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wel
com
e to
ch
emis
try
Peri
od
ic T
able
of
the
Elem
ents
20
11
ww
w.c
hem
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yad
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ture
.co
m
+1
Alk
ali
meta
ls
Alk
alin
eea
rth
met
als
+2
Tra
nsit
ion
meta
ls: 2
val
enc
e e
lect
rons
+3
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-4-3
-2
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Nob
lega
ses
hal
ogen
s
1H
hyd
roge
n1.
01
11N
aso
diu
m
22
.99
12M
gm
agne
sium
24
.31
3Li
lith
ium
6.9
4
4B
eb
eryl
lium
9.0
1
19
K pota
ssiu
m
39
.10
20
Ca
calc
ium
40
.08
37
Rb
rub
idiu
m
85
.47
21S
csc
andiu
m4
4.9
6
22T
iti
tani
um4
7.9
0
23V
vana
diu
m5
0.9
4
24
Cr
chro
miu
m5
2.0
0
25
Mn
man
gane
se5
4.9
4
26
Fe
iron
55
.85
38
Sr
stro
ntiu
m
87
.62
39
Yyt
triu
m
88
.91
40
Zr
zirc
oniu
m
91.
22
41 ni
obiu
m
92
.91
42
Mo
mol
ybden
um
95
.94
43T
cte
chne
tium
96
.91
44R
uru
then
ium
101.
07
55
Cs
cesi
um
132
.91
56
Ba
bar
ium
137
.33
71
Lu
Lut
etiu
m
174
.97
72
Hf
haf
nium
178
.49
73
Ta
tant
alum
180
.95
74
Wtu
ngst
en
183
.85
75R
erh
eniu
m
186
.21
76
Os
osm
ium
190
.20
87
Fr
fran
cium
22
3.0
2
88
Ra
radiu
m
22
6.0
2
103
Lr
law
renc
ium
26
2.1
1
104R
fru
ther
ford
ium
26
1.11
105D
bdub
nium
26
2.1
1
106
Sg
seab
orgi
um
26
3.1
2
107
Bh
boh
rium
26
4.1
2
108H
shas
sium
26
5.1
3
27
Co
cob
alt
58
.93
28
Ni
nick
el5
8.7
1
29C
uco
pper
63
.55
30
Zn
zinc
65
.37
31G
aga
lliu
m
69
.72
32G
ege
rman
ium
72
.59
13A
lal
umin
um
26
.98
45
Rh
rhod
ium
102
.91
46
Pdpa
llad
ium
106
.40
47
Ag
silv
er
107
.87
48
Cd
cadm
ium
112
.40
49
In
indiu
m
114
.82
50
Sn
tin
118
.69
33
As
arse
nic
74
.92
14S
isi
lico
n
28
.09
15P
phos
phor
us
30
.97
51
Sb
Ant
imon
y)
121.
75
77
Ir
irid
ium
192
.22
78
Ptpl
atin
um
195
.09
79A
ugo
ld19
6.9
7
80H
gm
ercu
ry2
00
.59
81
Tl
thal
lium
20
4.3
7
82
Pb lead
20
7.1
9
83
Bi
bis
mut
h
20
8.9
8
109
Mt
Mei
tner
ium
(26
8)
110D
sDarm
stadtium
(28
1)
111R
gro
entg
eniu
m
(27
2)
112U
ubU
nunb
ium
(28
5)
113U
utun
untr
ium
(28
4)
114U
uqun
unqu
adiu
m
(28
9)
115U
upun
unpe
ntiu
m
(28
8)
5B
bor
on
10.8
1
6C
carb
on
12.0
1
7N
nitr
ogen
14.0
1
8O
oxyg
en
16.0
0
9F
fluo
rine
19.0
0
2
He
hel
ium
4.0
0
10N
ene
on
20
.18
16S
sulf
ur
32
.07
17C
lch
lori
ne
35
.45
18A
rar
gon
39
.95
34
Se
sele
nium
78
.96
35
Br
79
.91
36
Kr
kryp
ton
83
.80
52
Te
tellur
ium
127
.60
53
I iodin
e12
6.9
0
54
Xe
xen
on
131.
30
84
Popo
loni
um
(210
)
85
At
asta
tine
(210
)
86R
nra
don
(22
0)
116U
uhun
unhex
ium
(28
9)
117 U
usun
unse
ptiu
m
(29
5)
118U
uoun
unoc
tium
(29
3)
57
La
lant
han
um
138
.91
58
Ce
ceri
um
140
.12
59
Prpr
aseo
dym
ium
140
.91
60
Nd
neod
ymiu
m
144
.24
61
Pmpr
omet
hiu
m
144
.91
62S
msa
mar
ium
150
.41
63
Eu
euro
pium
151.
96
65
Tb
terb
ium
158
.92
89A
cac
tini
um
22
7.0
3
90
Th
thor
ium
23
2.0
4
91
Papr
otac
tini
um
23
1.0
4
92
Uur
aniu
m
23
8.0
3
93
Np
nept
uniu
m
23
7.0
5
94
Pupl
uton
ium
24
4.0
6
95
Am
amer
iciu
m
24
3.0
6
96C
mcu
rium
(24
7)
66
Dy
dys
pros
ium
162
.50
67
Ho
Hol
miu
m
164
.93
68
Er
erb
ium
167
.26
69
Tm
thul
ium
168
.93
70
Yb
ytte
rbiu
m
173
.04
97
Bk
ber
kelium
(24
9)
98
Cf
califo
rniu
m
(25
1)
99E
sei
nste
iniu
m
(25
4)
100F
mfe
rmiu
m
25
7.1
0
101M
dm
endel
eviu
m
(25
6)
102N
o
(25
4)
Nb
Ace
tate
CH
3C
O2
-B
isul
fite
HS
O3
-C
hlo
rite
ClO
2-
Hyd
roxid
e O
H-
Nit
rite
NO
2-
Phos
phid
e P3
-
Am
mon
ium
NH
4+
Bro
mid
e B
r-C
hro
mat
e C
rO4
2-
Hyp
ochlo
rite
ClO
-O
xid
e O
2-
Sul
fide
S2
-
Bro
mid
e B
r-C
arbon
ate
CO
32
-C
yani
de
CN
-Io
did
e I
-Pe
rchlo
rate
ClO
4-
Sul
fate
SO
42
-
Bic
arbon
ate
HC
O3
-C
hlo
rate
ClO
3-
Dic
hro
mat
e C
r 2O
72
-N
itra
te N
O3
-Pe
rman
gana
te M
nO4
-T
hio
sulf
ate
S2O
32
-
Bis
ulfa
te H
SO
4-
Chlo
ride
Cl-
Flu
orid
e F
-N
itri
de
N3
-Ph
osph
ate
PO4
3-
com
mon
ani
ons
Mon
oval
ent
ca
tion
s:G
roup
1, A
g: +
1G
roup
2, Z
n: +
2G
roup
3, A
l: +
3
Gd
gadol
iniu
m
157
.25
64
nob
eliu
m
0
1s 2s
3s
4s
5s
6s
7s
3d
4d
5d
6d
4p
5p
6p
7p
3p
2p
4f
5f
Sym
bol
:S
olid
Liqu
idG
asM
anm
ade
nam
e
Ato
mic
mas
s
Ato
mic
nu
mber Sc
scan
diu
m
44
.96
21
Act
iniu
mA
c 22
7.08
Alu
min
um
Al 2
6.98
Am
eric
ium
Am
243
.06
An
tim
on
ySb
121
.75
Arg
on
Ar
39.9
6A
rse
nic
As
74.9
2A
stat
ine
At
(210
)B
ariu
mB
a 13
7.33
Ber
keliu
mB
k (2
49)
Ber
ylliu
mB
e 9.
01B
ism
uth
Bi 2
08.9
8B
oh
riu
mB
h 2
64.1
2B
oro
nB
Bro
min
eB
r 79
.91
Cad
miu
mC
d 1
12.4
0C
alci
um
Ca
40.0
8C
alif
orn
ium
Cf
(261
)C
arb
on
C 1
2.01
Cer
ium
Ce
140.
12
Ces
ium
Cs
132.
91C
hlo
rin
eC
l 35.
45C
hro
miu
mC
r 52
.00
Co
bal
tC
o 5
8.93
Co
pp
erC
u 6
3.55
C
uri
um
Cm
Dar
mst
adti
um
Ds
(281
)D
ub
niu
mD
b 2
62.1
1D
ysp
rosi
um
Dy
162.
