1. Chemistry For Nursing ClS 101

2. Course Content Introduction to Chemistry. Water ( importance, features, and structure). Acids and Bases (most common, features). Liquid mixtures (types: solutions, suspensions, colloids, and emulsions). Amino Acids: Classifications, features. Proteins: sources, functions, importance, level of structure, and classification.

3. Course Content Carbohydrates: Classification and origin.  Monosaccharide: common ones, structure, and chemical reactions.  Disaccharide: common ones, properties, and chemical reactions.  Polysaccharide: common ones and properties.

4. Course Contents Lipids: Classifications, functions, and importance.  Fatty Acids: classifications and properties.  Simple lipids (fats, oils, and waxes): chemical structures, features, importance, and chemical reactions.  Complex lipids (phosphoglycerides, sphingo lipids, and glycolipids): importance, and chemical structure.

5. Course Content  Derived lipids (prostaglandins and steroids).  Composition of cell membrane.

6. Refrences Lippincott's Illustrated Reviews: Biochemistry Pamela C. Champe Richard A. Harvey

7. 25% 1 st Midterm 25% 2 nd Midterm 5% Quizzes 5% Practical 40% Final exam

8. Introduction to Chemistry

9. Atoms Atom is the smallest portion of an element that can enter into chemical combination. They cannot be bracken down or changed into another form by ordinary chemical and physical means. If placed side by side one million would stretch a distance of 1cm.

10. Atomic Theory John Dalton gave the atomic theory in 1808 which can be summarized as: 1. All matter is made up of individual particles that are indivisible and indestructible.

11. Atomic Theory 2. All atoms of a given element are identical. 3. Atoms of different elements have different masses and properties.

12. Atomic Theory 4. Atoms of elements combine in simple ratios to form compounds. 5. A chemical reaction is a rearrangement of atoms.

13. Atomic Nucleus Atoms are normally electrically neutral. In 1909, Rutherford proposed that the atom consisted of tiny positively charged atomic nucleus with electrons outside to produce electrically neutral atom.

14. Atomic Structure positively noncharged At the center of the atom is a nucleus, which contains positively charged particles called protons, and noncharged particles called neutrons. In orbit outside the nucleus are electrons (negative charge)

15. ParticleChargeMass PROTON PROTON+ Approximately equal to that of hydrogen atom Approximately equal to that of hydrogen atom. NEUTRONNEUTRAL Approximately equal to that of hydrogen atom ELECTRON- 1/1837 of a hydrogen atom. hydrogen atom.

16. Energy Levels The electrons of an tom orbit at specific distances from nucleus in regions called energy levels. first two The first level, the closest to the nucleus, can hold only two electrons. first The first level

17. second The second energy level, the next in distance away from the nucleus, can hold 8 electrons. 18 More distant energy levels can hold 18 electrons.

18. Atomic structure All of the protons and the neutrons The 1 st ring can hold up to 2 e - The 2 nd ring can hold up to 8 e - The 3 rd ring can hold up to 18 e - The 4 th ring and any after can hold up to 32 e -

19. Draw a helium atom. Indicate where the protons, neutrons and electrons are.Draw a helium atom. Indicate where the protons, neutrons and electrons are. ++ - - PROTONS NEUTRONS ELECTRONS ATOMIC # = 2 (PROTONS) ATOMIC MASS = 4 (PROTONS & NEUTRONS)

20. Atomic Number Elements are different because they contain different numbers of PROTONS. The “atomic number” of an element is the number of protons in the nucleus. # protons in an atom = # of electrons.

21. Atomic Number Element # of protons Atomic # (Z) Carbon66 Phosphorus1515 Gold7979

22. Simplest form of a substance - cannot be broken down any further without changing what it is. There are 92 naturally occurring elements. 20 additional elements have been created in lab. Elements

23. Examples of elements hydrogen, mercury, gold

24. Isotopes Isotopes are atoms of a given elements that differ in the number of neutrons. OR Isotopes are elements which have the same atomic number but different atomic weight.

25. For example, carbon-12, carbon-13 and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13 and 14 respectively. The atomic number of carbon is 6 (every carbon atom has 6 protons); therefore the neutron numbers in these isotopes are 6, 7 and 8 respectively.

26. Mass Number Mass number is the number of protons and neutrons in the nucleus of an isotope: Mass # = p + + n 0 Nuclide p+p+p+p+ n0n0n0n0 e-e-e-e- Mass # Oxygen - 10 -3342 - - 3115 8 8 18 Arsenic 7533 75 Phosphorus 15 31 16

27. Complete Symbols Contain the symbol of the element, the mass number and the atomic number. X Mass number Atomic number Subscript → Superscript →

28. The Periodic table The periodic table is chart used by chemists to organize and describe the elements. Classification Groups : A group is a vertical column in the periodic table. There are 18 groups. Periods: A period is a horizontal row in the periodic table. There are 7 periods.

30. A molecule is formed when two or more atoms unite on the basis of their electron structures. A molecule can be made of like atoms, but more often molecule is made of atoms of two or more different elements. Ex: water, Molecules

31. Compounds Chemical compound is a pure chemical substance consisting of two or more different chemical elements that can be separated into simpler substances by chemical reactions.

32. What is the difference between a compound and a molecule? A molecule is formed when two or more atoms join together chemically. A compound is a molecule that contains at least two different elements. All compounds are molecules but not all molecules are compounds. Molecular hydrogen (H2), molecular oxygen (O2) and molecular nitrogen (N2) are not compounds because each is composed of a single element. Water (H2O), carbon dioxide (CO2) and methane (CH4) are compounds because each is made from more than one element.

33. TWO TYPES OF COMPOUNDS Organic molecules: Organic molecules: Usually associated with living things. Always contain CARBON. Always have covalent bonds (share electrons) Inorganic molecules: Any substance in which two or more chemical elements other than carbon are combined, nearly always in definite proportions Water (H2O),Water (H2O),

34. FORMULA The chemical symbols and numbers that compose a compound ("recipe")The chemical symbols and numbers that compose a compound ("recipe") Structural Formula – Line drawings of the compound that shows the elements in proportion and how they are bondedStructural Formula – Line drawings of the compound that shows the elements in proportion and how they are bonded Molecular Formula – the ACTUAL formula for a compoundMolecular Formula – the ACTUAL formula for a compound C2H6OC2H6OC2H6OC2H6O