Chemistry: Atoms First
Chemistry: Atoms First
2nd Edition
ISBN: 9780073511184
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
Question
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Chapter 3.8, Problem 3.8.4SR

(a)

Interpretation Introduction

Interpretation:

Anything wrong in the set of given quantum numbers have to be identified and should be explained.

Concept Introduction:

Quantum Numbers:

The distribution of electron density in an atom is defined by Quantum numbers.  They are derived from the mathematical solution of Schrodinger’s equation in the hydrogen atom.

Four types of quantum numbers:

Principal quantum number (n)

Angular momentum quantum number (l)

Magnetic quantum number (ml)

Electron spin quantum number  (ms).

Each atomic orbital in an atom is characterized by a unique set of the quantum numbers.

Principal Quantum Number (n)

The size of an orbital and the energy of an electron are specified by the principal quantum number (n).  If the value of n is larger, then the average distance from the nucleus to the specified orbital of an electron will be greater.  Hence, the orbital’s size is large with the increasing energy. The principal quantum numbers get the integral values of 1, 2, 3 and so on.  If the same value of ‘n’ is present in the orbitals, then, all the electrons are occupied in the same shell (level).  The total number of the orbitals corresponding to a given n value is found by n2.

Angular Momentum Quantum Number (l)

The shape of the atomic orbital is given by the angular momentum quantum number (l) which are integers and its values depend on the integral value of the principal quantum number, n The probable values of l range are given from 0 to n1 for n value.  There is one possible value of l (l = 0) for n= 1.  There are two values of l which are 0 and 1 for n = 2.  There are three values of l which are 0, 1 and 2 for n = 3.   The l value gives the type of orbitals namely, s, p, d and fs orbital comes for l = 0; p orbital for l = 1; d orbital for l = 2; f orbital  for l = 3.  If the orbitals have the same n and l values, they are present in the same subshell (sublevel) A smaller amount of energy is contributed by the l values which increase with the subshell levels (s < p < d < f).

Magnetic Quantum Number (ml)

The orientation of the orbital in space is given the magnetic quantum number (ml).  The value of ml depends on the l value in a subshell.  It divides the subshell into the individual orbitals which have the electrons.  There are (2l+1) integral ml values for a l value which is explained as follows:

 ml = l...0...+l

There is one possible ml value which is 0 for l = 0.

There are three ml values which are 1, 0 and +1 for l = 1.

There are five ml values which are 2, 1, 0, +1 and +2 for l = 2.

There are seven ml values which are 3, 2, 1, 0, +1, +2 and +3 for l = 3 and so on.

For a particular l value, the number of ml values specifies the number of orbitals in a subshell.  Therefore, each ml value gets a different orbital.

(b)

Interpretation Introduction

Interpretation:

Anything wrong in the set of given quantum numbers have to be identified and should be explained.

Concept Introduction:

Quantum Numbers:

The distribution of electron density in an atom is defined by Quantum numbers.  They are derived from the mathematical solution of Schrodinger’s equation in the hydrogen atom.

Four types of quantum numbers:

Principal quantum number (n)

Angular momentum quantum number (l)

Magnetic quantum number (ml)

Electron spin quantum number  (ms).

Each atomic orbital in an atom is characterized by a unique set of the quantum numbers.

Principal Quantum Number (n)

The size of an orbital and the energy of an electron are specified by the principal quantum number (n).  If the value of n is larger, then the average distance from the nucleus to the specified orbital of an electron will be greater.  Hence, the orbital’s size is large with the increasing energy. The principal quantum numbers get the integral values of 1, 2, 3 and so on.  If the same value of ‘n’ is present in the orbitals, then, all the electrons are occupied in the same shell (level).  The total number of the orbitals corresponding to a given n value is found by n2.

Angular Momentum Quantum Number (l)

The shape of the atomic orbital is given by the angular momentum quantum number (l) which are integers and its values depend on the integral value of the principal quantum number, n The probable values of l range are given from 0 to n1 for n value.  There is one possible value of l (l = 0) for n= 1.  There are two values of l which are 0 and 1 for n = 2.  There are three values of l which are 0, 1 and 2 for n = 3.   The l value gives the type of orbitals namely, s, p, d and fs orbital comes for l = 0; p orbital for l = 1; d orbital for l = 2; f orbital  for l = 3.  If the orbitals have the same n and l values, they are present in the same subshell (sublevel) A smaller amount of energy is contributed by the l values which increase with the subshell levels (s < p < d < f).

