bonding
- Created by: Emilyburkee
- Created on: 21-07-21 16:55
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- bonding
- ionic bonding
- metal + non-metal - transfer of electrons - full outer shells
- covalent
- non-metal + non-metal - electrons are shared on outer shells
- dative bonding
- when both electrons shared are form one atom
- indicated as an arrow -treated as covalent
- metallic bonding
- between 2 metals
- lattice of positive ions surrounded by delocalised electrons
- greater the positive charge greater force
- effects boiling point, melting point ect
- crystal structures
- ionic- high melting and boiling point
- strong electrostatic forces,conducts in solution
- metallic
- good conductors
- malluable - layers of ions are able to slide
- foces between ions and e = strong
- good conductors
- simple molecular
- covalent bonds held by van der waals forces
- very weak - low melting and boiling point
- covalent bonds held by van der waals forces
- macromolecular
- covalent giant lattice- each atom has multiple covalent bonds
- graphite = flat sheets
- covalent giant lattice- each atom has multiple covalent bonds
- ionic- high melting and boiling point
- shape of molecules
- depends on how many electrons surround central atom
- e- repel = largest bond angle exists
- if has 2 sites angle = 180 between = linear shqpe
- tigonal = 3 sites = 120 angle
- lone pairs = repel more strongly
- reduces bonding angle by 2.5 degrees
- 4 = tetrahedion
- depends on how many electrons surround central atom
- bond polarity
- covelent bonds - neg charge is not evenly spread
- electronegativity- power of an atom to attract negative charge
- covelent bonds - neg charge is not evenly spread
- ionic bonding
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