Quiz
S-block chapter
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Questions in this quiz (121)
1An s-block element is one which has its [blank_start]outermost electron in an s-orbital.[blank_end]
- Aoutermost electron in an s-orbital.
2The s-block contains two [blank_start]groups of reactive metals[blank_end]- the [blank_start]alkali metals[blank_end] and the [blank_start]alkaline earth metals[blank_end].
- Agroups of reactive metals
- Balkali metals
- Calkaline earth metals
3The standard periodic table places helium in [blank_start]group 18[blank_end] because it has a [blank_start]full valence shell[blank_end] of electrons and is inert.
- Agroup 18
- Bfull valence shell
4Many foods contain s-block salts because they are [blank_start]important for bodily function[blank_end].
- Aimportant for bodily function
5Calcium salts are needed by the body for [blank_start]bone formation[blank_end].
- Abone formation
6S-block metals are not generally used in their pure forms because they are s[blank_start]oft[blank_end], r[blank_start]eactive[blank_end] and have low b[blank_start]oiling points[blank_end] and d[blank_start]ensities[blank_end].
- Aoft
- Beactive
- Coiling points
- Densities
7Group 1 metals can be used as [blank_start]cooling agents[blank_end] because they have high [blank_start]thermal conductivities[blank_end] and low [blank_start]boiling points[blank_end]. They must be used in special conditions because they are very [blank_start]reactive[blank_end].
- Athermal conductivities
- Bcooling agents
- Cboiling points
- Dreactive
8Lithium is used in batteries because it has a very negative [blank_start]standard electrode potential[blank_end] .
- Astandard electrode potential
9The s-block metals are found as [blank_start]minerals[blank_end] in nature and not in their [blank_start]native states[blank_end] because they are [blank_start]very reactive[blank_end].
- Aminerals
- Bnative states
- Cvery reactive
10There is a higher concentration of sodium salts than potassium salts in the sea because sodium salts are more [blank_start]soluble[blank_end] than potassium salts. This is because sodium ions are more [blank_start]charge dense[blank_end] than potassium ions so have a more exothermic [blank_start]enthalpy change of hydration[blank_end].
- Asoluble
- Bcharge dense
- Centhalpy change of hydration
11The sea contains high concentrations of s-block salts because they are very [blank_start]soluble[blank_end] and so they [blank_start]wash into[blank_end] the sea. The s-block ions have high [blank_start]charge density[blank_end] and therefore they have very exothermic [blank_start]enthalpy changes of hydration[blank_end].
- Awash into
- Bsoluble
- Ccharge density
- Denthalpy changes of hydration
12All reactive s-block metals are produced by [blank_start]electrolysis[blank_end] of their [blank_start]molten metal chlorides[blank_end].
- Aelectrolysis
- Bmolten metal chlorides
13Molten NaCl can be produced from the [blank_start]sea[blank_end] by first [blank_start]evaporating off the water[blank_end], then taking the solid and adding [blank_start]calcium chloride[blank_end], and finally heating to [blank_start]580 degrees[blank_end].
- Asea
- Bevaporating off the water
- Ccalcium chloride
- D580 degrees
14Molten NaCl can be produced from rock salt by adding [blank_start]calcium chloride[blank_end] and then heating to [blank_start]580 degrees[blank_end].
- Acalcium chloride
- B580 degrees
15Molten NaCl is often produced from [blank_start]rock salt[blank_end] rather than from the [blank_start]sea[blank_end] since less [blank_start]energy[blank_end] is needed.
- Arock salt
- Bsea
- Cenergy
16Sodium is produced by electrolysing [blank_start]molten sodium chloride[blank_end] in a [blank_start]downs cell[blank_end].
- Amolten sodium chloride
- Bdowns cell
17Calcium is separated from the molten sodium/calcium mixture around the cathode in the downs cell by [blank_start]cooling[blank_end] the mixture. The calcium then [blank_start]crystallises[blank_end] out because it has a larger [blank_start]melting point[blank_end] than sodium.
