1.        By giving reasons,predict in each of the following pairs which ion is larger:

(a)        Mg²⁺    and Ca²⁺         (b) K⁺ and Ca²⁺         (c)          Na⁺ and F^-        (d)     Cu²⁺ and Cu⁺

2.        Briefly explain the following phenomena;

(a)                      When SO2is bubbledthrough acidified aqueoussolution of potassium dichromate, K2Cr2O7, the yellow colour of the latter turns green.

(b)                     Silver Chloride is insoluble in water but readily solublein aqueous ammonia.

(c)                      Iron (ii) solutionis stored in copper vesselcontainer but Copper(ii) solution cannotbe stored in iron vessel container.

(d)                     Lead (ii) Chlorideis soluble in concentrated HCl butinsoluble in dilute     HCl.

(e)                      Concentrated sulphuric acid is a drying agent but cannotbe used to dry hydrogensulphide gas

3.        Explain the meaning of the following terms;

(a)                      Paramagnetism

(b)                     Coordination number

(c)                      A ligand

(d)                     Disproportionate reaction

(e)                      Bidentate ligand.

(f)                      Lone pair of electron.

(g)                     Polarising power.

(h)                     Polarizability

(i)                       Catenation

(j)                       Expansion of valenceshell

(k)                     Inert pair effect

(l)                       Froth floatation

(m)                    Metal ore.

(n)                     Concentration of ore.

(o)                     Chelating agent

(p)                     Hybridization of atomicorbitals

(q)                     Coordination compound

(r)                      Ligand

(s)                      Complex ion

(t)                       Counter ion

(u)                     Periodicity.

(v)                     Screening effect.

(w)                    Effective nuclear charge.

(x)                     Neutral complex

(y)                     Ionization isomerism.

4.        (a)          Write the electronic configuration of Cr³⁺, Cr    and Cu    and explainwhy Cr and Cu violet Aufbau principle.

(b)          Write down the formula of the following Chromium complex: “Dichlorobis(ethylenediamine)chromium(III) nitrateand then identifythe anionic and neutral ligand from the complex.

5.        Write the IUPAC names of the following complexes and statethe coordination numberof each central atom.

(a)                      [Pt(NH3)3C2O4Cl]Cl

(b)                     K[Au(CN)2]

(c)                      [Co(NH3)5Br]SO4

(d)                  [ Co(CO)4]⁺

6.        Explain un ionic terms, the following     facts    with the help of a chemical equation    where necessary

(a)                       Silver chloride is almost insoluble in water but     dissolves readily into    solution    when excess ammonia is added.

(b)                      Iodine is readily soluble in a concentrated solution of potassium iodidebut only sparingly soluble in water.

(c)                       The addition of potassium cyanidesolution to a solution of silver nitrategiven a white precipitate which the dissolves in excess of potassium cyanide.

(d)                      Bromine has more electron affinitythan although they belong to the same group.

(e)                       The atomic radius of strontiumin group 2 is larger than that     of magnesium in group 2

(f)                       An hydrous aluminumchloride does not conduct electricity but is its aqueous does.

(g)                      An aqueous solutionof aluminum chlorideturns blue litmuspaper red.

(h)                      A white precipitate tend to be formed, dissolves when carbondioxide is   bubbled till excess through               calcium     hydroxide    solution.

7.        Give explanation of the following(use chemical equation where necessary).

(a)                    Aluminium metal does not reactwith hot water or stem.

(b)                   F2 and Cl2 exist gases Br2 exists in the liquidform while, I2 exist as solid.

(c)                    Lithium carbonate is easily decomposed thermally compared with sodium carbonate.

(d)                   Sodium metal is very soft compared with    magnesiummetal

(e)                    Silicon tetrachloride (SiCl4) can be hydrolyzed by water, but carbon tetrachloride (CCl4) cannot.

(f)                    Only lithium reactswith nitrogen to form nitridein group one.

(g)                   Group IV elements have in commonthe +2 and +4 oxidation states.

(h)                   Group three elementslargely show covalency

(i)                    

(j)                     Although it is hard to have

Al ³⁺ , [Al(H

O)6]3+

is stable.    At    the same is difficult to

find

[B(H O)6]3+

(k)                  

8.        (a)          State    four properties of diagonal relationship betweenBe and Al

(b)                  (i)            State    the modern period law

(ii)           What are the two factors to classify the elements in the periodictable?

(c)                      Define the following

(i)                       Electron affinity

(ii)                     Electronegativity

(iii)                    Ionization energy

9.        By using chemical equations, explain how Aluminium is extracted from Bauxite.

10.    Explain    the following

(a)                      Sodium is less reactive thanpotassium

(b)                     Sodium atom is large in size than aluminium atom

(c)                      Sodium compounds are more ionic than that Magnesium compounds.

