Basic chemistry○ Atomic structure

Nucleus = protons (positive) + neutrons (neutral)

http://www.rstp.uwaterloo.ca/manual/matter/graphic/atom.jpg

Electrons (negative charge)

Chemical bonds Attractive force that holds atoms together Three major types

○ Ionic bonds ○ Covalent bonds○ Hydrogen bonds

http://serc.carleton.edu/images/usingdata/nasaimages

○ Ionic bonds – weak bonds Atoms “exchange” electrons fill outer shell

- becomes positive ion if lose electron - becomes negative ion if gain electron - + & – ions attracted to each other

Na & Cl Na+ + Cl-

http://www.physicalgeography.net/fundamentals/images http://www.msnucleus.org/

membership/html/k-6/rc/minerals/3

Covalent bonds – strong bonds Atoms “share” electrons to fill outer shell H (hydrogen) has one electron, needs 1 more O (oxygen) has 6 electrons in outer shell, needs two

electrons Therefore, oxygen and 2 hydrogens bond to form water

Covalent bonds are stronger because there is sharing of the electrons

http://ghs.gresham.k12.or.us/science/ps/sci/ibbio/chem/notes/chpt2

http://www.theochem.ruhr-uni-bochum.de/~axel.kohlmeyer/cpmd-vmd

Polarity of covalent bonds○ Nonpolar covalent – electrons are shared

equally ○ Polar covalent - electrons not equally

distributed in molecule○ Water is a dipolar molecule (two polar covalent

bonds)

O strongly attracts electrons slightly negative

H slightly positive- Think of oxygen as being the “bully” – it’s larger so it pulls the

electrons towards it’s nucleus more often

○ Allows formation of H-bonding between water molecules

H2O molecule One hydrogen H and two oxygen O

atoms bonded by sharing electrons Both H atoms on same side of O atom Dipolar covalent bondDipolar covalent bond

Hydrogen bonding Polarity

small negative charge at O end

small positive charge at H end

Attraction between + and – ends of water molecules to each other or other ions

Happens because of the polar covalent bond

Fig. 5.3

Hydrogen bonding and water Hydrogen bonds are

weaker than covalent bonds but still strong enough to result in unique properties of water Cohesion = sticks to

other water molecules Adhesion = sticks to

other types of molecules High surface tension

http://faculty.uca.edu/~benw/biol1400

http://ucsu.colorado.edu/~meiercl/photography

Hydrogen bonding and waterH-bonds absorb red

light, reflect blue light blue color

High solubility of chemical compounds in water

Solid, liquid, gas at Earth’s surface

Unusual thermal properties

Unusual density

http://www.pacific-promotion.com.fr/Phototek

Unusual thermal properties of H2O H2O has high boiling

point H2O has high freezing

point

Most H2O is in liquid form of water on Earth’s surface VERY important for life

http://www.magnet.fsu.edu/education/tutorials/magnetacademy/superconductivity101/images/superconductivity-temperature.jpg

Fig. 5.6

Unusual thermal properties of H2O

Water high heat capacity (specific heat capacity (specific heat)heat)Amount of heat required to raise

temperature of 1 gram of any substance 1o C

Water can take in/lose lots of heat without changing temperature – must break H-bonds

On the other hand, rocks have low heat capacity○ Rocks quickly change temperature as they

gain/lose heat

Global thermostatic effects Moderates temperature on Earth’s

surface – water temp less variable and less extreme than air temperaturesEquatorial oceans (hot) don’t boilPolar oceans (cold) don’t freeze solid

Global thermostatic effects Marine effectMarine effect

Oceans moderate temperature changes day/night; different seasons

Continental effectContinental effectLand areas have greater range of temperatures

day/night and during different seasons

Look at the differences between coastal Florida compared to Orlando

Density of water Density of water

increases as temperature decreases down to 4oC

From 4oC to 0oC density of water decreases as temperature decreases

Density of ice is less than density of water http://www.grow.arizona.edu/img/water

Density of water

Fig. 5.10

Density of water Dissolved solids reduce

freezing point of waterAs water freezes, the

crystalline structure “pushes out” much of the dissolved solids

Creates icy “slush” and surrounding waters become saltier

Putting salt on icy roads melts ice○ Salt lowers freezing point

of water on roads allowing it to remain liquid at colder temps

http://www.ibarron.net/users/robert/pics/2003/Norway/OsloFjord11.jpg

Water = Life• Summary:

• Unique properties of water that make life possible• High heat capacity and specific heat

• Moderates climates• Keeps equatorial regions from boiling and pole regions from

freezing solid• High latent heat – when undergoing change of state, large amount

of heat is absorbed or released• Sweat evaporating from your skin draws heat from your body,

keep you cool• Ice is less dense than liquid water• Cohesion

• Water moving up xylem in plants• Surface tension – allows plankton to stay near surface of water

