Which of the statements below girxdj1 +k dsyw,*f aaq:br0 7h;ves a correct feature of a ligand?

  Which of the following can behave as 7 p0foaf gn*eql-u;m 8a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic table is shown belolaei5t 1c 0y7ay2;t3 i(brxbj*af wu1w:

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 mzgw p okrcwohwt( 6 gu2(d1qio6yu-u6 + 3f27jetals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of va;.x akwfye vd(xg0gi :-+xr/lnadium in the periodic table, as shown below:x/afy0- . xwl :(gidrgexvk+;

Which of the following statements is true?

  Which of the following salts would form coloureg.fvnqo;/fa7vakttik p; . ,4 d solutions when dissolved in water? .gi;avafkt np k7vt,q/4f;o.
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of fiejhc : ln)mn84bvhh /4rst ionization energy?

  Which of the following is NOT a potential compone, 7d5i1t bvp1 cry8abent 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 acig a6kbbs nm59y5( ydd6dic due to dissolved __________.

  Which element would have the least attraction for a shared pair of e wnq,7,8jo jxln x8es5lectrons in a coval8, qe7 x xswj8nj,o5nlent bond?

  Which of the following is NOT true of metal5 r; jg2uejbr1s?

Iron is a magnetic element in the first row of t-n dm zr8o9.zr -tdsj-he $d$-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 prr )h sj ha++5bkptfxjq:0ae//oduce a solution that is:

  Metalloid elements play important roles in electro ax-nhij.;l-knic components, such as solar cells and computer chips. Which of the followi;h.j-i al kxn-ng is the correct definition of a metalloid?

1.The valence electrons in I2IX​ are farther from their nuclei than the vale w5obb5d dt,r5nce ele5o 5,bb5r wtddctrons 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 energyzx:0er qdxy+0kk/)qd(e 8vfo ?

  Which one of the followbmu 3y v)2-i8oky trl:ing statements 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 dow1-1a vdfa b)ohn the group. The two main factors causing this trhabf- ) v1dao1end are:

  The electron affinity of carbptw)m +b0 x;xqon 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, s;etk5q u,jv g b)m+j ifk5)1qhome features of the outer electron shell remain )k,m fkjg1hbqjitv5; qu+5)e constant.

Which of the following is correct?

Scandium is a transition metal that can form both 2+ and 3+ complexej m4 avv,uxgmy;u:; 4as.
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 valu2ms5vxpjl+z r4:y k)ne of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, and taok(q wy rriq(67 xy+ s1rl;p4hese electron configurations can also be represented using orbital diagrams. Determine the identity ( a1rsoprw r74q qk;lx y(y6+iof 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 compoba wt0)hqqai 0gl5vp24te i)h./bqd9und formed between lithium and nitrogen?

  Which of the following is the co u z9ck y:g04*hr0d)3rhfper xmjb+ /j; (rowgrrect formula for strontium sulfide?

  Metal M is in group 2 of the periodiuvdc,cpt (+l374l/ ptn- b oalc table. Which is the correct formula?

  Metal M is in group 2 of the perioik3ti05usp.urh: aov bk1d/-dc- 6s ndic table. Which is the correct formula?

  Atom X is an isotope of an alkali meaj122e. 5qyh,tx1u ic)eh ywwtal. Which of the following is a possible symbol for atom 5xi q1hw,c.y )je2ha e tw21yuX?'

An atomic nucleus of element X is surrounded by electron she;nuv,o/ (xisjrlc y: 3 *7evfylls, as shown below:f*7xvyr:yj(lv,ue ;ocis 3/n

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 at *onm8 :6-ygfyy6voztom 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 oxio0r oelv9)8gpdation states?

  Which of the following statements regarding the p 3vswykphuq 3/x 88e d ke(ct*(p,gcl e,6m4pkeriodic 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 contai fun8z.g-f:r 5sr+:wak r:cg ons data for the elements nitrogen, fluorine, sulfur and chloffcrrs:.:a8g: u zrwgok5 -n+rine in no particular 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 statemenvt h+cfj*tv+/ 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 statements regardivg ;quj3 (r4a(ebsq.q )ujai 7vzeh;9ng the melting points of elements are co u brhg3q;9a(.()je4is uvvae z;jq7qrrect?
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 f1k hvr9lf dpc(qow.c ot 3,s/,ound in the second, fourteenth and sixteenth columns of tr,s(91/ , h wfpctod.vqk lc3ohe 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 metazxxgjee (p vh ,6 jj;20jh85pc3wzw w)l that reacts 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 ammoniu(-r :4b.bt,jtwu 2il +lzut ga)/w fga ($NH_3$​) 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 4ht 6+fcfdtc 1nf4+nxtable.
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 taz m)y8iu+e(aq ble 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 o bsfx; 9q tu1 yu*zb1b87d5ujfrom smallest to largest radius?

The oxides of two period 3 elements, X and Y, react in water according t4b)p6t t3 ,singv;zswo the equations bel;s43t i,)t vwb s6zgnpow.
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 i scd+n/gu v7vb(bm64nxl 70ft onization 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 +h ps 9 hqqj61g9ab(jlof the following except:

  The oxidation number of X is the same in n*bzr; l6l711:vxj:nee ckg 2f)lzggall the following compounds except:

The successive ionizat(b*t3bxequp n)jc. cgf t i;mt9) ,o5(pvwdt1ion energies 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 hofw h8c:j)ln+hg 84oof increasing radius for these isoelectronic specic+84)lhfjw:oog n h8 hes?

The bidentate ligand, phenanthrolin.xn3e2yd;( gihtl 84)ksdzv te (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.