- Acooling
- Bcrystallises
- Cmelting point
18The solid calcium produced from the Downs cell is reused by reacting with [blank_start]molten sodium chloride[blank_end] to produce [blank_start]molten calcium chloride[blank_end] and [blank_start]sodium[blank_end].
- Amolten sodium chloride
- Bmolten calcium chloride
- Csodium
19Potassium cannot be produced by electrolysis of molten potassium chloride because it is too [blank_start]volatile[blank_end] and [blank_start]soluble[blank_end] in the [blank_start]melt[blank_end].
- Avolatile
- Bsoluble
- Cmelt
20Potassium is produced by reaction of molten [blank_start]potassium chloride[blank_end] with [blank_start]sodium[blank_end].
This reaction is reversible, and the potassium produced is continually [blank_start]distilled off[blank_end] to shift the [blank_start]equilibrium position[blank_end] to the right.- Apotassium chloride
- Bsodium
- Cdistilled off
- Dequilibrium position
21Lithium is produced by electrolysis of [blank_start]molten lithium chloride[blank_end].
- Amolten lithium chloride
22Rubidium is produced by reaction of molten [blank_start]rubidium chloride[blank_end] with [blank_start]sodium[blank_end].
- Arubidium chloride
- Bsodium
23Caesium is produced by reaction of molten [blank_start]caesium chloride[blank_end] with [blank_start]sodium[blank_end].
- Acaesium chloride
- Bsodium
24Chlorine is used to produce [blank_start]bleach[blank_end] and extract [blank_start]bromine[blank_end].
- Ableach
- Bbromine
25Brine is [blank_start]concentrated sodium chloride solution[blank_end]. It can be produced either from the [blank_start]sea[blank_end] or by [blank_start]pumping water[blank_end] underground into [blank_start]rock salt reserves[blank_end] and collecting the solution at the surface.
- Aconcentrated sodium chloride solution
- Bsea
- Cpumping water
- Drock salt reserves
26The products of the electrolysis of brine are [blank_start]hydrogen[blank_end], [blank_start]sodium chloride[blank_end] and [blank_start]chlorine[blank_end].
- Ahydrogen
- Bsodium chloride
- Cchlorine
27The atom economy of the electrolysis of brine is [blank_start]100%[blank_end] because all of the products can be [blank_start]sold.[blank_end]
- A100%
- Bsold.
28In the electrolysis of brine, hydrogen and NaOH are described as being [blank_start]co-products[blank_end].
- Aco-products
29Co-products are [blank_start]useful products[blank_end] produced alongside the [blank_start]desired product[blank_end] which [blank_start]can be sold[blank_end].
- Auseful products
- Bcan be sold
- Cdesired product
30Electrolysis is the [blank_start]breaking down of a compound[blank_end] using [blank_start]electricity[blank_end].
- Abreaking down of a compound
- Belectricity
31Solid ionic compounds cannot conduct electricity because the ions are held in a [blank_start]crystalline lattice structure[blank_end] by [blank_start]strong ionic bonds[blank_end] so they are [blank_start]immobile[blank_end] and cannot [blank_start]carry their charges to the electrodes[blank_end].
- Acrystalline lattice structure
- Bstrong ionic bonds
- Cimmobile
- Dcarry their charges to the electrodes
32In the electrolysis of molten NaCl, the sodium ions [blank_start]migrate[blank_end] to the [blank_start]cathode[blank_end] where they are [blank_start]reduced[blank_end], and the chloride ions [blank_start]migrate[blank_end] to the [blank_start]anode[blank_end] where they are [blank_start]oxidised[blank_end].
- Amigrate
- Bcathode
- Creduced
- Dmigrate
- Eanode
- Foxidised
33At the cathode in the electrolysis of an aqueous ionic salt, the cationic species with the more [blank_start]positive[blank_end] standard electrode potential is discharged because it is the better [blank_start]oxidising[blank_end] agent.
