Chapter reference: 6. The emergence of biological function starts at the chemical level Everything...
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Transcript of Chapter reference: 6. The emergence of biological function starts at the chemical level Everything...
The emergence of biological function starts at the chemical level
• Everything an organism is and does depends on chemistry
• Chemistry is in turn dependent on the arrangement of atoms in molecules
ATOMS AND MOLECULES
Chemicals of Life video next slide
• Molecules and ecosystems are at opposite ends of the biological hierarchy
– Each level of organization in the biological hierarchy builds on the one below it
– At each level, new properties emerge
• A biological hierarchy
A. Molecule: Actin Atom
MyosinActin
B. Organelle: Myofibril (found only in muscle cells)
Myofibril (organelle)
C. Cell and tissue: Muscle cell within muscle tissue
Rattlebox moth
D. Organ: Flight muscle of a moth
• A chemical element is a substance that cannot be broken down to other substances by ordinary chemical means
Life requires about 25 chemical elements
Atomic Structure
Subatomic Particle Symbol Location Charge Mass (amu)
Neutron n0 Nucleus 0 1.0087
Proton p+ Nucleus +1 1.0073
Electron e- Electron Cloud -1 0.00006
Properties of Subatomic Particles
Useful Equations:protons = atomic #electrons = atomic #neutrons = atomic mass - atomic #
Elements• 92 elements occur in nature
• About 25 different chemical elements are essential to life
• Only 6 elements, CHNOPS, make up 99% of living tissue
• Carbon, hydrogen, oxygen, and nitrogen make up the bulk of living matter, but there are other elements necessary for life
• Goiters are caused by iodine deficiency
Atoms & Elements
Video next
A goiter is an abnormal enlargement of the thyroid gland.
• Chemical elements combine in fixed ratios to form compounds
• Example: sodium + chlorine sodium chloride
Elements can combine to form compounds
• The smallest particle of an element is an atom
• Different elements have different types of atoms
Atoms consist of protons, neutrons, and electrons
• An atom is made up of protons and neutrons located in a central nucleus
A. Helium atom
2
2
2
Protons
Neutrons
Electrons
Nucleus
• The nucleus is surrounded by electrons
• Each atom is held together by attractions between the positively charged protons and negatively charged electrons
B. Carbon atom
6
6
6
Protons
Neutrons
Electrons
Nucleus
• Neutrons are electrically neutral
• Atoms of each element are distinguished by a specific number of protons
– The number of neutrons may vary
– Variant forms of an element are called isotopes
– Some isotopes are radioactive
• Radioactive isotopes can be useful tracers for studying biological processes
• PET scanners use radioactive isotopes to create anatomical images
Why should I care? Radioactive isotopes can help or harm us
• Electrons are arranged in shells
– The outermost shell determines the chemical properties of an atom
– In most atoms, a full outer shell holds eight electrons
Electron arrangement determines the chemical properties of an atom
• Atoms whose shells are not full tend to interact with other atoms and gain, lose, or share electrons
HYDROGEN (H)Atomic number = 1
CARBON (C)Atomic number = 6
NITROGEN (N)Atomic number = 7
OXYGEN (O)Atomic number = 8
Electron
Outermost electron shell (can hold 8 electrons)
First electron shell (can hold 2 electrons)
• When atoms gain or lose electrons, charged atoms called ions are created
– An electrical attraction between ions with opposite charges results in an ionic bond
Ionic bonds are attractions between ions of opposite charge
NaSodium atom
ClChlorine atom
Na+
Sodium ionCl–
Chloride ion
Sodium chloride (NaCl)
Na Cl Na Cl
+–
• Some atoms share outer shell electrons with other atoms, forming covalent bonds
– Atoms joined together by covalent bonds form molecules
Covalent bonds, the sharing of electrons, join atoms into molecules
• Atoms in a covalently bonded molecule may share electrons equally, creating a nonpolar molecule
• If electrons are shared unequally, a polar molecule is created
Water is a polar molecule
THE PROPERTIES OF WATER
– This makes the oxygen end of the molecule slightly negatively charged
– The hydrogen end of the molecule is slightly positively charged
– Water is therefore a polar molecule
• In a water molecule, oxygen exerts a stronger pull on the shared electrons than hydrogen
(–)
O
(–)
(+)(+)
H H
• The charged regions on water molecules are attracted to the oppositely charged regions on nearby molecules
– This attraction forms weak bonds called hydrogen bonds
Overview: Water’s polarity leads to hydrogen bonding and other unusual properties
Hydrogen bond
• Like no other common substance, water exists in nature in all three physical states:
– as a solid
– as a liquid
– as a gas
• Due to hydrogen bonding, water molecules can move from a plant’s roots to its leaves
• Insects can walk on water due to surface tension created by cohesive water molecules
Hydrogen bonds make liquid water cohesive
Surface tension/Cohesion
Capillaryaction in plants
– Water is one of the few substances that remain a liquid at such a large range of temperatures (O-100 °C). A large amount of energy must be invested to overcome the hydrogen bonds in liquid water to change it to the gas phase.
