Inorganic chemistry

• Show, and be able to apply, knowledge of


  • Atomic structure and bonding
  • Trends in the Periodic Table with reference to the properties of elements of biological importance
  • Thermodynamics, kinetics, and chemical equilibria
  • How basic spectroscopic techniques can be used to investigate molecular structure and shape
  • The typical reactivity of main functional groups, as determined by the bonding and molecular structure
  • The typical reactions of a range of organic systems with particular reference to substances of importance in biological systems
  • Stereochemistry of organic molecules
  • The basic structure and properties of amino acids
  • Covalent and non-covalent bonding within proteins
  • How structures and properties of amino acids and the peptide bond lead onto higher levels of protein structure
  • Some of the methods used to purify and sequence proteins
  • The substrate concentration dependence of most enzyme catalysed reactions is described by a hyperbola predicted by the Michaelis-Menten equation
  • Perform simple calculations to determine values of V, Vmax, KM, Kcat, Ki, [Etot] and the specificity constant
  • The structures and functions of some monosaccharides and polysaccharides
  • The structures and functions of some lipids
  • The structures of DNA and RNA
  • How the structures of DNA and RNA facilitate their biological roles
  • The organisation of viral, prokaryotic, and eukaryotic genomes, and describe how DNA is packaged into eukaryotic chromosomes
  • The properties of viruses and prions
  • The key processes of DNA replication, transcription, and translation
  • The mechanisms that regulate expression of the genes required for lactose utilisation by E. coli
  • Perform simple calculations concerned with concentrations, kinetics, thermodynamics, acids and bases, enzymology etc.

  
• Nucleus


  Positively charged and consists of protons and neutrons
• Shell


  Negatively charged contains electrons
• Nucleus contains 99.9% of mass
• Shell is 100,000 times larger than nucleus
• Particles that make up atoms


  • Proton: relative mass 1, relative charge +1
  • Neutron: relative mass 1, relative charge 0
  • Electron: relative mass 1/1840, relative charge -1

  
• Atomic number


  Number of protons
• Atoms of the same element have the same number of protons
• Mass number


  Sum of protons and neutrons
• Atoms of the same element can have different numbers of neutrons. These are called isotopes
• Notation of elements


  𝐸

  𝑍

  𝐴 (e.g.

  𝐶,

  𝐶

  6

  13 ,

  𝐶

  6

  14

  6

  12

  )
• A = mass number = number of protons and neutrons (A = Z + N)
• Z = atomic number = number of protons = number of electrons

  
• Unit of mass = 1/12 of 12C (also called 1 Dalton = 1 D)
• Relative atomic mass (Ar)

  m(Si) ÷ (1/12 × m(12C)) = 28.0855
• Relative molecular mass (Mr)

  Mr(C6H12O6) = (6 x Ar(C)) + (12 x Ar(H)) + (6 x Ar(O)) = 180.1559
• Atomic mass (m)


  m(Si) = 28.0855 u
• Molecular mass


  m(C6H12O6) = 180.1559 u
• Avogadro's constant (Na)


  Number of atoms in 12 g of 12C = 6.022045 x 1023 / mol
• Molar Mass (M)


  Mass of Na atoms or molecules
• M(Si) = NA x m(Si) = 28.0855 g/mol
• M(C6H12O6) = NA x m(C6H12O6) = 180.1559 g/mol
• Summary of the Masses


  • Relative Atomic Mass (Ar), Atomic Mass (m), Molar Mass (M)
• Counting atoms and molecules


  1. 𝑛(𝑚𝑜𝑙) =

  𝑚(𝑔)

  𝑀(𝑔 𝑚𝑜𝑙

  ⁄

  )

  2. 𝑚(𝑔) = 𝑛(𝑚𝑜𝑙) ∙ 𝑀(𝑔 𝑚𝑜𝑙

  ⁄

  )
• Electrons


  Involved in the changes that happen during chemical reactions
• Electrons within atoms


  Occupy fixed (discrete) energy levels/shells which are numbered 1, 2, 3, 4, 5, 6, and 7 (principal quantum numbers, n)

  
• Each shell


  Contains maximum 2 n2 electrons (n = shell number)
• The lower the value of n, the closer the shell is to the nucleus and the lower the energy level
• Atomic orbitals

  Areas of space around the nucleus where there is a high probability of finding an electron of a given energy

  
• Orbitals


  Shanding probability waves, size reflects 95% of presence of electrons, number of nodes dependent on main shell n and defines kind of subshell

  
• Electrons


  Have a property called 'spin'. For two electrons to exist in the same orbital they must have opposite spins (reduces the effect of repulsion)
• Quantum numbers that characterise the energy level of an electron


  • Principle quantum number n (shell)
  • Angular quantum number I (subshell)
  • Magnetic quantum number m (no. of orbitals in subshell)
  • Spin quantum number s

  
• Shell/Energy level


  Area around a nucleus which is occupied by electrons. Those closest to the nucleus have lowest energy
• Orbital

  Region of a shell where there is a high probability of finding an electron of a particular energy. Each orbital can hold up to two electrons

  
• Subshell


  Part of a shell that contains orbitals of the same type. The table on the next page shows the subshells that are found in each shell and the number of electrons in each

  
• Maximum number of electrons in each subshell


  • s- 2 electrons
  • p- 6 electrons
  • 10 electrons
  • 14 electrons
• The higher the shell, the more subshells
• Number of electrons in each shell

  • n = 1: only 1 s subshell = 2 electrons
  • n = 2: one s and one p subshell = 2 + 6 = 8 electrons
  • n = 3: one s, one p, and one d subshell = 2 + 6 + 10 = 18
• Characteristics of electron shells and subshells

  • No. of shells (prinicple quantum no.) n = 1, 2, 3, etc.
  • No. of subshells: n
  • Quantum no. of subshells I: I = 0 to (n-1)
  • No. of orbitals in subshell: 2I + 1
  • Quantum no. of orbital m: -I to +I

  
• Valence shell


  Noble Gas configuration is the most stable valence shell. All other elements try to gain Noble Gas configuration