CH117
Consumer Chemistry:
Chemistry of Food and Cooking
Unit 2
Chemistry Basics
Periodic Table
Ionic and Covalent Compounds
Utensils in Cooking
Functional Groups in Flavor Molecules
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1-1
What is Chemistry?
“The study of Matter and its Changes.”
Matter
The stuff things are made of.
Has Mass and Volume (takes up space).
(Air, water, rocks, etc..)
Mass = The amount of stuff (in g’s)
(Bowling Ball > Balloon)
Weight = Pull of Gravity on matter.
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1-2
A model of matter
Pure Substance - something of uniform composition that
can’t be sorted further by differences.
• Element - Pure substance composed of only one kind
of atom.
•
ie. Table of known elements
Chemical Compound - A pure substance that is a
combination of different elements.
ie. Water (H2O)
ie. Carbon Dioxide (CO2)
ie. Salt (NaCl)
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1-3
A model of matter
Mixture-
NOT of uniform composition and CAN be
sorted further by differences.
• Homogeneous – Looks pure but is not.
ie. Salt or Sugar Water (H2O + NaCl)
ie. Homogenized Milk
•Heterogeneous - Visibly
a combination of
different substances.
ie. Pizza
ie. Chocolate Chip Cookies
ie. Granite
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1-4
A model of matter
Atom - The smallest unit of an element that is
still that element.
ie. Aluminum (Al)
Molecule -The smallest unit of bonded atoms
that is still that substance.
Contains > 1 atom or element.
ie. Water (H2O)
ie. Carbon Dioxide (CO2)
ie. Oxygen (O2)
ie. Not Salt (NaCl)
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1-5
Classification of matter
Matter
Pure Substance
Element
Fe
Mg
Compound
FeS
MgO
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Mixture
Heterogeneous
Homogeneous
Fe + S
Mg + O2
1-6
Mixtures
Mixture
Homogeneous
(Solution)
Uniform composition
Heterogeneous
Non-uniform composition
Air
Pizza
Tea w/ice
Gasoline
Urine
Milk
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Sand
1-7
Hydrogen
Elements & Symbols
Sodium (Natrium)
Potassium (Kalium)
Carbon
Aluminum
Calcium
Nitrogen
Iron
Chlorine
Copper
(Cu)
(Ferrum) Gold (Aurum)
Each element is assigned a unique symbol
1-2 letters; 1st is capitalized
The original name is often of Latin or Greek origin
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1-8
Modern periodic table
IA
1
2
Mendeleev, 1871
III A IV A V A VI A VIIA VIIIA
“Properties of the elements
He
vary in a periodic manner.”
II A
H
Li Be
Na Mg III B IVB V B VIB VIIB
3
4
5
6
7
K
Ca Sc Ti
Rb Sr
Y
V
IB
IIB
C
N
O
F
Al
Si
P
S
Cl Ar
Ne
CrThe
Mn periodic
Fe Co Nitable
Cu Zn Ga Ge As Se Br Kr
helps us understand
•behavior,
W Re •reactions
Os Ir Pt Au Hg Tl Pb
•properties
CeofPrthe
Nd elements.
Pm Sm Eu Gd Tb Dy Ho
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba Ls Hf Ta
Fr Ra Ac
VIII B
B
I
Xe
Bi Po At Rn
Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
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1-9
A row or period
Periods are
assigned numbers
1
H
2
Li Be
B
C
N
O
F
3
Na Mg
Al
Si
P
S
Cl Ar
4
K
5
Rb Sr
6
Cs Ba Ls Hf Ta W Re Os Ir
7
Fr Ra Ac
Ca Sc Ti
Y
V
He
Ne
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
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1 - 10
Common group names
Alkali Metals
Alkaline Earth Metals
IA
H
Noble gases
II A
Li Be
Ca Sc Ti
VIIIA
III A IV A V A VI A VIIA
Transition Metals
Na Mg III B IVB V B VIB VIIB
K
Halogens
V
VIII B
IB
IIB
He
B
C
N
O
F
Ne
Al
Si
P
S
Cl Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Lanthanides
Rb
Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir
I
Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Actinides
Th Pa U Np Pu AmCm Bk Cf Es Fm Md No Lr
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Xe
1 - 11
Why do we have those
rows on the bottom?
