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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 25.078 g• Mass of crucible & Cu 26.558 g• Heat Copper (2 min) re-mass 26.572 g
+ + + +
Ended solid BLACK
A major change!
Copper Lab
The red substance “rainbowed”, changed to black and gained mass. These three indicate the substance
underwent a
Chem
ical
chan
ge
Phys
ical
cha
nge
Nei
ther
0% 0%0%
1. Chemical change
2. Physical change
3. Neither
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 ????
DAY 2 – Part A
Oxygen in the air
The black and red substance you broke up in the bottom of the crucible and transferred to an
empty test tube was
A p
ure s
ubstan
...
A m
ixtu
re o
f s...
0%0%
1. A pure substance
2. A mixture of substances
The red substance by itself was
A p
ure s
ubstan
ce
A m
ixtu
re
0%0%
1. A pure substance
2. A mixture
The black substance by itself was
A p
ure s
ubstan
ce
A m
ixtu
re
0%0%
1. A pure substance
2. A mixture
2 Cu + O2 2 CuO
Which is/(are) elements?
Cu a
nd CuO
O a
nd CuO
Cu o
nly
O o
nly
CuO o
nly
Cu a
nd O
0% 0% 0%0%0%0%
1. Cu and CuO
2. O and CuO
3. Cu only
4. O only
5. CuO only
6. Cu and O
2 Cu + O2 2 CuO
Which is/(are) compounds?
Cu a
nd CuO
O a
nd CuO
Cu o
nly
O o
nly
CuO o
nly
Cu a
nd O
0% 0% 0%0%0%0%
1. Cu and CuO
2. O and CuO
3. Cu only
4. O only
5. CuO only
6. Cu and O
DAY 2 – Part A• Solution saved for
part B
• Mass the solid particles remaining from the HCl solution.
• Mass – the copper quantity has decreased. – Where is the copper?
GREEN
Copper now in the SolutionNOTE: a completely different phase of matter.
Which substance was soluble in HCl?
Cu –
red
subst
...
CuO –
bla
ck s
u...
Nei
ther
was
Both
wer
e
0% 0%0%0%
1. Cu – red substance
2. CuO – black substance
3. Neither was
4. Both were
CuO + HCl CuCl2 + H2O + Cu unreactedsolution
Which is/(are) elements?...compounds?
Elements – Cu
Compounds - CuO HCl CuCl2 H2O
• Zinc added to “saved solution”
• Bubbles • Bubbles• Bubbles• Color change• Red stuff precipitates
– Physical or Chemical Change?
DAY 2 – Part B
Chemical
• Reaction completed• Observe what is left
• Identify - COPPER
• Color - REDDISH• Squishy - YES
DAY 2 – Part B
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 a
nd ZnCl2
Zn a
nd Cu
0% 0%0%0%
1. CuCl2 and Cu
2. CuCl2 and ZnCl2
3. Zn and ZnCl2
4. Zn and Cu
CuCl2 + Zn ZnCl2 + Cu
Which is/(are) compounds?
CuCl2
and
Cu
CuCl2
and
ZnCl2
Zn a
nd ZnCl2
Zn a
nd Cu
0% 0%0%0%
1. CuCl2 and Cu
2. CuCl2 and ZnCl2
3. Zn and ZnCl2
4. Zn and Cu
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)
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?
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.
400 BC Democritus
1808 John Dalton:
1869 D. Mendeleev: organizes periodic table
1897 JJ Thompson
1911 Ernest Rutherford
1913 Niels Bohr
1923 Louis de Broglie
1932 James Chadwick
Atomic Theory through Time
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.
•
400 BC Democritus
1808 John Dalton:
1869 D. Mendeleev: organizes periodic table
1897 JJ Thompson
1911 Ernest Rutherford
1913 Niels Bohr
1923 Louis de Broglie
1932 James Chadwick
Atomic Theory through Time
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
• particles – most passed straight through
• Atom mostly empty space !– some scattered at large angles
• Center positively charged nucleus
Rutherford
Niels BohrElectrons 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?
Dal
ton
Chad
wic
k
Ruth
erfo
rd
Bohr
Thom
son
0% 0% 0%0%0%
1. Dalton
2. Chadwick
3. Rutherford
4. Bohr
5. Thomson
Who discovered the electron?
Dal
ton
Chad
wic
k
Ruth
erfo
rd
Bohr
Thom
son
0% 0% 0%0%0%
1. Dalton
2. Chadwick
3. Rutherford
4. Bohr
5. Thomson
Who discovered that atoms are mostly empty space?
Dal
ton
Chad
wic
k
Ruth
erfo
rd
Bohr
Thom
son
0% 0% 0%0%0%
1. Dalton
2. Chadwick
3. Rutherford
4. Bohr
5. Thomson
Who discovered the nucleus?
Dal
ton
Chad
wic
k
Ruth
erfo
rd
Bohr
Thom
son
0% 0% 0%0%0%
1. Dalton
2. Chadwick
3. Rutherford
4. Bohr
5. Thomson
Who discovered the proton in the nucleus?