50Ei
nst
ein
ium
Es 2
52.0
8Er
biu
mEr
167
.26
Euro
piu
mEu
151
.96
Ferm
ium
Fm 2
57.1
0Fl
uo
rin
eF
Fran
ciu
mFr
Gad
olin
ium
Gd
Gal
lium
Ga
Ge
rman
ium
Ge
19.0
0G
old
Au
196
.97
Haf
niu
mH
f 17
8.49
Has
siu
mH
s 26
5.13
H
eliu
mH
e 4.
00H
olm
ium
Ho
164
.93
Hyd
roge
nH
1.0
1In
diu
mIn
114
.82
Iod
ine
I 126
.90
Irid
ium
Ir 1
92.2
2Ir
on
Fe 5
5.85
Kry
pto
nK
r 83
.80
Lan
than
um
La 1
38.9
1La
wre
nci
um
Lr 2
62.1
1Le
adP
b 2
07.1
9Li
thiu
mLi
6.9
4Lu
teti
um
Lu 1
75.0
0M
agn
esiu
mM
g 24
.31
Man
gan
ese
Mn
54.
94
Mei
tner
ium
Mt
268.
14M
end
elev
ium
Md
258
.10
Mer
cury
Hg
200.
59M
oly
bd
enu
mM
o 9
5.94
Ne
od
ymiu
mN
d 1
44.2
4N
eo
nN
e 2
0.18
Ne
ptu
niu
mN
p 2
37.0
5N
icke
lNi 5
8.69
Nio
biu
mN
b 9
2.91
Nit
roge
nN
14.
01N
ob
eliu
mN
o 2
59.1
0O
smiu
mO
s 19
0.23
Oxy
gen
O 1
6.00
Pal
lad
ium
Pd
106
.42
Ph
osp
ho
rus
P 3
0.97
Pla
tin
um
Pt
195.
08P
luto
niu
mP
u 2
44.0
6P
olo
niu
mP
o 2
08.9
8P
ota
ssiu
mK
39.
10P
rase
od
ymiu
mP
r 14
0.91
Pro
met
hiu
mP
m 1
44.9
1P
rota
ctin
ium
Pa
231.
04
Rad
ium
Ra
226.
03R
ado
nR
n 2
22.0
2R
hen
ium
Re
186.
21R
ho
diu
mR
h 1
02.9
1R
ub
idiu
mR
b 8
5.47
Ru
then
ium
Ru
101
.07
Ru
ther
ford
ium
Rf
261.
11Sa
mar
ium
Sm 1
50.3
6Sc
and
ium
Sc 4
4.96
Seab
org
ium
Sg 2
66.1
2Se
len
ium
Se 7
8.96
Silic
on
Si 2
8.09
Silv
erA
g 10
7.87
Sod
ium
Na
22.9
9St
ron
tiu
mSr
87.
62Su
lfu
rS
32.0
7Ta
nta
lum
Ta 1
80.9
5Te
chn
etiu
mTc
97.
91Te
lluri
um
T6 1
27.6
0Te
rbiu
mTb
158
.93
Thal
lium
Tl 2
04.3
8Th
ori
um
Th 2
32.0
4Th
uliu
mTm
168
.93
Tin
Sn 1
18.7
1Ti
tan
ium
Ti 4
7.87
Tun
gste
nW
183
.84
Ura
niu
mU
238
.03
Van
adiu
mV
50.
94X
eno
nX
e 13
1.29
Ytt
erb
ium
Yb
173
.04
Ytt
riu
mY
88.
91Zi
nc
Zn 6
5.41
Zirc
on
ium
Zr 9
1.22
(and
NH
4+ )
met
alno
nmet
alm
etal
loid
metal
nonmetal
1 va
lenc
eele
ctro
n2
val
enc
eele
ctro
ns
Val
ence
ele
ctro
ns:
8
45
67
3
(H is
a no
nmet
al)
bro
min
e
Gro
up 1
Gro
up 2
Gro
up 3
Gro
up 4
Gro
up 5
Gro
up 6
Gro
up 7
Gro
up 8
Gro
up 9
Gro
up 1
0G
roup
11
Gro
up 1
2
Gro
up 1
3G
roup
14
Gro
up 1
5G
roup
16
Gro
up 1
7
Gro
up 1
8
to 71 to 10
3
error x 100accepted value
D
D D
D D D
D
D
D
D
D
D D
D D
° °
° °
seating chart period 2
normal
labs
tests
Craig A
Ben B
Elizabeth B
Matt B
Annalese D
Ambur-Lynn D Jake H
Anne K Anna K
Gabriella L
Joe F
Courtney O
Colton S
Sydney S Ashleigh W Mariana T Shaun S
Chris M
Craig A
Ben B
Elizabeth B Matt B An
nalese D
Am
bu
r-Lynn
D
Jake H
An
ne K
An
na K
Gabriella L
Joe F
Courtney O
Colton S
Sydney S Ashleigh W Mariana T Shaun S
Chris M
Craig A
Ben B
Elizabeth B Matt B An
nalese
D
Am
bu
r-Lynn
D
An
ne K
An
na K
Gabriella L
Jpe F
Courtney O
Colton S
Sydney S Ashleigh W Mariana T Shaun S
Chris M
seating chart period 3
normal
labs
tests
Halle A
Brittany B
William B
Cath
erine D
Alyssa D
Margerite
D
Ku
le H
Peyto
n J
Jessica M
Brian
na M
Elizabet D
Joshua O
Jenna P
Alexandra P Deanna V Lacey T Mckenzie S
Varun N
Halle A
Brittany B
William B Catherine D
Alyssa D
Margerite
D
Peyto
n J
Jessica M
Brianna M
Elizabet D
Joshua O
Jenna P
Alexandra P Deanna V Lacey T Mckenzie S
Varun N
Hal
le A
Brittany B
William B Catherine D
Alyssa D Margerite D Peyton J Jessica M
Brianna M
Elizabet D
Josh
ua O
Jenna P
Alexandra P Deanna V Lacey T Mckenzie S
Varun N
seating chart period 4
normal Ted A
Luciano A
Alexa B
Ryan
C
Ke
vin C
Dian
a D
Emm
a G
Aaro
n G
Qu
inn
G
Joe G
Sara D
Roland L
Chris M
Garrett M Ben S Steven S Jessica R
Mark L
Andrew T
Megan T
Mikayla V
Joe W
Amanda W
labs Ted A
Luciano A
Alexa B
Ryan C
Ke
vin C
Dian
a D
Emm
a G
Aaro
n G
Qu
inn
G
Joe G
Sara D
Roland L
Chris M
Garrett M Ben S Steven S Jessica R
Mark L
Andrew T
Megan T
Mikayla V
Joe W
Amanda W
tests Ted A
Luciano A Alexa B
Ryan
C
Kevin C
Dian
a D
Emm
a G
Aaro
n G
Qu
inn
G
Joe G
Sara D
Roland L
Chris M
Garrett M Ben S Steven S Jessica R
Mar
k L
Andrew T
Megan T
Mikayla V
Joe W
Amanda W
seating chart period 5
normal Kayleigh C
Aaron C
Lucas D
Ben
E
Dan
F
Seth G
Mich
ael I
Grace I
Ch
ris M
Am
and
a M
Evan H
Kathryn M
Alissa R
Bronwyn R David S Gabrielle S Olivia S
Julia M
Trevor V
Sam W
Ashley Z
Mary W
labs Kayleigh C
Aaron C
Lucas D
Ben
E
Dan
F
Seth G
Mich
ael I
Grace I
Ch
ris M
Am
and
a M
Evan H
Kathryn M
Alissa R
Bronwyn R David S Gabrielle S Olivia S
Julia M
Trevor V
Sam W
Ashley Z
Mary W
tests Kayleigh C
Aaron C
Ben
E
Dan F
Seth G
Michael I
Grace I
Ch
ris M
Amanda M
Evan H
Kath
ryn M
Alissa R
Bronwyn R David S Gabrielle S Olivia S
Julia M
Trevor V
Sam W
Ashley Z
Mary W
seating chart period 7
normal Nicole B
Zoe B
Klaire C
Kath
leen C
Brian
D
Reb
ecca E
Shan
e G
Dan
G
Mike G
Steph
anie M
Jack F
Megan O
Clara P
Lindsey U Paul W Claire W James W
Lauren M
Ian W
Xiao X
Anny Y
Alexandra Z
labs Nicole B
Zoe B
Klaire C
Kath
leen C
Brian
D
Reb
ecca E
Shan
e G
Dan
G
Mike G
Steph
anie M
Jack F
Megan O
Clara P
Lindsey U Paul W Claire W James W
Lauren M
Ian W
Xiao X
Anny Y
Alexandra Z
tests Nicole B
Zoe B
Kath
leen C
Brian D
Reb
ecca E
Shan
e G
Dan G
Mike G
Stephanie M Jack F
Megan
O
Clara P
Lindsey U Paul W Claire W James W
Lauren M
Ian W
Xiao X
Anny Y
Alexandra Z
SAFETY CONTRACT—CHEMISTRY
Mt. St. Joseph High School
Please read the following statements regarding your behavior in the chemistry laboratory.
