Which of the statements belsh)kmps* 2a,k-b wgv)oy2 xi;ow gives a correct feature of a ligand?

  Which of the following can behave as -tc sywp80k)pny 09 u4xdef(ya ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodino(dfh* 6b (cnc table is shown below:

Which of the following are the correct names for the groups labelled X, Y and Z?

  Which of the below is a chargls b-b;fw* i6/z e5egacteristic property of transition metals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of vanadium in the periodic table, n+ed+mq2.yn oas shown below: m.neod+2 qyn+

Which of the following statements is true?

  Which of the following salts would form coloured sol:rx xxyjc*+ ;m3 wbk.lutions when dissolved in wate;b3xrm: jkx l* x.ycw+r?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of first ionizatiosg)k 6z2lv rv6qmv;8t fhy+:qn energy?

  Which of the following is NOT a potential component of g,2k35sccy cqf9 k2kx acid rain?

  The $d$ orbitals of the $[Zn(H_2O)_6]^{2+}$ ion are split into two energy levels.
Why does the $[Zn(H_2O)_6]^{2+}$ ion appear colourless?

  All rain is naturally acidic due to disa 97myhc/by(gsolved __________.

  Which element would have the lea)9 2ilsbl /mffvf16ou st attraction for a shared pair of electrons in a 9bslf )612 fui/vm olfcovalent bond?

  Which of the following is NOT true of meta7iedjkkun:t;x:8x i) ls?

Iron is a magnetic eleck u 4(ny qw6wlu88i9nment in the first row of the $d$-block.
1.State two characteristic properties other than magnetism that allow iron to be classified as a transition metal.
2.State the full electron configuration for an iron atom.
3.Suggest why iron is more magnetic than scandium.

  A group 2 metal oxidva*sz7 m8)yz oe dissolved in water would produce a solution that is:

  Metalloid elements play important roles in ele 6 bqu5thlerb.n) :6zbctronic components, such as solar cells and computer chips. Which of the following is the correbh:blt brn) 665.uqz ect definition of a metalloid?

1.The valence electrons in I2IX​ are farther from their nucl+h.+1 z tynsp t5d2r 8wlxj4f.cq qg.oei than the valence elecot8z l+ft1rcwgspn+ j5qxdq.. y24h. trons in $Cl_2$. Explain how the size of the atoms in a covalent bond can affect the relative attraction to electrons and hence the bond's polarity.
2.Calculate the electronegativity differences and then deduce the type of bonding in the following compounds $Cl_2$,HCl,and NaClClX​,HCl,and NaCl (Refer to Table 8 from the data booklet) .

  Which of the following elements has the highest first ionizatixh vfxo,h/z( ;on energy?

  Which one of the following statements about fqw.z.k vbh;5 acids is/are true?
I. Acids will neutralize bases to form salts
II. Acids produce solutions with pH greater than 7
III. Acids ionize to form $H^+$ ions when dissolved in water

  Electronegativity decreases down the group. The )qs p45owhtg*two main factors causing this trend o gsq4h)t*w 5pare:

  The electron affinity of carbon is .n8 +mtk vy/-w9a xui (o njao8y9qws4$-122\,kJ\,mol^{−1}$, whereas the electron affinity of boron is $-27\,kJ\,mol^{−1}$. Which statement below best explains this difference?

  For elements in the same row X or column Y of the periolk4 kuw 67d*po y4t*f.s-pxi idic table, some features of the outer electron shell remain constantxft 4p46-k*. s7u kliiwy*odp .

Which of the following is correct?

Scandium is a transition metal that can form bothqk*r lt6w :b* (;ehqzk 2+ and 3+ complexes.
Draw the electron in boxes notation for the 4s and 3d electrons in an $Sc^{2+}$ ion.
State the equation for the third ionization energy of scandium, and indicate which electron is lost
Explain why $[Sc(H_2O)_6]^{2+}$ is coloured whereas $[Sc(H_2O)_6]^3+$ forms a colourless aqueous solution.

  Which gives the correct correct value6uxmc1;7y2y500r*xxeuh n: .f r c/rmiew lmn of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of wx9 4-tbmbhoa;) sx* zelectrons, and these electron configurations can also be represented using orbital diagrams. Determine the identity of each element dmz-t h *;sb aw49xbox)escribed below.
1.$1s^2$ $2s^2$ $2p^6$ $3s^2$ $3p^6$ $4s^1
2.$[Ne] $3s^2$ $3p^6$
3.In Period 33 with valence electrons of $3s^2$
4.
5.An ion with +1 charge, with valence electrons of:

  What is the formula of the compound fork9 oucdepg ;;6med between lithium and nitrogen?

  Which of the following is the correct formula for stronepbq/th9k2 yd/k,p 1qm-m 8x dtium sulfide?

  Metal M is in group 2 of the periodic table. Which is the correct 8yeblu+x1 3dm formula?

  Metal M is in group 2 o54 ew1gdw /awx 5nmyr(f the periodic table. Which is the correct formula?

