Which of the statemei:l.x,ps be: a x*v8ycrc 5gm6nts below gives a correct feature of a ligand?

  Which of the following can behave as a ligan -q:dkr6 xkpsxfarf),*j 67jrd?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic tablef0p/)gm(j 0bc q ru,zn 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 tram pgcjm14ly7vqwh / 14e 35uotnsition metals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of vanadium in the periodic tab(pxac9 /k fgh4e7(to mle, as shown below:xk /p(c7(eg a o9ft4hm

Which of the following statements is true?

  Which of the following salts would form coloym4qkv-i ;h nvn9oqge;80i1hyv 8l0 f ured solutions when dissolved in watvvq me4 ;gyf1 lnn -00o8vhqy8 ;k9ihier?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the /59rl naysm7e definition of first ionization energy?

  Which of the following is NOT a potential co4( fwpou98 jdflam0r ,mponent 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 ____ 5.o-ae;2- bxxcoeaep.x7wyn______.

  Which element would have the least attraction for a shared 1(pu ss,oo7lp rcv; +k)0q3tvvpag )spair of electrons in a covalentpuv1 s)ol3av;7,pk+ c0s(t p roqg)v s bond?

  Which of the following is NOT 130 t ie1er+,w mlbfn( rk2ac.,tzwpctrue of metals?

Iron is a magnetic element in the firs.6 jx i)-cdkdht 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 c8z6io mr1;ug dissolved in water would produce a solution that is:

  Metalloid elements playd9+ j1c jicgl/ important roles in electronic components, such as solar cells ajgj1 c+ic/ d9lnd computer chips. Which of the following is the correct definition of a metalloid?

1.The valence electrons in I2IX​ are fart wq y0.2dpho-q 7muuesdo83u3her from their nuclei than the valence electronsho37.edqmd u0 832y-u wspoqu 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 ionxbz+:x.2x- gs suqv 3 9s,jlmbization energy?

  Which one of the following statements about acids is/ar-cp59/x i1y t94d dz(aphjyzze 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 two c af,e(3bq6iymain factors causing this trenei6a(fq , b3ycd are:

  The electron affinity xd1t)u ykjd,ycpe4t, in+l9 ,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 8e8t cnk okq ;)g55ryrrow X or column Y of the periodic table, some features of the outer electron shell t8r ky5;c5)r 8qekng oremain constant.

Which of the following is correct?

Scandium is a transition metal that can form both 2+ and 3+ compq ch8v)u48r mckf( a;klexes.
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 correctvy ,t::/wksf rmuo(5p correct value of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, and these electvgvq/2;nzc+-sebkp 5 ron configurations can also be represented using orbital diagrams. Determine the identity of each eg; vsze-nc/k pb5q2+v lement 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 formej). kfv it:nlb:- d;ym/g*xc td between lithium and nitrogen?

  Which of the following is the correct formula f85- :spsg ew c (-ijusiefxn:a7p.oo*or strontium sulfide?

  Metal M is in group 2 ot8 vpw7uuiul;p /ks:fv3 7y q7f the periodic table. Which is the correct formula?

  Metal M is in group 2 of the periodic table. Which is the correct formul/dvvk.9d n 7krp ;bh .rv:u,jna?

  Atom X is an isotope of8lf q*r.n n1kh an alkali metal. Which of the following is a possible symb 1rqnklh nf.*8ol for atom X?'

An atomic nucleus of element X is surrounded by electron shellukw /s3;: fdfzs, as shown below: f3:u sw;zdk/f

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 confifth0()kf93glorr. 5(fyt gg zc9 hlb4guration 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:n 2fa1w 60fagxc2p4 syfpm( b different elements with identical oxidation states?

  Which of the following state 5 tayy-u/j0mg(, 4l8wtwnn/9 x y1xmuzqqmp1ments 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, fluorine)dy(1 )ta:rr cv pp;yp, sulfur and chlorine in no particular order:cd: )apprty(;p) 1vry
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 are true regarding the transi6cqu597gsbyn 0omopc,)wc9 u tion 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 meltih0** ztwfi )dpng points of elements are correct*iwft0z dhp*)?
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 su+ mu77mzd8xbn)2v tjulfur are found in the second, fourteenth and sixteen)b2jmumz+ v78 7dtu xnth 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 reackmo4 m()pj0r(e vb) wfts 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 ammonirap*xnc (74coa ($NH_3$​) 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,rta9di: bztp87t 9 hl 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 table is trunbq9h 1(tjbo, e?

  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 radius?; vula8p1m op*ocb 8(s

The oxides of two period 3 el1awsc 8ylls/guu.us24 eug4+uqi9 a3ements, X and Y, react in water according to the equations bel.l843 s9u2guau+i 1slqc e agsuwy4u/ow.
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 ncbl*y ;z9 oi/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 does not change in all of the folloh 4nupelqg-17e pttl7-) n:zfwing except:

  The oxidation number of X is the same in all the followindnhni:5n3 7 th-w sk6jg compounds except:

The successive ionization energies for element X is shown in the5avkz7 otdu2t j c+ygqj0u15by)xlc6 z3y9 ,k 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 increasieiqf*i v.2l2n ng radius for these isoelectronic species?2 ii.nfqe*vl2

The bidentate ligand, phenanthroline (phen) has the structure belowfaodh 4*:sp+ f.



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.