Applied Bioscience/401SCI Chemistry for Bioscience (401SCI)
Notes de cours
401SCI Chemistry for Biosciences
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Cours
Applied Bioscience/401SCI Chemistry for Bioscience (401SCI)
Établissement
Coventry University (West Midlands) (CU)
A summary of all lectures and key information in an easy to understand format. Topics include: Atomic Mass & Isotope distribution, Molecular & Empirical Formula, Avogadro’s Number / Moles, Mass, Molarity of Ions in a Solution, Density, VESPR Theory, Valency - Lewis Dot - Lone pairs, Periodic Tabl...
Applied Bioscience/401SCI Chemistry for Bioscience (401SCI)
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helenpeters100
Aperçu du contenu
Chemistry for Biosciences
Contents
Definitions ........................................................................................................................................................................ 2
Abbreviations ................................................................................................................................................................... 3
Atomic Mass & Isotope distribution ................................................................................................................................ 4
Molecular & Empirical Formula ....................................................................................................................................... 5
Avogadro’s Number / Moles ............................................................................................................................................ 6
Mass .................................................................................................................................................................................. 7
Molarity of Ions in a Solution........................................................................................................................................... 8
Density .............................................................................................................................................................................. 9
VESPR Theory ................................................................................................................................................................. 10
Valency - Lewis Dot - Lone pairs .................................................................................................................................... 10
Periodic Table Trends ..................................................................................................................................................... 11
Electron Configuration Rules ......................................................................................................................................... 12
Chemical Quantities ....................................................................................................................................................... 12
Bonding ........................................................................................................................................................................... 13
pH and pOH .................................................................................................................................................................... 16
Kw (Ionisation of H₂O).................................................................................................................................................... 16
Ka Acid Dissociation ........................................................................................................................................................ 17
Net Ionic Equations ........................................................................................................................................................ 18
Titration .......................................................................................................................................................................... 18
Acids & Bases .................................................................................................................................................................. 19
Acid Nomenclature......................................................................................................................................................... 20
Solubility Chart & Rules.................................................................................................................................................. 21
Spectroscopy .................................................................................................................................................................. 22
Beer-Lambert Law .......................................................................................................................................................... 23
Transmittance................................................................................................................................................................. 23
Calibration Curve ............................................................................................................................................................ 23
Gas Laws ......................................................................................................................................................................... 24
Enthalpy .......................................................................................................................................................................... 25
Standard Heats of Formation ......................................................................................................................................... 26
Avergae Bond Dissociation Energies ............................................................................................................................. 26
Gibbs Free Energy ........................................................................................................................................................... 27
Organic Chemistry - Hydrocarbons ................................................................................................................................ 28
Naming Alkanes – IUPAC Rules ...................................................................................................................................... 29
Naming Alkenes .............................................................................................................................................................. 30
Naming Alkynes .............................................................................................................................................................. 30
, Definitions
Miscible = a liquid able to dissolve into another liquid
Valency = same as group number in periodic table
Ion = Atom that has gained or lost an e¯
Isotope = Different types of the same element.
(same number of p⁺ and e¯ but differing neutrons)
Cation = ⁺ ion (goes first in nomenclature) usually metal
Anion = ¯ ion (goes second in nomenclature) usually a non-metal
Endothermic = Releases heat into surroundings
(Heat = product. Products have lower potential energy than reactants)
Exothermic = Absorbs heat from surroundings
(Heat = reactant. Products have higher potential energy than reactants)
Precipitation reaction = chemical reaction occurring in (aq) solution, where 1 of the
products is insoluble
Ionic equation = equation showing ions in a chemical reaction
Net ionic equation = equation showing only the participating ions
(spectator ions are removed)
Spectator ions = ions present in a chemical reaction but do not take part in it
Analyte = substance whose chemical constituents are being identified and measured
Oxidisation/Oxidised = lost electrons / Oxidising agent = gains electrons
Reduction/Reduced = gains electrons / Reducing agent = loses electrons
Dissolution = solid changing to liquid
Enthalpy = a measure of the energy stored in (or heat content of) a system.
It cannot be measured directly.
Entropy = measure of the degree of disorder/randomness of matter and energy in a
system.
, Abbreviations
Letter/Symbol Meaning
(aq) Aqueous solution
(g) Gas
(l) Liquid
(so) Solid
∆Hө298 or ΔHө Standard measurement conditions for ΔH
A Absorbance
amu Atomic mass unit of measurement
atm Atmospheric pressure
c Concentration (mol L¯¹)
D(X-X) ΔdissH
Ea Activation energy (units = + # kJ/mol)
Ei Ionisation energy (units = + # kJ/mol)
G Gibbs Free Energy
H Enthalpy
J Joule
Ka Acid dissociation
Kb Dissociation Constant
kPa Kilopascals
Ionic product/equilibrium constant/dissociation constant of water
Kw
= product of concentrations of hydronium and hydroxide ions
MM Molar mass
mmHg Milimeters of Mercury
n Energy level, (or number of moles depending on context)
P Irradiance leaving sample
P₀ Irradiance entering sample
pm Picometer = 10¯¹²m
q ΔH in joules
S Entropy
s, p, d, f, (g, h, i) Orbital levels (unused by ground state electrons)
T Temperature (or Transmittance depending on context)
Z Atomic number or A
α Proportionate to
ΔdissH Bond enthalpy for a specific bond breaking process
ΔH Change in enthalpy (kJ mol-1).
ΔT Change in temperature
ε Molar absorptivity (L/mol¯¹ cm¯¹)
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