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The Chemical Basis of Biology
1.
CAMPBELL BIOLOGY Reece • Urry
• Cain • Wasserman • Minorsky • Jackson © 2014 Pearson Education, Inc. TENTH EDITION CAMPBELL BIOLOGY Reece • Urry • Cain • Wasserman • Minorsky • Jackson TENTH EDITION 2 The Chemical Context of Life Lecture Presentation by Nicole Tunbridge and Kathleen Fitzpatrick
2.
© 2014 Pearson
Education, Inc. A Chemical Connection to Biology Biology is the study of life Living organisms and their environments are subject to basic laws of physics and chemistry One example is the use of formic acid by ants to protect themselves against predators and microbial parasites
3.
© 2014 Pearson
Education, Inc. Figure 2.1
4.
© 2014 Pearson
Education, Inc. Figure 2.1a
5.
© 2014 Pearson
Education, Inc. Concept 2.1: 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
6.
© 2014 Pearson
Education, Inc. Elements and Compounds Matter is made up of elements An element is a substance that cannot be broken down to other substances by chemical reactions A compound is a substance consisting of two or more elements in a fixed ratio A compound has characteristics different from those of its elements
7.
© 2014 Pearson
Education, Inc. Figure 2.2 Sodium Chlorine Sodium chloride
8.
© 2014 Pearson
Education, Inc. The Elements of Life About 20–25% of the 92 elements are essential to life (essential elements) Carbon, hydrogen, oxygen, and nitrogen make up 96% of living matter Most of the remaining 4% consists of calcium, phosphorus, potassium, and sulfur Trace elements are those required by an organism in only minute quantities
9.
© 2014 Pearson
Education, Inc. Table 2.1
10.
© 2014 Pearson
Education, Inc. Case Study: Evolution of Tolerance to Toxic Elements Some elements can be toxic, for example, arsenic Some species can become adapted to environments containing toxic elements For example, some plant communities are adapted to serpentine
11.
© 2014 Pearson
Education, Inc. Figure 2.3
12.
© 2014 Pearson
Education, Inc. Concept 2.2: An element’s properties depend on the structure of its atoms Each element consists of unique atoms An atom is the smallest unit of matter that still retains the properties of an element
13.
© 2014 Pearson
Education, Inc. Subatomic Particles Atoms are composed of subatomic particles Relevant subatomic particles include Neutrons (no electrical charge) Protons (positive charge) Electrons (negative charge)
14.
© 2014 Pearson
Education, Inc. Neutrons and protons form the atomic nucleus Electrons form a cloud around the nucleus Neutron mass and proton mass are almost identical and are measured in daltons
15.
© 2014 Pearson
Education, Inc. Figure 2.4 (b) + ++ + (a) Electrons -- Nucleus Cloud of negative charge (2 electrons)
16.
© 2014 Pearson
Education, Inc. Atomic Number and Atomic Mass Atoms of the various elements differ in number of subatomic particles An element’s atomic number is the number of protons in its nucleus An element’s mass number is the sum of protons plus neutrons in the nucleus Atomic mass, the atom’s total mass, can be approximated by the mass number
17.
© 2014 Pearson
Education, Inc. Isotopes All atoms of an element have the same number of protons but may differ in number of neutrons Isotopes are two atoms of an element that differ in number of neutrons Radioactive isotopes decay spontaneously, giving off particles and energy
18.
© 2014 Pearson
Education, Inc. Radioactive Tracers Radioactive isotopes are often used as diagnostic tools in medicine Radioactive tracers can be used to track atoms through metabolism They can also be used in combination with sophisticated imaging instruments
19.
© 2014 Pearson
Education, Inc. Figure 2.5 Cancerous throat tissue
20.
© 2014 Pearson
Education, Inc. Radiometric Dating A “parent” isotope decays into its “daughter” isotope at a fixed rate, expressed as the half-life In radiometric dating, scientists measure the ratio of different isotopes and calculate how many half-lives have passed since the fossil or rock was formed Half-life values vary from seconds or days to billions of years
21.
© 2014 Pearson
Education, Inc. The Energy Levels of Electrons Energy is the capacity to cause change Potential energy is the energy that matter has because of its location or structure The electrons of an atom differ in their amounts of potential energy An electron’s state of potential energy is called its energy level, or electron shell
22.
© 2014 Pearson
Education, Inc. Figure 2.6 (a) A ball bouncing down a flight of stairs provides an analogy for energy levels of electrons. Third shell (highest energy level in this model) Second shell (next highest energy level) First shell (lowest energy level) Atomic nucleus Energy lost Energy absorbed (b)
23.
© 2014 Pearson
Education, Inc. Electron Distribution and Chemical Properties The chemical behavior of an atom is determined by the distribution of electrons in electron shells The periodic table of the elements shows the electron distribution for each element
24.
