You can call me DOC!
“Please
take responsibility
for the energy
you bring into this
space”
…Jill Bolte Taylor
Introduction
Significant Figures
 What is that all about?
 Remember Atlantic and
Pacific rule.
 Present vs. absent
 Do not start to count sig figs
until you hit your first nonzero number, then don’t stop
counting.
Add / Subtract
 Ans. To least decimal place
Multiply / Divide
 Answer to the least number of
sig figs.
Pacific
Ocean
Atlantic
Ocean
Watch How Easy
Chemistry with Doc
Dalton
Dalton
1. The atom is made up of identical
particles throughout
2. Particles are indivisible
3. Atom is made up of mostly (+) charge
4. Solid Billiard Ball Model
J. J. Thompson “Plum Pudding model”
1. Discovered Electrons
2. Used the “Cathode Ray Tube”
a.k.a. “Crookes tube”
3. Shot particle beams through a magnetic field
4. Concluded that the beams were made up of
particles with a negative charge…..
called electrons
Rutherford “Gold foil experiment”
1. Shot alpha particles (+) through a gold (Au) foil
2. Saw that most particles went through undeflected
3. noticed some particles were deflected
4. concluded that the atom is made up of
Small dense (+) charged particles and
is mostly open space
Bohr Model
1. Places electrons outside the nucleus in specific locations
called orbits
2. Orbits = Energy levels (n) = Periods (Remember That!)
Energy Levels
1st
2nd
3rd
Modern Atomic Theory
“Wave Mechanical Theory, Electron Cloud”
1. Like the Bohr model but can’t place electrons in an
exact location
2. Show the Most Probable Location
Atoms are composed of subatomic particles
Name
Location
Charge Mass
Protons
(Nucleons)
Nucleus
+
1 amu
Neutrons
(Nucleons)
Nucleus
0
1 amu
Electrons
Outside nucleus
in orbits
-
1/1836 amu
AMU= Atomic Mass Unit
Based on C12 as the standard, therefore
a proton 1H1 = 1/12 the Mass of Carbon
Calculating Protons, Neutrons and Electrons
12
C
6
atomic mass = protons + neutrons
atomic number = number of protons =
which identifies the element!
(+) , Nuclear Charge
Assume….since all elements on the periodic table
are
Neutral, this must also represent the # of
electrons.
IONS
Metals
When they form
a bond
Form and Ion
It is called a….
Lose Electrons
(+)
Ca(t)ion
t=(+)
Non-Metals
Gain electrons
(-)
A(n)ion
n=negative
Isotopes
1. different form of the same element
2. Differ in the number of neutrons
therefore, they have different masses
12
C
6
12
X
6
=P=
=n=
=e=
=P=
=n=
=e=
14
C
6
14
7X
Characteristics of Isotopes
1. Tend to be unstable, therefore they emit energy
which makes them radioactive
2. There are no stable isotopes above element #82
Atomic Mass
vs
(the sum of the weighted avg.
of all naturally occurring isotopes
Mass #
P+N
(Whole number)
12.0171
C
6
12
C
6
Calculate the Atomic mass of carbon that is made up of
80% Carbon 12, 15% Carbon 10 and 5% Carbon 14?
Change % to decimal, multiply by the mass, then add.
.80 X 12 = 9.6
.15 X 10 = 1.5
.05 X 14 = 0.7
11.5 amu
Lewis Dot Diagrams
1. show only valence electrons
2. remember…group number = valence electrons
1 =1, 2 =2, 13 = 3, 14 = 4, 15 = 5 etc.
3. remember the last number in the configuration
also equals # of valence electrons
Cl
2-8-7
valence electrons
3 energy levels
This tells you:
3 energy levels are occupied (Cl is in per. 3)
7 valence electrons (Grp 17)
X
X
H
He
Li
Be
B
C
N
O
F
Ne
Electron Configurations
1. remember all configurations are located under
the elements symbol
2. configurations show you
a. total number of electrons
b. number of occupied energy levels = periods
c. # of valence electrons
Ca
2-8-8-2
4 energy levels occupied
2 valence electrons
18 kernel electrons
..
