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4520480
GCSE AQA Chemistry 2 Bonding
Description
Mind map showing information about bonding including ionic bonding, covalent bonding and metallic bonding.
No tags specified
gcse
aqa
chemistry
chemistry unit 2
bonding
atoms
ionic
covalent
chemistry
chemistry 2
gcse
Mind Map by
Lilac Potato
, updated more than 1 year ago
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Created by
Lilac Potato
almost 9 years ago
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Resource summary
GCSE AQA Chemistry 2 Bonding
Atoms
Mass no. -> total no. of protons and neutrons
Electrons not counted because their mass is negligible
Atomic no. -> no. of protons
Compounds
Atoms of two or more elements are chemically combined
Isotopes
Different atomic forms of the same element which have the same no. of protons but a different no. of neutrons
Same atomic no. but different mass no.
Ionic Bonding
Atoms gain/lose electrons to form charged particles (ions)
Strongly attracted to each other
Shells with 1/2 outer electrons want to get rid so left with full shells
Metals lose to form positive ions
Nearly full shells want to gain to get full shell
Non-metals gain to form negative ions
Ionic compounds
Giant regular ionic lattice structure
Strong electrostatic forces of attraction between oppositely charged ions
Properties - high melting & boiling points, will carry electric current when molten & dissolve easily in water
Covalent Bonding
Sharing electrons
In their outer shells
Both atoms feel like they have a full outer shell
Non-metals only
Covalent substances
Simple Molecular
Atoms form strong CBs to form small molecules
Intermolecular forces - v. weak
Melting & boiling points v. low - bonds easily broken
Most are gases/liquids at rm. temp.
Don't conduct electricity
Giant Covalent Structures (Macromolecules)
All atoms bonded to each other by strong CBs
V. high melting/boiling points
Don't conduct electricity
Examples:
Diamond
Forms 4 CBs
Hardest natural substance
Graphite
Forms 3 CBs
Creates layers - free to slide
Weak intermolecular forces between layers
Only non-metal - good conductor of heat/electricity
Each atom has one delocalised electron
Silicon dioxide (Silica)
Giant structure of silicon & oxygen
Metallic Structures
Giant structure
Delocalised electrons - come from outer shell of every metal atom
Free to move - good conductors of heat/electricity
Hold atoms in regular structure
Strong forces of electrostatic attraction between positive metal ions & negative electrons
Layers of atoms can slide - metals can be bent/shaped
Alloys
Mixture of 2 or more metals
Different elements have different sized atoms
Layers distorted - hard to slide so alloys are harder
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