Magnetic Quantum Number (ml)

The orientation of the orbital in space is given the magnetic quantum number (ml).  The value of ml depends on the l value in a subshell.  It divides the subshell into the individual orbitals which have the electrons.  There are (2l+1) integral ml values for a l value which is explained as follows:

 ml = l...0...+l

There is one possible ml value which is 0 for l = 0.

There are three ml values which are 1, 0 and +1 for l = 1.

There are five ml values which are 2, 1, 0, +1 and +2 for l = 2.

There are seven ml values which are 3, 2, 1, 0, +1, +2 and +3 for l = 3 and so on.

For a particular l value, the number of ml values specifies the number of orbitals in a subshell.  Therefore, each ml value gets a different orbital.

(c)

Interpretation Introduction

Interpretation:

Anything wrong in the set of given quantum numbers have to be identified and should be explained.

Concept Introduction:

Quantum Numbers:

The distribution of electron density in an atom is defined by Quantum numbers.  They are derived from the mathematical solution of Schrodinger’s equation in the hydrogen atom.

Four types of quantum numbers:

Principal quantum number (n)

Angular momentum quantum number (l)

Magnetic quantum number (ml)

Electron spin quantum number  (ms).

Each atomic orbital in an atom is characterized by a unique set of the quantum numbers.

Principal Quantum Number (n)

The size of an orbital and the energy of an electron are specified by the principal quantum number (n).  If the value of n is larger, then the average distance from the nucleus to the specified orbital of an electron will be greater.  Hence, the orbital’s size is large with the increasing energy. The principal quantum numbers get the integral values of 1, 2, 3 and so on.  If the same value of ‘n’ is present in the orbitals, then, all the electrons are occupied in the same shell (level).  The total number of the orbitals corresponding to a given n value is found by n2.

Angular Momentum Quantum Number (l)

The shape of the atomic orbital is given by the angular momentum quantum number (l) which are integers and its values depend on the integral value of the principal quantum number, n The probable values of l range are given from 0 to n1 for n value.  There is one possible value of l (l = 0) for n= 1.  There are two values of l which are 0 and 1 for n = 2.  There are three values of l which are 0, 1 and 2 for n = 3.   The l value gives the type of orbitals namely, s, p, d and fs orbital comes for l = 0; p orbital for l = 1; d orbital for l = 2; f orbital  for l = 3.  If the orbitals have the same n and l values, they are present in the same subshell (sublevel) A smaller amount of energy is contributed by the l values which increase with the subshell levels (s < p < d < f).

Magnetic Quantum Number (ml)

The orientation of the orbital in space is given the magnetic quantum number (ml).  The value of ml depends on the l value in a subshell.  It divides the subshell into the individual orbitals which have the electrons.  There are (2l+1) integral ml values for a l value which is explained as follows:

 ml = l...0...+l

There is one possible ml value which is 0 for l = 0.

There are three ml values which are 1, 0 and +1 for l = 1.

There are five ml values which are 2, 1, 0, +1 and +2 for l = 2.

There are seven ml values which are 3, 2, 1, 0, +1, +2 and +3 for l = 3 and so on.

For a particular l value, the number of ml values specifies the number of orbitals in a subshell.  Therefore, each ml value gets a different orbital.

(d)

Interpretation Introduction

Interpretation:

Anything wrong in the set of given quantum numbers have to be identified and should be explained.

Concept Introduction:

Quantum Numbers:

The distribution of electron density in an atom is defined by Quantum numbers.  They are derived from the mathematical solution of Schrodinger’s equation in the hydrogen atom.

Four types of quantum numbers:

Principal quantum number (n)

Angular momentum quantum number (l)

Magnetic quantum number (ml)

Electron spin quantum number  (ms).

Each atomic orbital in an atom is characterized by a unique set of the quantum numbers.

Principal Quantum Number (n)

The size of an orbital and the energy of an electron are specified by the principal quantum number (n).  If the value of n is larger, then the average distance from the nucleus to the specified orbital of an electron will be greater.  Hence, the orbital’s size is large with the increasing energy. The principal quantum numbers get the integral values of 1, 2, 3 and so on.  If the same value of ‘n’ is present in the orbitals, then, all the electrons are occupied in the same shell (level).  The total number of the orbitals corresponding to a given n value is found by n2.