Ca
Remember, after element #20 (Calcium), we then start to
fill in the d block which are the transitional metals.
(not so important)
Ground State vs Excited State
 Ground State
 Excited State
 Stable
 Unstable
 Lower energy
 Higher Energy State
Absorb energy
 Lower Energy
Release energy
 Higher energy
Bundle of Energy called a Quanta
Bright line Spectrum
35
17Cl
2-8-7
3 energy levels
(period 3)
Group 17
7 valence electrons
Spectral lines – identify the unknown
Matter
Elements
 A single pure substance
that can not be broken
down (decomposed)
 Ie: Periodic table of
elements
 ***
Diatomic Elements
Br2I2N2Cl2H2O2F2
Compounds
 Compounds
2 or more elements
combined in a fixed
definite ratio.
 Can be decomposed
 H2O CO2
Matter
Mixtures: Varied
Ratio
 HOMOGENEOUS
 HETEROGENEOUS
 True Solutions (aq)
 See multiple parts
 See only 1 part
 Sand and water
NaCl (aq)
 Separated by
evaporation and
Distillation
 Chocolate chip ice
 Boiling points
cream
 Separated by filtration
Formula Writing
Formulas show both:
Quantitative – how much, how many atoms
Qualitative – what types of elements present
3 C6H12O6
3 – coefficient, how many glucose
(3 moles)
This tells you:
Quantitative(subscripts) – 6 Carbon, 12 Hydrogen
and 6 Oxygen are present
Qualitative – Made up of Carbon, Hydrogen and Oxygen
Types of Formulas
1. Empirical – simplest whole number ratio
1. CH2O
2. Molecular (true formula)
1. C6H12O6
3. Condensed CH3CH2CH3
4. Structural
5. Hydrates
1. CuSO4
.
5 H2O
Formula Writing
1. Sum of all oxidation numbers of any formula must = 0
2. work only with the metals, non-metals and
polyatomic ions (table E)
CrissCross Method
K+ Cl-
Mg+2 S-2
KCl
MgS
Al+3
Cl-1
AlCl3
Mg +2 Br -
MgBr2
Formula Writing
1. Sum of all oxidation numbers of any formula must = 0
2. work only with the metals, non-metals and
polyatomic ions (table E)
CrissCross Method
K+ ClO4-
KClO4
Mg+2 PO4-3
Mg3(PO4)2
Al+3
NO2-1
Al(NO2)3
Mg +2 Mn04-
Mg(MnO4)2
*****Note the parenthesis around the polyatomic ions
Zone 1
Zone 3
Zone 2
M-NM = Ionic
Nm-Nm = covalent (molecular compounds)
Binary Compounds - ide
Zone 1-3
Zone 2-3
 Grp 1,2 M – NM
“Call it like you see it”
Trans M – NM
“Call it like you see it”
Roman Numerals to indicate
NaCl
Name Metal – Sodium
Name the Non Metal
(Chlorine) drop end
add - ide
Sodium Chloride
FeCl2
FeCl3
Name Metal with ox #
Iron II Chloride Iron III Chloride
KF
CuCl
MgCl2
CaO
Zone 3-3
Molecular compounds
(Covalent NM – NM)
Use Prefix on 2nd NM
Use on first if more than
1NM
1- mono, 2- di, 3-tri,
4 – Tetra, 5- penta, 6 hexa
CO Carbon Monoxide
CO2 Carbon Dioxide
N2O5 Dinitrogen Pentoxide
CuCl2
Zone 1
Zone 4
Zone 2
Zone 3
Ternary Compounds
Zone 1-3
Group 1,2 M–PInm
Na2SO4
Sodium Sulfate
Al2(SO4)3
Aluminum Sulfate
Zone 2-3
Zone 3-3
PI + - PI Transition M –PIm nm
nm
(Roman Numerals) (call it like you say
it)
Cu2SO4
Copper (I) Sulfate
CuSO4
Copper (II) sulfate
(NH4)2SO4
Ammonium Sulfate
NH4NO3
Ammonium Nitrate
Zone 3-4
PI+ - NM
m
(name it like a binary
–ide)
NH4Cl
Ammonium chloride
Naming Acids
Binary
vs
Ternary
(formula always begin with H)
HCl
1. Always start with “Hydro”
2. Name the non-metal
1. Chlorine
3. Change ending to
1. - ic acid
4. Name = Hydrochloric Acid
H – polyatomic ion
(end in ate or ite)
H – ate
H- ite
Remember, you ate it and it was
icky!
(ate-ic)
(ite-ous)
H2SO4
HNO2
Sulfuric Acid
Nitrous Acid
HNO3
HCl
H2SO4
HC2H3O2
HBr
HNO2
H2PO4
Sulfuric Acid
Nitric Acid
Hydrochloric Acid
Types of Equations
Synthesis
( 2 to 1)
A + B AB
Decomposition
(1 to 2)
AB  A + B
Fermentation (Organic)
Combustion (Organic)
(Always produces CO2 and H2O Always produces Alcohol and CO2
(C2H5OH + CO2)
Burn reaction – need O2
C3H8 + O2  CO2 + H2O
C6H12O6  C2H5OH + CO2
Types of Equations
Single Replacement
( element-compound element
compound)
Red is the Metal A + BC  AC + B
***Remember Table J Activity Series
Who is the Bully?
Ca + HCl  CaCl2 + H2 (g) works.
Cu + HCl  N.R. Why?
AG + MgCl2  Reaction….yes or no?
Types of Equations
Double Replacement
( compound-compound compound - compound)
Red is the Metal A B + C D  AD + CB
HCl + NaOH  NaCl + HOH
NaCl + HOH  NaOH + HCl
MgCl2 + (NH4)2SO4 
A Reaction will go to completion
when:
1. A gas (g) is produced
2. Water is a product
3. One of the products is
insoluble (does not dissolve)
Table F solubility Guidelines
Table F
Solubility Guidelines for Aqueous solutions
Try these out!
What type of reactions do we see?
 Zn + HCl  ZnCl2 + H2
 NaClO3  NaCl + O2
 P4 + Cl2  PCl3
 HCl + Mg(OH)2  MgCl2 + H(OH)
 BaO + SO3  BaSO4
 Pb + AgNO3  Ag + Pb(NO3)2
 AgNO3 + Na2CrO4  Ag2CrO4 + NaNO3
Balancing Equations
**An equation must show conservation of both Mass and
Charge and Energy!!!!!!
2Ca0 + O20  2Ca+2O-2
Steps to follow:
1. Write the correct formula first, if needed
2. Pick a start point and let it take you to the next……
3. If you see water, change the formula from H2O to H(OH)
4. Always work the polyatomic ions (SO4, NO3etc.) as a
whole
5. Try not to deal with any odd # coefficients.
a. if present, double their value to make it even
PRACTICE
___ Li + ___Br2  ___ LiBr
___Al + ___Cl3  ___AlCl3
___HgO  ___Hg + ___O2
___Al2O3  ___Al +
___O2
___Ca3(PO4)2 + ___H2SO4  ___Ca(SO4) + ___ H3PO4
(Combustion Reactions: Always do in this order- C,H,O)
____C3H8 + ___O2  ___CO2 + ____H2O
NaCl + F2  NaF + Cl2
AgNO3 + MgCl2  AgCl + Mg(NO3)2
FeCl3 + NaOH  Fe(OH)3 + NaCl
AlBr3 + K2SO4  KBr + Al2SO4
CH4 + O2  CO2 + H2O
Na + H2O  NaOH + H2
C3H6 + O2  CO2 + H2O
Given the unbalanced equation:
__Fe2O3 + __CO → __Fe + __CO2
When the equation is correctly balanced using the
Smallest whole-number coefficients, what is
the coefficient of CO?
(1) 1 (3) 3
(2) 2 (4) 4
Good Morning America!!!
Mole = a specific Quantity
like 1 dozen = 12
1. 22.4L of any gas
2. 6.02x1023 molecules
3. GFM gram formula mass
H2O H 2 x 1 = 2
O 1 x 16 = 16
18g = 1 mole
**GFM is the mass of a 1mole sample of
any substance.
**All base on C12 as the standard so……
H1 has a mass of 1 and = 1/12 of Carbon
Gas
Amount
H2
1 Mole
O2
1 Mole
CO2
1 Mole
Volume
Molecule
s
Mass
Doc’s Mole Bridge
÷
Volume
X
22.4L
22.4L
Molecule
Volume
6.02x1023
Mole
6.02x1023
Molecule
GFM
GFM
Mass
Mass
Doc’s Mole Bridge
(Continued)
X
# of moles of elements
Molecule
Atoms
What about atoms or particles?
Substance
Quantity
Volume
(L)
(L)(
Mass
(g)
Molecules
Mg
1 Mole
X
24 g
6.02x1023
6.02x1023
X 1 Atoms
2g
6.02x1023
1.02x1024
Atoms
H2
1 Mole
CO2
1 Mole
22.4L
X2
22.4L
44 g
6.02x1023
Atoms
Or
Particles
1.86x1024
X 3 Atoms
Mass to Mole and Mole to Mass
Volume to Mole and Mole to Volume
Volume to Mole and Mole to Volume
Determine percent composition
Mass of the part x 100 = % comp.
Whole
1. Determine the GFM
H2O H 2 x 1 = 2
O 1 x 16 = 16
18g
part x 100 =%
whole
2/18 x 100 = 11% for H
16/18 x 100 = 89% for O
100%
Determine the molecular (True) formula from
the empirical formula and molecular mass.
Empirical is NO2 and the molecular mass is 92g
1. Determine the empirical mass
NO2 N 1 x 14 = 14
O 2 x 16 = 32
46g
2. determine how many times this goes into the
molecular mass = quantity
Molec Mass = quantity
empirical mass
92/46 = 2
Molecular formula is N2O4
Determine Molecular (True) Formula
from Empirical Formula.
The empirical formula of a compound is CH2. Its
molecular mass is 70g/mole.
What is its molecular formula?
A compound is found to be 40.0% Carbon, 6.7%
Hydrogen and 53.5% Oxygen.
Its molecular mass is 60. g/mole. What is its Molecular
formula?
Determine the Empirical Formula from percent composition.
Steps
1. Change percent to gram 75% C = 75g
25% H = 25 g
2. Go from gram to mole
C 75/12 = 6.25 mole
H 25/1 = 25 mole
3. Determine mole ratio (divide each by the lowest)
6.25/6.25 = 1 C
25/ 6.25 = 4 H
Empirical Formula is CH4
Percent Composition of a Hydrate
1. Same as a % comp problem
2. Hydrate is a crystal that contains water
CuSO4
.5H O
2
This says that 1 mole of Copper II Sulfate
contains 5 moles of water
****Calculate the percent of Water in the Hydrate?
Steps
H2O
1. Calculate the gfm Cu 65, S 32 and 4 Oxy 64 + 5(18) = 251
part x 100
Whole
90 x 100 = 36%
251
2. Determine percent of water in Na2S . 9 H20?
A 10 gram sample of a hydrated crystal is heated to
constant mass (8grams), what is the percent
composition of water in this crystal?
A hydrate is a compound that includes water
molecules within its crystal structure. During an
experiment to determine the percent by mass of
water in a hydrated crystal, a student found the
mass of the hydrated crystal to be 4.10 grams.
After heating to constant mass, the mass was
3.70 grams. What is the percent by mass of
water in this crystal?
(1) 90.% (3) 9.8%
(2) 11% (4) 0.40%
Stoichiometry made Simple
 Remember not to panic, just do ratios
 Piece of cake