Comparing Atoms
REVIEW
1 type of matter
2 or more types of matter
OUR FOCUS in CH 4-7
1 type of matter
2 or more types of matter
Copper Lab
Steps 1 - 8
•
•
•
•
Started out DEEP MAROON / RED
Mass crucible
25.078 g
Mass of crucible & Cu
26.558 g
Heat Copper (2 min) re-mass ????
What happened to the
mass????
Copper Lab
Steps 1 - 8
•
•
•
•
Started out DEEP MAROON / RED
Mass crucible
Mass of crucible & Cu
Heat Copper (2 min) re-mass
25.078 g
26.558 g
26.572 g
++++
Ended solid BLACK
A major change!
The red substance “rainbowed”,
changed to black and gained mass.
These three indicate the substance
underwent a
1. Chemical change
2. Physical change
3. Neither
lc
ic
a
ys
Ph
N
ge
ha
n
ha
ng
lc
m
ic
a
he
C
0%
ei
th
er
0%
e
0%
Steps 9-12
• Heat 15 min. longer
• Hard solid formed–
hard to remove from
the bottom of the
crucible
• Some red still visible
on the bottom side –
mostly black though
• Observations:
• Some still black and some
still red
– Red is the original
copper that has not
reacted.
– Black – is copper that
reacted with ????
Oxygen in the air
DAY 2 – Part A
The black and red substance you
broke up in the bottom of the
crucible and transferred to an
empty test tube was
1. A pure substance
2. A mixture of
substances
0%
m
A
A
pu
re
su
b
ix
tu
re
st
an
of
s
...
...
0%
The red substance by itself was
1. A pure substance
2. A mixture
0%
A
pu
re
ix
tu
re
m
A
su
b
st
an
ce
0%
The red pure substance is a(n)
1. Element
2. Compound
0%
Co
m
po
un
d
Ele
m
en
t
0%
Copper
An element
The black substance by itself
was
1. A pure substance
2. A mixture
0%
A
pu
re
ix
tu
re
m
A
su
b
st
an
ce
0%
The black substance by itself is
a(n)
1. Element
2. compound
0%
co
m
po
un
d
Ele
m
en
t
0%
Copper II Oxide
A compound
2 Cu + O2  2 CuO
Which is/(are) elements?
0%
0%
an
u
C
uO
C
d
on
l
O
y
ly
on
ly
on
0%
O
d
an
0%
u
C
uO
C
O
d
an
u
0%
uO
0%
C
Cu and CuO
O and CuO
Cu only
O only
CuO only
Cu and O
C
1.
2.
3.
4.
5.
6.
2 Cu + O2  2 CuO
Which is/(are) compounds?
0%
0%
an
u
C
uO
C
d
on
l
O
y
ly
on
ly
on
0%
O
d
an
0%
u
C
uO
C
O
d
an
u
0%
uO
0%
C
Cu and CuO
O and CuO
Cu only
O only
CuO only
Cu and O
C
1.
2.
3.
4.
5.
6.
• Solution saved for
part B
DAY 2 – Part A
• Mass the solid
particles remaining
from the HCl solution.
GREEN
• Mass – the copper
quantity has
decreased.
– Where is the copper?
Copper now in the Solution
NOTE: a completely different phase of matter.
Which substance was soluble in
HCl?
Cu – red substance
CuO – black substance
Neither was
Both were
0%
B
ot
h
w
er
e
w
as
N
k
bl
ac
–
uO
C
0%
ei
th
er
su
t..
.
su
bs
re
d
–
u
0%
...
0%
C
1.
2.
3.
4.
CuO + HCl  CuCl2 + H2O + Cu
solution
unreacted
Elements –
Cu
Compounds CuO HCl
CuCl2 H2O
Which is/(are) elements?...compounds?
• Zinc added to “saved
solution”
• Bubbles
• Bubbles
• Bubbles
• Color change
• Red stuff precipitates
– Physical or Chemical
Change? Chemical
DAY 2 – Part B
DAY 2 – Part B
• Reaction completed
• Observe what is left
• Identify - COPPER
• Color - REDDISH
• Squishy - YES
CuCl2 + Zn  ZnCl2 + Cu
(Solution)
What
Happened?
