Quiz
P-block chapter
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1A p-block element is one with its outermost electron in a [blank_start]p-subshell[blank_end].
- Ap-subshell
2The [blank_start]bottom left[blank_end] of the p-block is most metallic.
- Abottom right
- Bbottom left
- Ctop right
- Dtop left
3The bottom left of the p-block is most metallic because as you go left and down in the periodic table, the [blank_start]first ionisation enthalpy[blank_end] decreases so the amount of energy that must be taken in to form a metallic structure [blank_start]decreases[blank_end].
- Afirst ionisation enthalpy
- Bdecreases
4The [blank_start]top right[blank_end] of the p-block is the most non-metallic.
- Abottom right
- Bbottom left
- Ctop right
- Dtop left
5The top right of the p-block is most non-metallic because as you go up and right in the periodic table the [blank_start]first electron affinity[blank_end] becomes more exothermic and the [blank_start]electronegativity[blank_end] increases. The elements therefore become more likely to form [blank_start]an[blank_end]ions.
- Afirst electron affinity
- Belectronegativity
- Can
6[blank_start]Metalloids[blank_end] are classes of elements which exhibit properties of both metals and non-metals.
- AMetalloids
7As you go across a period, in general the first ionisation enthalpy [blank_start]increases[blank_end] because the [blank_start]nuclear charge[blank_end] increases and consequently the [blank_start]atomic radius[blank_end] decreases as the [blank_start]valence[blank_end] electrons are [blank_start]dragged[blank_end] closer towards the more charge dense nucleus. The number of screening electrons is [blank_start]constant[blank_end] and therefore the electrostatic attraction of the valence electrons to the nucleus [blank_start]increases[blank_end] so more energy must be taken in to remove the most loosely held electron.
- Aincreases
- Bnuclear charge
- Catomic radius
- Dvalence
- Edragged
- Fconstant
- Gincreases
8As you go across a period, in general the first ionisation enthalpy increases because the [blank_start]effective[blank_end] nuclear charge increases as you go across a period and the atomic radius [blank_start]decreases[blank_end], and so the electrostatic attraction of the valence electrons to the nucleus increases so the amount of energy needed to remove the most loosely held electron increases.
- Aeffective
- Bdecreases
9The effective nuclear charge is equal to the [blank_start]nuclear charge[blank_end] minus the number of [blank_start]core electrons[blank_end].
- Anuclear charge
- Bcore electrons
10As you go down a group, the effective nuclear charge is [blank_start]constant[blank_end].
- Aconstant
11As you go down a group, in general the first ionisation enthalpy decreases because the atomic radius increases as there are more [blank_start]occupied shells[blank_end] of electrons and the number of [blank_start]screening electrons[blank_end] increases- this outweighs the effect of the increased [blank_start]nuclear charge[blank_end] and so the electrostatic attraction of the valence electrons to the nucleus [blank_start]decreases[blank_end].
- Aoccupied shells
- Bscreening electrons
- Cnuclear charge
- Ddecreases
12As you go down a group, in general the first ionisation enthalpy decreases because the [blank_start]effective nuclear charge[blank_end] is constant down a group but the [blank_start]atomic radius[blank_end] increases so the electrostatic attraction of the valence electrons to the nucleus decreases.
- Aeffective nuclear charge
- Batomic radius
13As you go across a period, in general the first electron affinity becomes [blank_start]more[blank_end] exothermic, because the [blank_start]nuclear charge[blank_end] increases and consequently the atomic radius [blank_start]decreases[blank_end] as the valence electrons are [blank_start]dragged[blank_end] closer to the charge dense nucleus. The screening effect is [blank_start]constant[blank_end]. Hence, the electrostatic attraction of incoming electrons to the nucleus increases and so more energy is given out when the electron is [blank_start]incorporated[blank_end] into the atom.
- Amore
- Bnuclear charge
- Cdecreases
- Ddragged
- Econstant
- Fincorporated
14As you go across a period, in general the first electron affinity increases as the [blank_start]effective[blank_end] nuclear charge increases across a period and the atomic radius [blank_start]decreases[blank_end]. Hence the electrostatic attraction of incoming electrons to the nucleus increases so more energy is given out when the electron is incorporated into the atom.
- Aeffective
- Bdecreases
15The general trend in first ionisation energy across a period is broken at groups [blank_start]13[blank_end] and [blank_start]16[blank_end].
- A13
- B16
16The general trend in first electron affinity across a period is broken at group [blank_start]15[blank_end].
- A15
17The trend in first ionisation enthalpy is broken at group 13 because the outermost electron is in a [blank_start]p[blank_end] orbital rather than an [blank_start]s[blank_end] orbital. The p orbital is [blank_start]larger[blank_end] so the p electron is, on [blank_start]average[blank_end], further from [blank_start]the nucleus[blank_end] than the s electrons and moreover is [blank_start]screened[blank_end] by the s electrons. This outweighs the effect of increased nuclear charge and reduced atomic radius so the electron requires less energy to remove.
- Ap
- Bs
- Clarger
- Daverage
- Ethe nucleus
- Fscreened
18The trend in first ionisation enthalpy across a period is broken at group 16 because the outermost electron is in a [blank_start]doubly occupied[blank_end] p-orbital rather than a [blank_start]singly occupied[blank_end] one. The [blank_start]mutual repulsion[blank_end] between the electrons in this orbital outweighs the effect of increased nuclear charge and reduced atomic radius and so the amount of energy needed to remove the most loosely held electron decreases.
- Adoubly occupied
- Bsingly occupied
- Cmutual repulsion
19The general trend in first electron affinity across a period is broken at group 15 because the incoming electron is placed in a [blank_start]doubly occupied[blank_end] p orbital rather than a [blank_start]singly occupied[blank_end] one. The [blank_start]mutual repulsion[blank_end] between electrons in this orbital outweighs the effect of increased nuclear charge and reduced atomic radius and causes the amount of energy released when the electron is [blank_start]incorporated[blank_end] into the atom to decline.
- Adoubly occupied
- Bsingly occupied
- Cmutual repulsion
- Dincorporated
20Anionic radius follows the same trend as [blank_start]atomic radius[blank_end].
