Concept explainers
(a)
Interpretation:
The IR absorption frequency of a typical
Concept introduction:
Carbon-deuterium bond is much like a carbon-hydrogen bond. They have similar stiffness which is measured by the spring constant. Due to the extra neutron, the deuterium atom has approximately twice the mass of a hydrogen atom.
The IR absorption frequency of a bond is proportional to
(b)
Interpretation:
The
Concept introduction:
Carbon-deuterium bond is much like a carbon-hydrogen bond. They have similar stiffness which is measured by the spring constant. Due to the extra neutron, the deuterium atom has approximately twice the mass of a hydrogen atom.
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Chapter 12 Solutions
Organic Chemistry (9th Edition)
- CO absorbs energy in the microwave region of the spectrum at 1.153 x 105 MHz. This absorption can be attributed to J=0 to J=1 transition. If the absorption is attributed to CO molecules containing the isotopes C¹2 and O¹6. What is the bond length?arrow_forwardFor molecules of similar size and number of atoms, those with double and triple bonds have smaller S than molecules with only single bonds. Why? O molecules with single bonds are larger than molecules with multiple-bonds O molecules with multiple bonds are more rigid and have less freedom of motion molecules with single bonds can move faster than those with multiple bonds molecules with multiple bonds have more vibrational energy than those with single bonds all of the statements above explain the given observationarrow_forwardWhat requirements must be met for a molecule to absorb IR radiation?arrow_forward
- 1. Neutrons as well as electrons and x-rays can be used to obtain information about molecular structure through diffraction patterns. What must the velocity of a neutron be for its de Broglie wavelength to be about five times smaller than a bond length? How does this velocity compare (bigger, smaller, or the same) if electrons were diffracted? A typical bond length for C-C is 1.54Å (1.54 x 10-1ºm).arrow_forwardWhat is the maximum strength of a bond, in kJ>mol, that can be brokenby absorption of a photon of 420-nm light?arrow_forwardIt takes 151./kJmol to break an iodine-iodine single bond. Calculate the maximum wavelength of light for which an iodine-iodine single bond could be broken by absorbing a single photon. Be sure your answer has the correct number of significant digits.arrow_forward
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- A bond vibration has a frequency of 8.52x1013 Hz. a. What is the energy associated with this transition?b. What is the wavelength of this transition, in microns?arrow_forwardSelect the factor that does not directly affect the frequency of a band in an infrared, IR, spectrum. the electronegativity difference between the two atoms in the bond the strength of the bond the masses of the two atoms in the bond the type of vibration that is inducedarrow_forward4.) The dissociation energy of a carbon-bromine bond is typically about 276 KJ/mol. What is the maximum wavelength of photons that cause C---- Br bonds dissociation? and which kind of electromagnetic radiation--ultraviolet, visible, or infrared--does the wavelength you calculated correspond to? Group of answer choices A) 435 nm; Blue visible light B) 570 nm; Green/yellow visible light C) 7.2 x 10-31 m; gamma rays D) 435 nm; Red visible lightarrow_forward
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