bonding and structure
- Created by: issy12345678910
- Created on: 29-05-19 15:36
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- Bonding and structure
- Ionic Bonding
- metal and non-metal
- the metal atom loses an electron to form a positive ion
- the oppositely charged ions are strongly attracted to each other by electrostatic charges
- the non-metal gains these electrons to form a negatively charged ion.
- the oppositely charged ions are strongly attracted to each other by electrostatic charges
- the non-metal gains these electrons to form a negatively charged ion.
- dot and cross diagrams show the arrangement of electrons in an atom or ion.
- ionic compounds
- regular lattice structure
- high melting and boiling points
- dissolve easily and can conduct when dissolved or molten
- can't conduct electricity when solid
- strong electrostatic attraction
- covalent bonding
- non-metal and non-metal
- sharing electrons
- very strong electrostatic forces
- can use a dot and cross diagram to demonstrate this
- giant covalent structures
- they are macro molecules
- high melting and boiling points
- don't conduct electricity
- eg allotropes of carbon
- Allotropes of carbon
- diamond
- giant covalent structure
- each carbon atom forms four covalent bonds
- very high melting point
- don't conduct electricity
- graphite
- each carbon atom forms three bonds
- arranged in hexagons
- high melting points
- conduct electricity
- delocalised electron
- graphene
- is one layer of graphite
- very strong
- light
- one atom thick
- can conduct
- fullerenes
- shaped like hollow balls
- can be used to cage other molecules
- can be used to deliver a drug in the body
- make good catalysts, as they have a high surface area
- diamond
- Allotropes of carbon
- simple molecular substances
- strong covalent bonds
- weak intermolecular forces
- as the size of the molecules increase the intermolecular force increses
- low melting and boiling point
- normally gas or liquid
- don't conduct electricity
- no free electrons
- polymers
- lots of small units linked together to form a long molecule
- joined together by strong covalent bonds
- intermolecular forces are still weaker than ionic and giant covalent
- so have a lower boiling point that them
- metallic bonding
- metal and metal
- giant regular structure
- the electrons in the outer shell are delocalised
- the electrostatic attraction between positive and negative ions are strong
- most are solid
- malleable
- alloys are harder than pure metals because in an alloy the atoms have different sizes so it makes it harder for them to slide over each other
- Ionic Bonding
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