Inorganic Flashcards
Binding energy
Energy used to bind the nucleus of an atom and overcome the proton-proton repulsion
This energy is the reason that the atomic mass of an atom is slightly less than the sum the masses of its constituent protons, neutrons, and electrons
Mass Number (A)
The total number of protons and neutrons in the nucleus
Atomic Number (Z)
Total number of protons in the nucleus
Alpha particle
4/2 He
Or helium nucleus
Normal beta particle
An electron ejected from neutron
A neutron is converted to a proton and an electron
Electron capture
A proton and an electron fuse to make a neutron
Positron Emission
Proton breaks down into a neutron and a positron
Gamma emission
And excited atom releases a Gamma Ray Photon
Transmutation
Process where one element is transformed into another
Primary quantum number, n
The energy level or shell of an orbital
Secondary quantum number, l
The angular momentum of an electron in an orbital. This describes the shape of an orbital
l = 0, s orbital
l = 1, p orbital
l = 2, d orbital
l = 3, f orbital
l = 4+, proceed in alphabetical order after f
Magnetic quantum number, ml
The subshells of a particular orbital are further divided into electron orbitals
s orbitals have 1
p orbitals have 3
d orbitals have 5
f orbitals have 7
Spin quantum number, ms
Each orbital can hold two electrons, the two electrons will have opposite spins given by the Spin Quantum Number.
ms = +1/2 or -1/2
Pauli exclusion principle
The principle states that no two electrons of the same atom will have completely identical quantum numbers (n, l, ml, ms).
Aufbau principal
To find the correct ground state electric configuration of an atom, always completely fill the lower energy orbitals before filling any higher energy orbitals.
Hund’s rule
When feeling degenerate orbitals for p, d, or f subshells always put one electron in all available orbitals, before pairing two electrons in the same subshell.
Exceptions to Aufbau principle and transition metal ions
The Aufbau principle can be violated as extra stabilization can be achieved when a d orbital is half or completely filled. (s electrons may be promoted to d orbital)
Transition metals will lose valence s electrons before losing any d electrons.
N-type conductor
A semiconductor that is doped with atoms that contain an extra e-
e- can be released which initiates a current
D-band is slightly below the Conductor Band
Group 5: P
Group 7: At
P-type conductor
A semiconductor that is doped with atoms that contain an empty p-orbital
e- can be accepted which initiates a current
A-band is slightly above the Valence Band
Group 3: B, Ga
Intrinsic semiconductor
A material where the CB is at a higher E level that the VB. Heat may be applied to cause an e- in the VB to jump to the CB.
Applying a current will cause e- to flow through the material as e- will move to fill the holes.
Extrinsic semiconductor
A material that is normally an insulator, that was made to be a semiconductor by doping the crystal lattice
Coulomb’s Law
F = (kQ1Q2)/r^2
k = 9.010^9 N(m^2)/(C^2)
If:
F<0, force is attractive.
F>0, force is repulsive.
Repulsive forces
e- cloud repulsion (or steric hindrance)
Cohesive forces
- ionic forces
- dipole forces (force is proportional to Q1*Q2)
- london dispersion forces (results from two instantaneous dipoles of atoms in close proximity)
Unit cell
The smallest repeating unit of a crystal lattice
Lattice energy (U)
The energy of electrostatic interactions of a crystal
Ionic solids
A solid composed of cations and anions
Covalent solids
Solid composed of atoms that are held together by very strong covalent bonds
Molecular solids
A solid composed of neutral molecules
Ex: H2O, sucrose, I2, P4
Metallic solids
Solid composed of a closely packed metal element
T-hole
An atom fills this void to make a tetrahedron
O-hole
An atom fills this void to make an octahedron
Cubic closest packed
Length = 2r
Volume = 8(r^3)
Body centered cubic cell
Length = 4/(sqrt(3))*r
Volume = 64/3(sqrt(3))*(r^3)
Face centered cell
Length = 4/(sqrt(2))*r
Volume = 32/(sqrt(2))*(r^3)
Radius of the nucleus
r = (1.33•10^-13)(A^(1/3)) cm
- A = mass number
Consequences of lattice energy
1) Thermal stability
- Generally large cations are stabilized by large anions and vice versa
2) High ox. #s and small ions
- Cations with high ox. #s are stabilized by small anions (allows for shorter bond length)
3) Solubility
- In general, compounds that contain ions with widely different radii are generally soluble in H2O (MgSO4, and BaOH are water soluble)
Le Chatelier’s Principal
The eq point can be disturbed by:
1) Concention
- add to reactance equals shift to products
- remove reactance equals shift to reactants
2) Pressure
- Increase pressure equals shift to the side with less gas molecules
- Decrease Pressure equals shift two the side with more gas molecules
3) Temperature
- If DeltaH > 0, heat is a reactant. Increase or reduce temperature fix EQ as rule #1
- Changing T is the only way to change EQ constant (K)
Amphoteric molecule/ion
A molecule/ion that will act either as an acid or a base, depending on the conditions of the solution that it is in
HCO3
Acidic: HCO3 + H -> H2CO3
Basic: HCO3 + OH -> CO3 + H2O
Strong acids
HCl HBr HI HNO3 H2SO4 HClO4
Strong bases
LiOH
NaOH
KOH
pH equations
pH + pOH = 14
pH = pKa + log([A-]/[HA])
pOH = pKb + log([HA]/[A-])
pH calculations
If the [acid] or [base] is 3 orders of magnitude greater than the Ka or Kb value, then you can exclude x from the denominator
K = (x^2)/(M - x) -> (x^2)/M
When do acid-base indicators change color?
At pH +/- 1 of their pka
H-Indicator —> H+ + Indicator-
Red) (Yellow
At what point of a titration curve does the pH = pKa?
Halfway to the equivalence point.
[HA] = [A-], so..
Henderson Hasselbach: pH = pKa
Borane classes:
Closoboranes: BnHn
Nidoboranes: BnH(n+4)
Arachnoboranes: BnH(n+6)
Most reactive noble gas
Xenon
XeF2 XeF4 XeF6
Xe is also know to bond with C, N, and O.
Solubility in H2O
MgCO3 vs BaCO3
MgOH vs BaOH
MgCO3 is more soluble in water then BaCO3
- Ba has a more similar radius to CO3(-2) so it is not water soluble
BaOH is more soluble in water than MgOH
