Quiz
Chemistry knowledge questions
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Questions in this quiz (194)
1Relative mass of an electron
- A1/1840
- B-1
- C1/2580
2Max number of electrons in shells 1,2,3,4
- A1,4,9,16
- B2,8,18,32
- C2,4,6,8
3Number of orbitals in shell s,p,d,f
- A1,2,3,4
- B2,6,10,14
- C1,3,5,7
4Electronic configuration
- A1s2 2s2 2p6 3s2 3p6 4s2 4p6 3d10 5s2
- B1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
- C1s2 2s2 3s2 4s2 5s2 2p6 3p6 4p6 3d10
5When will there be a jump in successive ionisation energies of aluminium
- A2 to 3
- B5 to 6
- C3 to 4
6The big jump is because the electron is in a [blank_start]new shell[blank_end] which is [blank_start]very much closer to[blank_end] the nucleus therefore [blank_start]higher[blank_end] in energy meaning [blank_start]more[blank_end] energy is required to move the next valence electron
- Anew shell
- Bvery much closer to
- Chigher
- Dmore
7ionisation energy [blank_start]decreases[blank_end] down a group as atomic radius [blank_start]increases[blank_end] and shielding [blank_start]increases[blank_end]
- Adecreases
- Bincreases
- Cincreases
8ionisation energy [blank_start]increases[blank_end] across a period as number of [blank_start]protons increases[blank_end] and shielding [blank_start]stays the same[blank_end] and atomic radius [blank_start]decreases[blank_end]
- Aincreases
- Bprotons increases
- Cstays the same
- Ddecreases
9The unexpected [blank_start]fall[blank_end] in IE between 2 and 3 is because the 3's valence e is on a [blank_start]new sub shell[blank_end] which is [blank_start]higher[blank_end] in energy and [blank_start]further[blank_end] from the nucleus so [blank_start]easier[blank_end] to remove
- Afall
- Bnew sub shell
- Chigher
- Dfurther
- Eeasier
10The unexpected [blank_start]fall[blank_end] between 5 and 6 is because 6's valence e is [blank_start]paired in a p orbital[blank_end] which causes [blank_start]extra repulsion[blank_end] making it [blank_start]easier[blank_end] to remove
- Afall
- Bpaired in a p orbital
- Cextra repulsion
- Deasier
11Mass triangle
- AM = n / mr
- Bn = mr / m
- CMr = m/n
12Avogadro's triangle
- A# = n x Na
- BNa = n/#
- Cn = # x Na
131 molecule is
- A1 atoms
- B2 atom
- C1/2 atom
14Molecular is simplist whole number ratio
- ATrue
- BFalse
15Less H2O than expected is because
- ANot heated to constant mass
- BHeated too vigorously
- COver exposed to water in atmosphere
16More H2O than expected
- ANot heated to constant mass
- BOver exposed to water in atmosphere or heated too vigorously
- CNot heated vigorously enough or over exposed to water in atmosphere
17 V = n x [blank_start]24[blank_end]
- A24
18P [blank_start]v[blank_end] = n R [blank_start]T [blank_end]
- Av
- BT
19P v = n r t units
- APa , m3, mol, data sheet, C
- BKpa, dm3 , mol,data, K
- CPa , m3 , mol, data, K
20Cm to dm
- AX 100
- BX 1000
- CDivide by 1000
21[blank_start]Cm[blank_end] /1000 [blank_start]dm[blank_end] /1000 [blank_start]m[blank_end]
- ACm
- Bdm
- Cm
22 gdm-3 = moldm-3 x [blank_start]Mr[blank_end]
- AMr
23Concentration triangle
- AC = n x v
- BN = c x v
- CV = c x n
24% yield = [blank_start]actual[blank_end] mass / [blank_start]theoretical[blank_end] mass
- Aactual
- Btheoretical
25% atom economy = [blank_start]mr desired[blank_end] / [blank_start]total mr[blank_end] of products
- Amr desired
- Btotal mr
26How to achieve higher atom economy
- AReplace metal with one in same group with larger Mr value
- BReplace metal with one in same group with smaller Mr value
27Metal oxide + acid = salt + [blank_start]water[blank_end]
- Awater
28Metal carbonate + acid = salt + [blank_start]water[blank_end] + [blank_start]carbon dioxide[blank_end]
- Awater
- Bcarbon dioxide
29Alkali + acid = salt+ [blank_start]water[blank_end]
- Awater
30Metal + acid = salt + [blank_start]hydrogen gas[blank_end]
- Ahydrogen gas
31What reactions with acids would give off effervescence
- AAlkali and metal
- BMetal oxide and metal carbonate
- CMetal carbonate and metal
32What two give off just water when reacted with an acid
- AAlkali and metal
- BAlkali and media oxide
- CMetal oxide and metal
33Metallic lattices have [blank_start]high[blank_end] melting and boiling points due to [blank_start]strong bonds[blank_end]. Theyre [blank_start]good[blank_end] conductors as they have [blank_start]delocalised electrons[blank_end]. They are [blank_start]insoluble[blank_end].