(d)                     Sodium ion is smaller than sodium atom .

(e)                      A chlorine ion is largein size than chlorine atom.

(f)                      Chlorine is a strong oxidizingagent than iodinethough are in the same group.

(g)                     Electron affinity of elements decreasedown the groupsof the periodic table but the electron affinity of chlorine is higher than that of fluorine

(h)                     Group VII elementshave the highestelectronegativity value while group 1 elements has the lowest.

(i)                       Reducing ability of group 1 elements increases as the     group descended

(j)                       Aluninium chlorine is a Lowesacid.

(k)                     Aluminium ore is first dissolved in cryolite beforeit is electrolyzed

11.    (a)          Briefly explain the termdiagonal relationship.

(b)                         Explain the differences between graphite and diamond basingon the following properties

(i)                   Hardness

(ii)                 Electrical and thermalconductivity

(iii)                Lubricating qualities

12.    Explain the effect of hydrogen bonding on the boilingpoint and solubility of a compound

13.    Concentrated sulphuricacid should not be used to dry hydrogen sulphide. Explain

14  Briefly explain    the following terms;-

(a)                      Beryllium halides     exist in dimmers in the vapourphase while calciumhalides in the same group exist inmonomers.

(b)                     Fluorine does not dissolve in water to form hypohalous acid like chlorine

(c)                      Alkali metals are good reducingagents.

(d)                     Common chemical reducinghave no action on      aluminium are

(e)                      BF3 is Lewis acid

(f)                      BF3 non polar but NH3 is polar.

(g)                     Aluminium fluoride has much high melting point than aluminium chloride

(h)                     Alkaline metals are not involvedin complex compound formation

(i)                       Alkaline    metals    does not occur uncombined in nature

(j)                       A solutionof ammonium ethanoate has a P^H  of 7

(k)                     Potassium ion (K ⁺ ) is smaller than chlorine ion (Cl ⁺ )

through

15.    With the aid of well labelled diagramdescribe how iron is extractedfrom its haematiteore.

16.  (a)           Give the oxidation state and coordination number of the central metalatoms in the following complexes.

(i)           K3 [Co(C2O4)2]

(ii)                     (NH4)2 [CoF6]

(iii)                    [Mn(H2O)6]SO4

(iv)                    [Cr(en)2Cl2]Cl

(b)        Write the IUPAC names of the coordination compoundsin  6 (a) above.

17.    Explain the following observations;-

(a)                      When potassium permanganate is used I volumetric analysisit is acidified using dilute sulphuric acid but                    not dilute hydrochloric acid or nitric acid

(b)                     Aqueous sodium hydroxide absorbs carbon dioxidereadily but it is neverused to test the gas.

(c)                      Nitric acid can be storedaluminium tanks but it is sulphuric acid or sodiumhydroxide

(d)                     Silicon has a much highermelting point than it is expected

(e)                      Graphite is used as a lubricant as well as cellelectrode but not diamond

(f)                      The first ionization energy of oxygenis lower than that of nitrogen althoughoxygen is towards the right across period two in the periodic table.

(g)                     Carbon dioxide is a gas at room temperature while silicon dioxideis solid

(h)                     Calcium carbonate    is insolublein water but dissolve in presence of dissolved carbon dioxide.

(i)                       While the pentavalent compounds of nitrogendo not exist.

19.                  (a)          Explain brieflyhow the oxide ores arereduced in the process of metal extraction.

(b)                     What is the difference between;-

(i)                       Calcination and roastingof metal ores.

(ii)                     Ore and mineral.

(c)                      With the aid of well balanced chemicalequations ,explain how tin is extracted from its Ore

(d)                     Discuss the environment effect of extraction metals and their remedial measures.

20.  (a)       Give evidence that [Co(NH3)5Cl]SO4 and [Co(NH3)5SO4 ]Cl are ionization isomers.

(b)               Draw the structures of the following compounds.

(i)                Hexaamminecolbalt(III) chloride.

(ii)               Bromopentaaquamanganese(III)sulfate.

(iii)             Potassiumtrisoxalatoferrate(III).

(iv)             Chlorodiamminemethylammineplatinum(II)  chloride.

21.  (a)     Justify the classification of manganese as a catalyst.

(b)               Give the type of hybridization of [Fe(CN)6]^-4 and draw the geometrical structureof the complex ion.

22.    Explain the following;-

(a)                      Aluminium is more metallic than boron throughboth or foundin group III of the periodic Table.

(b)                     Some compounds of lithium have a partially covalentcharacter

(c)                      Whereas carbon forms alimitless number of stable hydrides,this tendency

(d)                     Although water and hydrogen shlphideare the hydridesof the elements of the same group, boiling point of water is higher than of hydrogen sulphide

(e)                      Iodine and chlorineboth are found in group seven of the periodictable but hydrogeniodide is a stronger reducing           agent than hydrogen chloride

(f)                      Hydrogen iodide does not form hydrogen bondingwhile hydrogen fluoridedoes although both are hydrides of group seven.

