chem test 2

ionic bond

the electrostatic attraction between oppositely charged ions (metal and non-metal)

covalent bond

electrostatic attraction between shared electrons and adjacent nucleus. between non-metals

metallic bond

the electrostatic attraction between a lattice of positive metal ions and a sea of delocalized electrons

ionic compound high melting point

giant lattice held together by strong electrostatic forces in all directions, and a lot of force required to overcome the forces.

metals conducting electricity

delocalized electrons are free to move and carry a charge throughout the 3d lattice.

ionic solids brittle

distortion of the lattice brings like-charges together, causing them to repel and shatter.

metals malleable and ductile

layers of positive ions can slide over each other without breaking the metallic bond held by the delocalised electrons

covalent molecular, low boiling point

held together by weak intermolecular forces between molecules, and is easy to overcome.

ionic, does not conduct electricity as solid

ions are locked in a fixed lattice and cannot move, therefore cannot conduct electricity

ionic, conducts electricity as liquid/solution

when molten or dissolved in water (aqueous), the ions become free to move and can carry electrical charge.

covalent network substance, high melting point

every atom is held together by strong covalent bonds that require massive energy to break.

covalent molecular substance, non-conductor

they lack free-moving charged particles to carry electrical charge

intermolecular forces

the weak attractive force that existst between separate molecules

intramolecular force

the strong chemical bond (ionic, covalent, metallic) that holds atoms together within the molecule

why do larger molecules have higher boiling/melting point.

have more electrons, eading to stronger electrostatic forces between molecules.

allotrope

different structural forms of the same element in the same physical state

diamond structure

each carbon is covalently bonded to 4 others in a 3d lattice `

graphite structure

each carbon has one delocalized electron that is free to move between layers. each carbon is covalently bonded to 3 other carbons.