Topic 1 - Atomic Structure And The Periodic Table Flashcards
Mass and charge of the particles
Proton, 1, +1
Neutron, 1, 0
Electron, very small (1/1838), -1
What makes an ion different to an atom
The number of electrons are different to the number of protons
How big is an atom
0.1 nanometers
What determines the size of the atom?
The volume of orbit of the electrons
What is an element
This is a substance made up of atoms that all have the same number of protons in their nucleus
Out of the three particles, which one determines what atom it is?
The number of protons in the nucleus
If the neutrons or electron number changes, it is still the same atom
What makes an isotope?
What changes in the atomic and mass numbers?
Different forms of the same element with a different number of electrons
Same atomic number, different mass number
Name two common isotopes
Carbon - 12
Carbon - 13
Why is the relative atom mass used instead of the mass number when referring to an element as a whole
Because many elements can exist as a number of different isotopes
What is the relative atomic mass formula
Relative atomic mass =
Sum of (isotope abundance X isotope mass number)
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Sum of abundance of all isotopes
When is a compound formed
When elements react with other elements
What is a compound
A substance formed from 2 or more elements
What holds compounds together
Chemical bonds
What are the three ways bonds are made
By giving away, taking or sharing electrons
What is required in ionic, covalent and metallic bonding
Metals and non metals
Ionic: metal + non-metal
Covalent: non-metal + non-metal
Metallic: metal + metal