- Aatomic radius
21Write out all the period 2 fluorides and describe their properties. Type done when done. [blank_start]done[blank_end]
- Adone
22Write out all the period 3 fluorides and describe their properties. Type done when done. [blank_start]done[blank_end]
- Adone
23Write out all the period 6 fluorides and describe their properties. Type done when done. [blank_start]done[blank_end]
- Adone
24In the period 3 fluorides we observe an effect called [blank_start]octet[blank_end] expansion. This is caused by the availability of [blank_start]d-orbitals[blank_end] to participate in [blank_start]hybridisation[blank_end].
- Aoctet
- Bd-orbitals
- Chybridisation
25In the period 6 fluorides, we observe an effect called the [blank_start]inert pair[blank_end] effect. The principle of this effect is that as the atoms become larger, the tendency of [blank_start]s-electrons[blank_end] to participate in bonding declines.
- Ainert pair
- Bs-electrons
26Fluorine always gets priority with oxidation states because it is the most [blank_start]electronegative[blank_end] element and is the best [blank_start]oxidising agent[blank_end] and therefore forces the other element(s) in a compound to give up its electron(s).
- Aelectronegative
- Boxidising agent
27The period 2 p-block halides have anomalously high boiling points because these molecules have strong [blank_start]hydrogen bonds[blank_end] between them.
- Ahydrogen bonds
28The order of decreasing boiling points of the period 2 p-block hydrides is: [blank_start]water[blank_end], [blank_start]hydrogen fluoride[blank_end], [blank_start]ammonia[blank_end], [blank_start]methane[blank_end]
- Awater
- Bhydrogen fluoride
- Cammonia
- Dmethane
29Water molecules have a maximum of [blank_start]4[blank_end] hydrogen bonds between them.
- A4
30Hydrogen fluoride molecules have a maximum of [blank_start]2[blank_end] hydrogen bonds between them.
- A2
31Ammonia molecules have a maximum of [blank_start]2[blank_end] hydrogen bonds between them.
- A2
32VSPER is used to [blank_start]predict[blank_end] molecular shapes.
- Apredict
33When doing VSEPR, we assume that the shape of a molecule is determined solely by [blank_start]electron-electron interactions[blank_end].
- Aelectron-electron interactions
34The rules for VSEPR: bonding pairs and lone pairs always arrange themselves around the nucleus such that the [blank_start]extent[blank_end] of [blank_start]mutual repulsion[blank_end] between them is minimised- they will therefore arrange themselves [blank_start]as far apart[blank_end] as possible. Lone pairs occupy a [blank_start]larger solid angle[blank_end] at the nucleus than bonding pairs because lone pairs are [blank_start]closer[blank_end] to the nucleus since they are attracted to [blank_start]one[blank_end] nucleus as opposed to [blank_start]two[blank_end]. Double bonds also occupy a [blank_start]larger solid angle[blank_end] at the nucleus than single bonds because they are [blank_start]shorter[blank_end].
- Aextent
- Bmutual repulsion
- Cas far apart
- Dlarger solid angle
- Ecloser
- Fone
- Gtwo
- Hlarger solid angle
- Ishorter
35The model used to determine the molecular shapes places the nucleus at the centre of a [blank_start]sphere[blank_end]. The electrons are then placed on the [blank_start]surface of the sphere[blank_end] such that they are [blank_start]as far apart as possible[blank_end].
- Asphere
- Bsurface of the sphere
- Cas far apart as possible
36The two possibilities for arranging 4 bonding pairs are: s[blank_start]quare planar[blank_end] and t[blank_start]etrahedral[blank_end]. The bond angles for each of these respectively are [blank_start]90[blank_end] degrees and [blank_start]109.5[blank_end] degrees. The [blank_start]tetrahedral[blank_end] arrangement is preferred since the angle is [blank_start]larger[blank_end] so the electrons are further apart and thus repel less.
- Aquare planar
- Betrahedral
- C90
- D109.5
- Etetrahedral
- Flarger
37The two possibilities for arranging 5 electron pairs around the nucleus are: t[blank_start]rigonal bipyramidal[blank_end] and s[blank_start]quare based pyramid[blank_end]. The [blank_start]trigonal bipyramidal[blank_end] configuration is only slightly preferred.
- Atrigonal bipyramidal
- Brigonal bipyramidal
- Cquare based pyramid
38A square based pyramid molecular shape would be the equivalent of an [blank_start]octahedral[blank_end] geometry with one electron pair removed.
- Aoctahedral
39There are two types of groups in a trigonal bipyramid- a[blank_start]xial[blank_end] and e[blank_start]quatorial[blank_end]. These two types of groups are described as being [blank_start]chemically distinct[blank_end].
- Axial
- Bquatorial
- Cchemically distinct
40The two molecular geometries possible for 6 pairs of electrons are: o[blank_start]ctahedral[blank_end] and t[blank_start]rigonal prism[blank_end]. The [blank_start]octahedral[blank_end] geometry is preferred.
- Actahedral
- Brigonal prism
- Coctahedral
41Double and triple bonds are treated the [blank_start]same[blank_end] as single bonds when doing VSEPR because they repel to very [blank_start]similar[blank_end] extents.
- Asame
- Bsimilar
42Water has a [blank_start]bent[blank_end] molecular shape with a bond angle of [blank_start]104.5[blank_end] degrees.
- Abent
- B104.5
43Methane has a [blank_start]tetrahedral[blank_end] molecular shape with a bond angle of [blank_start]109.5[blank_end] degrees.
- Atetrahedral
- B109.5
44Ammonia has a [blank_start]trigonal pyramidal[blank_end] molecular shape with a bond angle of [blank_start]107[blank_end] degrees.
- Atrigonal pyramidal
- B107
45Hexafluorophosphate has an [blank_start]octahedral[blank_end] molecular shape with a bond angle of [blank_start]90[blank_end] degrees.
- Aoctahedral
- B90
46Sulphur dioxide has a [blank_start]trigonal planar[blank_end] molecular shape with a bond angle of [blank_start]120[blank_end] degrees.
- Atrigonal planar
- B120
47The bond angle in sulphur dioxide is very close to 120 degrees because the [blank_start]lone pair[blank_end] and [blank_start]double[blank_end] bonds repel to very similar extents.
- Alone pair
- Bdouble
48The bond angle in nitrogen dioxide is [blank_start]135[blank_end] degrees because the [blank_start]unpaired[blank_end] electron repels less than a lone pair.
- A135
- Bunpaired
49All of the G13 elements are metallic except [blank_start]boron[blank_end].