H
He
This arrangement takes too B C
Na Mg much space and is hard to read.Al Si
Li Be
N O F Ne
P S Cl Ar
K Ca Sc
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
Cs Ba Ls Ce Pr NdPmSmEu Gd Tb Dy Ho Er TmYb Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac Th Pa U Np PuAmCmBk Cf Es FmMdNo Lr
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Names & Symbols
Know the
names & symbols
1
H
2
Li Be
B
C
N
O
F
3
Na Mg
Al
Si
P
S
Cl Ar
4
K
5
Rb Sr
6
Cs Ba Ls Hf Ta W Re Os Ir
7
Fr Ra Ac
He
Ca Sc Ti
Y
V
Ne
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
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Lustrous, malleable and ductile.
Metals
Solids at room temp (except Hg)
H
Conductors (heat & electricity); electrons loose
so can move freely (flow) and spread energy so
He
make good cooking pans (ie. Al, Fe, Cu)
Li Be
Give electrons to nonmetalsB (Form
(+) ions
C N
O F). Ne
Na Mg
K
Al
Ca Sc Ti
Rb Sr
Y
V
P
S
Cl Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba Ls Hf Ta W Re Os Ir
Fr Ra Ac
Si
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
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Remember Specific Heat
30o
20o
Low SpHt; Heats quickly
Stainless steel (Fe/Cr/Ni all ~0.1) heats fast.
Cu on bottom heats faster.
10o
1o
Al
0.22
H2O
1.00
Sand
0.19
Fe
0.11
Cu
0.093
Au
0.031
Ag
0.057
High SpHt; Resists change
Cast Iron skillets (Fe/C) have more mass compared to normal Al
or Stainless steel pans which is why they heat & cool slowly and
hold heat longer than an Al or Fe pan of lower mass.
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Non-metals
H
Li Be
He
B
C
N
O
F
Na Mg
Al Si
Gas,
liquid, solid (dull, brittle); Many are diatomic
P
S
Cl Ar
K Ca
Sc Ti V Cr
Mn Fe Co Ni
Cu Zn Ga
Poor
conductors
(Insulators);
electrons
held rigid in covalent bonds so can’t flow.
Rb Sr SiO
Y Zr
Nb Mo Tc Ru Rh Pd Ag Cd In
Glass,
2, heats slower than metal;
Baking (hot air) is slower than Frying or
Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl
boiling.
Convection ovens make faster.
Ge As Se Br Kr
Sn Sb Te
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I
Xe
Pb Bi Po At Rn
Fr Ra
Ac
Take
electrons
from
(Form
ions);
Ce metals
Pr Nd Pm
Sm Eu(-)Gd
Tb Dy Ho
Th Pa Uwith
Np Pu
Am Cm
Bk Cf
Share electrons (covalent)
other
nonmetals
Ne
Er Tm Yb Lu
Es Fm Md No Lr
1 - 16
Metaloids
H
He
Li Be
B
C
N
O
F
Na Mg
Al
Si
P
S
Cl Ar
K
Ca Sc Ti
Rb Sr
Y
V
Ne
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Intermediate
properties
Cs Ba Ls Hf Ta W Re Os
Ir
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
Semi
conductors
Fr Ra Ac
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
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1 - 17
3 - 11
Metals
Non-metals
Metaloids
H
He
Li Be
B
C
N
O
F
Na Mg
Al
Si
P
S
Cl Ar
K
Ca Sc Ti
Rb Sr
Y
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba Ls Hf Ta W Re Os Ir
Fr Ra Ac
Ne
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
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1 - 18
A model of matter
Atom - The smallest unit of an element
that is still that element.
ie. Aluminum (Al)
Molecule -The smallest unit of a pure
substance that is still that substance.
May contain > 1 atom or element.
ie. Water (H2O)
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Structure of the atom
Nucleus
Small, dense, + charge in the center of
an atom.
contains
protons
&
+
+
+
+
+ +
neutrons
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1 - 20
Structure of the atom
Nucleus (+)
Electrons
- charged particles
that surround the
nucleus.
Electrons move around
nucleus in orbitals.
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Structure of the atom
The nucleus is a small part of an atom.
If the nucleus was the size
of a marble, the atom would
fill a football stadium.