- Apositive
- Boxidising
34The only metals which will always be discharged at the cathode if they are present in the aqueous electrolyte are c[blank_start]opper[blank_end], t[blank_start]itanium[blank_end], s[blank_start]ilver[blank_end] and g[blank_start]old[blank_end].
- Aopper
- Bitanium
- Cilver
- Dold
35Iron, zinc and lead will only be discharged at the cathode in electrolysis if their solutions are [blank_start]concentrated[blank_end].
- Aconcentrated
36Write the half-equations for the reactions at the anode and cathode in the electrolysis of molten NaCl. Type done when done. [blank_start]Done[blank_end]
- ADone
37In electrolysis of an aqueous ionic salt, at the anode the anionic species with the more [blank_start]negative[blank_end] standard electrode potential will be discharged. This is because it is the better [blank_start]reducing[blank_end] agent.
- Anegative
- Breducing
38Hydroxide ions have a more [blank_start]negative[blank_end] standard electrode potential than chlorine and are therefore better [blank_start]reducing[blank_end] agents. Chloride ions are nonetheless discharged at the anode, because water is only a [blank_start]weak electrolyte[blank_end] so the concentration of hydroxide is [blank_start]low[blank_end]; many more chloride ions reach the anode than hydroxide ions.
- Anegative
- Breducing
- Cweak electrolyte
- Dlow
39In electrolysis of dilute NaCl, the composition of the gas produced at the anode is mainly [blank_start]oxygen[blank_end].
- Aoxygen
40Universal indicator placed around the cathode in electrolysis of NaCl will turn [blank_start]purple[blank_end] due to the concentrated [blank_start]sodium hydroxide solution[blank_end] around the cathode.
- Apurple
- Bsodium hydroxide solution
41Universal indicator solution placed around the anode in electrolysis of NaCl initially turns [blank_start]red[blank_end] and then is [blank_start]bleached[blank_end] to [blank_start]white[blank_end] by the [blank_start]chlorine[blank_end] produced around the anode.
- Ared
- Bbleached
- Cwhite
- Dchlorine
42Sodium hydroxide needs to be kept separate from [blank_start]chlorine[blank_end] because it reacts to produce [blank_start]sodium hypochlorite.[blank_end]
- Achlorine
- Bsodium hypochlorite.
43Chlorine needs to be kept separate from [blank_start]hydrogen[blank_end] because the two produce an [blank_start]explosive[blank_end] mixture.
- Ahydrogen
- Bexplosive
44Draw a membrane cell. The membrane is made of a polymer [blank_start]which only allows cations through[blank_end]. The anode is [blank_start]titanium[blank_end] and the cathode is [blank_start]nickel[blank_end]. The brine is pumped in on the [blank_start]anode[blank_end] side. The NaOH produced is [blank_start]100% pure[blank_end] unless there are [blank_start]cation impurities[blank_end] in the brine.
- Awhich only allows cations through
- Btitanium
- Cnickel
- Danode
- E100% pure
- Fcation impurities
45Draw a diaphragm cell. The diaphragm is a [blank_start]porous mixture[blank_end] of [blank_start]asbestos and polymers[blank_end] which allows the solution to [blank_start]permeate through[blank_end]. The anode is [blank_start]titanium[blank_end] and the cathode is [blank_start]steel[blank_end]. The level of solution must be higher on the [blank_start]anode[blank_end] side than the [blank_start]cathode[blank_end] side. The NaOH is contaminated with [blank_start]NaCl[blank_end].
- Aporous mixture
- Basbestos and polymers
- Cpermeate through
- Dtitanium
- Esteel
- Fanode
- Gcathode
- HNaCl
46Draw a mercury-cathode cell. [blank_start]Sodium[blank_end] is discharged on the liquid mercury cathode to form a [blank_start]sodium-mercury amalgam[blank_end]. This is reacted with [blank_start]water[blank_end] to form [blank_start]sodium hydroxide[blank_end] and reform the [blank_start]mercury[blank_end].