Zinc replaces
copper in the
solution and
copper
precipitated
out
CuCl2 + Zn  ZnCl2 + Cu
Which is/(are) elements?
CuCl2 and Cu
CuCl2 and ZnCl2
Zn and ZnCl2
Zn and Cu
0%
Zn
an
d
C
u
Cl
2
Zn
d
an
Zn
d
an
uC
l2
C
0%
Zn
C
Cu
d
an
uC
l2
0%
l2
0%
C
1.
2.
3.
4.
CuCl2 + Zn  ZnCl2 + Cu
Which is/(are) compounds?
CuCl2 and Cu
CuCl2 and ZnCl2
Zn and ZnCl2
Zn and Cu
0%
Zn
an
d
C
u
Cl
2
Zn
d
an
Zn
d
an
uC
l2
C
0%
Zn
C
Cu
d
an
uC
l2
0%
l2
0%
C
1.
2.
3.
4.
CuCl2 + Zn  ZnCl2 + Cu
(Solution)
Zinc replaced
copper in the
solution
Neither Heating nor other
means breaks down copper
• ELEMENT
• True of all elements!
Pure substance with
one type of atom.
• LIME=??
• 1800 Battery
• 1807=H.Davy used
battery to decompose
(electrolyze) metal oxides
(= Ca)
• Later Muriatic Acid
broken down to find Cl
Today’s Element List
• 50 commonly used
• 10 = 99% of the mass
of the Earth (5=92%)
(O,Si,H, Al, Fe,
Ca,Na,Mg, Cl,K)
Scientists to Know …
CHADWICK
THOMSON
RUTHERFORD
DALTON
de BROGLIE
BOHR
Bellringer
When scientists wanted to find out what an
atom was, they were not able to look directly
at what the atom was made of. They had to
make inferences from the results of many
different experiments. It was like trying to
describe a picture, such as the one on the
next slide, with only small portions visible.
Bellringer, continued
1. Write four sentences describing what
you can see of the above picture.
2. What information or parts of the picture
would make
your descriptions more accurate
without revealing the entire picture?
The Beginnings of Atomic
Theory
〉 Who came up with the first theory of atoms?
.
Democritus
• 1st to “think” of atoms
• Derived from Greek
word – “unable to be
divided” (indivisible)
• Called them - atomos
• 4th century BC
Democritus did not have evidence for his atomic theory.
John Dalton
• 1808
• Atoms are tiny hard
spheres
• Created the atomic
theory.
– All atoms of a given
element are alike
– Atoms of elements
could join to form
compounds
Educated himself
age 12 became a school teacher
Dalton’s Atomic Theory,
continued
• Dalton used experimental evidence.
– Law of definite proportions: A chemical compound
always contains the same elements in exactly the same
proportions by weight or mass.
Dalton’s theory did not fit all observations.
Atomic Theory through Time
400 BC Democritus
1808 John Dalton:
1869 D. Mendeleev:
organizes periodic table
1897
1911
1913
1923
1932
JJ Thompson
Ernest Rutherford
Niels Bohr
Louis de Broglie
James Chadwick
Because of Mendeleev!!!
In 1898 …
W. Ramsay and M. Traves find Krypton,
Neon and Xenon within 3 months using
periodic table
• 1700s = indirect
evidence of atoms
• 1st real proof atom’s
existed (1905)
Einstein calculations
of Brownian motion,
heat as atomic motion
and momentum
conservation.
•
Atomic Theory through Time
400 BC Democritus
1808 John Dalton:
1869 D. Mendeleev:
organizes periodic table
1897
1911
1913
1923
1932
JJ Thompson
Ernest Rutherford
Niels Bohr
Louis de Broglie
James Chadwick
JJ Thomson
•
experimented with currents
of electricity inside empty
glass tubes.
•
PLAY THE SEGMENT FROM THE CD
JJ Thomson
•
•
experimented with currents
of electricity inside empty
glass tubes.