- Ahigh
- Bstrong bonds
- Cgood
- Ddelocalised electrons
- Einsoluble
34More [blank_start]electrons[blank_end] and a [blank_start]higher charged cation[blank_end] makes a metallic bond stronger
- Aelectrons
- Bhigher charged cation
35Ionic lattices have [blank_start]high[blank_end] melting and boiling points due to [blank_start]strong[blank_end] bonds. They conduct electricity when [blank_start]molten[blank_end] and are [blank_start]soluble[blank_end] they are also [blank_start]brittle[blank_end] as distorting the lattice causes [blank_start]repulsion[blank_end]
- Amolten
- Bhigh
- Cstrong
- Drepulsion
- Esoluble
- Fbrittle
36Types of bond shapes in order : [blank_start]linear[blank_end] , [blank_start]trigonal planar[blank_end] , [blank_start]tetrahedral[blank_end] , [blank_start]pyramidal[blank_end] , [blank_start]non linear[blank_end] , [blank_start]octahedral[blank_end]
- Alinear
- Btrigonal planar
- Ctetrahedral
- Dpyramidal
- Enon linear
- Foctahedral
37Linear
- A120
- B90
- C180
38Tirgonal planar
- A90
- B120
- C107
39Tetrahedral
- A109
- B107
- C120
- D109.5
40Pyramidal
- A120
- B104.5
- C107
- D107.5
41Non linear
- A107.5
- B120
- C104
- D104.5
42Octahedral
- A120
- B90
- C60
- D80
43All molecules are polar
- ATrue
- BFalse
44[blank_start]London forces[blank_end] are the weakest IMF, then [blank_start]permanent dipole dipole[blank_end] then [blank_start]hydrogen bonds[blank_end] are the strongest
- ALondon forces
- Bpermanent dipole dipole
- Chydrogen bonds
45London forces arise when there's a [blank_start]temporary shift[blank_end] which generates a [blank_start]temporary dipole[blank_end] which [blank_start]induces a dipole[blank_end] in neighbouring molecules. They both then [blank_start]attract[blank_end] each other
- Atemporary shift
- Btemporary dipole
- Cinduces a dipole
- Dattract
46London forces strength increases as the [blank_start]number of electrons[blank_end] increases and the [blank_start]surface area[blank_end] increases
- Anumber of electrons
- Bsurface area
47Molecules with [blank_start]permanent dipoles attract[blank_end] to form permanent dipole dipoles
- Apermanent dipoles attract
48H bonds form when he delta [blank_start]positive[blank_end] H is attracted to a delta [blank_start]negative[blank_end] [blank_start]N[blank_end] , [blank_start]O [blank_end], [blank_start]F [blank_end]
- Apositive
- Bnegative
- CF
- DN
- EO
49Ice is [blank_start]less[blank_end] dense than water as the molecules are structured [blank_start]further apart[blank_end] when solid and they adopt a [blank_start]tetrahedral[blank_end] shape
- Aless
- Bfurther apart
- Ctetrahedral
50Simple molecular lattices have [blank_start]low[blank_end] melting and boiling points as breaking [blank_start]IMF[blank_end] . They are [blank_start]bad[blank_end] conductors and are [blank_start]soluble[blank_end] in like for like.
