C2.1 Structure and Bonding Flashcards
What is the charge of an electron?
Negative (-1)
What is the charge of a neutron?
Neutral / No charge (0)
What is the charge of a proton?
Positive (+1)
What is the rule for shell capacity?
2,8,8,2
What are the subatomic particles?
Protons, electrons and neutrons
Define ionic bonding.
The bonding between metals and non-metals.
Define covalent bonding.
The bonding between non-metals.
Explain metallic bonding
Metallic bonding is the bonding between two metals. Electrons from the outer shell of the metal atom are delocalised (free) and become attracted to the metal ion (a ‘charged’ atom due to the loss or gain of electrons). The electrons and ion bond because of the electrostatic force of attraction between the negatively charged delocalised electrons and the positively charged metal ions.
What is electrostatic force of attraction?
The force of attraction between negative electrons and positive ions
Why are some metals malleable?
Some metals are malleable because they are constructed in layers. These layers can slide over each other meaning the metal will bend / change shape.
Explain ionic bonding.
Ionic bonding is the bonding between metals and non metals. The metal atom becomes a positively charged ion due to the fact it has lost an electron. The non metal atom becomes a negatively charged ion as it has gained an electron. Therefore the ions are attracted to each other (bond) because of the electrostatic forces of attraction between the oppositely charged ions.
Explain covalent bonding.
Covalent bonding is the bonding between two non metals. The non metals share the required amount of electrons between each other so they both have full outer shells. For example: Hydrogen has 1 electron & Chlorine has 17. To fill Chlorine’s shell, hydrogen shares it’s 1 electron with chlorine to make 18 (8 on the outer shell - a full capacity).
whats 9 + 10
21
