Chemistry Flashcards
Define molecular weight
Molecular weight is the weight in grams of one mole (6.02 x 10^23) of the substance, or the weight in atomic mass units (which should have the same coefficient)
Define empirical / molecular formula
Empirical formula is the simplest whole number ratio between the numbers of atoms of the different elements making up the compound. E.g. H2O -> 2:1, H2O2 -> 1:1
Molecular formula states the exact number of the different atoms that make up the molecule. E.g. H2O -> 2:1, H2O2 -> 1:1
What are the rules for oxidation numbers?
- In elementary substances, the oxidation number of an element is zero (e.g. O2, Na, S8).
- In monoatomic ions the oxidation number is equal to the charge of the ion.
- In a neutral molecule the sum of all the oxidation numbers that make up the molecule is zero.
- Useful oxidation numbers to memorise (don’t always apply): H = +1, O = -2, Alkali metals = +1, Alkaline Earth metals = +2, Aluminium = +3
Definitions of quantum numbers?
n = principle quantum number (shows period on PT) l = angular momentum quantum number (shape of orbital) ml = magnetic quantum number (which of 3 planes) ms = spin quantum number (rotates which of 2 directions)
Shapes of s, p orbitals?
s orbitals are spherical
p orbitals are “dumbells”
Order for filling atomic orbitals?
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d…
Don’t forget Hund’s rule: each empty ml sub orbital is filled before a second is added to any of them, convention is to add them facing upwards first
What are hybrid orbitals? Shapes?
In bonding, often orbitals combine and become hybridised. This changes their energy and shape. It’s particularly useful for explaining molecular shapes.
- 1 s and 3 p bonding electrons (?) become 4 sp3 hybrids. This molecular shape would be tetrahedral, about the central atom with angles of 109.5°
- 1 s and 2 p bonding electrons (?) become 3 sp2 hybrids. This molecular shape would be trigonal with 120° angles
- 1 s and 1 p bonding electrons (?) become 2 sp hybrids. This would be a linear shape of 180°
Define Lewis structure, acid, base
Lewis structure is a digram which shows each atom and how many valence electrons is has. In addition it may show the bonding as well.
When Lewis structures don’t accurately represent a molecule because its constituents shift around, more than one Lewis structure can be used. This is known as resonance structures
Define octet rule, formal charge
The Octet rule refers to the fact that the configuration of noble elements is the stablest valence electron configuration, due to energy factors other elements will try to achieve this stability of 8 valence electrons through bonding, ionising et cetera
Define temperature (both C and K), gas P and weight
Celsius and Kelvin both have the same unit magnitude. Celsius is defined by the freezing point and vaporising points of water (0° and 100° respectively). Kelvin is an absolute scale, beginning at 0° K (no heat energy). 0°K = -273.15°C.
Gas pressure is the pressure exerted on the walls of the container in which this gas is placed. At constant temperature pressure is inversely related to volume (P1V1 = P2V2) , at constant volume directly related to temperature. (P1V1 / T1 = P2V2 / T2).
The weight of a gas can be calculated by the number (N) of molecules present and vice versa
Define STP, ideal gas, deviation
Standard Temperature and Pressure of a gas is 0°C and 1 atm (760 mmHg)
Define H bonds, dipole forces
Hydrogen bonds are intermolecular forces which occur whenever hydrogen is covalently bonded to an atom which attracts electrons strongly. In particular O, N and F. This molecules become very polar - stronger than usual cases of dipole dipole interaction.
Dipole dipole forces are basically the intermolecular forces between polar molecules.
London forces are intermolecular forces which occur spontaneously in molecules which aren’t “formally” polar, due to random movement of electrons. These three forces are all called Van der Wall forces
Define saturated, supersaturated, nonvolatile
A solution is said to be saturated when under normal conditions no more solute can be dissolved into the solute - adding more solute leads to precipitation.
Supersaturation is where the usual limit of saturation is exceeded. Can be achieved for example by lowering temperature and not disturbing solution.
Non volatile is used to describe solutes which cannot evaporate
Common anions and cations in solution?
Common anions in solution are:
F-, Cl-, Br-, I-, O2-, S2-, N3-, OH-, NO3-, ClO4-, CO3(2-), SO4(2-), PO4(3-), CH3CO2-
Common cations in solution are:
Na+, Li+, K+, NH4+, H3O+, H+, Ca2+, Mg2+, Fe2+, Fe3+
Units of concentration?
M = MolaRity = # moles solute / litRe
m = MolaLity = # moles solute / kiLogram
N = Normality = Equivalence (number of reacting units) / litre
ρ = Density = mass per unit volume
Osm = Osmole = number of moles of particles that contribute to the osmotic pressure of a solution
Osmolarity = osmoles / litres solution
Osmolality = osmoles / kg solution