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One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (b) Determine the initial and final values of n associated with this emission.

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One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (a) In what region of the electromagnetic spectrum is this emission found?

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State whether the following is ionic or molecular: (h) N2O4

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State whether the following is ionic or molecular: (g) CoCO3

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State whether the following is ionic or molecular: (f) LaP

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Predict whether each of the following compounds is molecular or ionic: (h) Ag2SO4

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Predict whether each of the following compounds is molecular or ionic: (g) NF3

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Predict whether each of the following compounds is molecular or ionic: (f) NOCl

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For each of the following electronic transitions in the hydrogen atom, calculate the energy, frequency, and wavelength of the associated radiation, and determine whether the radiation is emitted or absorbed during the transition: (c) from n = 3 to n= 6. Does any of these transitions emit or absorb visible light?

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For each of the following electronic transitions in the hydrogen atom, calculate the energy, frequency, and wavelength of the associated radiation, and determine whether the radiation is emitted or absorbed during the transition: (b) from n = 5 to n = 2

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Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from n = 2 to n = 6

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Is energy emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from n = 4 to n = 2

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Sodium metal requires a photon with a minimum energy of 4.41 x 10 -19 J to emit electrons. (d) What is the maximum number of electrons that can be freed by a burst of light whose total energy is 1 .00 μJ?

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Sodium metal requires a photon with a minimum energy of 4.41 x 10 -19 J to emit electrons. (c) If sodium is irradiated with light of 439 nm, what is the maximum possible kinetic energy of the emitted electrons?

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Sodium metal requires a photon with a minimum energy of 4.41 x 10 -19 J to emit electrons. (b) What is the wavelength of this light?

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Sodium metal requires a photon with a minimum energy of 4.41 x 10 -19 J to emit electrons. (a) What is the minimum frequency of light necessary to emit electrons from sodium via the photoelectric effect?

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Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (c) If molybdenum is irradiated with light of wavelength of 120 nm, what is the maximum possible kinetic energy of the emitted electrons?

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Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (b) What wavelength of radiation will provide a photon of this energy?

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Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (a) What is the minimum energy needed to eject an electron?

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A stellar object is emitting radiation at 3.55 mm. (a) What type of electromagnetic spectrum is this radiation?

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A diode laser emits at a wavelength of 987 nm. (a) In what portion of the electromagnetic spectrum is this radiation found?

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The energy from radiation can be used to cause the rupture of chemical bonds. A minimum energy of 941 kJ/mol is required to break the nitrogen–nitrogen bond in N2. What is the longest wavelength of radiation that possesses the necessary energy to break the bond? What type of electromagnetic radiation is this?

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One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 325 nm. (d) These UV photons can break chemical bonds in your skin to cause sunburn—a form of radiation damage. If the 325-nm radiation provides exactly the energy to break an average chemical bond in the skin, estimate the average energy of these bonds in kJ/mol.

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One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 325 nm. (c) How many photons are in a 1.00 mJ burst of this radiation?

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One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 325 nm. (b) What is the energy of a mole of these photons?

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