It takes a lot of energy to disrupt hydrogen bonds
• A compound that releases H+ ions in solution is an acid, and one that accepts H+ ions in solution is a base
• Acidity is measured on the pH scale:
– 0-6 is acidic
– 7 is neutral
– 8-14 is basic
– Pure water and solutions that are neither basic nor acidic are neutral, with a pH of 7
The chemistry of life is sensitive to acidic and basic conditions
• The pH scale
pH scale
Acidic solution
Neutral solution
Basic solution
Incr
easi
ng
ly A
CID
IC(H
igh
er c
on
cen
trat
ion
of
H+)
Incr
easi
ng
ly B
AS
IC(L
ow
er
con
cen
trat
ion
of
H+)
NEUTRAL[H+] = [OH–]
Lemon juice; gastric juice
Grapefruit juice
Tomato juice
Urine
PURE WATER
Seawater
Milk of magnesia
Household ammonia
Household bleach
Oven cleaner
Human blood
H+
OH–
• Cells are kept close to pH 7 by buffers
• Buffers are substances that resist pH change
– They accept H+ ions when they are in excess and donate H+ ions when they are depleted
– Buffers are not foolproof
• Some ecosystems are threatened by acid precipitation
• Acid precipitation is formed when air pollutants from burning fossil fuels combine with water vapor in the air to form sulfuric and nitric acids
Why should I care? Acid rain threatens the environment
– These acids can kill fish, damage buildings, and injure trees
– Regulations, new technology, and energy conservation may help us reduce acid precipitation
• In a chemical reaction:
– reactants interact
– atoms rearrange
– products result
Chemical reactions rearrange matter
REARRANGEMENTS OF ATOMS
2 H2+ O2
2 H2O
• Life’s structural and functional diversity results from a great variety of molecules
• A relatively small number of structural patterns underlies life’s molecular diversity
INTRODUCTION TO ORGANIC COMPOUNDS AND THEIR POLYMERS
• A carbon atom forms four covalent bonds
– It can join with other carbon atoms to make chains or rings
Life’s molecular diversity is based on the properties of carbon
Structuralformula
Ball-and-stickmodel
Space-fillingmodel
Methane
The 4 single bonds of carbon point to the corners of a tetrahedron.
• Functional groups are the groups of atoms that participate in chemical reactions
– Hydroxyl groups are characteristic of alcohols
– The carboxyl group acts as an acid
Functional groups help determine the properties of organic compounds
Biological Molecules
Biological molecules are typically large molecules constructed from smaller subunits.
