Chem 1201 HW Ch. 6 p 2

Part A Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen.

Using equation E=(hcRH)(1n2)=(−2.18×10−18J)(1n2), calculate the energy of an electron in the hydrogen atom when n=2.

Using equation E=(hcRH)(1n2)=(−2.18×10−18J)(1n2), calculate the energy of an electron in the hydrogen atom when n= 5.

Calculate the wavelength of the radiation released when an electron moves from n= 5 to n=2.

Is this line in the visible region of the electromagnetic spectrum?

If so, what color is it?

One of the emission lines of the hydrogen atom has a wavelength of 93.07 nm. In what region of the electromagnetic spectrum is this emission found?

Determine the initial value of n associated with this emission.

Determine the final value of n associated with this emission.

Place the following transitions of the hydrogen atom in order from longest to shortest wavelength of the photon emitted. Rank from longest to shortest wavelength. To rank items as equivalent, overlap them.

Calculate the de Broglie wavelength associated with a muon traveling at a velocity of 8.25×105 cm/s

Which one of the following represents an impossible set of quantum numbers for an electron in an atom? (arranged as n, l, m l , and ms)

Classify the following statements as either true or false.

Give the numerical value of n corresponding to 3p.

Give the numerical value of l corresponding to 3p.

Give the numerical value of n corresponding to 2s.

Give the numerical value of l corresponding to 2s.

Give the numerical value of n corresponding to 4f.

Give the numerical value of l corresponding to 4f.

Give the numerical value of n corresponding to 5d.

Give the numerical value of l corresponding to 5d.

What is the azimuthal quantum number (also called the angular-momentum quantum number), ℓ, for the orbital shown here? Express your answer numerically as an integer.

What is the label for the orbital shown here that indicates the type of orbital and its orientation in space? Express your answer using appropriate letters (e.g., px). Do not include the energy level n.

Compare the orbital shown in Parts A and B to the orbital shown here in size, shape, and orientation. Which quantum number(s) would be different for these two orbitals?

How would the dx2−y2 orbital in the n=5 shell compare to the dx2−y2 orbital in the n=3 subshell? A. The contour of the orbital would extend further out along the x and y axes. B. The value of ℓ would increase by 2. C. The radial probability function would include two more nodes. D. The orientation of the orbital would be rotated 45∘ along the xy plane. E. The mℓ value would be the same. Drag the appropriate items to their respective bins.

A three-dimensional plot of the wave function squared (ψ2) produces a diagram showing the probability density for an electron as a function of distance from the nucleus. These solutions are called orbitals. Three solutions to ψ2 are plotted here. Identify the orbital shown in each plot.

The probability of finding an electron at a point in an atom is referred to as the probability density (ψ2). The spatial distribution of these densities can be derived from the radial wave function R(r) and angular wave function Y(θ,ϕ), then solving the Schrödinger equation for a specific set of quantum numbers. Which of the following statements about nodes and probability density are accurate?

The probability of finding an electron anywhere in a spherical radius of r is called the radial probability distribution. The shape of the plot depends on the principal quantum number (n) and the azimuthal quantum number (ℓ) for an orbital. As n increases for each value of ℓ, the number of nodes in the plot increases by one. To understand the radial distribution function for different orbitals, match the orbital that corresponds to the radial distribution function shown in each plot. Identify the radial distribution functions by dragging the appropriate orbitals to their respective targets.

Classify each orbital diagram for ground-state electron configurations by the rule or principle it violates. Drag the appropriate items to their respective bins.

The following sets of quantum numbers, listed in the order n, ℓ, mℓ, and ms, were written for the last electrons added to an atom. Identify which sets are valid and classify the others by the rule or principle that is violated. Drag the appropriate items to their respective bins.

Complete an orbital diagram for boron. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all.

Complete an orbital diagram for scandium (Sc). Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all.

Electron configurations are a shorthand form of an orbital diagram, describing which orbitals are occupied for a given element. For example, 1s22s22p1 is the electron configuration of boron. Use this tool to generate the electron configuration of arsenic (As).

Write the condensed electron configurations for the Ca atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

Write the condensed electron configurations for the Sn atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

Write the condensed electron configurations for the Br atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

Write the condensed electron configurations for the V atom. Express your answer in condensed form as a series of orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

Write the condensed electron configurations for the Y atom.

Write the condensed electron configurations for the Lu atom.

Indicate how many unpaired electrons each atom has. Drag the appropriate items to their respective bins

Identify which sets of quantum numbers are valid for an electron. Each set is ordered (n,ℓ,mℓ,ms). Check all that apply.

Identify the sets of quantum numbers that describe all the electrons in the ground state of a neutral beryllium atom, Be. Each set is ordered (n,ℓ,mℓ,ms).

1s^2 2s^2 3s^2

[Xe]6s^2 5d^4

1s^2 2s^2 2p^6 3s^2 3d^5

For each set of elements represented in this periodic table outline, identify the principal quantum number, n, and the azimuthal quantum number, ℓ, for the highest energy electrons in an atom of one of those elements.

The black line between elements 56 and 71 in the periodic table shown indicates that in the Lanthanide series elements 57 through 70 are listed below the main table, while in the Actinide series elements 89-102 are listed below the main table. Elements 71 and 103 are listed in main table. Identify the outer electron configuration of each element shown in this periodic table outline.

Identify the general outer electron configuration for each group of elements shown in this periodic table outline.