Chemistry of Life Matter… Energy… Life…

Objectives Objectives: Explain the nature of matter; Discuss the importance of water and solutions; Break down the chemistry of cells, and Recognize chemical reactions and understand enzymes.

A: Nature of Matter Matter is made of atoms Atom- smallest unit of matter that can not be broken down by chemical means Atoms consists of three kinds of particles Protons- Positively Charged (+) Neutrons- No Charged Electrons- Negatively Charged (-)

A: Nature of Matter Nucleus – Core of an atom made of protons (yellow) and neutrons (red) Electron cloud – The space around the nucleus that electrons (gray) may occupy at any time

A: Nature of Matter Protons and electrons are oppositely charged so they attract each other Typically atoms have no electrical charge protons = electrons Element – substance made of only one kind of atom, and is therefore a pure substance

A: Nature of Matter Compound – Substance made of the joined atoms of two or more different elements Every compound is identified by a chemical formula that identifies the elements in the compound and their proportions Example: Sodium (Na) joined with Chlorine (Cl) forms Sodium Chloride (NaCl) or Table salt Two Hydrogen atoms (H2) joined with one Oxygen atom (O) forms H20 or water

A: Nature of Matter Molecule – a group of atoms bonded together Types of bonds Covalent Hydrogen Ionic

A: Nature of Matter Covalent Bonds Atoms generally have a neutral charge Atoms are stable when they have eight electrons in their outer energy level Atoms share electrons so that they have eight in their outer energy level

A: Nature of Matter Hydrogen Bonds The shared electrons in a water molecule are attracted more strongly by the oxygen nucleus than the hydrogen nucleus The water molecule has partially positive and negative ends, or poles The opposite poles of two water molecules form a weak bond called a hydrogen bond (similar to opposing poles on a magnet) Hydrogen bond

A: Nature of Matter Ion – An atom or molecule that has gained or lost an electron Ions may interact to form ionic bonds Ions do not share electrons, but one atom “gives” an electron to the other so they have eight in their outer energy level Na+ positive sodium ion & Cl- Negative chloride ion interact to form NaCl

B: Water and Solutions Water is a major component of cells 70% of the human body is water Water stores heat efficiently Water helps regulate body temperature Water acts as a transport system for nutrients and wastes for animals.

B: Water and Solutions Water bonds to its self and other structures Cohesion – the polarity of water molecules cause them to cling to one another like magnets Caused by hydrogen bonds

B: Water and Solutions Adhesion – water molecules that are attracted to another surface, ie: water droplets stick to your skin after a shower Adhesion and cohesion Causes capillary action

B: Water and Solutions Compounds that dissolve in water form solutions. Dissolved nutrients that are transported along with the water move to the places where they are used.

B: Water and Solutions Solution: solute dissolved in a solvent Solute: thing that gets dissolved Solvent: thing that does the dissolving

B: Water and Solutions pH scale: indicates the concentration of H+ ions in a solution -------------------------------------------- 0 7 14 Acid Neutral Base

B: Water and Solutions Acid: Contain higher concentrations of H+ ions than pure water and have a number lower than 7 Bases: Contain lower concentrations of H+ ions and have numbers greater than 7 Neutral: Pure tap water Buffers: Weak acids or bases that react with strong acids or bases to prevent a sharp, sudden change in pH

C: Break Down Chemistry of Cells Carbon – most common substance found in all living organisms Four Main Carbon Compounds: Carbohydrates, Proteins, Lipids, Nucleic acids. Carbon has four electrons available for bonding in its outer energy level Able to form single (sharing one electron) double (sharing two electrons) or triple sharing (three electrons) covalent bonds with other elements

C: Break Down Chemistry of Cells The variety of covalent bond types allows carbon to form different shaped structures Isomers – Compounds with the same simple formula but a different three dimensional structure (ie. glucose and fructose C6H12O6)

C: Break Down Chemistry of Cells Carbon compounds also vary greatly in size Polymer – Large molecule formed when two smaller molecules bond together Condensation – Process through which polymers are formed when the two smaller molecules release an H and an OH group that can form Water Hydrolysis – Process through which polymers are broken apart by adding the H and OH group from a water molecule

C: Break Down Chemistry of Cells Four basic types of carbon polymers Carbohydrates Lipids Proteins Nucleic acids

C: Break Down Chemistry of Cells Carbohydrates Used by the cell to store and release energy Composed of Carbon, Hydrogen, and Oxygen at a ratio of 1:2:1 Monosaccharide – Simplest type (glucose or fructose) Disaccharide – Two monosaccharides (sucrose or table sugar) Largest type: Polysaccharide (many monosaccharides hooked together i.e. starch)

C: Break Down Chemistry of Cells Lipids (fats and oils) Used by the cell for energy storage, insulation, and protective coating Important part of cell membrane Have a much larger ratio of C-H than 2:1 and a much smaller ratio of C-O than 2:1 Insoluble in water Nonpolar (no electrical charge)

C: Break Down Chemistry of Cells Lipids (fats and oils) cont: Saturated Fatty Acids Solid at room temperature The carbon atom can not bond with any more hydrogen atoms Unsaturated Fatty Acids Liquid at room temperature The carbon atom can bond with more hydrogen atoms

C: Break Down Chemistry of Cells Proteins Provide structure for tissue and organs, carry out cell metabolism, help muscle tissue contract, provide immunity, and regulate other proteins Large complex polymer composed of carbon, hydrogen, oxygen, nitrogen and usually sulfur Basic building blocks of proteins are called amino acids

C: Break Down Chemistry of Cells Proteins cont. Twenty two(22) common amino acids These 22 amino acids in different combinations make thousands of proteins Enzyme – Type of protein that speeds up chemical reactions

C: Break Down Chemistry of Cells Nucleic acids Store cellular information in the form of a code DNA and RNA Made up of smaller subunits called nucleotides Composed of Carbon, Hydrogen, Oxygen, Nitrogen and Phosphorus arranged in three groups, base, simple sugar, and phosphate group

D. Recognize Chemical Reactions and understand Enzymes Reactant: elements or compounds that enter into a chemical reaction Product: produced b a chemical reaction

D. Recognize Chemical Reactions and understand Enzymes Chemical Reaction: a process that changes or transforms one set of chemicals into another The ------- in a chemical reaction is read “changes to” or “forms” CO2 + H2O - H2CO3 Carbon dioxide and water change to carbonic acid

D. Recognize Chemical Reactions and understand Enzymes Catalyst: is a substance that speeds up the rate of a chemical reaction Enzyme: are proteins that act as organic catalysts.

D. Recognize Chemical Reactions and understand Enzymes Activation Energy: energy input needed to start a reaction Substrate: a site where reactants can be brought together for a reaction with a reduced need for energy.