<< Chapter < Page Chapter >> Page >

Maximum number of electrons

Calculate the maximum number of electrons that can occupy a shell with (a) n = 2, (b) n = 5, and (c) n as a variable. Note you are only looking at the orbitals with the specified n value, not those at lower energies.

Solution

(a) When n = 2, there are four orbitals (a single 2 s orbital, and three orbitals labeled 2 p ). These four orbitals can contain eight electrons.

(b) When n = 5, there are five subshells of orbitals that we need to sum:

1 orbital labeled 5 s 3 orbitals labeled 5 p 5 orbitals labeled 5 d 7 orbitals labeled 5 f + 9 orbitals labeled 5 g ¯ 25 orbitals total

Again, each orbital holds two electrons, so 50 electrons can fit in this shell.

(c) The number of orbitals in any shell n will equal n 2 . There can be up to two electrons in each orbital, so the maximum number of electrons will be 2 × n 2

Check your learning

If a shell contains a maximum of 32 electrons, what is the principal quantum number, n ?

Answer:

n = 4

Got questions? Get instant answers now!

Working with quantum numbers

Complete the following table for atomic orbitals:

Orbital n l m l degeneracy Radial nodes (no.)
4 f
4 1
7 7 3
5 d

Solution

The table can be completed using the following rules:

  • The orbital designation is nl , where l = 0, 1, 2, 3, 4, 5, … is mapped to the letter sequence s, p , d , f , g , h , …,
  • The m l degeneracy is the number of orbitals within an l subshell, and so is 2 l + 1 (there is one s orbital, three p orbitals, five d orbitals, seven f orbitals, and so forth).
  • The number of radial nodes is equal to n – l – 1.
Orbital n l m l degeneracy Radial nodes (no.)
4 f 4 3 7 0
4 p 4 1 3 2
7 f 7 3 7 3
5 d 5 2 5 2

Check your learning

How many orbitals have l = 2 and n = 3?

Answer:

The five degenerate 3 d orbitals

Got questions? Get instant answers now!

Key concepts and summary

Macroscopic objects act as particles. Microscopic objects (such as electrons) have properties of both a particle and a wave. Their exact trajectories cannot be determined. The quantum mechanical model of atoms describes the three-dimensional position of the electron in a probabilistic manner according to a mathematical function called a wavefunction, often denoted as ψ . Atomic wavefunctions are also called orbitals. The squared magnitude of the wavefunction describes the distribution of the probability of finding the electron in a particular region in space. Therefore, atomic orbitals describe the areas in an atom where electrons are most likely to be found.

An atomic orbital is characterized by three quantum numbers. The principal quantum number, n , can be any positive integer. The general region for value of energy of the orbital and the average distance of an electron from the nucleus are related to n . Orbitals having the same value of n are said to be in the same shell. The angular momentum quantum number, l , can have any integer value from 0 to n – 1. This quantum number describes the shape or type of the orbital. Orbitals with the same principle quantum number and the same l value belong to the same subshell. The magnetic quantum number, m l , with 2 l + 1 values ranging from – l to + l , describes the orientation of the orbital in space. In addition, each electron has a spin quantum number, m s , that can be equal to ± 1 2 . No two electrons in the same atom can have the same set of values for all the four quantum numbers.

Chemistry end of chapter exercises

How are the Bohr model and the quantum mechanical model of the hydrogen atom similar? How are they different?

Both models have a central positively charged nucleus with electrons moving about the nucleus in accordance with the Coulomb electrostatic potential. The Bohr model assumes that the electrons move in circular orbits that have quantized energies, angular momentum, and radii that are specified by a single quantum number, n = 1, 2, 3, …, but this quantization is an ad hoc assumption made by Bohr to incorporate quantization into an essentially classical mechanics description of the atom. Bohr also assumed that electrons orbiting the nucleus normally do not emit or absorb electromagnetic radiation, but do so when the electron switches to a different orbit. In the quantum mechanical model, the electrons do not move in precise orbits (such orbits violate the Heisenberg uncertainty principle) and, instead, a probabilistic interpretation of the electron’s position at any given instant is used, with a mathematical function ψ called a wavefunction that can be used to determine the electron’s spatial probability distribution. These wavefunctions, or orbitals, are three-dimensional stationary waves that can be specified by three quantum numbers that arise naturally from their underlying mathematics (no ad hoc assumptions required): the principal quantum number, n (the same one used by Bohr), which specifies shells such that orbitals having the same n all have the same energy and approximately the same spatial extent; the angular momentum quantum number l , which is a measure of the orbital’s angular momentum and corresponds to the orbitals’ general shapes, as well as specifying subshells such that orbitals having the same l (and n ) all have the same energy; and the orientation quantum number m , which is a measure of the z component of the angular momentum and corresponds to the orientations of the orbitals. The Bohr model gives the same expression for the energy as the quantum mechanical expression and, hence, both properly account for hydrogen’s discrete spectrum (an example of getting the right answers for the wrong reasons, something that many chemistry students can sympathize with), but gives the wrong expression for the angular momentum (Bohr orbits necessarily all have non-zero angular momentum, but some quantum orbitals [ s orbitals] can have zero angular momentum).

Got questions? Get instant answers now!

What are the allowed values for each of the four quantum numbers: n , l , m l , and m s ?

Got questions? Get instant answers now!

Describe the properties of an electron associated with each of the following four quantum numbers: n , l , m l , and m s .

n determines the general range for the value of energy and the probable distances that the electron can be from the nucleus. l determines the shape of the orbital. m 1 determines the orientation of the orbitals of the same l value with respect to one another. m s determines the spin of an electron.

Got questions? Get instant answers now!

