Which of the statements below giv l8lclgt7;q1wj 3mq,ff) ;ofbes a correct feature of a ligand?

  Which of the following can behav 6lf4 x*,ty e5nvj/ b3dwetv:te as a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic tarb -nu6:cni)able 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 transition metals?as1)v dvokz8 5
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of vanadium in the periodic table, as shown below0h wa8 p+sefd0:0f0+psa8 we dh

Which of the following statements is true?

  Which of the following salts wouldw,rwfz 2kgf2l2y1dy 6 ,ojd. i form coloured solutions when dissolved in water?,dd oi6klffw.1,jz2wgyry22
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of first wm,e vz,r yxgcu k j0 wxg*t4tmk6;e63 sn4-o(ionization energy?

  Which of the following is Nl4rdn,min;/g:m pq g1OT 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 :b+0x.njt ;vx (kzc upacidic due to dissolved __________.

  Which element would have the least attraow ,j6p hmx) ok;pl 7s;x4fx2hncw+3xi+qd(f ction for a shared pair of electrons in a covalexhox(f,c7s4n)++ pfq;ok;hi6w x2plxmwd3jnt bond?

  Which of the following is NOT true of mez+73n*s t ani p25elketals?

Iron is a magnetic element in the first rowkruy (pux gdqu* urot5j2u81+.et -5b 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 i u:p2gsdiw2 a63d ck ttc(nc+7n water would produce a solution that is:

  Metalloid elements play important roles in electronic compfzcrvqjs8bd;7.8 8 wponents, such as solar cells and computer chips. Which of the following is the correct definition of a metalvbpc;r j8.s8dfz7qw 8loid?

1.The valence electrons in I2IX​ are farther from their nuclei than the va wbg bf,o2-.rpe i)y1dlence el,). fiwoy rpe1bg 2-bdectrons 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 firstd n5c(v) ;e *pjq) dny/tpym,0ohi,mc ionization energy?

  Which one of the followinbyjb-9 db:u0fc3.,+g hs za i9 qko6tc e)ps0fg 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 down the group. The two main facmj ry*memo ,st 228.qmy:x0hwtors causing this trend aes 0ym* 2jmmyx 8,ow. qtm2hr:re:

  The electron affinityg wyjo1y )tdic9d/fv8c; z:tl2m i :3l 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, somfjmw*q3kz,sxc oz ;ac,1* ec9w1,i vu e features of the o;xm9, 1wfau 3zz w,c,iv*1sekcojc* quter electron shell remain constant.

Which of the following is correct?

Scandium is a transition ( r,x;el;go egmetal 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 coglpw r,tpp3* :rrect value of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arr*w7d-7) dmurbr ou9m rangement of electrons, and these electron configurations can also be represented using orbital diagrams. Determine the identity oford*b7dm 7rumu w -9)r 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 comh6o+0n,wo76 qg6om r k 0npkbopound formed between lithium and nitrogen?

  Which of the following is the corregfsq q;.q+ e8oct formula for strontium sulfide?

  Metal M is in group 2ypcad 7e;37gytfq v2y9(2 lbn of the periodic table. Which is the correct formula?

  Metal M is in group 2 of the periodic table. Which isdti yj.x4tg of6f l (m/a(r* )jzv/m/p the correct formula?

  Atom X is an isotope of an alkali metal. Which of the following imfm gnd 11t9r6s a possible symbol for a1tm9fg6md1r ntom X?'

An atomic nucleus of eleme3n6 -kfq-kd w)*v12ejdya npint X is surrounded by electron shells, as shown below: kv-e*2jwdny 1 i-3)npa f6qdk

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 ek /ee;q,(msn neutral atom is shown below:

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

  Which compound contains two different enxtjw)r e1p e f8go-/+.2d lszlements with identical oxidation states?

  Which of the following statements regarding the periodic table armscwb/32f ; r)dzfd z1e 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 nitrogkhg fd1pq1hg8*p6k: znd -2agen, fluorine, sulfur and chlorine in no particul d 12q6k*pdfpghg1k 8g:z a-nhar 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 statements2b0ti9ux iqjuwjr837 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 regardi e.2m *9gi3+*yf.ixjh qjkuwxe,4d v tng the melting points of elements are cod+.9*evy. wiegmj k q42*xi h,j3tufxrrect?
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, silicoy,bulhnn 70m9 n and sulfur are found in the second, fourteenth and sixteenth columns of the periodic t7mh0n y,b9nl uable.
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 tkm ac*tx n f9:xtq0t(9hat 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 ammonia ( i3okh,uogl :vl;8u 9c$NH_3$​) 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 perceg oi 659ml.giodic 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 tdgxm 0; sl3b0zq0w a3crue?

  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 smallesx b37saj9 l(rot to largest radius?

The oxides of two period 3 elb. d.8j b,+qtagzd6z*n oco8rements, X and Y, react in water according to the equations8z t. 8.bdcaq *n +brozj6o,dg 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 iohz;l st f0:s8 4xegfx7nization 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 th : 5j8rx4frpa8 qw32nmnx: zwhe following except:

  The oxidation number of X is the samx0yp3 el c)ycord*v/7e in all the following compounds except:

The successive ionization energies fo6 t+798cncgbai;btwrm/ d *xk r 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 ord9wllz ogms a +*6y2fz7er of increasing radius for these isoelectronic speci 9gfml6z2zl*a+ oys7w es?

The bidentate ligand, phenant h7kj irdw0+juhm )l44hroline (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.