Which of the statemez;ywqx *c,1x mnts below gives a correct feature of a ligand?

  Which of the followin66+l+ o fcd0qp)tvuvj g can behave as a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the pe+okothw- .(nvn/ i jquj(mb8:riodic 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 characteris7et7dy waszw4z736s s7ug5 c mtic 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, as shown 5viz5 o jx-l6km7hrw .4guy7 z-2ktt cbelow:kr6v .tc7u-57l zjx2t 4ozm 5ikwy-hg

Which of the following statements is true?

  Which of the following salts would form coloured sol1vro9wmom f+(2ewbp p *x hi r6f)va:;utions when dissolved in watervrivo* ;fm6+9w(p1mh2ba :)epxwr o f?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the defini/3 ho vx0 pxy0;kkv6popdi(g;tion of first ionization energy?

  Which of the following is NOT a potential component of acid aqoba. /(tcb1rain?

  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 acidqfzje6,/ t2c x/m,idjic due to dissolved __________.

  Which element would have the least attraction for a shared pair of eleck.qid*cu8q 7 -srh1nbtrons in 8un*qi-.dr k7c1bq hs a covalent bond?

  Which of the following is NOT true of meqk7 a/vov6ns (5het.h(pq6fu j (at y6+dc)n ktals?

Iron is a magnetic element in the first row of thd9l rvm2 0i5uzs v*b8he $d$-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 oxide dissolved in wap(g*m ojgnvk:8 y0 c4vter would produce a solution that is:

  Metalloid elements play important roles in electronic components,7x s72qumo6k;kg p 7ds such as solar cells kos67sk q u;p 7m2gxd7and computer chips. Which of the following is the correct definition of a metalloid?

1.The valence electrons in I2IX​ are farther from their nuclei than the valence boe:vsv;5/dso: +pybcb 8 op7e5/eo bvsdc yv;op 7b :b8+:psolectrons 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 thek0p1s9rlhs l:rzvwfaup jr7g6 ; 0+ i (6p:sni highest first ionization energy?

  Which one of the follo/ho. :jr gk vi+ln+f7cwing statements about 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 thetfh-7eaf- ;,fa u vi1e group. The two main factors causing this trfvh-e ftfu , e1i7a-a;end are:

  The electron affinity of g3tf6zt39r.3;gzk 3 oq )bidzm u(whj carbon is $-122\,kJ\,mol^{−1}$, 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 n(qbl6:ed;l rthe periodic table, some features of the outer electron shell lb:qd;lr 6(en remain constant.

Which of the following is correct?

Scandium is a transition metal/n,+n rvzby k2 that can form both 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 val 4*jeo052fv y sfd5aipue of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, and these electro 9*ebv *l8ziei(r;o8fo o ;i:kitw5yhn configurations can also be represented using orbital diagrams. Determine the ;l it8o:oreib5(iw*y; 8* foivkeh9zidentity of each element described 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 thfx(56hb y/w8(gp1dim ukq vfk j;wx,4e compound formed between lithium and nitrogen?

  Which of the following is n .m8 -qdw*xftv3*ups the correct formula for strontium sulfide?

  Metal M is in group 2 of the perio6/g)cums7t 9qc1y y budic table. Which is the correct formula?

  Metal M is in group 2 of the periodic table 2uiq (,tt.mob. Which is the correct formula?

  Atom X is an isotope of an alkali metal. Which of the following is a possible sy w-9usl/:r )pk3znyhxmbol f9xh/lpsr u) w:y-zn3kor atom X?'

An atomic nucleus of element X is surrounded by electron shells, as60we 83 ddj2jrxtscjh)g hh -- shown below:6-rj8echw0hhd3 j)xs-d j2 tg

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 av+ i9; e5yvuw0n jb1q,0coktof a neutral atom is shown below:

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

  Which compound contains +h.az907zyknqo xr6p two different elements with identical oxidation states?

  Which of the following statements regarding the periodic table arwu)otafn;+mzs5 sejv +n+/ r0e 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 elesf2l t22kz;7t8 63dmf jxn uhzments nitrogen, fluorine, sulfur and chlorine in no particux83n6zz 2h;tdfmj7s2 lkft2 ular order:
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 are1u8o2ur acs6 t true regarding the transition metals?
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 me0;yrqlu 6gu8p )3,als2i slvdlting points of elements are cos ilg2 rl 0u,avly6;us) 8pq3drrect?
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 sulfur are found in the ha vme0t;-7ez second, fourteenth and sixteenth ae 07e;z-mvth columns of the periodic 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 chlorin6xwr qqs1m 9d-6rq3zr e 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 ammonia xak+:e, 0n9 hn6ccux b($NH_3$​) 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 elementz68x5o*zl 1ijyodrbz9 c,nxor tk(,1 in group 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 tpf x)t i xp8fjqvm0.3:able 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 largest6)o.nv/ 2c sapf(2wza )a msaf radius?

The oxides of two period 3 elemennp:ce ba;ijv *4iqep0.qgsd: .x0l5kts, X and Y, react in water according to the equie5gspnvbx: pj . .0e:i d* aqcqk04l;ations below.
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 the first ionization energies (A(g)→evyrb tam0-l ,jsa xn- 6dq+41$A^{+}$(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 all of the following naycv(9n2 vjj/;e cn4except:

  The oxidation number of X is the same in 8* - ufl6mwtygall the following compounds except:

The successive ionization ener (:v+,dqv(;z6e0i cvetwhbrhgies for element X is 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 correct order of increasing radiw lk xvks 2+k/l.,n lxk3cy31bus for these isoelectronic speciesw+k.vs kc,/3 k1blllxkxn2y3 ?

The bidentate ligand, phenanthroline (phen) has the str pk1mm1mqm wtv74wr-;ucture 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.