Discovered
– electron in every atom
– electrons have a negative charge
– “Plum-pudding” model
Ernest Rutherford
Geiger and Marsden
Lab 18.1 – Gold Foil Experiment
PLAY THE SEGMENT FROM THE CD
•  particles
Rutherford
– most passed straight through
• Atom mostly empty space !
– some scattered at large angles
• Center positively charged
nucleus
Niels Bohr
Electrons in an atom move
in a set path around the
nucleus / similar to planets
around the sun
Electrons orbit the nucleus
in fixed orbits
Orbits have fixed amount of energy
Louis de Broglie
• By 1925 Bohr’s Model was altered.
– Electrons behave more like waves on
– a vibrating string
– analyzed a moving particle
as a wave
James Chadwick
• Research focused on radioactivity.
• With Rutherford – knew there had to be
another particle with the proton in the
nucleus (missing mass)
• discovered neutron
• neutrons are the missing
mass in the atom
Atom
• 1955
• Mueller – Professor at Penn State
• 1st to see an atom with an ion
microscope
• synthetic Metals (???)
Atoms broken down further
• Nucleus – Center of atom: Dense
– Protons and Neutrons: similar in size and mass
• Protons – positive charge
• Neutrons – no electric charge
• Outside the Nucleus
– Electrons – cloud of tiny particles with little mass
• Electrons – negative charge (-1)
• Size – nucleus : marble – distance to
electrons : stadium
Relative Size of Atoms
• Atom : Person as
Person : Ave. Star
• Atom : Apple as
Apple : Earth
(picture apple full of
atoms and then Earth
full of apples)
Who stated that elements are
made of atoms?
Dalton
Chadwick
Rutherford
Bohr
Thomson
0%
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D
1.
2.
3.
4.
5.
Who discovered the electron?
Dalton
Chadwick
Rutherford
Bohr
Thomson
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D
1.
2.
3.
4.
5.
Who discovered that atoms are
mostly empty space?
Dalton
Chadwick
Rutherford
Bohr
Thomson
0%
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so
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D
1.
2.
3.
4.
5.
Who discovered the nucleus?
Dalton
Chadwick
Rutherford
Bohr
Thomson
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so
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D
1.
2.
3.
4.
5.
Who discovered the proton in the
nucleus?
Dalton
Chadwick
Rutherford
Bohr
Thomson
0%
om
so
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D
1.
2.
3.
4.
5.
Who discovered the neutron?
Dalton
Chadwick
Rutherford
Bohr
Thomson
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to
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0%
D
1.
2.
3.
4.
5.
Who stated that electrons are
located in fixed energy levels?
Dalton
Chadwick
Rutherford
Bohr
Thomson
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so
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D
1.
2.
3.
4.
5.
Number VS Mass
• Atomic Number
– # of protons in an
atom
• Atomic Mass
– # of protons and neutrons
Mass Number
Chemical Symbol
(# protons + # neutrons)
12
Atomic Number
(# protons)
6
Mass # - Atomic # = neutron #
12 – 6 = 6 neutrons
How many
protons?
How many
electrons?
How many
neutrons?
Draw a atomic
model for this
element?
14
6
How many
protons?
How many
electrons?
How many
neutrons?
Draw a atomic
model for this
element?
7
3
How many
protons?
How many
electrons?
How many
neutrons?
Draw a atomic
model for this
element?
14
How many
protons?
How many
neutrons?
238
Boron-11
atomic number?
1
2
3
4
5
6
11
0%
11
0%
6
0%
5
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
5.
6.
7.
Boron-11
number of protons?
1
2
3
4
5
6
11
0%
11
0%
6
0%
5
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
5.
6.
7.
Boron-11
number of electrons?
1
2
3
4
5
6
11
0%
11
0%
6
0%
5
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
5.
6.
7.
Boron-11
number of neutrons?
1
2
3
4
5
6
11
0%
11
0%
6
0%
5
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
5.
6.
7.
Boron-11
number of energy levels?
1
2
3
4
5
6
11
0%
11
0%
6
0%
5
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
5.
6.
7.
Boron-11
valence electrons?
