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Atomic Structure
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Edited at 2020-10-08 07:48:42- Recommended to you
- Outline
Atomic Structure
Metallic bonding
made up of metal atoms stacked ina lattice and a sea of free valenceelectrons
electrostatic attraction between atoms andvalence electrons is non dimensional andstrong
ionicbonding
Metal + nonmetal transfer electrons to from anions () and cations (+)
covalent bonding
Form between two or more nonmetal atoms
Electrons are shared between atoms
Lewis structures
Total all valence electrons in the molecule
Place remaining pairs around the outer atoms so that they each have 8 electrons
Bond polarity
Caused by differencesin electronegativity
If difference in electronegativityis less than 0.5, then thecovalent is nonpolar
Polar covalent molecules
occur when the bondpolarities do not cancel.
What makes up an atom?
electron arrangement
nucleus
Protons (P+)
Neutrons (n)
Properties of ionic compounds
solubility
variable solubility inwater (see solubilityrules)
electrical conductivity
as molten and solution onlyas need free moving ions
hardness
brittle
when forced, layers ofions shift causing positiveand negative ions to alignand repel.
Properties of covalent compounds
giant covalent networks
diamond structure
solubility
insoluble in water and nonpolar substances
electrical conductivity
nil, no free electrons
melting point
very high strong covalent bonds
hardness
very hard strong covalent bonds
silicon dioxide structure
bucky balls structure
graphite structure
solubility
insoluble in water andnonpolar solvents
electrical conductivity
conducts electricity due tofree electrons betweenlayers
melting point
very high strong covalent bonds
hardness
layers slide over eachother weakVan Der Waals forces betweenlayers
simple covalent molecules
solubility
soluble in water if polar, soluble innonpolar solvents if nonpolar
electrical conductivity
nil no free electrons orcharged particles
melting point
Very low MP is dependanton size of atoms in themolecule
hardness
nil, mostly gas, liquids ofsoft solids at roomtemperature
Breaking Van DerWaals forces
dipoledipoleinteractions
in molecules containingpolar covalent bonds
Hydrogenbonding
between moleculescontaining O, H or Fatoms
these are stronger than theother types of Van Der Waalforces
This leads to higher thanexpected melting points
instantaneous dipolemoments
halogens
melting point increasesdown the group
in molecules containingnonpolar covalent bonds
These dipolemoments get strongerthe more electronsthere are in themolecule