- Alow
- BIMF
- Cbad
- Dsoluble
51Saint covalent lattices have [blank_start]highest[blank_end] melting and boiling point as breaking [blank_start]covalent bonds[blank_end] . [blank_start]Graphite[blank_end] and [blank_start]graphene[blank_end] are conductive but [blank_start]diamond[blank_end] is not. They are completely [blank_start]insoluble[blank_end]
- Acovalent bonds
- Bhighest
- CGraphite
- Dgraphene
- Einsoluble
- Fdiamond
52Graphites properties
- ATrigonal planar and delocalised electrons
- BOne atom thick
- CTetrahedral shape and no delocalised electrons
53Diamonds properties
- AOne atom thick
- BTrig planar and delocalised electrons
- CTetrahedral and no delocalised electrons
54Graphene properties
- AOne atom thick
- BTetrahedral
- CNo delocalised electrons
55Atomic radius [blank_start]decreases[blank_end] across a period as [blank_start]more[blank_end] protons , [blank_start]same[blank_end] shells , sheilding [blank_start]constant[blank_end]
- Adecreases
- Bmore
- Csame
- Dconstant
56Atomic radius [blank_start]increases[blank_end] down a group as [blank_start]more[blank_end] shells , [blank_start]more[blank_end] shielding
- Aincreases
- Bmore
- Cmore
57Across the period the strength of metallic bonding [blank_start]increases[blank_end] so melting point [blank_start]increases[blank_end]
- Aincreases
- Bincreases
58[blank_start]Silicon[blank_end] has the highest melting point of the period
- ASilicon
59Simple molecular lattices melting point [blank_start]increases[blank_end] as the number of [blank_start]electrons[blank_end] increases
- Aincreases
- Belectrons
60Down group 2 reactivity [blank_start]increases[blank_end] as I.e. [blank_start]Decreases[blank_end] so electrons are [blank_start]easier[blank_end] to remove
- Aincreases
- BDecreases
- Ceasier
61Group 2 compounds treat [blank_start]stomach acid[blank_end] and [blank_start]neutralise[blank_end] acidified soil
- Astomach acid
- Bneutralise
62Metal + oxygen = [blank_start]metal oxide[blank_end]
- Ametal oxide
63Metal + water = [blank_start]metal hydroxide[blank_end] + [blank_start]hydrogen[blank_end] gas
- Ametal hydroxide
- Bhydrogen
64Metal + acid = [blank_start]salt[blank_end] + [blank_start]hydrogen[blank_end] gas
- Asalt
- Bhydrogen
65Metal oxide + water = [blank_start]metal hydroxide[blank_end]
- Ametal hydroxide
66Boiling point [blank_start]increases[blank_end] down group 7 as the number of electrons [blank_start]increases[blank_end] making London forces [blank_start]stronger[blank_end]
- Astronger
- Bincreases
- Cincreases
67Oxidising ability [blank_start]decreases[blank_end] down group 7 as atomic radius [blank_start]increases[blank_end] shielding [blank_start]increases[blank_end] so they accept the electron [blank_start]less[blank_end] readily
- Adecreases
- Bincreases
- Cincreases
- Dless
68A halogen will react with a halide if its higher up in the group
- ATrue
- BFalse
69If a halogen and Halide react the solution would be [blank_start]bright orange[blank_end] in [blank_start]hexane[blank_end]
- Abright orange
- Bhexane
70Test for halide ions
- AAmmonia
- BAqueous silver nitrate
- CSilver nitrate
- DConcentrated ammonia
71When added to AgNO3 a precipitate will form: chloride = [blank_start]white[blank_end] bromide = [blank_start]cream[blank_end] iodide = [blank_start]yellow[blank_end]
- Awhite
- Bcream
- Cyellow
72Adding ammonia will make this compound dissolve
- AChloride
- BBromide
- CIodide
73Adding concentrated ammonia confirms the presence of this as it's the only one that's insoluble in it
- ABromide
- BIodide
- CChloride
74Chlorine uses
- ANone its toxic
- BDisinfect water supplies