1
2
3
4
5
6
11
0%
11
0%
6
0%
5
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
5.
6.
7.
1
2
3
4
5
6
11
0%
11
0%
6
0%
5
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
5.
6.
7.
Boron-11
number of electrons in the first
energy level?
ELECTRONS
• Charge: –1
• Exact position can not
be identified (cloud)
• Found in Orbitals
within Energy Levels
- 1st orbital: 2 (1s)
- 2nd orbital: 8 (2s / 6p)
- 3rd orbital: 8 (2s / 6p )
- 4th orbital: 18 (2s / 6p / (*3rd -10d)
- 5th orbital: 18 (2s / 6p / (*4th -10d)
Complete the energy levels …
• # of Protons? 7
• # electrons? 7
2
• # e’ in
orbital?
• # e; in 2nd orbital? 5
• # of valence e’ ? 5
1st
NITROGEN
Electrons / Energy Levels
Some energy levels can overlap – subdivided into orbitals
As electrons FALL
BACK to a lower
energy level –
ENERGY is given
off.
- closest to nucleus / lowest energy
• Imagine floor is magnetic
and shoes repel. Paper
could pass under
shoes….
• Sub microscopic world
operates this way only it
is ELECTRIC, not
magnetic!
• Special Cases: nucleus of
two atoms touch= thermal
nuclear reaction.
FISSION / FUSION
ISOTOPES
•Result when neutrons are
added to an atom
•Vary in mass but are the same
element because proton # is
not changed
Atomic Mass Unit
• AMU
– Is equal to 1/12th of the mass of a carbon
atom
– 1 AMU = isotope of carbon ( 6 protons / 6
neutrons)
• Average atomic mass – weighted avg.
Center of a atom, contains most
of the atom’s mass
Proton
Neutron
Electron
Nucleus
Energy levels
Mass number
Electromagnetic
force
0%
0%
0%
0%
0%
0%
0%
Pr
ot
on
N
eu
tro
n
El
ec
tr
on
N
uc
En
le
us
er
gy
le
M
ve
as
ls
s
nu
El
ec
m
tr
om ber
ag
ne
ti.
..
1.
2.
3.
4.
5.
6.
7.
Positively charged particle that
exists in the nucleus
of an atom.
Proton
Neutron
Electron
Nucleus
Energy levels
Mass number
Eelctromagnetic
force
0%
0%
0%
0%
0%
0%
0%
Pr
ot
on
N
eu
tro
n
El
ec
tr
on
N
uc
En
le
us
er
gy
le
M
ve
as
ls
s
nu
Ee
m
lc
tr
om ber
ag
ne
ti.
..
1.
2.
3.
4.
5.
6.
7.
The least massive of the three
subatomic particles which also
carries an negative net charge.
Proton
Neutron
Electron
Nucleus
Energy levels
Mass number
Electromagnetic
force
0%
0%
0%
0%
0%
0%
0%
Pr
ot
on
N
eu
tro
n
El
ec
tr
on
N
uc
En
le
us
er
gy
le
M
ve
as
ls
s
nu
El
ec
m
tr
om ber
ag
ne
ti.
..
1.
2.
3.
4.
5.
6.
7.
Particle with no charge that
exists in the nucleus of an atom
Proton
Neutron
Electron
Nucleus
Energy levels
Mass number
Electromagnetic
force
0%
0%
0%
0%
0%
0%
0%
Pr
ot
on
N
eu
tro
n
El
ec
tr
on
N
uc
En
le
us
er
gy
le
M
ve
as
ls
s
nu
El
ec
m
tr
om ber
ag
ne
ti.
..
1.
2.
3.
4.
5.
6.
7.
Describes how electrons are
arranged around an atom
Proton
Neutron
Electron
Nucleus
Energy levels
Mass number
Electromagnetic
force
0%
0%
0%
0%
0%
0%
0%
Pr
ot
on
N
eu
tro
n
El
ec
tr
on
N
uc
En
le
us
er
gy
le
M
ve
as
ls
s
nu
El
ec
m
tr
om ber
ag
ne
ti.
..
1.
2.
