Which of the statements below gives a correct feature of an lp1acds/zps; 1 q1xdx,w32z1 b6fb a ligand?

  Which of the following* .0je asyqz8d can behave as a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic table is show i4/b jhw+uia7n 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 meto:,;cnwa8 sm zw qo4ct..-ij vals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the rig .o1hej,.t7az 5z. avo+xzk,sqcvh 4sht of vanadium in the periodic table, as shown below: 7et 5.1 +vxohjsk4.cashz voqaz,. z,

Which of the following statements is true?

  Which of the following salts would form coloured solutions when dissolved in w:/ni9cu 5px3lzea3t later? 3u3zex al:59ilcpn/t
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of first ionization enjx8m3 vv 3(nttergy?

  Which of the following is NOT a potentia .x2j)s(: dzv)urckn cwc;4lkl 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 dis95tpnz y 9ngky7z:,mhsolved __________.

  Which element would have the least attraction for a shared pcqfq1g19u9o3 idp*fq;b gx s3 air of electrons in a cov*u9;foq1g33qb9 pfi ds1gxcqalent bond?

  Which of the following is NOT truveudi9a5 35 rd;51 blv nrxe/ne of metals?

Iron is a magnetic element in thetp0,lggqzgz vfl6* 0v*-i 2 hz 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 solution th1hb9y4m wvfz.q jt ia9 i/,7hdat is:

  Metalloid elements play important roles in els*mub67p vj 3ti .;vyzqd7n :(is0 pdcectronic components, such as solar cells and co;tsp m0y vc7. nsqdi*zbv3u76:d j (ipmputer chips. Which of the following is the correct definition of a metalloid?

1.The valence electrons.eu.vm99 6qgbzdl m- n in I2IX​ are farther from their nuclei than the valence 6u vze9.ln 9m.mdqg-belectrons 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 tgp1co 5 1flql1he highest first ionization energy?

  Which one of the following s-/z,tf de7z7abm2mt v tatements about 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 group. The two ma;0jq rp9l ;g.prox mp/in factors causing this trendg;r/p9mqxl0o;jp . rp are:

  The electron affinity e8t-2uk p6sof 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, sfi-/ryk8 .cq tome features of the outer electi f/y.q trc8-kron shell remain constant.

Which of the following is correct?

Scandium is a transition metal that caokllq5( 5nx vw)m lg1l/dd:)5gw,4 hc8jmq bon 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 corre l7muh;s g9wn-ct correct value of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different68zm apze8 2 ekzizs:y, e.1hr arrangement of electrons, and these electron configurations can also be represented using orbital diagrams. Determine the ident8asz,8zkh.:ze 6 erzpyi me21ity 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 tqsqncxh 3b 0 p ,or32be2f(xku4 ;1mqthe compound formed between lithium and nitrogen?

  Which of the following is the correct n)ik8iz8d, s xhe85toformula for strontium sulfide?

  Metal M is in group 2 hwgv;h /f3w 8oof the periodic table. Which is the correct formula?

  Metal M is in group 2 of the periodic table. Which is the co)m / gaf6knir+r*5hsm4:m z+4r zvpgb rrect formula?

  Atom X is an isotope ofnr856be5r3ffli b10ccgs p/.8zlkew an alkali metal. Which of the following is a possible symbol for atom gb k6c 5ln8el.1icsz0 /fewrr53pfb8 X?'

An atomic nucleus of elemen z6q5obxc *t 0 bmj7omtpcb8)/t X is surrounded by electron shells, as shown below: o 6/tjbc8zbo*tmqm0 7xc5b)p

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 neutrpo::z oe6lgu)al 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 oxidation states?lgoa kt8j+e2 -j:ard4

  Which of the following statements regazl a8:t9d3ndhrding 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, sulfur gc6w p18lly- er/ 7 fjs-8*ale crk/tcand chlorine in no pafj / *gt a7lll8r kcce1-ecr ysw/-6p8rticular 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 statements are true regarding the transition metals?m :h-.vdkra/ q
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 poip ,x5 ssb ow2byk85p(jnts of elements are cor2p8wbb( sx 5pys,k5oj rect?
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 magne ;h-(*amnh (v,zc vjoqsium, silicon and sulfur are found in the second, fourteenth and sixteenth columns of the periodic table. (;z hjvv( n*aqc ,m-oh
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 chlorine to progye xu uf5u,bp.g;/b :duce 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 ammoniuoo9:wpji89a5u n: 1.pnw 8c:z ()ugma kaqoea ($NH_3$​) 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 elemenx u;rzid497 ;rpz:hhn6kc l, bt 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 thj h vf w9+g.q/vzou .1xpu9w- h1pxo+de 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 correcee7dp7ah p f(6t order from smallest to largest radius?

The oxides of two period 3 elements, - 4fsd/6z0r zi9 6m;mvniufzm X and Y, react in water according to the equations below.n-mufsiz6d ;i9z/f vz0m 46mr
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 esn4-s x(vy.s *.rlukd* 9qafe 8ye9l;9ra gy 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 Cro *yti-ns eu3q9p2b8 p does not change in all of the following except:

  The oxidation number of X is the same in all the following5 a92cxpiurwo o/pptu 4pz ))3z:; wha compounds except:

The successive ionization energiebdh0k bb3/d;ys 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 radoue*a)/iwc 0vius for these isoelectronic species? /aw*) ocuev0i

The bidentate ligand, phenanthros*ux3 2dm. bseline (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.