- CCauses cancer as its reactive so none
75Which reaction is this
- AEndothermic
- BExothermic
76Which reaction is this
- AEndothermic
- BExothermic
77In an enthalpy diagram the arrow points down if it is
- AEndothermic
- BExothermic
78In an enthalpy diagram the arrow points up if it is
- AEndothermic
- BExothermic
79Exothermic is
- AHeat loss and positive value
- BHeat loss and negative value
- CHeat gain and positive value
- DHat gain and negative value
80Endothermic is
- AHeat loss and negative value
- BHeat loss and positive value
- CHeat gain and negative value
- DHeat gain and positive value
81What are standard conditions
- A100pa and 298k
- B100kpa and 297k
- C100kpa and 298k
- D100pa and 297k
82Measuring enthalpy change
- AQ= m c ^ T then q/n
- BA = m c ^ T
- CQ = m c ^T then -q/ n
83Calculate average bond enthalpy
- ABond formed - bonds broken
- BBonds broken - bonds formed
84Hess' law provides an alternate route that could be
- AMore dangerous and harder to measure
- BHarder to control
- CSafer and easier to measure
- DEasier to see reaction
85How should you draw a Hess' law diagram
- AUsing data values
- BUsing the type of question
- CThe question and data values will add up
86In enthalpy of combustion data the arrows point [blank_start]down[blank_end]
- Adown
87[blank_start]Oxygen[blank_end] doesn't have a enthalpy combustion value as its just [blank_start]adding more[blank_end]
- AOxygen
- Badding more
88In enthalpy of formation the arrows point [blank_start]up [blank_end]
- Aup
89Elements under [blank_start]standard conditions[blank_end] don't have a enthalpy of formation value
- Astandard conditions
90Increasing the pressure to increase rate of reaction only applies to [blank_start]gases[blank_end]
- Agases
91Increasing surface area to increase rate f reaction only applies to [blank_start]solids[blank_end]
- Asolids
92Increasing the concentration to increase rate of reaction only applies to [blank_start]liquids[blank_end]
- Aliquids
93Unsuccessful collisions transfer energyb
- ATrue
- BFalse
94Increasing concentration [blank_start]increases[blank_end] rate of reaction As [blank_start]more[blank_end] particles in [blank_start]same[blank_end] amount of space so collisions are [blank_start]increased[blank_end]
- Aincreases
- Bmore
- Csame
- Dincreased
95Increasing pressure [blank_start]increases[blank_end] rate of reaction as particles are [blank_start]pushed together [blank_end]in a smaller volume
- Aincreases
- Bpushed together
96As volume increases [blank_start]pressure[blank_end] decreases
- Apressure
97Increasing temperature [blank_start]increases[blank_end] rate of reaction as particles have [blank_start]more[blank_end] energy
- Aincreases
- Bmore
98Area under the curve of a Boltzmann curve is total number of [blank_start]molecules[blank_end]
- Amolecules
99Boltzmann curve shows number of [blank_start]molecules[blank_end] compares to [blank_start]energy[blank_end]
- Amolecules
- Benergy
100The Boltzmann curve never touches the x axis as there is no maximum [blank_start]energy value[blank_end] a molecule can have
- Aenergy value
101The Boltzmann curve use start at origin as its impossible to have a molecule with [blank_start]no[blank_end] energy
- Ano
102Increasing temperature makes the Boltzmann curve [blank_start]decrease[blank_end] in peak height and shift to [blank_start]right[blank_end] hand side
- Adecrease
- Bright
103Irreversible reactions are because the activation energy of the reverse is [blank_start]too[blank_end] [blank_start]high[blank_end]
- Atoo
- Bhigh
104Catalyst [blank_start]reduce[blank_end] our demand on fossil fuels