© 2014 Pearson
Education, Inc. Figure 2.7 Atomic mass Atomic number Element symbol Electron distribution diagram 2 4.003 He Helium 2He Neon 10Ne Fluorine 9F Oxygen 8O Nitrogen 7N Carbon 6C Boron 5B Beryllium 4Be Lithium 3Li Second shell First shell Hydrogen 1H Argon 18Ar Chlorine 17Cl Sulfur 16S Phosphorus 15P Silicon 14Si Aluminum 13Al Magnesium 12Mg Sodium 11Na Third shell
25.
© 2014 Pearson
Education, Inc. Figure 2.7a Atomic mass Atomic number Electron distribution diagram 2 4.003 He Helium 5He Element symbol
26.
© 2014 Pearson
Education, Inc. Figure 2.7b Helium 2He Hydrogen 1H First shell
27.
© 2014 Pearson
Education, Inc. Figure 2.7c Boron 5B Carbon 6C Beryllium 4Be Lithium 1Li Second shell Third shell Aluminum 13Al Silicon 13Si Magnesium 12Mg Sodium 11Na
28.
© 2014 Pearson
Education, Inc. Figure 2.7d Fluorine 9F Neon 10Ne Oxygen 8O Nitrogen 7N Second shell Third shell Chlorine 17Cl Argon 18Ar Sulfur 16S Phosphorus 15P
29.
© 2014 Pearson
Education, Inc. Valence electrons are those in the outermost shell, or valence shell The chemical behavior of an atom is mostly determined by the valence electrons Elements with a full valence shell are chemically inert
30.
© 2014 Pearson
Education, Inc. Electron Orbitals An orbital is the three-dimensional space where an electron is found 90% of the time Each electron shell consists of a specific number of orbitals
31.
© 2014 Pearson
Education, Inc. Figure 2.8 Second shellFirst shell First shell Second shell 1s orbital 2s orbital Three 2p orbitals x y z Neon, with two filled shells (10 electrons) (a) Electron distribution diagram (b) Separate electron orbitals 1s, 2s, and 2p orbitals (c) Superimposed electron orbitals
32.
© 2014 Pearson
Education, Inc. Concept 2.3: The formation and function of molecules depend on chemical bonding between atoms Atoms with incomplete valence shells can share or transfer valence electrons with certain other atoms These interactions usually result in atoms staying close together, held by attractions called chemical bonds
33.
© 2014 Pearson
Education, Inc. Covalent Bonds A covalent bond is the sharing of a pair of valence electrons by two atoms In a covalent bond, the shared electrons count as part of each atom’s valence shell
34.
© 2014 Pearson
Education, Inc. Figure 2.9-1 Hydrogen atoms (2 H) + +
35.
© 2014 Pearson
Education, Inc. Figure 2.9-2 Hydrogen atoms (2 H) + + + +
36.
© 2014 Pearson
Education, Inc. Figure 2.9-3 Hydrogen atoms (2 H) Hydrogen molecule (H2) + + + + + +
37.
© 2014 Pearson
Education, Inc. A molecule consists of two or more atoms held together by covalent bonds A single covalent bond, or single bond, is the sharing of one pair of valence electrons A double covalent bond, or double bond, is the sharing of two pairs of valence electrons
38.
© 2014 Pearson
Education, Inc. The notation used to represent atoms and bonding is called a structural formula For example, H—H This can be abbreviated further with a molecular formula For example, H2
39.
© 2014 Pearson
Education, Inc. Figure 2.10 Name and Molecular Formula Electron Distribution Diagram Lewis Dot Structure and Structural Formula Space- Filling Model (d) Methane (CH4) (c) Water (H2O) (b) Oxygen (O2) (a) Hydrogen (H2) H H O O O H H C H H H H
40.
© 2014 Pearson
Education, Inc. Figure 2.10a Name and Molecular Formula Electron Distribution Diagram Lewis Dot Structure and Structural Formula Space- Filling Model (a) Hydrogen (H2) H H
41.
© 2014 Pearson
Education, Inc. Figure 2.10b Name and Molecular Formula Electron Distribution Diagram Lewis Dot Structure and Structural Formula Space- Filling Model (b) Oxygen (O2) O O
42.
© 2014 Pearson
Education, Inc. Figure 2.10c Name and Molecular Formula Electron Distribution Diagram Lewis Dot Structure and Structural Formula Space- Filling Model (c) Water (H2O) O H H
43.
© 2014 Pearson
Education, Inc. Figure 2.10d Name and Molecular Formula Electron Distribution Diagram Lewis Dot Structure and Structural Formula Space- Filling Model (d) Methane (CH4) C H H H H
44.
© 2014 Pearson
Education, Inc. Animation: Covalent Bonds
45.
© 2014 Pearson
Education, Inc. Covalent bonds can form between atoms of the same element or atoms of different elements A compound is a combination of two or more different elements Bonding capacity is called the atom’s valence
46.
