The ionization energy is the energy needed to remove an electron from an atom. For hydrogen in the ground state this corresponds to raising the electron from n=1 to an orbit that has n=?. What is the energy needed to remove the electron from a hydrogen atom (in J) and what is the wavelength of that radiation (in nm)? Solve for the absolute change in energy, |?E| from n = 1 to n=?: use En = -B/nĀ² where B = 2.179 x 10?Ā¹? J Next convert the energy to wavelength using E = hc/? where Planckās constant: h=6.6262 x 10?Ā³? J s and speed of light: c=2.998 x 10?m/s
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179 \times 10^{-18} \, J \) and \( n = 1 \). Plugging in the values, we get: \[ \Delta E = \frac{2.179 \times 10^{-18} \, J}{1^2} = 2.179 \times 10^{-18} \, J \] Show moreā¦
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The ionization energy of an atom can be measured by photoelectron spectroscopy, in which light of wavelength $\lambda$ is directed at an atom, causing an electron to be ejected. The kinetic energy of the ejected electron $\left(E_{\mathrm{K}}\right)$ is measured by determining its velocity, $v_{y}$ since $E_{\mathrm{K}}=1 / 2 m v^{2}$. The $E_{\mathrm{i}}$ is then calculated using the relationship that the energy of the incident light equals the sum of $E_{i}$ plus $E_{\mathrm{K}}$ (a) What is the ionization energy of rubidium atoms in kilojoules per mole if light with $\lambda=58.4 \mathrm{~nm}$ produces electrons with a velocity of $2.450 \times 10^{6} \mathrm{~m} / \mathrm{s}$ ? (The mass of an electron is $9.109 \times 10^{-31} \mathrm{~kg}$.) (b) What is the ionization energy of potassium in kilojoules per mole if light with $\lambda=142 \mathrm{~nm}$ produces electrons with a velocity of $1.240 \times 10^{6} \mathrm{~m} / \mathrm{s} ?$
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The ionization energy of an atom can be measured by photo electron spectroscopy, in which light of wavelength $\lambda$ is directed at an atom, causing an electron to be ejected. The kinetic energy of the ejected electron $\left(E_{K}\right)$ is measured by determining its velocity, $v,$ since $E_{K}=1 / 2 mv^{2} .$ The $E_{i}$ is then calculated using the relationship that the energy of the incident light equals the sum of $E_{i}$ plus $E_{K}$. (a) What is the ionization energy of rubidium atoms in kilo joules per mole if light with $\lambda=58.4 nm$ produces electrons with a velocity of $2.450 \times 10^{6} m/s?$ (The mass of an electron is $9.109 \times 10^{-31} kg.$ ) (b) What is the ionization energy of potassium in kilo joules per mole if light with $\lambda=142 nm$ produces electrons with a velocity of $1.240 \times 10^{6} m/ s ?$
Ionization involves completely removing an electron from an atom. How much energy is required to ionize a hydrogen atom in its ground (or lowest energy) state? What wavelength of light contains enough energy in a single photon to ionize a hydrogen atom?
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