  Atom X is an isotope of an alkali metal. Which of th4um 3gf7k5bq8d 3tij we following is a possible symbol for atom X?'f8q4m3 7k3t5w dbi ujg

An atomic nucleus of element X is surroune4qm0 qbv.6l9adsek(h(w t 8pded by electron shells, as shown below: .ebqqa(l m8s0 4w9(keh6ptd v

1.The diagram does not fully describe the electron configuration of the atom or ion or the identity of element X.
(1)State why it is not possible to determine the position of element X in the periodic table from the electron configuration alone.
(2)An alternative method for describing the electron configuration of an atom or ion is to draw the orbitals as boxes and the electrons as arrows. The box-and-arrow diagram for a helium atom is shown below:

Draw a similar diagram for the atom or ion of element X, including labels for the occupied subshells.
(3)Suggest the block of the periodic table in which element X is likely to be found, giving a reason for your answer.
2.Element X could be found in group 1 of the periodic table.
(1)State the name given to elements in group 1 of the periodic table.1
(2)State the most likely period number of element X, assuming that the electron configuration in the diagram is as close as possible to that of the neutral atom.

  The complete electron configuration of a neutral a3 e/(mx o;g/d wewd3oltom is shown below:

In which group and period of the periodic table would this element be found?

  Which compound contains two different elemen /ixm2kx6 0wwwts with identical oxidation states?

  Which of the following statements regardi,i qbpo:/j-epten;, xng the periodic table are correct?
I. Anions have larger ionic radii than the atomic radius of their parent atom
II. Elements in the periodic table are arranged according to their number of protons
III. Elements within the same period will have similar physical properties

The table below contains data for the elements nitroy2) r16g z:qj3ky o+:ikzokycgen, fluorine, sulfur and chlorine in no particular order::1ok kyjy6 z)yqi: rk+32o zgc
Element is 1 ; Radius ($10^{−12}\,m$) is 71 ; First Ionization Energy ($kJ\,mol\,^{−1}$) is 1402.
Element is 2 ; Radius ($10^{−12}\,m$) is 104 ; First Ionization Energy ($kJ\,mol\,^{−1}$) is 1000.
Element is 3 ; Radius ($10^{−12}\,m$) is 100 ; First Ionization Energy ($kJ\,mol\,^{−1}$) is 1251.
Element is 4 ; Radius ($10^{−12}\,m$) is 60 ; First Ionization Energy ($kJ\,mol\,^{−1}$) is 1681.
1.Identify element 2 and justify your answer using the atomic radius and the first ionization energy data shown.
2.(1)Identify the number of valence electrons for element 1 and justify your answer using
the atomic radius and first ionization energy data shown.2
(2)State the electron configuration for the common ion formed from element 1.1
(3)Using section 9 (Section 10- 2025 Syllabus) in the data booklet, compare the size of the ionic radius of the common ion formed from element 1 to its atomic radius. Explain this change in size.2
3.An electron affinity for element 1 is not published and the electron affinity for element 4 is -328 $\,kJ\,mol^{−1}$. In terms of atomic structure, explain why element 1 does not have a value for electron affinity.

  Which of the following statements are true regarding the transition metals?kd) 5by2on. d(h :6 ul+*xgbecm* obgy
I. Only the electrons found in the d orbitals are involved in bonding
II. Transition metals typically have higher electrical conductivity due to the metallic bonding of the d orbital electrons
III. All of the 3d block metals will form colored compounds

  Which of the following statements regarding the mea 2v -7kybc,ralting points of elements are correct?rykvab a ,2c-7
I. Group 17 melting points increase down the group due to increased covalent bond strength
II. Lithium has a higher melting point than potassium
III. Bromine has a higher melting point than chlorine

The period 3 elements magnesium, silicon and sulcs *bl,:vyel3 fur are found in the second, fourteenth and sixteenth columns of the pcs :*le 3vlyb,eriodic table.
1.State the name given to a column of elements in the periodic table.
2.State how the numbers of electron shells and outer shell electrons vary across period 3.
3.Selected physical properties of magnesium, silicon and sulfur are given in the table below:
Element is Magnesium ; Appearance is Shiny, grey ; Mechanical properties is Ductile
Element is Silicon ; Appearance is Shiny, grey ; Mechanical properties is Brittle
Element is Sulfur ; Appearance is Dull, yellow ; Mechanical properties is Brittle
Explain how the positions of the elements across period 3 help to explain their similarities and differences.
4.Period 3 contains more elements than period 1 but is equal in size to period 2. Suggest why the number of elements increases between periods 1 and 2 but not between periods 2 and 3.

Copper is a transition metal that reacts with ch lz .zyk)8o0wglorine to produce both $CuCl$ and $CuCl_2$​.
1.State the charge and electron configurations of copper ions in each of the above compounds.
2.Use your answer to part (a) to explain why $CuCl$ is a colourless compound whereas CuCl2CuClX​ is green-blue.
3.In the presence of excess HCl, copper ions form complexes with chloride ligands to produce $H_2[CuCl_4]$.
(1)Explain why chloride ions are able to act as ligands.2
(2)Deduce the charge of the complex ion.