- Aboron
50Boron exists in nature as many [blank_start]allotropic forms[blank_end]. The most common form is made up of two B12 [blank_start]icosahedra[blank_end] joined by a [blank_start]B-B bond[blank_end].
- Aallotropic forms
- Bicosahedra
- CB-B bond
51Aluminium has a [blank_start]metallic[blank_end] structure.
- Ametallic
52Aluminium can be used as a pure metal in many structures despite its reactivity because there is always an [blank_start]inert[blank_end] surface layer of [blank_start]aluminium oxide[blank_end] present.
- Ainert
- Baluminium oxide
53Aluminium can be coloured by adding [blank_start]transition metal ions[blank_end] to the inert [blank_start]aluminium oxide[blank_end] surface layer.
- Atransition metal ions
- Baluminium oxide
54Aluminium is extracted from the ore [blank_start]Bauxite[blank_end]. This ore is [blank_start]hydrated[blank_end] aluminium oxide. It contains [blank_start]Iron(III) oxide[blank_end] and [blank_start]silicon dioxide[blank_end] impurities.
- ABauxite
- Bhydrated
- CIron(III) oxide
- Dsilicon dioxide
55Bauxite is treated with [blank_start]sodium hydroxide[blank_end] solution. This produces a solution containing [blank_start]sodium aluminate[blank_end] and [blank_start]sodium silicate[blank_end], and the iron is [blank_start]left behind as a solid[blank_end]. [blank_start]Carbon dioxide[blank_end] is then bubbled through the solution which causes the aluminium to [blank_start]precipitate[blank_end] out as [blank_start]aluminium hydroxide[blank_end]. The sodium silicate remains in solution. The precipitate is [blank_start]filtered[blank_end], [blank_start]washed[blank_end] and [blank_start]heated[blank_end] to form [blank_start]aluminium oxide[blank_end], which is then [blank_start]melted[blank_end] and [blank_start]electrolysed[blank_end].
- Asodium hydroxide
- Bsodium aluminate
- Csodium silicate
- Dleft behind as a solid
- ECarbon dioxide
- Faluminium hydroxide
- Gprecipitate
- Hfiltered
- Iwashed
- Jheated
- Kaluminium oxide
- Lmelted
- Melectrolysed
56Alumina [blank_start]cannot[blank_end] be reduced by heating with carbon because aluminium is a better [blank_start]reducing agent[blank_end] than carbon.
- Areducing agent
- Bcannot
57Gallium melts at [blank_start]30[blank_end] degrees and boils at [blank_start]2200[blank_end] degrees. It is special because it has the largest [blank_start]liquid range[blank_end] of any element.
- A30
- B2200
- Cliquid range
58G13 elements react either by forming [blank_start]3+[blank_end] ions (except [blank_start]boron[blank_end]) or by forming covalent compounds with general formula MX[blank_start]3[blank_end]
- A3+
- Bboron
- C3
59The chemistry of BF3 is dominated by the fact that it is an [blank_start]electron deficient[blank_end] molecule and a Lewis [blank_start]acid-[blank_end] it has a tendency to [blank_start]accept[blank_end] a pair of electrons from a Lewis [blank_start]base[blank_end] to form a [blank_start]dative[blank_end] bond.
- Aelectron deficient
- Bacid-
- Caccept
- Dbase
- Edative
60The bond order in BF3 is [blank_start]greater[blank_end] than one.
- Agreater
61The B-F bond lengths in BF3 are [blank_start]shorter[blank_end] than one would expect.
- Ashorter
62The vacant [blank_start]P[blank_end]-orbital on the boron in BF3 interacts with the [blank_start]electron density[blank_end] of the [blank_start]lone pairs[blank_end] on the fluorine atoms, resulting in slight [blank_start]dative[blank_end] bonds between the fluorines and boron.
- AP
- Belectron density
- Clone pairs
- Ddative
63Corundum is a mineral which is pure [blank_start]aluminium oxide[blank_end]
- Aaluminium oxide
64[blank_start]Corundum[blank_end] is a mineral which is pure aluminium oxide
- ACorundum
65Pure corundum looks [blank_start]clear[blank_end].
- Aclear
66If corundum contains [blank_start]chromium(III)[blank_end] ion impurities, it will appear red and is called [blank_start]ruby[blank_end].
- Achromium(III)
- Bruby
67If corundum contains [blank_start]titanium(III)[blank_end] ion impurities, it will appear blue and is called [blank_start]sapphire[blank_end].
- Atitanium(III)
- Bsapphire
68The most stable oxidation state of Tl is [blank_start]Tl(I)[blank_end] due to the [blank_start]inert pair[blank_end] effect.
- ATl(I)
- Binert pair
69When TlCl3 is heated, [blank_start]TlCl[blank_end] is produced.
- ATlCl
70The most common allotrope of carbon is [blank_start]graphite[blank_end]. The other allotrope of carbon is [blank_start]diamond[blank_end].
- Agraphite
- Bdiamond
71In graphite, each carbon is bound to [blank_start]3[blank_end] other carbons. The final valence electron becomes [blank_start]delocalised[blank_end] across the layer. The carbons in graphite are [blank_start]sp2[blank_end] hybridised. The final valence electron is in an untouched [blank_start]p[blank_end] orbital. The p orbitals of all of the carbons [blank_start]overlap[blank_end] to produce the extended [blank_start]delocalised system[blank_end] across the layer.
- A3
- Bdelocalised
- Csp2
- Dp
- Eoverlap
- Fdelocalised system
72Graphite can conduct electricity because there is an extended system of [blank_start]delocalised electrons[blank_end]. These electrons are [blank_start]mobile[blank_end] and free to move [blank_start]throughout[blank_end] the structure and carry their [blank_start]charges[blank_end] to the [blank_start]electrodes[blank_end].
- Adelocalised electrons
- Bmobile
- Cthroughout
- Delectrodes
- Echarges
73Graphite has a layered structure- the layers are made up of many [blank_start]hexagons[blank_end]. There are only weak [blank_start]intermolecular[blank_end] bonds between the layers which take little [blank_start]energy[blank_end] to overcome and therefore graphite is [blank_start]soft[blank_end] and [blank_start]slippery[blank_end].
- Asoft
- Bslippery
- Chexagons
- Dintermolecular
- Eenergy
74Diamond is the [blank_start]hardest[blank_end] naturally occuring substance.