You are required to sign this document and turn it into your teacher today.
I have seen the video, Safety in the Chemistry Laboratory (at the beginning of the year), that describes laboratory safety, laboratory hazards, and safe
laboratory techniques.
My teacher has pointed out to my class all of the following safety features in the chemistry laboratory: safety shower, eye wash stations, first aid kit, fire
blanket, fire extinguishers and fire exit.
I agree to the following safety procedures when I am in the chemistry laboratory:
Wear goggles on my eyes at all times during chemistry laboratory experiment when using any amount of chemicals or whenever my teacher deems it
necessary to wear goggles. An apron is also required.
Conduct yourself in a responsible manner at all times in the laboratory.
Follow all written and verbal instructions carefully. If you do not understand a direction or part of a procedure, ask the instructor before proceeding.
Perform only those experiments authorized by the instructor. Never do anything in the laboratory that is not called for in the lab procedures or by your
instructor. Unauthorized experiments are prohibited.
Never remove chemicals or laboratory equipment from the lab area without permission from your instructor.
Never enter the chemical storage room or preparation area (behind the front desk) unless given specific permission from your instructor.
Be prepared for your work in the laboratory. Read all procedures thoroughly and have the objectives and procedure portion of your report completed
before you come to lab. Never fool around in the laboratory. Horseplay, practical jokes, and pranks are dangerous and prohibited. They are reason for not
only detention, removal from the lab resulting in a failing grade, but also suspension from school.
Keep aisles clear. Push your stool under the table when not in use.
Experiments must be personally monitored at all times. You are assigned a laboratory station at which to work. Do not wander around the room, distract
others, interfere with the experiments of others, or talk across the room.
Contact lenses should not be worn if possible whenever in the laboratory. No coats, sweaters, or loose clothes. No book bags in the lab.
Report an accident or spill to the instructor no matter how trivial it may appear.
Never handle broken glass with your bare hands. Use a brush and dustpan to clean up broken glass. Place broken glassware in the designated glass
disposal container.
Examine glassware before each use. Never use chipped or cracked glassware. Always wash dirty glassware.
* Do you wear contact lenses? Do you own glasses that you could wear to perform a lab?
YES YES
NO NO
Agreement:
I, _____________________________________, (student’s name) have read and agree to follow all of the safety rules set forth in this contract. I realize
that I must obey these rules to insure my own safety, and that of my fellow students. I will cooperate to the fullest extent with my instructor and fellow
students to maintain a safe lab environment. I will also closely follow the oral and written instructions provided by the instructor. I am aware that any
violation of this safety contract may result in being removed from the laboratory, detention, receiving a failing grade, and/or dismissal from the lab.
_______________________________________________
Student signature
_______________________________________________
Date
Dear Parent or Guardian:
We feel that you should be informed regarding the school’s effort to create and maintain a safe science classroom/laboratory environment.
With the cooperation of the instructors, parents, and students, a safety instruction contract can eliminate, prevent,
and correct possible hazards.
Your signature on this contract indicates that you have read this Student Safety Contract, are aware of the measures taken to insure the safety of your son
in the laboratory, and will instruct your son to uphold his agreement to follow these rules and procedures in the laboratory.
________________________________________________
Parent signature
________________________________________________
Date
1
4
Oh heck I know that
Controls:
StandardsFor comparison
O
HE
C
The 4-letter mnemonic for this simplified scientific method
all experiments need these: What is a positive control? Example:
What is a positive control? Example:
5
O OH
NH2
O O
O
O
NH
O
OH
O
alkenealkanealkyne ether alcohol
amine amide carboxylic acidaldehyde ketone ester
CC C
H
H
H
H
C
C
C
C
C
C
C
O
O OH
C
O
C
H
H
H
H
H
HH
Br
Br
Br
Br
Br
Br
Br
Br
NH
O
1. What is chemistry?
2. What is matter?
3. What is not matter? Give examples.
4. What do chemists do?
5. Where does chemistry fit in with the other branches of science?
6. Name a branch of science more basic than chemistry.
7. List the branches of science from basic to applies.
8. What is our simple scientific method?
9. Give an example of a positive and negative control
10. What is a synonym for a negative control
11. Why are negative controls important for most drug studies?
12. Provide a positive control for an experiment designed to
produce bubble gum that blows big bubbles
13. How many bonds to the atoms C, N , H, and O form?
14. What is a useful mnemonic device for the bonding pattern of
hydrogen, oxygen, nitrogen, and carbon?
15. Who wrote The Skeptical Chymist?
16. What constitutes a reliable reference when writing a scientific
paper, and why?
17. Why is chemistry awesome?
18. Compare and explain the flammability of liquids to gases.
19. True or false: most combustion reactions produce water
20. What is the difference between a physical and a chemical
change?
21. Provide an example of a physical and a chemical change.
22. How could you identify methanol?
23. Provide a balanced chemical equation for the combustion of
isopropanol, C3H8O.
24. Provide two isomers of C3H8O by drawing their structural and
skeletal formulas
25. Draw an ether with the formula C3H8O.
26. Draw an amine, an alcohol, a carboxylic acid, an ester, and an
amide.
27. Provide the molecular formula, skeletal formula, and functional
groups present in leucine shown at right.
28. What organic functional groups are present in sodium chloride,
NaCl?
29. Explain what is implied by the wedges and hatches used in the
drawing of leucine. Does contain straight chains, branched
chains, or rings?
30. What happens to molecular formulas when double bonds and
rings are used?
31. Describe what you know about aristolochic acid, palytoxin, and
the kahalalides.
32. In the rock candy lab, sugar crystallizes, meaning it change from
being dissolved in a liquid to becoming a solid. Is crystallization
a physical or a chemical process?
33. Define density, viscosity, and solubility. What role, if any, do
these play when solutions are mixed?
34. Draw a molecule that has an aldehyde, an ether, and a amide in
it. Provide the molecular formula as well.
35. Be prepared to answer the essential question for this unit: what
is chemistry all about?
I’m sure you would all like to ace your first chemistry test. Here’s how:
1. Test yourself on the topics below to see what you know and don’t know.
2. Review this packet in its entirety. Be familiar with each of the topics that were covered in the powerpoint presentation.
3. Write down what you don’t know yet. If you don’t know something, ask a friend or ask me.
4. If you are missing anything it may be available on the class website: http://www.chemistryadventure.com
data
table of contents unit 2 data
1
m
1
1
1
1
1
1
1
1
1
1
3. Complete the table Unit of measurement We usually use But SI units require
Length Mass
Temperature density
6. Complete the table. Prefix Symbol Factor Scientific
notation example
Giga mega 1,000 centi 10-3 micro microgram n
SI Units Unit Prefixes measurement unit symbol size Prefix Scientific
notation mass kilogram kg nano (n) billionth 10-9
volume liter L micro (m) millionth 10-6
distance meter m milli (m) thousandth 10-3
amount mole mol centi (c) hundredth 10-2
brightness candela cd kilo (k) thousand 103
current ampere A mega (M) million 106
time Second s giga (G) billion 109
•
•
•
•
•
•
•
•
•
•
•
•
•
sand
sand
sugar
salt
Method
pebbles
Iron filings
sugar
salt
pebbles
Iron filings Method
Methodsugar
salt
pebbles
Iron filings
sugar
salt
Iron filings
Iron filings salt
Method
1
2
3
4
5
6
7
8
9
10
The 1989 IBM Atomic Image By Your Name Here
Abstract: In 1989 Don Eigler from IBM ushered in the nanotechnology revolution
by moving individual Xenon atoms to create the image shown above.
