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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

(a) When n = 4, ℓ = 2, and mℓ = −1, to what orbital type does this refer? (Give the orbital label, such as 1s.) (b) How many orbitals occur in the n = 5 electron shell? How many subshells?
A possible excited state of the H atom has the electron in a 4p orbital. List all possible sets of quantum numbers n, ℓ, and mℓ for this electron.
A possible excited state for the H atom has an electron in a 5d orbital. List all possible sets of quantum numbers n, ℓ, and mℓ for this electron.
How many subshells occur in the electron shell with the principal quantum number n = 4?
How many subshells occur in the electron shell with the principal quantum number n = 5?
Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom. (a) n = 2, ℓ = 2, mℓ = 0(b) n = 3, ℓ = 0, mℓ = −2(c) n = 6, ℓ = 0, mℓ = 1
Which of the following represent valid sets of quantum numbers? For a set that is invalid, explain briefly why it is not correct.(a) n = 3, ℓ = 3, mℓ = 0(b) n = 2, ℓ = 1, mℓ = 0(c) n = 6, ℓ
What is the maximum number of orbitals that can be identified by each of the following sets of quantum numbers? When “none” is the correct answer, explain your reasoning. (a) n = 3, ℓ = 0,
What is the maximum number of orbitals that can be identified by each of the following sets of quantum numbers? When “none” is the correct answer, explain your reasoning. (a) n = 4, ℓ = 3(b) n
Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom. In each case, change the incorrect value (or values) to make the set valid. (a) n = 4,
Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom. In each case, change the incorrect value (or values) to make the set valid. (a) n = 2,
State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
State which of the following orbitals cannot exist according to the quantum theory: 3p, 4s, 2f, and 1p. Briefly explain your answers.
Write a complete set of quantum numbers (n, ℓ, and mℓ) that quantum theory allows for each of the following orbitals: (a) 2p,(b) 3d, and (c) 4f.
Write a complete set of quantum numbers (n, ℓ, and mℓ) for each of the following orbitals: (a) 5f,(b) 4d, and(c) 2s.
A particular orbital has n = 4 and ℓ = 2. What must this orbital be:(a) 3p, (b) 4p,(c) 5d, or (d) 4d?
A given orbital has a magnetic quantum number of mℓ = −1. This could not be a(n)(a) f orbital (b) d orbital(c) p orbital(d) s orbital
How many nodal surfaces through the nucleus (planar nodes) are associated with each of the following orbitals?(a) 2s(b) 5d(c) 5f
How many nodal surfaces through the nucleus (planar nodes) are associated with each of the following atomic orbitals?(a) 4f (b) 2p (c) 6s
Which of the following are applicable when explaining the photoelectric effect? Correct any statements that are wrong. (a) Light is electromagnetic radiation.(b) The intensity of a light beam is
In what region of the electromagnetic spectrum for hydrogen is the Lyman series of lines found? The Balmer series?
Give the number of nodal surfaces through the nucleus (planar nodes) for each orbital type: s, p, d, and f.
Match the values of ℓ shown in the table with orbital type (s, p, d, or f). Value Orbital Type 3 O 1 2
What is the maximum number of s orbitals found in a given electron shell? The maximum number of p orbitals? Of d orbitals? Of f orbitals?
Sketch a picture of the 90% boundary surface of an s orbital and the px orbital. Be sure the latter drawing shows why the p orbital is labeled px and not py, for example. Orbital Type S d f Number
Excited H atoms have many emission lines. One series of lines, called the Pfund series, occurs in the infrared region. It results when an electron changes from higher energy levels to a level with n
An advertising sign gives off red light and green light. (a) Which light has higher-energy photons?(b) One of the colors has a wavelength of 680 nm, and the other has a wavelength of 500 nm. Which
Radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. It is this radiation that causes dyes to fade and your skin to develop a sunburn. If you are bombarded with
A cell phone sends signals at about 850 MHz (where 1 MHz = 1 × 106 Hz or cycles per second). (a) What is the wavelength of this radiation? (b) What is the energy of 1.0 mol of photons with a
Assume your eyes receive a signal consisting of blue light, λ = 470 nm. The energy of the signal is 2.50 × 10−14 J. How many photons reach your eyes?
If sufficient energy is absorbed by an atom, an electron can be lost by the atom and a positive ion formed. The amount of energy required is called the ionization energy. In the H atom, the
Rank the following orbitals in the H atom in order of increasing energy: 3s, 2s, 2p, 4s, 3p, 1s, and 3d.
How many orbitals correspond to each of the following designations? (a) 3p (b) 4p (c) 4px (d) 6d (e) 5d (f) 5f (g) n = 5 (h) 7s
Cobalt-60 is a radioactive isotope used in medicine for the treatment of certain cancers. It produces β particles and γ rays, the latter having energies of 1.173 and 1.332 MeV. (1 MeV = 106
Exposure to high doses of microwaves can cause tissue damage. Estimate how many photons, with λ = 12 cm, must be absorbed to raise the temperature of your eye by 3.0°C. Assume the mass of an eye is
When the Sojourner spacecraft landed on Mars in 1997, the planet was approximately 7.8 × 107 km from Earth. How long did it take for the television picture signal to reach Earth from Mars?