Dal
ton
Chad
wic
k
Ruth
erfo
rd
Bohr
Thom
son
0% 0% 0%0%0%
1. Dalton
2. Chadwick
3. Rutherford
4. Bohr
5. Thomson
Who discovered the neutron?
Dal
ton
Chad
wic
k
Ruth
erfo
rd
Bohr
Thom
son
0% 0% 0%0%0%
1. Dalton
2. Chadwick
3. Rutherford
4. Bohr
5. Thomson
Who stated that electrons are located in fixed energy levels?
Dal
ton
Chad
wic
k
Ruth
erfo
rd
Bohr
Thom
son
0% 0% 0%0%0%
1. Dalton
2. Chadwick
3. Rutherford
4. Bohr
5. Thomson
C12
6
Mass Number(# protons + # neutrons)
Atomic Number(# protons)
Chemical Symbol
Mass # - Atomic # = neutron #
12 – 6 = 6 neutrons
C14
6
How many protons?
How many electrons?
How many neutrons?
Draw a atomic model for this element?
Li 7
3
How many protons?
How many electrons?
How many neutrons?
Draw a atomic model for this element?
Boron-11number of energy levels?
1 2 3 4 5 6 11
0% 0% 0% 0%0%0%0%
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
7. 11
Boron-11number of electrons in the first
energy level?
1 2 3 4 5 6 11
0% 0% 0% 0%0%0%0%
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
7. 11
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?• # electrons?
• # e’ in 1st orbital?• # e; in 2nd orbital?• # of valence e’ ?
NITROGEN7
7
2
5
5
Electrons / Energy Levels
- closest to nucleus / lowest energy
As electrons FALL BACK to a lower energy level – ENERGY is given off.
Some energy levels can overlap – subdivided into orbitals
• 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
Pro
ton
Neu
tron
Ele
ctro
n
Nucl
eus
Ener
gy le
vels
Mas
s num
ber
Ele
ctro
mag
neti.
..
0% 0% 0% 0%0%0%0%
1. Proton
2. Neutron
3. Electron
4. Nucleus
5. Energy levels
6. Mass number
7. Electromagnetic force
Positively charged particle that exists in the nucleus
of an atom.
Pro
ton
Neu
tron
Ele
ctro
n
Nucl
eus
Ener
gy le
vels
Mas
s num
ber
Eel
ctro
mag
neti.
..
0% 0% 0% 0%0%0%0%
1. Proton
2. Neutron
3. Electron
4. Nucleus
5. Energy levels
6. Mass number
7. Eelctromagnetic force
The least massive of the three subatomic particles which also carries an negative net charge.
Pro
ton
Neu
tron
Ele
ctro
n
Nucl
eus
Ener
gy le
vels
Mas
s num
ber
Ele
ctro
mag
neti.
..
0% 0% 0% 0%0%0%0%
1. Proton
2. Neutron
3. Electron
4. Nucleus
5. Energy levels
6. Mass number
7. Electromagnetic force
Particle with no charge that exists in the nucleus of an atom
Pro
ton
Neu
tron
Ele
ctro
n
Nucl
eus
Ener
gy le
vels
Mas
s num
ber
Ele
ctro
mag
neti.
..
0% 0% 0% 0%0%0%0%
1. Proton
2. Neutron
3. Electron
4. Nucleus
5. Energy levels
6. Mass number
7. Electromagnetic force
Describes how electrons are arranged around an atom
Pro
ton
Neu
tron
Ele
ctro
n
Nucl
eus
Ener
gy le
vels
Mas
s num
ber
Ele
ctro
mag
neti.
..
0% 0% 0% 0%0%0%0%
1. Proton
2. Neutron
3. Electron
4. Nucleus
5. Energy levels
6. Mass number
7. Electromagnetic force
The force that holds the atom together is called
Pro
ton
Neu
tron
Ele
ctro
n
Nucl
eus
Ener
gy le
vels
Mas
s num
ber
Ele
ctro
mag
netic
forc
e
0% 0% 0% 0%0%0%0%
1. Proton
2. Neutron
3. Electron
4. Nucleus
5. Energy levels
6. Mass number
7. Electromagnetic force
The total number of protons and neutrons in the nucleus of an
atom
Pro
ton
Neu
tron
Ele
ctro
n
Nucl
eus
Ener
gy le
vels
Mas
s num
ber
Ele
ctro
mag
neti.
..
0% 0% 0% 0%0%0%0%
1. Proton
2. Neutron
3. Electron
4. Nucleus
5. Energy levels
6. Mass number
7. Electromagnetic force
Fireworks• 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
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)
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 (???)
Key Questions
• What are atoms and how are they put together?
• What does atomic structure have to do with the periodic table?
Subatomic Particles
• The marbles represent these particles. Can you guess which marble represents which particle?
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})
• 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!!!
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 MetalAlkali
EarthMetalMetalloids
Halogen Noble GasNon
Metal
Rare Earth Other-Metal Transition Metal
Orange Light Blue Circle Them
Dark Blue
Green
Dark Orange REDYellow
PurpleRoyal Blue