- ASodium
- Bsodium-mercury amalgam
- Cwater
- Dsodium hydroxide
- Emercury
47Write the half-equations of the discharge of a) Protons at the cathode and b) Hydroxide ions at the anode. Type done when done. [blank_start]Done[blank_end]
- ADone
48The enthalpy change of atomisation is a measure of the enthalpy change when [blank_start]one mole of gaseous atoms of an element[blank_end] is produced from [blank_start]the element in its standard state[blank_end].
- Aone mole of gaseous atoms of an element
- Bthe element in its standard state
49Write the general equation for the enthalpy change of atomisation of an s-block metal. Type done when done. [blank_start]Done[blank_end]
- ADone
50For a metal, the boiling point and enthalpy change of atomisation are [blank_start]directly proportional[blank_end] because both are a measure of the [blank_start]attraction between particles[blank_end] in the metallic structure.
- Adirectly proportional
- Battraction between particles
51In chlorine, the boiling point is a measure of the strength of the [blank_start]intermolecular bonds[blank_end] while the enthalpy change of atomisation is a measure of the strength of the [blank_start]Cl-Cl bond[blank_end].
- Aintermolecular bonds
- BCl-Cl bond
52In a metal, the [blank_start]valence shell orbitals[blank_end] in each atom interact with adjacent atoms.
- Avalence shell orbitals
53The MP, BP and enthalpy change of atomisation of a metal increase as the n[blank_start]uclear[blank_end] c[blank_start]harge[blank_end] increases, as the i[blank_start]onic[blank_end] r[blank_start]adius[blank_end] decreases, as the number of [blank_start]screening electrons[blank_end] decreases and as the [blank_start]charge density[blank_end] of the delocalised sea of electrons increases.
- Auclear
- Bharge
- Conic
- Dadius
- Escreening electrons
- Fcharge density
54Going from G1 to G2, the melting point [blank_start]increases,[blank_end] because the [blank_start]nuclear charge[blank_end] increases which causes the [blank_start]ionic radius[blank_end] to decrease as the outer electrons are [blank_start]dragged[blank_end] towards the nucleus. An extra [blank_start]electron[blank_end] per atom is also contributed to the delocalised electron sea, increasing its [blank_start]charge density[blank_end]. The screening effect is [blank_start]constant[blank_end].
- Aincreases,
- Bnuclear charge
- Cionic radius
- Ddragged
- Echarge density
- Felectron
- Gconstant
55As you go from Na to K, the melting point [blank_start]decreases[blank_end], because the [blank_start]ionic radius[blank_end] increases and the number of [blank_start]screening electrons[blank_end] increases. This outweighs the effect of [blank_start]increased nuclear charge[blank_end]. The charge density of the electron sea is [blank_start]constant[blank_end].
- Aionic radius
- Bdecreases
- Cscreening electrons
- Dincreased nuclear charge
- Econstant
56Deviations in the general trends of melting point across the s-block are caused by variation in the [blank_start]packing[blank_end] methods of the lattices.
- Apacking
57G1 has a [blank_start]BCC[blank_end] structure, Be and Mg have a [blank_start]HCP[blank_end] structure, Ca and Sr have a [blank_start]CCP[blank_end] structure, and Ba has a [blank_start]BCC[blank_end] structure.
- ABCC
- BHCP
- CCCP
- DBCC
58Atomic radius will decrease if the n[blank_start]uclear charge[blank_end] increases, the number of [blank_start]screening electrons[blank_end] decreases or the number of [blank_start]occupied shells[blank_end] increases.
- Auclear charge
- Bscreening electrons
- Coccupied shells
59As you go across a period, the atomic radius [blank_start]decreases[blank_end] as the [blank_start]nuclear charge[blank_end] increases so the valence electrons are [blank_start]dragged[blank_end] closer to the nucleus. The number of [blank_start]screening[blank_end] electrons is constant and the number of [blank_start]occupied shells[blank_end] are constant.