Answer the following questions as a summary quiz on this chapter. (a) The quantum number n describes the __________ of an atomic orbital, and the quantum number ℓ describes its __________. (b)
Answer the following questions as a summary quiz on the chapter. (a) The quantum number n describes the __________ of an atomic orbital.(b) The shape of an atomic orbital is given by the quantum
The most prominent line in the emission spectrum of chromium is found at 425.4 nm. Other lines in the chromium spectrum are found at 357.9 nm, 359.3 nm, 360.5 nm, 427.5 nm, 429.0 nm, and 520.8 nm.(a)
A large pickle is attached to two electrodes, which are then attached to a 110-V power supply. As the voltage is increased across the pickle, it begins to glow with a yellow color. Knowing that
For an electron in a hydrogen atom, calculate the energy of the photon emitted when an electron falls in energy from the n = 5 level to the n = 2 state. What are the frequency and wavelength of this
The spectrum shown here is for aspirin. The vertical axis is the amount of light absorbed, and the horizontal axis is the wavelength of incident light (in nm). What is the frequency of light with a
The infrared spectrum for methanol, CH3OH, is illustrated below. It shows the amount of light in the infrared region that methanol transmits as a function of wavelength. The vertical axis is the
Bohr pictured the electrons of the atom as being located in definite orbits about the nucleus, just as the planets orbit the Sun. Criticize this model.
Light is given off by a sodium- or mercury-containing streetlight when the atoms are excited. The light you see arises for which of the following reasons?(a) Electrons are moving from a given energy
How do we interpret the physical meaning of the square of the wavefunction? What are the units of 4πr2ψ2?
What does “wave–particle duality” mean? What are its implications in our modern view of atomic structure?
Which of these are observable? (a) Position of an electron in an H atom(b) Frequency of radiation emitted by H atoms(c) Path of an electron in an H atom(d) Wave motion of electrons(e) Diffraction
A photon with a wavelength of 93.8 nm strikes a hydrogen atom, and light is emitted by the atom. How many emission lines would be observed? At what wavelengths? Explain briefly (see Figure 6.10).Data
In principle, which of the following can be determined?(a) The energy of an electron in the H atom with high precision and accuracy(b) The position of a high-speed electron with high precision and
Suppose you live in a different universe where a different set of quantum numbers is required to describe the atoms of that universe. These quantum numbers have the following rules:N, principal 1, 2,
Figure 6.12b shows the probability of finding a hydrogen 1s electron at various distances from the nucleus. To create the graph in this figure, the electron cloud is first divided into a series of
The radioactive element technetium is not found naturally on Earth; it must be synthesized in the laboratory. It is a valuable element, however, because it has medical uses. For example, the element
Explain why you could or could not measure the wavelength of a golf ball in flight.
Write the electron configurations for P and Cl using both spdf notation and orbital box diagrams. Describe the relationship between each atom’s electron configuration and its position in the
Write the electron configurations for Mg and Ar using both spdf notation and orbital box diagrams. Describe the relationship of the atom’s electron configuration to its position in the periodic
Using spdf notation, write the electron configurations for atoms of chromium and iron, two of the major components of stainless steel.
Using spdf notation, give the electron configuration of vanadium, V, an element found in some brown and red algae and some toadstools.
Depict the electron configuration for each of the following atoms using spdf and noble gas notations. (a) Arsenic, As. A deficiency of As can impair growth in animals, and larger amounts are
Use noble gas and spdf notations to depict electron configurations for the following metals of the third transition series.(a) Tantalum, Ta. The metal and its alloys resist corrosion and are often
The lanthanides, once called the rare earth elements, are really only “medium rare.” Using noble gas and spdf notations, depict reasonable electron configurations for the following elements. (a)
Americium, Am, is a radioactive element isolated from spent fuel in nuclear reactors and used in home smoke detectors. Depict its electron configuration using noble gas and spdf notations.
Predict electron configurations for the following elements of the actinide series of elements. Use noble gas and spdf notations.(a) Plutonium, Pu. The element is best known as a by-product of nuclear
What is the maximum number of electrons that can be identified with each of the following sets of quantum numbers? In some cases, the answer may be “none.” In such cases, explain why “none”
What is the maximum number of electrons that can be identified with each of the following sets of quantum numbers? In some cases, the answer may be “none.” In such cases, explain why “none”
Depict the electron configuration for magnesium using an orbital box diagram and noble gas notation. Give a complete set of four quantum numbers for each of the electrons beyond those of the
Depict the electron configuration for phosphorus using an orbital box diagram and noble gas notation. Give one possible set of four quantum numbers for each of the electrons beyond those of the
Using an orbital box diagram and noble gas notation, show the electron configuration of gallium, Ga. Give one possible set of quantum numbers for the highest-energy electron.
