Download matter - eweb.furman.edu

Lecture I: The Living Planet
I. Formation of the Solar System
The Earth, from 6 billion kilometers, taken by the
Voyager 1 space probe on Feb 14, 1990, as it leaves
our solar system.
Planets
“Dwarf” planets (smaller than the Moon)
Body
Diameter
SUN
12 inches
Distance
Mercury 0.04 in
41 feet
Venus
0.10 in
77 feet
Earth
0.11 in
107 feet
Mars
0.06 in
163 feet
Asteriod belt……………………………………….
Jupiter
1.23 in
559 feet
Saturn
1.00 in
1025 feet
Uranus
0.40 in
2062 feet
Neptune 0.39 in
3232 feet
Pluto
4248 feet
0.02 in
Lecture I: The Living Planet
II. The Earth and its Neighbors
A. Size and Temps
-153 – 20oC
-88 – 58oC
462oC
Lecture I: The Living Planet
II. The Earth and Its Neighbors
A. Size and Temps
B. Atmospheric Composition
CO2
N2
H2O
Ar
O2
Earth
0.035%
77%
1%
0.93%
21%
Venus
96%
3.5%
0.01%
0.007%
trace
Mars
95%
2.7%
0.007%
1.6%
trace
Lecture I: The Living Planet
II. The Earth and Its Neighbors
III. Why The Differences?
A. The Effects of Liquid Water
About 4.4 bya, the period of
heavy asteroid bombardment
ended, and water could collect
at the surface without being
vaporized by meteorite
impacts.
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
Chemistry basics:
1. Atoms and subatomic particles
2. Molecules and covalent bonds
3. Polar covalent bonds
Spatial Scales:
Earth is ~4 x 107 m in circumference
Smallest Mammal - Pygmy Shrew: 2 inches (5 x 10-2 m)
Largest Animal Ever - Blue Whale: 100 feet (3 x 101 m)
Human - 6 ft... 2 x 100 m
1.
Individual:
2.
3.
Organs: variable
Cells:
Liver Cell: 2 x 10-5 m (2/100ths of a mm)
E. coli Bacterium: 2 x 10-6 (1/10th of a liver cell)
Virus: 2.5 x 10-8 (1/100th of a bacterium)
Organelles:
Ribosome: 1.8 x 10-8 m
Mitochondrion: 2.5 x 10-6 m (about bacteria sized)
Molecules:
Hemoglobin (average protein): 6.8 x 10-9 m (1/1000th of a bact.)
Phospholipid: 3.5 x 10-9 m
Amino Acid: 5.0 x 10-10 m
Atoms:
Carbon: 1 x 10-10 m (1/10,000,000,000 m - a ten billionth of a meter)
(a ten millionth of a millimeter)
(a ten thousandth the length of a liver cell)
Nucleus:
2 x 10-15 m. 5 orders of magnitude smaller than the width of the atom!!!
4.
5.
6.
7.
So, the nucleus is only 1/50,000th the width of the atom.
Atoms are mostly space… matter is mostly space…
In fact, a cubic centimeter of nuclear matter (no space) would weigh 230
million tons (Physics by J. Orear, 1979)
Analogy: If a basketball 1 ft. in diameter represents the nucleus of an atom,
the edge of the electron cloud would be about 5 miles away in either
direction; the atom would be 10 miles wide (~ 50,000 ft.)… that’s a lot
of empty space.
Analogy: You and the Earth are separated by 7 orders of linear magnitude.
A millimeter (about the size of a bold-faced period) and a carbon atom
are separated by 7 orders of linear magnitude. So, to a carbon atom,
the period is it's Earth.... mind blowing...
