ch2-bonding and structure Flashcards
whats ionic bonding
when a metal and nonmetal react to achieve a full outter shell and become stable
what happens when lithium and fluorine are ionicly bonded
1 electron passes from lithium to florine, lithium becomes a positive ion and fluorine becomes negative ion. they both have full outter shells
what typa forces are ionic compounds held together by
strong electrostatic forces between oppositely charged ions
whatre the properties of ionic lattices
-high melting and boiling point since string ionic bonds
-only conduct electricity when melted or dissolved in water because then electrons become delocalised and are free to move around
why do metals need delocalised electrons to conduct electicity or heat
bc then the electrons can move around freely and carry a current/energy
define covalent bonding
when 2 nonmetals share electrons so they can both have full outtermost energy shells
whatre the properies of covalent structures
- low melting and boiling points due to atoms being strongly covalently bonded but have weak intermolecular forces
-cannot conduct electricity cause they dont have an overall charge
whats metalic bonding
layers of positively charged ions within a sea of delocalised electrons thatre free to move
whats diamond made of
4 carbon atoms bonded covalently to eachother
why cant diamonds conduct electricity
theres no free elctrons/delocalised electrons to carry the current
whatre the properties of sillicon dioxide
-solid at room temp due to high mp and bp
-strong covalent bonds
why is graphite (3carbon) soft and slipper
-because the layers in between the graphite macromolecule arent covalently bonded so they can slide in different directions
- they can alsp conduct heat and electricity due to delocalised electrons from carbon atom
whatre fullerenes
-hollow carbon structures
whatre fullerenes used for
-as catalysts
-drug delivery to the human body
