Inorganic Chemistry

• Atoms – Smallest unit of matter

• Elements – Different types of matter– 92 in nature, 15 in life, 4 major elements in life

• Molecules – 2 or more atoms ex) H2, O2, N2

• Compounds – 2 or more elements ex) H2O

Atomic Structure

• Particles – protons +, electrons -, neutrons n

• Nucleus – contains protons & neutrons

• Energy levels – electrons orbit nucleus– 1st – 2 electrons max– 2nd – 8 electrons max– 3rd – 8 electrons max

Characteristics of atoms

• Atomic Number - # of Protons = # of Electrons

• Atomic Mass - # Protons + # Neutrons

What atoms like to be…..

1) Neutral

2) Full outer energy level

Elements of Life

• Hydrogen – 1 proton, 0 neutrons, 1 electron– 1 outer electron (1 needed)

• Carbon – 6 protons, 6 neutrons, 6 electrons– 4 outer electrons (4 needed)

• Nitrogen – 7 protons, 7 neutrons, 7 electrons– 5 outer electrons (3 needed)

• Oxygen – 8 protons, 8 neutrons, 8 electrons– 6 outer electrons (2 needed)

Electron ConfigurationChapter 2: Small Molecules: Structure and Behavior

2.5

Figure 2.5Figure 2.5

figure 02-05.jpg

Isotopes

• Different forms or the same element– Carbon 14 vs. Carbon 12– Hydrogen 2 or 3 vs. Hydrogen 1– Nitrogen 15 vs. Nitrogen 14– Oxygen 18 vs. Oxygen 16

• Tracers – use of radioisotopes to trace chemical pathways in living things.

IsotopesChapter 2: Small Molecules: Structure and Behavior

2.2

Figure 2.2Figure 2.2

figure 02-02.jpg

Chemical Bonding

• Covalent Bonds

• Ionic Bonds

• Hydrogen Bonds

Covalent Bonding

• Covalent bonding – sharing electron pairs

• Single – share 1 pr. of electrons (H2)

• Double – share 2 prs. of electrons (O2)

• Triple – share 3 prs. of electrons (N2)

MethaneChapter 2: Small Molecules: Structure and Behavior

2.7

Figure 2.7Figure 2.7

figure 02-07.jpg

Polar Covalent Bonds

• Unequal sharing of the electrons creates partial charges on the molecule– Ex) Water

• Hydrogen bonds form between partial positive and negative charges on atoms

Ionic Bonding

• Ionic bonding – transfer of electrons from one atom to another atom.– Ex) NaCl - Na+ & Cl-

• Ions – charged atoms or groups of atoms

Ionic BondsChapter 2: Small Molecules: Structure and Behavior

2.10

Figure 2.10Figure 2.10

figure 02-10.jpg

Salt dissolves in waterChapter 2: Small Molecules: Structure and Behavior

2.11

Figure 2.11Figure 2.11

figure 02-11.jpg

Organic ChemistryCompounds found in living things.

Contain C,H,O, but based on carbon.

Form long chains, branched chains, rings.

4 Types:

Carbohydrates

Proteins

Lipids

Nucleic Acids

Carbohydrates

Characteristics

• Contain C, H, O & H:O ratio = 2:1

• Primary energy source for living things.

• Form ring structures

• Names end in –ose.

CarbohydratesBuilding Blocks

• Monosaccharide ex) Glucose – C6H12O6

Galactose, Fructose• Isomers – Different forms of the same molecule

• Disaccharide ex) Maltose, Lactose, Sucrose

C12H22O11

• Dehydration Synthesis – Remove water to make a larger molecule.

• Polysaccharide ex) Starch, Cellulose, Glycogen

MonosaccharidesChapter 3: Macromolecules: Their Chemistry and Biology

3.12 –Part 2

Figure 3.12 Figure 3.12 –– Part 2Part 2

figure 03-12b.jpg

Dehydration SynthesisChapter 3: Macromolecules: Their Chemistry and Biology

3.2

Figure 3.2Figure 3.2

figure 03-02.jpg

Lipids

Characteristics

• Contain C,H,O, but much less oxygen

• Cell membranes, secondary energy source

• Lipids are NOT soluble in water

• Common examples: Fats, oils, waxes

Lipids

Building Blocks

• Glycerol + 3 Fatty Acids

• Glycerol has 3 –OH groups

• Fatty Acids have –COOH group

• Dehydration Synthesis removes 3 waters.

Lipid formationChapter 3: Macromolecules: Their Chemistry and Biology

3.19

Figure 3.19Figure 3.19

figure 03-19.jpg

Fatty Acid Chains• Saturated

– Maximum # of hydrogen atoms

• Unsaturated – 1 double bond, 2 less hydrogens

• Polyunsaturated– Many double bonds, much fewer hydrogens

• Cholesterol – forms from saturated F.A.’s

Fatty Acid ChainsChapter 3: Macromolecules: Their Chemistry and Biology

3.20

Figure 3.20Figure 3.20

figure 03-20.jpg

Proteins

Characteristics

• Contain C,H,O,N (S)

• Cell structures, pigments, hormones, antibodies, contractile materials, enzymes.

• Forms: helixes, folded chains, globular.

• Names end in _______.

Proteins

Building Blocks

• Amino Acids – 20 different types• Central carbon atom

• Amino group –NH2

• Acid Group –COOH• Single Hydrogen• 20 different ® groups

Charged Amino AcidsChapter 3: Macromolecules: Their Chemistry and Biology

Table 3.2 –Part 1

Table 3.2 Table 3.2 –– Part 1Part 1

table 03-02a.jpg

Polar & Special Amino AcidsChapter 3: Macromolecules: Their Chemistry and Biology

Table 3.2 –Part 2

Table 3.2 Table 3.2 –– Part 2Part 2

table 03-02bc.jpg

Hydrophobic Amino AcidsChapter 3: Macromolecules: Their Chemistry and Biology

Table 3.2 –Part 3

Table 3.2 Table 3.2 –– Part 3Part 3

table 03-02d.jpg

Proteins

• Dipeptide – 2 Amino acids

• Dehydration synthesis forms peptide bond.

• Polypeptide – many amino acids.

Dehydration SysnthesisChapter 3: Macromolecules: Their Chemistry and Biology

3.4

Figure 3.4Figure 3.4

figure 03-04.jpg

4 levels of structural organization

• 1) Order of amino acids

• 2) Initial folding (helix, sheets)

• 3) Folding of folds (globular)

• 4) Multiple polypeptide chains together

• 3-D shape determines protein function

• Hydrogen bonds hold molecule in it’s shape

3.5 – Part 1

Figure 3.5 – Part 1

figure 03-05a.jpg

3.5 – Part 2

Figure 3.5 – Part 2

figure 03-05b.jpg

Enzymes

• Proteins that act as catalysts to speed up chemical reactions in a cell.

• Active Site – reaction part of enzyme.

• Substrate – substance enzyme acts on.

• Lock & key theory – substrate exactly fits into enzyme active site to perform reaction.

• Enzyme is not affected by the reaction.

Characteristics of Enzymes

• Enzymes are Reusable. Only need a little.

• Work best at an Optimal Temperature.

• Work best at an Optimal pH.

• Rate depends on concentration of both the enzyme and the substrate.

• Co-enzymes assist enzyme action.

• Most work inside cells, some outside.