Which of the statements below gives a correct feature of + 6c dviz1:ncna ligand?

  Which of the following can ).8felqd 9ekjo n/ rj/ul,12wirq5wobehave as a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodmo*s sh fd7x+5:sowe8 ic table 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 metal ovaj ea.1zd)6htw.x 4s?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the rig,.s)j rx4 hxwwht of vanadium in the periodic table, as shown below:jxhww s,.r4x)

Which of the following statements is true?

  Which of the following salts would form coloured solutions when mlbd0 p58j) na(rj 6ppdissolved in water?r6a 5)jdljb80(pn ppm
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represc37ug qco1.* ai. ro5indla5vi1ou,q ents the definition of first ionization energy?

  Which of the following is NOT a potential componeobf8lw1y zap m ;(q)srz p92w,nt 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 dissolvezoo94 nu+qvf103gxih) o g/ wqd __________.

  Which element would have the least attraction for a shared pair of ele5 kr epou/uer9+ufn.i(*v .tlctrons in a covalent uoek el/p * r+5tuuf(.rn vi.9bond?

  Which of the following is NOT true xwc- h8y:kxi5 of metals?

Iron is a magnetic element in the f) f/ iln4sgzt3irst 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 w6ddjlt;i z/a6sp-,oz pn* 4o aater would produce a solution that is:

  Metalloid elements play important roles in electronicq ejsq/w/2.h s components, such as solar cells and computer chips. Which of theswqq j/2 h/es. following is the correct definition of a metalloid?

1.The valence electrons in I2IX​ are farther f0,g hw5js2 vlp04l5feimtw0n (e(si rk1 j :iprom their nuclei than the valence electrons inn p(5j2irt,w 01i(klpgwilem j0fh ss :405ve $Cl_2$. 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 ionh1l;s4c k)qau7t: kji o;m5c zization energy?

  Which one of the following statements about acids i s7 o5wqsrs7)ph2zlj, s/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 factors causing thisnbw 2mcc--pj b9;uyv6 trendp9m -bv2n 6bycwjc;u- are:

  The electron affinity of c(qgeaa x xat83,ag4l)nza/7v arbon 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 r0os );/cqol;jgdb) f0svxl 5b/k.f dx ow X or column Y of the periodic table, some features of xdckxs/;s 0bg/)l.q)bff05;o dv loj the outer electron shell remain constant.

Which of the following is correct?

Scandium is a transitionft/bq/ hk6f d. metal 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 correct valxetj.3 /+ gic0a dfleg3-l y/eue of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrons, and thes d46k9y xic4k/ir get+24 muam:pp0 kve electron configurations can also b:dt k9ym4ucg pp4a0+6/4ier im x2 kkve represented using orbital diagrams. 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 between lie iy*t kv s(bw-,hgjkg b,:0/bthium and nitrogen?

  Which of the following isgx dt9p09dfqs 4 s0jq. the correct formula for strontium sulfide?

  Metal M is in group 2 of the periodic table. Which is th6 abf: j.epwxbx 69 jgw1,hsl,e correct formula?

  Metal M is in group 2 of the periodic table. Which is the correct for(c0 * 5l zincno.gopc2mula?

  Atom X is an isotope of an alk vhbrrf2*p: i-ali metal. Which of the following is a possible symb2f*:bv h-rpi rol for atom X?'

An atomic nucleus of element X is surrounded by electron shells, as shown belp;mmm x y ;9r:ks4nlz0nl ;h e zaho/p0,+o8zzow: 0h;m/,m:nn4prolz ;0zyakx+s9o p l ehm8;zz

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 yw5s. 3lz0 bicaolq bjdmdi+e5);(g.dcs0h :om is shown below:

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

  Which compound contains two different elements w/g1nfs; jp,e*m io j0qith identical oxidation states?

  Which of the following statements regarding the periodicq2;cja+ khfx+ 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 and 2euzsyqwigyou3v*1+ v )co 2 ;chlorine in no +oswg2)2uqivuyyo z v; c1*3eparticular 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 transitbf 1 z9glm2 .g8yz;syyion 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 staga l3et) :gob(tements regarding the melting points of elements are correla 3btggo)e:( ct?
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 m khe+nixb+*0f8m 9uq gagnesium, silicon and sulfur are found in the second, fourteenth and sixteen9xk*nim feu bg h0q+8+th 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 reacts with chlorine to) e)p3xsn09nc4dcud -dwe0b r 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 ()w(s d*ufnh 8e$NH_3$​) 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 tabs-rhwgkr455 vqczx .9c z ,8mwle.
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,)m (oferjfvg4 o):dr 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 from smallest to largesbnrqha5gw0x5)q m y +*t radius?

The oxides of two period 3 elements, X and Y, react in water accor 5.i-6 r4lz9ecx+xneky 9mairding to the equations belomcxrnz5eerak l99 .y-4i+i6xw.
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 (A(g)→ 6: 8s:goiymk0iq( peq$A^{+}$(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 follym3 tj38h pn0oowing except:

  The oxidation number of X is the same in all the following compounds except:8dc( cq8rjg* bh c.ey-

The successive ionizqq y8,.3(4d uli xgxhlation 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 of increaz2jb.o/j rng7sing radius for these isoelectronic species?7n o2rz.bgj /j

The bidentate ligand, phenanthroline (phen) has the sb6v7mhpx(: k3 f )z pytzcr7v,tructure 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.