Which of the statements below gives a correct featf 6atq(6hq hc/ure of a ligand?

  Which of the following can behave as a s 8l7wa ( -arnsep(0arligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic tqa ,aw2qws7c/3: d dehable 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,in 9iemult( + metals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the right of vanadium in the periodic table, :s-x a17r5 suhpwr7 w2z1mu uelnip1; as shown below: wp7xhn7ui1-sz ;1uuw 1 arr ml5p:2es

Which of the following statements is true?

  Which of the followiuq rh)nhg 41v)ng salts would form coloured solutions when dissolved in watergvqr) uh)1 4nh?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of g :wcoqp :st h-(n.(ljfirst ionization energy?

  Which of the following is NOT a o:cih jtd+ g5us1 t9n1potential 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 dissolv6,kz7j8ujlfwyi+ h7 ied __________.

  Which element would have the least attraction for a shared paa qz8*xn-p3m lbyt z/+nsx0n;tit2 +eir of electrons in a covalent *z/ +yn-;paxn tn2m elxz3qs +0ibt t8bond?

  Which of the following is NOT true 4 wbtrtkm6 j(h)/6kxz ,c sh8cof metals?

Iron is a magnetic element izi mo/tr/+q vg,dl*wxcs134l4 l 3cxpn the 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) l/1kflupfs lx7 4kz2 that is:

  Metalloid elements play important roles in electronic compvjo ;ze8tf 8 o)6vcpk5onents, such as solar cells and computer chips. Which of the following is the correct definition o)ec8 o8zvfjt ; vkp6o5f a metalloid?

1.The valence electrons in I2IX​ are fpd fp4m)c;lv ;arther from their nuclei than the valence electro; );vp mpdcfl4ns 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 fi b(ujcblqx.at1b./. st1zib8rst ionization energy?

  Which one of the following statements az5ud4 hrva 14zbout 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. Thx9 uhu c8q3olstd;)8 me two main factors causing this tru9u dm8o)lqhs x3c t8;end are:

  The electron affinity of o n)+r0med5o,h);r efpx j6o-wrl0r f 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 tabo6mk:f3 i i.dvle, some features of the outer electron shell remain constmdi6vi.k3of: ant.

Which of the following is correct?

Scandium is a transition metal that 8 +xf:lyx2:(z0ct qy0 wkc+qmo+igg6jzgb1o 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 of 0/,i(uxk.msrh;r y o y$x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons,ngm0p8q nd5cop0y: f 5 and these electron configurations can also be represented using orbital diapo0g:q 5yn5 0pdnfmc8grams. Determine the identity 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 the compound formed bu)zw) 7 cckft9pqj.2;e kst;:buaa4 tetween lithium and nitrogen?

  Which of the following is the correct formula for strontd3+fxywr)3au ium sulfide?

  Metal M is in group 2 of the periodic table. t1ca wt;,x3vu.9qk ypWhich is the correct formula?

  Metal M is in group 2 of the periodic table. Which is the 8whi6wt tr e/z8y k*e2correct formula?

  Atom X is an isotopesn 4 mn pq.7p3d6hqj+ eoyonl)2j,kv4 of an alkali metal. Which of the following is a possible symbol for atom X?j3 74,lpp ovjd y)nm6qe.2hq4+nsonk'

An atomic nucleus of element X is surrounded by elugk2 , k*l(2+lexwflq ectron shells, as shown below: u2*2w ll,xel+qfgkk(

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 co8-l) *j/xgbk2st egd7 snbmq:nfiguration of a neutral atom is shown below:

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

  Which compound contac9w+a8(u rpab k0mn) wzo 00rfins two different elements with identical oxidation states?

  Which of the following statements regarding the period5ezqo,l9nhgck5n, tfp9xup s:g7u 1 1ic 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, sulfurbflag 3b44mf * and chlorine in no particular order:abb4ff l3mg*4
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 zgu3r76zvp-j 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 regardin6l tb8ojach6; g the melting points of elements are corrt86a lo;hb 6jcect?
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 dj+/3w4)/yhwkoy hfple85t g and sulfur are found in the second, fourteenth and sixteenth columns of the periodic table.wg4/t8d wo hh+l kyfpy3/ej)5
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 wuz p/m6wd+u7yith 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 ammon/:k fy8 hf,co b7z-oiedjm r*+ia ($NH_3$​) 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 gro; 5f t all5g/k8je lp.8*jnekh6em .itup 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 t5d-*+qrz obic-hz:wm ++ xujz 5t 4yxqrue?

  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 radic(ud2xa/l 1*mvxw ah(us?

The oxides of two period 3 elements, X and Y, rearqo05;-: o:pcx 9vrbx.jjjan) thio +ct in water according to the equations bitp jhq:c b+.a9r:o -jr xx)no 5;0vojelow.
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 463wujtd4 f: , bii e)z,zvkuv(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 u47fg*x2 5dcbcsghm *change in all of the following except:

  The oxidation number of X is the same i f/n96adpdpazgn; :;gn all the following compounds except:

The successive ionization energies fo;1 posy /ce)dtr 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 oge y s6dio z3,wsi:0cc, t.da(f increasing radius for these isoelectronic species:z6td , i0s3 ,oie(c c.sgaywd?

The bidentate ligand, phenanthroline (phen) has the structure bsieu3torv 55/elow.



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.