Chem Flashcards
% composition
mass in 1 mole / molar mass
4 examples of nucleophiles
Hydroxide
Ammonia
Water
Cyanide
Are salts soluble or insoluble
Soluble
4 examples of salts
nitrates
sulphates
phosphates
chlorides
are bases soluble or insoluble
insoluble
3 types of bases
carbonates
hydroxides
oxides
what happens to s orbitals as energy levels increase
get larger
test for carbonates
nitric acid - add until bubbling stops
limewater - goes cloudy
test for sulfates
barium nitrate - forms white ppt
test for halides
silver nitrate
Cl- white
Br- cream
I- yellow
ammonium test
warm with dilute NaOH to produce ammonia
red litmus turns blue
acid test
blue litmus turns red
alkali test
red litmus turns blue
no. particles
moles x avogadros
salt def
H+ in an acid is replaces by an ion
Silver ion
Ag+
Zinc ion
Zn2+
Lead ion
Pb2+
what are the two non octet molecules
S8 P4
What is Le Chatiliers principal
if dynamic equilibrium is disturbed the position of equilibrium shifts to counteract it
cm3 to m3
cm / 1 000 000
general formula for dienes
CnH2n-2
what does IR radiation do to covalent bonds
makes them vibrate more
nucleophile def
an electron pair accepter attracted to low electron density
ionisation enthalpy def
the enthalpy required to remove one mole of electrons from one mole of atoms in gaseous form
what happens to ionisation energy across the period
increases
why does ionisation energy increase across the period (3)
atomic radius decreases
nuclear charge increases
nuclear attraction increases
why does atomic radius decrease across the period (3)
nuclear charge increases
electrons fed into same principal shell
no increase in shielding
what happens to ionisation energy down the group (4)
decreases:
atomic radius increases
shells increase
increased shielding
outer electron further away
electronegativity def
the ability of an atom to withdraw an electron pair across a covalent bond
ionic bonding def
the electrostatic attraction between a positive and negative ion
aliphatic
branches or unbranched or non-aromatic rings
alicyclic
rings with or without branches but non-aromatic
aromatic
benzene rings
sigma bond def
an overlap of orbitals directly between bonding atoms
Pi bond
the sideways overlap of p orbitals above and below bonded atoms
Standard conditions
pressure
temp
conc
100kPa
298K
1 mol dm-3
standard enthalpy change of reaction
the energy change associated with a stated equation with all reactants and products in their standard states
st enthalpy change combustion
the enthalpy change taken place during the complete combustion of 1 mole of a substance under standard conditions
st enthalpy change formation
the enthalpy change when 1 mole of a substance is formed from its elements under standard conditions
st enthalpy change neutralisation
the enthalpy change that accompanies the formation of 1 mole of water from neutralisation under standard conditions
2 bond pairs
name
angle
linear
180
3 bond pairs
name
angle
trigonal planar
120
2 bond pairs, 1 lone pairs
name
angle
non-linear
117.5
4 bond pairs
name
angle
tetrahedral
109.5
3 bond pairs, 1 lone pairs
name
angle
pyramidal
107
2 bond pairs, 2 lone pairs
name
angle
non-linear
104.5
5 bond pairs
name
angle
trigonal bipyramidal
90
120
6 bond pairs
name
angle
octahedral
90
4 bond pairs, 2 lone pairs
name
angle
square planar
90
what can hydrogen bonds form between
O N F
alkane to haloalkane
alkane + halogen
UV
alkene to alkane
alkene + H2
Ni catalyst
150’
alkene to alcohol
alkene + water
H3PO4
high temp and pressure
haloalkane to alcohol
haloalkane + NaOH/water
reflux
alcohol to alkene
alcohol
conc H2SO4
reflux
1alcohol to aldehyde
alcohol + [O]
acidified potassium dichromate
distil
1alcohol to carboxylic acid
alcohol + 2[O]
acidified potassium dichromate
reflux
2 alcohol to ketone
alcohol + [O]
acidified potassium dichromate
reflux
alcohol to ester
alcohol + carboxylic acid/conc H2SO4
reflux
