Chapter 1 basics1. For an isotope of argon (Z = 18), the mass number is 40. The number of neutrons in this isotope is: 18 40 22 the same as in any other isotope of argon

2. Allotropes of sulfur include: 32S and 34S S8 and S6

S8 and [S8]2+ S in different oxidation states

3. Energy is inversely proportional to: wavelength frequency wavenumber Planck's constant

4. How many radial nodes does a 3p atomic orbital possess? 0 1 2 3

5. Which of the following atomic orbitals can overlap with an atomic orbital of the same type on an adjacent atom (both atoms lie on the x axis ) to give a π bond? 2px 3dxy 2s 3px

6. Which of the following atomic orbitals contains one nodal plane? 3s 3py 3dz2 3dxy

7. An atom with a valence electronic configuration of 1s22s22p63s23p3 belongs to group 3 5 11 15

8.An element has an outer ground state electronic configuration of 4s13d10. The element: is a metal is a non-metal is in group 10 is a liquid at 298 K

9. Sketch an MO diagram to describe the bonding in [He2]2+. From the result, you can say that: the ion is paramagnetic the ion has a bond order of zero the ion is likely to be less stable than He2

the ion is diamagnetic

10. The correct ordering of the electronegativities of the following atoms is: N < O < H H < N < O H < O < N O < N < H11. Atoms of the elements N and P have: the same number of valence electrons the same number of protons the same number of electrons the same number of neutrons

12. How many radial nodes does a 5f orbital possess? 1 0 3 5

13. For which of the following molecules would VSEPR theory predict a trigonal pyramidal structure?PF3 BF3 ClF3 BrF3

14. Which of the following molecules is non-polar? BCl3 SO2 H2S OF2

15. Sketch an MO diagram for O2. Using the information in the diagram, which statement is incorrect?O2 is diamagnetic The bond order in O2 is 2 The bonding in O2 has a π-component. The bonding in O2 has a σ-component

Chapter 2 Nuclearchemistry1. The relative penetrating powers of a- and b-particles, g radiation and neutrons (n) are: a > b > g > n n> g > b > a n> a > b > g n< a < b < g

2. An a - particle is: He2+ [He2]2+ He+ He

3. The product of the a-decay of 234U92 is 230U92 234Np93 230Th90 234Th90

4.The half-life of 222Rn is 3.82 days. The decay constant, k, is: 1.26 x 10–4 s–1 5.47 x 10–5 s–1

9.12 x 10–7 s–1 2.10 x 10–6 s–1

5.The decay of a radioactive isotope (assuming that there is no complication by decay of a daughter nuclide) follows: first order kinetics zero order kinetics second order kinetics no particular type of kinetics

6.Which of the following are transuranium elements? Pa, Np, Am Ac, Am, Bk Cf, Bk, No Th, Pu, Cm

7. Which of the following elements is not man-made? Es Bh U No

8. Deuteration of C2H5OH to C2H5OD: shifts the wavenumber for the O–H/D stretch to a higher valueshifts the wavenumber for the O–H/D stretch to a lower value has no effect on the absorption due to n(O–H/D) dramatically alters all absorptions in the IR spectrum of the compound

9. The nuclear spins of 1H and 2H are, respectively: ½ and 1 ½ and ½ 1 and ½ ½ and 0

10. The 19F NMR spectroscopic signal of NH4PF6 is a: doublet septet sextet singlet

11. The 11B{1H} NMR spectrum of H3B.PF3 is a: doublet singlet doublet of quartets doublet of quartets of quartets

12. You are trying to distinguish between Ph2PH (compound A) and Ph2PCH2PPh2(compound B) using 31P NMR spectroscopy. You would: see one signal for A and two for B. be able to readily distinguish A by running 31P and 31P{1H} NMR spectra. see a doublet in the 31P NMR spectrum of A but a triplet for B, both with large values of JPH. not be able to distinguish the compounds by this method.

13. 195Pt is spin-active with I = ½ (33.8%). The 31P{1H} NMR spectrum of cis-[PtCl2(PPh3)2] would exhibit:

a doublet superimposed on a singlet a binomial triplet a doublet two doublets

14. If you were to record the solution 31P{1H} NMR spectrum of the octahedral complexmer-[IrCl3(PEt3)3], the spectrum (assuming isotopes of Ir are not spin active) would exhibit: a doublet and a triplet with relative integrals 2:1 a doublet and a triplet with relative integrals 1:2 a singlet two singlets with relative integrals 2:1

