…arrow_forward
- An EM wave has a wavelength of 1.54 angstroms. What is the frequency of this wave? What is the energy (in J) of one photons of this radiation? (1 angstrom = 1 x 10–10m exact, The Planck constant h = 6.626 x 10–34 J·s)arrow_forward(a) How does the Bohr model differ from the quantum mechanical model of the atom? Describe at least 2 differences.(b) Define each of the 4 quantum numbers (n, l, ml, ms) and what they physically represent about the orbital and/or electron.(d) How many quantum numbers are needed to completely define a specific orbital? Provide the quantum numbers for the 2s orbital.(d) How many quantum numbers are needed to completely define a specific electron? Provide the quantum numbers for the second electron to fill into a 2s orbital.arrow_forwardCompare the wavelengths of an electron (mass 9.11X10⁻³¹kg) and a proton (mass 1.67X10⁻²⁷kg), eachhaving (a) a speed of 3.4106m/s; (b) a kinetic energy of2.7X10¹⁵ J.arrow_forward
- Current theories of atomic structure suggest that all matter and all energy demonstrate both particle-like and wave-like properties under the appropriate conditions, although the wave-like nature of matter becomes apparent only in very small and very fast moving particles. The relationship between the wavelengths (A) observed for a particle and the mass and velocity of that particle is called the de Broglie relationship. It is λ = h my in which h is Planck's constant ( 6.63 x 10-34 J-s), rences] m represents the mass of the particle in kilograms, and v represents the velocity of the particle in meters per second. a. Calculate the de Broglie wavelength for an electron moving at 0.91 times the speed of light. Wavelength = b. Calculate the de Broglie wavelength for a 140. g ball moving at a speed of 10 m/s. Wavelength = c. Calculate the de Broglie wavelength for a 66 kg person walking at a speed of 6.0 km/h. Wavelength = m m marrow_forwardThe quantum numbers for the electron(s) in the valence shell of thallium (81TI) are: NOTE: the designation electron(s) with brackets around the s means that there might be only one: "electron" or there might be more than one: "electrons" O (6,1,-1,2) (6,1,0,½) (6,1,1,½) O (6,1,-1,12) O (6,0,0,±12) (6,1,-1,½) O (6,0,0,±½/2)arrow_forward1. A. A cornstalk grows from a seed that is watered and fertilized. Is this a physical or chemical change? Justify your answer. В. Calculate the number of molecules in 60.0 g of C6H12O6. C. Explain wave-particle duality of light. A hydrogen atom with its electron in the n=6 energy level emits a photon of IR light. Calculate (a) the change in energy of the atom and (b) the wavelength (in Å) of the photon. RH=2.18×10-18 J. D. Е. The wavelengths of two electromagnetic radiation is 800 nm and 300 nm, respectively. Which one have relatively higher energy? Justify your answer. F. Name three electromagnetic radiations, whose speed is the same.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co