Biology Properties of Water
Dec 31, 2015
Biology
Properties of Water
Matter consists of chemical elements in pure form and in combinations called compounds
• Organisms are composed of matter• Matter is anything that takes up space and has
mass
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Matter is made up of elements An element is a substance that cannot be broken down to other substances by chemical reactionsA compound is a substance consisting of two or more elements in a fixed ratioA compound has characteristics different from those of its elements
Table 2-1
Fig. 2-UN3
Nucleus
Protons (+ charge)determine element
Neutrons (no charge)determine isotope Atom
Electrons (– charge) form negative cloudand determinechemical behavior
Fig. 2-UN6
Ionic bond
Electrontransferforms ions
NaSodium atom
ClChlorine atom
Na+
Sodium ion(a cation)
Cl–
Chloride ion(an anion)
Fig. 2-9
Hydrogen
1H
Lithium
3LiBeryllium
4BeBoron
5BCarbon
6CNitrogen
7NOxygen
8O
Fluorine
9FNeon
10Ne
Helium
2HeAtomic number
Element symbol
Electron-distributiondiagram
Atomic mass
2He
4.00Firstshell
Secondshell
Thirdshell
Sodium
11NaMagnesium
12Mg
Aluminum
13AlSilicon
14SiPhosphorus
15PSulfur
16S
Chlorine
17ClArgon
18Ar
Electron-distributiondiagram
(a)
(b) Separate electronorbitals
Neon, with two filled shells (10 electrons)
First shell Second shell
1s orbital 2s orbital Three 2p orbitals
(c) Superimposed electronorbitals
1s, 2s, and 2p orbitals
x y
z
Fig. 2-10-4
Hydrogen Bonds
• A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom
• In living cells, the electronegative partners are usually oxygen or nitrogen atoms
Copyright © 2008 Pearson Education, Inc., publishing as Benjamin Cummings
Fig. 2-16
+
+
+
+
+
Water (H2O)
Ammonia (NH3)
Hydrogen bond
Overview: The Molecule That Supports All of Life
• Water is the biological medium on Earth
• All living organisms require water more than any other substance
• Most cells are surrounded by water, and cells themselves are about 70–95% water
• The abundance of water is the main reason the Earth is habitable
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
The polarity of water molecules results in hydrogen bonding
• The water molecule is a polar molecule: The opposite ends have opposite charges
• Polarity allows water molecules to form hydrogen bonds with each other
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
Fig. 3-2
Hydrogenbond
–H
+
H
O
——
——
+
+
+
–
–
–
Four emergent properties of water contribute to Earth’s fitness for life
• Four of water’s properties that facilitate an environment for life are:
– Cohesive behavior– Ability to moderate temperature– Expansion upon freezing– Versatility as a solvent
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
Cohesion
• Collectively, hydrogen bonds hold water molecules together, a phenomenon called cohesion
• Cohesion helps the transport of water against gravity in plants
• Adhesion is an attraction between different substances, for example, between water and plant cell walls
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
Fig. 3-3
Water-conductingcells
Adhesion
Cohesion
150 µm
Directionof watermovement
• Surface tension is a measure of how hard it is to break the surface of a liquid
• Surface tension is related to cohesion
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
Fig. 3-4
Water’s High Specific Heat
• The specific heat of a substance is the amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1ºC
• The specific heat of water is 1 cal/g/ºC
• Water resists changing its temperature because of its high specific heat
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
Insulation of Bodies of Water by Floating Ice
• Ice floats in liquid water because hydrogen bonds in ice are more “ordered,” making ice less dense
• Water reaches its greatest density at 4°C• If ice sank, all bodies of water would eventually
freeze solid, making life impossible on Earth
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
20
Heat Capacity• Water has a high heat capacity
Temperature = rate of vibration of molecules Apply heat to liquid
Molecules bounce faster Increases temperature
But, when heat applied to water Hydrogen bonds restrain bouncing Temperature rises more slowly per unit heat Water at a given temp. has more heat than most liquids
• Thermal inertia – resistance to temperature change More heat required to raise water one degree than most other liquids (1 calorie
per gram) Also, more heat is extracted/released when lowering water one degree than most
other liquids
21
Properties of Water:Heat of Vaporization
• High heat of vaporization
To raise water from 98 to 99 ºC; ~1 calorie
To raise water from 99 to 100 ºC; ~1 calorie
However, large numbers of hydrogen bonds must be broken to evaporate water
To raise water from 100 to 101 ºC; ~540 calories!
• This is why sweating (and panting) cools
Evaporative cooling is best when humidity is low because evaporation occurs rapidly
Evaporative cooling works poorest when humidity is high because evaporation occurs slowly
22
Evaporative Cooling
of Animals
23
Heat of Fusion
• Heat of fusion (melting)
– To raise ice from -2 to -1 ºC; ~1 calorie
– To raise water from -1 to 0 ºC; ~1 calorie
– To raise water from 0 to 1 ºC; ~80 calories!
• This is why ice at 0 ºC keeps stuff cold MUCH longer than water at 1 ºC
• This is why ice is used for cooling
– NOT because ice is cold
– But because it absorbs so much heat before it will warm by one degree
24
Heat Content of Water
at Various Temperatures
25
Properties of Water:Uniqueness of Ice
• Frozen water less dense than liquid water
Otherwise, oceans and deep lakes would fill with ice from the bottom up
Ice acts as an insulator on top of a frozen body of water
Melting ice draws heat from the environment
26
A Pond in Winter
27
Density of Waterat Various Temperatures
Fig. 3-6a
Hydrogenbond
Liquid waterHydrogen bonds break and re-form
IceHydrogen bonds are stable
Hydrophilic and Hydrophobic Substances
• A hydrophilic substance is one that has an affinity for water
• A hydrophobic substance is one that does not have an affinity for water
• Oil molecules are hydrophobic because they have relatively nonpolar bonds
• A colloid is a stable suspension of fine particles in a liquid
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings
Basic ChemistryBasic Chemistry 30Properties of Water:Properties of Water:Water as a SolventWater as a Solvent
Solutions consist of:Solutions consist of: A A solventsolvent (the most abundant part) and (the most abundant part) and A A solutesolute (less abundant part) that is dissolved in (less abundant part) that is dissolved in the solventthe solvent
Polar compounds readily dissolve; Polar compounds readily dissolve; hydrophilichydrophilicNonpolar compounds dissolve only slightly; Nonpolar compounds dissolve only slightly;
hydrophobichydrophobicIonic compounds dissociate in waterIonic compounds dissociate in water
NaNa++
Attracted to negative (O) end of HAttracted to negative (O) end of H22OO Each NaEach Na++ completely surrounded by H completely surrounded by H22OO
ClCl--
Attracted to positive (HAttracted to positive (H22) end of H) end of H22OO Each ClEach Cl-- completely surrounded by H completely surrounded by H22OO