Electronic Structure of Atoms

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Nov 12, 2013 (3 years and 8 months ago)

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Electronic

Structure

of Atoms

Electronic Structure of Atoms

Resources


Our TB: Ch. 6 of
Chemistry: The Central
Science AP version
(10
th

edition)



Powerpoint * (from pearson) and in
-
class work



POGIL activities: (1)
Analysis of Spectral
Lines
and (2)
Interaction of Radiation and
Matter


Online resources for our TB (in particular
online quiz)



Chem tours from ch. 7 of the W.W.
Norton online book by Gilbert:



http://www.wwnorton.com/college/chemistry/gi
lbert2/contents/ch07/studyplan.asp


Animations from Glencoe site:


http://glencoe.mcgraw
-
hill.com/sites/0023654666/student_view0/chapter7/



Extra quizzes from Glencoe


http://glencoe.mcgraw
-
hill.com/sites/0023654666/student_view0/chapter7/




Video lectures from chem guy


http://www.kentchemistry.com/moviesfiles/chemguy/AP/C
hemguyAtomicTheory.htm




Handouts and practice problems from M.
Brophy’s web site

Electronic

Structure

of Atoms

Chapter 6

Electronic Structure

of Atoms

Chemistry, The Central Science
, 10th edition

Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

John D. Bookstaver

St. Charles Community College

St. Peters, MO



2006, Prentice Hall, Inc.

Electronic

Structure

of Atoms

Waves


To understand the electronic structure of
atoms, one must understand the nature of
electromagnetic radiation.


The distance between corresponding points
on adjacent waves is the
wavelength

(

)
.

Electronic

Structure

of Atoms

Waves


The number of waves
passing a given point per
unit of time is the
frequency (

)
.


For waves traveling at
the same velocity, the
longer the wavelength,
the smaller the
frequency.

Electronic

Structure

of Atoms

Electromagnetic Radiation


All electromagnetic
radiation travels at the
same velocity: the
speed of light (
c
), 3.00


10
8

m/s.


Therefore,

c

=


Electronic

Structure

of Atoms

The Nature of Energy


The wave nature of light
does not explain how
an object can glow
when its temperature
increases.


Max Planck explained it
by assuming that
energy comes in
packets called
quanta
.

Electronic

Structure

of Atoms

The Nature of Energy


Einstein used this
assumption to explain the
photoelectric effect.


He concluded that energy
is proportional to
frequency:

E

=
h



where
h

is Planck’s
constant, 6.63


10

34

J
-
s
(i.e. units for
h

are J•s)

Electronic

Structure

of Atoms

The Nature of Energy


Therefore, if one knows the
wavelength of light, one
can calculate the energy in
one photon, or packet, of
that light:


c

=


E

=
h


Electronic

Structure

of Atoms



For electromagnetic radiation
animation and problems see:




http://www.wwnorton.com/coll
ege/chemistry/gilbert2/tutorial
s/interface.asp?chapter=chap
ter_07&folder=frequency_wa
velength



For All Chem tours for the electrons
in atoms and periodic properties
topic see:


http://www.wwnorton.co
m/college/chemistry/gilb
ert2/contents/ch07/study
plan.asp


Recommeded chem tours
animations:


Electromagnetic radiation

Light Emission and Absorbtion

Bohr Model of the Atom

De Broglie Wavelngth

Quantum numbers

Electron configuration


Electronic

Structure

of Atoms

The Nature of Energy


Another mystery
involved the
emission spectra
observed from
energy emitted by
atoms and
molecules.

Electronic

Structure

of Atoms

The Nature of Energy


One does not observe
a continuous
spectrum, as one gets
from a white light
source.


Only a
line spectrum

of
discrete wavelengths
is observed.