Angular Momentum Quantum Number (l)

The shape of the atomic orbital is given by the angular momentum quantum number (l) which are integers and its values depend on the integral value of the principal quantum number, n The probable values of l range are given from 0 to n1 for n value.  There is one possible value of l (l = 0) for n= 1.  There are two values of l which are 0 and 1 for n = 2.  There are three values of l which are 0, 1 and 2 for n = 3.   The l value gives the type of orbitals namely, s, p, d and fs orbital comes for l = 0; p orbital for l = 1; d orbital for l = 2; f orbital  for l = 3.  If the orbitals have the same n and l values, they are present in the same subshell (sublevel) A smaller amount of energy is contributed by the l values which increase with the subshell levels (s < p < d < f).

Magnetic Quantum Number (ml)

The orientation of the orbital in space is given the magnetic quantum number (ml).  The value of ml depends on the l value in a subshell.  It divides the subshell into the individual orbitals which have the electrons.  There are (2l+1) integral ml values for a l value which is explained as follows:

 ml = l...0...+l

There is one possible ml value which is 0 for l = 0.

There are three ml values which are 1, 0 and +1 for l = 1.

There are five ml values which are 2, 1, 0, +1 and +2 for l = 2.

There are seven ml values which are 3, 2, 1, 0, +1, +2 and +3 for l = 3 and so on.

For a particular l value, the number of ml values specifies the number of orbitals in a subshell.  Therefore, each ml value gets a different orbital.

