,
.:
, >,
Unwittingly, and
advice,
Vince the first-row transition metal had been
lured far away from home, and now found himself
i
.
::::, surrounded by heavier elements of the P-block.
! copyright Nick Kim
:.::: :: ÿ:ÿ!ÿ : :: ."!ÿ'' "iÿ -ÿ "'. :i
http:/lstrangematter.sci.waikato.ac.nzlÿ:ÿiÿ ' ÿi 'ÿiÿi,." :,: : • " ÿ:.
::
Name:
Class Period:
Test Date:
Chemistry Calendar
October 12
No school
Student Holiday!
Electrons
Introduction
20
19
Electron
Configurations s,
15
14
13
Orbitals and
Flame Test Lab
Energy Levels
22
21
p, d
Electron
Configurations f,
Electron
Configuration
and orbital
and Shorthand
Battleship
Test Review DUE! /
diagrams
24
25
16
½ DaV oÿÿ school
26
27
Electrons Test
NOTES Day 1: Let's Review
Niels Bohr's Model of the Atom
• Placed the ÿ1
ÿT irÿI
• Each orbit is called an
around the nucleus.
Iÿÿ6ÿ
and electrons will absorb or release
as they move between orbits.
• The
ÿjf}ÿ
absorbed or released is in the form of
• The lowest level was known as the ÿ ÿ0 i.} ÿ"} 6ÿ.
Schr6dinger Model of the Atom
• Mathematical modelthat
CCJIÿ ÿ !0E'ÿUV'ÿ
of the electrons of an
atom:
1. Electrons are found in
bÿ? ÿ0 ÿ
that predict the most likely place to find
the electron.
are weird shapes
.
3.
Each electron is
tÿ)ÿ ij ÿ
and no two electrons will have the exact same
"address."
Electrons
Electrons are found orbiting the nucleus and as you move down the periodic table, the electrons are
"ÿTIÿ ÿ"
away from the nucleus.
Each of the rows on the periodic table are called
I
The electrons in higher principle energy levels have
When elements are heated to high temperaturesÿ some of their
are
excited to iÿ }, 0ÿÿ'l ÿ ÿ} ÿJ
Characteristic colors of i} !!ÿiÿ
are emitted when these
excited electrons fall back to their original lower energy level, also known as ÿI ÿ ÿ ÿ
Match the term with the labels in the wave diagram to the right:
1. wavelength
2. amplitude
A
3. crest
ÿ
4. trough
B
Matching: {You try these.)
•
5. amplitude
'
a. number of waves cycles to pass a given point per unit of time
6. wavelength (;L)
b. the SI unit for frequency in cycles per second
7. frequency (f)
c. product of frequency & wavelength equaling 3.0 x 10l° cm/s
8. hertz (Hz or s-I)
d. range of wavelengths of electromagnetic radiation
9. speed of light (c)
B
e. the wave's height from the origin to the crest
10. spectrum
f. the distance between two crests in a wave
60o
I. ÿfalse? Explain. The frequency and wavelength of all waves are inversely related. :ÿ
2. White light separates into a rainbow of colors when iJ; passes through a glass prism. What visible color
has the longest wavelength & lowest frequency? ÿ0 ÿ! ÿ ÿ IV'
,
Max Planck showed mathematically that the amount of radiant energy (E) absorbed or emitted by a
bodyis ÿvÿ?ÿO(ÿOÿQdTÿi
to the frequency of the radiation: E = hxf, This helped explainthe
color change when a substance is heated.
.
In 1905 Einstein proposed iiÿ iÿ;ÿ
could be described as
that behave as if particles.
5. Light quanta are called
Calculations:
We have three equations we can use to calculate the energy transitions of electrons in atoms. They are
1. c=fk
2. E=hf
3.
E=hc
k
.
c=3.00 X 108 m/s or the speed of light
f-=frequency (s-1 or Hertz - Hz )
k=wavelength (meters - m)
E=Energy (Joules - J)
h=6.63 X 10-34 (Js)
What is the energy of a photon of green light with a frequency of 5.80 x 1014 S47 (/1 = 6.626 x 10-34 J.s)
E=hxfI
........