Using an orbital box diagram and noble gas notation, show the electron configuration of titanium. Give one possible set of four quantum numbers for each of the electrons beyond those of the preceding
The effective nuclear charge, Z*, is the net force of attraction experienced by the outermost electron in an atom. Which of the following statements best describes how Z* varies among the elements of
Which of the following statements correctly describes the value of the effective nuclear charge, Z*, felt by(a) The 2s electron at a large distance from a Li atom?(i) Z* equals 1.(ii) Z* is between 1
List the first five orbitals (the five orbitals in an atom at lowest energy) in order of filling, according to the Aufbau principle.
The values of n and ℓ are useful to determine the order of filling (Aufbau principle). Use n and ℓ to determine which orbital, 4f, 5d, or 6s, will fill first.
Using orbital box diagrams, depict an electron configuration for each of the following ions: (a) Mg2+, (b) K+,(c) Cl−, and (d) O2−.
Using orbital box diagrams, depict an electron configuration for each of the following ions: (a) Na+, (b) Al3+, (c) Ge2+, and (d) F−.
Using orbital box diagrams and noble gas notation, depict the electron configurations of (a) V,(b) V2+, and(c) V5+. Is the element or any of the ions paramagnetic?
Using orbital box diagrams and noble gas notation, depict the electron configurations of (a) Ti, (b) Ti2+, and (c) Ti4+. Is the element or any of the ions paramagnetic?
Manganese is found as MnO2 in deep ocean deposits. (a) Depict the electron configuration of this element using the noble gas notation and an orbital box diagram. (b) Using an orbital box diagram,
One compound found in alkaline batteries is NiOOH, a compound containing Ni3+ ions. When the battery is discharged, the Ni3+ is reduced to Ni2+ ions [as in Ni(OH)2]. Using orbital box diagrams and
Arrange the following elements in order of increasing size: Al, B, C, K, and Na.
Arrange the following elements in order of increasing size: Ca, Rb, P, Ge, and Sr.
Select the atom or ion in each pair that has the larger radius. (a) Cl or Cl−(b) Al or O(c) In or I
Select the atom or ion in each pair that has the larger radius. (a) Cs or Rb (b) O2− or O (c) Br or As
Which of the following groups of elements is arranged correctly in order of increasing ionization energy?(a) C < Si < Li < Ne(b) Ne < Si < C < Li(c) Li < Si < C < Ne(d) Ne < C < Si < Li
Arrange the following atoms in order of increasing ionization energy: Li, K, C, and N.
Compare the elements Na, Mg, O, and P. (a) Which has the largest atomic radius? (b) Which has the most negative electron attachment enthalpy?(c) Place the elements in order of increasing ionization
Compare the elements B, Al, C, and Si. (a) Which has the most metallic character? (b) Which has the largest atomic radius? (c) Which has the most negative electron attachment enthalpy? (d) Place
Explain each answer briefly.(a) Place the following elements in order of increasing ionization energy: F, O, and S.(b) Which has the largest ionization energy: O, S, or Se?(c) Which has the most
Explain each answer briefly. (a) Rank the following in order of increasing atomic radius: O, S, and F. (b) Which has the largest ionization energy: P, Si, S, or Se? (c) Place the following in
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L. Martin, S. P. Kowalczyk, F. R. McFeely, and L.
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L. Martin, S. P. Kowalczyk, F. R. McFeely, and L.
Explain why the photoelectron spectra of hydrogen and helium each has one peak whereas that for lithium has two peaks. What would be the relative intensity of each of the peaks in these spectra?
Sketch the major features (number of peaks and relative intensities for the peaks) of the expected photoelectron spectrum for atoms of nitrogen.
The red color of rubies is the result of the substitution of some Cr3+ ions for Al3+ ions in solid Al2O3. (a) Using spdf notation with the noble gas notation, write the electron configuration for
The deep blue color of sapphires comes from the presence of Fe2+ and Ti4+ in solid Al2O3. Using spdf notation with the noble gas notation, write the electron configuration for each of these ions.
Using an orbital box diagram and noble gas notation, show the electron configurations of uranium and of the uranium(IV) ion. Is either of these paramagnetic?
Sulfur (2.56 g) was burned in a constant-volume calorimeter with excess O2(g). The temperature increased from 21.25°C to 26.72°C. The bomb has a heat capacity of 923 J/K, and the calorimeter
Use standard enthalpies of formation in Appendix L to calculate enthalpy changes for the following:(a) 0.054 g of sulfur burns, forming SO2(g)(b) 0.20 mol of HgO(s) decomposes to Hg(ℓ) and O2(g)(c)
The first step in the production of nitric acid from ammonia involves the oxidation of NH3. (a) Use standard enthalpies of formation to calculate the standard enthalpy change for this reaction.(b)
The Romans used calcium oxide, CaO, to produce a strong mortar to build stone structures. Calcium oxide was mixed with water to give Ca(OH)2, which reacted slowly with CO2 in the air to give

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