3.
4.
5.
6.
7.
The force that holds the atom
together is called
Proton
Neutron
Electron
Nucleus
Energy levels
Mass number
Electromagnetic
force
0%
0%
0%
0%
0%
0%
0%
Pr
ot
on
N
eu
tro
n
El
ec
tr
on
N
E n u cl
eu
er
s
gy
l
El
M
as eve
ec
l
tr
s
om
nu s
m
ag
be
ne
r
tic
fo
rc
e
1.
2.
3.
4.
5.
6.
7.
The total number of protons and
neutrons in the nucleus of an
atom
Proton
Neutron
Electron
Nucleus
Energy levels
Mass number
Electromagnetic
force
0%
0%
0%
0%
0%
0%
0%
Pr
ot
on
N
eu
tro
n
El
ec
tr
on
N
uc
En
le
us
er
gy
le
M
ve
as
ls
s
nu
El
ec
m
tr
om ber
ag
ne
ti.
..
1.
2.
3.
4.
5.
6.
7.
• Heat added puts
electrons at a higher
energy level –
coming down emits
light.
• Different elements
burn different colors
because light is
emitted a different
wave frequencies
Fireworks
18.3 Periodic Table
PERIODIC TABLE
• Groups similar elements together
– Arranged by the # of protons
– Helps predict properties of an element
PERIODIC LAW – states that when elements
are arranged in order by # of protons,
similarities in properties will occur in a pattern
Today’s Element List
• 50 commonly used
• 10 = 99% of the mass
of the Earth (5=92%)
(O,Si,H, Al, Fe,
Ca,Na,Mg, Cl,K)
Atom Building Reminders
Symbol
GROUPS
PERIOD
To keep table
shorter/ in line
GROUPS • Atoms of elements in the same
group have the same # of
valence electrons and therefore
behave similarly
PERIODS •All elements in a period have the
same # of atomic orbitals.
•Every element in period 1 has one
orbital filled
FAMILIES OF ELEMENTS
• Metals
– Shiny
– Solids
– Stretched and
Shaped
– Conductors of heat
and electricity
• Nonmetals
– Solids, liquids or
gases
– Solids – dull and
brittle
– Poor conductors of
heat and electricity
• Semiconductors /
Metalloids
METALS
• 4 Different kinds of metals
– Alkali metals: soft, shiny and very reactive
• Group 1: not found in nature as elements
– Alkaline earth-metals: less reactive
• Group 2: have two valence electrons
– Transition Metals: many uses
• Groups 3-12
– Synthetic Metals (???)
The Atom – Atom Building
Game
Key Questions
• What are atoms
and how are they
put together?
• What does atomic
structure have to do
with the periodic
table?
Subatomic Particles
• What three basic particles
make up all atoms?
Subatomic Particles
• Protons
• Neutrons
• Electrons
Subatomic Particles
• The marbles represent
these particles. Can you
guess which marble
represents which
particle?
Subatomic Particles
• Protons
• Neutrons
• Electrons
Build a Carbon –13
atom
• Protons= carbon’s atomic #
• Neutrons = 13 – 6 = 7
• Electrons = carbon’s atomic number when
electrically neutral
If you add a proton (+) and an
electron (-) , what
element/isotope do you
have?
• Protons = 7
(tells what the element is)
• Neutrons = 7 still
• (tells what the isotope is)
• Electrons = 7 (electrically neutral when
same # as protons … or it is an ion
{charged})
The game of Atomic
Challenge
• 4 players or teams per board
• Each player starts with 6 blues, 5
reds, and 5 yellows in their board
pocket.
• Each player takes turns adding
marbles to the atom (up to 5 per
turn) to make real, stable atoms.
• The first player to lose all their
marbles wins!!!
Alkali Metal
Orange
Halogen
Yellow
Alkali
EarthMetal
Metalloids
Light Blue
Circle Them
Noble Gas
Dark Orange
RED
Rare Earth
Other-Metal
Royal Blue
Purple
Non
Metal
Green
Transition
Metal
Dark Blue
Y R
E E
L D
L
O
W
Noble Gases