15. WCl2F4 has an octahedral structure. Which of the following statements about the 19F NMR spectra of cis- and trans-WCl2F4 is not true. Ignore coupling to 183W. The spectrum of trans-WCl2F4 contains two signals16. The spectrum of trans-WCl2F4 contains one signal The spectrum of cis-WCl2F4contains two triplets, relative integrals 1:1 A value of J(19F-19F) can be measured from the spectrum of cis-WCl2F4

Chapter 4: Bonding in polyatomic molecules

1. Appropriate hybridization schemes for the C atoms in molecular CH3CO2H are sp3 and sp sp3 and sp2 sp2 and sp sp3 and sp3

2. sp3 hybridization would not be appropriate for the central atom in: SiF4 [PCl4]+ XeF4 [Me4N]+

3.In the equation for the normalized wavefunction: y sp = Ny2s + Ny2p, N =? ½ 1 1/√2 √2

4. sp hybridization for the C atom in CS2 is all that is required to allow for : the formation of two C=S bonds the formation of the s components of two double bonds the formation of two s bonds and two p bonds the formation of a s bond and accommodation of one lone pair

5. In an MO diagram for the formation of H2O in which the z axis bisects the H–O–H angle: the O 2pz atomic orbital interacts with an in-phase combination of H 1s atomic orbitals the O 2pz atomic orbital interacts with an out-of-phase combination of H 1s atomic orbitals the O 2pz atomic orbital is non-bonding the O 2s atomic orbital is non-bonding

6. In monomeric BH3, let an axis definition place the molecule in the xz plane. Which atomic orbital on B is non-bonding? 2s 2px 2py 2pz

10. Which statement is true about the bonding in B2H6? A localized bonding picture can be developed for B2H6 in which each B atom obeys the octet rule. Bonding pictures for B2H6 involve multicentre bridge

bonds. B-H terminal bonds cannot be considered as 2c-2e interactions.The observed structural parameters in B2H6 suggest the presence of a localized B-B interaction.12. An MO diagram for a model compound XH6 (Oh) can be constructed by considering the interactions between the orbitals of atom X and the LGOs for the Oh H6 fragment. What are the correct symmetry labels for these LGOs? a1g, t1u, eg a1g, t2g, eg

a1, t1, e a1, t2, e

13. The bonding in XH3 can be considered in terms of the interactions between the orbitals of atom X and the LGOs of the H3 fragment. For the LGOs, when X = B, the in-phase combination of H 1s orbitals has a1' symmetry, but when X = N, it has a1symmetry. This is because: NH3 has C3v symmetry, but BH3 belongs to the D3h point group. NH3 has D3h symmetry, but BH3 belongs to the C3v point group. NH3 has C3v symmetry, but BH3 belongs to the D3d point group. NH3 has C3 symmetry, but BH3 belongs to the C3v point group.

14. The bonding in [NO3]– can be considered in terms of a set of three resonance structures which describe the predominant contributions to the bonding. Which statement is incorrect about this set of resonance structures? Each resonance structure possesses two localized N=O double bonds. N carries a formal positive charge in each resonance structure. The set of resonance structures has to account for the equivalence of the N–O bonds. The N atom obeys the octet rule in each resonance structure.

7. Look at Figure 4.19 in Inorganic Chemistry. Which property does each of the eorbitals not possess?Lone pair character. N–H bonding character. One nodal plane. No contribution from one H 1s orbital

8. Look at Figure 4.21 in Inorganic Chemistry. Which statement is not true? All the bonding MOs involve C and H character. There are 4 bonding and 4 antibonding MOs. The molecule of diamagnetic. All the bonding MOs are equivalent

9. Look at Figures 4.27 and 4.28 in Inorganic Chemistry. Which statement is not true?All six S–F bonds in SF6 are equivalent. A reasonable bonding picture for SF6 can be developed using an S basis set of 3s and 3p orbitals. The S–F bond order is 1. SF6 is diamagnetic

Chapter 5: Structures and energetics of metallic and ionic solids

1. Which statement is incorrect about a cubic close-packed lattice? All atoms have a coordination number of 12. Layers of close-packed atoms are stacked in an ABCABC... pattern. Layers of close-packed atoms are stacked in an ABABAB... pattern.The packing is more efficient than in a body-centred cubic lattice

2. The coordination numbers of spheres in body-centred cubic, simple cubic and cubic close-packed lattices are, respectively: 8, 6, 12 6, 8, 12 6, 12, 8 8, 12, 12

3. Look at Table 5.2 in Inorganic Chemistry. Use the data to estimate the metallic radius of Ba in metallic barium at 298 K. The value (in pm) is: 231 217 215 197

