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For hydrogen, the Lyman emission series is the collection of all photons emitted when an excited electron drops to the ground state. What are the 3 largest wavelengths in the Lyman series?

In hydrogen emission, a famous emission line called the H-alpha line occurs at a wavelength of 656.28 nm. Which hydrogen series is the H-alpha line a part of?
A) The Lyman series (nf = 1)
B) The Balmer series (nf = 2)
C) The Paschen series (nf = 3)
D) The Brackett series (nf = 4)

A photon of 2.28 eV is absorbed by an electron in hydrogen. What is the minimum energy level (n) that the electron can be in to be ionized by this photon?

An atom undergoes a transition from a state with energy - 3.0 eV to a state with energy - 9.0 eV. What is the wavelength of the photon emitted in this transition?

Determine the frequency of the fourth Lyman line (n = 5 to n = 1transition) using the figure below. What photon energy does that correspond to?

The electron orbiting a hydrogen atom has an excited energy of -0.85 eV. What's the largest energy photon that can be emitted by this electron?

Doubly ionized Lithium, Li2+, has an electron in the ground state. What frequency photon does it need to jump from the ground state to the n = 3 excited state?

What is the potential energy and kinetic energy of an electron in hydrogen in the n = 3 excited state?

An electron in hydrogen is in the n = 5 ground state when it decays to the ground state. Estimate the recoil speed of the atom after the electron drops to the ground state. Note that the mass of a proton is about 1.67x10-27 kg, and the mass of an electron is about 9.11x10-31 kg.

In the quantum mechanical description of a hydrogen atom, the electron is in a state that has orbital angular momentum √12ℏ. What is the maximum possible ionization energy of this state of the atom?
A) 0.378 eV
B) 0.544 eV
C) 0.850 eV
D) 1.51 eV
E) 3.40 eV
F) none of the above answers

The nucleus 2612Mg has a radius of approximately 3.55 fm. Which of the following nuclei has a radius approximately twice as large?
A) 5224Cr
B) 15296Cm
C) 136C
D) 32He
E) 20882Pb
F) none of the above answers

What is the longest wavelength light capable of ionizing a hydrogen atom in the n = 6 state?

The electron in the n = 5 orbital stays in then n = 5 orbital for 5 * 10 -10 s on average. Estimate the uncertainty of the proton energy from Heisenberg's uncertainty principle.

Consider the following diagram.
Say which arrows in the above diagram correspond to the following processes respectively: Absorption of a photon from the ground state to the first excited state; Emission of a photon from an excited state to another excited state.
1. Transition IV; Transition II
2. Transition I; Transition II
3. Transition IV; Transition III
4. Transition III; Transition IV
5. Transition II; Transition III
6. Transition I; Transition IV
7. Transition II; Transition IV
8. Transition III; Transition I
9. Transition III; Transition II
10. Transition I; Transition III

In the Bohr model description of a hydrogen atom, the atom is an state where the electron has angular momentum L = 4. What is the ionization energy of this state of the atom?A) 13.6 eVB) 3.40 eVC) 1.51 eVD) 0.850 eVE) 0.544 eVF) none of the above answers

An atom is in a state that has energy -8.60 eV. What is the energy of the atom after it absorbs a photon that has wavelength 400 nm?A) -3.10 eVB) -11.7 eVC) -5.50 eVD) -8.60 eVE) none of the above answers

The energy levels of a particular quantum object are −8.2 eV, −4.4 eV, and −1.8 eV. If a collection of these objects is bombarded by an electron beam so that there are some objects in each excited state, what are the energies of the photons that will be emitted?
1. 12.6 eV, 2.6 eV, 10 eV
2. 3.8 eV, 12.6 eV, 2.6 eV
3. −8.2 eV, −4.4 eV, −1.8 eV
4. 3.8 eV, 6.4 eV, 2.6 eV
5. 8.2 eV, −4.4 eV, −1.8 eV
6. −3.8 eV, −6.4 eV, −2.6 eV
7. 6.4 eV, −4.4 eV, 1.8 eV
8. 3.8 eV, 6.2 eV, 12.6 eV
9. 10 eV, −3.8 eV, 6.4 eV
10. 12.6 eV, 10 eV, 6.2 eV

A particle is described by a wave function Ψ(x) = Ae–αx2, where A and α are real, positive constants. If the value of a is increased, what effect does this have on (a) the particle's uncertainty in position and (b) the particle's uncertainty in momentum? Explain your answers.

(a) Derive planar density expressions for FCC (111) in terms of the atomic radius R. (b) Compute linear density value for this plane for aluminum.