- Ahardest
75In diamond, each carbon atom is bound to 4 other carbon atoms. Each carbon is [blank_start]sp3[blank_end] hybridised.
- Asp3
76The heavier G14 elements all have allotropes which are analogous to [blank_start]diamond[blank_end].
- Adiamond
77The evidence that graphite has an extended delocalised system is that the C-C bonds in graphite are [blank_start]shorter[blank_end] than one would expect.
- Ashorter
78Graphite can be converted to diamond through application of [blank_start]heat[blank_end] and [blank_start]pressure[blank_end]
- Aheat
- Bpressure
79Amorphous forms of carbon like [blank_start]soot[blank_end] are made up of the [blank_start]graphite[blank_end] allotrope.
- Asoot
- Bgraphite
80Buckminsterfullerene has a [blank_start]simple molecular[blank_end] structure with molecular formula [blank_start]C60[blank_end],. It is a net of h[blank_start]exagons[blank_end] and p[blank_start]entagons[blank_end] [blank_start]folded into a sphere[blank_end].
- Asimple molecular
- BC60
- Cexagons
- Dentagons
- Efolded into a sphere
81Fullerenes are used for [blank_start]drug delivery[blank_end] and for production of [blank_start]lubricants[blank_end].
- Alubricants
- Bdrug delivery
82Lead has a [blank_start]cubic close packed[blank_end] metallic structure.
- Acubic close packed
83Silicon dioxide has a [blank_start]macro[blank_end]molecular structure, within which each silicon atom is bound to [blank_start]4[blank_end] oxygen atoms and each oxygen atom is bound to [blank_start]2[blank_end] silicon atoms.
- Amacro
- B4
- C2
84Silicon dioxide is also called [blank_start]quartz[blank_end] or [blank_start]common[blank_end] sand.
- Aquartz
- Bcommon
85Silicon dioxide is used to produce [blank_start]glass[blank_end].
- Aglass
86In the production of soda-lime glass, silicon dioxide is melted with [blank_start]sodium carbonate[blank_end] and [blank_start]calcium carbonate[blank_end]. When the mixture is cooled, a solid transparent glass forms made up of s[blank_start]odium silicate[blank_end] and c[blank_start]alcium silicate[blank_end].
- Asodium carbonate
- Bcalcium carbonate
- Codium silicate
- Dalcium silicate
87Write the equations that occur in the production of soda-lime glass. Type done when done. [blank_start]done[blank_end]
- Adone
88When forming borosilicate glass (aka [blank_start]Pyrex[blank_end]), [blank_start]boron oxides[blank_end] are added to the soda-lime melt.
- Aboron oxides
- BPyrex
89Soda-lime glass can be coloured by adding [blank_start]transition metal oxides[blank_end] to the melt.
- Atransition metal oxides
90The boiling points of the group 14 elements [blank_start]decrease[blank_end] down the group because the effective nuclear charge is [blank_start]constant[blank_end] while the atomic radius [blank_start]increases[blank_end], so the electrostatic attraction of the bonding electrons in the macromolecular structures to the nuclei decrease. Hence less energy is needed to break all of the covalent bonds in the macromolecular structure.
- Adecrease
- Bconstant
- Cincreases
91The group 15 elements are called the [blank_start]pnictogens[blank_end]
- Apnictogens
92Bismuth is the heaviest element with [blank_start]non-radioactive isotopes[blank_end].
- Anon-radioactive isotopes
93[blank_start]78[blank_end]% of the air is nitrogen.
- A78
94Atmospheric nitrogen cannot be used directly by plants and animals because it is [blank_start]inert[blank_end] as a result of the strong N-N [blank_start]triple[blank_end] bond
- Ainert
- Btriple
95Nitrogen is very important in the atmosphere since it dilutes [blank_start]oxygen[blank_end] concentrations to safe levels.
- Aoxygen
96A paramagnetic species is one with a [blank_start]single unpaired electron[blank_end].
- Asingle unpaired electron
97A [blank_start]diamagnetic[blank_end] species is one without any single unpaired electrons.
- Adiamagnetic
98Nitrogen is [blank_start]diamagnetic[blank_end]
- Adiamagnetic
- Bparamagnetic
99The solid state structure of nitrogen is described as being a [blank_start]herring-bone[blank_end] structure
- Aherring-bone
100The allotropes of phosphorus are: w[blank_start]hite[blank_end], r[blank_start]ed[blank_end] and b[blank_start]lack[blank_end]
- Ahite
- Bed
- Clack
101All allotropes of phosphorus in the gas phase are [blank_start]P4[blank_end] tetrahedra
- AP4
102The solid state structure of [blank_start]white[blank_end] phosphorus is P4 tetrahedra
- Awhite
103[blank_start]Red[blank_end] and [blank_start]black[blank_end] phosphorus are stable in air
- ARed
- Bblack
104[blank_start]White[blank_end] phosphorus is unstable in air- it [blank_start]ignites[blank_end] when placed in air. Hence it must be stored [blank_start]underwater[blank_end].
- AWhite
- Bignites
- Cunderwater
105Nitrogen has distinct properties from the rest of the pnictogens because the element at the top of the group always has a very small [blank_start]atomic radius[blank_end]. Hence the [blank_start]2[blank_end]-level electrons are very close to the nucleus and furthermore they experience very little screening from the [blank_start]1[blank_end]-level electrons. Consequently the first i[blank_start]onisation enthalpy[blank_end], first e[blank_start]lectron affinity[blank_end] and [blank_start]bond enthalpy[blank_end] of the element at the top of any group is [blank_start]exaggerated[blank_end].
- Aatomic radius
- B2
- C1
- Donisation enthalpy
- Electron affinity
- Fbond enthalpy
- Gexaggerated
106Elements further down group 15 exhibit multiple oxidation states (octet expansion) since [blank_start]d[blank_end]-orbitals are available to participate in [blank_start]hybridisation[blank_end].
- Ad
- Bhybridisation
107The metallicity of elements increases down a group because the first [blank_start]ionisation enthalpy[blank_end] decreases.
- Aionisation enthalpy
108The M3- ions do not form in the pnictogens because the first [blank_start]electron affinity[blank_end] of group 15 atoms is not adequately [blank_start]exothermic[blank_end] for formation of the ion to be energetically favourable in reaction.