Source: http://www-03.ibm.com/press/us/en/pressrelease/22260.wss
Source: http://www.flickr.com/photos/jurvetson/456735511/in/set-30000/
Source: http://www.tainano.com/chin/Eigler.htmSource: http://www.theregister.co.uk/2006/06/13/don_eigler_valley/
Eigler with his STM
Don Eigler (2006)
Eiglers Lab Notebook
35 Xenon Atoms
Don Eigler and the 1989 IBM Atomic Image
The question “What is everything made out of” is one of the most fundamental questions of mankind, right up there with “Why are we here?”,
and “Will that be on the test?”. Recorded ideas date back over 6000 years,1first popularized in the west by the work of Democritus.
Arguably the most compelling evidence for the atom being the fundamental particle of nature involves the human senses- smell, touch, sight,
etc. Because of the small size of the atom, none of these are directly possible, so perhaps the next best thing is to observe it with the help of
an instrument. This may have first occurred as early as 1981,2
but the image that popularized it was taken by Dr. Don Eigler in 1989.3
Don Eigler is a ponytailed, well educated physicist and surfer. In 1989, he designed his own scanning tunneling microscope. An image of him with
his instrument was taken during a 2006 interview.4
While studying the surfaces of solids, he came up with the idea of limiting the movement
of atoms by performing his experiments at a few degrees Kelvin- close to absolute zero. In his own words from the 2006 interview, he found
that
“Through a combination of hard work, some horse sense and good, old fashioned blind luck, I happened to be positioned to discover that I could
manipulate individual atoms with a scanning tunneling microscope.”
Having discovered the ability to move individual atoms, Eigler decided to create a work of art to document his discovery. What he created is an
image of the letters I B M using the noble gas Xenon, a dense and unreactive colorless gas. Was he forced at gunpoint to do the bidding of his
IBM bosses?? According to Eigler:
“I made that decision on my own. Management never said anything to me beforehand, and I did it with a very clear purpose in my mind. IBM
gave me a job, gave me the opportunity when I needed one, gave me the opportunity to excel at doing the things that I love in life, and it
was payback time. I pull no punches on that. It was my way of giving back to the corporation some of what the corporation gave to me.”
Does Eigler get bored recounting the discovery, now that two decades have passed?
“I don't mind talking to people when they're curious, for instance, about what I was thinking about or why did I do this or something like that.
The thing is that I always get introduced to people as the guy who wrote I-B-M in atoms. After you have heard that enough times, you don't really
need to hear it five more times.”
Eiglers current interests are in the field of Spintronics,5 a speculative field where future computers will be based not electricity (the translational
movement of electrons) but on their spin…a sort of electricity where the electrons stay where they are.
Sources:
1. Gangopadhyaya, Mrinalkanti (1981). Indian Atomism: History and Sources. Atlantic Highlands, NJ: Humanities Press. ISBN 0-391-02177.
2. G. Binnig, H. Rohrer “Scanning tunneling microscopy” IBM Journal of Research and Development 30,4 (1986) reprinted 44,½ Jan/Mar
(2000). Available on the web at http://researchweb.watson.ibm.com/journal/rd/441/binnig.pdf
3. Imaging Xe with a low-temperature scanning tunneling microscope. DM Eigler, PS Weiss, EK Schweizer, ND Lang - Physical Review
Letters, 1991 1189-1192.
4. A man and his microscope: IBM's quest to make atom-sized chips. The silver surfer speaks. Ashlee Vance, The Register, June 13, 2006.
Available on the web at http://www.theregister.co.uk/2006/06/13/don_eigler_valley/
5 Spintronics: A Spin-Based Electronics Vision for the Future. S. A. Wolf et al., Science 2001, Vol. 294. no. 5546, pp. 1488 - 1495
The 1989 IBM Atomic Image By Your Name Here
Abstract: In 1989 Don Eigler from IBM ushered in the nanotechnology revolution
by moving individual Xenon atoms to create the image shown above.
Source: http://www-03.ibm.com/press/us/en/pressrelease/22260.wss
Source: http://www.flickr.com/photos/jurvetson/456735511/in/set-30000/
Source: http://www.tainano.com/chin/Eigler.htmSource: http://www.theregister.co.uk/2006/06/13/don_eigler_valley/
Eigler with his STM
Don Eigler (2006)
Eiglers Lab Notebook
35 Xenon Atoms
Don Eigler and the 1989 IBM Atomic Image
The question “What is everything made out of” is one of the most fundamental questions of mankind, right up there with “Why are we here?”,
and “Will that be on the test?”. Recorded ideas date back over 6000 years,1first popularized in the west by the work of Democritus.
Arguably the most compelling evidence for the atom being the fundamental particle of nature involves the human senses- smell, touch, sight,
etc. Because of the small size of the atom, none of these are directly possible, so perhaps the next best thing is to observe it with the help of
an instrument. This may have first occurred as early as 1981,2
but the image that popularized it was taken by Dr. Don Eigler in 1989.3
Don Eigler is a ponytailed, well educated physicist and surfer. In 1989, he designed his own scanning tunneling microscope. An image of him with
his instrument was taken during a 2006 interview.4
While studying the surfaces of solids, he came up with the idea of limiting the movement
of atoms by performing his experiments at a few degrees Kelvin- close to absolute zero. In his own words from the 2006 interview, he found
that
“Through a combination of hard work, some horse sense and good, old fashioned blind luck, I happened to be positioned to discover that I could
manipulate individual atoms with a scanning tunneling microscope.”
Having discovered the ability to move individual atoms, Eigler decided to create a work of art to document his discovery. What he created is an
image of the letters I B M using the noble gas Xenon, a dense and unreactive colorless gas. Was he forced at gunpoint to do the bidding of his
IBM bosses?? According to Eigler:
“I made that decision on my own. Management never said anything to me beforehand, and I did it with a very clear purpose in my mind. IBM
gave me a job, gave me the opportunity when I needed one, gave me the opportunity to excel at doing the things that I love in life, and it
was payback time. I pull no punches on that. It was my way of giving back to the corporation some of what the corporation gave to me.”
Does Eigler get bored recounting the discovery, now that two decades have passed?
“I don't mind talking to people when they're curious, for instance, about what I was thinking about or why did I do this or something like that.
The thing is that I always get introduced to people as the guy who wrote I-B-M in atoms. After you have heard that enough times, you don't really
need to hear it five more times.”
Eiglers current interests are in the field of Spintronics,5 a speculative field where future computers will be based not electricity (the translational
movement of electrons) but on their spin…a sort of electricity where the electrons stay where they are.
Sources:
1. Gangopadhyaya, Mrinalkanti (1981). Indian Atomism: History and Sources. Atlantic Highlands, NJ: Humanities Press. ISBN 0-391-02177.
2. G. Binnig, H. Rohrer “Scanning tunneling microscopy” IBM Journal of Research and Development 30,4 (1986) reprinted 44,½ Jan/Mar
(2000). Available on the web at http://researchweb.watson.ibm.com/journal/rd/441/binnig.pdf
3. Imaging Xe with a low-temperature scanning tunneling microscope. DM Eigler, PS Weiss, EK Schweizer, ND Lang - Physical Review
Letters, 1991 1189-1192.
4. A man and his microscope: IBM's quest to make atom-sized chips. The silver surfer speaks. Ashlee Vance, The Register, June 13, 2006.
