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Chapter 3, Problem 3.77QP

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CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

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Chapter
Section
FindFindarrow_forward

CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933
Interpretation Introduction

Interpretation:

The possible subshells and orbitals associated with the principal quantum number, n=4 is to be given.

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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