C3 - Structure and bonding 1️⃣✅
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What bonding occurs between a metal and non-metal?
Ionic bonds
What bonding occurs between a non-metal and a non-metal?
Covalent bonds
What bonding occurs between a metal and a metal?
Metalic bonds
What is ammonia?
A compound containing the elements nitrogen and hydrogen NH3
What is ionic bonding?
Ionic bonding is when a non-metal and a metal react together, one element looses electrons in order to make the other elements outer shell full
What is covalent bonding?
Covalent bonding is when a non-metal and a non-metal share electrons to complete each others outer shell
What is metallic bonding?
Metallic bonding is the electrostatic attraction between the positive metal ions and the free moving delocalised electrons
What are the 2 allotropes of carbon?
Diamond and graphite
Why is melting a ionic substance so difficult?
Because ionic substances have a regular repeating and strong structure with many bonds, in order to melt the substance, you would have to break all the bonds. Therefore the melting point is very high as breaking all of the bonds takes a very long time
What is the structure of ionic substances?
Giant ionic lattice (regular, repeating pattern, like covalent ionic bonds are strong)
How do you calculate mr?
You do the elements mass number x its occurrence for however many elements there are and then add them together
What is a single bond?
When each atom shares one pair of electrons
What is a double bond?
When each atom shares two pairs of electrons
What ions do group 1 form?
1+
What ions do group 2 form?
2+
What ions do group 3 form?
3+
What ions do group 4 form?
They do no t form ions
What ions do group 5 form?
3-
What ions do group 6 from?
2-
What ions do group 7 form?
1-
What ions do group 0 form?
They do not form ions as they already have full outer shells so there are no free spaces for a bond
When you melt a substance are what are you actually melting?
You arent melting the strong bonds as they are way too strong, you are actually melting the weak intermolecular forces that hold together the strong bonds. The bigger the molecule the bigger/ stronger the intermolecular forces are, therefore, the higher the melting point
What are the properties of diamond?
• Each carbon covalently bonded to 4 other carbons therefore no free delocalised electrons • lots of strong bonds • melting point of 4000℃ • doesn’t conduct electricity because no spare delocalised electrons • hard & sparkly
What are the properties of graphite?
• Each carbon covalently bonded to 3 other carbons therefore one (delocalised) electron left • delocalised electrons hold layers together so not bonded • melting point of 3600℃ • conducts electricity because of free delocalised electrons • brittle and breaks easily • slippery & layers can slide