- Adecreases
- Bnuclear charge
- Cdragged
- Dscreening
- Eoccupied shells
60As you go down a group, the atomic radius [blank_start]increases[blank_end] because the number of [blank_start]occupied shells[blank_end] increases and the number of [blank_start]screening[blank_end] electrons increases. The [blank_start]nuclear charge[blank_end] also increases but its effect is outweighed.
- Aincreases
- Boccupied shells
- Cscreening
- Dnuclear charge
61Cations are always [blank_start]smaller[blank_end] than the atoms they are formed from because the number of occupied [blank_start]shells[blank_end] decreases and the number of [blank_start]screening electrons[blank_end] decreases, while the nuclear charge is [blank_start]constant[blank_end].
- Asmaller
- Bshells
- Cscreening electrons
- Dconstant
62First ionisation enthalpy is a measure of the energy required to remove the [blank_start]most loosely held[blank_end] electron from one mole of [blank_start]gaseous atoms[blank_end] to produce [blank_start]one mole of gaseous cations[blank_end] and [blank_start]one mole of electrons[blank_end].
- Amost loosely held
- Bgaseous atoms
- Cone mole of gaseous cations
- Done mole of electrons
63The first ionisation enthalpy increases as the n[blank_start]uclear charge[blank_end] increases, as the [blank_start]atomic radius[blank_end] decreases and as the number of [blank_start]screening electrons[blank_end] decreases.
- Auclear charge
- Batomic radius
- Cscreening electrons
64As you go from G1 to G2, the first ionisation enthalpy [blank_start]increases[blank_end] as the [blank_start]nuclear charge[blank_end] increases and the [blank_start]atomic radius[blank_end] decreases but the [blank_start]number of screening electrons[blank_end] remains constant.
- Aincreases
- Bnuclear charge
- Catomic radius
- Dnumber of screening electrons
65First ionisation enthalpy is often measured using [blank_start]optical spectra[blank_end]
- Aoptical spectra
66As you move down a group, the first ionisation enthalpy [blank_start]decreases[blank_end] as the atomic radius [blank_start]increases[blank_end] and the [blank_start]number of screening electrons[blank_end] increases. The nuclear charge also increases but its effect is [blank_start]outweighed[blank_end].
- Adecreases
- Bincreases
- Cnumber of screening electrons
- Doutweighed
67Electronegativity is a measure of the [blank_start]ability[blank_end] of an atom to attract a [blank_start]bonding pair of electrons[blank_end] in a [blank_start]covalent bond[blank_end] towards it.
- Aability
- Bbonding pair of electrons
- Ccovalent bond
68Electronegativity increases as nuclear charge [blank_start]increases[blank_end], [blank_start]atomic radius[blank_end] decreases and the number of screening electrons [blank_start]decreases[blank_end].
- Aincreases
- Batomic radius
- Cdecreases
69Standard electrode potential is a measure of the [blank_start]tendency[blank_end] of an element to [blank_start]ionise under standard conditions[blank_end].
- Atendency
- Bionise under standard conditions
70A negative standard electrode potential means that an element ionises [blank_start]easily[blank_end] and is therefore a good [blank_start]reducing[blank_end] agent.
- Aeasily
- Breducing
71Write a general equation for the first ionisation enthalpy of an s-block metal. Type done when done. [blank_start]done[blank_end]
- Adone
72Write the general equilibria representing the standard electrode potentials of G1 and G2 metals. Type done when done. [blank_start]done[blank_end]
- Adone
73Draw an energy diagram showing the enthalpy changes involved with the standard electrode potential equilibrium. Type done when done. [blank_start]done[blank_end]
- Adone
74The standard electrode potential becomes more negative as the first ionisation enthalpy [blank_start]decreases[blank_end] in magnitude and the hydration enthalpy [blank_start]increases[blank_end] in magnitude.
- Adecreases
- Bincreases
75In general, going down G1, the standard electrode potential becomes [blank_start]more[blank_end] negative as the [blank_start]first ionisation enthalpy[blank_end] becomes [blank_start]smaller[blank_end] in magnitude.