The nucleus would weigh
over 10,000 tons.
Atoms are mostly empty space.
Atoms have a small, dense nucleus with + charge.
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1 - 22
The atomic symbol
C = Charge
A = Atomic mass
= + or - values
A
Z
X
Z = Atomic number
= # protons = # electrons
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C
#
# = Number of
atoms in a formula.
1 - 23
The atomic symbol
C = Charge
A = Atomic mass
= + or - values
16
8
O
Z = Atomic number
= # protons = # electrons
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2-
# = Number of
atoms in a formula.
1 - 24
Electron arrangement
24
Mg
12
32
18
2
Electrons
fill layers around
nucleus
Low  High
8
A new layer is
added for each
row or period in
the table.
Shells = Energy levels
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1
H
1
IA
7
Li
3
II
A
4
He
2
9
Be
4
2, 1
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2, 2
1 - 26
1
H
1
IA
7
Li
3
II
A
9
Be
4
2, 1
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2, 2
IIIA
11
B
5
2, 3
1 - 27
IIIA
11
B
5
IVA
13
N
7
12
C
6
2, 3
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VA
2, 4
2, 5
1 - 28
IA
IIA
1
1H
7
Li
3
4
He
2
9
4Be
2, 2
2, 1
23
Na
11
VIIIA
24
12Mg
2, 8, 1
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2, 8, 2
20
Ne
10
2, 8
40
18Ar
2, 8, 8
1 - 29
1
1
1
Octet Rule
H
2
9
4 Be
7
3 Li
2, 1
23
Na
11
8
4
2 He
20
Ne
10
2, 2
24
12
2, 8, 1
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Mg
2, 8, 2
2, 8
40
18 Ar
2, 8, 8
1 - 30
1
1
1
Valence electrons
Where most chemical
Reactions occur.
H
2
9
4 Be
7
3 Li
2, 1
23
Na
11
3
11
5 B
2, 3
2, 2
24
12
2, 8, 1
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Mg
2, 8, 2
27
13
Al
2, 8, 3
1 - 31
1
1H
Electron Dot Structures
H
7
Li
3
Li
23
11 Na
Show only
Valence
Electrons
Na
K
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1 - 32
1
H
8
He
2
3
4
5
6
7
Li
Be
B
C
N
O
F Ne
Na
Mg
Al
Si
P
S
Cl
As
Se
Br Kr
K
Ca Ga Ge
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Ar
1 - 33
Electron Affinity
Relative ability of atoms to attract electrons
Oxidation: When electrons are grabbed by a “hungry”
element like Oxygen (O) or Chlorine (Cl)
H
Li
Be
B
C
N
O
F
Na
Mg
Al
Si
P
S
Cl
K
Ca
Ga
Ge
As
Se
Br
Rb
Sr
In
Sn
Sb
Te
I
Cs
Ba
Tl
Pb
Bi
Po
At
© Chemeketa Community College: CH117
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4 - 50
23
11 Na
Ions
11 +’s
11 -’s
0
Na
Metals give e-s to make (+) ions (Cations)
11 +’s
10 -’s
1+
Na1+
2, 8 = [Ne]
Now has e-s like Ne
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1 - 35
35
Cl
17
Ions
17 +’s
17 -’s
Cl
0
Nonmetals take e-s to make (–) ions (anions)
17 +’s
18 -’s
2, 8, 8 = [Ar]
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1-
Cl = Cl1-
11 - 36
Formation of NaCl
e- moves from Metal  Nonmetal
Stable octets
Na + Cl
+
Na
Metal
Cation
_
+ Cl
Nonmetal
Anion
+ and - ions attract to form an ionic bond.