Ii x/O . :+ /
7. Calculate the wavelength of yellow light emitt d if the frequency is 5.10 x 1014 s-l? (c = 3.00 x 108 m/s)
I I 8
4;
8. Calculate the energy of a photon with a wavelength 0f6.7 x lO-7m?
E=hc
Day i Homework: Calculations
Part I
c=Zÿ
c = speed of light = 3.00 x 108 m/s
wavelength (L) should be expressed in meters (m)
frequency 0)) should be expressed in reciprocal seconds (s-1 or Hz)
1. What is th
radiation with a wavelength of 3.82 x 10 - 7 m? ÿat part of the
electromagnetic spectrum does this fall in? ÿes) ÿ-"'ÿv
2. Wh
..........
.
......
..............
'
..................
])
electromagnetic spectrum does this fall in?,
/
/
..... - ........ -ÿ-,,(,ÿ. 4oxlO
cÿred'light
if tl,e
3. What is the
-ÿ-/ .°
ox.
4. The green light
is 5.58 x 10-7m? Whatis the
emitted by excited
green light?
5. Gamma rays have frequencies around 1.0 x 10 Hz.
Part 2 of Homework
E = h ÿ)
h = Planck's constant = 6.626 x 10-34 J" s
L-;tÿ.,
6. How much
oes a photon of light with frequency 4.2 x 108 Hz have? what part of the
electromagneti6ÿectrum does this fall in?
7. It takes 6.63 x 10-18j of energy to eject an electron from a certain atom.
I/,oo
Notes Day 2
Electrons- Energv levels, Sublevels, and Orbitals
Where is the Electron?
o In the quantum mechanical model, the electrons are found OL}ÿtÿt!ÿ
the nucleus.
o To describe an electron's location, we can include
.
• Level I- Energy Level
Principle Energy Levels
The first horizontal row of the periodic table represents the
principle energy level. Show how these are organized in the Bohr model below.
I
n= i ; sublevels=
n= ÿ ' sublevels=ÿ'/pi
o Represented bythe letter,
n=l--)
o Each new
on the periodic table starts a new energy level.
o Each energy level has a di.f]:erentnumberofsublevels, a different number of orbitals, and a different
number of electrons.
Level II- Sublevels
o Based on the number of elements in our Periodic Table, there are four sublevels.
o Each sublevel has a unique ,ÿiQÿ}lÿ{ÿ
o The
o Higher Energy Level =
of the sublevel depends on the energy level.
Content Frame for IMPORTANT INFORMATION about the Sublevels
Shape
Number of Atomic Orbitals
Number of Electrons
Sublevel
You won't need to know the shape of
the orbitals in the d-sublevel.
You won't need to know the shape of
the orbitals in the f-sublevel.
Level III- Atomic Orbitals
o All electrons are located in an atomic orbital or [ÿ ÿF ÿ i'ÿ i
o An UÿYÿ lÿÿ
ÿ{" ÿIÿ/'ÿ ÿrepresents the area in which there is a
o Each atomic orbital can hold ÿ,ÿJO
chance of finding an electron.
electrons.
ij ÿ fiÿ ÿI#ÿ lÿ paths.
o Inside these orbitals, electrons take ÿtÿCÿ'ÿ and
Processing Your Notes
_1.
Which sublevel has a dÿbell shape?
a) s sublevel ÿsublevel c) d sublevel d) f sublevel
-J 2. Which sublevels will havÿthe same shape?
a) 3s and 3p ÿp and4p c)ls and 2p d) 4d and 3s
Sodium is found on the third row or Period 3 of the periodic table. How many energy levels do the
electrons of a sodium aÿ occupy?
a) 1(ÿ
c)11
d)23
How many orbitals are found in a d-sublevel?
a) 4
bÿbiÿ)
How mÿlÿy electrons caÿe
Lÿ2
c)10
d)14
held in one atomic orbital?
b)6
c)10
d)14
Which letter does not represent a curreÿsublevel of an energy level?
a) d
b)fÿ
d)p
As scientists create new elements, we will need to add new sublevels to the four existing sublevels. In
fact, the next sublevel will be called g. After looking at the trend in the number of orbitals for the
current sublevels, how many orbitals wzgÿd you predict would exist in a g-sublevel?
a) 7
b)8"ÿ(oÿ
d)32
7
Notes from PowerPoint = Continued
J
-II
First Energy Level
n= I
t
Putting it All Together
Different
Energy Levels
/
Second Energy Level
n=
T
T
Sublevels Present
Sublevels Present
T
T
Total # of OrbitaLs
Total # o* Orbitals
J
T
Total # of Electrons
I
T
(n)
I
i
Ft
\
Third Energy Level
I
Fourth Energy Level
n=
T
Sublevels Present
T
I
[
J
Sublevels Present
I
,Pjd
V
Total # of Orbitals
Total # of##ÿectrons
# of Electrons = ÿ ÿ) ÿ) ÿ¢
L
T
Total # of Orbitals Lÿ
T
T
Total: # ÿJÿlectrons
Total # of Electrons
of orbitals X
Electron Configurations
Electron Configurations
Processing Your Notes
the location of the electrons in an atom or ion.