Available on the web at http://www.theregister.co.uk/2006/06/13/don_eigler_valley/
5 Spintronics: A Spin-Based Electronics Vision for the Future. S. A. Wolf et al., Science 2001, Vol. 294. no. 5546, pp. 1488 - 1495
F-9
19
Ca20
41 2+
U92
235
9 protons
10 neutrons
10 electrons
20 protons
21 neutrons
18 electrons
92 protons
143 neutrons
92 electrons
22 n
1
2
101097.0
1w
+1Alkalimetals
Alkalineearthmetals
+2
Transition metals: 2 valence electrons
+3+4, -4 -3 -2
-1
Noblegases
halogens
1 Hhydrogen
1.01
11Na
sodium
22.99
12 Mgmagnesium
24.31
3 Lilithium
6.94
4 Beberyllium
9.01
19
Kpotassium
39.10
20 Cacalcium
40.08
37 Rbrubidium
85.47
21 Scscandium44.96
22 Tititanium47.90
23 Vvanadium50.94
24 Crchromium52.00
25 Mnmanganese
54.94
26 Feiron
55.85
38 Srstrontium
87.62
39Y
yttrium
88.91
40 Zrzirconium
91.22
41
niobium
92.91
42 Momolybdenum
95.94
43 Tctechnetium
96.91
44 Ruruthenium
101.07
55 Cscesium
132.91
56Ba
barium137.33
71 LuLutetium
174.97
72 Hfhafnium
178.49
73 Tatantalum
180.95
74 Wtungsten
183.85
75 Rerhenium
186.21
76 Ososmium
190.20
87 Frfrancium
223.02
88 Raradium
226.02
103Lr
lawrencium
262.11
104 Rfrutherfordium
261.11
105 Dbdubnium
262.11
106Sg
seaborgium
263.12
107 Bhbohrium
264.12
108 Hshassium
265.13
27 Cocobalt
58.93
28 Ninickel
58.71
29 Cucopper
63.55
30 Znzinc
65.37
31 Gagallium
69.72
32 Gegermanium
72.59
13 Alaluminum
26.98
45 Rhrhodium
102.91
46 Pdpalladium
106.40
47 Agsilver
107.87
48 Cdcadmium
112.40
49 Inindium
114.82
50 Sntin
118.69
33 Asarsenic
74.92
14 Sisilicon
28.09
15 Pphosphorus
30.97
51 SbAntimony)
121.75
77 Iriridium
192.22
78 Ptplatinum
195.09
79 Augold196.97
80 Hgmercury
200.59
81 Tlthallium
204.37
82 Pblead
207.19
83 Bibismuth
208.98
109Mt
Meitnerium
(268)
110DsDarmstadtium
(281)
111 Rgroentgenium
(272)
112 UubUnunbium
(285)
113Uutununtrium
(284)
114Uuqununquadium
(289)
115Uupununpentium
(288)
5 Bboron10.81
6 Ccarbon
12.01
7 Nnitrogen
14.01
8O
oxygen
16.00
9F
fluorine
19.00
2He
helium4.00
10 Neneon
20.18
16 Ssulfur
32.07
17 Clchlorine
35.45
18 Arargon
39.95
34 Seselenium
78.96
35 Br79.91
36 Krkrypton
83.80
52 Tetellurium
127.60
53 Iiodine126.90
54 Xexenon
131.30
84 Popolonium
(210)
85 Atastatine
(210)
86 Rnradon
(220)
116Uuhununhexium
(289)
117Uusununseptium
(295)
118Uuoununoctium
(293)
57La
lanthanum
138.91
58 Cecerium
140.12
59Pr
praseodymium
140.91
60Nd
neodymium
144.24
61 Pmpromethium
144.91
62 Smsamarium
150.41
63Eu
europium
151.96
65Tb
terbium
158.92
89 Acactinium
227.03
90 Ththorium
232.04
91 Paprotactinium
231.04
92 Uuranium
238.03
93 Npneptunium
237.05
94Pu
plutonium
244.06
95 Amamericium
243.06
96 Cmcurium(247)
66
Dydysprosium
162.50
67 HoHolmium
164.93
68 Ererbium
167.26
69 Tm
thulium
168.93
70 Ybytterbium
173.04
97 Bkberkelium
(249)
98 Cfcalifornium
(251)
99 Eseinsteinium
(254)
100 Fmfermium
257.10
101 Mdmendelevium
(256)
102 No
(254)
Nb
common anions
Monovalentcations:
Group 1, Ag: +1Group 2, Zn: +2Group 3, Al: +3
Gdgadolinium
157.25
64
nobelium
0
1s
2s
3s
4s
5s
6s
7s
3d
4d
5d
6d
4p
5p
6p
7p
3p
2p
4f
5f
Symbol:SolidLiquidGasManmade
name
Atomic mass
Atomic number
Scscandium
44.96
21
(and NH4+)
metal nonmetalmetalloi
dm
eta
l
nonm
eta
l
1 valenceelectron
2 valenceelectrons
Valence electrons: 8
4 5 6 73
(H is a nonmetal)
bromine
Group 1
Group 2
Group 3 Group 4 Group 5 Group 6 Group 7 Group 8 Group 9 Group 10 Group 11 Group 12
Group 13 Group 14 Group 15 Group 16 Group 17
Group 18
to71
to103
:solution
1s2 2s2 2p2 3s2 3p4
16S:
Unit 5 electrons Dr. B.’s ChemAdventure
Principles and rules of electron configuration
Pauli
(opp. spins)
Hund’s Rule
(spread out)
1s22s11s22p1Aufbau
(build up)
Heisenberg(e-position uncertain)
GoodBadPrinciple or rule
1s22s22p2 1s22s22p2
1s2 1s2
1s1
our essential question:
OO
OOH
O OH
OO
O
O
O
O
OH
NHO H
1. taxol (paclitaxel)
I
I
W
W
investment x price original
price new estock valu
dollars 1150 dollars 1000 x dollars 485
dollars 560
O
investment x price original
price new estock valu
$525,000 $500,000 x $20
$21
I
OO
OOH
O OH
OO
O
O
O
O
OH
NHO H
1. taxol (paclitaxel)
O
OOH
H
OO
OH
H
H
O
O
OOO
O
O
O
O
OH
H
H
azadirachtin
Co3+
N
N
N
N
N
R
N
O
NO
NO
N
O
O
N O
N O
N
O
N O
O
O
PO
O
O
3. Vitamin B12
O
O
O
OH
OH
OH
OH
OH
OH
OH
H
H
O
OH
H
H
H
H
O
O
O
OHOH
OH
OH
OH
OH
O
4. ginsenoside rb2
OH
OOH
OH
OH
S
O
OO
O
O
O
O
O
O
OH
OHOH
OH
OHOH
OH
O
O
O
O
O
O S
O
OO
OH
OH
OH
OHO
O
O
O
OHOH
OH
OH
OH
O O
OO
O
O
O
OH
OH
O
O
O
OO
O
O
O
O
O
OH
OH
OH
OH
OH
OH
H
H
H
H
HH
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
H
HH
H
H
H
H
H
H
H
H
H
H H
H
H
H
H
Na
Na
I
F F FF
H
HH
H H
H
HH
CC
C
OH
HH
H
HH
CC H
HH
H H
OHC
C
OOH
OH
OH
OH
OH
H
H
H H
C
C C
Lithium Beryllium Boron fluoride permanganate oxide
Sodium MagnesiumAluminum bromide bicarbonate sulfide
Potassium Calcium Chloride hypochlorite chromate
Rubidium Strontium iodide chlorite dichromate
Cesium Barium chlorate
Francium Radium nitrite perchlorate carbonate
Ammonium Zinc nitrate bromate sulfite nitride
silver bisulfateiodate
sulfate phosphide
hydroxide acetate
cyanidephosphate
M
C
NSi
O
ONa
O
H
Br
F Li
W
N
+2 +3 -3 -2 -1
polyvalent
+1 0
F
O
G
NH
H H
H
H
H
H
N H
H
H
H H
H H
C C and CC
D
U
O OO+
-
I
W
C
r
r
r
r
Our Essential Question:
Our Essential Question:
W
S
→
C
Mix 24 g Mg with 32 g S. Makes 56 g MgS.
I
16 S
sulfur
32.07
12 Mg magnesium
24.31
I
1. Ice melts. What are the COOL signs of a chemical reaction you observed?
Is it a chemical reaction? _____
How could you prove it?
2. Wood burns. What are the COOL signs of a chemical reaction you observed?
3. Iron rusts. What are the COOL signs of a chemical reaction?
Is it a chemical reaction? _____
How could you prove it?
Is it a chemical reaction? _____
How could you prove it?
I
I
H
H
H
O H
O H
H
H
O
O
Na H OH
C C+ C C +
baking soda acetic acidethyl acetate water
_____ g _____ g _____ g _____ g
NaHCO3 + CO2
_____ mol _____ mol _____ mol _____ mol
carbondioxide
_____ g
_____ mol
E
C
NO2
NO2
O2N
H H
HH
H
N
T
A
OH moles 5 H moles 2
OH moles 2 x
H grams 2
H mole x H grams 10 2
2
2
2
22
E
I
A
I
’
º
1
2
M
M
2
Gas Formulas and
conversions
1
2
M
M
3
;2211 VPVP
’
2
2
1
1
V
T
V
T
’
mL 50 140
K 340 ; 2
2
2
1
1 T
mLV
T
V
T
2
2
1
1
P
T
P
T
’
;;x
’
200
’
’
(
’
NaOH g 4 solution liter 0.1 x NaOH mole
NaOH g 40 x
solutionliter
NaOH mole 1
D
D
Greasy: will dissolve in
greasy solvents
watery region
OH
watery: will dissolve in
watery solvents (like
water)
A “brick”: hard to
dissolve in anything.