Chemical Equation = expression of a reaction
Na + Cl  NaCl
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Properties of Ionic compounds
•
•
•
•
Not individual molecules
Form crystal arrays
Ions touch many others
Formula represents the average ion ratio
Na Cl
Cl Na Cl Na
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NaCl
sodium chloride
1 - 38
Common ions
Representative Elements
1+
4+
H
2+
Li
Be
3+ 4- 3- 2- 1-
He
Transition Elements
Variable
Na Mg
K
Ca Sc Ti
Rb Sr
Y
V
C
N
O
Al
Si
P
S
F
Ne
Cl Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba Ls Hf Ta W Re Os Ir
Fr Ra Ac
B
I
Xe
Pt Au Hg Tl Pb Bi Po At Rn
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
© Chemeketa Community College: CH117
1 - 39
Ionic Formulas
Metal Cations + Nonmetal Anions
Na1+
Cl1-
NaCl
Sodium Chloride
Mg2+
Cl1Cl1-
MgCl2
Magnesium Chloride
Table Salt
Used for taste & preserving
Mined from earth & from Sea
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In Sea Salt; tastes bitter
1 - 40
Polyatomic Ions
Ca2+
CO32-
CaCO3
Calcium Carbonate
Sea shells, egg shells,
Limestone, Marble;
Mg2+
SO42-
MgSO4
Magnesium Sulphate
In Sea Salt
Used to remove Ca from sea salt
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1 - 41
Naming Practice
Common ingredients
KI
CuO
TiO2
SiO2
KNO3
Fe2SO4
Potassium Iodide (to iodize salt)
Copper (II) Oxide or Cupric Oxide
Titanium oxide (white paint pigment)
Silicon Dioxide (anti-caking agent)
Potassium Nitrate (in fertilizer)
Ferric Sulfate (Iron in vitamins)
Sodium bicarbonate
NaHCO3
Ca3(PO4)2 Calcium Phosphate (in milk)
(baking soda)
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1 - 42
Nonmetals Share e-s
1
H
with other nonmetals
2
3
4
5
Be
B
C
N O
Na Mg
Al
Si P
Li
6
S
7
8
He
F Ne
Cl Ar
Metals give e-s to nonmetals
K
Ca Ga Ge As Se Br Kr
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Properties of covalent
compounds
Covalent compounds
•Discrete molecular units O=O
•Atoms held together by bonds
•Covalent compounds exist in all states
(CO2 - gas, H2O - liquid, SiO2 - solid)
•Formula represents atoms in a molecule
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Covalent Bonds
H
+
H
H H
Cl
+
Cl
Cl Cl
O
+
O
O O
N
+
N
N
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N
1 - 45
Covalent Bonds
H H
H-H
H2
Cl Cl
Cl-Cl
Cl2
O O
O=O
O2
N
N
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N N N2
1 - 46
Covalent Bonds
Carbon monoxide
C
O
CO
C O
CO2
O=C=O
Carbon dioxide
O C O
May modify rules to improve sound.
ie - monoxide not monooxide.
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1 - 47
Common Covalent compounds
CO
CO2
SiO2
CH4
carbon monoxide
carbon dioxide
silicon dioxide (in sand, glass)
CH3CH2CH3
CH3CH2OH
CH3CO2H
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Methane (Natural gas)
Propane (cooking gas)
Ethanol (drinking alcohol)
Acetic Acid (vinegar)
1 - 48
Tetrahedral electron-pair
Geometries
Tetrahedral
Pyramidal
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Bent
1 - 49
Bond Polarity, Electron pull
This unequal sharing results in polar bonds.
H Cl
Electrons in covalent
bonds
rarely get shared equally.
H
+
•Slight positive side
•Smaller electron pull
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Cl
-
•Slight negative
•Larger electron pull
1 - 50
Electronegativity
Relative ability of atoms to attract electrons
when they form bonds.
