Basic chemistry

1. Basic chemistry Chapter 2 – Advanced Human Anatomy

2. Introduction • Chemistry is the branch of science that considers the composition of matter and how this composition changes. • Chemistry is essential for understanding anatomy and physiology because body structures and functions result from chemical changes within cells.

3. Structure of Matter • Matter is anything that has mass (weight) and takes up space. • Matter is found in various forms: gases, liquids, and solids • Elementsmake up all matter. • Elements are composed of tiny particles called atoms. • Atoms are the smallest unit of matter

4. Atomic Structure • Nucleus is the central portion of the atom which contains neutrons (neutral) and protons (positive). • Electrons: found outside the nucleus in energy shells (orbitals); negative charge.

5. Drawing atoms • Atomic number is the number of protons in an element. • The number of protons in the nucleus of an atom equal the number of electrons in its shells. • Atoms are neutral • Electron shells or orbitals: • 1st shell can hold a max of 2 electrons • 2nd – 6th shells can hold a max of 8 electrons

6. Drawing atoms continued… • Atomic mass = the number of protons plus neutrons. • Therefore… • atomic mass minus atomic number equals # of neutrons.

7. Atoms want Stability • The defining characteristic of stable elements is the maximum number of electrons in its valence (outer) shell. • Unstable elements achieve stability by gaining, losing, or sharing electrons in their energy levels or shells.

8. Bond Types • Ionic bonds occur between a metal and nonmetals when theytransfer electrons forming ions. • Atoms that gain or lose electrons and become electrically charged • Charged atoms = ions • Covalent bond between two nonmetals they share electrons. • Hydrogen Bonds: electromagnetic attractive interaction between polar molecules, in which hydrogen is bound to a highly electronegative atom, such as nitrogen or oxygen.

9. Molecules and Compounds • A molecule is formed when two or more atoms combine. • If atoms of different elements combine, the resulting structure can also be called a compound. Examples: Baking soda, sugar • Molecular formula represents the numbers and types of atoms in a molecule. Examples… H2O & C6H12O6

10. Chemical Reactions • Synthesis when two or more atoms or reactants bond to form a new, more complex structure. • Synthesis requires energy and is important to the growth of body parts. • Decomposition the opposite of synthesis • Single Replacement: A single free element replaces or is substituted for one of the elements in a compound • Double Replacement: reaction type can be viewed as an "exchange of partners." A + B  AB AB  A + B AB + C  AC + B AB + CD  AD + CB

11. Reaction Speed • Catalysts affect the speed of a reaction • Many reactions occur to slowly to sustain life • Not consumed by the reaction. • Biological catalysts? • Enzymes! 

12. Acids and Bases • pH scale ranges from 0 to 14. It indicates how the concentration of H+ in a substance • Acids have pH less than 7 • More H+ than OH- • Neutral pH equal to 7 • Bases have pH greater than 7 • More OH- than H+

13. Organic AND Inorganic Compounds Day 2 – Basic Chemistry (Chapter 2)

14. Organic vs. Inorganic • 2 types of chemicals • Organic must contain carbon and hydrogen but may contain other elements as well. (C6H12O6) • Inorganic all the other compounds that do NOT contain carbon-hydrogen bonds; (H20)

15. Inorganic Compounds • Water: plays an important role in dissolving solid substances, moving chemicals around the body, and absorbing and moving heat • Most abundant compoundin cells and is a solvent in which chemical reactions occur. • Polar molecule • Oxygen: Releases energy from glucose and other nutrients. • This energy drives metabolism! • Carbon Dioxide: inorganic substances that is a metabolic waste product, exhaled from the lungs. • Salts: provide a variety of ions that metabolic processes require.

16. Organic Compounds • Carbohydrates • Lipids • Proteins • Nucleic acids

17. Carbohydrates • Supply most of the energy needed by cells • Composed of what 3 elements? • Carbon, Hydrogen, Oxygen • Building blocks = sugars • Monosaccharides (simple sugars) • Disaccharides are two sugars joined together • Polysaccharides, such as starch, are built of many sugars. • Humans synthesize the complex carbohydrate called glycogen.

18. Dehydration Synthesis • Type of condensation reaction in which monomers (monosaccharides) join together into polymers while losing a water molecule • This process is carried out by losing (-OH) from one of the monomers and (H) from another.

19. Lipids • Lipids = concentrated energy molecules • Building block (monomer) = fatty acid • Not soluble in water • Common Categories • Fats • Oils • Waxes hydrophobic

20. Function of Lipids • energy storage • very concentrated • 2x the energy as carbohydrates! • cell membrane • cushion • Organs • Nerve cells • insulates body • Whale blubber!

21. Saturated vs. Unsaturated • Saturated = single carbon bond, maximum # of hydrogen bonds • Unsaturated = carbon-carbon double bond • Polyunsaturated = more than one carbon-carbon double bond

22. Fat molecule is not a polymer, just a big “fat” molecule.

23. amino acid amino acid amino acid amino acid amino acid Proteins • Proteins have many of functions in the body---as structural materials, as energy sources, as certain hormones, as receptors on cell membranes, as antibodies, and as enzymes • Building blocks of proteins are the amino acids (20) • Give their identity by their R-Group • Link up to form chains – these chains become proteins!

24. Amino Acids are composed of: • Amino group • Carboxyl group • Hydrogen • R-group

25. Amino Acids • Alanine • Glutamic acid      • Leucine • Serine   • Arginine • Glutamine   • Lysine   • Threonine • Asparagine • Glycine • Methionine 12.  Tryptophan      13. Aspartic acid      14. Histidine 15.Phenylalanine   16. Tyrosine   17. Cysteine 18.Isoleucine 19. Proline 20.Valine (NOTE: the 8 essential amino acids are in blue.  These cannot be synthesized by the human body and must be obtained from food)

26. Protein Shapes • Proteins have complex shapes held together by hydrogen bonds. (their many shapes changes their functions) • Their complex shapes are known as conformations • Protein shapes can be altered by pH, temperature, radiation, or chemicals. • When the H bonds break this is called denaturing

27. Enzymes Some chemical reactions are too slow or have activation energies way too high so we need a…. • Catalyst: speeds up reaction and lowers the activation energy • enzyme: biological catalysts! Enzymes are PROTEINS. • Found in cells

28. Enzyme-Substrate Complex • Enzymes provide a site where reactants can be brought together to react • Reactants in an enzyme reaction are called substrates • Enzyme and the substrate fit together a bit like a puzzle! • Active site: place where substrate and enzyme bind • Once the reaction is over, products are released and the enzyme is free to start the process over again

29. Induced-Fit Model Hypothesis • Induced-Fit model: This model proposes that the initial interaction between enzyme and substrate is relatively weak, but that these weak interactions rapidly cause shape changes in the enzyme that strengthen binding • Enzyme changes shape during the reaction

30. Nucleic Acids • Nucleic acids form genes and take part in protein synthesis. • Contain the elements C,H,O,N,P • The building blocks are nucleotides. • Two major types: DNA (with deoxyribose) and RNA (with ribose).

31. DNA & RNA Deoxyribonucleic acid: DNA (deoxyribonucleic acid) stores the molecular code in genes. • How many strands does it have? Ribonucleic acid: RNA (ribonucleic acid) functions in protein synthesis. • How many strands does it have?

32. sugar N base phosphate Nucleotides • Building block of nucleic acids – Nucleotides • Nucleotides consist of 3 parts: • Five carbon sugar • Phosphate group • Nitrogenous base