- Amore
- Bfirst ionisation enthalpy
- Csmaller
76Lithium has a very negative standard electrode potential because it is very [blank_start]charge dense[blank_end] and therefore has a highly exothermic [blank_start]enthalpy change of hydration[blank_end] which outweighs the endothermic [blank_start]first ionisation enthalpy[blank_end].
- Acharge dense
- Benthalpy change of hydration
- Cfirst ionisation enthalpy
77The s-block metals generally react by forming [blank_start]M+[blank_end] and [blank_start]M2+[blank_end] ions. They react with [blank_start]electronegative p-block[blank_end] elements to form ionic compounds.
- AM+
- BM2+
- Celectronegative p-block
78Metals react with p-block elements. This is because metals are good [blank_start]reducing agents[blank_end] and therefore form [blank_start]cations[blank_end] easily, and p-block elements are good [blank_start]oxidising agents[blank_end] and therefore form [blank_start]anions[blank_end] easily.
- Areducing agents
- Bcations
- Coxidising agents
- Danions
79Metals are good reducing agents because they have relatively low [blank_start]first ionisation enthalpies[blank_end].
- Afirst ionisation enthalpies
80P-block elements are good oxidising agents because they are quite [blank_start]electronegative[blank_end] and have exothermic [blank_start]first electron affinities[blank_end].
- Aelectronegative
- Bfirst electron affinities
81Ionic lattices are only stable primarily due to the highly exothermic [blank_start]lattice enthalpy[blank_end]
- Alattice enthalpy
82MgCl2 has a [blank_start]higher[blank_end] lattice enthalpy than NaCl because the Mg2+ ion has higher [blank_start]charge density[blank_end] than the Na+ ion and therefore the [blank_start]electrostatic attraction[blank_end] between ions in the lattice is stronger.
- Acharge density
- Bhigher
- Celectrostatic attraction
83NaCl2 doesn't exist as a compound because the [blank_start]second ionisation enthalpy[blank_end] of sodium is huge since the electron must be removed from a [blank_start]2p[blank_end] orbital which is much closer to the [blank_start]nucleus[blank_end] and is [blank_start]screened[blank_end] less than the 3s orbital the first electron is removed from. Hence the enthalpy of formation would be [blank_start]positive[blank_end], meaning the compound would be less stable than [blank_start]the individual elements[blank_end].
- Asecond ionisation enthalpy
- B2p
- Cnucleus
- Dscreened
- Epositive
- Fthe individual elements
84The three possible oxygen anions are: o[blank_start]xide[blank_end], p[blank_start]eroxide[blank_end] and s[blank_start]uperoxide[blank_end]. [You should write their formulae out]
- Axide
- Beroxide
- Cuperoxide
85Oxide ions are formed when an oxygen molecule splits into two [blank_start]oxygen atoms[blank_end] and then each atom gains [blank_start]two electrons[blank_end].
- Aoxygen atoms
- Btwo electrons
86Peroxide ions are formed when the double bond in an oxygen molecule becomes a [blank_start]single bond[blank_end] and before the molecule gains [blank_start]two electrons[blank_end].
- Asingle bond
- Btwo electrons
87Superoxide ions are formed when the double bond in an oxygen molecule becomes a [blank_start]single bond[blank_end] before the molecule gains [blank_start]one electron[blank_end]. Superoxide ions can also be described as being a reactive type of species called a [blank_start]radical[blank_end].
- Asingle bond
- Bone electron
- Cradical
88When an excess of s-block metal is heated in oxygen, the metal [blank_start]oxide[blank_end] is produced.
- Aoxide
89When lithium is heated in excess oxygen, lithium [blank_start]oxide[blank_end] is produced.
- Aoxide
90When sodium is heated in excess oxygen, sodium [blank_start]peroxide[blank_end] is produced.
- Aperoxide
91When potassium is heated with excess oxygen, potassium [blank_start]superoxide[blank_end] is produced.
- Asuperoxide
92When rubidium is heated with excess oxygen, rubidium [blank_start]superoxide[blank_end] is produced.
