test 2 (first)
physical properties of all metals
electricity and heat conductors, lustrous when cut/polished
properties of most metals
-high boiling points
-malleable (shapeable)
-ductile (drawn into wire)
-often hard
electronagativity if metals
low ionisation/electronegativity
if metals conduct electricity in a solid state
they must have charged particles that can move (electrons)
if metals are good conductors of heat (kinetic energy)
must contain mobile particles that can move quickly from areas of high temp (sea of delocalised electrons)
if metals are malleable/ductile
must have forces between particles that can adjust when particles out of position
if metals are lustrous
they must have a sea of delocalised electrons that reflect light
if metals have a high boiling/meting point
they must have strong attractive forces that exist between particles
do metallic crystals have a sea of delocalised electrons within their lattice
yes
characteristics of sea of delocalised electrons
-malleable
-dense
-conductors of heat and electricity
-lustrous when cleaned
reactivity in periodic table increases
down the group
reactive metal + water =
metal hydroxide +hydrogen
reactive metal +acid =
metal salt + hydrogen (violent)
reactive metal + oxygen =
metal oxide
circular economy
-mined
-refined
-made into product
-used
-disposed
-recycled
-product
stages for obtain metals from ores
-mining
-metal extraction (electrolysis)
-refining metal (often electrolysis)
steps in metal recycling
-collecting
-sorting
-processing
-melting
-purification/refining
-cooling/transportation
-new products
properties of ionic substances
-high boiling/melting point
-hard/brittle
-not conductivity in solid state (no sea of delocalised electrons)
-conductive in molten/dissolves state (sea of delocalised electrons)
what two things interact in the ionic bonding model
metals bond with non-metals
what donates to what in ionic bonding
metals donate electrons to become cations (non metals accept and become anion)
what are cations
pawsitive ions!! đđ
what do the cations and anions form in ionic
a 3D lattice with ions held togeyher by electrostatic forces
in ionic why high melting point
strong 3D ionic bonding within salts
in ionic why hard/brittle
string ionic bonding within crystal mean that when struck, layes slide, causing repulsion of similarly charged ions, causing it to break
in ionic how electrical conductivity (charged particle=electricity)
in solid
-no freedom of movement (not conductive)
in molten/aqueous
-ions free to move therefore carry a current
in conductivity in ionic, what moves?
ions move but electrons do not (no sea of delocalised electrons)
how is lattice held together in ionic
strong electrostatic attraction (ionic bond)
how to name ionic compound
metal first (eg sodium chloride)
what is a polyatomic ion
tightly bond group of atoms that behaves as a single unit as it has an overall charge (eg CO3(2-)
what do hydrated ionic compounds contain
H2O bonded with crystal (water releases as crystal decomposes (changes state))
what is the solvent
fluid
what is the solute
the substance taht dissolves
what is the solution
solvent +solute
if the solvent is water then what is the solution
aqueous
why do particles disolve basically
if particles of the solvent and solute attract each other more than they attract the original compound
what is it called for covalent and ionic when dissolving
ionic =dissociation
covalent =ionisation
why does precipitation
when two solutions of soluble compounds mix and because two ions attract more, they create a solid
what is the solid formed by two ions in different compounds being attracted to each other more called?
a precipitate
what are ions not involved in the formation of a precipitate called
spectator ions
what do ionic equations in precipitations not include
spectator ions
what is electronegativity
the relative attraction (increased up and right on pt)
what has a stron electrostatic attraction in covalent
positive nuclei and negative shared electrons
what is VSEPR
velence shell electrion pair repulsion theory
what does VSEPR state
electron pairs in molecules repel each other and take up positions as far away from one another as possible
does VSEPR treate double triple bonds diff
nope
what is an exception of VSEPR and why
boron flouride as it is a trigonal planar due to its way of filling the schrodinger model of electrons (1s2,2p6)
how to lone pair electrons act
just like another molecule attached to the positive nuclei
when do polar bonds form
when reasonable eectronegativity difference between atoms on either end of covalent bond
what must the difference be for a polar bond
>=0.4
what does a polar bond create
a permanent dipole
which atoms are most likely to come up
H=2.2
C=2.6
N=3.0
C=3.4
how does a non-polar covalent molecule occur
a molecule that doesnt contain polar bonds and is symmetrical
what is a polar covalent molecule
a molecule that does contain polar bonds and is asymmetrical (all ways)
what is a dipols
an imbalance of electrons due to electronegativity that causes one side to be positively charged and the other to be negatively charged
traits of intermolecular bonding forces
between molecules (outside)
relatively week compared to intra
due to electrostatic attraction
types of intermolecular bonds
dispersion forces
dipole dipole attraction
hydrogen bonding (extreme dipole dipole)
ion dipole attraction
characterstics of intramolecular bonding
internal covalent bonds in molecule
sharing electrons
strong bonds
types of intra bonds
covalent, ionic and metallic
what is BP/MP based on in inter forces
the inter forced between molecules
characteristics of inter forces in solids
inter forces are strong
holds molecules in place (vibrate on the spot)
lowest energy
characteristics of inter forces in liquids
inter forces are moderate
holds molecules closesly packed but can move/flow
mid energy
characteristics of inter forces in gases
inter forces are broken
free moving molecules
highest energy
when is dispersion
in all covalent molecules but especially important for non-polar
due to instantaneous dipoles caused by electrons perfectly placed during their movement to create a negative and positive charge
when is dispersion forces stronger
in bigger cells (more electrons)
closely packed
linear
smaller in double/triple bonds
what is dipple dipole attraction
attractive forces between polar molecules
this takes energy to break up (solids have this)
what is hydrogen bonding
attractive forces between molecules containing hydrogen, bonded to flourine, oxygen and nitrogen (basically just extreme dipole dipole)
increasing strength of inter forces
dispersion
ion dipole
dipole dipole
hydrogen bonding
what is ion dipole forces
attractive forces between ion and polar molecules
the larger the charge the stronger the force
does it take more energy to break bonds than change state?
yes!
therefore covalent bonding takes even more energy to break down than hudrogen bonding
examples of carbon lattices
diamond, graphite, buckyballs, carbon nanotubes (all diff arrangements)
what do diff covalent arrangement of carbon stoms lead to
diff properties of carbon allotropes
structure if diamon covalent bonds
covalent network lattice in the shape of a tetrahedral
if a lattice is hard/brittle
no sea of delocalised electrons (meaning must have string attraction (electrostatic/negative or covalent bond))
structure of graphite
covalent layer lattice with a shape of layers
lone pairs in diamond
none as each carbon atom has 4 bonding pairs of electrons
lone pairs in graphite
1 pair as each carbon atom has 3 other carbon atoms bonded
graphite have sea of delocalised electrons?
yes, therefore electrical conductivity and weak dispersion forces between layers meaning layers can slide meaning good lubricant
not clearly definied shaps (amorphous) forms of carbon structure
no consisten structure and is reacgive and conductive
hor is amorphous carbon forms formed
combustion of plant material in limited O2 supply
carbon black
used in rubber products and printer toner
activated charcoal
very porous surface used to adsorb (no typo) impurities
if metals are dense
they must have tightly packed lattices
why is ice less dense than water
the orientation of hydrogen bonds causes the molecules to push further apart, lowering the density
why is ice less dense than water
the orientation of hydrogens cause molecules to push each ither further apart, lowering the density