Basic Chemistry Biology.

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Presentation transcript:

Basic Chemistry Biology

Matter Matter takes up space and has mass. All matter (living and nonliving) is composed of basic elements. Elements cannot be broken down to substances with different chemical or physical properties

CHNOPS Six elements are commonly found in living things. Carbon Hydrogen Nitrogen Oxygen Phosphorus Sulfur These elements account for about 98% of most organisms

Atoms, Molecules, Compounds Atoms – smallest part of an element that retains the elements properties Molecules – Groups of two or more atoms held together by Chemical Bonds Compounds – Substance having two or more different elements chemically bonded together.

Protons and Neutrons are in nucleus of atoms; Electrons move around nucleus. Protons are positively charged particles; Neutrons have no charge; both have about 1 atomic mass unit of weight. Electrons are negatively charged particles

Protons,Neutrons & Electrons.ram

2P=8e- Octet Rule (outermost shell most stable with 8 electrons, if there’s more than one shell) Valence Shell 2S=8e- 1S=2e-

Isotopes Isotopes are atoms with the same number of protons but differ in number of neutrons; thus a different atomic mass e.g., a carbon atom has six protons but may have more or less than usual six neutrons. Isotopes have many uses: tracers of biochemical pathways; determine age of fossils using radioactive isotopes; radiation used in medical treatment

How Many Neutrons?

Molecular Formulas Reactants Products

What types of chemical bonds do we find in molecules? Covalent- share electrons Nonpolar covalent – electrons shared equally Polar covalent - Electrons are shared unequally Ionic- transfer of electrons Hydrogen-weak bond between a partial positive and a partial negative.

Covalent Bond 2 atoms share electrons in such a way that each atom has an octet of electrons in the outer shell. Single bond (H-H) Double bond (O=O) Triple bond (N N)

Electrons shared equally Nonpolar Covalent Bonds Electrons shared equally Atoms with same electronegativity, usually diatomic molecules (ex. H2, O2, CH4)

Nonpolar Covalent Bonds

Polar Covalent Bonds Electrons are shared unequally Has electronegativity.

Polar Covalent Bonds

Ionic Bonds Electrons transferred from one atom to another. Losing or gaining electrons, atoms fill outer shells, and are more stable. Attraction of oppositely charged ions holds the two atoms together in an ionic bond.

Nonpolar Covalent Bonds Ionic Bonds Electrons Shared Equally Electrons Shared Unequally Electrons Transfered Increasing difference of electro- negativity between bonding atoms

Weak bonds BETWEEN molecules. Hydrogen Bonds Weak bonds BETWEEN molecules. A hydrogen atom covalently bonded to one electronegative atom is attracted to another electronegative atom.

Hydrogen Bonds Biologically important weak bonds helps stabilize 3 dimensional shape of large molecules(DNA and proteins).

What are the differences between: nonpolar covalent bonds Chemical Bonds What are the differences between: nonpolar covalent bonds polar covalent bonds ionic bonds

Properties of Water High Specific Heat Capacity High Heat of Vaporization Good Solvent Cohesion & Surface tension Adhesion & capillary action Ice Floats

Because water is polar molecule, it can form Hydrogen Bonds Because water is polar molecule, it can form Hydrogen Bonds. Because of the Hydrogen Bonds, water has some very UNIQUE Properties!

The Chemistry of Water: Heat Capacity Water has a high heat capacity Temperature = rate of vibration of molecules Apply heat to liquid Molecules bounce faster Increases temperature

Water has a high Specific Heat = the energy needed to heat 1g of a substance by 1°C. Very high for water b/c the H bonds must be broken; it takes a great deal of energy to heat or cool water.

The high specific heat of water is due to hydrogen bonds The high specific heat of water is due to hydrogen bonds. Hydrogen bonds must be broken before water can evaporate. Evaporative cooling is why animals pant or sweat; it also stabilizes temperatures in ponds.

Evaporative cooling: when water evaporates, the heat is taken with it & the person (or solution) cools and their temperature decreases.

Water also has a high heat of vaporization, the amount of heat required to convert a liquid into a vapor without a change in temperature. This is due to the hydrogen bonds that must be overcome.

San Bernardino Burbank Santa Barbara 73° 100° 90° Riverside 96° This property of water stabilizes temperatures of oceans, and is why coastal areas have moderate climates. San Diego 72° 40 miles Pacific Ocean 70s (°F) 80s 90s 100s Santa Barbara 73° Los Angeles (Airport) 75° Burbank 90° San Bernardino 100° Riverside 96° Santa Ana 84° Palm Springs 106°

Significance??? Because water temp rises and falls more slowly, organisms are better able to maintain their normal internal temperatures and are protected from rapid temperature change. Also moderates temperature on our planet.

The Chemistry of Water: 1. Good Solvent Water facilitates chemical reactions both outside of and within living systems. (Water is a good solvent – it dissolves other molecules because it is a polar molecule)

Hydrophobic -substances that do not dissolve in water (substances w/ nonpolar covalent bond) Hydrophilic– substances that dissolve in water (substances w/ polar covalent bond)

In Cohesion, water has a tendency to cling to other water molecules In Cohesion, water has a tendency to cling to other water molecules. Cohesion is due to hydrogen bonding. Surface tension is how difficult it is to break the surface of a liquid. Due to cohesion.

In Adhesion, water has a tendency to cling to other substances In Adhesion, water has a tendency to cling to other substances. Adhesion is also due to hydrogen bonding.

Cohesion & Adhesion

Ice is less dense than water due to hydrogen bonds forming a crystal Ice is less dense than water due to hydrogen bonds forming a crystal. Most other solids are more dense than their liquids. The fact that ice floats means that lakes don’t freeze solid in winter.

Figure 2.12a Figure 2.12

Water expands when it freezes Hydrogen bond Ice Hydrogen bonds are stable Liquid water Hydrogen bonds break and re-form

Figure 2.12b Figure 2.12

Acids, bases, and pH Acid molecules dissociate in water, releasing hydrogen ions (H+ ) ions Bases are molecules that take up hydrogen ions or release hydroxide ions (OH-). The pH scale indicates acidity and basicity (alkalinity) of a solution .

Figure 2.13 Figure 2.13

Buffers Buffers stabilize pH of a solution by accepting or donating H+. Organisms use buffers to maintain homeostasis. Blood pH is 7.4 Carbonic Acid helps to maintain this pH