An experiment called the Stern–Gerlach experiment helped establish the existence of electron spin. In this experiment, a beam of silver atoms is passed through a magnetic field, which deflects half of the silver atoms in one direction and half in the opposite direction. The separation between the two beams increases as the strength of the magnetic field increases. (c) Would this experiment work for a beam of fluorine (F) atoms?

What is the maximum number of electrons that can occupy each of the following subshells? a. 3p, b. 5d, c. 2s, d. 4f.

What is the maximum number of electrons in an atom that can have the following quantum numbers? a. n = 3, ml = -2; b. n = 4, l = 3; c. n = 5, l = 3, ml = 2; d. n = 4, l = 1, ml = 0.

(a) What are 'valence electrons'?

(b) What are 'core electrons'?

(c) What does each box in an orbital diagram represent?

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: a. nitrogen

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: c. chlorine

Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (a) Mg (b) Ge (c) Br (d) V (e) Y.

Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (f) Lu.

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (a) 1s²2s² (b) 1s²2s²2p⁴

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (c) 3Ar⁴4s¹3d⁵

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (d) 3Kr45s24d105p4.

The following do not represent valid ground-state electron configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled in order of increasing energy. Indicate which of these two principles is violated in each example. b. 3Xe46s25d4

The following electron configurations represent excited states. Identify the element and write its ground-state condensed electron configuration. (b) 3Ar44s13d104p25p1

Consider the two waves shown here, which we will consider to represent two electromagnetic radiations: (a) What is the wavelength of wave A?

Consider the two waves shown here, which we will consider to represent two electromagnetic radiations: (b) What is the frequency of wave A?

If you put 120 volts of electricity through a pickle, the pickle will smoke and start glowing orange-yellow. The light is emitted because sodium ions in the pickle become excited; their return to the ground state results in light emission. b. What is the energy of 1.00 mol of these photons? (A mole of photons is called an Einstein.)

Certain elements emit light of a specific wavelength when they are burned or heated in a non-luminous flame. Historically, chemists used such emission wavelengths to determine whether specific elements were present in a sample. Some characteristic wavelengths for a few of the elements are given in the following table:

Ag 328.1 nm Fe 372.0 nm

Au 267.6 nm K 404.7 nm

Ba 455.4 nm Mg 285.2 nm

Ca 422.7 nm Na 589.6 nm

Cu 324.8 nm Ni 341.5 nm

(c) When burned, a sample of an unknown substance is found to emit light of frequency 6.58 * 1014 s-1. Which of these elements is probably in the sample?

In August 2011, the Juno spacecraft was launched from Earth with the mission of orbiting Jupiter, arriving nearly five years later in July of 2016. The distance between the two planets varies depending on where each planet is in its orbit, but at the closest, the distance between Jupiter and Earth is 391 million miles. What is the minimum amount of time it takes for a transmitted signal from Juno to reach the Earth?

In an experiment to study the photoelectric effect, a scientist measures the kinetic energy of ejected electrons as a function of the frequency of radiation hitting a metal surface. She obtains the following plot. The point labeled 'n0' corresponds to light with a wavelength of 542 nm. (a) What is the value of n0 in s - 1?

Consider a transition in which the electron of a hydrogen atom is excited from n = 1 to n = ∞. (a) What is the end result of this transition?

Consider a transition in which the electron of a hydrogen atom is excited from n = 1 to n = ∞. (b) What is the wavelength of light that must be absorbed to accomplish this process?

Consider a transition in which the electron of a hydrogen atom is excited from n = 1 to n = ∞. (d) How are the results of parts (b) and (c) related to the plot shown in Exercise 6.88?

The human retina has three types of receptor cones, each sensitive to a different range of wavelengths of visible light, as shown in this figure (the colors are merely to differentiate the three curves from one another; they do not indicate the actual colors represented by each curve):

(c) Explain why the sky appears blue even though all wavelengths of solar light are scattered by the atmosphere.

The series of emission lines of the hydrogen atom for which nf = 3 is called the Paschen series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Paschen series are observed.

The series of emission lines of the hydrogen atom for which nf = 3 is called the Paschen series. (b) Calculate the wavelengths of the first three lines in the Paschen series—those for which ni = 4, 5, and 6.