- Aelectron affinity
- Bexothermic
109Ammonia has a bond angle of [blank_start]107[blank_end] degrees. PH3 has a bond angle of [blank_start]90[blank_end] degrees. Both molecular shapes are described as [blank_start]trigonal pyramidal[blank_end]. The bond angle changes because ammonia undergoes [blank_start]sp3[blank_end] hybridisation while PH3 does not undergo hybridisation- rather the [blank_start]p[blank_end]-orbitals of the phosphorus overlap with the atomic orbitals of the hydrogens to form the P-H bonds.
- A107
- B90
- Ctrigonal pyramidal
- Dsp3
- Ep
110Outline the formulae and properties of all the nitrogen oxides. Type done when done. [blank_start]done[blank_end]
- Adone
111The two oxides of phosphorus are [blank_start]phosphorus(V)[blank_end] oxide, P[blank_start]4[blank_end]O[blank_start]10[blank_end] and [blank_start]phosphorus(III)[blank_end] oxide, P[blank_start]4[blank_end]O[blank_start]6[blank_end].
- Aphosphorus(V)
- B4
- C10
- Dphosphorus(III)
- E4
- F6
112Phosphorus(V) oxide is often used as a [blank_start]drying[blank_end] agent.
- Adrying
113When phosphorus(V) oxide absorbs water, it forms [blank_start]orthophosphoric[blank_end] acid.
- Aorthophosphoric
114Phosphoric acid is an important chemical because it is used to produce [blank_start]fertilisers[blank_end].
- Afertilisers
115The group 16 elements are generally called the [blank_start]chalcogens[blank_end].
- Achalcogens
116Oxygen has distinct properties from the rest of the chalcogens because the element at the top of the group has a very small [blank_start]atomic radius[blank_end] so the [blank_start]2[blank_end]-level electrons are very close to the nucleus and furthermore they experience a relatively small amount of [blank_start]screening[blank_end] from the [blank_start]1[blank_end]-level electrons. Consequently the electrostatic attraction of the valence electrons to the nucleus is very strong so the first i[blank_start]onisation enthalpy[blank_end], first e[blank_start]lectron affinity[blank_end] and [blank_start]bond enthalpy[blank_end] are exaggerated.
- Aatomic radius
- B2
- Cscreening
- D1
- Eonisation enthalpy
- Flectron affinity
- Gbond enthalpy
117In the chalcogens, [blank_start]polonium[blank_end] is a metal and [blank_start]tellurium[blank_end] is a metalloid.
- Apolonium
- Btellurium
118Oxygen is a very good [blank_start]oxidising[blank_end] agent, because it has a high [blank_start]electronegativity[blank_end] so can attract electrons towards itself to form anions, and has an exothermic [blank_start]first electron affinity[blank_end] so lots of energy is given out when the anion forms. It can oxidise nearly every [blank_start]element[blank_end].
- Aoxidising
- Belectronegativity
- Cfirst electron affinity
- Delement
119Oxygen is found in nature as a gas in the [blank_start]air[blank_end] and also [blank_start]dissolved[blank_end] in [blank_start]water[blank_end].
- Aair
- Bdissolved
- Cwater
120Oxygen can be produced in the lab through [blank_start]liquifying[blank_end] air under [blank_start]pressure[blank_end], or by [blank_start]thermal decomposition[blank_end] of potassium [blank_start]chlorate(V)[blank_end] to produce oxygen and [blank_start]potassium chloride[blank_end].
- Aliquifying
- Bpressure
- Cthermal decomposition
- Dchlorate(V)
- Epotassium chloride
121Oxygen is [blank_start]paramagnetic[blank_end].
- Aparamagnetic
- Bdiamagnetic
122The Lewis structure of oxygen would predict it to be [blank_start]diamagnetic[blank_end].
- Aparamagnetic
- Bdiamagnetic
123The two possible allotropes of oxygen are di[blank_start]oxygen[blank_end] and [blank_start]ozone[blank_end].
- Aoxygen
- Bozone
124Ozone is [blank_start]diamagnetic[blank_end]. [You should draw the structure of ozone]
- Aparamagnetic
- Bdiamagnetic
125In the troposphere, ozone is [blank_start]toxic[blank_end] and is a [blank_start]pollutant[blank_end] because it contributes to the formation of [blank_start]photochemical smogs[blank_end].
- Atoxic
- Bpollutant
- Cphotochemical smogs
126In the stratosphere, ozone is extremely important because it absorbs high energy [blank_start]UVB[blank_end] and [blank_start]UVC[blank_end] radiation when it [blank_start]photodissociates[blank_end].
- AUVB
- BUVC
- Cphotodissociates
127C[blank_start]hlorine[blank_end] radicals produced from [blank_start]CFCs[blank_end] and natural emissions of [blank_start]chloromethane[blank_end], b[blank_start]romine[blank_end] radicals produced by natural emissions of [blank_start]bromomethane[blank_end], [blank_start]hydroxyl[blank_end] radicals produced by the reaction of [blank_start]water[blank_end] molecules with [blank_start]oxygen[blank_end] radicals in the stratosphere, and [blank_start]nitric oxide[blank_end] radicals produced in [blank_start]car engines[blank_end] all act as homogenous catalysts of the destruction of ozone.
- ACFCs
- Bchloromethane
- Chlorine
- Dromine
- Ebromomethane
- Fhydroxyl
- Gwater
- Hoxygen
- Initric oxide
- Jcar engines
128Sulphur is found in nature both in [blank_start]ores[blank_end] and in its [blank_start]native state[blank_end].
- Aores
- Bnative state
129The possible allotropes of sulphur are S[blank_start]8[blank_end]. S[blank_start]12[blank_end], and S[blank_start]20[blank_end]
- A8
- B12
- C20
130Draw the side on and top down structures of S8. Type done when done. [blank_start]done[blank_end]
- Adone
131Sulphur impurities in fuels are problematic since they combust to produce [blank_start]sulphur dioxide[blank_end], which contributes to the formation of [blank_start]acid rain[blank_end].
- Asulphur dioxide
- Bacid rain
132Sulphur dioxide reacting with water produces [blank_start]sulphuric(IV)[blank_end] acid.
- Asulphuric(IV)
133Sulphur dioxide reacts with [blank_start]oxygen[blank_end] in the [blank_start]stratosphere[blank_end] to produce [blank_start]sulphur trioxide[blank_end]. Sulphur trioxide reacts with water to produce [blank_start]sulphuric(VI)[blank_end] acid.
