Class notes

401SCI Chemistry for Biosciences

19 views 0 purchase

Course
Applied Bioscience/401SCI Chemistry for Bioscience (401SCI)

Institution
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...

[Show more]

Preview 3 out of 30 pages

View example

Uploaded on April 18, 2023
Number of pages 30
Written in 2020/2021
Type Class notes
Professor(s) Applied biosciences
Contains All classes

mass
density
vespr theory
per
atomic mass amp isotope distribution
molecular amp empirical formula
avogadro’s number moles
molarity of ions in a solution
valency lewis dot lone pairs

Institution
Coventry University (West Midlands) (CU)
Education Unknown
Course
Applied Bioscience/401SCI Chemistry for Bioscience (401SCI)

CA$13.71

Added

Add to cart

Add to wishlist

100% satisfaction guarantee
Immediately available after payment
Both online and in PDF
No strings attached

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)

The benefits of buying summaries with Stuvia:

Guaranteed quality through customer reviews

Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.

Quick and easy check-out

You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.

Focus on what matters

Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!

Frequently asked questions

What do I get when I buy this document?

You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.

Satisfaction guarantee: how does it work?

Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.

Who am I buying these notes from?

Stuvia is a marketplace, so you are not buying this document from us, but from seller helenpeters100. Stuvia facilitates payment to the seller.

Will I be stuck with a subscription?

No, you only buy these notes for CA$13.71. You're not tied to anything after your purchase.

Can Stuvia be trusted?

4.6 stars on Google & Trustpilot (+1000 reviews)

75632 documents were sold in the last 30 days

Founded in 2010, the go-to place to buy study notes for 14 years now

Start selling