ÿi::t ÿ
'g. How manyorbitals
a) 4
b)8
c)16
d)32
9. How many electrons are held in n=2?
d)16
10.
2followingAÿJevels
b)4 does; (ÿl
Whicha)
of the
not exist?
d)4f
,__ÿ11,
a) of
ls
b)ÿwould be
c)
3p
Which
the following
an expression
used to calculate the number of orbitals based on the energy level
(n)?
2n
b)n2
c) n + 6
d)2n2
8
1S22S22p63s23p4
Use the following electron configuration to answer the following three questions:
12. Which element is repÿented by this electron configuration?
a) Sodium"ÿ b)ÿlfur
c)argon
d)selenium
13. What is the highest ÿgy level in this electron configuration?
a) 2Lÿ
c)4
d)6
How many electronsÿcÿe.found in the s-ÿubJ.evel?
d)8
Day 2 Homework
I. How many orbitals are found in a 2p sublevel?
,
How many electrons can be held in a 2d sublevel? ÿÿ'ÿ/ IÿO ÿd
f
3. How many electrons exist in a f-sublevel where n = 4? l+0
4. How many orbitals are in a 5f sublevel?
°
Answer the questions based on the electron configuration.
1s22s22p63s23p64s23ds
a. What element is represented by this electron configuration?
b. What is the highest energy level occupied?
c. Which energy levels are incomplete?
,J
d. Which sublevel contains the most electrons?
,
f
6. Give the symbol for the element that has an electron configuration ending in 3ps.
7. If the electron configuration of an element ends in 4d3, what is the name of this element?
Use the following electron configuration to answer the following three questions:
lS22S22p63s23 p64s23d1°4pI
ÿ.ÿ /ÿ
15. Which sublevÿba, s the most electrons?
a) s
tÿ,b)p)'ÿ/
c)d
How many electrons are in t bÿhighest energy level?
a) 1
b)2
(.ÿ3
What element is represented by the electron configuration?
a) titanium b)copper ÿ¢c}galliu m d)germanium
9
Day 3 Notes
Writing Electron Configurations
Notes from the PowerPoint
• Rule #1: fUld i l !ÿ
Rule #2:
s
1
2
p
3
6
d
5
10
f
7
14
fÿtJÿ c!?i?.
orient41
1s22s22.p°3s23p64s23d1°4pI
Energy --)
Rule #3:
I0
Energy
8
TSi I
2
2A
3
3B
4
4B
5
58
6
68
7
7g
I8
13
@
88
I0 I
1]
1B
14
15
16
17
3A 4A
ÿA
6R
7A
12
2B
:'" -94
8
Kr
• Ge Ae
,:K /
o 52
Vÿy
i:;iiÿ: tn .Sn Sb
Te
iÿTJEÿ
ubÿ
Sÿ
:ÿHg TI ..... Pb ...... Bi
Lanÿntÿ Seÿs
..........
Ce
.....
-Pr-Nd
:
..........
Gd- Er
Acÿint@Seriÿs
1. Color-code the periodic table according to
the table posted by your teacher.
2. Label the s, p, d, and f blocks on your table
/
{- J .
Orbital Diagrams
.... J
iS
2s
2ÿ
3s
1 box = t atomic orbital
s-subtevel -) 1 box
p-sublevel--> 3 boxes
d-subleve! --> 5 boxes
f-sublevel -) 7 boxes
I arrow- = 1 electron
11
a;
. :At Rn
ÿ::ÿ:::: :Yb•
Sample Electron Configuration and Orbital Diagram
Hydrogen
• Beryllium
• Fluorine
t+
h
• Chlorine
•ÿP°tassiumÿ
ÿ
ÿ
ÿ ,
• Important Reminders
•
Your
number tells you the energy level or coefficient fdr, yOur configurations.
• Knowyour limits for each sublevel!
• You have to use your periodic table be sure that you are following the Aufbau Plÿirÿiÿleand Hund's Rule.
