1.2 Bonding
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Molecular ion
Charged particle containing more than one atom
Ion
Charged particle formed when an atom gains or loses electrons
Cation
Positively charged ion
Anion
Negatively charged ion
If an ion loses an electron what charge does it have?
Positive +
If an ion gains an electron what charge does it have?
Negative -
Where does ionic bonding take place?
In metals and non metals in groups 1, 2, 6, 7
Ionic bonding
• between metals and non metals • involves attraction between oppositely charged ions • ionic bonds are strong and substantial energy is required to break them • is typical of metal compounds
What are single covalent bonds?
A shared pair of electrons between two non metals
Covalent bonding
• non metal elements and compounds • covalent bonds are strong and substantial energy is required to break them
Molecule
Contains 2 or more atoms covalently bonded
Diatomic
Means there are 2 atoms covalently bonded in the molecule
How can a covalent bond be represented?
Dot and cross diagram, or in the structural format with lines between elements eg Cl-Cl
What are the lone pairs in covalent bond diagrams?
The electrons that stay the same and aren’t shared
What are the bonding pairs in covalent bond diagrams?
The electrons in the middle which share with other elements
What is metallic bonding?
The attraction between delocalised electrons and the positive ions in a regular lattice that happen in metals
Metallic bonding diagram
Regular rows of ions of the element with delocalised electrons around it depending on how many are lost per ion
How are ions formed?
When one element doesn’t have enough/too many electrons in its outer shell, it can take/give them to another element which also needs the same amount to complete its outer shell as elements are more stable this way