1 2
1 2
S S
P P
1 2
1 2
S S 3.3 g /L 9.9 g/L (1 atm)(9.9 g/L); ; x = 3 atm
P P 1 atm x (3.3 g/L)
mass solutePercent solution by mass x 100
mass solution
volume solutePercent solution by volume x 100
volume solution
moles of solute
Liters of solution
40 g NaCl0.5 moles NaCl x x 0.08 Liters solution = 1.6 grams NaCl
Liter of solution mole NaCl
mass solute
Percent solution by mass x 100mass solution
volume solutePercent solution by volume x 100
volume solution
moles of solute
Liters of solution
°
°
Chemistry
1. Intro
2. data
3. matter
4. the atom
5. electrons
6. periodic table
7. bonding
8. reactions
9. the mole
10. gases
11. solutions
12. Energy
13. Reaction rates
14. equilibrium
15. Acids and bases
D
D
D
D
D
D
D
D
D
Percent error = measured chip calories/actual chip calories x 100
Title
Name, Date
(For example:
Potato Chip Calorimetry
Or Energy Analysis of a common Snack Food)
Schematic drawing
With labels
Of your
calorimeter
caption
Conclusions
Include the Nutritional
Calories calculated for
your chip, the estimated
real nutritional calories for
your chip, and an
explanation for the
difference.
Data
Q = mcDT
Q=
M=
C=
DT =
= ( ) ( ) ( )
= ___ J
= ___Nutritional
Calories
Pick a topic:
1. What is calorimetry?
2. Sources of Error
in our calorimeter design
3. A better design for
the next experiment
10 points:
1. Effort: 5 points
-does this represent
45 minutes of effort?
2. Calculations: 3 Points
-are they accurate?
3. Analysis: 2 points:
Why are the results so
bad (or so good).
D
D
D
D D
D
D
D D
D
D
D
D
D
D
D
D
D
D
D D D
D
D
D
D
D D D
D D D
DD
D
D
D
° °
° °
°
° °
D
° ° °
° °
° °
D
D
D
D
D
D
D
D
° ° ° °
°
D
DG = DH –TDS
Where
DG = Gibbs Free Energy
DH = Enthalpy in Joules
T = Temperature (K)
And DS = Entropy in Joules/K
D D D
D D D
D
D
D D
D
D . D
D
D D
D D
D D D
D
D
D
D
D D D
D D D
D
D
D
D
D
D
Chemistry
1. Intro
2. data
3. matter
4. the atom
5. electrons
6. periodic table
7. bonding
8. reactions
9. the mole
10. gases
11. solutions
12. Energy
13. Reaction rates
14. equilibrium
15. Acids and bases
Δtime
tionΔconcentrarate reaction
Δtime
tionΔconcentraratereaction
ss
LmolLmol
04
/22.0/100.0
sec03.0
liter
mol
collision theory
•
•
•
•
•
Unit 14
The problem with chemical reactions is that the reverse reaction can, and usually does occur. To put
it another way, for the reaction AB, while A ⇌ is being converted to B, B is often being converted
back to A. And what good is that?! This is equilibrium, a balance between forward and reverse
reactions. In a sense, this means that a chemical reaction is never “done”; it never stops; it simply
gets to a point where the rate of the forward reaction is equal to the rate of the reverse
reaction. Fortunately it is usually an easy matter to destroy this reversibility, this equilibrium. For
example a reaction can be irreversibly driven to completion by removing the products as they are
formed.
Note that this doesn’t necessarily mean the reaction will now happen quickly: equilibrium and rate are
two separate aspects of a chemical reaction…and just what is the relationship between equilibrium
and rate? What does it mean to have something that can go forwards and backwards at the same
time, at different speeds? Will the product ever form? Will the product ever stay formed?
In practice, reversible reactions can give lousy yields of product, and chemists are always trying to
come up with a way to drive the reaction to completion.
The graph below shows the typical result of a reversible chemical reaction. Dinitrogen tetroxide is
decomposing into nitrogen dioxide, but since the reaction is reversible, the reaction never goes to
completion.
In this unit we will learn how to
calculate the concentrations of
reactants and products at equilibrium,
and we will use several methods to
adjust the equilibrium in the direction
we prefer. ∏
How do I recognize and deal with a reversible chemical reaction?
Name: __________________________ Period: _____ equilibrium lab 1
Paper Clip Equilibrium Activity
To demonstrate the characteristics of a reversible chemical reaction, imagine the reaction
A + B C below:
This is an example of a _______________ reaction. The reverse reaction is an example of a
_________ reaction. At your instructors prompts, make as many C molecules as you can in 15
seconds. Then see how many you can take apart in 15 seconds. Record your answers in the box.
6. Before returning the materials to the front of the classroom, be certain the composition of the
paper clips in the pile are the same as when your received them.
Summary Question:
You have just simulated a reversible chemical reaction. In actual practice, the rate of a chemical
reaction at constant temperature and pressure slows down over time until there is no change in the
ratio of product to reactants. Explain this using collision theory.
A B C
Summary:
C molecules made in 15 seconds (forward reaction): __________
C molecules decomposed in 15 seconds (reverse reaction): ________
At this rate, it would take ____ minutes for this reversible reaction to go to completion.
↔
D
D
↔ D
Name: _______________________ Period: _____ equilibrium lab 2
Perfume Lab
Introduction:
Esters may be prepared through the reaction of a carboxylic acid RCO2H with an Alcohol (R’OH),
using a small amount of sulfuric acid as a catalyst.
RCO2H + R’OH + H2SO4 RCO2R’ + H2O + H2SO4
carboxylic acid alcohol sulfuric acid ester water sulfuric acid
Esters often have strong pleasant aromas. Carefully guarded mixtures of esters create expensive
perfumes including Chanel #5, Aramis (for men) and others, some of which sell for hundreds of
dollars per bottle. In this lab each student will create his own ester, and we will then share them to
make perfumes.
For this chemical reaction, all of these reactants and products remain in solution. Therefore this
reaction is reversible, and yields for this reaction can be low. In this experiment we will investigate
the equilibrium mixture for this mixture after 24 hours.
Materials:
Carboxylic acids listed on board
Alcohols listed on board
Sulfuric Acid (to be distributed by instructor) as a catalyst
.
Chemical Reaction Procedure:
Mix 0.1 moles of your carboxylic acid, 0.1 moles of ethanol, and 5 drops of sulfuric acid. The
calculations below will help make sure you are using the right amounts. Heat but do not boil on
a hot plate for 20 minutes then store covered overnight.
Calculations:
My carboxylic acid has a formula of _____, therefore one mole has a mass of ______g, and
0.1 mole has a mass of ______g.
My alcohol has a formula of ______, therefore one mole has a mass of ______g, and 0.1 mole
has a mass of ______g.
Workup
The following day, carefully neutralize the mixture with a measured amount of baking soda (NaHCO3).
This reaction required ____g of baking soda for neutralization.
Calculation: Sodium bicarbonate has a molecular formula of NaHCO3. Therefore one mole of NaHCO3
has a mass of ____g and 0.1 mole has a mass of ____g. Since ____ g of sodium bicarbonate reacted,
this is ____moles of sodium bicarbonate. Therefore it reacted with ____moles of my carboxylic
acid. Based on this we estimate that the reaction is ____% complete.
All of the substances in the mixture are water soluble, except the fragrant ester you have produced.
Bottle and artistically label the ester you have created.
If time permits, combine small amounts of your perfume with those made by others to create your
own perfume.
Results:
1. Based on our workup, our reaction created ___ g of ester after ____ hours for a ____ %
yield.
I would describe the odor of our ester produced as __________
I would describe the odor of our perfume as _______..
Questions
1. Show a balanced chemical equation for the reaction of acetic acid with baking soda.
3. Based on chemical equilibrium, indicate three ways the yield of this reaction could be improved.
1
Name: _____________________________________ Date: ______ Period: _____
Science and Technology Posters
100 Points
Introduction:
Choose a poster on a topic of your choice.
