The Periodic Table Periodic Table Elements - Atomic Number
- Average Atomic Mass
- Mass number Isotopes - Isotope
- Isotope Symbol Ions - Ion
- Cation
- Anion Atomic Model - John Dalton's model
- Ernest Rutherford's model
- J.J. Thomson's model
- Niels Bohr's model
- Atomic Number The atomic number increases as you move to the right and down the periodic table. It tells you how many protons are in an element. Average Atomic Mass The average atomic mass is the average mass of all the ions of each element. Mass Number The mass number is the amount of protons and neutrons. The electrons only effect the mass number slightly because they are so small. Isotope An isotope is when the same element has different amount of neutrons, which changes the atomic mass. Isotope Symbol The charge is the number of neutrons minus the number of protons. Anion An Ion is an element with a charge Ion An anion is when there are more electrons than protons. Cation A Cation is when there are fewer electrons then protons John Dalton's model Solid sphere model
The five postulates of Atomic Theory
All matter is made of atoms
All atoms with the same element are alike
Atoms are indivisible
Atoms combine in whole number ratios to make compounds
Atoms rearrange in chemical reactions Ernest Rutherford's model - A positive nucleus
- Nucleus is surrounded by negatively charged electrons
- most mass was in nucleus
- most of an atom is empty space
-Gold foil experiment Niels Bohr's model - Electrons move in stationary orbits Gold Foil Experiment Using a particle emitter, Rutherford shot particles into a sheet of gold foil. Behind the sheet, there was a sensor that recorded the particles that pass through. at an angle, he placed another sensor. A majority of the particles went through the golf foil, while some were reflected off. J.J. Thomson's model - Used a cathode ray tube
- The light is repelled by the negative end of the magnet
- The beam of light is negatively charged with electrons Atomic Particles -Protons
-Neutrons
-Electrons The Periodic Table - Metals
-Non-metals
-Metalloid
-Trend
-Reactivity
-Electronegativity
- Electron affinity
- Ionization
- Effective nuclear Charge
- Coulomic Attraction
- Family vs. Period Protons - Positively Charged Particle
- Inside atom nucleus Neutron -Neutral particle
- Inside atom nucleus Electron - Negatively charged particle
- Orbits atom nucleus
- Very small compared to protons/ neutrons Electron Principles -Puali's exclusion principle
- Hund's rule
- Aufbua Principle Puali's Exclusion Principle Electrons in the same orbital repel and spin in opposite dirctions Hund's Rule Electrons fill empty orbitals in a sub level before they pair up. Aufbau Principle Electrons fill sub levels of lowest energy first. Configurations - Orbital Diagram
-Electron configuration
- Nobel gas configuration Orbital Diagram - A representation of the electrons in each orbital/ energy sun level
- Shows direction of electrons Electron Configuration - Shows amount of electrons in each energy level Noble Gas Configuration - A simplified version of the electron configuration, but uses noble gasses as a checkpoint/ landmark Metals -Majority of PT
- Conducts electricity Non-Metals -Right side of PT Metalloids Have characteristics of both Metals and non-metals Trends -Reactivity
-Atomic Radius
- Electronegativity
-Ionization Energy
-Atomic Mass
-Atomic # Electronegativity The tendency to attract electrons Electron Affinity The amount of energy released when electron is added to a neutral atom Ionization The amount of energy to move an electron Effective Nuclear Charge - The "net" charge of an element
- Number of protons minus number of non-valence electrons Coulobic Attraction -The force generated by the protons and the electrons in an atom (attraction)
-Opposite forces attract Valence Electron -The electron(s) in the outer most orbital
- used for bonding Family vs. Period -Period= rows
-Family= columns
