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Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
AP Biology Ch. 2 The Chemical Context of Life
Bombardier Beetle’s Defense:
Ejecting a spray of hot irritating chemicals, an example of the interconnectedness of biology and chemistry.
•Essential elements of life
•Structure of atoms
•Chemical bonding
•Chemical reactions
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
25 Essential Elements of Life
96% of living matter –
O, C, H, N
Table 2.1 Naturally Occurring Elements in the Human Body
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Effects of essential-element deficiencies
(a) Nitrogen deficiency (b) Iodine deficiency –trace element
Trace elements – required only in minute quantities
deficiency results in great consequences0.15 mg iodine required
Malaysian woman – can be reversed with iodine
supplementsFigure 2.3
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
An element’s properties depend on the structure of its atoms.
• Atom – smallest unit of matter
• Mass number
– sum of protons + neutrons
• Atomic number
– Number of protons in the nucleus; 2He
• Atomic weight
– Mass number; 4He
• Isotopes
– 2 atoms of same element; differ in # of neutrons
Nucleus
Cloud of negativecharge (2 electrons)
Electrons
Model of Helium
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Radioactive isotopes
• Unstable nuclei decay, emitting particles & energy
• Applications: date fossils trace atoms through metabolic processes diagnose disorders
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Figure 2.5 Research Method Radioactive Tracers
Scientists use radioactive isotopes to label certain chemical substances, creating tracers that can be used to follow a metabolic process or locate the substance within an organism. In this example, radioactive tracers are being used to determine the effect of temperature on the rate at which cells make copies of their DNA.
APPLICATION
DNA (old and new)
Ingredients includingradioactive tracer (bright blue)
Human cells
Incubators1 2 3
4 5 6
987
10°C 15°C 20°C
25°C 30°C 35°C
40°C 45°C 50°C
TECHNIQUE
2
1
The cells are placed in test tubes, their DNA is isolated, and unused ingredients are removed.
1 2 3 4 5 6 7 8 9
Ingredients for making DNA are added to human cells. One ingredient is labeled with 3H, a radioactive isotope of hydrogen. Nine dishes of cells are incubated at different temperatures. The cells make new DNA, incorporating the radioactive tracer with 3H.
Radioactive isotopes –
elements with unstable nuclei; give off particles and energy as
they decay
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Placed in a Scintillation Chamber
Temperature (°C)
The frequency of flashes, - counts per minute, proportional to the amount of the radioactive tracer present, indicating the amount of new DNA. In this experiment, when the counts per minute are plotted against temperature, it is clear that temperature affects the rate of DNA synthesis—the most DNA was made at 35°C.
10 20 30 40 50
Optimumtemperaturefor DNAsynthesis
30
20
10
0
Co
un
ts p
er
min
ute
(x 1
,00
0)
RESULTS
In scintillators the part of the energy lost by a particle is converted into the energy of a light flash
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Secondshell
Helium
2He
Firstshell
Thirdshell
Hydrogen
1H
2He
4.00Atomic mass
Atomic number
Element symbol
Electron-shelldiagram
Lithium
3LiBeryllium
4BeBoron
3BCarbon
6CNitrogen
7NOxygen
8OFluorine
9FNeon
10Ne
Sodium
11NaMagnesium
12MgAluminum
13AlSilicon
14SiPhosphorus
15PSulfur
16SChlorine
17ClArgon
18Ar
Chemical Behavior - determined by it’s electron configuration. Valence electrons – only unpaired electrons are involved
Atoms with the same # of valence e- have similar chemical behaviors.
nonreactiveFigure 2.8 Electron-shell diagrams of the first 18 elements in the periodic table.
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Formation & function of molecules depend on chemical bonding between atoms.
• Chemical bonds (4)
– Covalent bond –
– Ionic bond –
– Hydrogen bonds –
– van der Waals interactions –
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Covalent bonding – atoms sharing e-
Name(molecularformula)
Electron-shell
diagram
Structuralformula
(c)
H
Methane (CH4). Four hydrogen atoms can satisfy the valence ofone carbonatom, formingmethane.
Space-fillingmodel
Hydrogen (H2). Two hydrogen atoms can form a single bond.
(a)
H H
O O
Oxygen (O2). Two oxygen atoms share two pairs of electrons to form a double bond.
(b)
Water (H2O). Two hydrogenatoms and one oxygen atom arejoined by covalent bonds to produce a molecule of water.
O H
H
H H
HO
H
O O
H
HH C H
H
H
HC
(d)
Pair of equally shared e-
Pair of unequally shared e-
polar (e- shared unequally) vs. nonpolar (e- shared equally)
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Polar / Nonpolar Covalent Rules
• Nonpolar – e- shared equally -b/t 2 atoms of same element – H-H -b/t atoms w/similar electronegativity – CH4
• Polar – e- shared unequally ex. H2O; oxygen – higher electronegativity
• Electronegativity – attraction of an atom for the shared e- of a covalent bond (strong electronegative atoms attempt to pull the shared e- toward themselves)
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Figure 2.12 Polar covalent bonds in a water molecule
This results in a partial negative charge on theoxygen and apartial positivecharge onthe hydrogens.
H2O
–
O
H H+ +
Because oxygen (O) is more electronegative than hydrogen (H), shared electrons are pulled more toward oxygen.
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Ionic bond– one atom strips e- from another
cations (atom w/+ charge) anions (atom w/- charge)
– The attraction between oppositely charged atoms, or ions, is an ionic bond.
Cl–
Chloride ion(an anion)
–
The lone valence electron of a sodiumatom is transferred to join the 7 valenceelectrons of a chlorine atom.
1 Each resulting ion has a completedvalence shell. An ionic bond can formbetween the oppositely charged ions.
2
Na NaCl Cl
+
NaSodium atom(an uncharged
atom)
ClChlorine atom(an uncharged
atom)
Na+
Sodium ion(a cation)
Sodium chloride (NaCl)
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Hydrogen bonds –
– H atom of one compound is attracted to another compound
– Holds water together
Water(H2O)
Ammonia(NH3)
– +
OH
H
+
–
N
HH H
A hydrogenbond results from the attraction between thepartial positive charge on the hydrogen atom of water and the partial negative charge on the nitrogen atom of ammonia.
+
+
+
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
van der Waals interactions –
Molecules in close proximity exert attraction in concert
Hair tip molecules and the molecules of the wall’s surface are so numerous, collectively they form strong bonding patterns temporarily.
Gecko lizard – walks up
walls
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Molecule’s biological function -related to its shape
• Biological molecules:
– Recognize, interact with one another with a specificity based on molecular shape.
Ex. morphine affects pain perception and emotional state by mimicking the brain’s natural endorphins.
Naturalendorphin
Morphine
Endorphinreceptors
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings
Chemical reactions make / break chemical bonds.
• Change reactants into products conserving matter
• Most are reversible.
• Chemical equilibrium is reached - when the forward and reverse reaction rates are equal
Elodea, a freshwater plant, produces sugar by rearranging the atoms of carbon dioxide and water in the chemical process
known as photosynthesis. Much of the sugar is then converted to other food molecules. Oxygen gas is a by-product of
photosynthesis; hence the bubbles of oxygen escaping from the leaves.