Which of the statements below gives a co3 ((5t u,vjo cwn izsquy6vkjq 6)t8o*rrect feature of a ligand?

  Which of the followingd65 ,pqbpnn)q can behave as a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic tabj2(gsf jp7;g:tn,jt f7g asxs3kb5+gle 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 characteristic property of transition metals?6-t+gr1p/zy6pm 2uuq bh+if x
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the 3ijun 7dmo;j738 +vxq4uxewa right of vanadium in the periodic table, as shown below:d+q3j877anw j;m oxi34vuuxe

Which of the following statements is true?

  Which of the following salts would form colourablxs,9 : 5dtl 92 vjkwefe+,yed solutions when dissolved in waterksxveb9fj5 9dyl 2a:,t le,w +?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definiuc 1f+xyt)f u jbn01x.tion of first ionization energy?

  Which of the following is NOT a potential componqy +x n)sux9q3 -)helyent of 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 ddpuxt.3j: zo z+ n1k*0wg 6:vvewi)lx ue to dissolved __________.

  Which element would have the least attraction for a shared pair of electrons m-psge38g q r1in a covalep81 e-3gsr qgmnt bond?

  Which of the following is NOT true oo4xbv2.f gjil+ p3g) k+z)x+qpawl l-f metals?

Iron is a magnetic element in the first oe m9mlf9eb+j4*ach 1row 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 wo2,ii.8yh eev uo0 jl;buld produce a solution that is:

  Metalloid elements play important roles in electronic components, such as s9dbi( l1s4g*e:cgih tolar cells and computer chips.bih t*gs14:g 9ldc (ie Which of the following is the correct definition of a metalloid?

1.The valence electrons in I2IX​ are farther from their nuclei than th m1sbjx2vvfzb.u lj(tb24c(y+l b;g3e valence y 22b+fz mbtj;((l g v4 uxjb3c1vsb.lelectrons 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 highestnn;ku 5 w7iom4 first ionization energy?

  Which one of the following statements about acids is/ary ,(6l ,ygnnsne 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 d5lv b4fsg5v ws ,c4fp52c6 ,b1aboauoown the group. The two main factors causing this trend ars bf 4cu512,bbvc,6w 5afv45gaposloe:

  The electron affinity of carbon 8h 47ttx avr3iis $-122\,kJ\,mol^{−1}$, 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 th)qw)i /5hntz he periodic table, some features of the outer electron shell remain consi) hhtzn5)/qwtant.

Which of the following is correct?

Scandium is a transit + rvzu8frjg3ta*sekt b6gefz;7 (v59ion 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 omee6 i.ghf7k +f $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, and these electron (na;f bnqf93d,t p5c xconfigurations can also be represented using orbital diagrams. Determine the idenbp a(9d xq5nfc;3n,tf tity 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 the compound formed between lithium arz)v3+21 i ggl6sf :lnq1ocj und nitrogen?

  Which of the following is the correct formulz l 47h)l)fdvhn 3s+gzet2 os*a for strontium sulfide?

  Metal M is in group 2 of the pexn s q+kww5lrn-xv,0)ss +*kz riodic table. Which is the correct formula?

  Metal M is in group 2 of the periodic table. Which is the c 4nqpk 7l x3-(pqn9xq1l vtx*forrect formula?

  Atom X is an isotope of an alkali metal. Which of the following is a possi :;ag un -meim.,pmth1ble sym; tpn ehia,mg-1m.:umbol for atom X?'

An atomic nucleus of element X is surrounded by electron shellkm0 j) vx i.3a c9knm+e,3uiqys, as shown below: kkqv3i9amxe i.uj,m03n) c y+

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..oj w4jz jxr t i0mu)l khr*l.30f8lk a neutral atom is shown below:

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

  Which compound contains two dif 9:wks8t 52rmc*9qbxccp q4fwferent elements with identical oxidation states?

  Which of the following statements regarding the periodic ta. 1o2tka,k 3vssa x;0gh,4.v8wym1ntq bbrkeble 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 bqs+ m1-o w(ohelements nitrogen, fluorine, sulfur and chlorine in no particular w mo1s(- +hqboorder:
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 statemenjr;w+ap7/ -uajn0bz c)o/fam ts 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 statemene9,.1 tn0shkd/ 7uy (vqqqcu 1yorqr4ts regarding the melting points of elements are corre4c 0yn qq9hq(u v 1sr7,y.oet/qkd1urct?
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 iyp:db0/boe k/7ky0 oz2 p izc)n the second, fourteenth and kdyobp 2zib0) z/cpy :ko/e07sixteenth 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 chlor4 std,s-u lmy)ine 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 ammoni eegt vs ;w;0zhr.ur/l:,yvn (a ($NH_3$​) 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 4- c8a fyf8:* egqxbgyin 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 tasw8xfx ,-mo;c q +9kpable 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 fo 50acv+jz(resb2ig: : nl4 be(0dnlw rom smallest to largest radius?

The oxides of two period 3 elements, X and Y, react in water accob22ldxfyu/i ,vb hvjp 3e:.6 y*kzfd -rding to the equations vyhzb,jbvldk xy /36ief2p.uf -2 *d: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 *ep kazkd*+d2 the 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 t er-z4 hl7ya3does not change in all of the following except:

  The oxidation number of X is the same in all the foleodde3ww fvl e 64c pbq2hwv8/c3(8h,lowing compounds except:

The successive ionization energies for element X is sqb + ; eu lsv1sq64+ugtrbk((zhown 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 increasiuilb7-u a sizx-t47- 6bt5j nyng radius for these isoelectronic specie-7z b bu x6j 4sny-lia7it-tu5s?

The bidentate ligand, phenanthroline (phen) has the struct+9unv 7 ux; bm h/tf52ltaz /cjebuqn84mf)m5ure 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.