1.The bonds in ammoniyhj,i2/5 fv r:kuc6 tua ($NH_3$​) are polar covalent.
(1)Draw the Lewis structure of ammonia.
(2)Explain why the covalent bonds in ammonia are polar.
(3)State the molecular geometry of ammonia.
(4)Explain why the bond angle of ammonia differs from that of the ammonium ion, $NH^{4+}$.
2.The boiling points of ammonia and the other group 15 compounds are shown.


Explain the variation of boiling points shown in the graph, using section 8 ($Section\,9- 2025\,Syllabus$) of the data booklet.

Magnesium is an element in gro2xlk+bs1 k0 8uiydkd 8up 2 of the periodic table.
1.State the full electron configuration for magnesium and the block it can be found in the periodic table.
2.Explain how successive ionization energies can prove that magnesium is in group 2 and period 3 of the periodic table.
3.State the equation for the second ionization energy of magnesium.
4.State an equation for the reaction between magnesium oxide and water, and comment on the pH of the resultant solution.
5.By referring to their relative ionization energies, compare the metallic behavior of magnesium to calcium and beryllium (values from the data booklet are not required).

  Which statement regarding the periodic tab5epl.hcc,l w +zhp1q :po0sy0 5wr, zyle is true?

  The complex ion $[Cu(NH_3)_4]^{2+}$ appears a deep blue color in aqueous solution, whereas $[CuCl_4]^{2−}$ appears a green color in aqueous solution. Which of the following statements are correct regarding the two complexes?

I. $[CuCl_4]^{2−}$ appears a green color as a result of the red light being absorbed because $Cl^−$ is a weaker field ligand than $NH_3$​
II. $[Cu(NH_3)4]^{2+}$ appears a deep blue color as a result of the blue light being absorbed because $NH_3$ is a stronger field ligand than $Cl^−$
III. $[Cu(NH_3)_4]^{2+}$ appears a deep blue color as a result of the orange light being absorbed because $NH_3$​ is a stronger field ligand than $Cl^−$

  Which is in the correct order from smallest to lar3hp / 5z5lqlpbg pnaxfr4/+ w)gest radius?

The oxides of two period 3 2 f2a5h6j0hoo f676n2p jozk iqt eyz:elements, X and Y, react in water according to the equations b60in f zh 22ojjz:t5o hfq 7oke6yp26aelow.
I. $X_2​O_{(S)​}$​ + $H_2​O_{(l)}​$ → $H_2X​O_3$$_{(aq)}$
II. $YO_{(s)}$​ + $H_2​O_{(l)​}$ → $Y(OH)_2$​$_{(aq)}$
1.Identify elements X and Y. Justify your response.
2.Predict whether element X or Y would have a higher melting point. Justify your prediction.

  Which statement regarding tauv-- m tel56e5( cfz: xmgts0he first ionization energies (A(g)→$A^{+}$(g)​+e-) of the period 2 correctly supports the evidence of sublevels in atoms?
I.Each period 2 element shows an increase in ionization energies across the table from left to right
II.Boron has a lower first ionization energy than beryllium because boron has an electron in the 2p sublevel
III.Oxygen has a lower first ionization energy than nitrogen due to oxygen’s greater effective nuclear charge

  The oxidation state of Cr does not change in jxm+tzt d +a4i6-ay+8aztcd; all of the following except:

  The oxidation number of X is t0ss:6*iab2m33u6lg qh r pqt zhe same in all the following compounds except:

The successive ionization energies for element X iuz3 ojw*3n9 1z t 2wd0tv4iodzs shown in the table below:
Successive Ionization Energies ($kJ\,mol^{−1}$):
1st IE2nd IE3rd IE4th IE5th IE6th IE7th IE8th IE
1000 2252 3363 4556 7004 8496 27108 31724
1.Write the equation that represents the 2nd ionization energy of element X.
2.Predict the number of valence electrons for element X and justify your response.
3.Another element, Y, is found below and in the same group as element X in the periodic table. The electronegativity value of element Y is 2.6. Predict a reasonable value for the electronegativity value of element X. Explain your reasoning.

  Which gives the correcodwy;*yg4ilpgje + zz /1u1a8t order of increasing radius for these isoelectronic speciel;pjy* y+4 gwa 1oid1z/eugz8s?

The bidentate ligand, phenanthroline (phen) has the structure hweps45t q2 ;uc g r;3s7oupt:s-d jw-below.



1.Use the diagram above to demonstrate how phenanthroline can act as a ligand to $M^+$ ions.
2.Phenanthroline forms the complex $[Cr(phen)_3]^{3+}$ with chromium ions.
(1)State the charge and the electron configuration of the central chromium ion.2
(2)Explain why the salts of $[Cr(phen)_3]^{3+}$ complex exhibit magnetic properties.1
3.The tetradentate (4-coordinate) ligand, salen, forms complexes with $Co^{3+}$ ions and can produce the compound [Co(salen)]Cl. Deduce the charge of the salen ligand.