PCP Flashcards
(29 cards)
This theory states that elements are composed of atoms.
Dalton’s Atomic Theory
A law stating that the ratio of the mass of an element to the mass of the other element is a whole number or simple fraction.
Law of Multiple Proportions
A law stating that a chemical reaction only involves separation, combination, or rearrangement of atoms.
Law of Conservation of Mass
A law stating that a pure compound is made up of elements in the same proportion by mass.
Law of Definite Proportions
Number of protons in nucleus.
Atomic number
Total number of protons and neutrons in nucleus.
Mass number
Atoms with the same atomic number but different mass numbers.
Isotopes
Average of the atomic masses of isotopes based on their %abundance.
Average Atomic Mass
Enumerate the 4 quantum numbers and briefly describe it.
- Principal QN (n)
- distance of electron from nucleus
- energy level
- corresponds to the row in periodic table
- n = 1,2,3, etc. - Azimuthal/Angular Momentum QN (l)
- shape of orbital
- l = 0 to (n-1)
- s, p, d, f (spherical, dumbbell, rosette, undefined) - Magnetic QN (m_l)
- orientation of orbitals in space
- (-l) to 0 to (+l) - Spin QN (m_s)
- spin of electrons
- (+ 1/2) clockwise, (- 1/2) counterclockwise
A principle stating that orbitals must be filled in increasing energy levels.
Aufbau Principle
A principle stating that no 2 electrons can have the same set of quantum number, and an orbital can have a maximum of 2 electrons with opposite spins.
Pauli’s Exclusion Principle
The most stable arrangement of electrons in subshell is one with more parallel spins.
Hund’s Rule of Multiplicity
Law stating that properties of elements are functions of their atomic numbers.
Modern Periodic Law
This is the average distance between the nucleus and valence electron.
Atomic Size or Atomic Radius
The energy required to remove an electron in its ground state. The lower this energy, the easier it is to form a cation.
Ionization Energy
The change in energy when an anion is formed.
Electron Affinity
Ability of an atom to attract towards itself a bonding electron.
Electronegativity
Energy associated with the formation and breaking of bonds.
Bond Energy
Measures the distance between the nuclei of the atoms.
Bond Length
Refers to single/double/triple bonds and its intermediate bonds.
Bond Order
A theory stating that formation of a bond is due to the overlap of 2 atomic orbitals.
Valence Bond Theory
The electron in the bonding orbital is greater than the electron in the non-bonding orbital.
Molecular Orbital Theory
A type of property that is dependent on the amount.
Extensive Property
A type of property that is independent of the amount.
Intensive Property