B. Temporal Scales:
1. Age of Earth: 4.5 x 109 yrs (4.5 billion)
2. History of Life on Earth: 3.5 x 109 years
3. Oldest Eukaryotic Cells: 1.8 x 109 years
4. Oldest Multicellular Animals: 6.1 x 108 years
5. Oldest Vertebrates: 5.0 x 108 (500 million)
6. Oldest Land Vertebrates: 3.6 x 108
7. Age of Dinosaurs - Mesozoic: 240-65 million
8. Oldest Primates: 2.5 x 107 (25 million)
9. Oldest Hominids: 4.0 x 106 (4 million – 1/1000th of earth history)
10. Oldest Homo sapiens: 2.0 x 105 (200,000)
11. Oldest Art: 3.0 x 104 (30,000; 1/100,000th of Life's History)
12. Oldest Agriculture: 1.0 x 104 (10,000)
13. Oldest Organism: Bristlecone pines: 5 x 103
14. Human cell:
brain/muscle 70 yrs
Red Blood Cell - weeks
Skin cell – days
15. Supply of ATP in cell - 2 seconds
16. Rates of chemical reactions - milliseconds (3.1 x 10-10 ms/year).
The history of life, spanning billions of years, is dependent on reactions that occur at
a temporal scale separated by 19 orders of temporal magnitude.
Atoms and Bonds
I. Atoms
A. Matter
1. Elements are different forms of matter which have different chemical and
physical properties, and can not be broken down further by chemical reactions.
2. The smallest unit of an element that retains the properties of that element is
an atom.
3. Atoms are composed of protons and neutrons in the nucleus, orbited by
electrons:
Proton: in nucleus; mass = 1, charge = +1 - Defines Element
Neutron: in nucleus; mass = 1, charge = 0
Electron: orbits nucleus; mass ~ 0, charge = -1
Atoms and Bonds
I. Atoms
A. Matter
B. Properties of Atoms
1. Subatomic Particles
Proton: in nucleus; mass = 1, charge = +1 - Defines Element
Neutron: in nucleus; mass = 1, charge = 0
Electron: orbits nucleus; mass ~ 0, charge = -1
Orbit at quantum distances (shells)
Shells 1, 2, and 3 have 1, 4, and 4 orbits (2 electrons each)
Shells hold 2, 8, 8 electrons = distance related to energy
Neon (Bohr model)
Atoms and Bonds
I. Atoms
A. Matter
B. Properties of Atoms
1. Subatomic Particles
2. Mass = protons + neutrons
8
O
15.99
Atoms and Bonds
I. Atoms
A. Matter
B. Properties of Atoms
1. Subatomic Particles
2. Mass = protons + neutrons
3. Charge = (# protons) - (# electrons)...
If charge = 0, then you have an ...ION
Atoms and Bonds
I. Atoms
A. Matter
B. Properties of Atoms
4. Isotopes -
Atoms and Bonds
I. Atoms
A. Matter
B. Properties of Atoms
4. Isotopes - 'extra' neutrons... heavier
Some are stable
Some are not... they 'decay' - lose the neutron
These 'radioisotopes' emit energy (radiation)
Atoms and Bonds
I. Atoms
A. Matter
B. Properties of Atoms
4. Isotopes - 'extra' neutrons... heavier
Some are stable
Some are not... they 'decay' - lose the neutron
These 'radioisotopes' emit energy (radiation)
This process is not affected by environmental conditions and is
constant; so if we know the amount of parent and daughter isotope, and we know
the decay rate, we can calculate the time it has taken for this much daughter
isotope to be produced.
Atoms and Bonds
I. Atoms
A. Matter
B. Properties of Atoms
4. Isotopes - 'extra' neutrons... heavier
Gamma decay - neutron emits energy as a photon - no change in
neutron number, mass, or element.
Alpha decay - loss of an alpha particle (2 protons and 2 neutrons) from
the nucleus. This changes the mass and element.
(Uranium with 92 protons decays to Thorium with 90 protons)
Beta decay - a neutron changes to a proton, and an electron is emitted.
This changes only the element (determined by the number of protons), but not the
mass.
(C14 decays, neutron changes to proton, and N14 is produced)
Lecture I: The Living Planet
I.
II.
