Which of the statements below gives a correfhqm297xn 3t ect feature of a ligand?

  Which of the following ct on(/d( wkd +e+zrg*kan behave as a ligand?
I. $BH_3$
II. $NH_3$
III. $CH_4$

  An outline of the periodic table is b ,h8be h6ow+b2xhy0zp 0+ rjzshown 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 transitryw0yl)z * nv3( 3aurkion metals?
I. Catalytic behaviour
II. Coloured compounds
III. Variable oxidation states

  Chromium appears to the-ltys14t0ui50ws o :)nq b gmk right of vanadium in the periodic table, as shown below: s o1:lmik 4n-)t0y50 qgtubsw

Which of the following statements is true?

  Which of the following salts would form cole)2 g8uhvxlg*ydr z(l z2)x c7oured solutions when dissolved in wate7ugr)zcx(l2hge y*zxl 8d)2 vr?
I. $CuCl_2$
II. $ScCl_2$
III. $ZnCl_2$

  Which chemical equation represents the definition of first ionization energa uh7;qt 6wbl:y?

  Which of the following is NOT a potential component of acik0o2so1g p0 fzx1ip,hd 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 dissolved h + )km9y6 d *jiokpmjb12-lpf__________.

  Which element would have the least attractif y2 b,zp5trc-2ghu s7on for a shared pair of electrons in a covhu2t72g5 zyc-f sbpr ,alent bond?

  Which of the following is N crywor (qe+t0i/m,1cOT true of metals?

Iron is a magnetic elemenyedx5l 39u6hx lit xc dk(1e7-t in 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 disso1nh + srwdmu5;lved in water would produce a solution that is:

  Metalloid elements play important roles l1u;ps +br,b a9px e0pin electronic components, such as solar cells and computer chips. Whi1,pr9up0sa pelb;b+x ch of the following is the correct definition of a metalloid?

1.The valence electrons in I2IX​ are farth) j0tn2cu5ilr er from their nuclei than the valence elli 50tjurc2 n)ectrons 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 - hmcv k-kg*:t.l4hle;* hydt c3quo5has the highest first ionization energy?

  Which one of the following statements abou1ehloqlsu3: mxf9)y)3j 5g vit 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 factors caus(xtevns)wr6;e 6pu2 aing this tree6 ;u)x t(v2an6 rswpend are:

  The electron affinity of carbon ib qvbqr9,8r1a s $-122\,kJ\,mol^{−1}$, 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 per*svu(f yti(my//e1 pliodic table, some features oftef1vp /uys(m* (/yi l the outer electron shell remain constant.

Which of the following is correct?

Scandium is a transition metal that can form both 2+ and 3+ complexes. da 8szuu e4cpsc,)tt;s4ts+8
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 correctt)5c oi 80ucvk correct value of $x$ and the shape of the $Cu^{2+}$ complex, $[CuCl_4]^{x-}$?

Each element contains a different arrangement of electrp+r2 /ur 1qako;gel6z b4twt9ons, and these electron configurations c;go /ezrw4k+1tl26utq9brpaan also be 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 form0kbjrby 1+.hjed between lithium and nitrogen?

  Which of the followin pwp6dr:t ;m2dg is the correct formula for strontium sulfide?

  Metal M is in group 2 of thsqeu j;g*98bse periodic table. Which is the correct formula?

  Metal M is in group 2 of the .luu(2a)allp periodic table. Which is the correct formula?

  Atom X is an isotope of an alkali metal. Which of the followinb1j*.skw3 :ee .,,mwmk;f p:lultvnog is a possible symbol for atom X?' :*euvwkn,.kms,eomb 3l 1pjt: lw.;f

An atomic nucleus of element X is surrounded by electron shells, as sffwq vm .b;xtlhx9 ;x+l:g26uhown below:9lbvx.u +fg; fq 2x;6h tm:wlx

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 electrono0j e nqe394mw configuration of a neutral 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?6hyj8v lin2tuss88m6

  Which of the following statements regarding the periodic table ar929tuofyj6o p e 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, fluorinegosvfg+,+y ur d7,ohxqq79:w , sulfur and chlorine in no u7w,h7o++gfqrs, g:vx 9o qydparticular 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 truesw+9*tegi, l b 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 regar 1/gsmr; :eer0yoe--jc ovag 9ding the melting points of elements are corr: m1orjg - 0rog;y va9ecee/s-ect?
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 andll;l4n r+: ax1j doilqk3-4qu sulfur are found in the second, fourteenth and sixtee:1+ 4-kdxli4 alju3 lql;o qrnnth 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;dtg donwd3+3 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 ammoniizlg:s4sr cpr (9j10b/l co)da ($NH_3$​) 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 table.-mp f6 ay8nq.m m20uvh
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 qgt ik t42y5,,,keq dtthe 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 correct order from smallest to lar2gmb)v/rnm 5st vqw 3)gest radius?

The oxides of two period 3 elements, X and Y, react in water accordingcgha 3j4dfmvvh8n- 5e 2zq0v1 to the equations b1q-ghe 3fc2 4jmvn8vh0 d5vazelow.
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(vg-+qcyqhgnd 3evoa n*,.,h* 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 chang)ibgpc: 6nmd1l bo6(w7hg *m3d3xfpie in all of the following except:

  The oxidation number of X is the same in all the fw7c 3ohxt;h+v 0c*vut8x,l7i4s or eoollowing compounds except:

The successive ionizat(9 y8m pv g4iudmr k0op8-8crhion 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 increasing radiugnx sb1aykaim/z4 c /*8wqc(/ s for these isoelectronic speciesnc/4a8 zmq * (s/ix gkcbya1/w?

The bidentate ligand, phenant n:bh;,nnj3 *rrz fmx/hroline (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.