(look at what energy level and what orbitals are present for that levelÿ.ÿrÿ+iÿ
ls -) 2s --> 2p --> 3s -> 3p --> ÿ
ls -> 2s -> 2p --> 3s --> 3p --> 4s
/ÿ%
ÿ%ÿ
Electron Configurations Containing the d-Sublevel
The energy level of d-sublevel will ALWAYS be ÿ,IVÿ iÿ than the row or period number.
"ÿ
Iÿ+ 7f
, ,ÿ ÿ.ÿ
Electron Configuration
-+
Day 3 Homework
Element °
Energy Levels
Sublevels
1S22S22p63sZ3pO4sz
+++
!ÿ,-+? ++++++0ÿ
lsZ2s2
"
lsZ2sZ2pÿ3sZ3pÿ4sZ3dÿ°4p0
lsZ2sZ2pÿ3sZ3pÿ4sz
+j_
//i h+i+.t
Write the electron configurations and draw the orbital diagrams for each of the following elements:
Os
I
• TI
++" +++;++ 8+;+'++ 7%
12
+++
Day 4 Notes
Where does the f-block "fit in"?
The f-block is considered to be part of ÿ ÿ/IO ÿJÿ@
1
2
71
2 3: :4 .5 6 7 8ÿ 9110
6 7 8 910 1112!3 1;4
• Electron Configurations Containing the f-Sublevel
The energy level of f-sublevel will ALWAYS be
than the row or period number.
Processing Your Notes
• Europium
• Tungsten
Bismuth
Bohrium
/
13
Writing Short Hand Electron Configurations
Key Terms
• Noble Gases
• Lewis dot diagrams
• Valence Electrons
• Groupsor Families
Key Questions
• What elements are exceptions to the rules for electron configurations?
• How do you write short hand electron configurations for the elements in the periodic table?
• How do you determine the number of valence electrons from an electron configuration?
• How do you determine the number of valence electrons from the periodic table?
• How do you draw Lewis dot diagrams?
Notes from PowerPoint
• Exceptions to the Rules
MAKE SURE YOU KNOW THESE!
O
Chromium, Cr
1s22s22p63s23p64s23d4
o Predicted:
%'
o Actual:
o Copper, Cu
o Predicted:
1s22s22p63s23p64s23d9
o Actual:
1s22s22p63s23p6 ÿ-ÿ 156!dO
Short Hand Notation
[Ne]3s23p2
Uses a ÿ ÿJÿÿJÿÿI ÿt2_
(Group 18) to represeÿ.ÿ the
electrons are represented
innermost electrons.
the same way.
Noble Gases= ÿ/ ÿ/ /ÿ ÿ/ ÿi#!ÿ/
Short Hand Notation Hints
• To find the noble gas, look at the noble gas from the previous row or the row above the element.
The energy level or coefficient of the -(ÿ and ]ÿ_._-sublevel is equal to the row or period number.
The energy level or coefficient of the Cÿ
-sublevel is ÿ)ÿ ÿ than the period
number and for the
than the period number.
ÿ
-sublevel -ÿ'lAÿ ÿ
14
Draw Lewis Dot diagrams for the following elements:
Sodium
p°
Phosphorus
Iodine
,ÿ o
Neon
Q
0
0
Day 4 Homework
1. Write the shorthand notation for the following elements:
a. Hg [ÿ ÿZ IL]:ÿ ÿ ÿ-LÿL.IO
C°
-Is ÿ-ÿ ÿ--4:I
Study Guide for the Electron
DUE 10/18/151!
1. What is a quanta of energy?
4,
2. If an electron moves farther from the nucleus, it has
.
ÿÿÿ
energy.
To emit energy, electrons move to a lower energy level, which is G[ 0.ÿ J(ÿ
to the
nucleus.
4. Can an electron exist in between energy levels?
Yes
or
5. Who developed the quantum mechanical model?
6. How many electrons can occupy each atomic orbital?
o
What percent chance do you have of finding an electron in its orbital?
.
How many orbitals are found in a d-sublevel?
.
In order for electrons to occupy the same atomic orbital, electrons must have {ÿ ÿ00 ÿtÿ(ÿpins.
ÿ"
iÿ-/ÿ/ÿ/I
10. The letter, n, is used to represent the
. In other words, n =2 is the
same thing as saying the second energy level.
