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Biology 1111K
Lecture 2
Slide 2 - particles
Slide 3 – particle charge
Slide 4 – Atomic symbols
Element Atomic symbol
Hydrogen H
Carbon C
Potassium K
Magnesium Mg
Calcium Ca
Slide 5 – atomic mass or weight
Element Atomic mass
Carbon 12
Nitrogen 14
Oxygen 16
Slide 6 – atomic number
Slide 7 – periodic table
Slide 8 - isotope
Slide 9 – carbon 14
Slide 10 – C 14 half-life sample
Time (Y) Isotope Amount Element Amount
0 C14 20 N14 0
1500 C14 17.5 N14 2.5
3000 C14 15 N14 5
6000 C14 10 N14 10
Slide 11 – energy
Slide 12 – stored energy
Slide 13 – electron shells
Slide 14 – electron shells
Slide 15 – octet rule
Slide 16 – chemical formulas
H2O – water - 2 hydrogen and one oxygen
CO2 – carbon dioxide - 1 carbon, 2 oxygen
H2SO4 – sulfuric acid – 2 hydrogen, one sulfur, and four oxygen
HCl – hydrochloric acid – one hydrogen, one chlorine
Slide 17 – chemical equation
6 CO2 + 6 H2O = C6H12O6 + O2
Slide 18 - compound
Slide 19 – electron donor and acceptor
Slide 20 - ions
Slide 21 – covalent bonding – non-polar
Slide 22 – polar covalent bonding
Slide 23 – hydrogen bonding
Slide 24 – shape of molecules
Slide 25 – acids and bases
Acids – molecules that dissociates in water and releases hydrogen ions (H+). When dissociation is complete, the acid is called a strong acid.
HCl H+ and OH-
H2SO4 H+ and HSO4-
Bases – molecules that either takes up hydrogen ions (H+) or releases hydroxide ions (OH-). When dissociation is complete, the base is known as a strong base.
NaOH Na + and OH –
Pure water is neutral since in its rare ionic form it gives off equal numbers of hydrogen and hydroxide ions.
H2O H+ and OH-
Slide 26 – pH scale
Slide 27 – carbonic acid - buffer
Slide 28 – inorganic vs. organic molecules
Inorganic molecule Organic molecule
Usually contains positive and negative ions Always contains carbon and hydrogen
Usually ionic bonding Covalent bonding
Contains small numbers of atoms Large numbers of atoms