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The s-block elements are characterised b...

The s-block elements are characterised by their larger atomic sizes, lower ionisation enthalpies, invariable +1 oxidation state and solubilities of their oxosalts. In the light of these features describe the nature of their oxides, halides and oxosalts.

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Due to low ionisation energy and large atomic size, alkali metals form cation readily and so their compounds are ionic. Oxides Due to `+1` oxidation state, alkali metals form normal oxides of general formula `M_(2)O`. Only Li forms normal oxide `Li_(2)O` when heated in air. Other form peroxide and superoxide. Oxides of alkali metals are strongly basic and are soluble in water. The basix character of oxide increases gradually from `Li_(2)O` and `Cs_(2)O` due to increased ionic character. Halides Except lithium halides all other alkali metal halides are ionic. Due to high polarising power of `Li^(+)`, Lithium halide is covalent in nature. Due to +1 oxidation states alkali metal halides halides have general formula `MX`. Low ionisation enthalpy allows formation of ionic halides. Oxo salts All alkali metals form solid carbonates of general formula `M_(2)CO_(3)`. Carbonates are stable except `Li_(2)CO_(3)` due to high polarising capacity of `Li^(+)` which is unstable and decomposes. All the alkali metals (except Li) form solid bicarbonates `MHCO_(3)`. All alkali metals form nitrates having formula `MNO_(3)`. They are colourless, water soluble, electrovalent compounds.
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The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . In 3d series, the maximum oxidation state is shown by

The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . Identify the correct statement

Knowledge Check

  • Metallic elements are described by their standard electrode potential , fusion enthalpy , atomic size , etc . The alkali metals are characterised by which of the following properties ?

    A
    High boiling point
    B
    High negative standard electrode potential
    C
    High density
    D
    Large atomic size

  • Which element(s) of d-block have full d^(10) configuration in their ground state as well as in their common oxidation states?

    A
    `Zn`
    B
    `Cd`
    C
    `Hg`
    D
    `Ag`

  • Transition metals combine with halogens at high temperature to form compounds called halides. On account of high activation energy , the reactions require high temperature to start, but once the the reaction is started , the heat of reaction is sufficient to maintain the continuity . Metals in higher oxidation state form flourides as it is the most electronegative element . Flourides are ionic in nature . The chlorides , bromides and iodides have ionic as well as covalent character . Halides of metals is higher oxidation states are relatively unstable and hydrolysed very easily . DeltaH_(f) is negative for

    A
    Flourides
    B
    Bromides
    C
    Iodides
    D
    All of these

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    The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . In which of the following pairs , the first species is more stable than second one

    The heavier elements of group 13, 14 and 15 besides their group oxidation state exhibit another oxidation state which is two units lower than the group oxidation state. The stability of lower oxidation state increases down the group. The display of lower oxidation state is due to inert pair effect. QWhich of the halide does not exist?

    The IUPAC definition of a transition element is that it is an element that has an incomplete d-subshell in either the neutral atom or its ion. Thus the group 12 elements are member of the d-block but are not transition elements. Chemically solft members of the d-block occurs as sulphide minerals and are partially oxidised to obtain the metal, the more electropositive 'hard' metals occurs as oxides and are extracted by reduction. Opposite to p-block elements, the higher oxidation states are favoured by the heavier elements of d-block Metals on the right of the d-block tend to exist in low oxidation states and form complexes with the ligands. Square-planar complexes are common for the platinum metals and gold in oxidation states that yield d^8 electronic configuration, which include RH(I),Ir(I),Pd(II),Pt(II) and Au(III). The most distinctive features/properties of transition metal complex is their wide range of colours.The crystal field theory attributes the colour of the coordination compounds to d-d transition of the electron.It is important to note that (a) in absence of ligand, crystal field spilling does not occur and hence the substances is colourless, (b) the type of ligand also influences the colour of the complexes. Which of the following has dsp^2 hybridisation and is diamagnetic in nature ? (i) Na_4[Cr(CO)_4] , (ii) [Ni(DMGH)_2] , (iii) [PtHBr(PEt_3)_2] (iv) [As(SCN)_4]^(3-) , (v) [AuBr_4]^(-)

    The IUPAC definition of a transition element is that it is an element that has an incomplete d-subshell in either the neutral atom or its ion. Thus the group 12 elements are member of the d-block but are not transition elements. Chemically solft members of the d-block occurs as sulphide minerals and are partially oxidised to obtain the metal, the more electropositive 'hard' metals occurs as oxides and are extracted by reduction. Opposite to p-block elements, the higher oxidation states are favoured by the heavier elements of d-block Metals on the right of the d-block tend to exist in low oxidation states and form complexes with the ligands. Square-planar complexes are common for the platinum metals and gold in oxidation states that yield d^8 electronic configuration, which include RH(I),Ir(I),Pd(II),Pt(II) and Au(III). The most distinctive features/properties of transition metal complex is their wide range of colours.The crystal field theory attributes the colour of the coordination compounds to d-d transition of the electron.It is important to note that (a) in absence of ligand, crystal field spilling does not occur and hence the substances is colourless, (b) the type of ligand also influences the colour of the complexes. Which of the following statements is incorrect ?

    The IUPAC definition of a transition element is that it is an element that has an incomplete d-subshell in either the neutral atom or its ion. Thus the group 12 elements are member of the d-block but are not transition elements. Chemically solft members of the d-block occurs as sulphide minerals and are partially oxidised to obtain the metal, the more electropositive 'hard' metals occurs as oxides and are extracted by reduction. Opposite to p-block elements, the higher oxidation states are favoured by the heavier elements of d-block Metals on the right of the d-block tend to exist in low oxidation states and form complexes with the ligands. Square-planar complexes are common for the platinum metals and gold in oxidation states that yield d^8 electronic configuration, which include RH(I),Ir(I),Pd(II),Pt(II) and Au(III). The most distinctive features/properties of transition metal complex is their wide range of colours.The crystal field theory attributes the colour of the coordination compounds to d-d transition of the electron.It is important to note that (a) in absence of ligand, crystal field spilling does not occur and hence the substances is colourless, (b) the type of ligand also influences the colour of the complexes. Select the correct statement.

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