Which of the statements below gives a corresdt4i )ef9*n ect feature of a ligand?

  Which of the following can behave as a phs rtdb7l*zrhu b0w2 2-)+ j3sr l;qaligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic table is showg*clbk3nx 53lr ; fi6tn 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 tranwb 23qzayp)r1 x1m2j wsition metals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of nend4+dfkyqp z)vj- c8x *.qr*1zu4j vanadium in the periodic table, as shown below: ce )dzqr -*4 funj8xykvd pnzj1+4q.*

Which of the following statements is true?

  Which of the following salts would form coloured solutions when dissolved in 5,+sa 7ow 5 e 2dec i+fw5xz4ypgf9cxzwater zwi75ce 2s,ofxw5a ge+9 xy5 c4dfz+p?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of first i. yx* e,npl:kzonization energy?

  Which of the following iswbe w 1rc;0(jj-yxgb8f 6d.v v NOT a potential component 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 due to dissolved ajz)tcjlv,:3ia+-co __________.

  Which element would have the least attraction for a shared pair of electron.( c+ dijanfca aq7j7-s in a c n+d aja(afi c7j7q-.covalent bond?

  Which of the followingqil2k e /q0qj;-2ndcim p1a2 i is NOT true of metals?

Iron is a magnetic element inds . gv+)vm5bt 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 oxide gc;7fumthy6 :ke 1x3 vdissolved in water would produce a solution that is:

  Metalloid elements play important roles in electronic com/u +u*z s/ , ghe; imsqzlcz.k6o2v;qmponents, such as solar cells and computer chips. Wm+/ v;.lszu;hc6*esiqmqzk /zgo u, 2hich of the following is the correct definition of a metalloid?

1.The valence electrons in I2IX​ are farther 6fz 9xibxo1u7 from their nuclei than the valence electro x9fzox7 b16iuns 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 ionization ener)3vb1oy:za mewn 3:lv gy?

  Which one of the following statements about acids is/ayq(7n gi2 vbnz,6g(y mre 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 m8ct675chhd e two main factors causing this trend arht8d7 56checme:

  The electron affinitydohn+hu.6 i pnzg-/793-2fm teco eqt 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,4i4 ek+7fuhao some features of the outer electron shell remaia47 hkef+oiu4 n constant.

Which of the following is correct?

Scandium is a transition me w;8.)xb7zwbq 00o 0oelrv/h qgd:xo ctal 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 correp*j t 8vx5n z)zklz1l3o7 ;ubact correct value of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, and2+e f 3m1vjpwdc.qxlt:n7 a-x these electron configurations can also be represented using orbital diagrams. Determine the ident7e-23l :fxj t nqpm cv.d+1waxity 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 compounde3j*/)taip gng9lni ( formed between lithium and nitrogen?

  Which of the following is the correct formula zovx 2 9 o y)7 (omm5:3gxvjlf-ux;sfpfor strontium sulfide?

  Metal M is in group 2 of the periodic table. Which is the correct formula,rk8dz( :ubx q8wwh9yt-evg 8?

  Metal M is in group 2 of mc y 5n i ,ly6yx.9t9yb7cwmy5:aqqi- the periodic table. Which is the correct formula?

  Atom X is an isotope of an al b3hz.;o q*ekzf.ico 0kali metal. Which of the following is a possible symbol foqb*.0;e iokzh.of z c3r atom X?'

An atomic nucleus of element X is surrounded by electron shells, as shoyw2z89 qn3*tjs pfl-vwn below: wn vzjy2 8*q9s-flpt3

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 atom ilf.jajv 1xj ycr0 9;dmlgb3/1s shown below:

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

  Which compound contains two different elements witk* tt1r-vr f6yqe4 4qwh identical oxidation states?

  Which of the following stal 9nt h n9241yym)ukk jemp2 zf+n6r9vtements regarding 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 nitrogen, fvxjj7t y2 gkg)ded01mo7k6 1iluorine, sulfur and chlorine in no particular ordkv1o 7761d2xdkjjt mye)gg 0i er:
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 followitwvdys (+p zhvfh;hg,8 - b0t9ng statements 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 r*0i*v5)smsdptums 0q egarding the melting points of elements are correctd pmms5uss*i)0v0 t *q?
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, siliconoe5 ihb zfihj3gu/ ;xsmf73/ 7 and sulfur are found in the second, fourteenth and sixteenth columns of the periodic table. /i jzmh7s7 3uo/f3gh feb;ix5
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 redq uz*uo.oazi1; a;4macts 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 ammonc2 qu.tzr-stjhp bel zvhb 0d1w8286)ia ($NH_3$​) 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 group 2 of the perio-e q g;z(5eo/chsbx4 qdic 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 rega8(qfa)anum)o no.+e nrding the periodic 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 order from sma zqf 9kne/c3+cllest to largest radius?

The oxides of two period 3 e2mv 40fmbrezcm ,ye:07 mbf 0vlements, X and Y, react in water according to the eqm0:e zbyv04 b7e,cf2 mmfrv0 muations 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(gg x0en- pv/kpmyw(0 c))→$A^{+}$(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 fo4.da.c shhru7ic: s:zllowing except:

  The oxidation number of X is the same in aka 4 o;,7rd-xkpcggu4)rxg2 cll the following compounds except:

The successive ionization energies for element X iwsf/e6tzo9hf kb)(6 qs 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 radius for these isoelectroniojd5. /y-fllipzphi;.dmd 8n* (la .nc speci .ho 8lmdlj-5in/p .a(d;f *liznp y.des?

The bidentate ligand, phenanthifeimg f.-p48roline (phen) has 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.