Predict which bond length will be the longest: C- F, C-I, C-Br.

Consider the noble gas xenon.

(a) Write the electron configuration of xenon using the abbreviation of the previous noble gas.

(b) When xenon absorbs 801 kJ/mol of energy, it is excited into a higher-energy state in which the outermost electron has been promoted to the next available subshell. Write the electron configuration for this excited xenon.

(c ) The energy required to completely remove the outermost electron from the excited xenon atom is 369 kJ/mol, almost identical to that of cesium 1376 kJ/mol2. Explain.

An energetically excited hydrogen atom has its electron in a 5 subshell. The electron drops down to the 3d subshell, releasing a photon in the process.

(a) Give the n and l quantum numbers for both subshells, and give the range of possible m$_l$ quantum numbers.

(b) What wavelength of light is emitted by the process?

(c ) The hydrogen atom now has a single electron in the 3d subshell. What is the energy in kJ/mol required to remove this electron?

How many nodal planes through the nucleus do you think a g orbital has?

A photon produced by an X ray machine has an energy of 4.70 X 10$^{-16}$ J.

(a) What is the frequency of the photon?

(b) What is the wavelength of radiation of frequency (a)?

(c ) What is the velocity of an electron with a de Broglie wavelength equal to (b)?

(d) What is the kinetic energy of an electron traveling at velocity (c )?

A minimum energy of 7.21 X 10$^{-19}$ J is required to produce the photoelectric effect in chromium metal.

(a) What is the minimum frequency of light needed to remove an electron from chromium?

(b) Light with a wavelength of 2.50 X 10$^{-7}$ m falls on a piece of chromium in an evacuated glass tube. What is the minimum de Broglie wavelength of the emitted electrons? (Note that the energy of the incident light must be conserved; that is, the photon’s energy must equal the sum of the energy needed to eject the electron plus the kinetic energy of the electron.)

A hydrogen atom with an electron in the first shell (n = 1) absorbs ultraviolet light with a wavelength of 1.03 X 10$^{-7}$ m. To what shell does the electron jump?

Given the subshells 1s, 2s, 2p, 3s, 3p, and 3d, identify those that meet the following descriptions:

(a) Has l = 2

(b) Can have m$_l$ = -1

(c ) Is empty in a nitrogen atom

(d) Is full in a carbon atom

(e) Contains the outermost electrons in a beryllium atom

(f) Can contain two electrons, both with spin m$_s$ = +1>2

Assume that the rules for quantum numbers are different and that the spin quantum number ms can have any of three values, m$_s$ = -1>2, 0, +1>2, while all other rules remain the same.

(a) Draw an orbital-filling diagram for the element with Z = 25,showing the individual electrons in the outermost sub shell as up arrows, down arrows, or 0. How many partially filled orbitals does the element have?

(b) What is the atomic number of the element in the third column of the fourth row under these new rules? What block does it belong to 1s, p, d, or f2?

In the Bohr model of atomic structure, electrons are constrained to orbit a nucleus at specific distances, given by the equation

$$r=\frac{n^2 a_0}{Z}$$

where $r$ is the radius of the orbit, $Z$ is the charge on the nucleus, $a_0$ is the Bohr radius and has a value of $5.292 \times 10^{-11} \mathrm{~m}$, and $n$ is a positive integer $(n=1,2,3, \ldots)$ like a principal quantum number. Furthermore, Bohr concluded that the energy level $E$ of an electron in a given orbit is

$$E=\frac{-Z e^2}{2 r}$$

where $e$ is the charge on an electron. Derive an equation that will let you calculate the difference $\Delta E$ between any two energy levels. What relation does your equation have to the Balmer-Rydberg equation?

The amount of energy necessary to remove an electron from an atom is a quantity called the ionization energy, E$_i$. This energy can be measured by a technique called 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 electro9n (E$_k$) is measured by determining its velocity, (v E$_k$) = mv$^{2}$/2),and E$_i$ is then calculated using the conservation of energy principle. That is, the energy of the incident light equals E$_i$ plus E$_k$.What is the ionization energy of selenium atoms in kilojoules per mole if light with $\lambda$ = 48.2 nm produces electrons with a velocity of 2.371 X 10$^{6}$ m/s? The mass, m, of an electron is 9.109 X 10$^{-31}$ kg.

Photochromic sunglasses, which darken when exposed to light, contain a small amount of colorless AgCl embedded in the glass. When irradiated with light, metallic silver atoms are produced and the glass darkens: AgCl $\rarr$ Ag + Cl. Escape of the chlorine atoms is prevented by the rigid structure of the glass, and the reaction therefore reverses as soon as the light is removed. If 310 kJ/mol of energy is required to make the reaction proceed, what wavelength of light is necessary?

Microwave ovens work by irradiating food with microwave radiation, which is absorbed and converted into heat. Assuming that radiation with l = 15.0 cm is used, that all the energy is converted to heat, and that 4.184 J is needed to raise the temperature of 1.00 g of water by 1.00 degree celcius, how many photons are necessary to raise the temperature of a 350 mL cup of water from 20 degree celcius to 95 degree celcius?

One watt 1W2 is equal to 1 J/s. Assuming that 5.0% of the energy output of a 75 W light bulb is visible light and that the average wavelength of the light is 550 nm, how many photons are emitted by the light bulb each second?