Write the orbital diagram tor an atom of
(a) Na (b) O (c) Co
(d) Cl
(a)
Interpretation:
The orbital diagram for Na should be written.
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration one can get details of the number of electrons present in each sublevel. To show the distribution of electrons in the various orbitals, orbital diagrams are used. The filling of electrons in the atomic orbitals takes place according to the Aufbau principal which states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
Answer to Problem 40QAP
The orbital diagram for Na is:
Explanation of Solution
When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. Atomic number of an element gives the total number of electrons present in an atom. Since the atomic number of sodium atom denoted by Na is 11, therefore its ground state electronic configuration is:
According to Hund’s Rule, when several orbitals having equal energy are available, then electrons are filled singly with parallel spins. No two electrons can have same spin in a given orbital. The most stable arrangement of electrons is the one in which two electrons present in two different orbitals have parallel spins. The total number of orbitals in a given sublevel are given by 2l+1, where l = 0,1,2,3 for s, p, d and f sublevels respectively. In case of Sodium, since the electrons are present in both the s and p-sublevel, therefore l=0 for s- sublevel,
This means 2l+1 = 2(0) +1= 1
This means that I orbital is present in each s- sublevel.
In case of p-sublevel the total number of orbitals are:
2l +1
2 (1) +1
2 +1=3.
The orbital diagram for its electronic configuration is shown below:
(b)
Interpretation:
The orbital diagram for O should be written.
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration one can get details of the number of electrons present in each sublevel. The filling of electrons in the atomic orbitals takes place according to the Aufbau principal which states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
To show the distribution of electrons in the various orbitals, orbital diagrams are used.
Answer to Problem 40QAP
The orbital diagram for O is:
Explanation of Solution
When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. Atomic number of an element gives the total number of electrons present in an atom. Since the atomic number of Oxygen atom denoted by O is 8, therefore its ground state electronic configuration is:
According to Hund’s Rule, when several orbitals having equal energy are available, then electrons are filled singly with parallel spins. No two electrons can have same spin in a given orbital. The most stable arrangement of electrons is the one in which two electrons present in two different orbitals have parallel spins. The total number of orbitals in a given sublevel are given by 2l+1, where l = 0,1,2,3 for s, p, d and f sublevels respectively. In case of Oxygen, since the electrons are present in both s and p-sublevel, l=0 for s and l=1 for p-sublevels
This means 2l+1 = 2(0) +1= 1
Hence one orbital is present for each s-sublevel.
For a p-sublevel, the total number of orbitals are
2(1) +1
2+1
3
This means that three orbitals are present in each p-sublevel of Oxygen atom.
The orbital diagram for its electronic configuration is shown below:
(c)
Interpretation:
The orbital diagram for Co should be written.
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration one can get details of the number of electrons present in each sublevel. The filling of electrons in the atomic orbitals takes place according to the Aufbau principal which states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
To show the distribution of electrons in the various orbitals, orbital diagrams are used.
Answer to Problem 40QAP
The orbital diagram for Co is:
Explanation of Solution
When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. Atomic number of an element gives the total number of electrons present in an atom. Since the atomic number of Cobalt atom denoted by Co is 27, therefore its ground state electronic configuration is:
According to Hund’s Rule, when several orbitals having equal energy are available, then electrons are filled singly with parallel spins. No two electrons can have same spin in a given orbital. The most stable arrangement of electrons is the one in which two electrons present in two different orbitals have parallel spins. The total number of orbitals in a given sublevel are given by 2l+1, where l = 0,1,2,3 for s, p, d and f sublevels respectively. In case of Cobalt, since the electrons are present in both s and p-sublevel, l=0 for s and l=1 for p-sublevels
This means 2l+1 = 2(0) +1= 1
Hence one orbital is present for each s-sublevel.
For a p-sublevel, the total number of orbitals are
2(1) +1
2+1
3
This means that three orbitals are present in p-sublevel of Cobalt atom.
For d- sublevel since l=2, therefore number of orbitals = 2(2)+1=5
The orbital diagram for its electronic configuration is shown below:
(d)
Interpretation:
The orbital diagram for Cl element should be written.
Concept introduction:
The simplest method for describing the arrangement of electrons in an atom is by writing its electronic configuration. Since the set of four quantum numbers is used to describe the atomic orbitals in an atom, therefore by writing the electronic configuration one can get details of the number of electrons present in each sublevel. The filling of electrons in the atomic orbitals takes place according to the Aufbau principal which states that when an atom is present in its ground state, electrons are filled in order of increasing energy of the orbitals, which means that firstly lower energy orbitals are filled, and then filling of higher energy orbitals takes place.
To show the distribution of electrons in the various orbitals, orbital diagrams are used.
Answer to Problem 40QAP
The orbital diagram for Cl is:
Explanation of Solution
When the electronic configuration of an atom is written, it describes the number of electron present in each sublevel by the superscript. Atomic number of an element gives the total number of electrons present in an atom. Since the atomic number of Chlorine atom denoted by Cl is 17, therefore its ground state electronic configuration is:
According to Hund’s Rule, when several orbitals having equal energy are available, then electrons are filled singly with parallel spins. No two electrons can have same spin in a given orbital. The most stable arrangement of electrons is the one in which two electrons present in two different orbitals have parallel spins. The total number of orbitals in a given sublevel are given by 2l+1, where l = 0,1,2,3 for s, p, d and f sublevels respectively. In case of Chlorine, since the electrons are present in s and p-sublevel, l=0 for s and l=1 for p
This means 2l+1 = 2(0) +1= 1
Hence one orbital is present for each s-sublevel.
For a p-sublevel, the total number of orbitals are
2(1) +1
2+1
3
This means that three orbitals are present in each p-sublevel of Cl atom.
The orbital diagram for its electronic configuration is shown below:
Want to see more full solutions like this?
Chapter 6 Solutions
Chemistry: Principles and Reactions
- The first ionization energy of helium is 2370kJmol1 , the highest for any element. (a) Define ionization energy and discuss why for helium it should be so high. (b) Which element would you expect to have the highest second ionization energy? Why? (c) Suppose that you wished to ionize some helium by shining electromagnetic radiation on it. What is the maximum wavelength you could use?arrow_forwardow does probability ?t into the description of the atom?arrow_forwardMany times the claim is made that subshells half-filled with electrons are particularly stable. Can you suggest a possible physical basis for this claim?arrow_forward
- Use the aufbau procedure to obtain the electron configuration and orbital diagram for atoms of the following elements. (a) Be (b) B (c) Ne (d) Rbarrow_forwardThe energy needed to ionize an atom of element X when it is in its most stable state is 500kJmol1 . However, if an atom of X is in its lowest excited state, only 120kJmol1 is needed to ionize it. What is the wavelength of the radiation emitted when an atom of X undergoes a transition from the lowest excited state to the ground state?arrow_forwardConstruct an energy level diagram showing all orbitals for the hydrogen atom up to n=5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?arrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning