Transcript Atomic Theory PowerPoint Notes

Improvements
• More info about the people, but take only 1-2
days to cover them
Bell Work 12/9/13
• Start new bellwork titled “Atoms”
1.What do you remember about atoms? (their
structure, the subatomic particles, the
charges…)
2.W5SAYWoS
Happy
th
16
Birthday Kendle
Rivera!
Atoms:
The Building
Blocks of Matter
• Prior knowledge
• Today
Schedule
– Elements to memorize
– Notes on history of atom
– Worksheet
• Monday
– Electron configuration
• Tuesday
– Isotope quiz!
Elements to Memorize
• 1-20, 26-30, 47, 50, 78-80, 82
#
Name
Symbol
How remember
Today you are going to…take notes on the history of the
atom.
So you can…explain how & by whom the parts of the
atom have been discovered.
You’ll know you’ve got it when you can
• List the scientists of the atom and their achievements
History of Atom Overview Video
• http://www.youtube.com/watch?v=B2aFTN
hgyII&feature=related
Leucippus & Democritus
• Democritus 460 BC - 370 BC
– Student of Leucippus
– Believed all matter is made up of various
imperishable, indivisible things which he
called atoma, or “indivisible units”
– Basically, they named the atom!
Aristotle
• 384 BC – 322 BC
• Believed matter consisted of 4 basic elements
• Wrong, but people
believed
him because he
was popular with
important people
& the church.
Alchemists
• 1100’s
• European “scientists” that tried to make
gold from other metals
– Couldn’t be done
• Added ideas of observation &
experimentation!
• Recorded info on properties of matter
Bell Work 12/10/13
1.What did Democritus think?
2.What did Aristotle think?
3.What did alchemist try to do? How did this
advance science?
John Dalton
• 1766 – 1844
• Had a theory…
Dalton’s Atomic Theory
1. All matter is composed of atoms
2. Atoms of a given element are identical in size,
mass, and other properties; atoms of different
elements are different
3. Atoms cannot be subdivided, created, or
destroyed
4. Atoms of different elements combine in simple
whole-number ratios to form compounds
5. In chemical reactions, atoms are combined,
separated, or rearranged.
Dalton’s Atomic Theory
(Simplified)
1. All matter is composed of atoms
2. Atoms of same element are identical; atoms of
different elements are different
3. Atoms cannot be subdivided, created, nor
destroyed
4. Atoms of different elements combine to form
compounds
5. In chemical reactions, atoms are rearranged.
Modern Atomic Theory
• Still True…
– All matter is composed of atoms
– Atoms of any one element differ in properties
from atoms of another.
• Different
– Atoms of the same element may have
different masses! (Called isotopes)
– Atoms are divisible (not by ordinary chem. means).
• Nuclear reactions!
Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle...DISCOVERED THE ELECTRON!!
Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.
Discovery of the Electron
TV Demo!
Cathode rays – stream of electrons
e- moved ______________ the positive
charged plate
Some Modern
Cathode Ray Tubes
Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless of
the element used to produce them. All elements must
contain identically charged electrons.
Atoms are neutral, so there must be positive particles
in the atom to balance the negative charge of the
electrons
J.J. Thomson’s Atomic Model
I love me some
plum puddin’!
Discovered all electrons have equal charge, but couldn’t
measure mass or charge of the electrons.
Thomson believed that the electrons were like plums
embedded in a positively charged “pudding,” thus it was
called the “plum pudding” model.
Mass of the Electron
1909 – Robert Millikan
determines the mass of
the electron.
Enables him to calculate
the charge too!
The oil drop apparatus
Mass of the
electron is
9.109 x 10-31 kg
Conclusions from the Study of
the Electron
Electrons have so little mass that atoms must
contain other particles that account for most of
the mass
1911: Rutherford’s Gold Foil
Experiment
 Fired alpha particles (helium nuclei, ___ charge)
 Particles were fired at a thin sheet of gold foil
 Particle hits on the detecting screen (film) are
recorded
 “Gold foil” demo
Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”
Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged
Top of worksheet
Bohr Model of Atom
aka “planetary model”
1. Electrons assume only certain orbits around the nucleus.
These orbits are stable and called "stationary" orbits.
2. Each orbit has an energy level associated with it. For
example the orbit closest to the nucleus has an energy E1, the
next closest E2 and so on.
3. Light is emitted when an electron jumps from a higher orbit
to a lower orbit and absorbed when it jumps from a lower to
higher orbit.
4. Energy of light emitted is the difference between the two
orbit energies.
Bohr Model of Atom
aka “planetary model”
1st shell  2 e2nd shell  8 e3rd shell  8 e4th shell  18 e5th shell  18 e6th shell  32 e7th shell  32 e-
Electron Cloud
• More accurate
• e- don’t travel in simple, specific orbits
• e- travel around nucleus in random,
unpredictable orbits at superfast speeds
• Can’t tell exactly where they are, but they’re
somewhere in the “e- cloud”
Orbitals
Electrons can be in 4
types of orbitals within
an energy level…
Named s, p, d, or f
Don’t worry about them
for now…we’ll talk more
about them later.
Bell Work 11/27/12
1.Discovered the nucleus
2.Planetary model of atom
3.Plum pudding model of atom
4.Discovered most of the atom is empty space
5.Cathode rays
6.Discovered electron
7.Gold foil experiment
8.W5SAYBoS
Today you are going to…take notes on the parts of an
atom & isotopes.
So you can…explain the basic structure of an atom,
which will help you to predict bonds in the future.
You’ll know you’ve got it when you can
• Identify all parts of an atom, their relative masses,
charges, and location. (complete chart)
• Determine the mass of an isotope
Atom – smallest particle of an element that
retains the chemical properties of that
element.
Composed of:
protons
neutrons
electrons
Protons
Subatomic Particles
Positive charge
In nucleus (tiny, dense, center of atom)
Mass of 1 amu (atomic mass unit)
Neutrons
Neutral (no charge)
In nucleus
Mass of 1 amu
Electrons
Negative charge
In “electron cloud” around nucleus (“orbit” nucleus)
Very little mass (about 1/2000 P, or 0.0006 amu)
Atomic Particles
Particle
Charge
Mass (kg)
Location
Electron
-1
9.109 x 10-31
Electron
cloud
Proton
+1
1.673 x 10-27
Nucleus
0
1.675 x 10-27
Nucleus
Neutron
Force in the Nucleus
•Two protons extremely close to each other attract
•(indirect effect of strong nuclear force, the
strongest force in the universe!)
•Over 100 protons can exist together in a nucleus!
•Strong nuclear force has same effect on neutrons.
“e-”
Protons
cathode rays
“no” “p+”
+ charge
Determines what
element atom is
no charge
- charge
Electron
very little
mass
orbits nucleus
subatomic
particles
found in atom
charged
about same
mass
Neutrons
in nucleus
Understanding Isotopes
Atomic Number
• Number of protons in an atom
• Tells which element atom is
– Atoms of the same element ALWAYS have
the same number of protons.
• Above atom on periodic table
• What subatomic particles have the most mass?
• What subatomic particle has hardly any mass?
• Therefore, an atom’s mass depends on how
many ___ and ___ it has.
• All atoms of the same element have the same
____ ____, which means they have the same
number of _____.
• Do all atoms of the same element have the
same mass?
• What must be different about these atoms?
• Atoms of the same element with a different
number of neutrons are called isotopes.
Isotopes
Elements occur in
nature as mixtures
of isotopes.
Isotopes are atoms of
the same element that
differ in the number
of neutrons
Isotopes are named by
their mass number
Isotopes
atoms of same element with different number of
neutrons and, therefore, different masses
Isotope
Protons
Electrons
Neutrons
Hydrogen–1
(protium)
1
1
0
Hydrogen-2
(deuterium)
1
1
1
Hydrogen-3
(tritium)
1
1
2
Nucleus
Mass Number
•number of protons and neutrons in the nucleus of an atom.
•measured in atomic mass units (amu)
• 1 proton = 1 amu
1 neutron = 1 amu
Mass # = p+ + n0
Assume the particles below are atoms, meaning they
have no charge.
Isotope
p+
n0
e-
Mass #
Oxygen - 18
8
10
8
18
Arsenic - 75
33
42
33
75
Phosphorus - 31
15
16
15
31
Atomic Mass
• average mass of all the naturally isotopes of that
element
• Found under symbol on periodic table
Atomic mass of Carbon = 12.011
Symbol
Composition of
the nucleus
% in nature
Carbon-12
12C
6 protons
6 neutrons
98.89%
Carbon-13
13C
6 protons
7 neutrons
1.11%
Carbon-14
14C
6 protons
8 neutrons
<0.01%
Isotope
Atomic Mass
• average mass of all the naturally
isotopes of that element
• Also the mass of 1 mole of an element!
There are two isotopic notations
Element name – mass # or mass#
Symbol
atomic #
Chlorine – 37
___ protons
___ electrons
___ neutrons
108
Ag
47
___ protons
___ electrons
___ neutrons
Carbon – 10
___ protons
___ electrons
___ neutrons
Gold -200
___ protons
___ electrons
___ neutrons
13
C
6
___ protons
___ electrons
___ neutrons
197
Au
79
___ protons
___ electrons
___ neutrons
Sulfur-31
___ protons
___ electrons
___ neutrons
197
Hg
80
___ protons
___ electrons
___ neutrons
Calcium-39
___ protons
___ electrons
___ neutrons
19
F
9
Strontium-87
___ protons
___ electrons
___ neutrons
119
Sn
50
Ions – charged atoms!
• Charge of –2 has 2 more electrons than
protons
• Charge of +3 has 3 more protons than
electrons
Bell Ringer 12/5/12
Sulfur-31
___ protons
___ electrons
___ neutrons
4. W5SAYW
197
Hg
80
___ protons
___ electrons
___ neutrons
Quiz answers
Quiz answers
Quiz answers
Bell Work 12/7/12
1. What do you know about electron configuration?
Bell Work 12/11/12 – 3 min
Determine the number of electrons, protons, and
neutrons in the following neutral atoms.
1. Helium-5
2. Sulphur-34
Bonus!
• Empty 2 liter bottles
• Big pop cans (the bigger the better)
• Now lets review chart!
Today you are going to…take notes on and begin writing
the electron configuration of atoms
So you can…better understand the structure of an atom
and predict ionic bonds
You’ll know you’ve got it when you can
• Write the electron configurations and draw the
Bohr models for
– All elements to calcium
– All atoms up to barium
– All elements!
Valence electrons
• electrons in the outermost shell of an atom.
• IMPORTANT! - determine many of the
properties of an atom
• What row?
• What orbital (letter)?
• How many over?
Bell Work 12/13/12
• Turn in bonus
• Write the electron configuration for
1.Bromine
2.Iodine
3.Astatine
Valence electrons
• electrons in the outermost shell of an atom.
• IMPORTANT! - determine many of the
properties of an atom
Electron Configurations
• Electron “locations”
• Identifies which energy level the electrons
are in
• There are 4 orbitals – s, p, d, & f
– s orbital, holds up to 2 electrons
– p orbital, holds up to 6 electrons
– d orbital, holds up to 10 electrons
– f orbital, holds up to 14 electrons
Electron Configuration
Energy
Level
2
1s
Orbital
# of
electrons
Bell Work 12/14/12 – 5 min
• Turn in bonus
• Write the electron configuration & Bohr
diagram for
1. Fluorine-19
2. Bromine-80
3. Astatine-210
4.What are valence electrons?
Schedule
•
•
•
•
Bell work/check homework
Grades
Review homework
Electron dot diagram
Today you are going to…take notes on and begin writing
the electron dot diagram of atoms
So you can…better understand the structure of an atom
and predict ionic bonds
You’ll know you’ve got it when you can
• Write the electron configurations, draw the Bohr
models, and electron dot diagrams for
– All elements!
Electron Configuration
Energy
Level
1
3s
Orbital
# of
electrons
Electron Configuration
4
2p
Energy level?
Orbital?
# of electrons?
Beryllium (Be) – Atomic # 4
1s2, 2s2
Sulfur (S)
1s2, 2s2,2p6, 3s2, 3p4
Iron (Fe) – Atomic # 26
1s2, 2s2,2p6, 3s2, 3p6, 4s2, 3d6
Bohr Models
• Where are the valence electrons?
Homework (or Homeroom work)
Write the electron configuration AND draw the
following atoms
• Helium-5
• Nitrogen-15
• Iron- 54
• Antimony-123 (symbol Sb)
• BONUS CHART!
Bell Work 12/11/12
Put your homework upside-down on your desk.
Write the electron configuration AND draw the
following atoms
1. Phosphorus-30
2. Cobalt-56
Bell Work 12/10/12
Put your homework upside-down on your desk.
1. Chlorine-36
2. Nickel-56
Electron Dot Diagram
1s2
Bell Work 12/20/12
Which numbers go together?
1.Discovered the nucleus
2.Planetary model of atom
3.Plum pudding model of atom
4.Discovered most of the atom is empty space
5.Cathode rays
6.Gold foil experiment
7.Discovered electron
Which subatomic particles…
+ charge
no charge
- charge
very little mass
orbits nucleus
found in atom
subatomic particles
charged
about same mass
in nucleus
cathode rays
“p+”
“no”
“e-”
Atom & Solar System
Similar
little stuff (planets n e-) orbits big stuff
both mostly empty space
orbiting things are always moving
Different
orbits less precise in space
solar system bigger!
solar system has life
some atomic particles have charges!
planets have moons
Atomic structure
Proton - +, has mass of 1amu, in nucleus,
always same # in atom!
Neutron – neutral (no charge), 1 amu, in nucleus,
different # in different atoms (isotopes)
Electron – orbits nucleus, negative charge,
1/2000 mass of proton/nutron, can be lost
through bonding
Dalton’s Atomic Theory
(Simplified)
1. All matter is composed of atoms
2. Atoms of same element are identical; atoms of
different elements are different
3. Atoms cannot be subdivided, created, nor
destroyed
4. Atoms of different elements combine to form
compounds
5. In chemical reactions, atoms are rearranged.
STOP
Bromine-81
___ protons
___ electrons
___ neutrons
protons
40
Ar
18
___
___
electrons
___
neutrons
Bell Ringer 11/14 – 5 minutes
1. The number of ___________ an atom
has; gives it it’s identity.
2. Atoms of the same element that have a
different number of neutrons are called
______________.
3. W5SAYW
4. Study
Element Poster Project (33 pts)
Chemical Symbol, average atomic mass, &
atomic number
_______ 3 points
Electron configuration
_______ 3 points
All known isotopes
______ 2 points
Electron Dot Diagram
______ 2 points
At least 3 uses
______ 3 points
Atomic Particles
Particle
Charge
Mass (kg)
Location
Electron
-1
9.109 x 10-31
Electron
cloud
Proton
+1
1.673 x 10-27
Nucleus
0
1.675 x 10-27
Nucleus
Neutron
Bell Work
•number of protons and neutrons in the nucleus of an atom.
•measured in atomic mass units (amu)
Mass # = p+ + n0
Assume the particles below are atoms, meaning they
have no charge.
Nuclide (new clyde)
p+
n0
e-
Mass #
Oxygen - 17
8
9
8
17
Arsenic - 73
33
40
33
73
Phosphorus - 34
15
19
15
34
Bell Work 12/4
1. Atoms of the same element may have different
numbers of ____________, and they may gain
or lose ____________, but they ALWAYS have
the same number of _____________.
Bell Work 11/3
Protons
Electrons
“p+”
+ charge
charged
- charge
very little mass
cathode rays
“e-” orbits nucleus
about same mass
sum gives atomic
mass
in nucleus
subatomic
particles
found in atom
no charge
Neutrons
sub
“n0”
a
v
Protons
Neutrons
Electron
subatomic part
charged
+ charge
- charge
no charge
about same m
very little ma
in nucleus
orbits nucle
found in ato
cathode ray
“e-”
“n0”
“p+”
subatomic particles
charged
+ charge
- charge
no charge
about same mass
very little mass
in nucleus
orbits nucleus
found in atom
sum gives atomic mass
cathode rays
“e-”
“n0”
“p+”
The Atomic
Scale
 Most of the mass of the
atom is in the nucleus
(protons and neutrons)
 Electrons are found
outside of the nucleus (the
electron cloud)
 Most of the volume of
the atom is empty space
“q” is a particle called a “quark”
Bell Work 11/4/10
1. How much would 1 gallon of mercury weigh?
2. If a 185 lb man on mercury, how much volume
would you displace? (This is individual as it
depends on your mass.)
3. How many m&m’s do you think are in the jar?
Mercury has a density of 13.5 cm3.
Use your conversion factors…
Charge
Charged atoms have an unequal number of
protons & electrons and are called ions.
Charge = p+ - e-
Ion
p+
N0
e-
Oxygen
8
7
10
Sodium
11
12
10
Barium
56
65
Charge
+2
Size of Atoms
We think of the area occupied by electrons as an
“electron cloud”.
Radius of atom – distance from center of nucleus
to outer part of e- cloud.
Measured in picometers (pm)
1 pm = 10-12 m = 1/1,000,000,000,000 meter
pm is to cm as cm is to km
Nuclei are extremely dense…
200,000,000 metric ton/cm3
= 200,000,000,000 kg/cm3
weighs 440,000,000,000 lb/cm3
Bohr Model of Atom
1st shell  2 e2nd shell  8 e1. Find element’s atomic
3rd shell  8 enumber on p. table.
4th shell  18 e2. Draw nucleus & write
5th shell  18 e# of p+ & n0
6th shell  32 e• Mass # = p+ + n0
7th shell  32 e3. Draw electrons in
1. Helium – 5
orbitals
2. Beryllium – 11
3. Neon – 20
4. Carbon – 14
5. Potassium – 41
The Elements!
1 dozen = 12
1 gross = 144
1 ream = 500
1 mole = 6.02 x 1023
There are exactly 12 grams of
carbon-12 in one mole of carbon-12.
Bell Work 11/10 – 5 min
Take out yesterday’s work.
How many molecules of O2 are in 85.02 g
of O2? (Use dimensional analysis to find
your answer.)
1 mole O2 = 31.9988 g
1 mole = 6.02 x 1023
Avogadro’s Number
6.02 x 1023 is called “Avogadro’s Number” in
honor of the Italian chemist Amadeo Avogadro
(1776-1855).
I didn’t discover it. Its
just named after me!
(Probably cuz I’m hot.)
Amadeo Avogadro
Calculations with Moles:
Converting moles to grams
How many grams of lithium are in 3.50 moles of
lithium?
3.50 mol Li
6.941 g Li
1 mol Li
=
24.2935 g Li
24.3 g Li
Calculations with Moles:
Converting grams to moles
How many moles of lithium are in 18.2 grams of
lithium?
18.2 g Li
1 mol Li
6.941 g Li
=
2.62247 mol Li
2.62 mol Li
Calculations with Moles:
Using Avogadro’s Number
How many atoms of lithium are in 3.50 moles of
lithium?
3.50 mol Li 6.022 x 1023 atoms Li
1 mol Li
= 21.077 x 1023
2.1077 x 1024
2.11 x 1024
2.11 x 1024 atoms Li
Calculations with Moles:
Using Avogadro’s Number
How many atoms of lithium are in 18.2 g of
lithium?
18.2 g Li 1 mol Li
6.94 g Li
6.022 x 1023 atoms Li
1 mol Li
(18.2)(6.022 x 1023)/6.94
= 1.58 x 1024 atoms Li
Bell Work 11/11 – 5 min
Take out your homework.
How many molecules of H2O are in 6,022 g
of H2O? (Use dimensional analysis to find
your answer.)
Bell Work 11/15 – 5 min
6CO2 + 6H2O (+ light energy)  C6H12O6 + 6O2
1. During photosythesis, a 1000 leaved plant
produces about 1.429 g of O2 in an hour.
Convert this to moles.
2. W5SAYW
Mole Ratio
6CO2 + 6H2O (+ light energy)  C6H12O6 + 6O2
According to the above equation...
if 6 mol carbon dioxide are combined with
6 mol water, how many moles of glucose
will be produced?
How many moles of oxygen will be
produced?
This is called the mole ratio!
Moles of one substance: moles of another
Mole Ratio
Cu(s) + 4HNO3(aq)  Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)
In an experiment where nitric acid reacts
with a penny, 3.100 g of copper (Cu) are
lost and 4.489 g of nitrogen dioxide
(NO2) are produced. What is the mole
ratio of this reaction?
To find the mole ratio, calculate how many
moles of each participate in the reaction.
Law of Conservation of Mass
Mass is neither
created nor destroyed
during chemical or
physical reactions.
Total mass of reactants
=
Total mass of products
Antoine Lavoisier
Bell Work 11/17 – 5 min
Take out mole conversions wksts 1 & 2.
Turn your lab in if you haven’t already.
1. Calculate the number of molecules in
32.47 g of water.
Calculations with Moles:
Using Avogadro’s Number
1. Calculate the number of in 32.47 g of water.
From periodic table:
1 mol H = 1.0079
1 mol O = 15.999
1 mol H2O = 2(1.0079 g) + 1(15.999 g) = 18.0148 g
32.47 g H2O
1 mol Li
6.022 x 1023 atoms H2O
18.0148 g H2O 1 mol H2O
(32.47)(6.022 x 1023)/ 18.0148
= 1.085409 x 1024
1.085 x 1024 molecules H2O
1. How many moles of silver are in 57.00 g of Ag?
From periodic table: 1 mol Ag = 107.87 g
57.00 g Ag X 1 mol Ag
1
107.87 g Ag
0.5284 mol Ag
=
0.5284138
2. How many moles of gold are in 89.0 g of Au?
From periodic table: 1 mol Au = 196.97 g
89.0 g Au
1
X
1 mol Au
196.97 g Au
0.452 mol Au
=
0.4518454
3. How many moles of iron are in 2.43 x 1025 atoms of Fe?
From your brain (Av’s #): 1 mol = 6.022 x 1023
2.43 x 1025 atoms Fe
1 mol Fe
= 0.40352 x 102
X
1
6.022 x 1023 atoms Fe
4.04 x 101 mol Fe
40.4 mol Fe
4. How many atoms of copper are in 3.1 g of Cu?
From periodic table: 1 mol Cu = 63.546 g
From your brain (Av’s #): 1 mol = 6.022 x 1023
3.1 g Cu X 1 mol Cu X 6.022 x 1023 atoms Cu =
1
63.546 g Cu
1 mol Cu
0.29377 x 1023
2.9 x 1022 atoms Cu
5. How many molecules of carbon dioxide are in 86.00 g of
CO2?
