1. Chemistry of Life
Matter…
Energy…
Life…

2. 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.

3. 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 (-)

4. 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

5. 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

6. 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

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

8. 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

9. 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

10. 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

11. 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.

12. 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

13. 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

14. 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.

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

16. B: Water and Solutions
pH scale: indicates the concentration of H+ ions in a solution
 
Acid Neutral Base

17. 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

18. 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

19. 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)

20. 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

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

22. 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)

23. 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)

24. 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

25. 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

26. 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

27. 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

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

29. 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

30. 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.

31. 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.