22. The electron configurations described in this chapter all refer to gaseous atoms in their ground states. An atom may absorb a quantum of energy and promote one of its electrons to a higher-energy orbital. When this happens, we say that the atom is in an excited state. The electron configurations of some excited atoms are given. Identify these atoms and write their ground-state configurations: (a) 1s¹2s¹ (b) 1s²2s²2p²3d¹ (c) 1s²2s²2pº4s¹ (d) [Ar]4s¹3d¹º4p4 (e) [Ne] 3s²3p+3d¹ 23. Draw orbital diagrams for atoms with the following electron configurations: (a) 1s²2s²2p³ (b) 1s²2s²2p3s²3p³ (c) 1s 2s 2p 3s²3p 4s²3d" 24. If Rutherford and his coworkers had used electrons instead of alpha particles to probe the structure of the nucleus as described in Section 2.2, what might they have discovered? 25. Scientists have found interstellar hydrogen atoms with quantum number n in the hundreds. Calculate the wavelength of light emitted when a hydrogen atom undergoes a transition from n = 236 to n = 235. In what region of the electromagnetic spectrum does this wavelength fall? 26. Calculate the wavelength of a helium atom whose speed is equal to the root-mean-square speed at 20°C. 27. Ionization energy is the minimum energy required to remove an electron from an atom. It is usually ex- pressed in units of kJ/mol, that is, the energy in kilo- joules required to remove one mole of electrons from one mole of atoms. (a) Calculate the ionization energy for the hydrogen atom. (b) Repeat the calculation, assuming in this second case that the electrons are removed from the n = 2 state.
22. The electron configurations described in this chapter all refer to gaseous atoms in their ground states. An atom may absorb a quantum of energy and promote one of its electrons to a higher-energy orbital. When this happens, we say that the atom is in an excited state. The electron configurations of some excited atoms are given. Identify these atoms and write their ground-state configurations: (a) 1s¹2s¹ (b) 1s²2s²2p²3d¹ (c) 1s²2s²2pº4s¹ (d) [Ar]4s¹3d¹º4p4 (e) [Ne] 3s²3p+3d¹ 23. Draw orbital diagrams for atoms with the following electron configurations: (a) 1s²2s²2p³ (b) 1s²2s²2p3s²3p³ (c) 1s 2s 2p 3s²3p 4s²3d" 24. If Rutherford and his coworkers had used electrons instead of alpha particles to probe the structure of the nucleus as described in Section 2.2, what might they have discovered? 25. Scientists have found interstellar hydrogen atoms with quantum number n in the hundreds. Calculate the wavelength of light emitted when a hydrogen atom undergoes a transition from n = 236 to n = 235. In what region of the electromagnetic spectrum does this wavelength fall? 26. Calculate the wavelength of a helium atom whose speed is equal to the root-mean-square speed at 20°C. 27. Ionization energy is the minimum energy required to remove an electron from an atom. It is usually ex- pressed in units of kJ/mol, that is, the energy in kilo- joules required to remove one mole of electrons from one mole of atoms. (a) Calculate the ionization energy for the hydrogen atom. (b) Repeat the calculation, assuming in this second case that the electrons are removed from the n = 2 state.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter6: The Periodic Table And Atomic Structure
Section: Chapter Questions
Problem 13CO: • identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.
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![22. The electron configurations described in this chapter
all refer to gaseous atoms in their ground states. An
atom may absorb a quantum of energy and promote
one of its electrons to a higher-energy orbital. When
this happens, we say that the atom is in an excited
state. The electron configurations of some excited
atoms are given. Identify these atoms and write their
ground-state configurations:
(a) 1s¹2s¹
(b) 1s²2s²2p²3d¹
(c) 1s²2s²2pº4s¹
(d) [Ar]4s¹3d¹º4p4
(e) [Ne] 3s²3p+3d¹
23. Draw orbital diagrams for atoms with the following
electron configurations:
(a) 1s²2s²2p³
(b) 1s²2s²2p3s²3p³
(c) 1s 2s 2p 3s²3p 4s²3d"
24. If Rutherford and his coworkers had used electrons
instead of alpha particles to probe the structure of the
nucleus as described in Section 2.2, what might they
have discovered?
25. Scientists have found interstellar hydrogen atoms with
quantum number n in the hundreds. Calculate the
wavelength of light emitted when a hydrogen atom
undergoes a transition from n = 236 to n = 235. In
what region of the electromagnetic spectrum does this
wavelength fall?
26. Calculate the wavelength of a helium atom whose
speed is equal to the root-mean-square speed at
20°C.
27. Ionization energy is the minimum energy required to
remove an electron from an atom. It is usually ex-
pressed in units of kJ/mol, that is, the energy in kilo-
joules required to remove one mole of electrons from
one mole of atoms. (a) Calculate the ionization energy
for the hydrogen atom. (b) Repeat the calculation,
assuming in this second case that the electrons are
removed from the n = 2 state.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4328c9cc-6fa0-407f-9af0-e59e5fb1715c%2F7c371498-1781-4d55-8dfc-a63a642fb488%2F3ezen6k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:22. The electron configurations described in this chapter
all refer to gaseous atoms in their ground states. An
atom may absorb a quantum of energy and promote
one of its electrons to a higher-energy orbital. When
this happens, we say that the atom is in an excited
state. The electron configurations of some excited
atoms are given. Identify these atoms and write their
ground-state configurations:
(a) 1s¹2s¹
(b) 1s²2s²2p²3d¹
(c) 1s²2s²2pº4s¹
(d) [Ar]4s¹3d¹º4p4
(e) [Ne] 3s²3p+3d¹
23. Draw orbital diagrams for atoms with the following
electron configurations:
(a) 1s²2s²2p³
(b) 1s²2s²2p3s²3p³
(c) 1s 2s 2p 3s²3p 4s²3d"
24. If Rutherford and his coworkers had used electrons
instead of alpha particles to probe the structure of the
nucleus as described in Section 2.2, what might they
have discovered?
25. Scientists have found interstellar hydrogen atoms with
quantum number n in the hundreds. Calculate the
wavelength of light emitted when a hydrogen atom
undergoes a transition from n = 236 to n = 235. In
what region of the electromagnetic spectrum does this
wavelength fall?
26. Calculate the wavelength of a helium atom whose
speed is equal to the root-mean-square speed at
20°C.
27. Ionization energy is the minimum energy required to
remove an electron from an atom. It is usually ex-
pressed in units of kJ/mol, that is, the energy in kilo-
joules required to remove one mole of electrons from
one mole of atoms. (a) Calculate the ionization energy
for the hydrogen atom. (b) Repeat the calculation,
assuming in this second case that the electrons are
removed from the n = 2 state.
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