Chemistry 11

Atomic number(location)

lower left corner

Atomic number(definition)

the number of protons in an atom

oxidation state/charge(location)

Upper right corner

electron configuration(location)

lower left corner (under atomic number)

electron configuration(definition)

the way electrons are arranged in an atom

average atomic mass(location)

upper left corner

average atomic mass(definition)

the weighted average of all the isotopes of an element

atomic symbol

One or a two letter abbreviation that represents an element

average atomic mass(formula)

AAM amu=(relative abundance X mass #) + (relative abundance X mass #)

aufbau principle (3 rules)

1. within any PEL the s-sublevel is always the lowest energy
2.electrons enter orbitals in order of least to most potentially energy(inner to outer)
3.orbitals in the same sublevel have the same energy as eachother

Pauli's exclusion principal

isotope

atoms of the same element with the same number of protons and different numbers of electrons( they have different masses)

rutherford model of an atom

has electrons and protons(no neutrons) protons are in the nucleus and the electrons are just floating around in empty space

bohr model

has protons and electrons(no neutrons) protons are in the nucleus and electrons are held in quantized PELs and orbit the nucleus

PEL

principal energy level

the isotope used as a standard in order to define amu

C-12

AMU

atomic mass unit

valance electron

the number of electrons on the outermost PEL

The scientist who developed the Plum Pudding model

JJ Thomson

Daltons atomic theory

The idea that atoms are tiny indivisible particles that can physically or chemically combine. They are identical to each other and different from other elements. (cannonball model)

Coordinate covalent bond

a type of alternate covalent bond that is formed by sharing of electron pair from a single atom

Covalent bond

A bond that consists of the mutual sharing of one or more pairs of electrons between two atoms

Diamagnetic

A substance that does not have unpaired electrons and is not attracted to a magnetic field

Paramagnetic

materials that tend to get weakly magnetized in the direction of the magnetizing field when placed in a magnetic field

Ferromagnetic

the basic method in which a compound forms a permanent magnet or is attracted to a magnetic field

Molecular orbital

the molecular orbital theory states that each atom tends to combine together and form molecular orbitals

Bonding orbital

Orbitals that are formed when atomic orbitals combine in ways that lead to predominantly constructive interference

Antibonding orbital

a type of molecular orbital that weakens the chemical bond between two atoms and helps to raise the energy of the molecule relative to the separated atoms

Sigma bond

The covalent bond formed by the coaxial overlap of atomic orbitals

Pi bond

covalent bonds that involve the lateral overlapping of two lobes of an atomic orbital with two lobes of another atomic orbital that belongs to a different atom

Hybrid orbital

orbitals that each have partial s character and partial p character

Polarity

The distribution of electrical charge over the atoms connected by the bond

Electronegativity

a chemical property that describes the tendency of an atom or a functional group to attract electrons toward itself

Nonpolar covalent bond

a type of chemical bond that is formed when electrons are shared equally between two atoms

Polar covalent bond

A covalent bond in which the electron density is unevenly shared between the two bonded atoms, due to a difference in electronegativity or due to inductive effects