seawater chemistry 003. pure substances that cannot be broken down into simpler chemical entities by...
Post on 22-Dec-2015
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Pure substances that cannot be broken down into simpler chemical entities by ordinary chemical reactions.
Pure substances that cannot be broken down into simpler chemical entities by ordinary chemical reactions.
ElementsElements
Periodic Table 112 known elements
An element is composed of atoms (0.1-1 nm in diameter)
Atom cluster of small particles (proton, neutron, electron)
Protons (p +)
Neutrons (n o)
Electrons (e -)
atomic mass (atomic wt.): sum of masses of p+nHe 2p + 2n, atomic mass = 4
4
2He
He
p + n e-
O16 O17 O18
stable isotopes
IsotopeIsotopeatoms that differ in the number of neutrons
16
8 O
18
8 O17
8 O#p
#p+n
O
Major Elements Comprising the Biological Molecules of
Living Things
Major Elements Comprising the Biological Molecules of
Living Things
• CCarbonarbon• HHydrogenydrogen• OOxygenxygen• NNitrogenitrogen• PPhosphorushosphorus• SSulfurulfur
Other Major Elements of Living Things
Other Major Elements of Living Things
• Calcium (Ca)Calcium (Ca)• Potassium (K)Potassium (K)• Chlorine (Cl)Chlorine (Cl)• Magnesium (Mg)Magnesium (Mg)
Some Important Trace Elements of Living Things
Some Important Trace Elements of Living Things
• Boron (B)Boron (B)• Cobalt (Co)Cobalt (Co)• Iron (Fe)Iron (Fe)• Copper (Cu)Copper (Cu)• Fluorine (F)Fluorine (F)• Zinc (Zn)Zinc (Zn)
MoleculeTwo or more atoms held
together by chemical bondsOxygenOxygen OO2 2
NitrogenNitrogen NN22
AmmoniaAmmonia NHNH33
Carbon DioxideCarbon Dioxide COCO22
WaterWater HH22OO
MethaneMethane CHCH44
GlucoseGlucose CC66HH1212OO66
• Carbohydrates: C6H12O6 (glucose)
• Lipids: C3H8O3 (glycerol) + 3C16H32O2 (fatty acids)
• Proteins: COOH-NH2
• Nucleic Acids: sugar, PO4, N2 containing base
Organic Molecules
• Hydrogen H+
• Potassium K+
• Fluoride F-
• Calcium Ca+2
• Magnesium Mg+2
• HydroxideHydroxide OHOH--
• BicarbonateBicarbonate HCOHCO33--
• NitrateNitrate NONO33--
• PhosphatePhosphate POPO44-3-3
Between Water Molecules
Covalent bond
Hydrogen bond
Boiling Point: 100oCFreezing Point: 0oCDensity: 1g/cm3
Properties of WaterProperties of Water
gas liquid solid
The formation of ice• As water cools to
4°C:– Molecules slow– Water contracts– Density increases
• Below 4°C:– Hydrogen bonds form– Water expands
• As water freezes:– Expands by 9%
Properties of WaterProperties of Water
1.High heat capacity
2.High heat of vaporization
3.High Surface tension
4.Polarity solvent properties
The ocean moderates coastal temperatures
• Water has high heat capacity, so it can absorb (or release) large quantities of heat without changing temperature
• Moderates coastal temperatures
The ocean moderates coastal temperatures
Hawaii Average High and Low Temperature
Hawaii Average Ocean Water Temperature
Interconnections of water molecules
• Polarity causes water molecules to form weak (hydrogen) bonds between water molecules
• Water sticks to itself and to other substances
• Allows water to be the universal solvent
Water as a solvent
• Water dissolves table salt (NaCl) by attracting oppositely charged particles
• Pulls particles out of NaCl structure to dissolve it
Water in the 3 states of matter• Latent (hidden) heat = energy that is either
absorbed or released as water changes state
Properties of SeawaterProperties of Seawater
Heat capacity: • Heat capacity with salinity
Evaporation:• Evaporates more slowly than fw
Specific gravity:• Pure water density = 1.000 g/cm3
• Seawater (2 oC) density = 1.028 g/cm3
Seawater’s Boiling Point:
• As salinity , the boiling point
Seawater’s Freezing Point:
• As salinity , the freezing point
• Salt is an antifreeze- doesn’t freeze until -2oC (@35 o/oo)
Lattice structure of an ice crystal
Sea ice (pancake ice)
Salt Ion Ions in sw (0/00)Cl- 18.980Na+ 10.556SO4
2- 2.649Mg2+ 1.272Ca2+ 0.400K+ 0.380HCO3- 0.140Br- 0.065H3BO3 0.026Sr2+ 0.013F- 0.001 Total 34.38
• Na+ - Weathering of crustal rock
• Cl- - from the mantle by way of volcanic vents and outgassing from mid-ocean rifts
• Mg ++ - mid ocean rifts
White sections represent warm surface currents. Purple sections represent deep cold currents
Bases
Na+ + OH- NaOHNH3 + H+ NH4
OH - + H+ H2O
HCO3 +H+ H2CO3
Proton acceptor, i.e., they take up H+ ions
NaOH is a strong base ~pH 12
NeutralizationHCl + NaOH H2O + NaCl
BasesBases
Na+ + OH- NaOHNH3 + H+ NH4
OH - + H+ H2O
HCO3- +H+ H2CO3
Proton acceptor, i.e., they take up H+ ions
NaOH is a strong base ~pH 12
Neutralization- HCl + NaOH H2O + NaCl
Buffer- resists dramatic changes in pH; ex. tums, rolaids…buffers stomach acid
Neutralization & BuffersNeutralization & Buffers
Dep
th (
m)
Concentration of dissolved gas (ppm)
0
500
1000
1500
2000O2
CO2
90 94 98 102 106 110
1.5 3.0 4.5 6.0 7.5
CO2O2
O2 and CO2 vs ocean depth
Compensation depth
Carbon Dioxide System in the OceanCarbon Dioxide System in the Ocean
Respiration
Photosynthesis
C6H12O6 +6O2 6CO2 + 6H2O
6CO2 + 6H2O C6H12O6 +6O2
Air
Water
CO2 gas
CO2 + H2O ↔ H2CO3 ↔ HCO3- + H + ↔ CO3
2- + 2H+
By-product of respiration
carbonic acidbicarbonate
carbonate
The addition of CO2 makes water acidic
The effects of pH in an ocean systemThe effects of pH in an ocean system
Carbonate bufferCarbonate buffer
Seawater too basic:
H2CO3 HCO3- + H + pH drops
Seawater too acidic:
HCO3- + H + H2CO3 pH rises
Consequences of Ocean Acidity
Animals with CaCO3 skeletons affected• Plankton• Corals• Mollusks • Fish
http://news.bbc.co.uk/2/hi/science/nature/7933589.stm
Fisheries
In a high CO2 world, the ocean will be…
• More acidic• More stratified• More oligotrophic, but better light conditions • Less oxygenated
Consequences of Ocean Acidity
Inquiry
1. How many neutrons in 7 N?2. Why do all the oceans have relatively the same
proportion of salinity?3. At what temperature is fw most dense?4. Of the following pH’s which is most acidic? 3 7 6 25. Why are there no plants at the compensation depth?6. Why can a water strider walk on water?7. Besides temperature and salinity, what physical factor
effects thermohaline circulation?8. What is the oceans most dense sea water called?
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