AP Chemistry Sem 1 Final Concepts
Pyramidal
3 bonds, 1 lone pair; about 109.5 degrees
T-shaped
3 bonds, 2 lone pairs; 90, 180
Trigonal Planar
3 domains
Seesaw
4 bonds, 1 lone pair; 120, 90, 180
Square planar
4 bonds, 2 lone pairs; 90
Tetrahedral
4 domains
square pyramidal
5 bonds, 1 lone pair; 90
Bipyramidal
5 domains
Acid-base reaction
a reaction where an acid reacts with a base to produce water and a salt
ionization energy trend
decreases from top to bottom in a group; increases from left to right in a period
Polar
non-symmetrical; bent, trig pyramidal
Electron affinity trend
not much change down a group; increases from left to right in a period
JJ Thompson
studied electrical discharges in partially evacuate tubes called cathode-ray tubes, postulated the ray was a stream of negatively charged particles called electrons, plum pudding model
Rutherford
tested Thompson's plum pudding model and found it incorrect, founded the nuclear atom- atom with a dense center of positive charge with electrons moving around the nucleus at a distance that is large relative to the nuclear radius
Bond length
the average distance between the nuclei of two bonded atoms
Electron affinity
the change associated with the addition of an electron to a gaseous atom
Oxidation state
the condition of an atom expressed by the number of electrons that the atom needs to reach its elemental form
Lattice energy
the energy change occurring when separated gaseous ions are packed together to form an ionic solid
Specific heat
The amount of energy required to raise the temperature of 1 gram of a substance by 1 degree Celcius
ionization energy
The amount of energy required to remove an electron from an atom
effective nuclear charge (Zeff)
the pulling force that a valence electron actually feels from the nucleus; affects electron affinity, ionization energy, atomic radius
Electronegativity
the tendency of an atom in a molecule to attract shared electrons to itself
Molecular polarity
the uneven distribution of molecular charge
Heisenberg uncertainty principle
there is a fundamental limitation to just how precisely we can know both the position and momentum of a particle at a given time
Polar
unlike atoms bonded; tetrahedral, linear, trigonal planar
Bent
2 bonds, 1 lone pair; 120 degrees
Bent
2 bonds, 2 lone pairs; about 109.5 degrees
Linear
2 bonds, 3 lone pairs; 180
Linear
2 domains
Octehedral
6 domains
Redox reaction
A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation-reduction reaction.
Aufbau Principle
An electron occupies the lowest-energy orbital that can receive it
Atomic radius trend
Increases from top to bottom down a group, decreases from left to right in a period
Oxidizing agent
The electron acceptor in a redox reaction.
Reducing agent
The electron donor in a redox reaction.
negative and exothermic
When an electron moves from excited state to ground state, the energy change is ____
positive and endothermic
When an electron moves from ground state to excited state, the energy change is ____
Precipitate reaction
a double replacement reaction that produces an insoluble solid
n-1 / shape
angular momentum quantum number (l)
Schrodinger
attacked the problem of atomic structure by giving emphasis to the wave properties of an electorn
Millikan
by using oil drops, determined the magnitude of the electron charge and calculated the mass of an electron
f orbitals
complex : 7 : 14 electrons
Einstein
derived the theory of relativity
Quantum theory
describes matter behaves as particles and waves
Bohr
developed the quantum model for the hydrogen atom
Chadwick
discovered the neutron
p orbitals
dumbbell shaped : 3 : 6 electrons
Coulomb's Law
electric force between charged objects depends on the distance between the objects and the magnitude of the charges; affects ionization energy and atomic radius
Bond strength
energy required to break a bond
d orbitals
flower shape : 5 : 10 electrons
Reduced
gains electrons, oxidation state decreases
Nonpolar
like atoms bonded; tetrahedral, linear, trigonal planar
Oxidized
loses electrons, oxidation state increases
between l and -1 / orientation in space
magnetic quantum number (ml)
-1/2 and 1/2 / spin
magnetic spin quantum number (ms)
Quantum numbers
n, l, ml, ms
Atomic radius
one-half the distance between the nuclei of identical atoms that are bonded together
Debroglie
originated the idea that the electron, previously considered to be a particle, also shows wave properties
integral values: 1,2,3... / size and energy
principal quantum number (n)
s orbitals
spherical : 1 : 2 electrons
