Module 1, Part 2 of 2

Question 1

Synthesis Reaction

Answer 1

substance produced by combination of 2 or more simple substances

Question 2

Decomposition Reaction

Answer 2

Breakdown of a more complex molecule into a less complex molecule

Question 3

Exergonic reaction

Answer 3

release energy because potential E of reactant is more than that of products

Question 4

Endergonic reaction

Answer 4

absorbs energy because potential E of reactants is less than that of products

Question 5

Catabolic Reactions

Answer 5

-decomposition reactions but in living organisms
-ex breakdown of fat for energy

Question 6

Anabolic reaction

Answer 6

process that uses E to make complex molecules from simpler ones
(usually also synthesis and energonic too )

Question 7

Catalysts

Answer 7

speed up chemical reaction by reducing activation E needed to get it started
–> therefore reactions dont usually occur spontaneously

Question 8

Lactase as a Catalyst

Answer 8

lactase breaks lactose into galactose and glucose - we cant digest if we cant break it down

Question 9

Hydrolysis Reaction

Answer 9

a larger molecule forms two (or more) smaller molecules and water is consumed as a reactant.

or lysis = break

Question 10

Moles

Answer 10

-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

Question 11

Molarity

Answer 11

M= # of mols/litres of solution

Question 12

Elemental Abundance

Answer 12

-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

Question 13

Structure of Atoms

Answer 13

-smallest unit of an element
-consist of 3 subatomic particles (proton + in nucleus), neutron (neutral in nucleus), electron (negative surrounding nucleus)

Question 14

Electron Shells
number of electrons =…

Answer 14

-similar to circles around the nucleus
-each shell can hold specific number of e-
-number of e- = number of protons
-each atom is neutral

Question 15

Interaction of Elements

Answer 15

-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

Question 16

Octet Rule

Answer 16

elements interact to produce chemically stable arrangements of 8 electrons in outer shell

Question 17

Atomic Number

Answer 17

number of protons in nucleus

Question 18

Mass Number

Answer 18

sum of protons and neutrons

Question 19

Isotopes

Answer 19

-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)

Question 20

Benefits and Risks of Radiation

Answer 20

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

Question 21

Ions

Answer 21

a particle that has a -ve or +ve charge due to unequal number of electrons compare to protons

Question 22

Ion examples

Answer 22

Cl- gained 1 electron to become stable

Ca2+ lost 2 electrons to become stable

Question 23

Free Radicals

Answer 23

-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)

Question 24

Free Radicals and Human Health

Answer 24

-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

Question 25

Table Salt

Answer 25

sodium chloride NaCl =Na+ and Cl- attracted to each other

Question 25

Ionic Bonds in the Body

Answer 25

Ionic bonds found commonly in bones and teeth, giving them strength

Question 25

Electrolytes in Body

Answer 25

electrolytes are ionic compounds that can break into +ve and -ve ions

Question 26

Surfactant

Answer 26

mixture of phosphoplipids and lipoproteins, produced by type 2 alveolar cells in lungs

Question 27

Potential Energy

Answer 27

stored energy that is available to do work

Question 28

Potential Energy

Answer 28

potential energy stores in the bonds of compounds and molecules

Question 29

Energy cannot be created or destroyed

Question 30

Metabolism

Answer 30

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)

Question 31

Anabolsim example

Answer 31

combining amino acids to make a protein molecule anabolism and endergonic

Question 32

Reversibility of Chemical Reactions

Answer 32

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

Question 33

Carbonic Acid-Bicarbonate Buffer System

Answer 33

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

Question 34

Enzymes and Catalysts

Answer 34

-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

Question 35

Inorganic and Organic Compounds

Answer 35

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

Question 36

pH

Answer 36

-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

Question 37

pH item examples

Answer 37

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 =

Question 38

Practice Mole Calculations

Answer 38

3 from week 1

Question 39

Practice

Answer 39

drawing mass number, atomic number, protons/electrons/neutrons, a bohr diagram, why we care about element