BONDING Flashcards
what is ionic bonding between?
metal and non-metal
ionic bonding definition
the transferring of electrons from one atom to another in order to achieve a full outer shell
lose electron = what charge
positive
gain electron, what charge
negative
how would u write 2 electrons being lost
2+
diagrams used in ionic bonding
dot-and-cross diagrams
if calcium needs 2 electrons and chlorine needs 1, what do u do?
make it one calcium bonded to 2 chlorine
what is covalent bonding between?
non-metal and non-metal
what happens to electrons in covalent bonding?
they are SHARED
20 first elements rule for covalent bonding
atom puts in what the want back as extra
how is a double bond written?
with 2 lines
how is a single bond written?
with 1 line
how is a triple bond written?
3 lines
1 pair= what bond
1 pair= single bond
ionic bonding features
- soluble in water (not organic solvents)
- conducts electricity in water (as mobile)
- giant ionic structure
- crystal lattice// regularly arranged
- strong electrostatic forces
- HIGH melting and boiling points
molecular substances features (covalent)
- bonds within= strong
- intermolecular forces= weak
- low melting/ boiling points
- insoluble in water (with exceptions)
- no conduct electricity as no charged molecules
DIAMOND FEATURES (MACROMOLECULE)
- 4 covalent bonds
- giant lattice
- high melting/boiling points
- v hard
- colourless, glittering crystals
- doesn’t conduct electricity
GRAPHITE FEATURES (MACROMOLECULE)
- 3 covalent bonds
- layers// hexagons
- high melting/boiling points (as strong covalent bonds)
- soft/ slippery (as intermolecular forces= weak)
- black, shiny solid
- conducts electricity (as delocalised electron)
what is metallic bonding between
metal plus metal
metallic bonding arrangement
packed closely together in regular arrangement
what happens to valence electrons in metallic bonding? what does this create?
as so close together, they move away from the atom. this creates a “sea” of delocalised electrons surrounding lattice of positively charged metal ions
how are metallic bonding structures held together?
by strong attraction between mobile electrons and metal
metals properties
- high melting/ boiling points
- good conductors of heat/ electricity
- malleable and ductile (as layers they are arranged in slide when force is applied)
