Inorganic chem lec: quiz 3

atomic theory, quantum numbers, electric charge

principal

distance from the nucleus

angular/azimuthal

shape of the orbitals

magnetic

spatial orientation

spin

spin of electrons

possible directions

democritus

“atomos”/atom - “indivisible”

aristotle

5 elements - fire, water, earth, air, aether

john dalton

1. That the elements are made up of very small, indivisible particles called atoms. These atoms are the smallest particles of a substance that take part in a chemical reaction. (We know that atoms can be split)

2. That the atoms of particular elements are the same in size, chemical properties, and weight. (We now know of the existence of atoms of the same element which differ in weight -- called isotopes).

3. That the atoms of the different elements differ in size, chemical properties, and weights. (We also know that there are atoms of different elements that have the same weights -- the isobars).

4. That atom of the same elements unite to form molecules of that elements such as H₂, N₂, O₂; and atoms of different elements unite to form molecules of compounds such as CO₂, KOH, NaCl, and H₂ (The formation of molecules is due to some chemical affinity or attraction of atoms of different elements for each other.)

5. That chemical combination between two or more elements consists in the union of the atoms of these elements in simple numerical ratios to form the smallest possible unit particles of a compound called molecules.

6. Atoms of the same elements can unite in more than one ratio to form more than one compound.

isotopes

same elements, different mass/weight

isobars

diff elements, same weight

JJ thomson

electrons

cathode rays

plum pudding

ernest rutherford

protons

gold foil

niels bohr

planetary model

fixed orbits

erwin schrodinger

quantum mechanical models

cathode rays

steams of electrons between electrodes

quantum mechanical model

propability of finding electrons within given orbitals or 3-D response of space within an atom

Aufbau Principle

In filling orbitals with electrons, atomic orbitals of low energy are filled first, and then proceed to orbitals of higher energy.

Pauli’s Exclusion Principle

Only two electrons can fill each orbital with an opposite spin

Hund’s Rule of Maximum Multiplicity

Electrons are distributed among the orbitals of a sublevel in a way that gives the maximum number of unpaired electrons with parallel spin

Atomic number

refers to the number of proton/s inside the nucleus.

atom

smallest unit of an element that has the properties of the element.

Nucleus

the small, dense center of positive charge in the atoms.

Neutron

uncharged particle

Proton

positively charged particle

neutron and proton

The nucleus contains two types of stable particles, which comprise most of the mass of an atom.

Mass number

refers to the sum of the number of proton/s and neutron/s inside the nucleus

Atomic mass or atomic weight

the weighted average of the mass of all naturally occurring isotopes of a particular element reported in atomic mass unit (amu).