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Chapter 2The Chemical Context
of Life
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Comment
Much of this chapter should be review from a basic chemistry course. Much of the material is unlikely to be brand new.
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Matter Anything that has mass and
occupies space.
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Atoms
Smallest particle of elements.
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Element
Matter made up of only one type of atom.
92 natural elements. Each element has a symbol.
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Compound
Elements combined in fixed ratios.
A compound has characteristics beyond those of its combined elements.
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Question?
What Elements are necessary For Life?
Life requires about 25 chemical elements.
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Macroelements
Elements needed in large amounts or quantities.
Examples:
C HOPKNS CaFe Mg NaCl
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Control Minus Nitrogen
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Microelements
Elements needed in very small quantities.
Also known as Trace Elements.
Examples:
Cu, Co, Zn, Mo, I, Mn
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Goiter – minus Iodine
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Atomic Number
The number of protons in the nucleus.
Each element has its own atomic number. If you change the atomic number, you no longer have the same element.
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Atomic Mass
The number of protons and neutrons in the nucleus.
The atomic mass can change.
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Atomic Model
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Isotopes
Atoms of the same (iso-) element with different atomic mass.
Caused by changes in the number of neutrons.
Used as “tracers”.
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Types of Isotopes
1. Radioactive- where the nucleus decays
spontaneously, giving off particles and energy.
2. Heavy- has a stable nucleus, but masses
more than the standard isotope for the element.
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Energy
The ability to do work.
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Potential Energy
Is the energy that matter stores because of its position or location.
Electrons have potential energy because of their position relative to the nucleus.
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Electron Energy Levels Energy levels around the
nucleus of an atom. 1st level can have 2 electrons
and has the lowest potential energy.
Other levels can hold more than 2 electrons and have higher energy levels.
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Electron Orbitals
The three dimensional space where an electron is found 90% of the time.
Different orbitals have different shapes.
Each orbital can hold only 2 electrons.
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Electron Orbitals
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Chemical Behavior Of An Atom
Is determined by its electron configuration in the energy levels and orbitals.
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Valence Electrons
The electrons in the outermost energy level.
Electrons available chemical bonds.
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Octet Rule The most stable condition is to
have an outer level of 8 electrons.
Exception - 1st level is stable with only 2 electrons.
When stable - no chemical reactions will take place. Ex: Ne, He, (Noble gases)
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Electrons of the first elements
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Chemical Bonds
Forces that join atoms together to form molecules.
Usually caused by sharing or transferring valence electrons.
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Bond Formation Depends On:
The number of valence electrons that must be gained, lost, or shared to reach the stable condition.
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Chemical Bond Types
Nonpolar Covalent Polar Covalent Ionic Hydrogen
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Nonpolar Covalent
When electrons are shared equally between atoms.
Very strong bond. Important in many molecules
found in living things. Ex: carbon to hydrogen
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Nonpolar Covalent
Can be single, double, or triple between two atoms.
Each nonpolar covalent bond involves a pair of electrons.
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Polar Covalent
When electrons are shared unequally between atoms.
Results in “polar” molecules that have charged areas. Ex: Water, H to O bonds
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Ionic Bonds
Formed when electrons are transferred from one atom to another and ions are formed.
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Types of Ions
Cations - have lost electrons (p+ > e-) giving them a positive charge.
Anions - have gained electrons (p+ < e-) giving them a negative charge.
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Ionic Bonds
Formed when cations and anions attract each other.
Weak chemical bond.
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Ionic Bonds
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Hydrogen Bonds When a hydrogen atom
bonded to one molecule is attracted to the slightly negative area (often N or O) of another molecule.
Very weak individual bond. Can be a “strong” force if
there are many H bonds.
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Hydrogen Bonds
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Molecular Shape
Determined by the positions of the atom’s orbitals.
Molecular shape is crucial in Biology because it determines how most molecules of life recognize and respond to one another.
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Chemical Reactions
The making and breaking of chemical bonds.
Reactions do not destroy matter, they only rearrange it.
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Parts of the Equation2 H2 + O2 2 H2O
Reactants: - the starting materials. Products: - the ending materials. Note - all atoms of the reactants
must be accounted for in the products.
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Chemical Equilibrium
When the conversion of reactants to products is balanced to the reverse reaction.
Ex:
3 H2 + N2 2 NH3
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Summary
Element vs compound Macro and micro elements Atomic Number and Mass Isotopes Valence electrons Chemical Bonds
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Summary
We will now put elements together to form molecules and build the next level in the hierarchy.