H
2.20
Li
Be
B
Na
Mg
Al
C
2.55
Si
N
3.04
P
2.19
O
F
3.44
3.98
S
Cl
2.58
3.16
K
Ca
Ga
Ge
As
Se
Rb
Sr
In
Sn
Sb
Te
I
Cs
Ba
Tl
Pb
Bi
Po
At
© Chemeketa Community College: CH117
Br
2.96
1 - 51
Ionic vs Covalent
Ionic
Polar Covalent
Nonpolar covalent
Like NaCl
Like sugar, water,
ethanol, Vit C
Like oil, gasoline,
hexane, Vit C
Strong attractions: Moderate attractions:
Ionic
Polar; H-bonds
High mp (1474F,801C) Low mp H2O (0C),
High bp
Low bp H2O 100C;
(2575F, 1413C)
EtOH 78C
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Weak attractions:
Vander Waals
Lowest mp/bp
1 - 52
Attractive Forces
Ionic Bonds
150 - 3000 kcal
mol
Melting Point
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NaCl
801oC
Na2S
920oC
MgF2
1248oC
1 - 53
Attractive Forces
Dipole-Dipole
0.1 - 1 kcal
mol
H
Melting Point
+
Cl
-
+
H
+
H
Cl
-
© Chemeketa Community College: CH117
- HCl
Cl
CH3F
+
H
Cl
-114oC
-142oC
-
1 - 54
Attractive Forces
Van der Waals
0.01 kcal
mol
(Dispersion Forces)
+
Cl
Cl
-
Melting Point
+
+
Cl
Cl
-
Cl
Cl
-
+
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Cl
Cl2
-102oC
CH4
-183oC
Cl
-
1 - 55
Attractive
Forces
Hydrogen Bonds
-
O
+
H
H
+
O
+
H
H
+
Polar Attraction
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1 - 56
Hydrogen Bonding of Water
5 - 10 kcal
mol
Hydrogen Bonds
Melting Point
H 2O
0oC
NH3
-78oC
Boiling Point
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H 2O
100oC
NH3
-33oC
1 - 57
Ionic vs Covalent
Ionic
Polar Covalent
Nonpolar covalent
Like NaCl
Like sugar, water,
ethanol, Vit C
Like oil, gasoline,
hexane, Vit C
Strong attractions: Moderate attractions:
Ionic
Polar; H-bonds
Weak attractions:
Vander Waals
High mp (1474F,801C) Low mp H2O (0C),
High bp
Low bp H2O 100C;
(2575F, 1413C)
EtOH 78C
Lowest mp/bp
Many water soluble Soluble in water
Insoluble in water
Form ions in water
(electrolytes)
Don’t ionize in water
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1 - 58
Dissoving of Ionic
Compounds
Polar water attracts to
Na+ and Cl- ions
“Like Dissolves Like”
When an ionic solid
dissolves in water, the
polar solvent removes
ions from the crystal
lattice.
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1 - 59
Dissoving of Ionic
Compounds
“Like Dissolves Like”
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1 - 60
Dissolving covalent
compounds
Covalent compounds do not break into ions.
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Electrolytes
Ionic
(Salt)
(sugar)
C6H12O6
NaCl
Cl-
Covalent
Na+
Na+
Cl
Dissolved Ions in solution
NaCl  Na+ + Cl© Chemeketa Community College: CH117
C6H12O6
C6H12O6
No Ions in solution
1 - 62
Ionic vs Covalent
Ionic
Polar Covalent
Nonpolar covalent
Like NaCl
Like sugar, water,
ethanol, Vit C
Like oil, gasoline,
hexane, Vit C
Strong attractions: Moderate attractions:
Ionic
Polar; H-bonds
Weak attractions:
Vander Waals
High mp (1474F,801C) Low mp H2O (0C),
High bp
Low bp H2O 100C;
(2575F, 1413C)
EtOH 78C
Lowest mp/bp
Many water soluble Soluble in water
Insoluble in water
Form ions in water
(electrolytes)
Don’t ionize in water
Not flammable
Flammable
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Flammable
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Organic Functional Groups
Hydrocarbons
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Drawing Covalent Compounds
Practice building: Build with models
Hexane
Ethylene
Ethanol (an alcohol)
Isopropyl alcohol
Cinnamaldehyde (an aldehyde)
Acetone (a ketone)
Acetic Acid (a carboxylic acid)
Butyric Acid
Phenol
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Flavors: Terpenes
CH3
Limonene
Citronellol
Orange/lemons
Roses/geraniums
OH
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Smell:
R-(-)-carvone
Spearmint
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S-(+)-carvone
Caraway
(Dill)
(Manderine Orange Peel)
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Flavors: Phenols
Compounds of phenol are the active ingredients in the
essential oils of cloves, vanilla, nutmeg, and mint.
Vanilla
Cloves
OH
Rosmarinic Acid
O
Thyme
O
OH
OH
O
Nutmeg
Rosemary
HO
OH
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Pungent Flavors
Thiocyanates: in Mustards and Horseradish
Allyl isothiocyanate
Alkylamides: in chilli’s, & pepper
Capsaicin
Gingerol
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Piperine
Shogoal
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