- Areduce
105The rate of forward and reverse reactions is [blank_start]equal[blank_end] and the concentrations are [blank_start]constant[blank_end]
- Aequal
- Bconstant
106A shift to the right
- AIncreases product yield
- BDecreases product yield
107A shift to the left
- AIncreases product yield
- BDecreases product yield
108If concentration is increased in an equilibrium
- AShift to the opposite side
- BShift to the same side as increased concentration
109If concentration is decreased in an equilibrium
- AShift to opposite side
- BShift to same side as concentration change
110If pressure is increased at equilibrium
- AEquilibrium shifts to side with more moles to exert more pressure
- BEquilibrium shifts to side with fewer moles to exert less pressure
111If pressure is decreased at equilibrium
- AEquilibrium shifts to side with more moles to exert more pressure
- BEquilibrium shifts to side with fewer moles to exert less pressure
112Adding a catalyst to equilibrium
- AShift to right
- BNo change
- CShift to left
113Increasing temperature in an equilibrium
- AShift in endothermic to lower temp
- BShift in exothermic to increase temp
114Decreasing temperature in an equilibrium
- AShift in endothermic to lower temp
- BShift in exothermic to raise temp
115In industries conditions must be [blank_start]compromised[blank_end] as low temp [blank_start]decreases[blank_end] rate of reaction and high pressure is [blank_start]expensive[blank_end] and is not [blank_start]safe [blank_end]
- Acompromised
- Bdecreases
- Cexpensive
- Dsave
116Kc less than 1 is on the
- ALeft hand side
- BRight hand side
117Kc more than one is
- ALeft hand side
- BRight hand side
118Kc is
- AConcentration products / concentration reactants
- BConcentration reactants / concentration products
119All the things needed in a titration
- AClamp stand
- BClamp
- CBurette
- DPipette
- EPipette stand
- FPipette filler
- GMeasuring flask
- HConical flask
- IIndicator
120During a titration the more hazardous chemical goes in
- ABurette
- BConical flask
121During a titration the results must be concordant
- ATrue
- BFalse
122Concordant results means
- AWithin 1.0 of each other
- BWithin 0.1 of each other
- CWithin 0.01
123When using a volumetric flask there could be a problem as adding too much water reduces [blank_start]concentration[blank_end]
- Aconcentration
124The activation energy on an enthalpy diagram is
- AReactants line to product line
- BProduct line to reactant line
- CReactant line to peak of curve
- DProduct line to peak of curve
125The enthalpy change on a diagram is
- AProduct to reactant line
- BReactant to product line
- CReactant to peak
- DProduct to peak
126How does the coefficient change the way Kc is calculated
- ADoesn't change
- BEach concentration is divided by its coefficient
- CEach concentration is multiplied by its coefficient
- DEach concentration is to the power of its coefficient
127Bond angle of C-H
- A120
- B107
- C109
- D104.5
128General formula of Alkane
- ACnH2n
- BCnH2n+2
129General formula of Alkene
- ACnH2n
- BCnH2n+2
130General formula of alcohol
- ACnH2nO
- BCnH2n+2O
131General formula for aldehydes and ketones
- ACnH2nO
- BCnH2n+1O
132General formula of haloalkane
- ACnH2nX
- BCnH2n+1X
133General formula carboxylic acid
- ACnH2O2
- BCnH2nO2
134How to make a structural isomer of an Alkene
- AMove c=c bond
- BIntroduce a branch
- CAdd a H
- DChange functional group to anything
- EChange functional group to cyclo
135Structural isomers of alkanes
- AMove c c double bond
- BChange functional group
- CIntroduce branch
136Structural isomerism in alcohols and haloalkanes