4. Which statement is true? The electrical conductivity of a metal increases with temperature. The electrical conductivity of a semiconductor increases with temperature. The resistivity of a semiconductor increases with temperature Metals and semiconductors have similar electrical conducting properties

5. The behaviour of metals and semiconductors is usually discussed in terms of band theory. Which statement is not true? A partially filled band is characteristic of a metal. Doping Si with As enhances its semiconducting properties. Band gaps vary among different semiconductors but are always relatively large. Band gaps for insulators are large

6. Which statement gives incorrect information about the formation of NaCl(s) from Na(s) and Cl2(g)?Na is oxidized and Cl reduced. An ionic lattice forms. Both the ionization of Na and electron attachment to Cl are exothermic processes. When NaCl forms from its gaseous ions, energy is released.

7. Which statement is true about an XY2 lattice: the coordination number of X2n+ is twice that of Yn–

the coordination number of X2n+ is half that of Yn–

the unit cell contains twice as many X2n+ ions as Yn–

the coordination environments of X2n+ and Yn– are the same.

8. The standard enthalpy of formation of NaCl is –411 kJ mol–1. Using data from the appendices of Inorganic

Chemistry, the value of ΔlatticeHo(NaCl,s) (defined for the formation of NaCl) is determined to be: –1485 kJ mol–1 –787 kJ mol–1 +1485 kJ mol–1

+787 kJ mol–1

9. Which of the following statements is incorrectMadelung constants for MX2 lattices are greater than those for MX lattices. Use of the Born-Landé equation is restricted to lattices for which an electrostatic model is appropriate. Madelung constants are structure dependent. A lattice energy is an internal energy change, and latticeU(0 K) = latticeH(298 K).

10. Ions such as [CN]– may be regarded as being spherical in some lattices. This is because: each ion is approximately spherical the ions are freely rotating the ions are in random orientations the ions are either freely rotating or in random orientations

11. The coordination nos of Ti(IV) and O2– in rutile are, respectively: 6 and 3 3 and 6 2 and 4 4 and 2

12. An example of a compound that crystallizes with a layer structure is: CdI2 CaF2 ZnS SnO2

13. Na2S crystallizes with an antifluorite structure. Which statement is true about this structure?The coordination number of each S2– centre is 8. Each Na+ ion is within a cubic arrangement of S2– ions.The structure is based on an CaF2 structure, with Na+ ions in Na2S occupying the same sites as Ca2+ions in CaF2. The S2– ion is tetrahedrally sited.

14. Which statement is incorrect? CaO crystallizes with the CsCl structure. Wurtzite and zinc blende are polymorphs of ZnS. β-Cristobalite is one crystalline form of SiO2. CaTiO3 (perovskite) is an example of a double oxide

15. A unit cell of ReO3 consists of a cubic arrangement of Re atoms with O atoms centred along each edge of the cube. The coordination number of each Re atom is: 6 3 8 2

Chapter 6 Acids bases ions and aqueous solutions

1. In group 1, values of the first ionization energies follow the order Li > Na > K Na > K ≈ Rb ≈ Cs K > Na > Li Rb > K > Na

2. In group 1, values of the metallic radii follow the order: Li > Na > K Na < K < Rb K > Rb > Cs Cs < K < Li

3. Which ion liberates the most energy on hydration? Na+ K+ Rb+ Cs+

4. Which statement is correct? Sodium nitride has the formula NaN3 K reacts with N2 to give K3NLithium nitride forms when Li reacts with N2 Solid lithium nitride is an insulator

5. Peroxide, superoxide and ozonide ions are, respectively: [O2]–, [O2]2–, [O3]– [O2]2–, [O2]–, [O3]– [O2]–, [O2]2–, [O3]2– [O2]2–, [O2]–, [O3]2–

6. Peroxide and superoxide ions are, respectively: diamagnetic and diamagnetic paramagnetic and paramagnetic paramagnetic and diamagnetic diamagnetic and paramagnetic

7. What happens when Al dissolves in aqueous NaOH? Soluble NaAl(OH)4 forms Al2O3 precipitatesAl(OH)3 precipitates [Al(OH2)6]3+ forms which then loses H+

8. When alkali metal ions are complexed with the cyclic ether 18-crown-6, the most stable complex is formed with: Li+ Na+ K+ Rb+

9.The equilibrium: 2Na = Na+ + Na– can be shifted to the right-hand side by: carrying out the reaction in liquid NH3 adding THF (a monodentate cyclic ether) to complex the cation adding 18-crown-6 (a hexadentate cyclic ether) to complex the cation forming a cryptate complex