- Asulphur trioxide
- Boxygen
- Cstratosphere
- Dsulphuric(VI)
134In industry, sulphur trioxide is formed by heating sulphur dioxide with [blank_start]oxygen[blank_end] and a [blank_start]vanadium(V) oxide[blank_end] catalyst.
- Aoxygen
- Bvanadium(V) oxide
135In the industrial production of sulphuric(VI) acid, sulphur trioxide is dissolved in [blank_start]98[blank_end]% sulphuric acid to produce [blank_start]fuming sulphuric acid[blank_end]. This is then diluted with water to form [blank_start]100[blank_end]% sulphuric acid.
- A98
- Bfuming sulphuric acid
- C100
136Sulphuric(VI) acid cannot be produced by dissolving sulphur trioxide in water because this reaction is exceptionally [blank_start]exothermic[blank_end] and is therefore [blank_start]unsafe[blank_end].
- Aexothermic
- Bunsafe
137Hydrogen sulphide is a [blank_start]foul[blank_end]-smelling gas which is more toxic than [blank_start]hydrogen cyanide[blank_end].
- Afoul
- Bhydrogen cyanide
138The bond angle in water is [blank_start]104.5[blank_end] degrees while the bond angle in hydrogen sulphide is [blank_start]90[blank_end] degrees.
- A104.5
- B90
139In water, [blank_start]sp3[blank_end] hybridisation occurs while in hydrogen sulphide, no hybridisation occurs, rather the [blank_start]p[blank_end]-orbitals of the sulphur overlap with the [blank_start]s[blank_end]-orbitals of the hydrogen to form the S-H bonds.
- Asp3
- Bp
- Cs
140The thermal stability of the hydrogen chalcogenides [blank_start]decreases[blank_end] as you go down the group. This is because the effective [blank_start]nuclear charge[blank_end] down a group is [blank_start]constant[blank_end] while the atomic radius [blank_start]increases[blank_end] as the number of occupied electron shells increases. Hence the bond enthalpy [blank_start]decreases[blank_end] since the electrostatic attraction of the bonding electrons to the nucleus decreases.
- Adecreases
- Bnuclear charge
- Cconstant
- Dincreases
- Edecreases
141In general, the boiling point of the hydrogen chalcogenides [blank_start]increases[blank_end] going down the group. This trend is broken by water because water molecules have 4 strong [blank_start]hydrogen bonds[blank_end] between them.
- Aincreases
- Bhydrogen bonds
142The group 17 elements are called the [blank_start]halogens[blank_end].
- Ahalogens
143The halogens are found in [blank_start]minerals[blank_end] and in the [blank_start]sea[blank_end] in nature. They are not found in their native states because they are too [blank_start]reactive[blank_end].
- Aminerals
- Bsea
- Creactive
144Solutions of halide salts are [blank_start]colourless[blank_end]
- Acolourless
145Solid halide salts are [blank_start]white[blank_end] crystals.
- Awhite
146The general chem. properties of the halogens are: they exist as [blank_start]diatomic molecules[blank_end], they react vigorously with the [blank_start]alkali metals[blank_end], they react with metals by acting as [blank_start]oxidising[blank_end] agents, and they react with metals to form [blank_start]white salts[blank_end].
- Adiatomic molecules
- Balkali metals
- Coxidising
- Dwhite salts
147The general physical properties of the halogens are: they form [blank_start]toxic coloured vapours[blank_end], they have relatively low [blank_start]boiling points[blank_end], they are very soluble in [blank_start]non-polar[blank_end] solvents and they are not very soluble in [blank_start]polar[blank_end] solvents.
- Atoxic coloured vapours
- Bboiling points
- Cnon-polar
- Dpolar
148Halogens react either by acting as [blank_start]oxidising[blank_end] agents and [blank_start]accepting[blank_end] an electron from a metal to form an [blank_start]anion[blank_end] or by sharing [blank_start]valence[blank_end] electrons with another non metal to form a covalent bond.
- Aoxidising
- Baccepting
- Canion
- Dvalence
149Fluorine is a [blank_start]pale yellow[blank_end] gas which is not deemed to be soluble in water because it just [blank_start]reacts[blank_end] with water to form [blank_start]hydrofluoric acid[blank_end] and [blank_start]oxygen[blank_end].
- Apale yellow
- Breacts
- Chydrofluoric acid
- Doxygen
150Chlorine is a [blank_start]pale green[blank_end] gas which forms a [blank_start]pale green[blank_end] solution in water and a [blank_start]pale green[blank_end] solution in cyclohexane.
- Apale green
- Bpale green
- Cpale green
151Bromine is a [blank_start]dark red volatile[blank_end] liquid which forms an [blank_start]orange[blank_end]/[blank_start]yellow[blank_end] solution in water and an [blank_start]orange[blank_end]/[blank_start]brown[blank_end] solution in cyclohexane
- Adark red volatile
- Borange
- Cyellow
- Dorange
- Ebrown
152Iodine is a shiny [blank_start]grey/black[blank_end] solid which [blank_start]sublimes[blank_end] on heating to produce a [blank_start]purple[blank_end] vapour. It forms an [blank_start]orange[blank_end]/[blank_start]brown[blank_end] solution in water and a [blank_start]violet[blank_end] solution in cyclohexane.
- Agrey/black
- Bpurple
- Csublimes
- Dorange
- Ebrown
- Fviolet
153The boiling points of the halogens [blank_start]increase[blank_end] down the group because the strengths of the ID-ID bonds increase as the number of [blank_start]electrons[blank_end] in the molecules increase since the strengths of the [blank_start]instantaneous[blank_end] and [blank_start]induced[blank_end] dipoles increase.
- Aincrease
- Belectrons
- Cinstantaneous
- Dinduced
154There is [blank_start]no[blank_end] real trend in solubility of the halogens in water because [blank_start]none[blank_end] of them are particularly soluble in water.
- Ano
- Bnone
155The halogens are not very soluble in water. This is because the energy that must be taken in to break the [blank_start]hydrogen[blank_end] bonds between water molecules and the [blank_start]ID-ID[blank_end] bonds between halogen molecules is greater than the amount of energy that is given out when [blank_start]PD-ID[blank_end] bonds form.
