Which of the statements below gives a correct featurej3(: ji2cv ksjzn 5) t)xj9yy4i9s mte of a ligand?

  Which of the following can o+x3l34xmt iom:m v; qbehave as a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic table is shown below:m 9/kdml xhf(lop1u* e7se8 o*

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

  Which of the below is a characteristic property / 7f 7/iuv aj.mo(bnwgyytf4wb+7j9m9/rc orof transition metals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of vanadium inqg-*mpm)-t 7:yyvci a the periodic table, as shown below:ymm v-*p7 g)aic:q-t y

Which of the following statements is true?

  Which of the following salts would form coloured solutions whe.b6xgt 1r xa)qn dissolved in watea 1bx)6xg.rtq r?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definiti,i d gc g3ep4kir(;2lvlwe*: mon of first ionization energy?

  Which of the following is NOT a potential component oz8 zs-v9 gdxvxv.9;bc/ky uh6f 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 dissolved __________grcd-,jc)zjnc/cy/z( hw s* *.

  Which element would haveyvqy8 iszt;nm lk,,-( the least attraction for a shared pair of electrons in n- y(m q,,y t8lvskzi;a covalent bond?

  Which of the followinax9.v w/j gc*dx3/g cxg is NOT true of metals?

Iron is a magnetic element in (zkr2l bii(t 4the 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 oxide dissolved in water would produce a soxaecl3i 7143xvm )q gu uj;)-j8odgef lution that is:

  Metalloid elements play impxrfx)t-x;3fda)mi m 3yl;4 amortant roles in electronic components, such as solar cells and computer chips. Which of the following is the correct definition of x3a4i3 xx;)m d mtar)fyml-f;a metalloid?

1.The valence electrons in I2IX​ are farther from theimc3v6 fjnt6cpmz , )d61ap xt8r nuclei than the valence electrons m86xt 6 mdfc acvtpp1,z3)6njin $Cl_2$. 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 highekxhptj k/n(r +f 7;l1hst first ionization energy?

  Which one of the following statements about acids is/are true ythic 79w,n8ela.dy 4?
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. T4)+anj1t 9r teib; rehhe two main factors causing this trend ar+rb teanr)4jih ;1t9 ee:

  The electron affinit ;iygwwo 9/xvz4ac: v-x:sh ;ky of 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 the periodic table, xo;twj 1 xi,7bq7k*vj7: u,up8 ,hlkr-biuhb some features of the outer electron shell remain constan,:iqu17 ohlj7 r7,vx w *u8bxt jbphik;ubk,-t.

Which of the following is correct?

Scandium is a transitionki*z,ki qui *1 metal 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 value ofw/6h. ref n,sk3ncj c4 $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, y jpyxls,.57yand these electron conj y,py.y7 sl5xfigurations can also be represented using orbital diagrams. Determine the identity 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 of8 4vy1jusem i5u;5 ouh the compound formed between lithium and nitrogen?

  Which of the following is the correct formula for szn 5nbdr 6z07z e4g7nbtrontium sulfide?

  Metal M is in group 2 of the periodic table. r3 tyb4 hhxrq--v1uil9(;fnke b) e,r Which is the correct formula?

  Metal M is in group 2 of the periodic table ve:g/4fiu22. .7fsplvbh vce. Which is the correct formula?

  Atom X is an isotope of an alkali metal. Whe/*mx5-- okir qx/k 6hl hby2tich of the following is a possible symbol kk tx xr2/-miobe/qy5l*h6 h-for atom X?'

An atomic nucleus of element X is surrounded by electron shells, as shown bel8m dmyx/ct/skwh+/:k l7ed me191q pvow: y79mkwd1c:mk1+ d/qh8 mt/pve l/xes

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 electronms7dra x ;6a,x configuration of a neutral atom is shown below:

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

  Which compound contains two different elements with identical 6zo .e2+x wgxzr8bd0oikjn44 oxidation states?

  Which of the following statements regarding theyd.jw0v3dkn*/oz:8m v9n myd b 1g7wm 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 wjo.3o twdis78pke;* elements nitrogen, fluorine, sulfur and chlorine in no particwt j3k8w.e pi;s*oo7dular 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 statemenx3o8u)laieo 4(qy3rvau5y 1 xts are 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 melting poi,adg yq /j ;sm3wmlyb:1+h3gni4 ci 6cnts of elements are correct? jm 6g+,gwy4ic abqch3m1/syi ;d n:l3
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 fib3up) -.rt )5dpxy.w hmwu +round in the second, fourteentpirpm 3..ywhd5b +)w)uut- xrh and sixteenth 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 reactv,n;b cy7 0jqus with chlorine 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 ammonins q/3r9,pt 2,y:vr d4ahjfy ka ($NH_3$​) 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 inv2ei)d p8be9 h 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 pefk6 bol/nmfz 7q+vk2-riodic table 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 8fj4n4ai)z cg fr ab 9d.6cp7torder from smallest to largest radius?

The oxides of two period 3 elements, X and Y, react in water accorn9u58 lsk jj)p.ymw oo+ep4;rding to the equations beepj yw m485r+jpl u;ok9)nos.low.
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);a:fllw,uq 7u: x 8 he;ceqd:k→$A^{+}$(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 fol6j dwhi a2a9f2fk sb9,lowing except:

  The oxidation number of X is the same in all the following colz y)l)of/ze )mpounds except:

The successive ionization energiespfstw;0* te988 hzbxk4osg.aco9ci9 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 radiy7rwdjm si /02us for these isoelectronic speci /7y0w jri2smdes?

The bidentate ligand, phenanthroline (phen) txx74w q6p 60w9ds ;cooyr0flhas the structure 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.