Topic:
Each group of two will present a poster on any approved topic that is titled:
The Chemistry of ____________________
Choose something that you are personally interested in. Possible topics include
The Chemistry of :
1. A rose
2. Explosives
3. DNA
4. skin cream
5. chocolate
6. dirt
7. car tires
8. the space shuttle
rocket engine
9. A battery
10. Hybrid vehicles
11. nuclear power
12. Nuclear warheads
13. The Connecticut
river
14. The ozone layer
15. Liquid crystals
16. A baseball
17. carbon
18. Coca-cola
19. Scopolamine
20. Mouthwash
21. flavonoids
22. Cellular phones
23. Reverse osmosis
24. artificial blood
25. hydrofluoric acid
26. chemical warfare
agents
27. organ transplants
28. the bliss molecule
29. pain
30. anabolic steroids
31. mucous
32. energy drinks
33. really smelly gases
34. combinatorial
chemistry
35. dynamite
Scoring Rubric
1. These posters are purely informational, not research-based. The goal is to instruct the
reader in a logical, succinct, and interesting way. No experiments are necessary.
2. These posters should reflect the fact that we are near to completion of a full year high
school level chemistry course. Try to get as deep as you can into your subject.
3. There should be several chemical structures included in your poster (2 minimum).
4. There should be a properly cited reference section for your poster. Include trusted
scientific sources wherever possible. Include enough details in your citation that anyone could
easily retrieve that source.
5. Include numerous images in your poster (2 minimum). Cite the source below the image if it is
not original.
All posters must be typed. Your instructor will provide details.
Name: ____________________________________ Period: _____ equilibrium worksheet 1
Writing Equilibrium Concentration Expressions
Directions: Write the equilibrium constant expression for each of the equations illustrated below.
1. At 1405 K, hydrogen sulfide, also called rotten egg gas because of its bad odor, decomposes to
form hydrogen and a diatomic sulfur molecule, S2.
2H2S(g) ↔ 2H2(g) + S2(g)
Write the equilibrium constant expression for this reversible reaction.
2. Methanol, a formula-1 race car fuel, can be made from carbon monoxide and hydrogen gas:
CO(g) + 2H2 (g) ↔ CH3OH(g)
Write the equilibrium constant for this reversible reaction.
3. Write the balanced reaction for the combustion of hydrogen at 200 OC, and show that this is a
reversible reaction.
These all follow the format:
for aA + bB cC +dD
c d
eq a b
[C] [D]K
[A] [B]
Example: write the equilibrium constant expression for the gas-phase synthesis of ethane (C2H6)
from the elements.
Solution: First, we write the balanced chemical equation:
2C(g) + 3H2 ↔ C2H6 (g)
Then we use the format above to write the equilibrium constant expression:
2 6eq 2 3
2
[C H ]K
[C] [H ]
Write the equilibrium constant for this reversible reaction.
4. Write a balanced reaction for the combustion of methane at room temperature. Be sure to include
the physical states of the reactants and products.
Write the equilibrium constant for this reversible reaction.
Name: _______________________ Date: ______Period: _____ eauilibrium worksheet 2
Calculating Equilibrium Concentrations
Directions: Write the equilibrium constant expression for each of the equations illustrated below
and solve for the missing value.
1. Lead sulfide may be prepared under high pressure by the reaction of lead with elemental sulfur:
Pb(g) +S(g) ↔ (PbS(g)
What is the value of the equilibrium constant (Keq) if [Pb] = 0.30 mol/L and [S] = 0.184 mol/L,
and [PbS] is 2.00 mol/L?
How far has this reaction progressed?
A. Unfortunately, it is still mostly reactants
B. This reaction is mostly products
These all may be solved using the equilibrium constant expression:
for aA + bB ↔ cC +dD c d
eq a b
[C] [D]K
[A] [B]
And then plugging in the given data and solving for the unknown.
Example: For the reaction of carbon monoxide with oxygen to form carbon dioxide, determine the
equilibrium concentration of carbon dioxide when the concentration of carbon monoxide is 0.8
moles/liter, the concentration of oxygen is 2.1 moles/liter, and the equilibrium constant is 225.
Solution: We begin by writing a balanced chemical, equation for the reaction:
2CO + O2 ↔ 2CO2
We then write the equilibrium constant expression and plug in the numbers given: 2 2
2 2eq 2 2
2
[CO ] [CO ]K ; 225
[CO] [O ] [0.8] [2.1]
Finally, we solve for the concentration of carbon dioxide: 2
2[CO ] 225(0.8) (2.1) 17.4
The concentration of carbon dioxide is 17.4 moles/liter
2. Methanol can be prepared from carbon monoxide and hydrogen:
CO(g) + 2H2 (g) ↔ CH3OH(g)
Calculate these equilibrium constants:
a. Keq when all substances have a concentration of 1 mol/L
b. Keq when all substances have a concentration of 2 mol/L
C. Keq when all substances have a concentration of 3 mol/L
d. For each reaction indicate if the reaction is mostly products, or mostly starting
material.
3. For the combustion of methanol, determine the concentration of methanol given the following
data:
Keq = 0.32
[O2] = 2 mol/liter
[CO2] = 4 mol/liter
[H2O] = 5 mol/liter
Name: ____________________________ Period: _____ equilibrium worksheet 3
Le Chatelier’s Principle
Henri Le Chatelier came up with a cryptic quote for explaining what causes chemical equilibrium, and
what to do about it:
"Placing a stress on an equilibrium causes the equilibrium to shift so as to relieve the stress"
What he was referring to were some common things one can do to modify a chemical reaction and the
net result:
Add reactant: reaction moves forward ()
Add product: Reaction moves backward (reverse;
Add temperature: Moves forward if endothermic (positive DH)
Add pressure: moves toward the fewer number of moles.
Remember, liquids and solids are considered to be outside of the reaction mixture – don’t
count them when adding up moles.
1. For the following reaction
5 CO(g) + I2O5(s) I2(g) + 5 CO2(g) DHo = -1175 kJ/mol
for each change listed, predict the equilibrium shift and the effect on the indicated quantity.
Example: For the aqueous reaction of table salt with magnesium sulfide, the standard enthalpy of
formation is +22.6 kJ/mol. Predict the equilibrium shift if the temperature is increased, if the
pressure is increased, or if sodium sulfide is added to the reaction mixture.
Solution: We begin by writing a balanced chemical equation:
2NaCl (aq) + MgS (aq) ↔ Na2S (aq) + MgCl2 (aq) DHo = +22.6 kJ/mol
Note that in this case 3 moles of reactants form 2 moles of products, and that the standard
enthalpy of formation indicates this reaction is endothermic. Using this information and the tips
at the top of this worksheet, we can conclude
Increasing temperature will shift the equilibrium forward () since this reaction needs
heat
Increasing pressure will shift the equilibrium forward ( ) since the product has fewer
moles
Adding sodium sulfide is like adding water to a fire, and shift the equilibrium backwards
()
Change
Direction
of Shift ( ; ; or no change)
Effect on
Quantity
Effect (increase, decrease,
or no change)
(a) decrease in volume amount of CO (g)
(b) raise temperature amount of CO(g)
(c) addition of I2O5(s) amount of CO(g)
(d) addition of CO2(g) amount of I2O5(s)
(e) removal of I2(g) amount of CO2(g)
2. Consider the following equilibrium system in a closed container:
Ni(s) + 4 CO(g) Ni(CO)4(g) DHo = - 161 kJ
In which direction will the equilibrium shift in response to each change, and what will be the effect on the
indicated quantity?
Change
Direction
of Shift ( ; ; or no change)
Effect on
Quantity
Effect (increase, decrease,
or no change)
(a) add Ni(s) Ni(CO)4(g)
(b) raise temperature Keq
(c) add CO(g) amount of Ni(s)
(d) remove Ni(CO)4(g) CO(g)
(e) decrease in volume Ni(CO)4(g)
(f) lower temperature CO(g)
(g) remove CO(g) Keq
3. For the conversion of oxygen (O2) to ozone (O3), predict the equilibrium shifts from the following
changes:
Change
Direction
of Shift ( ; ; or no change)
(a) add Ni(s)
(b) raise temperature
(c) add CO(g)
(d) remove Ni(CO)4(g)
(e) Apply a vacuum
(f) lower temperature
(g) remove CO(g)
Name__________________________ Period________ equilibrium worksheet 4
Equilibrium Review Worksheet
1. What is the best way to drive a reversible reaction to completion?
If you were watching a chemical reaction, list three observations that would indicate that the
reaction is not subject to equilibrium and can only move forward.