- Ahydrogen
- BID-ID
- CPD-ID
156The halogens are very soluble in non-polar solvents like cyclohexane because the amount of energy needed to be taken in to break the [blank_start]ID-ID[blank_end] bonds between the cyclohexane molecules and between the halogen molecules is equal to the amount of energy given out when new [blank_start]ID-ID[blank_end] bonds form between the cyclohexane molecules and halogen molecules.
- AID-ID
- BID-ID
157To remove ambiguity in which halogen is present in an aqueous solution, we [blank_start]shake[blank_end] the aqueous solution with [blank_start]cyclohexane[blank_end]. The [blank_start]cyclohexane[blank_end] is [blank_start]less dense[blank_end] than water and [blank_start]immiscible[blank_end] in water so forms a top layer with the unambiguous colours.
- Ashake
- Bcyclohexane
- Ccyclohexane
- Dless dense
- Eimmiscible
158The most reactive halogens are the best [blank_start]oxidising[blank_end] agents. Going down the group, the [blank_start]atomic radius[blank_end] increases as the number of occupied electron shells increases and the number of [blank_start]screening electrons[blank_end] increases. This [blank_start]outweighs[blank_end] the effect of increased nuclear charge and so the electrostatic attraction of incoming electrons to the nucleus [blank_start]decreases[blank_end] and moreover the amount of energy given out when the electron is [blank_start]incorporated[blank_end] into the atom decreases. Hence the atom less readily accepts electrons, so the reactivity of the halogens [blank_start]decreases[blank_end] down the group.
- Aoxidising
- Batomic radius
- Cscreening electrons
- Doutweighs
- Edecreases
- Fincorporated
- Gdecreases
159The most reactive halogens are the best [blank_start]oxidising[blank_end] agents. Going down the group, the [blank_start]effective nuclear charge[blank_end] is constant at [blank_start]7+[blank_end] but the atomic radius increases as more electron shells are occupied. Hence the electrostatic attraction of incoming electrons to the nucleus [blank_start]weakens[blank_end] and moreover less energy is given out when the electron is [blank_start]incorporated[blank_end] into the atom. Consequently the atom less readily accepts an electron, so the reactivity of the halogens [blank_start]decreases[blank_end] down the group.
- Aoxidising
- Beffective nuclear charge
- C7+
- Dweakens
- Eincorporated
- Fdecreases
160Write the equation of the reaction between KI and Cl2. The colour change in the reaction is from [blank_start]pale green[blank_end] to [blank_start]orange/brown[blank_end]. The [blank_start]potassium[blank_end] ions are spectator ions in the reaction. The reaction is described as being both a [blank_start]redox[blank_end] reaction and a [blank_start]displacement[blank_end] reaction.
- Apale green
- Borange/brown
- Cpotassium
- Dredox
- Edisplacement
161In a redox reaction, both [blank_start]reduction[blank_end] and [blank_start]oxidation[blank_end] occur.
- Areduction
- Boxidation
162In a displacement reaction, a [blank_start]more[blank_end] reactive species displaces a [blank_start]less[blank_end] reactive species from a [blank_start]compound[blank_end].
- Acompound
- Bmore
- Cless
163Silver chloride is [blank_start]fully[blank_end] soluble in ammonia.
- Afully
164Silver bromide is [blank_start]partially[blank_end] soluble in ammonia.
- Apartially
165Silver iodide is [blank_start]insoluble[blank_end] in ammonia.
- Ainsoluble
166Fluorine is found in nature in [blank_start]minerals[blank_end] like [blank_start]fluorspar[blank_end] (aka [blank_start]calcium fluoride[blank_end])
- Aminerals
- Bfluorspar
- Ccalcium fluoride
167Fluorine is usually produced through [blank_start]electrolysis[blank_end] of a [blank_start]molten[blank_end] mixture of [blank_start]hydrogen fluoride[blank_end] and [blank_start]potassium fluoride[blank_end].
- Aelectrolysis
- Bmolten
- Chydrogen fluoride
- Dpotassium fluoride
168It is difficult to store fluorine because it [blank_start]reacts[blank_end] with most materials. It is stored in a [blank_start]steel[blank_end] or [blank_start]monel metal[blank_end] vessel. These are protected by an [blank_start]inert[blank_end] layer of [blank_start]surface fluorides[blank_end].
- Areacts
- Bsteel
- Cmonel metal
- Dinert
- Esurface fluorides
169Poly([blank_start]tetrafluoroethene[blank_end]) is used in non-stick pans. It is resistant to chemical attack because the large fluorine atoms protect the [blank_start]carbon skeleton[blank_end] from other species.
- Atetrafluoroethene
- Bcarbon skeleton
170Fluorine reacts with water to produce [blank_start]hydrofluoric[blank_end] acid and [blank_start]oxygen[blank_end].
- Ahydrofluoric
- Boxygen
171Chlorine is found in nature mostly as [blank_start]chloride[blank_end] ions in the [blank_start]sea[blank_end].
- Achloride
- Bsea
172Chlorine is produced by [blank_start]electrolysis[blank_end] of [blank_start]brine[blank_end].
- Aelectrolysis
- Bbrine
173When chlorine is reacted with water, an [blank_start]equilibrium[blank_end] is set up between aqueous chlorine and [blank_start]hydrochloric[blank_end] acid / [blank_start]chloric(I)[blank_end] acid.
- Aequilibrium
- Bhydrochloric
- Cchloric(I)
174Chlorate (I) ions can be converted to chlorate(V) ions in a [blank_start]disproportionation[blank_end] reaction.
- Adisproportionation
175The conversion of chlorate(V) to chlorate(VII) ions is dangerous due to the risk of [blank_start]explosion[blank_end]
- Aexplosion
176Bromine is found in nature as [blank_start]bromide[blank_end] ions in the [blank_start]sea[blank_end].
- Abromide
- Bsea
177Bromine is produced by adding chlorine to [blank_start]warm[blank_end], partly [blank_start]evaporated[blank_end] seawater. This causes the bromide ions to be oxidised to [blank_start]bromine[blank_end]. [blank_start]Steam[blank_end] is then bubbled through the solution which produces a mixture of [blank_start]bromine[blank_end] and [blank_start]water[blank_end] vapour- the bromine evaporates because it is very [blank_start]volatile[blank_end]. The two vapours are [blank_start]condensed[blank_end] together and the bromine forms the [blank_start]bottom[blank_end] layer because it is more [blank_start]dense[blank_end] than water and not very [blank_start]soluble[blank_end] in water.