(a) Derive planar density expressions for (100) in terms of the atomic radius R. (b) Compute linear density values for the plane for aluminum. (c) Consider the (100) plane in FCC: How many atoms are centered on the [100] In FCC?

1. How many electrons are contained in the atom 6Li?2. How many protons are contained in the atom 6Li?3. How many neutrons are contained in the atom 6Li?

Suppose you have 2.0 mol of O2 gas.How many coulombs of positive charge are contained in this gas in the atomic nuclei?Express your answer using two significant figures.

Which of the following observations led Bohr to formulate his model of the hydrogen atom? A) Neutrons form a diffraction pattern when scattered from a nickel crystal. B) The peak of blackbody radiation moves to shorter wavelengths as temperature increases. C) A low-density gas emits a series of sharp spectral lines. D) Electrons are observed to have wave nature.

Why do lithium, potassium, and sodium exhibit similar chemical properties?

Because the amount of screening of the nucleus is related to distance from the nucleus, the sand p subshells of a many-electron atom with the same value of n are not of equal energy, as they are in hydrogen. An electron in the p subshell has a lower probability of being inside the electrons of the n=1 shell than does an electron in the s subshell. Thus, the nucleus is screened somewhat more completely for electrons in the p subshell than for electrons in the ssubshell. This makes states in the p subshell of higher energy than states in the s subshell.The electron structure of an atom shows how many electrons are in each subshell. For instance, helium's electron structure is written 1s2, signifying the two electrons in the 1ssubshell. Neon, with ten electrons, has electron structure 1s22s22p6, signifying two electrons in the 1s subshell, two in the 2s subshell, and six in the 2p subshell. Observe that the exponents sum to the number of electrons in the atom.Which of the following is not a valid electron structure for an atom in its ground state? Use the fact that electrons fill the lowest energy states first and keep in mind the number of allowed states for each subshell.

Hydrogen gas absorbs light of wavelength 103nm. Afterward, what wavelengths are seen in the emission spectrum?

Consider the (100) plane in FCC: How many atoms are centered on the [100] In FCC?

A monochromatic laser is exciting hydrogen atoms from the n = 2 state to the n = 5 state. Eventually, all of the excited hydrogen atoms will emit photons until they fall back to the ground state. (a) How many different wavelengths can be observed in this process?(b) What is the shortest wavelength λmin observed?

A second important result is that electrons will fill the lowest energy states available. This would seem to indicate that every electron in an atom should be in the n=1 state. This is not the case, because of Pauli's exclusion principle. The exclusion principle says that no two electrons can occupy the same state. A state is completely characterized by the four numbers n, l, ml, and ms, where ms is the spin of the electron.An important question is, How many states are possible for a given set of quantum numbers? For instance, n=1 means that l=0 with ml=0 are the only possible values for those variables. Thus, there are two possible states: (1, 0, 0, 1/2) and (1, 0, 0, ?1/2). How many states are possible for n=2?Express your answer as an integer.

a) What is the angular momentum of a hydrogen atom in a 4p state? Give your answer as a multiple of h.b) What is the angular momentum of a hydrogen atom in a 5f state? Give you answer as a multiple of ?.

Describe how the structure of atoms would differ if the Pauli exclusion principle were not valid. What consequences would follow, both at the atomic level and at the world at large?

Are there transitions of higher or lower energy for hydrogen that we don't see?How may total transitions are there for hydrogen? Please provide at least one example.

Why do the balmer lines of hydrogen get closer together as you go towards shorter wavelengths?

The orbital angular momentum of an electron has a magnitude of 4.716 × 10–34 kg•m2/s. What is the angular-momentum quantum number l for this electron?

Which of the following gives the correct permitted values of ml for l=2?

Compared to the size of its nucleus, the size of an atom is about A) the same. B) ten times greater. C) a hundred times greater. D) a thousand times greater. E) one hundred thousand times greater

A liquidus line separates which of the following combinations of phase fields?α and Liquid + αLiquid + α and α+ βα and α+ βLiquid and Liquid + α

Which statements about a neutral atom are correct? Check all that apply.A. A neutral atom is composed of both positively and negatively charged particles.B. Positively charged protons are located in the tiny, massive nucleus.C. The positively charged particles in the nucleus are positrons.D. The negatively charged electrons are spread out in a "cloud" around the nucleus.E. The electrons are attracted to the positively charged nucleus.F. The radius of the electron cloud is twice as large as the radius of the nucleus.

Schroedinger equation:Express the energy of the particle E in terms of the wavenumber of the particle k.Express your answer in terms of wave number k, mass m, and Planck's constant divided by 2pi:h(barr).

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