Electronic

Structure

of Atoms

Go To Glencoe
Animation


http://glencoe.com/sites/common_a
ssets/advanced_placement/chemist
ry_chang9e/animations/chang_7e_
esp/pem1s3_1.swf



POGIL activity on Spectral Lines

(To Complete)

Electronic

Structure

of Atoms

The Nature of Energy


Niels Bohr adopted Planck’s
assumption and explained
these phenomena in this
way:

1.
Electrons in an atom can only
occupy certain orbits
(corresponding to certain
energies).

Electronic

Structure

of Atoms

The Nature of Energy


Niels Bohr adopted Planck’s
assumption and explained
these phenomena in this
way:

2.
Electrons in permitted orbits
have specific, “allowed”
energies; these energies will
not be radiated from the atom.

Electronic

Structure

of Atoms

The Nature of Energy


Niels Bohr adopted
Planck’s assumption and
explained these
phenomena in this way:

3.
Energy is only absorbed or
emitted in such a way as to
move an electron from one
“allowed” energy state to
another; the energy is
defined by

E

=
h


Electronic

Structure

of Atoms

The Nature of Energy

The energy absorbed or emitted
from the process of electron
promotion or demotion can be
calculated by the equation:


E

=

R
H


( )

1

n
f
2

1

n
i
2

-

where
R
H

is the Rydberg
constant, 2.18


10

18

J, and
n
i

and
n
f

are the initial and final
energy levels of the electron.

Electronic

Structure

of Atoms

Go To Glencoe and
Norton Animations


http://glencoe.com/sites/common_a
ssets/advanced_placement/chemist
ry_chang9e/animations/chang_7e_
esp/pem1s3_1.swf



POGIL activity on Interaction of
Radiation and Matter

(To Complete)


Go to Chem tour for Bohr Model of
atom (and Rydberg equation)


http://www.wwnorton.com/college/c
hemistry/gilbert2/tutorials/interface.
asp?chapter=chapter_07&folder=hy
drogen_energies

Electronic

Structure

of Atoms

The Wave Nature of Matter


Louis de Broglie posited that if light can
have material properties, matter should
exhibit wave properties.


He demonstrated that the relationship
between mass and wavelength was



=

h

mv

Electronic

Structure

of Atoms

The Uncertainty Principle


Heisenberg showed that the more precisely
the momentum of a particle is known, the less
precisely is its position known:




In many cases, our uncertainty of the
whereabouts of an electron is greater than the
size of the atom itself!

(

x
) (

mv
)


h

4


Electronic

Structure

of Atoms

Quantum Mechanics


Erwin Schrödinger
developed a
mathematical treatment
into which both the
wave and particle nature
of matter could be
incorporated.


It is known as
quantum
mechanics
.

Electronic

Structure

of Atoms

The Quantum Mechanical Model


Energy is quantized
-

It comes in chunks.


A
quantum

is the amount of energy needed to
move from one energy level to another.


Since the energy of an atom is never “in
between” there must be a quantum leap in
energy.


In 1926, Erwin Schrodinger derived an
equation

that described the energy and
position of the electrons in an atom


(this slide from: J. Hushen’s presentation on Atomic Structure at
http://teachers.greenville.k12.sc.us/sites/jhushen/Pages/AP%20Chemistry.aspx)

Electronic

Structure

of Atoms

Schrodinger’s Wave Equation

2
2
2 2
8
d
h
E
V
m dx

 

  
Equation for the
probability

of a single
electron being found
along a single axis (x
-
axis)

Erwin Schrodinger

(this slide from: J. Hushen’s presentation on Atomic Structure at
http://teachers.greenville.k12.sc.us/sites/jhushen/Pages/AP%20Chemistry.aspx)

Electronic

Structure

of Atoms

Quantum Mechanics


The wave equation is
designated with a lower
case Greek
psi

(

).


The square of the wave
equation,

2
, gives a
probability density map of
where an electron has a
certain statistical likelihood
of being at any given instant
in time.

Electronic

Structure

of Atoms

Quantum Numbers


Solving the wave equation gives a set of
wave functions, or
orbitals
, and their
corresponding energies.


Each orbital describes a spatial
distribution of electron density.


An orbital is described by a set of three
quantum numbers
.