2.
3.
4.
Write the gas equilibrium constant (Kc) for each of the following chemical reactions.
5) CS2(g) + H2 (g) CH4 (g) + H2 (g)
6) Ni (s) + CO(g) Ni(CO)4 (g)
7) HgO(s) Hg (l) + O2(g)
8) In your own words, paraphrase Le Chatelier's Principle.
9) Balance the following reaction:
___N2 (g) + ___H2 (g) ___NH3 (g) DH= -386 KJ/mole
10. Known as the Born-Haber Process, this is an example of a __________ reaction.
Predict the direction the equilibrium will shift if:
11) N2 is added?
12) H2 is removed?
13) NH3 is added?
14) NH3 is removed?
15) the volume of the container is increased?
16) the pressure is increased by adding Argon gas?
17) the reaction is cooled?
18) equal number of moles of H2 and NH3 are added?
The equilibrium constant for the following reaction is 5.0 at 400 C.
CO (g) + H2O(g) CO2 (g) + H2 (g)
Determine the direction of the reaction if the following amount (in moles) of each compound is placed
in a 1.0 L flask.
CO (g) H2O (g) CO2 (g) H2 (g)
19. 0.50 0.40 0.80 0.90
20. 0.01 0.02 0.03 0.04
21. 1.22 1.22 2.78 2.78
22. At a particular temperature a 2.0 L flask contains 2.0 mol H2S, 0.40 mol H2, and 0.80 mol S2.
Calculate Keq at this temperature for the reaction:
H2 (g) + S2 (g) H2S (g)
23) Balance the following conversion of methane into the monomer ethylene, used to make the
polymer polyethylene:
___CH4 (g) ___H2C2 (g) + ___H2(g)
The initial concentration of CH4 is 0.0300 M and the equilibrium concentration of H2C2 is 0.01375 M:
24) calculate the equilibrium concentrations of CH4 and H2;
25) Determine the numerical value of Keq.
26) At a particular temperature, 8.0 mol NO2 is placed into a 1.0 L container and the NO2 dissociates
by the reaction (which needs balancing):
___NO2(g) ____NO (g) + ___O2(g)
27. At equilibrium, the concentration of NO is 2.0 M. Calculate Keq for this reaction.
28. At a certain temperature, 4.0 mol NH3 is introduced into a 2.0 L container, and the NH3 partially
dissociates by the reaction (please balance it):
___NH3 (g) ___N2 (g) + ___H2(g)
At equilibrium, 2.0 mol NH3 remains. What is the value of Keq for this reaction?
Howtoaceitunit18
How to Ace the Equilibrium Exam
In our previous unit we investigated the rate of chemical reactions- how fast do they go? In this
equilibrium unit we point out that even if a reaction is going fast, it might not be going very far
overall if the reverse reaction is also occurring. This is the big idea behind chemical equilibrium, the
condition where the rate of a forward reaction is equal to the rate of the reverse reaction.
We can write the equilibrium constant expression and from this we can determine if we are getting
anywhere or whether the reaction is standing still. Generally speaking, if we mix chemicals together
we would like them to go forward, and this will happen if the value of the equilibrium constant (Keq) is
greater than one. Note that Keq is only true at a specific temperature, and it says nothing about the
rate of a reaction- only the direction.
A nice benefit of the equilibrium constant expression is that it can also tell you what the
concentration of a reactant is, given enough information.
Since chemical equilibrium can prevent a reaction from going to completion, it would be nice to know
how we can destroy it, or at least get things moving forward. Simple. To destroy chemical equilibrium,
one must remove the product as it is formed- this makes the reverse reaction impossible. This is
accomplished by having the product precipitate, for example by precipitating as a solid. As a general
rule, this is why we omit liquids and solids from our equilibrium constant expression. In practice, it is
easy to observe a precipitate. Examples include the gaseous precipitate we observe when we mix
baking soda and vinegar, or the solids that crash out of solution during many double replacement
reactions. These reactions can only move forward, since collisions between products to form
reactants are no longer possible.
There are several other ways one can adjust chemical equilibrium. Known as Le Chatelier’s Principle,
the direction of a reaction after a stress is applied may be summarized:
Le Chatelier’s Principle
Adding reactant:
Adding product:
Heating: if endothermic
Pressurizing: if there are fewer moles of product
Each of these may be reversed; for example cooling an endothermic reaction will favor the reverse
reaction.
Imagine going on a trip. It’s nice to know in what direction you are going, and how long it will take.
These last two units have shown us just that for a chemical reaction. In the next unit we can apply
these navigational skills to the study of acids and bases.
To ace this exam you should know:
1. What is chemical equilibrium?
2. What is a synonym for equilibrium?
3. What is the best way to destroy chemical equilibrium?
4. What does it mean if the rate of a forward chemical reaction
a. Is faster than the reverse reaction
b. Is the same as the reverse reaction?
c. Is slower than the reverse reaction?
5. Please balance the reaction below and write the chemical equilibrium expression:
___Fe3O4(s) + ___H2(g) ___Fe(s) + ___H2O (g)
Keq =
6. Please determine the direction of the reaction given the following data:
C2H4(g) + H2 (g) C2H6(g) DH = +32kJ/mol
a. 1M 2M 3M Direction of reaction:______
b. 1.0520M 3.0400M 3.1909M Direction of reaction:______
7. For the reaction below the rate of the forward reaction is equal to the rate of the reverse
reaction. Therefore, Keq = ____. Determine the concentration of ethane (C2H6) in the mixture:
C2H4(g) + H2 (g) C2H6(g) DH = +32kJ/mol
2M 4M ?
8. Please determine the direction of the following hypothetical reversible reaction:
4A(g) + 7B(g) + 13C +D (l) 9E (g) + 3F (g)+ 2G (g)
Concentrations (M): 1.06 2.12 1.42 3 2.10 1.44 3.26
9 (L1 only). Please determine the concentration of G in the following reaction if it is at equilibrium.
4A(g) + 7B(g) + 13C +D (l) 9E (g) + 3F (g)+ 2G (g)
Concentrations (M): 1.06 2.12 1.42 3 2.10 1.44 ?
9. List five ways to help the following reaction move forward:
C2H4(g) + H2 (g) C2H6(g) DH = +32kJ/mol
1.
2.
3.
4.
5.
10. In our next unit we will be studying acids and bases. Write a balanced chemical equation for the
reaction of hydrochloric acid with sodium hydroxide to form table salt and water:
a. Can you move this reaction forward by pressurizing it?
b. If the standard enthalpy of formation for this reaction is 0.004KJ/Mol, can you move it
forward by heating it?
c. What is the only product that might precipitate from this reaction at room temperature?
d. Why would it be a big deal if that product did precipitate?
e. Would it be a good idea to add water to this reaction?
f. This is a segue into the next unit: If this reaction used 10 grams of sodium hydroxide and
ten grams hydrochloric acid, would it result in a neutral, acidic, or basic solution (assuming a
complete reaction)?
M
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
3
5
10
10
molarity of known x liters of knownMolarity of unknown =
liters of unknown
(NaOH Molarity)(NaOH volume) vinegar Molarity =
vinegar volume
60 grams acetic acid 180 g acetic acid3 moles acetic acid 1 liter solution x x = = 18%
Liter solution 1 mole acetic acid 1000 grams solution 1000 g solution
common name name formula
stomach acid hydrochloric acid HCl
hydrofluoric acid HF
hydrobromic acid HBr
hydrioidic acid HI
nitric acid HNO3
sulfuric acid H2SO4
phosphoric acid H3PO4
vinegar acetic acid CH3CO2H
lye sodium hydroxide NaOH
milk of magnesia magnesium hydroxide Mg(OH)2
calcium hydroxide Ca(OH)2
ammonia NH3
triethylamine (CH3CH2)3N
6.0 x 10-11
[OH-]Acid
Orange juice10.221.66 x 10-43.78
Acid or base?
ExamplepOH[H+]pH
pH + pOH = 14[H+] = 10-pH
pH>7 = basepH<7 = acid
[H+][OH-] = 10-14
Use the change sign (-) button, not the subtract button
Enter 10^-14/1.66E-4
Enter 10^-3.78Enter 14-3.78