Concepts Flashcards
Bohr Model
A hydrogen atom consists of a central proton around which an electron travels in a circular orbit, centripetal force, and electrical force, electrons can only exist in fixed-energy states
Heisenberg Uncertainty Principle
Impossible to simultaneously determine the momentum and the position of an electron
Pauli Exclusion Principle
No two electrons in a given atom can possess the same four quantum numbers
Principal Quantum Number
n, represents the shell where an electron is present in an atom, the element’s row (N -> 1,2)
Quantum Numbers
n, l, ml, ms
Magnetic Quantum Number
ml, the orientation of the orbital in space (i.e. p subshell (-1,0,+1)
Spin Quantum Number
ms, spin of a particle up or down, (+1/2, -1/2)
Paired Electron
Electrons with opposite spins, different ms, but the same ml
Aufbau Principle
Subshells are filled from lowest to highest energy
Phase Diagram
Right (Gas), Left (Solid), Middle (Liquid), Critical Point (Top of l/g)
Hund’s Rule
Electrons prefer empty orbitals to half-filled ones
Raoult’s Law
Vapor pressure of a pure solvent is equal to the product of the mole fraction of the solvent and the vapor pressure of the solvent
Paramagnetic
A material has unpaired electrons, the magnetic field will align the spins
Boyle’s Law
P1V1 = P2V2
Charles Law
V1/T1 = V2/T2
Nuclear Effective (Zeff)
Net positive charge from the nucleus as felt by an electron, max at top right of PT
Ionization Energy
The energy required to remove an electron from an atom, max at top right PT
Atomic Radius Trend
Decreases up/right, Largest Bottom Left, Smallest Top Right
Electronegativity Trend
Increasing Up/Right, Highest Top Right
Soluble Salts
SO4-2, Cl-, Br-, I-, NH4+, Alkali metals
Insoluble Salts
Metal oxides, hydroxides, salts with CO3-2, PO4-3, SO3-2
Combination Reactions
Two or more reactants form one product
Decomposition Reactions
A compound breaks down into two or more substances (electrolysis
Spectator Ions
Ions do not take part in the chemical reaction
Double-Displacement Reaction
Elements from two different compounds displace each other to form two new compounds
Oxidation Electrode
Anode
Reduction Electrode
Cathode
Electrolytic Cell
Nonspontaneous, electrical energy required, same container, no salt bridge, presence of a battery or power source used to drive nonspontaneous reactions
Lewis Acid
Electron-pair acceptor
Lewis Base
Electron-pair donor
Bronsted Acid
Donates protons
Bronsted Base
Accepts Protons
Alpha Decay
A-4, Z-2
Beta (-) Decay
A, Z+1
Gamma Decay
No change, emission of gamma particle (high-energy photon)
Electron Capture
A, Z-1 (add e-)
Le Chetelier’s Principle
Stress on an environment:
1. Concentration -> shift to relieve pressure
2. Pressure -> shift decrease moles
3. Temperature -> heat as a product/reactant
Bond-Dissociation
Energy required to break a specific chemical bond in one mole of a gaseous molecule, bond breaking is endothermic
Titrations
- Strong acid/base of known concentration
- Titrate added in small amounts
- Neutral = equivalents equal
- SB/SA -> pH 7
- SB/WA -> above pH 7
- WB/SA -> below pH 7
Nerst Equation
Potential under non-standard conditions
Galvanic Cell
Supply energy, used to do work, separate containers for oxidation and reduction half-reactions, connected by an apparatus, allow flow of electrons
Angular Momentum Quantum Number
l, the shape of the orbitals (0(s),1(p), 2(d), 3(f))
Isobaric
Constant pressure
Isochoric
Constant volume
Isothermal
No temperature change
Adiabatic
No heat exchange
Deposition
Gas to solid
Sublimation
Solid to gas
Avogadro’s Principle
n1/V1 = n2/V2
Ideal Gas Law
PV = nRT
Beta (+) Decay
A, Z-1