Electronic

Structure

of Atoms

Principal Quantum Number,
n


The principal quantum number,
n
,
describes the energy level on which the
orbital resides.


The values of
n

are integers ≥ 0.

Electronic

Structure

of Atoms

Azimuthal Quantum Number,
l


This quantum number defines the
shape of the orbital.


Allowed values of
l

are integers ranging
from 0 to
n

1.


We use letter designations to
communicate the different values of
l

and, therefore, the shapes and types of
orbitals.

Electronic

Structure

of Atoms

Azimuthal Quantum Number,
l

Value of
l

0

1

2

3

Type of orbital

s

p

d

f

Electronic

Structure

of Atoms

Magnetic Quantum Number,
m
l


Describes the three
-
dimensional
orientation of the orbital.


Values are integers ranging from
-
l

to
l
:



l


m
l


l.


Therefore, on any given energy level,
there can be up to 1
s

orbital, 3
p

orbitals, 5
d

orbitals, 7
f

orbitals, etc.

Electronic

Structure

of Atoms

Magnetic Quantum Number,
m
l


Orbitals with the same value of
n

form a
shell
.


Different orbital types within a shell are
subshells
.

Electronic

Structure

of Atoms

Level

n 1 2 3

Sublevel

l

Orbital
m
l


Spin
m
s


0

0

0

0

1

0

-
1

0

1

0

-
1

2

1

0

-
1

-
2

2

1

0

1

= +1/2

=
-
1/2


Allowed Sets of Quantum Numbers for Electrons in Atoms

Electronic

Structure

of Atoms

s

Orbitals


Value of
l

= 0.


Spherical in shape.


Radius of sphere
increases with
increasing value of
n.

Electronic

Structure

of Atoms

s
Orbitals


Observing a graph of
probabilities of finding
an electron versus
distance from the
nucleus, we see that
s

orbitals possess
n

1
nodes
, or regions
where there is 0
probability of finding an
electron.

Electronic

Structure

of Atoms

p

Orbitals


Value of
l

= 1.


Have two lobes with a node between them.


Electronic

Structure

of Atoms

d

Orbitals


Value of
l

is 2.


Four of the
five orbitals
have 4 lobes;
the other
resembles a
p

orbital with a
doughnut
around the
center.

Electronic

Structure

of Atoms

Energies of Orbitals


For a one
-
electron
hydrogen atom,
orbitals on the same
energy level have
the same energy.


That is, they are
degenerate
.

Electronic

Structure

of Atoms

Energies of Orbitals


As the number of
electrons increases,
though, so does the
repulsion between
them.


Therefore, in many
-
electron atoms,
orbitals on the same
energy level are no
longer degenerate.

Electronic

Structure

of Atoms

Spin Quantum Number,
m
s


In the 1920s, it was
discovered that two
electrons in the same
orbital do not have
exactly the same energy.


The “spin” of an electron
describes its magnetic
field, which affects its
energy.

Electronic

Structure

of Atoms

Spin Quantum Number,
m
s


This led to a fourth
quantum number, the
spin quantum number,
m
s
.


The spin quantum
number has only 2
allowed values: +1/2
and

1/2.

Electronic

Structure

of Atoms

Pauli Exclusion Principle


No two electrons in the
same atom can have
exactly the same energy.


For example, no two
electrons in the same
atom can have identical
sets of quantum
numbers.

Electronic

Structure

of Atoms

Go To
www.ptable.com




IMPORTANT


Use periodic Table to help you write
electron configurations of atoms (and
ions)


Dynamic Periodic Table and
Investigate (play with) the
Orbitals

option (on Top Tabs) for quantum
numbers, orbitals and electron
configurations of various elements


Go To


Glencoe site for animations on
electron configuration


http://glencoe.mcgraw
-
hill.com/sites/0023654666/student_
view0/chapter7/animations_center.
html#


Electronic

Structure

of Atoms

Electron Configurations


Distribution of all
electrons in an atom


Consist of


Number denoting the
energy level


Electronic

Structure

of Atoms

Electron Configurations


Distribution of all
electrons in an atom


Consist of


Number denoting the
energy level


Letter denoting the type
of orbital



Electronic

Structure

of Atoms

Electron Configurations


Distribution of all
electrons in an atom.