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Chapter 3 Solutions

Chemistry: Atoms First

Ch. 3.1 - Prob. 3.1.3SRCh. 3.2 - One type of laser used in the treatment of...Ch. 3.2 - What is the wavelength (in meters) of an...Ch. 3.2 - What is the frequency (in reciprocal seconds) of...Ch. 3.2 - Which of the following sets of waves best...Ch. 3.2 - Prob. 3.2.1SRCh. 3.2 - Prob. 3.2.2SRCh. 3.2 - Prob. 3.2.3SRCh. 3.2 - Prob. 3.2.4SRCh. 3.3 - Calculate the energy (in joules) of (a) a photon...Ch. 3.3 - Calculate the energy (in joules) of (a) a photon...Ch. 3.3 - (a) Calculate the wavelength (in nanometers) of...Ch. 3.3 - Prob. 3.3.1SRCh. 3.3 - Prob. 3.3.2SRCh. 3.3 - Prob. 3.3.3SRCh. 3.3 - Prob. 3.3.4SRCh. 3.3 - Prob. 3.3.5SRCh. 3.4 - Calculate the wavelength (in nanometers) of the...Ch. 3.4 - What is the wavelength (in nanometers) of a photon...Ch. 3.4 - What is the value of ni for an electron that emits...Ch. 3.4 - For each pair of transitions, determine which one...Ch. 3.4 - Prob. 3.4.1SRCh. 3.4 - Prob. 3.4.2SRCh. 3.4 - Prob. 3.4.3SRCh. 3.4 - Prob. 3.4.4SRCh. 3.5 - Calculate the de Broglie wavelength of the...Ch. 3.5 - Calculate the de Broglie wavelength (in...Ch. 3.5 - Use Equation 3.11 to calculate the momentum, p...Ch. 3.5 - Consider the impact of early electron diffraction...Ch. 3.5 - Prob. 3.5.1SRCh. 3.5 - Prob. 3.5.2SRCh. 3.5 - Prob. 3.5.3SRCh. 3.6 - An electron in a hydrogen atom is known to have a...Ch. 3.6 - Prob. 7PPACh. 3.6 - (a) Calculate the minimum uncertainty in the...Ch. 3.6 - Using Equation 3.13, we can calculate the minimum...Ch. 3.6 - Prob. 3.6.1SRCh. 3.6 - Prob. 3.6.2SRCh. 3.7 - What are the possible values for the magnetic...Ch. 3.7 - Prob. 8PPACh. 3.7 - Prob. 8PPBCh. 3.7 - Prob. 8PPCCh. 3.7 - Prob. 3.7.1SRCh. 3.7 - Prob. 3.7.2SRCh. 3.7 - Prob. 3.7.3SRCh. 3.7 - Prob. 3.7.4SRCh. 3.8 - Prob. 3.9WECh. 3.8 - Prob. 9PPACh. 3.8 - Prob. 9PPBCh. 3.8 - Prob. 9PPCCh. 3.8 - Prob. 3.8.1SRCh. 3.8 - Prob. 3.8.2SRCh. 3.8 - Prob. 3.8.3SRCh. 3.8 - Prob. 3.8.4SRCh. 3.9 - Write the electron configuration and give the...Ch. 3.9 - Prob. 10PPACh. 3.9 - Write the electron configuration and give the...Ch. 3.9 - Prob. 10PPCCh. 3.9 - Prob. 3.9.1SRCh. 3.9 - Prob. 3.9.2SRCh. 3.9 - Prob. 3.9.3SRCh. 3.10 - Without referring to Figure 3.26, write the...Ch. 3.10 - Prob. 11PPACh. 3.10 - Prob. 11PPBCh. 3.10 - Consider again the alternate universe and its...Ch. 3.10 - Prob. 3.10.1SRCh. 3.10 - Prob. 3.10.2SRCh. 3.10 - Prob. 3.10.3SRCh. 3.10 - Prob. 3.10.4SRCh. 3 - Define these terms: potential energy, kinetic...Ch. 3 - What are the units for energy commonly employed in...Ch. 3 - A truck initially traveling at 60 km/h is brought...Ch. 3 - Describe the interconversions of forms of energy...Ch. 3 - Prob. 3.5QPCh. 3 - Prob. 3.6QPCh. 3 - Prob. 3.7QPCh. 3 - Prob. 3.8QPCh. 3 - Prob. 3.9QPCh. 3 - (a) How much greater is the electrostatic energy...Ch. 3 - Prob. 3.11QPCh. 3 - Prob. 3.12QPCh. 3 - List the types of electromagnetic radiation,...Ch. 3 - Prob. 3.14QPCh. 3 - Prob. 3.15QPCh. 3 - Prob. 3.16QPCh. 3 - The SI unit of time is the second, which is...Ch. 3 - Prob. 3.18QPCh. 3 - Prob. 3.19QPCh. 3 - Four waves represent light in four different...Ch. 3 - Prob. 3.21QPCh. 3 - Prob. 3.22QPCh. 3 - Prob. 3.23QPCh. 3 - What is a photon? What role did Einsteins...Ch. 3 - A photon has a wavelength of 705 nm. Calculate the...Ch. 3 - The blue color of the sky results from the...Ch. 3 - A photon has a frequency of 6.5 109 Hz. (a)...Ch. 3 - Prob. 3.28QPCh. 3 - Prob. 3.29QPCh. 3 - Prob. 3.30QPCh. 3 - Prob. 3.31QPCh. 3 - A particular form of electromagnetic radiation has...Ch. 3 - Photosynthesis makes use of visible light to bring...Ch. 3 - The retina of a human eye can detect light when...Ch. 3 - Prob. 3.35QPCh. 3 - The binding energy of magnesium metal is 5.86 ...Ch. 3 - What is the kinetic energy of the ejected electron...Ch. 3 - A red light was shined onto a metal sample and the...Ch. 3 - A photoelectric experiment was performed by...Ch. 3 - Which of the following best explains why we see...Ch. 3 - One way to see the emission spectrum of hydrogen...Ch. 3 - How many lines would we see in the emission...Ch. 3 - For a hydrogen atom in which the electron has been...Ch. 3 - Prob. 3.40QPCh. 3 - Prob. 3.41QPCh. 3 - Briefly describe Bohrs theory of the hydrogen atom...Ch. 3 - Explain the meaning of the negative sign in...Ch. 3 - Consider the following energy levels of a...Ch. 3 - Prob. 3.45QPCh. 3 - Calculate the wavelength (in nanometers) of a...Ch. 3 - Calculate the frequency (hertz) and wavelength...Ch. 3 - What wavelength of light