10. Sodium amalgam is used as: an oxidizing agent a reducing agent a drying agent a source of Na–

11. Of the options given below, which is the safest way to dispose of Na metal? Add small amounts of Na to propan-2-ol Add small amounts of Na to ethanol Add small amounts of Na to propan-1-ol Add small amounts of Na to water

12. Na3N adopts an anti-ReO3 structure. Which statement is true about the unit cell of Na3N? N3– ions occupy corner sites Na+ ions occupy corner sites N3– ions occupy edge sites Na+ ions occupy face sites

13. HPMA (hexamethylphosphoramide,) is used in the synthesis of lithium-containing compounds under non-aqueous conditions. Which statement about HMPA is incorrect? HMPA is a non-coordinating solvent HMPA is polar HMPA dissolves LiBr HMPA has the potential to form hydrogen bonds

14. The enthalpy change for the dissociation: M2(g) → 2M(g) is: more positive for Li2 than for K2

more positive for Rb2 than for K2 more positive for Na2 than for Li2 more positive for Cs2 than for K2

15.Which statement is true? Cs reacts explosively with H2O Li reacts explosively with H2O Rb does not react with H2O The reaction between K and H2O is less vigorous than that of Na and H2O

16. Which two chemicals are manufactured on a large scale in the chloralkali industry? Na and Cl2 NaCl and Cl2 NaOH and Cl2 NaCl and NaOH

17. The Downs process is used: to manufacture NaOH to electrolyse molten NaCl as the main manufacturing process for Cl2 to manufacture NaCl

18. Which one of the following salts is sparingly soluble in water, the other salts being readily soluble? LiCl LiNO3 Li2CO3 LiI

19. Na2O reacts with water to give: NaOH as the only product NaOH and H2O2 NaOH and O2

NaOH and H2

20. Which is exothermic?K(g) + e- → K-(g) K(g) → K+(g) + e- K(s) → K(g) K+(aq) → K+(g)

Chapter 7: Reduction and oxidation

1. In which of the following is the metal reduced? (These are not balanced equations). [Fe(CN)6]4– [Fe(CN)6]3– [MnO4]– MnO2

[MnO4]2– [MnO4]– [Cr2O7]2– [CrO4]2–

2. For the cell: 2Ag+(aq) + Zn(s) 2Ag(s) + Zn2+(aq) Eo cell = 1.56 V. The value of ΔGo is:150 kJ per mole of Zn –602 kJ per mole of Ag –301 kJ per mole of Ag –301 kJ per mole of Zn

3. If ΔGo(350 K) = –72 kJ mol–1, the value of K is 5.6 x 1010 4.2 x 1012 5.5 x 1024 1.2 x 1029

4. For a thermodynamically spontaneous cell reaction, which statement is correct? Eo (reduction) must be more negative than Eo (oxidation). Eo

(oxidation) must be more negative than Eo (reduction).Eo

cell should be negative. The difference between Eo

(reduction) and Eo (oxidation) must be more than 1.0 V

5. Use Appendix 11 in Inorganic Chemistry to determine Eo

cell for the reaction: Cl2 + 2Br– 2Cl– + Br2 The value is: –2.45 V –0.27 V 0.27 V 2.45 V

6. Use Appendix 11 in Inorganic Chemistry for this question. For a Cu2+(aq) / Cu(s) half-cell (at 298 K) in which [Cu2+] = 0.02 mol dm–3, E is +0.44 V +0.39 V +0.29 V +0.24 V

7.pH affects the E value for: the reduction of [Cr2O7]2–

to Cr3+ the reduction of Cr3+ to Cr2+ the reduction of Cr2+ to Cr the reduction of Cr3+ to Cr

8. Look at Figure 7.2 in Inorganic Chemistry. In alkaline solution, the value of Eo (at pH 14) for the reduction of [MnO4]– to Mn(OH) 2 is: +0.63 V +0.55 V +0.34 V +1.69 V

9.Look at Figure 7.4 in Inorganic Chemistry. Carbon will reduce FeO to Fe at: 1500 K 900 K 700 K 500 K

11. Look at the representations of the MOs in Figure 4.23 in Inorganic Chemistry. Which statement about these MOs is incorrect? The a2'' MO does not possess B–F bonding character. The e' MO contains a nodal plane. The a1' MO has B–F σ-bonding character. The e' MO is one of a pair of degenerate MOs.

15.Figure 4.29 in Inorganic Chemistry gives an MO diagram for the formation of [HF2]–. Which statement is incorrect about this bonding picture? The bond order of each H–F bond is 1. There is one MO with net bonding character. The bonding can be described as a 3-centre 2-electron interaction.The σg* MO contains 3 nodal planes.