© 2014 Pearson
Education, Inc. Atoms in a molecule attract electrons to varying degrees Electronegativity is an atom’s attraction for the electrons in a covalent bond The more electronegative an atom, the more strongly it pulls shared electrons toward itself
47.
© 2014 Pearson
Education, Inc. In a nonpolar covalent bond, the atoms share the electron equally In a polar covalent bond, one atom is more electronegative, and the atoms do not share the electron equally Unequal sharing of electrons causes a partial positive or negative charge for each atom or molecule
48.
© 2014 Pearson
Education, Inc. Figure 2.11 H H O H2O d+ d+ d-
49.
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Education, Inc. Ionic Bonds Atoms sometimes strip electrons from their bonding partners An example is the transfer of an electron from sodium to chlorine After the transfer of an electron, both atoms have charges A charged atom (or molecule) is called an ion
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Education, Inc. Figure 2.12-1 Na Cl Na Sodium atom Cl Chlorine atom
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Education, Inc. Figure 2.12-2 + - Na Cl Na+ Sodium ion (a cation) Cl- Chloride ion (an anion) Sodium chloride (NaCl) Na Cl Na Sodium atom Cl Chlorine atom
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Education, Inc. Animation: Ionic Bonds
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Education, Inc. A cation is a positively charged ion An anion is a negatively charged ion An ionic bond is an attraction between an anion and a cation
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Education, Inc. Compounds formed by ionic bonds are called ionic compounds, or salts Salts, such as sodium chloride (table salt), are often found in nature as crystals
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Education, Inc. Figure 2.13 Na+ Cl-
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Education, Inc. Figure 2.13a
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Education, Inc. Weak Chemical Bonds Most of the strongest bonds in organisms are covalent bonds that form a cell’s molecules Weak chemical bonds are also indispensable Many large biological molecules are held in their functional form by weak bonds The reversibility of weak bonds can be an advantage
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Education, Inc. 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
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Education, Inc. Figure 2.14 Water (H2O) Ammonia (NH3) Hydrogen bond d+ d- d+d+ d+ d+d-
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Education, Inc. Van der Waals Interactions If electrons are distributed asymmetrically in molecules or atoms, they may accumulate by chance in one part of a molecule Van der Waals interactions are attractions between molecules that are close together as a result of these charges
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Education, Inc. Collectively, such interactions can be strong, as between molecules of a gecko’s toe hairs and a wall surface
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Education, Inc. Figure 2.UN02
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Education, Inc. Molecular Shape and Function A molecule’s shape is usually very important to its function A molecule’s shape is determined by the positions of its atoms’ orbitals In a covalent bond, the s and p orbitals may hybridize, creating specific molecular shapes
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Education, Inc. Molecular shape is crucial in biology because it determines how biological molecules specifically recognize and respond to one another Opiates, such as morphine, and naturally produced endorphins have similar effects because their shapes are similar and they bind the same receptors in the brain
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Education, Inc. Figure 2.16 Natural endorphin (a) Structures of endorphin and morphine Morphine Key Carbon Hydrogen Oxygen Sulfur Nitrogen Morphine Natural endorphin Endorphin receptorsBrain cell (b) Binding to endorphin receptors
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© 2014 Pearson
Education, Inc. Concept 2.4: Chemical reactions make and break chemical bonds Chemical reactions are the making and breaking of chemical bonds The starting molecules of a chemical reaction are called reactants The final molecules of a chemical reaction are called products
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Education, Inc. Figure 2.UN03 Reactants Reaction Products 2 H2 O2 2 H2O
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Education, Inc. Photosynthesis is an important chemical reaction Sunlight powers the conversion of carbon dioxide and water to glucose and oxygen 6 CO2 + 6 H2O → C6H12O6 + 6 O2
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Education, Inc. Figure 2.17
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Education, Inc. All chemical reactions are reversible: products of the forward reaction become reactants for the reverse reaction Chemical equilibrium is reached when the forward and reverse reactions occur at the same rate At equilibrium the relative concentrations of reactants and products do not change
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Education, Inc. Figure 2.UN01a 1.0 0.9 0.8 0.7 0.6 0.5 0.4 0.3 0.2 0.1 0 0 1 2 3 4 5 6 7 8 9 10 Time before present (half-lives) Fractionofisotoperemaininginfossil
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Education, Inc. Figure 2.UN01b Neanderthal fossils
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Education, Inc. Figure 2.UN04 Nucleus Protons (+ charge) determine element Neutrons (no charge) determine isotope Atom Electrons (− charge form negative cloud and determine chemical behavior + + − −
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Education, Inc. Figure 2.UN05 Single covalent bond Double covalent bond
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Education, Inc. Figure 2.UN06 Ionic bond Electron transfer forms ions Na+ Sodium ion (a cation) Cl− Chloride ion (a anion) ClNaClNa Cl Chlorine atom Na Sodium atom + −
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Education, Inc. Figure 2.UN07 (a) (b)
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Education, Inc. Figure 2.UN08
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Education, Inc. Figure 2.UN09
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