(a)
Interpretation: The number of orbitals in the 3p sublevel needs to be determined.
Concept introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. There are four quantum numbers; principal quantum number ( n ), azimuthal quantum number ( l ), magnetic quantum number (
(a)
Explanation of Solution
The given sublevel is 3p . Here, the principal quantum number (n) is 3. For p orbital, the value of azimuthal quantum number (l) is 1. Since possible orbitals
will be from -l to +l that is -1, 0, +1 thus, the number of orbitals will be 3. They are represented as follows:
(b)
Interpretation: The number of orbitals in the 2s sublevel needs to be determined.
Concept introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. There are four quantum numbers; principal quantum number ( n ), azimuthal quantum number ( l ), magnetic quantum number (
(b)
Explanation of Solution
The given sublevel is 2s. Here, the principal quantum number (n) is 2. For s orbital, the value of azimuthal quantum number (l) is 0. Since possible orbitals
will be from -l to +l which is only 0, thus, the number of orbitals will be 1. They are represented as follows:
(c)
Interpretation: The number of orbitals in the 4p sublevel needs to be determined.
Concept introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. There are four quantum numbers; principal quantum number ( n ), azimuthal quantum number ( l ), magnetic quantum number (
(c)
Explanation of Solution
The given sublevel is 4p . Here, the principal quantum number (n) is 4. For p orbital, the value of azimuthal quantum number (l) is 1. Since possible orbitals
will be from -l to +l that is -1, 0, +1, thus, the number of orbitals will be 3. They are represented as follows:
(d)
Interpretation: The number of orbitals in the 3d sublevel needs to be determined.
Concept introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. There are four quantum numbers; principal quantum number ( n ), azimuthal quantum number ( l ), magnetic quantum number (
(d)
Explanation of Solution
The given sublevel is 3d . Here, the principal quantum number (n) is 3. For d orbital, the value of azimuthal quantum number (l) is 2. Since possible orbitals
(e)
Interpretation: The number of orbitals in the 4f sublevel needs to be determined.
Concept introduction: An atomic orbital explains the position of an electron in an atom. An atomic orbital can be occupied by a maximum of two electrons with opposite spins. The four basic atomic orbitals are s, p, d, and f . The number of electrons in each orbital can be explained with the help of quantum numbers. There are four quantum numbers; principal quantum number ( n ), azimuthal quantum number ( l ), magnetic quantum number (
(e)
Explanation of Solution
The given sublevel is 4f . Here, the principal quantum number (n) is 4. For f orbital, the value of azimuthal quantum number (l) is 3. Since possible orbitals
Chapter 5 Solutions
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