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AS Inorganic Chemistry > AS Chemistry > Flashcards

AS Chemistry Flashcards

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1
Q

isotope

A

each atom of element has same no of protons, different number of neutrons

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2
Q

mass number

A

total number of protons and neutrons

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3
Q

atomic number

A

number of protons,

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4
Q

ammonium

A

nh+4

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5
Q

hydrogencarbonate

A

hco3-

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6
Q

manganate

A

mno4-

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7
Q

dichromate

A

cr2o7-2

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8
Q

phosphate

A

PO4-3

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9
Q

relative isotopic mass

A

the mass of an atom of an element relative to one twelfth of the mass of an atom of carbon-12

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10
Q

one mole

A

amount of substance, contain same no of particles as 12g of carbon 12.

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11
Q

no of moles

A

no of things/6.02x10^24

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12
Q

yield

A

actual/max theroticaly

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13
Q

why is yield never 100%

A

side reactions can occur
reactions may not be complete
reaction can be reversible.

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14
Q

atom economy

A

desired product mR/sum of Mr of all

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15
Q

gases at room temp

A

mol x 24dm^3

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16
Q

if not at room temp

A

pV=nRT

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17
Q

standard solution

A

solution of known concentratiion, made in voncial flasks

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18
Q

how do you prepare a standard solution?

A

1)zero balance and weigh mass to small beaker
2)dissolve in small amount of distilled water.
3)using funnel, transfer to volumetric flask,
4)rinse with distilled water, and make it to the line.

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19
Q

concentration

A

moles/volume of solution.

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20
Q

acids

A

proton donors
can be strong/weak depending on dissociation.

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21
Q

bases

A

protons acceptors
some are soluble, and release OH

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22
Q

acid+metal

A

salt+water

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23
Q

acid+metal hydroxide

A

salt+water

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24
Q

acid+metal carbonate

A

salt+water+co2

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25
hydrous salt
salt containing water, which is heated to release.
26
oxidiation number
pure elements=0 flurione=-1, O=+2 oxygen=.2, peroxides=-1 Cl=-1, Fl or O=1
27
disproportion reaction
same reaction is oxidised and reduced
28
oxdising agent
gets reduced electron acceptors
29
reducing agent
gets oxidised reduction of others
30
ionic bonding
metals and non mentasl
31
structure of ionic
giant ionic lattice need large amount of energy to overcome electrostatic forces. electron conductivty as can conduct when molten as particles are mobile.
32
covalent bonding
happens between non metals electrostatic attraction between shared pair of electrons and nuceli of bonded atoms.
33
dalative covalent
involve share pair of electrons, where only one pair supplies electrons.
34
linear
2 bond pairs=180
35
trignoal planer
3 bond pairs=120
36
bent
2 bond, and 1 lone-117.5
37
tetracadal
4 bond paairs=109.5
38
pyramdial
3 bond and 1 lone=107
39
octacherdal
6 bond=90
40
london forces
electron density is uneven, so temp dipole. more electrons=stronger induced dipole so is stronger. happens in all molecules, only intermolecular between non polar.
41
permanent dipole
occur between polar molecules opposite ends of each pole attract each other.
42
hydrogen bonds
lone pair attracted to H+
43
polar
different electronegativty, +-more share.
44
polar-has to be any of these
different molecules central has a lone pair.
45
polar
not symmetrical bonds dont cancel.
46
first ionisation energy
energy required to remove any electron from each atom in mole of gaseous to form +1 ions. x->x+e
47
nuclear charge
more protons, more attraction so electron removed
48
atomic radius
larger atomic weaker nucleus attraction
49
electron shielding
electrons
50
ionisation energy increases due to
large atomic greater shielding Higher nuclear(this is outweighed by other 2)
51
dips in Al and P
due to change in subshell. and less energy, as due to less repulsion, from orbital of 2 then one.
52
period 2 is higher ionisation energy
dip for boron=higher sub shell 0=first paired electron
53
period 2 melting points
Li and Be decrease in ionic radius more delocalised electrons B and C b=3 covalent bonds c=4 covalent N, O, F, Ne needs less energy to break forces
54
group 2
lose electrons to form 2+ reducing agents reactivity increases as go down antacids neutralise soils
55
group 2=reactivity increases as go down
increase of atomic more shielding less attraction electrons lost easily
56
halogens
solid=simple covalent lattices f2=pale yellow c2=pale green br2=red brown i2=shiny gra
57
why does oxidising decrease as you go down
higher atomic higher shielding weaker attraction
58
test of chlorine
add small of dilute nitric acid, to remove carbonate. add silver nitrate=white bromine-cream iodine=yellow
59
bond enthalpy
one mole of covalent bond broken in gas state.
60
enthalpy change
bonds broken-bonds formed
61
hess law
if reaction can take place by two routes, enthalpy is same. Formation=products-reactants Combustion=reactants-products.
62
enthalpy change of neutrallisation
enthalpy change for reaction between acid and base to produce one mole of water under standard conditions.
63
enthalpy change
heat change at constant pressure One mole of covalent bonds broken in gas state
64
formation
one mole of compound formed from constituent elements in standard states and conditions.
65
combustion
one mole of substance in standard states burned in excess of O2 under standard conditions.
66
collision theroy
particles must collide for reactions to occur. need =correct oreniation sufficent energy
67
dynamic equillbrium
reactants to products closed same concentration factors = pressure, temperature, and concentration
68
temperatyre
+ endothermic=increase temp favours - exothermic=decrease temp favours
69
test for ammonium
add NaOH=warm test with damp red litmus should go blue
70
test for carbonate
add dilute acid, should be efferceveness
71
test for sulfate
add barium nitrate, and white
72
order for tests
carbonate, sulfide, halidie

AS Inorganic Chemistry (1 decks)

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