Bonding Flashcards
what is an ionic bond ?
a bond between a metal and a non metal where an electrostatic force of attraction occurs between oppositely charged ions
state the charges on :
group 1
group2
group6
group7
+
2+
2-
-
what is a structure of an ionic bond ?
each ion attracts to opposiute charges - forms giant ionic lattice containing billions of ions (lattice structure)
what is formula for :
sulfate
hydroxide
nitrate
carbonate
ammonium
so42-
oh-
no3-
co32-
nh4+
ionic bonding properties :nacl
melting and boiling point
high MP &BP as a lot of energy is needed to overcome strong force of electrostatic force of attraction (the higher the charge of the ionic compound the higher the mp and bp - e.g mgo and nacl )
ionic bonding strength :nacl
when size of ions decrease , strength increases( . e.g fluoride ions are smaller than chloride ions so calcium fluoride has higher melting point then calcium chloride )
hard and brittle
ionic bonding solubility : nacl
they are soluble - but ionic lattice must be broken and water molecules attract and surround ions
as ionic charge increases - solubility decreases
ionic bonding electricity nacl
can conduct electricity when molten or in aqueous solution as ions are free to move and conduct electricity . in solid ions cannot move = not conduct electricity
when can ionic compounds split ?
if pressure / forces cause ions to one closer to each other , some charged ions may repel causing it to split .
what is a covalent bond ?
electrostatic force of attraction between a shared pair of electrons and nuclei of bonded atoms - when atoms are combined by covalent bionds they form molecules
what is the difference between multiple and single covalent bonds ?
single = shaired pair of electrons
multiple bonds = multiple pairs of electrons
what is a coordinate covalent bond
it is a covalent bond which includes a shaired pair of electrons from 1 atom
simple molecular properties iodine MP & BP
low as there are weak forces of attraction
simple molecular properties iodine electrical conductivity
doesn’t as no charged particles free to move
simple molecular properties iodine strength - brittle
weak intermolecular forces
simple molecular properties iodine solubility
depending on intermolecular forces (slightly )
giant covalent (diamond ) properties (MP AND BP
high as lots of strong covalent bonds (electrostatic forces of attraction ) between atoms
giant covalent (diamond ) properties electrical conductivity ?
cannot as no delocalised electrons around it
giant covalent (diamond ) properties strength ?
very strong due top strong force of attraction between carbon atoms - rigid arrangement of atoms held y covalent bonds
giant covalent (diamond ) properties solubility ?
insoluble
what is metallic bonding ?
sea of delocalised electrons surrounding by poitive ions arranged in a lattice
metallic bonding properties - melting point and boiling point
high MP AND BP as high metallic attraction as strong bonds =strong metallic bond between the -ve and +ve charge
what is metallic bonding ? strength
strong as force of electrostatic attraction between opposite charges = high metallic bond as layers can slide while maintaining metallic bond
what is metallic bonding ? electrical conductivity
high as surrounded by sea od delocalised electrons = conduct electricity
what is metallic bonding ? solubility
insoluble
graphite + graphene properties MP + BP
high MP AND BP as a lot of energy needed to break all strong covalent bonds
graphite + graphene properties electrical conductivity
yes as 1 delocalised electron free per carbon atom = can conduct electricity
graphite + graphene properties strength
brittle as weak forces between layers = easy for layers to slide
graphite + graphene properties solubility
insoluble
ICE properties : MP +BP
low mp amnd bp as there are weak froces of attraction between molecules
ICE properties : electrical conductivity
doesn’t conduct as there are no mobile charged particles surrounding it
density of ice versus water ?
ice is less dense then water as ice molecules are arranged in a lattice structure due to hydrogen bonds - liquid molecules are closer but not in a lattice
electronegativity ?
relative ability of an atom to attract pairs of electrons in covalent bonds
electronegativity down a group
electronehativity decreases
electronegativity across a period ?
electronegativity increases
factors effecting electronegativity
atomic radius - closer to nucleus = stronger attraction between nucleus and bonding pair of electrons
shielding - less shells of electrons between nuclei and the electrons = less shielding = less repulsion = stronger attraction between nucleus and outer bonding electrons
nuclear charge - more protons , stronger attraction between nucleus and bonding pairs of electrons
a bond will be non polar when
bonded atoms are the same
bonded atoms have same or similar electronegativity