- AMove same group
- BIntroduce branch
- CMove double bond and
137Shape of alkanes
- APyramidal
- BTetrahedral
- CTrig planar
138Alkanes have greater boiling boils when they have a [blank_start]greater[blank_end] surface area contact between molecules and [blank_start]more[blank_end] electrons therefor [blank_start]more[blank_end] london forces
- Agreater
- Bmore
- Cmore
139Alkanes are
- AHighly flammable
- BInflammable
140In a limited oxygen environment alkanes undergo [blank_start]incomplete combustion[blank_end] producing [blank_start]carbon monoxide[blank_end]
- Aincomplete combustion
- Bcarbon monoxide
141Carbon monoxide is [blank_start]toxic[blank_end] to humans as sis [blank_start]prevents[blank_end] transport of blood in the body
- Atoxic
- Bprevents
142To react alkanes with halogens [blank_start]uv[blank_end] light is required to form a [blank_start]free radical[blank_end] as it's a non polar bond
- Auv
- Bfree radical
143The steps in free radical substitution are : 1 for [blank_start]initiation[blank_end] , 2 for [blank_start]propagation[blank_end] , 3 for [blank_start]termination[blank_end]
- Ainitiation
- Bpropagation
- Ctermination
144The initiation step of free radical substitution is [blank_start]homolytic[blank_end] fission
- Ahomolytic
145Propagation step of free radical substitution is a [blank_start]chain[blank_end] reaction
- Achain
146Single bonds result from
- AS orbital overlap
- BP orbital overlap
147Double bonds are formed by
- AS orbital overlap
- BP orbital overlap
- CA combination of an s orbital overlap and p orbital overlap
148Shape round carbon of an Alkene
- ATrig planar
- BTetrahedral
- CPyramidal
149Bond angle round C in Alkene
- A109
- B120
- C107.5
150Double carbon bonds can rotate
- ATrue
- BFalse
151Each carbon in the double bond must be bonded to two [blank_start]different[blank_end] groups to be E/Z Isomer
- Adifferent
152CIP rules state that the larger the proton number the [blank_start]higher[blank_end] the priority
- Ahigher
153To be CIs/trans each carbon in the double bond must be directly bonded to a [blank_start]hydrogen[blank_end] atom
- Ahydrogen
154E isomers can also be
- ACis
- BTrans
155Z isomers can also be
- ACis
- BTrans
156Alkenes are very reactive as the H bond has a low [blank_start]enthalpy[blank_end]
- Aenthalpy
157Hyrogenation is
- AAdding H20 to an Alkene to get an alkane
- BAdding H2 to an Alkene to get an alkane under acid catalyst
- CAdding H2 to an alkane to get an Alkene under Nickle catalyst
- DAssing H2 to an Alkene to get an alkane under nickle catalyst
158Halogenation is
- AAdding HX to an Alkene to get a alcohol
- BAdding X2 to an Alkene to get an alcohol
- CAdding X2 to an Alkene to get a haloalkane under heat
- DAdding X2 to an alkane to get a haloalkane under heat
159Halogenation can test for a [blank_start]double[blank_end] bond
- Adouble
160Addition of HX is
- AAdding HX to an Alkene under reflux
- BAdding HX to an Alkene under heat
- CAdding HX to an alkane under reflux
161Markownikoffs rule states the [blank_start]more[blank_end] stable carbocation is preferred by the mechanism and stability increases as the number of hydrogen atoms the C is bonded to [blank_start]decreases[blank_end]
- Amore
- Bdecreases
162Addition of H2O is
- AAdding H2O to an Alkene to get an alcohol
- BAdding steam to an Alkene under H3PO4 catalyst to get an alcohol
- CAdding H2O to an Alkene under H3PO4 catalyst to get an alcohol
- DAdding steam to an alkane to get an alcohol
163The bonds in alcohols are
- ACH 109 and OH 104.5
- BCH 120 and OH 104.5
- CCH 109.5 and OH 104.5
164When polymerising a monomer what changes?
