Which of the statements below gives a corw1*( 0icpyae5lf1r-b qtt wy2rect feature of a ligand?

  Which of the following can behave a o98magp+5gy js a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic table is shown 5x7kqls, mdv .below:

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

  Which of the below is a characteristio e;elcli+,0 ec property of transition metals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of vanadium in the peri* *b.adxoi8 yuodic table, as shown below:.o *i* a8yxudb

Which of the following statements is true?

  Which of the following salts would form coloured sob o pzq4xo/4:zw*c74aqpwe r5kd( s 3ilutions when dissolved in wat* apw4w7/z:qd5ikb(4sx4oeqz3o p rc er?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of first ionization ener 2* gcac1gfyb9gy?

  Which of the following is NOT a potential component of acid rain5l mcvj 2z, 1yzs8b1gy?

  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 acidi:di:tpc: (9 v/qg6 as vziu*ddc due to dissolved __________.

  Which element would have the least attractiofvo(crxa t ,t.t9a-5on for a shared pair of electrons in a t9(v-,.t frooxact a5covalent bond?

  Which of the following is NOT true of mety p;uwghp e13-f b;:gtals?

Iron is a magnetic element in the first rkb4z,/bdg7eqpo+y9 wu0c e0bow 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 dissovqzk /0yy om54lved in water would produce a solution that is:

  Metalloid elements play important roles infxchr(uem5l2/rt8 l0po+p+o3 c dbv vor4s:9 electronic components, such as solar cells and computer chips. Which of the following is the r28rvde:x+c/9o0to s35cm ( plbu4+pf ovhrlcorrect definition of a metalloid?

1.The valence electrons in I2IX​ are farther from their nuclei than ts jo+n x*8aqt(k..z gihe valence electrons.g qaj(+xktz nio *8.s 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 hv /. h9r 2lguo88boi (/r;pwz+xh+sre askz5cighest first ionization energy?

  Which one of the following statements about/ 2:vda3ofuje 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 nrflt tys9cxb57t808group. The two main factors causing this trebl ct9ntyrfsx885t0 7nd are:

  The electron affinity of carbon is 85 * skzfq/jpp+tk30gw1v4du8zu r cd $-122\,kJ\,mol^{−1}$, 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;2 o7a97qaixa gkue*z of the periodic table, some features of the outer electron shell 7kaq;uo2zaea9*g x7 iremain constant.

Which of the following is correct?

Scandium is a transiibslgr)hyb7ro*9of h 6v -1, ftion 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 9r9v-x 4zk nj )hx/seshrz(iqyvm3mr10-d3v of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, and tr kv3vz6 z5gw1hese electron configurations can also be represented using orbital diagrams. Determine the identity of each element describvk rzw5v6g1z3ed 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 formrt:kr r4sfa;6. o6 jkied between lithium and nitrogen?

  Which of the following is the correct formula for strontium sulfir,ok h, qzn4-yde?

  Metal M is in group 2 of the periodic table. Which is the correct formul(:1 t)p/ ih z( 4vqjj qxkm5.dst(hjsfa?

  Metal M is in group 2 of qeg1gwf0x zmzv; w 20 2zp+4etps ck/+the periodic table. Which is the correct formula?

  Atom X is an isotope of an alkali metal. Which of the following is a possibvo0tyehg3 xk .*a)0 olle symbolx*.h3 v) olgyk0to0ea for atom X?'

An atomic nucleus of element X is surrounded by electron shells,py4* gv*ca4e ar;-fcp as shown below: * 4-pgc;ypc4ev far*a

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 ne *eu;w1 t gfoip57)ied mg-zk)utral atom is shown below:

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

  Which compound contains two different elements wit vv r1ewm;ct. w2qyp9ycl02* g m9tef1h identical oxidation states?

  Which of the following statements regarding the periodic table are corso24 vi+d :tk(i*g ar eqd xmxc.ea*;)rect?
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 cont:6be hwo o24vouxk9bs *d(d .qains data for the elements nitrogen, fluorine, sulfur and chlorine in no particod9b*:hs6qk . u w(4x2v edoobular 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 followingd9;mgat yandb 7)95gm 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 rega-wqy ,/joqa; crding the melting points of elements are correct? cwqq,yjo/a -;
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 sulfuiai - b a9 d5g7v2ua-ty.g*xahr are found in the second, fourteenth and sixteenth columns a*iha9 xvdba.-a2 yigg7 -5utof 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 chlorineho+zdp5 9qk50 ep1gg t 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 (6efyj+9jr q4g$NH_3$​) 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 periodic table. 2 ;c(;0w omxnpxb8ccpnrb+ j:
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 periodz wr fy: e5h;oemsoc.;234vrwic 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 smallest to largest radl.+d eeyht/: kius?

The oxides of two period 3 elements, X and Y, react in water q pz 5u)l+h0xuaccording to the equations below.)uqzx +u0ph5l
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 0 /7m0e:hey9tdd vwtt(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 doeswpvum:s2fpf1quqo)9) 4 0y ai not change in all of the following except:

  The oxidation number q40l6; qain:/ g5cdgwa/ rzuk of X is the same in all the following compounds except:

The successive ionization epi r0f:oxs5u 6nergies 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 radius for these isoelectroni6yuhg)jfb 1pg 4m 4gw4c specieg)bfh16 jg pyw44um g4s?

The bidentate ligand, phen;vx5(9.j ssaxx2rcib anthroline (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.