The Earth and Its Neighbors
Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is called the “universal solvent”
- ions and polar compounds dissolve in water
Charged regions of a glucose
molecule
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is known as the “universal solvent”
Chlorine (Cl): 17P, 17eChemistry basics:
1. Atoms and subatomic particles
2. Molecules and covalent bonds
3. Polar covalent bonds
4. Ionic bonds and compounds
- transfer creates atoms with unequal
number of protons and electrons.
These are “ions” Cl-, Na+
Sodium (Na): 11P, 11e
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is called the “universal solvent”
- ions and polar compounds dissolve in water
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is called the “universal solvent”
- ions and polar compounds dissolve in water
- Rocks are composed of ionic compounds (minerals)
- So many rocks dissolve
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is called the “universal solvent”
3. Water dissociates
Hydronium:
Oxygen: 8 protons, 2e first shell, 8 second
3 H:
3 protons
Total:
11 protons, 10 electrons = +1 charge
(will readily give up H+ ion
Hydronium can give up an H+, so
same net effect as above…
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is called the “universal solvent”
3. Water dissociates
Chemistry basics:
1. Atoms and subatomic particles
2. Molecules and covalent bonds
3. Polar covalent bonds
4. Ionic bonds and compounds
- transfer creates atoms with unequal
number of protons and electrons.
These are “ions” Cl-, Na+
5. pH, acids, and bases
In pure water, 1 in 10,000,000 (1 x 10-7) molecules
will be dissociated at any one time
The “power” (in terms of exponent) of Hydrogen…
you can think of it as percent or proportion of H+.
pH scale is negative exponent… so water = 7.0
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
17+
1+
1. Water’s molecular structure
2. Water is called the “universal solvent”
3. Water dissociates
Chemistry basics:
1. Atoms and subatomic particles
2. Molecules and covalent bonds
3. Polar covalent bonds
4. Ionic bonds and compounds
- transfer creates atoms with unequal
number of protons and electrons.
These are “ions” Cl-, Na+
5. pH, acids, and bases
HCl (Hydrochloric acid) dissociates much more
readily in solution.
1 in 100 molecules are dissociated = 1 x 10-2
pH = 2.0
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is called the “universal solvent”
3. Water dissociates
Chemistry basics:
1. Atoms and subatomic particles
2. Molecules and covalent bonds
3. Polar covalent bonds
4. Ionic bonds and compounds
- transfer creates atoms with unequal
number of protons and electrons.
These are “ions” Cl-, Na+
5. pH, acids, and bases
CATION DISPLACEMENT
Feldspar Minerals (60%)
K-Al-Si3O8
Na-Al-Si3O8
Ca-Al-Si2O8
In presence of water, H+
replaces K+, Na+, and CA+2
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
1. Water’s molecular structure
2. Water is called the “universal solvent”
3. Water dissociates
4. Carbon dioxide reacts with water to form carbonic acid
Abiogenic Limestone Formation
Bicarbonate ion
Carbonic acid
Carbonate ion
Calcium Carbonate (limestone)
Abiogenic Limestone Formation
Earth
CO2
0.035%
Venus
96%
Mars
Bicarbonate ion
95%
Carbonic acid
Carbonate ion
Calcium Carbonate (limestone)
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
B. Tectonic Activity and Subduction
Limestone
Lecture I: The Living Planet
Coccolithophore
(single celled marine algae)
III. Why The Differences?
A. The Effects of Liquid Water
B. Tectonic Activity and Subduction
C. The Effects of LIFE
1. Biogenic Limestone Formation
“Coquina”
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
B. Tectonic Activity and Subduction
C. The Effects of LIFE
1. Biogenic Limestone Formation
SHELLS
Settled out
400 m
4 um (4/1000’s of a mm; 250,000 per meter)
100,000,000 deep, but they are
crushed, so it’s actually more…
400 m
4 um (4/1000’s of a mm; 250,000 per meter)
100,000,000 deep, but they are
crushed, so it’s actually more…
Little things, big effects…
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
B. Tectonic Activity and Subduction
C. The Effects of LIFE
1. Biogenic Limestone Formation
2. Photosynthesis
Photosynthetic bacteria
Overview:
A. Step One: Transferring radiant energy to chemical energy
eEnergy of photon
Transferred to
an electron
e-
Overview:
A. Step Two: storing that chemical energy in the bonds of molecules
eATP
e-
ADP
+P
Light Dependent
Reaction
Electron becomes trapped in a chemical bond
(phosphate bond) between PO4 and ADP
Overview:
A. Step Two: storing that chemical energy in the bonds of molecules
eATP
eLight Dependent
Reaction
Where do the electrons come from?