Monomer: single subunit
(mono = 1; -mer = unit)
Polymer: many units
(poly = many)
• Cells link monomers to form polymers by dehydration synthesis
1 2 3
Unlinked monomer
Removal ofwater molecule
1 2 3 4
Longer polymer
Short polymer
• Polymers are broken down to monomers by the reverse process, hydrolysis
Coating of capture strand
1 2 3
Addition ofwater molecule
1 2 3
4
• Carbohydrates are a class of molecules
– They range from small sugars to large polysaccharides
– Polysaccharides are long polymers of monomers
CARBOHYDRATES
• Monosaccharides are single-unit sugars
• These molecules typically have a formula that is a multiple of CH2O
• Each molecule contains hydroxyl groups and a carbonyl group
• Monosaccharides are the fuels for cellular work
Monosaccharides are the simplest carbohydrates
• The monosaccharides glucose and fructose are isomers
– They contain the same atoms but in different arrangements
Glucose Fructose
• Monosaccharides can join to form disaccharides, such as sucrose (table sugar) and maltose (brewing sugar)
Cells link single sugars to form disaccharides
Glucose Glucose
Maltose
Sucrose
• These large molecules are polymers of hundreds or thousands of monosaccharides linked by dehydration synthesis
Polysaccharides are long chains of sugar units
• Starch and glycogen are polysaccharides that store sugar for later use
• Cellulose is a polysaccharide in plant cell walls
Figure 3.7
Starch granules in potato tuber cells
Glucosemonomer
STARCH
GLYCOGEN
CELLULOSE
Glycogen granules in muscle tissue
Cellulose fibrils ina plant cell wall
Cellulosemolecules
Carb video next slide
• These compounds are composed largely of carbon and hydrogen
– They are not true polymers
– They are grouped together because they do not mix with water
Lipids include fats, which are mostly energy-storage molecules
• Phospholipids are a major component of cell membranes
• Waxes form waterproof coatings
• Steroids are often hormones
Phospholipids, waxes, and steroids are lipids with a variety of functions
Lipid video next
• Proteins are involved in – cellular structure
– movement
– defense
– transport
– communication• Mammalian hair is composed of structural
proteins
• Enzymes regulate chemical reactions
• “All enzymes are proteins but not all proteins are enzymes!”
PROTEINSProteins are essential to the structures and activities
of life
• Proteins are the most structurally and functionally diverse of life’s molecules
– Their diversity is based on different arrangements of amino acids
Proteins are made from just 20 kinds of amino acids
• Each amino acid contains:
– an amino group
– a carboxyl group
– an R group, which distinguishes each of the 20 different amino acids
Aminogroup
Carboxyl (acid)groupFigure 3.12A
• Cells link amino acids together by dehydration synthesis
• The bonds between amino acid monomers are called peptide bonds
Amino acids can be linked by peptide bonds
Amino acid Amino acid Dipeptide
Dehydrationsynthesis
Carboxylgroup
Aminogroup
PEPTIDEBOND
• A protein, such as lysozyme, consists of polypeptide chains folded into a unique shape
– The shape determines the protein’s function
– A protein loses its specific function when its polypeptides unravel
Overview: A protein’s specific shape determines its function
A protein’s primary structure is its amino acid sequence
Secondary structure is polypeptide coiling or folding produced by hydrogen bonding
Amino acid
Hydrogen bond
Alpha helix
Pleated sheet
Primarystructure
Secondarystructure
Tertiary structure is the overall shape of a polypeptide
Quaternary structure is the relationship among multiple polypeptides of a protein
Polypeptide(single subunitof transthyretin)
Transthyretin, with fouridentical polypeptide subunits
Tertiarystructure
Quaternarystructure
• Nucleic acids such and DNA and RNA serve as the blueprints for proteins
• They ultimately control the life of a cell
NUCLEIC ACIDSNucleic acids are information-rich polymers of
nucleotides
• The monomers of nucleic acids are nucleotides
Phosphategroup
Sugar
– Each nucleotide is composed of a sugar, phosphate, and nitrogenous base
Nitrogenousbase (A)
• DNA consists of two polynucleotides twisted around each other in a double helix
– The sequence of the four kinds of nitrogenous bases in DNA carries genetic information Nitrogenous
base (A)
Basepair
• Stretches of a DNA molecule called genes program the amino acid sequences of proteins– DNA information is transcribed into RNA,
a single-stranded nucleic acid
– RNA is then translated into the primary structure of proteins
Nucleic Acid video next