11. How many electrons can occupy a f-sublevel?
12. Which sublevel has a spherical shape?
13. What sublevel has three atomic orbitals?
P
14. What was incorrect about Bohr's planetary model of the atom?
15. What element has the electron configuration of 1s22s22p63s23p64s23dS? tÿA ÿ ÿ(ÿ
16. What is wrong with this electron configuration: ls22s22pT? ÿ) ÿVÿiJ ÿ ÿ 1ÿ/ÿ
17. For the electron configuration, 1s22s22p1, how many electrons are in the second energy level?ÿ
18. For the electron configuration, 1s22s22p63s23p64s13ds, which sublevels are incomplete? Also specify
the energy level of the sublevel.
/ÿ ÿ-ÿ Cÿÿiÿ ÿ C
16
I
19. If the first energy level only has an s-sublevel, there will be
a maximum of
(ÿ
atomic orbital and
electrons on n = 1.
20. If the second energy level has a s sublevel and a p sublevel, there will be
0ÿ
atomic orbitals and a maximum of ÿJ
electrons on n = 2.
I Ve
21. If the third energy level has a s-sublevel, a p ble , and a
atomic orbitals and a maximum of i ÿ
3-
blevel, there will be
electrons on n =3.
22. If the fourth energy level
ÿ
•
.ÿb aÿf sublevel,
a shas ÿublevel,ÿa
p sublevel, aÿsublevel,
and
there will be
Iÿ
atomic orbitals and a maximum of ÿ ÿ electrons on n =4.
23. Which two elements have electron configurations that are exceptions to the rules? Write their name
AND symbol.
Cv - O,hv-omioÿ
C,O- coppur
24. Write the electron configuration for each of the following elements.
a. Titanium (Ti) !ÿ2-ÿ2ÿ[p ÿ¢2 ÿCÿ q;ÿ ÿ ÿCI/ÿ,
c. Lopper (Cu)
iSz ÿ-z ÿfÿ0 % z 3p ÿ 4.ÿa .ÿd to
25. The electron configuration below represents the configuration of an ion with a -2 charge, What
element would this represent?
Pÿloÿphovuÿ
lS22S22p6
26. Which sublevels do not exist and on which energy levels?
27. What two elements have exactly 5 electrons in their 3d sublevel?
28. State/Explain Aufbau Principle.
kcdYrÿoÿ0!ll %/1 .4ÿ¢ o/4ÿi c uvbi4ÿoll
29. State/Explain Pauli s Exclusion Principle,
30. State/Explain Hund's rule. ÿ 60.,ÿ ÿ...0 LV.ÿ
<,9
31. Who proposed the quantum mechanical model?
32. How many orbitals are located in n=2?
33. How many d-orbitals are found in n=3?
34. How many p-orbitals are found in the first energy level? LJ
35. How many sublevels are in the fourth principal energy level? ÿ/ÿ/
36. List the types of electromagnetic radiation in order of increasing energy.
37. Which has more energy: red light or violet light? ÿ 10"iÿ>ÿ
38. What element has an electron configuration that ends in 5p2?
39. What element has an electron configuration: [Xe]6s24f145d47 Tÿ)ÿ ÿ ÿ?ÿ/ÿ
40. What element has the electron configuration, lsZ2s22p63s23p2? ÿ(ÿ111 C(ÿ
41. How many energy levels are found in a potassium atom?
42. Draw the orbital diagram for phosphorus. How many electrons are in the p sublevel?
43. Draw the orbital diagram for carbon. How many unpaired electrons are found in carbon?
18
Using your equations on page 6, fill out the table below. You will need to use the work space
provided.
Wavelength (m)
Frequency ÿz or s"l)
Energy (J)
0.001
,
2.
- S
7.0 x 1013
: -4 <+, ÿ /
1.2 X 10-7
3.
. jz ÿ x
2.0 x 10-is
4.
f: >: ;-, <? /'
ii,i;) ?> :'ÿ
1.3 X 1022
5. ,,h
>
Show work for questions above here!
"
,s,ooxto --
4,ooi
2,
"<,
\
4ÿ
S,
...........
\
. +
Element
Element
Symbol
Name
Electron Configuration
Noble gas shorthand
B
C
N
F
I
Ne
iÿ ÿ •:
S•
Na
,i
A1
S
i
Si
•
/ +
i¸,
]
s¸
?
P
iÿ,t¸ ÿ• !ÿÿ ÿ
Y..-
-+
C1
K
Ca
Sc
Ti
9
Cr
•j
Co
i
[ i
20