bonding Flashcards
Graphite
consists of carbon atoms bonded to 3 other carbon atoms in a 2-D lattice. Delocalised valence electrons are between the layers and the forces of attraction between the layers are weak.
Diamond
Consists of carbon atoms covalently bonded in 4 other carbon atoms in a tetrahedral 3-D lattice structure. The covalent bonds are strong so atoms cannot be easily removed.
Ion
Consists on ions, ionic bonds
Metal
cations and electrons, metallic bonds
Molecule
atoms, covalent bonds, covalent network solid
Metal conduction
3-D lattice of positively charged metal cations, with delocalised valence electrons bonded to all the metal cations. As these electrons move the metal will conduct electricity as solid & molten
Requirement for conduction
Free moving charged particles
Ion conduction
ionic solid is a 3-D lattice of cations and anions. In solid, charged particles (ions) are in fixed position and as they do not move, the solid cannot conduct electricity. Molten, ions can move and is able to conduct electricity.
Melt ice
endothermic to absorb
Heat pack heats up
exothermic as heat is released
Shape
_ regions of electron density around the central _ atom. These regions are arranged as far apart as possible to minimise repulsion. They take a _ arrangement with a bond angle of _.
All Bonding regions
all regions are bonding therefore the shape is _
Not all bonding regions
_ regions are bonded and _ non-bonding lone pair of electrons, therefore the observed shape is _
Polarity factors
presence of polar bonds (due to electronegativity differences of the atoms in a bond)
distribution of polar bonds around a central atom
symmetrical/asymmetrical to cancel dipole
Polarity
bonded atoms are different and have different electronegativity so there is a bond dipole and the bonds are polar. If symmetrical, the dipole cancels and is non-polar.