Entropy- A measure of the dispersal of energy or disorder of a system. The system becomes energetically more stable when disordered.

System- The particular investigation (the reaction itself).

Surroundings- In enthalpy changes, anything other than the chemical reactants and products, for example the solvent, the test tube in which the reaction takes place, the air around the test tube.

Spontaneous Changes- Changes that tend to happen naturally continually.

Standard Molar Entropy- At standard conditions (p of 10^5 Pa, temp of 298K, and each substance involved in reaction is in its normal physical state) units are J*K^-1*mol^-1.

Feasibility (of reaction)- In entropy, whether or not the reaction will occur spontaneously.

Gibbs Free Energy (ig you could say how likely the rxn is going to Gibb us energy)- The energy change that takes into account both the entropy change of a reaction and enthalpy change; reactions are likely to be feasible if the value of the Gibbs free energy change of reaction is negative; the Gibbs free energy change of reaction is given by the relationship [delta]G[naught]=[delta]H[naught] - T[delta]S[naught].

Standard Molar Gibbs Free Energy of Formation ([delta]G[subscript f][naught])- The free energy change that accompanies the formation of one mole of compound from its elements in their standard states; units KJ/mol.

Standard Gibbs Free Energy of Reaction ([delta]G[naught]=[delta]H[naught] --T[delta]S[naught], T is in K not celsius, the Gibbs free energy change when the amount of the reactants in the stoichiometric equation react to give products (must be standard so 298K, 10^5 Pa, reactants in normal states).

Chapter 24 (metals! 🚄)

Transition Element- A d-block element that forms one or more stable ions with an incomplete d sub shell.

Variable Oxidation State- A property of transition elements, the ability to form more than one ion.

Ligand - A molecule or ion with one or more lone pairs of electrons available to donate to a transition metal ion.

Complex (ion)- A central transition metal ion surrounded by ligands.

Co-ordinate Number - The number of co-ordinate (dative) bonds formed by ligands to the central transition metal ion in a complex.

Bidentate 🦷🦷(ligands)- Ligands that can form two co-ordinate bonds from each ion or molecule to the central transition metal ion, for example water (the Mickey Mouse ears, or whatever you call them).

Monodentate 🦷(ligands)- Ligands that can only form one co-ordinate bond from each ion or molecule to the central transition metal ion, such as ammonia.

Stereoisomers- Compounds whose molecules have the same atoms bonded to each other but with different arrangements of the atoms in space.

Geometric Isomers- Complexes with the same molecular formulas but different geometrical arrangements of their atoms (same thing as stereo).

Optical isomers- Two compounds which contain the same number and kinds of atoms, bonds, and different spatial arrangements of the atoms, but which have non-superimposable mirror images (and can’t be rotated b/c the molecules around complex twist, so they still look different even when rotated).

Stability Constant (K[stab 🔪])- The equilibrium constant for the formation of the complex ion in a solvent from its constituent ions or molecules.

Degenerate 😔 (orbitals)- Atomic orbitals at the same energy level.

Non- degenerate 😃 (orbitals)- Atomic orbitals that have been split to occupy slightly different energy levels.