- Asuperoxide
93When caesium is heated with excess oxygen, caesium [blank_start]superoxide[blank_end] is produced.
- Asuperoxide
94When beryllium is heated in excess oxygen, beryllium [blank_start]oxide[blank_end] is produced.
- Aoxide
95When magnesium is heated in excess oxygen, magnesium [blank_start]oxide[blank_end] is produced.
- Aoxide
96When calcium is heated with excess oxygen, calcium [blank_start]peroxide[blank_end] is produced.
- Aperoxide
97When strontium is heated with excess oxygen, strontium [blank_start]peroxide[blank_end] is produced.
- Aperoxide
98When barium is heated with excess oxygen, barium [blank_start]superoxide[blank_end] is produced.
- Asuperoxide
99The order of increasing stability of oxygen anions is [blank_start]superoxide[blank_end] < [blank_start]peroxide[blank_end] < [blank_start]oxide[blank_end]
- Asuperoxide
- Bperoxide
- Coxide
100Going up a group, the oxygen anion tends to be the [blank_start]oxide[blank_end] ion, because the O-O bond in the superoxide and peroxide ions is [blank_start]weak[blank_end] and is easily broken by the distorting effect charge dense metal cations towards the top of the groups have.
- Aoxide
- Bweak
101There are fewer superoxides in group 2 than group 1 because the group 2 cations are more [blank_start]charge dense[blank_end] and therefore have a more potent polarising effect on the [blank_start]negative charge[blank_end] cloud around the anion, causing the weak [blank_start]O-O[blank_end] bond in the superoxide ion to break.
- Acharge dense
- Bnegative charge
- CO-O
102Peroxides and superoxides are used to replenish [blank_start]oxygen[blank_end] reserves and to absorb [blank_start]carbon dioxide[blank_end] on spacecraft.
- Aoxygen
- Bcarbon dioxide
103G1 metals react with [blank_start]cold[blank_end] water to produce the metal [blank_start]hydroxide[blank_end] and [blank_start]hydrogen[blank_end].
- Acold
- Bhydroxide
- Chydrogen
104The reaction between a metal and water is a [blank_start]redox[blank_end] reaction. [You should write the half-equations]
- Aredox
105Write the general equations of the reactions of G1 and G2 metals with water. Type done when done. [blank_start]done[blank_end]
- Adone
106When lithium reacts with cold water, you would observe [blank_start]effervescence[blank_end].
- Aeffervescence
107When sodium reacts with cold water, you would observe [blank_start]effervescence[blank_end] and the hydrogen produced would [blank_start]ignite[blank_end] to give an [blank_start]orange[blank_end] flame. The sodium metal would form a [blank_start]perfect sphere[blank_end].
- Aeffervescence
- Bignite
- Corange
- Dperfect sphere
108As you go down G1, the reaction between the metals and water become [blank_start]more[blank_end] vigorous because the reaction is a [blank_start]redox[blank_end] reaction and as you go down the group the metals become better [blank_start]reducing[blank_end] agents since the [blank_start]atomic radius[blank_end] increases and the number of [blank_start]screening electrons[blank_end] increases, which outweighs the effect of increased [blank_start]nuclear charge[blank_end] and means [blank_start]less[blank_end] energy is required to remove the most loosely held electron.
- Amore
- Bredox
- Creducing
- Datomic radius
- Escreening electrons
- Fnuclear charge
- Gless
109The reaction of G2 metals with water is [blank_start]less[blank_end] vigorous than that with G1 metals. The reaction is a [blank_start]redox[blank_end] reaction, and G2 metals are weaker [blank_start]reducing[blank_end] agents than G1 metals, since the [blank_start]nuclear charge[blank_end] is greater and the [blank_start]atomic radius[blank_end] is smaller, so [blank_start]more[blank_end] energy is needed to remove the most loosely held electron.
- Aless
- Bredox
- Creducing
- Dnuclear charge
- Eatomic radius
- Fmore
110When magnesium reacts with warm water, there is a [blank_start]slow[blank_end] reaction.
