Inorganic Chemistry Atoms – Smallest unit of matter Elements – Different types of matter –92...
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Transcript of Inorganic Chemistry Atoms – Smallest unit of matter Elements – Different types of matter –92...
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
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)
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
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.