Answers chapter 41. sp3 and sp2 2. XeF4 3. 1/√2

4. the formation of the σ components of two double bonds5. the O 2pz atomic orbital interacts with an in-phase combination of H 1s atomic orbitals 6. 2py 7. lonepair character 8. All the bonding MOs are equivalent. 9. The S–F bond order is 1. 10. Bonding pictures for B2H6 involve multicentre bridge bonds. 11. The a2'' MO does not possess B–F bonding character. 12. a1g, t1u, eg 13. NH3 has C3v symmetry, but BH3 belongs to the D3h point group 14. Each resonance structure possesses two localized N=O double bonds 15. The bond order of each H–F bond is 1.

1. n> γ > β > α 2. He2+ 3. 230 4. 2.10 x 10–6 s–1 5. first order kinetics 6. Cf, Bk, No 7 . U 8 . shifts the wavenumber for the O–H/D stretch to a lower value 9. ½ and 1 10 doublet 11. doublet of quartets 12. be able to readily distinguish A by running 31P and 31P{1H} NMR spectra 13. a doublet superimposed on a singlet 14. a doublet and a triplet with relative

integrals 2:1 15. The spectrum of trans-WCl2F4

contains two signalsAnswers 1. ClF3 2. a C2 axis 3. SO3 4. H2S and OF2

5 NH3 6 XeF4 . 7. C2v 8 C2v 9 XeF4 10 [PF6]–

11SF5Cl 12. The point group changes from D3h to Td

13. 4 vibrational modes, 2 of which are degenerate 14. 9. 15. Symmetric stretch; asymmetric stretch (doubly degenerate); one absorptionChapter1 answers?Covalent NaCp is formed. is polymeric with tetrahedral Be. Tetrahedral It is sparingly soluble in waterIn Al2Ph4(µ -C≡ CPh)2, the bridge bonds can be described in a similar way to those in Al2Me4(µ -Ph)2. Ph > Me polymeric with trigonal bipyramidal Pb.R3As from AsCl3 and a suitable Grignard reagent; R5As from oxidative addition of Cl2 to R3As and treatment with RLi. {(Me3Si)2CH}4Sn2; the Sn2C4 unit is non-planar. Me2GeCl2 + 2Li Me2Ge + 2LiClIn the solid state, Cp2Pb has a polymeric structure[(C5Me5)2Ga]+ is isostructural with [(C5Me5)2Al]+.The product contains the [Ph3C]+ ion.Cp2Mg is monomeric.A diamagnetic salt is formedChapter 3 Symmetry1. Which of the following does not contain a C3 axis? POCl3 [NH4]+ [H3O]+ ClF3

2.Which symmetry elements does cis-N2F2 contain? a C2 axis a h plane an inversion centre, I an S2 axis

3. Which if the following species possesses both C3 and C2 axes? SO3 NH3 PCl3 [H3O]+

4. Which two species belong to the same point group? XeF2 and OF2 H2O and CO2 H2S and OF2

[NO2]+ and [NO2]–

5. Which of the following belongs to the C3v point group? SO3 BBr3 NH3 AlCl3

6. Which molecule does not have Td symmetry? SiF4 P4 CH4 XeF4

7.Which molecule or ion has D3h symmetry? [H3O]+ CHCl3 [CO3]2– NF3

8. SO2 belongs to which point group? C2v C2 D∞h C2h

9. Which of the following molecules or ions possesses a C4 principal axis? XeF4 CF4 SF4 [PF4]+

10. Which of the following molecules or ions possesses an inversion centre (centre of symmetry)? [PF6]– SiH4 BF3 PF5

11. Which of the molecules or ions belongs to the C4v point group? SF5Cl [BH4]– XeF4 trans-WCl2F4

12. Which statement is true about the change in symmetry on going from BF3 to [BF4]–? The point group changes from D3h to Td The point group changes from C3v to Td The point group changes from D3h to D4h The point group changes from D3h to C3v

13. CO2 has: 3 vibrational modes 4 vibrational modes, 2 of which are degenerate stretching modes onlyan IR active symmetric stretch

14. The number of degrees of vibrational freedom possessed by CH4 is: 10 6 4 9

15. Which of the following gives the correct description of the vibrational modes of SO3, and how many absorptions do these vibrational modes give rise to in the IR spectrum of SO3? Symmetric stretch; asymmetric stretch (doubly degenerate); one absorption Symmetric stretch; asymmetric stretch (doubly degenerate); two absorptions Symmetric stretch; asymmetric stretch; two absorptions Symmetric stretch; asymmetric stretch; one absorption