Science Atoms Study

1: The atom
Introduction
Atoms are the building blocks for matter
Everything is made up of atoms
1A: Sub-atomic particles
Atoms are made up of 3 sub-atomic particles, 2 of which are located in the nucleus (the heart of the atom)
Positively charges protons and neutrally charged (non-charged) neutrons are found in the nucleus
Negatively charged electrons are located orbiting the nucleus in shells. They stay in orbit because the electrons are attracted to the protons

2: The Element
Introduction
An element is a singular type of atom, like candy in a candy shop
If there is an atom that has 8 protons and 8 electrons, then it is an oxygen element. If it has 1 proton and 1 electron, then it is a hydrogen element
3: Molecules
Introduction
A molecule is where elements come together to stabilsie, either with the same or different elements.
1A: Compounds
A compound is where different elements come together to stabilsie Hydrogen and Oxygen = Water
4: History of the atom
4A: Democridus
Solid-ball model
First to use the term, ‘atomos’ meaning invisible
A point in matter where you can not break it down any further

4B: John Dalton – 1808
Atomic Theory
Atoms cannot be subdivided
Atoms can not be created or destroyed
All matter is made up of tiny particles called atoms
All toms of a given element are alike, but are different from the atoms of any other element
4C: Dynamide model - 1904
Described atoms as mostly empty spaces filled with fast-moving ‘dynamides’. These were neutrally charged particles made up of a heavy positive particle stuck to a light negative particle.

4D: Joseph John Thompson – 1897
Plum Pudding model – a round ball of positive charge with negative electrons embedded in it
Discovered the electron and its negative charge
4E: Earnest Rutherford – 1911
Nuclear model – positive charged nucleus surrounded by a large space occupied by negative electrons

4F: Niels Bohr – 1913
Planetary model – model of the planetary model, which can be called the rutherford-bohr model.
Proposed that electrons travel in orbits and each orbit has a different energy level
4G: James Chadwick – 1932
Discovered neutrons and added them to the nucleus of the rutherford-bohr model
Model that we use today in schools as it is the easiest to draw
4H: Electron cloud model
Electrons form clouds around the nucleus. Scientists can predict the shape of these clouds (orbital) but never the exact location of the electrons within them
5: Isotopes and Ions
5A: Isotopes
Isotopes are the same element with the same amount of protons and electrons but different amounts of neutrons
5B: Ions
Ions are elements that have gained or lost electrons in order to achieve a full outer shell.
6: Periodic Table
6A: Atomic number & weight

6B: Groups and Periods
Groups show the amount of electrons in the shell
Groups also show similar properties
Periods show the amount of shells – period 3, 3 shells
6C: Nobel gases
Nobel gases have full outer shells, meaning they do not form molecules and compounds
They are located in group 18 – furthest to the right