(g)                     The size of electrons

Na ⁺ ion is large than of

Mg ²⁺ ion althoughboth have the same number of

23.    (a)          Compare and contrast the arrangement of elements in Mendeléev’s PeriodicTable and the Modern Periodic Table.

(b)                     Study the variation in the    first ionization of elements across period 2 and 3 and then

answer the questions that follow;-

(i)                       Explain why argonhas higher firstionization energy than the other elements in period 3.

(ii)                     Explain why Boron has lower first ionization energy than Beryllium?

(iii)                    How would the tendency to gain and loosing electronschange as you go from left to right across a period 3?Give reasons to support your answer.

(iv)                    Arrange the period3 element in order of increasing atomicsize.

24.    With the aid of chemical equation where necessary,explain the following;-

(a)                      Aluminium carbonate does not exist.

(b)                     Aqueous solution of Fe³⁺ is acidic.

(c)                      When ammonium solutionis added to into aqueousof Cu²⁺ ions,pale blue precipitate will appear ,but these will dissolve in excess of alkali to form a deep blue solution.

(d)                     Silver nitratemay react with the compound [Pt(NH3)3Cl3]Clbut not with the compound [Pt(NH3)2Cl4].

25.    Explain why Iron (Fe) ;-

(a)                      is ferromagnetic.

(b)                     Conducts heat and electricity.

(c)                      Exhibit variable oxidationstates.

(d)                     Is used as catalyst a catalyst in hydrogenation of unsaturated hydrocarbons.

26.      (a)      Give explanation on the following.

(i)                  Compounds containing the Zn²⁺ are colourless while those containing Cr³⁺ are Coloured.

(ii)                 Co(CN)6]^3- is yellow while [Co(NH3)6]³⁺  isgreen.

(b)          Consider the complex compoundof the formula [Cu(H2O)6] [ Fe(CN)6]

(i)                  What are centralmetal atoms?

(ii)                 What is anioniccomplex in the compound?

(iii)               What are oxidation states of the central metal atoms?

(iv)               Write the name of the compound ..

(c)              Write the IUPAC names of the following compounds.

(i)                  K [Al(OH)4]

(ii)                 [Co (NH3)3(H2O)2Br](NO3)2

(iii)              [Ni(CN)5]^3-

(iv)              [Cr(H2O)5Cl]Cl2.H2O.

27.            (a)      Give reasons for the following

(i)                       Transition metal ions form complexes.

(ii)                      Transition metal saltsare generally coloured

(iii)                    Transition elements have high enthalapy of hydration

(iv)                    Transition metals form alloys.

(b)               [Co(NH3)5Br]SO4 and [Co(NH3)5SO4]Br are isomers

(i)                       Which ions will these isomersyield in solution?

(ii)                      What is the coordination numberof cobalt in each isomer?

(iii)                    Given two chemicaltests that could be used to distinguish between them.

28.            (a)      Write the formulas for the following compounds, using bracketsto enclose the complex ion portion

(i)                       Bromotriammineplatinum(II) nitrite

(ii)                      Dichlorobis(ethylenediamine)cobalt(II) bromide

(iii)                    Sulphatopentaamminecobalt(III) bromide

(iv)                    Dibromotetraamminecobalt(III)tetrachlorozincate(II)

(b)               How do [PtCl2(NH3)2] and [Pt(NH3)6]Cl4 differ in theirelectrolytic conductance. What are hybridization states of Pt in these compounds?

(c)               Using well definedelectronic configuration and (when necessary) hybridization pattern account for the following

(i)                       The complex[ Fe(CN)6]^-3 is an innerorbital complex whereas[ Fe(H2O)6]⁺³ is outer orbital complex ion

(ii)                      Shape and magnetic properties of the complex[ Co(CO)4]⁺

(iii)                    Ni in its ground state appears to have unpairedelectrons but the complex [Ni(CN)4]^-2 is diamagnetic

29.            (a)      Using hybrization principles , prove that the complex

(i)                       [Ni (CN)5]^3- is dsp³ hybridized

(ii)                     [Fe (CN)6]^4- is d²sp³(ii) [CoF6]^3- is sp³d² hybridized.

(b)           Balance the followingredox reactions usinghalf oxidation and reduction

(i)    SO2 + MnO4-                                               SO42- + Mn²⁺

(ii)     H2O2    + H2C2O4                                       CO2 + H2O

(c)          What mass of KIO3 would be required to make 500cm³ of solution containing one sixtieth of a mole per litre?

30.                  Explain the following

(a)        Some of the compounds of Li have partially covalent character