Lecture notes
Solid State Chemistry and Lattice Enthalpies
- Institution
- Cardiff University (CF)
Questions and answers for exam prep. Active recall for exam prep. Used to pass 1st-year exam in Foundations of Inorganic Chemistry.
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SOLID STATE CHEMISTRY- What is a solid?
A state of matter in which the constituent particles are arranged so their
shape and volume are stable
- What types of solids exist?
Ionic, covalent network, metals, molecular
- What are molecular solids?
Made up of molecules
- What types of bonding exist in molecular solids?
Strong covalent bonds within the molecules and weak intermolecular
bonds
- What is an example of a molecular solid?
Iodine – solid sublimes to vapour
- What are covalent network solids?
Consist of atoms all bonded covalently = continuous network
Hard and brittle with high melting and boiling points
- What is an example of a covalent network solid?
Carbon
- What are allotropes?
Different solid-state structures of the same element
Examples include graphite and diamond
- What are polymorphs?
Different solid-state structures of the same compound
- What is a metallic solid?
Cations in a “sea” of delocalised electrons
Strong forces of attraction between them = strong metallic bonding
- What is an ionic solid?
Consists of cations and anions held by strong electrostatic interactions
- What is a crystal?
Solid consisting of a regular and repeating array of particles, extending in
three dimensions
- What kind of symmetry does a crystal have?
Translational – unit cell is translated in 3 directions
- What is a unit cell?
The smallest repeating unit
- What are the 6 parameters of a unit cell?
3 lengths – a, b and c
3 angles – alpha, beta and gamma
- What are examples of cubic unit cells?
Face-centred cubic, body-centred cubic and primitive
- What are the parameters of a cubic unit cell?
All lengths equal
All angles = 90 degrees
- How do we determine a crystal structure?
X-ray crystallography
- What is the most efficient way of packing atoms in a solid?
Close packing – minimises the space between them
- What are the two most common close packing arrangements?
, Cubic close packing (ccp) (ABCABC) – spheres in layer 3 lie directly above
layer 1 gaps (not directly above the spheres in layer 1)
Hexagonal close packing (hcp) (ABABAB) – spheres in layer 3 lie directly
above layer 1 spheres
- How can we visualise close packing?
Ball and stick model
Space-filling model
- What is cubic close packing (ccp) also referred to?
Face-centred cubic (fcc)
- What is the structure of a ccp/fcc unit cell?
Atoms on all vertices
Atoms in the centres of all faces
- What other cubic unit cells exist?
Body-centred cubic (bcc)
Primitive cubic
- What is special about them?
They are not close-packed
- What are their structures?
Primitive – atoms on all vertices only
Bcc – atoms on all vertices with one atom in the centre
- What are interstitial sites?
Gaps in the structure due to atoms/ions not packing efficiently
- What are the two types of interstitial sites?
Octahedral – lies between a triangle of atoms above and a triangle below
Tetrahedral - lies between a triangle of atoms and a single atom (above or
below)
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