Consist of


Number denoting the
energy level.


Letter denoting the type
of orbital.


Superscript denoting the
number of electrons in
those orbitals.


Electronic

Structure

of Atoms

Orbital Diagrams


Each box represents
one orbital.


Half
-
arrows represent
the electrons.


The direction of the
arrow represents the
spin of the electron.

Electronic

Structure

of Atoms

Hund’s Rule


“For degenerate
orbitals, the lowest
energy is attained
when the number of
electrons with the
same spin is
maximized.”

Electronic

Structure

of Atoms

Periodic Table


We fill orbitals in
increasing order of
energy.


Different blocks on
the periodic table,
then correspond to
different types of
orbitals.

Electronic

Structure

of Atoms

Some Anomalies


Some
irregularities
occur when there
are enough
electrons to half
-
fill
s

and
d

orbitals on a
given row.

Electronic

Structure

of Atoms

Some Anomalies


For instance, the
electron
configuration for
chromium is


[Ar] 4
s
1

3
d
5


rather than the
expected


[Ar] 4
s
2

3
d
4
.

Electronic

Structure

of Atoms

Some Anomalies


This occurs
because the 4
s

and 3
d

orbitals
are very close in
energy.


These anomalies
occur in
f
-
block
atoms, as well.

Electronic

Structure

of Atoms


ELECTRON SPIN


1920
--
chemists realized that since electrons interact
with a magnetic field, there must be one more concept
to explain the behavior of electrons in atoms.


m
s
--
the 4th quantum number; accounts for the reaction
of electrons in a magnetic field












MAGNETISM


magnetite
--
Fe
3
O
4
, natural magnetic oxide of iron


1600
--
William Gilbert concluded the earth is also a large spherical magnet with
magnetic south

at the north pole (Santa's habitat).


NEVER FORGET: opposites attract & likes repel



PARAMAGNETISM AND UNPAIRED ELECTRONS


diamagnetic
--
not magnetic [magnetism
di
es]; in fact they are
slightly

repelled. All electrons are PAIRED.


paramagnetic
--
attracted to a magnetic field; lose their magnetism when removed from the magnetic field; HAS ONE OR MORE
UNPAIRED ELECTRONS


ferromagnetic
--
retain magnetism upon introduction to, then removal from a magnetic field


All of these are explained by electron spins


Each electron has a magnetic field with N & S poles


electron spin is quantized such that, in an external magnetic field, only two orientations of the electron magnet and its spi
n a
re
possible


+/
-

1/2


H is paramagnetic; He is diamagnetic, WHY?


H has one
unpaired

electron


He has
NO

unpaired
electrons; all spins offset and cancel each other out



(Taken from summary notes posted on M. Brophy’s website)



Electronic

Structure

of Atoms


What about ferromagnetic?


clusters of atoms have their unpaired electrons aligned
within a cluster, clusters are more or less aligned and
substance acts as a magnet.
Don't drop it!!




When all of the domains, represented by these arrows
are aligned, it behaves as a magnet. This is what happens
if you drop it! The domains go indifferent directions and it
no longer operates as a magnet.

(Taken from summary notes posted on M. Brophy’s website)

Electronic

Structure

of Atoms


Activities and Problem set __

TB ch. 6


all sections required for
SAT II and AP exams and most
are required for regents exam


View and take notes on the
recommended animations


POGIL activities on

(1)
Analysis of
Spectral Lines
and (2)
Interaction
of Radiation and Matter




Online practice quiz
and work
due by
______



Ch 6 Problems: write out questions (or
photocopy them) ; write out answers &
show

work


First carefully study the sample
exercises in chapter 6 (you don’t have to
copy them out) and then
DO

all in
-
chapter practice exercises according to
the directions above.



Do all GIST, and Visualizing concepts,
problems


end of chapter 6 exercises
: To
be
assigned
in class