From periodic table: 1 mol C = 12.011 g
1 mol O = 15.999 g
Therefore: 1 mol CO2 = 1(12.011) + 2(15.999 )
= 44.009 g
From your brain (Av’s #): 1 mol = 6.022 x 1023
86.00 g CO2 X 1 mol CO2
1
44.009 g CO2
X
6.022 x 1023 molecules CO2
1 mol CO2
11.77 x 1023
1.177 x 1024 molecules CO2
=
6. How many molecules of copper sulfate are in 8 g of
CuSO4?
From periodic table: 1 mol Cu = 63.546 g
1 mol S = 32.065 g
1 mol O = 15.999 g
Therefore: 1 mol CuSO4 = 1(63.546) + 1(32.065 ) + 4(15.999)
= 159.607 g
From your brain (Av’s #): 1 mol = 6.022 x 1023
8 g CuSO4 X 1 mol CuSO4 X
1
159.607 g CuSO4
6.022 x 1023 molecules CuSO4 =
1 mol CuSO4
0.30184 x 1023
3 x 1022 molecules CuSO4
8. How many atoms of oxygen are in 2.0 mol of CO2?
From chemical formula: there are 2 moles of O atoms for each
mole of CO2 molecules
1 mol CO2 = 1 mol C
2.0 mol CO2
1
X
2 mol C
1 mol CO2
=
4 mol C
4.0 mol O
7. How many atoms of carbon are in 2.0 mol of CO2?
From chemical formula: there are 1 mole of C atoms for each
mole of CO2 molecules
1 mol CO2 = 1 mol C
2.0 mol CO2
1
X
1 mol C
1 mol CO2
X
6.022 x 1023 atoms C
1.2 x 1023 atoms
1 mol C
9. How many atoms of oxygen are in 86.00 g of CO2? (See #
5)
From periodic table: 1 mol C = 12.011 g
1 mol O = 15.999 g
Therefore: 1 mol CO2 = 1(12.011) + 2(15.999 )
= 44.009 g
From your brain (Av’s #): 1 mol = 6.022 x 1023
86.00 g CO2 X 1 mol CO2
1
44.009 g CO2
X
X
2 atoms CO2
1 molecule CO2
6.022 x 1023 molecules CO2
1 mol CO2
3.9082 x 1023
3.908 x 1023 molecules CO2
On Quiz
Just like bohring worksheets!
Test Tuesday
Law of conservation of mass
Atom
Dalton’s atomic theory
Isotopes
Bohring worksheet
Protons, neutrons, electrons (chart)
Discovery of electron – who & how
Plum pudding model
Rutherford & gold foil experiment
Bohring worksheets, # e- in each shell
Avagadro’s number (memorized)
Mole problems
1 mole ratio question
1 atomic mass unit - 1/12 the mass of a carbon-12
atom
Molecular mass (m) of a substance is the mass of
one molecule of that substance, in atomic mass
units(s) u
About Quarks…
Protons and neutrons are
NOT fundamental particles.
Protons are made of
two “up” quarks and
one “down” quark.
Neutrons are made of
one “up” quark and
two “down” quarks.
Quarks are held together
by “gluons”
Protons
Neutrons
Electron
subatomic part
charged
+ charge
- charge
no charge
about same m
very little ma
in nucleus
orbits nucle
found in ato
cathode ray
“e-”
“n0”
“p+”
Bell Work 11/30/11 – 5 min
1. Who discovered the electron?
2. If a substance had a density of
200,000,000,000 kg/cm3, how much mass
would be in a 32.7 cm3 sample?
3.One kilogram weighs 2.2 lbs. How much
would the sample weigh?
Bell Work 11/29/11 – 5 min
1. 25 m = ? km
2. Who named the atom?
3. W5SAYWorS
Bell Work 11/23/11 – 5 min
1. What did J.J. Thomson discover?
2. Explain J.J. Thomson’s model of the
atom.
3. What atom is represented in the Bhor
diagram below?