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
PRINCIPLES OF MODERN CHEMISTRY-OWLV2
- 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_forwardWhat 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_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
- When 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_forwardThe electron volt (eV) is a convenient unit of energy for expressing atomic-scale energies. It is the amount of energy that an electron gains when subjected to a potential of 1 volt; 1 eV = 1.602 × 10–19 J. Using the Bohr model, determine the energy, in electron volts, of the photon produced when an electron in a hydrogen atom moves from the orbit withn= 5 to the orbit with n= 2. Show your calculationsarrow_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_forward
- Using Planck's constant as h = 6.63 × 10−34 J⋅s, what is the wavelength of a proton with a speed of 5.00 × 106 m/s? The mass of a proton is 1.66 × 10−27 kg. Remember to identify your data, show your work, and report the answer using the correct number of significant digits and units.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_forwardAn 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 container with 0.2450.245 L of water is placed in a microwave and radiated with electromagnetic energy with a wavelength of 10.510.5 cm. The temperature of the water rose by 69.969.9 °C. Calculate the number of photons that were absorbed by the water. Assume water has a density of 1.00 g⋅mL−11.00 g·mL−1 and a specific heat of 4.184 J⋅g−1⋅°C−14.184 J·g−1·°C−1. number of photons =__________________________________photonsarrow_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_forwardElectromagnetic radiation with a wavelength of 575 nm appears as yellow light to the human eye. If a laser emits 3.8 x 1016 photons of this energy in a pulse, what is the energy of the pulse in mJ?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