- Aslow
111When barium reacts with warm water, there is a [blank_start]rapid[blank_end] reaction with a steady [blank_start]stream[blank_end] of [blank_start]hydrogen[blank_end] evolving.
- Astream
- Bhydrogen
- Crapid
112Draw an energy diagram of the reaction between a G1 metal and water. Type done when done. [blank_start]done[blank_end]
- Adone
113The two steps in the dissolution of an ionic lattice are: supplying the [blank_start]lattice enthalpy[blank_end] to break up the lattice and [blank_start]hydrating[blank_end] the resulting gaseous ions.
- Alattice enthalpy
- Bhydrating
114In the G1/2 hydroxides, the solubility [blank_start]increases[blank_end] going down the group. As you go down the group, the [blank_start]charge density[blank_end] of the ions decreases so the electrostatic attractions between ions in the lattice decreases so the lattice enthalpy [blank_start]decreases[blank_end]. This outweighs the effect of the less exothermic [blank_start]hydration[blank_end] enthalpy of the cation, meaning the enthalpy change of [blank_start]solution[blank_end] becomes more exothermic.
- Aincreases
- Bcharge density
- Cdecreases
- Dhydration
- Esolution
115In the G1 chlorides, in general, the solubility [blank_start]increases[blank_end] down the group. [blank_start]Lithium[blank_end] breaks this trend. It is very charge [blank_start]dense[blank_end] and therefore [blank_start]distorts[blank_end] the negative charge cloud around the chloride ion, causing the lattice to adopt a slight [blank_start]covalent[blank_end] nature as electron density is [blank_start]shared[blank_end]. This destabilises the lattice and reduces the lattice enthalpy, thereby making the enthalpy change of solution of lithium chloride very [blank_start]exothermic[blank_end].
- Aincreases
- BLithium
- Cdense
- Ddistorts
- Ecovalent
- Fshared
- Gexothermic
116In the G2 chlorides, sulphates and carbonates, the solubility [blank_start]decreases[blank_end] down the group. As the [blank_start]charge[blank_end] density of the cations increases going up the group, the extent of [blank_start]distortion[blank_end] of the negative charge cloud around the anion increases, thereby increasing [blank_start]covalent[blank_end] nature and destabilising the lattice, making the lattice enthalpy smaller and making the enthalpy change of solution more [blank_start]exothermic[blank_end].
- Adecreases
- Bcharge
- Cdistortion
- Dcovalent
- Eexothermic
117In the G1 sulphates, the solubility generally [blank_start]increases[blank_end] down the group. However, [blank_start]lithium[blank_end] breaks this trend. It has particularly high [blank_start]charge[blank_end] density so [blank_start]distorts[blank_end] the negative charge cloud around the sulphate ion, leading to some [blank_start]covalent[blank_end] nature in the lattice, which destabilises the lattice and reduces the lattice enthalpy thereby making the enthalpy change of solution very [blank_start]exothermic[blank_end].
- Aincreases
- Blithium
- Ccharge
- Ddistorts
- Ecovalent
- Fexothermic
118Explain the trend in solubility of the G1 carbonates. Type done when done. [blank_start]done[blank_end]
- Adone
119Lithium chloride and beryllium chloride are special because they are soluble in [blank_start]organic[blank_end] solvents.
- Aorganic
120Write the general equations representing thermal decomposition of the G1 and G2 carbonates. Explain the trend in thermal stability of the carbonates. Type done when done. [blank_start]done[blank_end]
- Adone
121Write general equations of the thermal decomposition of the G1 and G2 nitrates. Explain trends in this decomposition and thermal stability. Type done when done. [blank_start]done[blank_end]
- Adone
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- Description
- Chemistry Quiz on S-block chapter, created by Dylan Reilly on 14/08/2021.
- Author
- Dylan Reilly
- Language
- English
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- 1
- History
- Created on 14 Aug 2021 · updated on 15 Aug 2021
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