- Awarm
- Bevaporated
- Cbromine
- DSteam
- Ebromine
- Fwater
- Gvolatile
- Hcondensed
- Ibottom
- Jdense
- Ksoluble
178Iodine is found in nature mostly as [blank_start]iodide[blank_end] ions in the [blank_start]sea[blank_end].
- Aiodide
- Bsea
179Solutions of iodine in [blank_start]alcohol[blank_end] are useful as they are antiseptic.
- Aalcohol
180Fluorine is a particularly reactive element because the F-F bond enthalpy is unexpectedly [blank_start]low[blank_end]. This is because of the mutual [blank_start]repulsion[blank_end] between [blank_start]lone pairs[blank_end] on the nearby fluorine atoms. Hence the energy required to be taken in to break the F-F bonds in the reactants is much [blank_start]smaller[blank_end] than the energy given out when new bonds form in the products, especially since ionic and covalent bonds involving fluorine are very strong due to the high [blank_start]charge density[blank_end] of the fluoride ion and the small [blank_start]atomic radius[blank_end] of the fluorine atom.
- Alow
- Brepulsion
- Clone pairs
- Dsmaller
- Echarge density
- Fatomic radius
181In general the bond enthalpy of the halogens [blank_start]decreases[blank_end] down the group because the [blank_start]atomic radii[blank_end] increase and the number of [blank_start]screening electrons[blank_end] increases- this [blank_start]outweighs[blank_end] the effect of increased nuclear charge and means the electrostatic attraction of the bonding electrons to the nucleus is reduced.
- Adecreases
- Batomic radii
- Cscreening electrons
- Doutweighs
182Silver bromide is used in black & white [blank_start]photographic[blank_end] films. It [blank_start]decomposes[blank_end] when exposed to light, producing [blank_start]silver[blank_end]. Only a [blank_start]small[blank_end] amount of light is needed since the produced silver in turn [blank_start]induces[blank_end] production of more silver. The film is treated with [blank_start]silver thiosulphate[blank_end] solution, which causes the excess silver bromide to be removed as the soluble [blank_start][Ag(S2O3)2]3-[blank_end] ion.
- Aphotographic
- Bdecomposes
- Csilver
- Dsmall
- Einduces
- Fsilver thiosulphate
- G[Ag(S2O3)2]3-
183Hexafluoride compounds are useful because they place high [blank_start]oxidation states[blank_end] on the central atom and yet are [blank_start]covalent[blank_end] compounds. Hence the [blank_start]melting point[blank_end] is kept low. Uranium hexafluoride is used to separate the [blank_start]isotopes[blank_end] of uranium in gas [blank_start]diffusion[blank_end].
- Aoxidation states
- Bcovalent
- Cmelting point
- Disotopes
- Ediffusion
184The group 18 elements are generally called the [blank_start]noble gases[blank_end].
- Anoble gases
185The G18 elements are naturally found in the [blank_start]air[blank_end] in trace amounts. Most of them are produced by [blank_start]fractional distillation[blank_end] of liquid air.
- Aair
- Bfractional distillation
186The G18 elements have [blank_start]monatomic[blank_end] molecules.
- Amonatomic
187Helium can be produced from the [blank_start]air[blank_end], but is more commonly produced from [blank_start]natural gas wells[blank_end]. Helium exists in natural gas due to [blank_start]radioactive[blank_end] decay of elements in [blank_start]rocks[blank_end].
- Aair
- Bnatural gas wells
- Cradioactive
- Drocks
188The noble gases are unreactive because they already have a [blank_start]closed shell electron configuration[blank_end].
- Aclosed shell electron configuration
189Radon is produced from [blank_start]granite[blank_end]. It is a problem as it is [blank_start]radioactive[blank_end] and builds up in poorly [blank_start]ventilated[blank_end] buildings.
- Agranite
- Bradioactive
- Cventilated
190Helium is special as it is the only element with no [blank_start]triple point[blank_end]. This means there is no combination of temperature and pressure at which helium exists as a [blank_start]liquid[blank_end], [blank_start]solid[blank_end] and [blank_start]gas[blank_end].
- Atriple point
- Bliquid
- Csolid
- Dgas
191When helium is cooled to around 2K, it forms HeII, which is a [blank_start]superfluid[blank_end]- it can flow without [blank_start]friction[blank_end].
- Asuperfluid
- Bfriction
192Argon is used in labs to provide an [blank_start]inert[blank_end] atmosphere in which [blank_start]sensitive reactions[blank_end] can be done.
- Ainert
- Bsensitive reactions
193Most chemistry of the noble gases involves [blank_start]Xenon[blank_end]. This is because it is the most reactive non-radioactive noble gas since it has the largest [blank_start]atomic radius[blank_end] with the most [blank_start]screening electrons[blank_end], so is the only noble gas able to forcedly have an electron [blank_start]removed[blank_end] by a powerful [blank_start]oxidising[blank_end] agent like [blank_start]fluorine[blank_end] or [blank_start]oxygen[blank_end].
- AXenon
- Batomic radius
- Cscreening electrons
- Dremoved
- Efluorine
- Foxidising
- Goxygen
194Xenon difluroide, tetrafluoride and hexafluoride are produced by reacting xenon with fluorine under high [blank_start]temperature[blank_end] and [blank_start]pressure[blank_end].
- Atemperature
- Bpressure
195Explain the hybridisation, molecular geometry and isomeric form in xenon difluoride. Type done when done. [blank_start]done[blank_end]
- Adone
196Explain the hybridisation and molecular shape in xenon hexafluoride. Type done when done. [blank_start]done[blank_end]
- Adone
197When xenon hexa/tetrafluoride react with water, [blank_start]xenon trioxide[blank_end] is produced. This reaction is dangerous since there is risk of [blank_start]explosion[blank_end].
- Axenon trioxide
- Bexplosion
198Explain hybridisation and molecular shapes in XeO3, XeF4O, XeF2O2. Type done when done. [blank_start]done[blank_end]
- Adone
Informationen
- Beschreibung
- Chemistry Quiz am P-block chapter, erstellt von Dylan Reilly am 19/08/2021.
- Autor
- Dylan Reilly
- Sprache
- English
- Aufrufe
- 0
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