- AThe general formula
- BLoss of all hydrogen bonds
- CLoss of double bond between carbons
165Alternatives to disposal of waste polymers
- ADon't use polymers anymore
- BRecycle and reuse
- CCombustion for energy production
- DBurn them
- EUse as organic feedstock
- FUse biodegradable polymers
- GUse photosynthesis polymers
- HUse photodegradable polymers
166A primary alcohol is bonded to
- ANo hydrogen
- BOne hydrogen
- CTwo hydrogens
- DFour hydrogens
167Secondary alcohols are bonded to
- ATwo hydrogens
- BThree hydrogens
- COne hydrogen
168Tertiary alcohols are bonded to
- AOne hydrogen
- BThere hydrogens
- CNo hydrogens
169Alcohols are [blank_start]soluble[blank_end] in water because the delta positive [blank_start]hydrogen[blank_end] forms a h bond with the free pair of electrons from the delta negative [blank_start]oxygen[blank_end]
- Asoluble
- Bhydrogen
- Coxygen
170Combustion is
- AAdding O2 to an alcohol
- BAdding o2 to an alcohol with high heat source
- CRemoving o2 from an alcohol
171What is [O]
- AK7O2CR7
- BH+/ K7CR2O7
- CH+/K2Cr7O2
- DH+/K2Cr2O7
172Oxidation needs [blank_start]heat[blank_end] conditions
- Aheat
173Oxidation turns solutions from [blank_start]orange[blank_end] to [blank_start]green[blank_end]
- Aorange
- Bgreen
174Primary alcohols are oxidised to be
- AAldehydes
- BSecondary alcohol
- CCarboxylic acid
- DKetone
175How to get from a primary alcohol to carboxlyic acid
- AReflux of primary alcohol
- BDistillation of primary alcohol
- CDistillation of primary alcohol then reflux of product
176Combustion of secondary alcohol gives
- AEither ketone or aldehyde
- BCarboxylic acid
- CKetone
- DAldehyde
177Tertiary alcohols oxidise to [blank_start]nothing[blank_end]
- Anothing
178Elimination of H2O is
- AHeating an alcohol in H3PO4 catalyst to get Alkene and h20
- BHeating an alcohol in h2so4 catalyst to get an Alkene and h20
- CHeating an alcohol in h2so4 catalyst to get an alkane and h20
- DHeating an alcohol in H3PO4 catalyst to get an alkane and H2O
179HX is made in still by adding
- ANaX and H3PO4
- BNaX and H2SO4
180Substitution with halide ion is
- AAdding HX to an alcohol to get alkane and water under reflux
- BAdding HX to alcohol to get haloalkane and water under reflux
- CAdding HX to alcohol to get alkane and water under distillation
- DAdding HX to alcohol to get haloalkane and water under distillation
181C-X bond enthalpy [blank_start]decreases[blank_end] down group 7 as shielding [blank_start]increases[blank_end] and atomic radius [blank_start]increases[blank_end] so there's a [blank_start]greater[blank_end] distance between shared pair of electrons and the nuclei of two bonded atoms
- Adecreases
- Bincreases
- Cincreases
- Dgreater
182Hydrolysis of haloalkanes using [blank_start]AgNO3[blank_end] and H20 under [blank_start]heat[blank_end] measures the strength of the C-X bond
- AAgNO3
- Bheat
183Hydrolysis of haloalkanes using [blank_start]NaOH[blank_end] under [blank_start]reflux[blank_end] gives an alcohol by nucleophillic substitution
- ANaOH
- Breflux
184Natural Ozone layer equation
- AO2 + O2 = 2O2
- BO2 + O = O3
- CO2+O2=O4
185Photodissociation is the breaking down of a bond under [blank_start]uv[blank_end] light and is an example of [blank_start]homolytic[blank_end] fission
- Auv
- Bhomolytic
186What radicals can cause the breakdown of the ozone layer
- AChlorine
- BNitrogen
- COxygen
- DNitrogen oxygen
- ECarbon
187How are chlorine free radicals formed
- AAir traffic
- BDry cleaning
- CFlame retardant
- DLightening storms
188How are nitrogen oxygen radicals formed
- ADry cleaning
- BAir traffic
- CFlame retardant
- DLightening storms
189Overall equation for human breakdown of the ozone
- AO2 + O = O3
- BO3 + O = 2O2
- CO2 + O2 = O4
- DO3 + O = O4
190Which are the propagation steps of the breakdown of the ozone
- AStep 1 : X* + O2 = XO* + O
- BStep 1: X* + O3 = XO* + O2
- CStep 2 : XO* + O = X* + O2
- DStep 2: XO* + O2 = X* + O3
191[blank_start]Global warming[blank_end] is caused by molecules absorbing IR and releasing it back towards earth
- AGlobal warming
192How to monitor a greenhouse gas
- AConcentration
- BVolume
- CMass
- DHow much it absorbs
- EHow much it releases
193The largest peak to the [blank_start]right[blank_end] off the mass spectrometer gives the [blank_start]Mr[blank_end]
- Aright
- BMr
194Other peaks on the mass spectrometer are because the molecule can split into [blank_start]fragments[blank_end] by breaking [blank_start]covalent[blank_end] bonds
- Afragments
- Bcovalent
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- Quiz on Chemistry knowledge questions , created by amy shann on 13/05/2017.
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- amy shann
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