Answer the following questions:

(a) Without using quantum numbers, describe the differences between the shells, subshells, and orbitals of an atom.

(b) How do the quantum numbers of the shells, subshells, and orbitals of an atom differ?

Got questions? Get instant answers now!

Identify the subshell in which electrons with the following quantum numbers are found:

(a) n = 2, l = 1

(b) n = 4, l = 2

(c) n = 6, l = 0

(a) 2 p ; (b) 4 d ; (c) 6 s

Got questions? Get instant answers now!

Which of the subshells described in the previous question contain degenerate orbitals? How many degenerate orbitals are in each?

Got questions? Get instant answers now!

Identify the subshell in which electrons with the following quantum numbers are found:

(a) n = 3, l = 2

(b) n = 1, l = 0

(c) n = 4, l = 3

(a) 3 d; (b) 1 s; (c) 4 f

Got questions? Get instant answers now!

Which of the subshells described in the previous question contain degenerate orbitals? How many degenerate orbitals are in each?

Got questions? Get instant answers now!

Sketch the boundary surface of a d x 2 y 2 and a p y orbital. Be sure to show and label the axes.

This figure contains two diagrams. The first is of a 2 p subscript y orbital. The second is of a d subscript x squared minus y squared orbital. The first diagram has two spherical shapes joined at the origin when oriented along the y axis on an x y and z coordinate plane. The second diagram shows four ellipsoid lobes with ends centered around the origin. Two of these ellipsoid lobes are oriented along the x axis and two are oriented along the y axis on the x y and z coordinate plane.
Got questions? Get instant answers now!

Sketch the p x and d xz orbitals. Be sure to show and label the coordinates.

Got questions? Get instant answers now!

Consider the orbitals shown here in outline.

This figure contains three diagrams. In x, a circle is drawn with a dot at the center. In y, two nearly ellipsoid shapes are oriented horizontally with a dot between them. In z, four shapes like those in y are oriented in an x shape with a dot at the center.

(a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)?

(b) How many orbitals of type (x) are found in a shell with n = 2? How many of type (y)? How many of type (z)?

(c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell with n = 4. Of an orbital of type (y) in a shell with n = 2. Of an orbital of type (z) in a shell with n = 3.

(d) What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)?

(e) What are the possible l and m l values for an orbital of type (x)? Of type (y)? Of type (z)?

(a) x. 2, y. 2, z. 2; (b) x. 1, y. 3, z. 0; (c) x. 4 0 0 1 2 , y. 2 1 0 1 2 , z. 3 2 0 1 2 ; (d) x. 1, y. 2, z. 3; (e) x. l = 0, m l = 0, y. l = 1, m l = –1, 0, or + 1, z. l = 2, m l = –2, –1, 0, +1, +2

Got questions? Get instant answers now!

State the Heisenberg uncertainty principle. Describe briefly what the principle implies.

Got questions? Get instant answers now!

How many electrons could be held in the second shell of an atom if the spin quantum number m s could have three values instead of just two? (Hint: Consider the Pauli exclusion principle.)

12

Got questions? Get instant answers now!

Which of the following equations describe particle-like behavior? Which describe wavelike behavior? Do any involve both types of behavior? Describe the reasons for your choices.

(a) c = λν

(b) E = m ν 2 2

(c) r = n 2 a 0 Z

(d) E = hν

(e) λ = h m ν

Got questions? Get instant answers now!

Write a set of quantum numbers for each of the electrons with an n of 4 in a Se atom.

n l m l s
4 0 0 + 1 2
4 0 0 1 2
4 1 −1 + 1 2
4 1 0 + 1 2
4 1 +1 + 1 2
4 1 −1 1 2
Got questions? Get instant answers now!

Questions & Answers

What a homogenous mixture
Allison Reply
Define homologous series
Chizoba Reply
when iron is exposed to moisture and it rusts,the value of deltaG for the reaction is
Mary Reply
what is chemistry
Siyanbola Reply
define aci according to Lewis
Ryhanna Reply
an acid is an electron pair acceptor according to lewis
Mary
What is a homogenous mixture
Allison
the third ionization energy of aluminium
sanmi Reply
name the allotrope of carbon used in gas masks
Moses Reply
Discuss the synthesis of sucrose
Ojiya Reply
What is a glycoside and discuss the formation
Ojiya
explain the transitioning of glucose molecules from Fischer projection of glucose to the Haworth projection
Rosey Reply
what is quantum
hezekiah Reply
what are metalliod
hezekiah
Metalloids are substances having the characteristics of both metals and non-metals
Ngwesse
what is acid
Tobi
define acid according to lewis
Ryhanna
what is valency
odukoya Reply
The number of chemical bonds the atoms of a certain element can form.
kenicia
what is ionization energy?
Hussniz Reply
ionization energy is qualitatively defined as the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom, molecule or io
Tobi
If a sample of neon gas at 25.00∘C and 0.500 atm is heated at a constant volume until the pressure is 0.850 atm, what must be the final temperature of the gas in Kelvin? Use −273.15∘C for absolute zero. Report your answer with three significant figures.
Philomina Reply
The final temperature of the gas in Kelvin is 506.855
Ngwesse
Define the term chemistry
Ahmed Reply
alchemy
MLG
explain law of definite proportion
MOTIA Reply
yes same idea
DEMGUE
wat?
Advic

Get the best Chemistry course in your pocket!





Source:  OpenStax, Chemistry. OpenStax CNX. May 20, 2015 Download for free at http://legacy.cnx.org/content/col11760/1.9
Google Play and the Google Play logo are trademarks of Google Inc.

Notification Switch

Would you like to follow the 'Chemistry' conversation and receive update notifications?

Ask