is needed to excite the...Ch. 3 - An electron in the hydrogen atom makes a...Ch. 3 - Explain why elements produce their own...Ch. 3 - Some copper-containing substances emit green light...Ch. 3 - Prob. 3.52QPCh. 3 - Prob. 3.53QPCh. 3 - Prob. 3.54QPCh. 3 - Why is Equation 3.11 meaningful only for...Ch. 3 - Prob. 3.56QPCh. 3 - Thermal neutrons are neutrons that move at speeds...Ch. 3 - Protons can be accelerated to speeds near that of...Ch. 3 - Prob. 3.59QPCh. 3 - Prob. 3.60QPCh. 3 - Prob. 3.61QPCh. 3 - Prob. 3.62QPCh. 3 - What are the inadequacies of Bohrs theory?Ch. 3 - What is the Heisenberg uncertainty principle? What...Ch. 3 - Prob. 3.65QPCh. 3 - Prob. 3.66QPCh. 3 - Prob. 3.67QPCh. 3 - The speed of a thermal neutron (see Problem 3.57)...Ch. 3 - Alveoli are tiny sacs of air in the lungs. Their...Ch. 3 - In the beginning of the twentieth century, some...Ch. 3 - Suppose that photons of blue light (430 nm) are...Ch. 3 - Prob. 3.72QPCh. 3 - Prob. 3.73QPCh. 3 - Which of the four quantum numbers (n, , m, ms)...Ch. 3 - Prob. 3.75QPCh. 3 - Prob. 3.76QPCh. 3 - Prob. 3.77QPCh. 3 - Prob. 3.78QPCh. 3 - Describe the shapes of s, p, and d orbitals. How...Ch. 3 - Prob. 3.80QPCh. 3 - Describe the characteristics of an s orbital, p...Ch. 3 - Why is a boundary surface diagram useful in...Ch. 3 - Prob. 3.83QPCh. 3 - Give the values of the four quantum numbers of an...Ch. 3 - Describe how a 1s orbital and a 2s orbital are...Ch. 3 - Prob. 3.86QPCh. 3 - Prob. 3.87QPCh. 3 - Make a chart of all allowable orbitals in the...Ch. 3 - Prob. 3.89QPCh. 3 - Prob. 3.90QPCh. 3 - A 3s orbital is illustrated here. Using this as a...Ch. 3 - Prob. 3.92QPCh. 3 - Prob. 3.93QPCh. 3 - State the Aufbau principle, and explain the role...Ch. 3 - Indicate the total number of (a) p electrons in N...Ch. 3 - Calculate the total number of electrons that can...Ch. 3 - Determine the total number of electrons that can...Ch. 3 - Determine the maximum number of electrons that can...Ch. 3 - Prob. 3.99QPCh. 3 - The electron configuration of an atom in the...Ch. 3 - List the following atoms in order of increasing...Ch. 3 - Determine the number of unpaired electrons in each...Ch. 3 - Determine the number of impaired electrons in each...Ch. 3 - Determine the number of unpaired electrons in each...Ch. 3 - Prob. 3.105QPCh. 3 - Portions of orbital diagrams representing the...Ch. 3 - Prob. 3.107QPCh. 3 - Prob. 3.108QPCh. 3 - Prob. 3.109QPCh. 3 - Define the following terms and give an example of...Ch. 3 - Explain why the ground-state electron...Ch. 3 - Write the election configuration of a xenon core.Ch. 3 - Comment on the correctness of the following...Ch. 3 - Prob. 3.114QPCh. 3 - Prob. 3.115QPCh. 3 - Write the ground-state electron configurations for...Ch. 3 - Write the ground-state electron configurations for...Ch. 3 - What is the symbol of the element with the...Ch. 3 - Prob. 3.119QPCh. 3 - Prob. 3.120QPCh. 3 - Discuss the current view of the correctness of the...Ch. 3 - Distinguish carefully between the following terms:...Ch. 3 - What is the maximum number of electrons in an atom...Ch. 3 - Prob. 3.124QPCh. 3 - Prob. 3.125QPCh. 3 - A baseball pitchers fastball has been clocked at...Ch. 3 - A ruby laser produces radiation of wavelength 633...Ch. 3 - Four atomic energy levels of an atom are shown...Ch. 3 - Prob. 3.129QPCh. 3 - Spectral lines of the Lyman and Balmer series do...Ch. 3 - Only a fraction of the electric energy supplied to...Ch. 3 - The figure here illustrates a series of...Ch. 3 - When one of heliums electrons is removed, the...Ch. 3 - The retina of a human eye can detect light when...Ch. 3 - An electron in an excited state in a hydrogen atom...Ch. 3 - Prob. 3.136QPCh. 3 - The election configurations described in this...Ch. 3 - Draw the shapes (boundary surfaces) of the...Ch. 3 - Prob. 3.139QPCh. 3 - Consider the graph here. (a) Calculate the binding...Ch. 3 - Scientists have found interstellar hydrogen atoms...Ch. 3 - Ionization energy is the minimum energy required...Ch. 3 - Prob. 3.143QPCh. 3 - Prob. 3.144QPCh. 3 - The cone cells of the human eye are sensitive to...Ch. 3 - (a) An electron in the ground state of the...Ch. 3 - Prob. 3.147QPCh. 3 - Prob. 3.148QPCh. 3 - When an election makes a transition between energy...Ch. 3 - Blackbody radiation is the term used to describe...Ch. 3 - Suppose that photons of red light (675 nm) are...Ch. 3 - In an election microscope, electrons are...Ch. 3 - According to Einsteins special theory of...Ch. 3 - The mathematical equation for studying the...
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