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