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Take a guess. What do you think is a likely ground-state electron configuration for the sodium ion, Na+, formed by loss of an electron from a neutral sodium atom?
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Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.6 - Ionic Compounds: Periodic Trends and Bonding TheoryProblema 104c
McMurry 8th EditionCh.6 - Ionic Compounds: Periodic Trends and Bonding TheoryProblema 104cCapitolo 6, Problema 104c
Iron is commonly found as Fe, Fe2++, and Fe3+. (c) The third ionization energy of Fe is Ei3 = +2952 kJ/mol. What is the longest wavelength of light that could ionize Fe2+(g) to Fe3+(g)?
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Identify the process: The problem involves the ionization of Fe^{2+} to Fe^{3+}, which requires the third ionization energy, E_{i3}.
Use the relationship between energy and wavelength: The energy of a photon is related to its wavelength by the equation E = \(\frac{hc}{\lambda}\), where E is the energy, h is Planck's constant (6.626 \(\times\) 10^{-34} \(\text{ J s}\)), c is the speed of light (3.00 \(\times\) 10^8 \(\text{ m/s}\)), and \(\lambda\) is the wavelength.
Convert the ionization energy from kJ/mol to J/photon: Since the ionization energy is given per mole, convert it to energy per photon by dividing by Avogadro's number (6.022 \(\times\) 10^{23} \(\text{ mol}\)^{-1}).
Rearrange the equation to solve for wavelength: \(\lambda\) = \(\frac{hc}{E}\). Substitute the values for h, c, and the energy per photon into this equation.
Calculate the wavelength: Perform the calculation to find the longest wavelength of light that can ionize Fe^{2+} to Fe^{3+}.
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Ionization Energy
Ionization energy is the energy required to remove an electron from an atom or ion in the gas phase. For Fe<sup>2+</sup>, the ionization energy to form Fe<sup>3+</sup> is significant because it indicates how much energy is needed to overcome the attraction between the positively charged nucleus and the negatively charged electron. The third ionization energy of Fe, given as +2952 kJ/mol, provides a reference for understanding the energy required for this specific transition.
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01:19
Ionization Energy
Photon Energy and Wavelength Relationship
The energy of a photon is inversely related to its wavelength, described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. This relationship means that longer wavelengths correspond to lower energy photons. To find the longest wavelength capable of ionizing Fe<sup>2+</sup> to Fe<sup>3+</sup>, one must calculate the wavelength associated with the ionization energy of +2952 kJ/mol.
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00:31Frequency-Wavelength Relationship
Conversion of Energy Units
In chemistry, it is often necessary to convert energy units to work with different equations. Ionization energy is typically given in kJ/mol, while photon energy is expressed in joules. To use the ionization energy in the photon energy equation, one must convert kJ/mol to joules per photon by dividing the energy by Avogadro's number (6.022 x 10²³ mol<sup>-1</sup>). This conversion is crucial for accurately determining the corresponding wavelength of light.
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01:56Conversion Factors
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Domanda del libro di testo
The ionization energy of an atom can be measured by photo-electron spectroscopy, in which light of wavelength l is directed at an atom, causing an electron to be ejected. The kinetic energy of the ejected electron 1EK2 is measured by determining its velocity, v since EK = 1/2 mv2. The Ei is then calculated using the relationship that the energy of the inci-dent light equals the sum of Ei plus EK.
(a) What is the ionization energy of rubidium atoms in kilo-joules per mole if light with l = 58.4 nm produces elec-trons with a velocity of 2.450 * 106m/s? (The mass of an electron is 9.109 * 10-31 kg.)
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Iron is commonly found as Fe, Fe2+, and Fe3+. (b) What are the n and l quantum numbers of the electron removed on going from Fe2+ to Fe3+?
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Order the following atoms according to increasing atomic radius: S, F, O.
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Consider the electronic structure of the element bismuth. (a) The first ionization energy of bismuth is Ei1 = +703 kJ/ mol. What is the longest possible wavelength of light that could ionize an atom of bismuth?
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