Module 1, Part 2 of 2 Flashcards
Synthesis Reaction
substance produced by combination of 2 or more simple substances
Decomposition Reaction
Breakdown of a more complex molecule into a less complex molecule
Exergonic reaction
release energy because potential E of reactant is more than that of products
Endergonic reaction
absorbs energy because potential E of reactants is less than that of products
Catabolic Reactions
-decomposition reactions but in living organisms
-ex breakdown of fat for energy
Anabolic reaction
process that uses E to make complex molecules from simpler ones
(usually also synthesis and energonic too )
Catalysts
speed up chemical reaction by reducing activation E needed to get it started
–> therefore reactions dont usually occur spontaneously
Lactase as a Catalyst
lactase breaks lactose into galactose and glucose - we cant digest if we cant break it down
Hydrolysis Reaction
a larger molecule forms two (or more) smaller molecules and water is consumed as a reactant.
or lysis = break
Moles
-unit of measurement
-a mole of any substance is the amount of that substance in grams that contains avogadros number
-avogadros = 6.022x10^23
-the mass of 1 mol of a substance is called the molar mass and is measured in grams/mol
Molarity
M= # of mols/litres of solution
Elemental Abundance
-96% of body = oxygen, carbon, hydrogen, nitrogen
-3.6% of body = calcium, phosphorus, potassium, sulphur, sodium, chlorine, magnesium and iron
-a.4% of body = aluminum, cobalt, copper fluorine, iodine, manganese, molybdenum, selenium, silicon, tin, zinc
Structure of Atoms
-smallest unit of an element
-consist of 3 subatomic particles (proton + in nucleus), neutron (neutral in nucleus), electron (negative surrounding nucleus)
Electron Shells
number of electrons =…
-similar to circles around the nucleus
-each shell can hold specific number of e-
-number of e- = number of protons
-each atom is neutral
Interaction of Elements
-an atom with a full outer electron shell is stable, and is unlikely to bond with another atom
-first shell can only have two electrons, 8, 8
Octet Rule
elements interact to produce chemically stable arrangements of 8 electrons in outer shell
Atomic Number
number of protons in nucleus
Mass Number
sum of protons and neutrons
Isotopes
-different neutrons, same electrons
-all isotopes of an element have the same chemical properties (such as number of e-)
isotopes can be stable and unstable
-radioactive isotopes are unstable (nuclei spontaneously decay to a new configuration over time, emitting radiation particles)
Benefits and Risks of Radiation
harmful = cancer
-radon-222 is a colourless/odourless cas as a result of uranium breakdown and is connected to lung cancer in non smokers
beneficial = medical imaging and iodine-131 to treat hyperthyroidism
Ions
a particle that has a -ve or +ve charge due to unequal number of electrons compare to protons
Ion examples
Cl- gained 1 electron to become stable
Ca2+ lost 2 electrons to become stable
Free Radicals
-an atom with an unpaired electron in its outermost shell is a free radical
-they are unstable, highly reactive and destructive to tissue
-cause damage to cell membranes, DNA
-free radicals can become stable by gaining or losing electron(s)
Free Radicals and Human Health
-produced by UV light from sun, xrays, during normal metabolic reactions, air pollution, cigarette smoke, alcohol and drugs
-linked to many diseases: premature aging, pre-eclampsia, fetal alcohol syndrome
-damage may be slowed with antioxidants such as vit C and E and selenium
Table Salt
sodium chloride NaCl
=Na+ and Cl- attracted to each other
Ionic Bonds in the Body
Ionic bonds found commonly in bones and teeth, giving them strength
Electrolytes in Body
electrolytes are ionic compounds that can break into +ve and -ve ions
Surfactant
mixture of phosphoplipids and lipoproteins, produced by type 2 alveolar cells in lungs
Potential Energy
stored energy that is available to do work
Potential Energy
potential energy stores in the bonds of compounds and molecules
Energy cannot be created or destroyed
Metabolism
all chemical reactions occurring in the body/cell
-human metabolism is exergonic and endergonic reactions so the energy released from one can fuel the other
glucose breakdown releases energy = exergonic
that energy can contribute to building muscle and bone (endergonic)
Anabolsim example
combining amino acids to make a protein molecule
anabolism and endergonic
Reversibility of Chemical Reactions
if chemical bonds can be made, they can also be broken
-reversibility indicated by double sided arrow
-reactants can become products or products can become reactants
Carbonic Acid-Bicarbonate Buffer System
CO2 + H2O = H2CO3 = H+ + HCO3-
-when pH increases and there is low H+ concentration, reaction shifts right
-when pH decreases and there is H+ concentration, reaction shifts left
Enzymes and Catalysts
-catalysts in living cells are called enzymes
-enzymes can only react with their specific substrate
-many vitamins are coenzymes
-riboflavin B2 is a coenzyme that plays a role in carb and protein metabolism
Inorganic and Organic Compounds
inorganic compounds:
-lack carbon and are structurally simple
-may have ionic or covalent bonds
-ex. H2O, NH3
Organic compounds:
-contain carbon and usually hydrigen
-always covalent bonds
-must drugs are organic compounds
pH
-measures H+ concentration
–pH is -ve log scale so when it becomes more acidic (low number). H+ conc is higher
-log scale so difference of pH 5 and 6 is 10x more H+ at pH of 5
-acidic less than 7
basic/alkaline = more than 7
pH item examples
pH 0 = battery acid
pH 1 = stomach acid
pH 2 = lemon juice
pH 3 = white vinegar
pH 4 = tomato juice
pH 5 = black coffee
pH 6 = milk
pH 7 =water
pH 8 = blood
pH 9 = hand soap
pH 10 = laundry soap
pH 11 = ammonia cleaner
pH 12 = bleach
pH 13 =
pH 14 =
Practice Mole Calculations
3 from week 1
Practice
drawing mass number, atomic number, protons/electrons/neutrons, a bohr diagram, why we care about element