ADP
+P
Overview:
A. Step Two: storing that chemical energy in the bonds of molecules
eATP
ADP
+P
eLight Dependent
Reaction
Where do the electrons come from?
Photosynthetic organisms split WATER:
to harvest electrons
2 (H-O-H)
2O + 4H+ + 4eO2
Overview:
A. Step Two: storing that chemical energy in the bonds of molecules
eATP
ADP
+P
e-
BUT… P~P bonds are weak. To
“store” this energy, stronger,
more stable bonds need to be
made.
ATP bonds are broken and C-C
bonds are made.
Light Dependent
Reaction
Where do the electrons come from?
Photosynthetic organisms split WATER:
2 (H-O-H)
2O + 4H+ + 4eO2
Overview:
A. Step Two: storing that chemical energy in the bonds of molecules
e-
C6 (glucose)
ATP
ADP
+P
eLight Dependent
Reaction
6 CO2
Light Independent
Reaction
Where do the electrons come from?
Photosynthetic organisms split WATER:
2 (H-O-H)
2O + 4H+ + 4eO2
Lecture I: The Living Planet
III. Why The Differences?
A. The Effects of Liquid Water
B. Tectonic Activity and Subduction
C. The Effects of LIFE
1. Biogenic Limestone Formation
2. Photosynthesis
Little things (photosynthetic bacteria), big effects…
CO2
N2
H2O
Ar
O2
Earth
Venus
Mars
0.035%
77%
1%
0.93%
96%
3.5%
0.01%
0.007%
95%
2.7%
0.007%
1.6%
trace
trace
21%
Where did all the CO2 go?
The atmosphere is no longer a major
“reservoir” for carbon on our planet.
Where did all the CO2 go?
The atmosphere is no longer a major
“reservoir” for carbon on our planet.
Most has been transferred to the
lithosphere by limestone formation
Where did all the CO2 go?
The atmosphere is no longer a major
“reservoir” for carbon on our planet.
Most has been transferred to the
lithosphere by limestone formation
And there is nearly as much carbon
In living terrestrial biomass as in the
atmosphere
Where did all the CO2 go?
The atmosphere is no longer a major
“reservoir” for carbon on our planet.
Most has been transferred to the
lithosphere by limestone formation
And there is nearly as much carbon
In living terrestrial biomass as in the
atmosphere
More in the entire biosphere, including
decomposing material in soils and marine
life
How do we know that oxygen wasn’t always present in the Earth’s atmosphere?
Maybe Earth is just different from Venus and Mars…
Banded iron formations are first seen 2.5 billion years ago, showing that oxygen must have been
present in the ocean to precipitate iron out of solution as iron oxides in sedimentary strata. There
absence in older strata means that oxygen was not present in appreciable amounts.
The Carboniferous “Pulse”
1. Terrestrial plants were radiating, sucking up CO2 and producing O2.
2. Huge expanses of swamp forests dominated the equatorial zone. Photosynthetic rates were high, but the trees
were preserved under sediments when they died and fell…. Creating our coal deposits. Photosynthesis
produced lots of O2, but with less decay, it stayed in the air instead of being breathed in and used by
decomposing bacteria.
The K-T Extinction affected atmospheric
oxygen levels as plants went extinct and
terrestrial photosynthetic activity declined.
And today?
The Earth is a living planet… it
breathes…
21% = 210,000,000 ppm,
So a decline of 70 ppm is not dramatic.