Unit 1: Periodic Table Flashcards
Atomic Number
No. of protons
Relative Atomic Mass
Protons + Neutrons mass/Nucleolus mass
Isotopes
Same element with different Mass no/R. atomic mass (or changes in no of neutrons)
Excited Electrons
When electrons gain enough energy to jump shells
What happens with an Electron returns to its shell after jumping shells?
It produces an Electromagnetic wave that leads to Electromagnetic Radiation.
It can be heat, light, ultraviolet waves, etc.
Ionisation
The act of an electron gaining enough energy to move out of the atom
Ionizing Radiation
An energy that ionizes an atom or removes an electron
Give an example of Ionizing Radiation
X-rays
They penetrate our bodies by removing electrons from the area they pass
Also present in soil, water and vegetation
Why do groups have similar properties?
They have the same no. of electrons
Physical Properties of Metals
Good conductors
High melting and boiling points
Metallic Luster (shiny)
Malleable and Ductile (can turn into wires) - because of crystalline atomic structure
Sonorous
Durable (varies)
Best and Worst Metal Conductors
Best - Silver (Ag) and Copper (Cu)
Worst - Lead (Pb) and Mercury (Hg)
Chemical Properties of Metals
High Density
Reacts with Oxygen (some burn and some oxidize)
Form positive ion (because they’re more likely to donate electrons given their low valency)
Comment on the Lattice of a Metal
Solid metals are a lattice of positively charged nuclei in a ‘sea’ of mobile electrons or delocalised electrons.
This is what makes metals so conductive, because the delocalised electrons move freely and carry electricity.
What state are Metals found in?
Solid (- Mercury in Liquid)
What state are Non-Metals found in?
All (maybe more gases)
Main Properties of Non-Metals
Opposite of Metals
Good Insulators
Name all the Metals in the Periodic Table
Metals, Transition Metals, Non-metals, Metalloids