Salinity Six elements make up

99% of dissolved solids in seawater – from erosion of land, volcanism

Total amount of solid material dissolved in water- Traditional definition

Typical salinity is 3.5% or 35o/oo o/oo or parts per thousand (ppt) =

grams of salt per kilogram of water (g/Kg )

Adding salts changes many properties of water

Fig. 5.12

Pure water vs. seawater

Salinity variations

Open ocean salinity 33 to 38 o/oo However, coastal areas salinity varies

more widelyInflux of freshwater lowers salinity or creates

brackishbrackish conditionsGreater rate of evaporation raises salinity or

creates hypersalinehypersaline conditions Salinity may vary with seasons (dry/rain)

Deep ocean variation of salinity

Surface ocean salinity is variable

○ Due to occurrences at surface – rain, evaporation, etc

Deeper ocean salinity is nearly the same (polar source regions for deeper ocean water)

HaloclineHalocline, rapid change of salinity with depth

pH – Acidity and alkalinity Acid releases H+ when

dissolved in water (HCl, H2SO4)

Alkaline (or base) releases OH- (NaOH)

pH scale measures the hydrogen ion concentrationLow pH value, acidHigh pH value, alkaline (basic)pH 7 = neutral

http://www3.oes.edu/ms/science6/Pictures%20of%20Science%20Concepts/pH%20Scale.gif

Figure 5.17

Oceans absorb carbon dioxide from the atmosphere○ How do humans put excess CO2 in atmosphere?

CO2 reacts with seawater to form carbonic acidReleases H+ , decreasing pH

The additional H+ bind to carbonate ions to form bicarbonate

○ Less carbonate in the water makes it difficult for corals, mollusks, echinoderms, calcareous algae, etc. to form calcium carbonate

Ocean Acidification

Ocean water is basic – pH ~8.1○ Surface waters have already absorbed

enough CO2 to experience a pH decrease of 0.1 since pre-industrial times

- May not seem like a lot but remember that pH is measured on a logarithmic scale so that represents a 30% drop in a relatively short time period

Density of seawater 1.022 to 1.030 g/cm3 surface seawater Saltwater more dense than pure water

That is why you can float better in saltwater

Ocean layered according to density Density seawater controlled by

temperature, salinity, and pressureMost important influence is temperatureDensity increases with decreasing

temperature

Density of seawater Overall, temp has greatest

effect on density However, salinity greatest

influence on density in polar oceans polar ocean is isothermal

(same temperature as depth increases)

Currents from lower latitudes bring higher salinity water into polar areas

But polar waters are overall isothermal AND isopycnal

http://www.waterencyclopedia.com/images/wsci_03_img0394.jpg

Density versus depth

PycnoclinePycnocline, abrupt change of density with depth

ThermoclineThermocline, abrupt change of temperature with depth

Density differences cause a layered ocean

Mixed surface water Pycnocline and thermocline Deep water

Misconceptions Increases in global temperatures in the

atmosphere and the consequent warming of the oceans will only create a problem for people living along the coast.

Water exists in the ground in actual rivers or lakes that are constantly renewed.

People drink bottle water because it is better for our health; the safety of tap water is below consumption standards.

Ocean Literacy Principles 1e - Most of Earth’s water (97%) is in the ocean. Seawater has unique properties: it is saline, its

freezing point is slightly lower than fresh water, its density is slightly higher, its electrical conductivity is much higher, and it is slightly basic. The salt in seawater comes from eroding land, volcanic emissions, reactions at the seafloor, and atmospheric deposition.

1g - The ocean is connected to major lakes, watersheds and waterways because all major watersheds on Earth drain to the ocean. Rivers and streams transport nutrients, salts, sediments and pollutants from watersheds to estuaries and to the ocean.

3a - The ocean controls weather and climate by dominating the Earth’s energy, water and carbon systems.

Sunshine State Standards SC.6.E.7.1 Differentiate among radiation, conduction, and convection, the three mechanisms by

which heat is transferred through Earth's system. SC.6.E.7.6 Differentiate between weather and climate. SC.8.P.8.1 Explore the scientific theory of atoms (also known as atomic theory) by using models to

explain the motion of particles in solids, liquids, and gases. SC.8.P.8.4 Classify and compare substances on the basis of characteristic physical properties that

can be demonstrated or measured; for example, density, thermal or electrical conductivity, solubility, magnetic properties, melting and boiling points, and know that these properties are independent of the amount of the sample.

SC.8.P.8.6 Recognize that elements are grouped in the periodic table according to similarities of their properties.

SC.8.P.8.8 Identify basic examples of and compare and classify the properties of compounds, including acids, bases, and salts.

SC.912.E.7.9 Cite evidence that the ocean has had a significant influence on climate change by absorbing, storing, and moving heat, carbon, and water.

SC.912.P.8.4 Explore the scientific theory of atoms (also known as atomic theory) by describing the structure of atoms in terms of protons, neutrons and electrons, and differentiate among these particles in terms of their mass, electrical charges and locations within the atom

SC.912.P.8.5 Relate properties of atoms and their position in the periodic table to the arrangement of their electrons.