Grade 9-12 exam based short note and worksheet
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14 ΒΆΒΆΒΆ α₯α£α«α½α ααα΄α α α΅αα ααα αα΅αα
ΒΆΒΆΒΆ
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15 πBiology grade 9 all unit summarized short note
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17 α αα΅ α¨ααΉα«α α°ααͺ α¬αα΅α΅αͺ αα αα«αααΈα α¨ααα‘ αααααα½
π₯Increasings or Decreasing Orderπ₯
π΄ 01. Melting point=
Li > Na > K > Rb > Cs
π΄ 02. Colour of the flame=
Li-Red, Na-Golden, K-Violet, Rb-Red, Cs-Blue, Ca-Brick red, Sr-Blood red, Ba-Apple green
π΄ 03. Stability of hydrides =
LiH > NaH > KH > RbH> CsH
π΄ 04. Basic nature of hydroxides=
LIOH < NaOH < KOH < RbOH < CsOH
π΄ 05. Hydration energy=
Li> Na > K> Rb > Cs
π΄ 06. Reducing character=
Li > Cs > Rb > K > Na
π΄ 07. Stability of +3 oxidation state=
B> Al > Ga > In > T1
π΄ 08. Stability of +1 oxidation state= Ga < In < TI
π΄ 09. Basic nature of the oxides and hydroxides=
B< Al< Ga < In < TI
π΄ 10. Relative strength of Lewis acid= BF3 < BCl3 < BBr3 < BI3
π΄ 11. Ionisation energy=
B> Al <Ga > In <TI
π΄ 12. Reactivity=
C<Si< Ge < Sn <Pb
π΄ 13. Metallic character=
C< Si < Ge < Sn < Pb
π΄ 14. Acidic character of the oxides=
Co2 > SiO2 > Ge02 > SnO2 > PbO2
π΄ 15. Reducing nature of hydrides=
CH4 < SiH4Β < GeH4Β < SnH4 < PbH4
π΄ 16. Thermal stability of tetrahalides=
CCl4> SiCl4> GeCl4> SnCl4 > PbCl4
π΄ 17. Oxidising character of M+4 species=
GeCl4 < SnCl4 < PbCl4
π΄ 18. Ease of hydrolysis of tetrahalides=
SiCl4 < GeCl4 < SnCl4 < PbCI4
π΄ 19. Acidic strength of trioxides=
N203 > P2O3 > As2O3
π΄ 20. Acidic strength of pentoxides=
N2O2 > P2O2> As202 > Sb2O2 > Biβ202
π΄ 21. Acidic strength of oxides of nitrogen=
N2O < NO <N2O3 <N2O4 < N2O5
π΄ 22. Basic nature/ bond angle/ thermal stability and dipole moment of hydrides=
NH3 > PH3 > AsH3 > SbH3 > BiH3
π΄ 23. Stability of trihalides of nitrogen=
NF3 > NCl3 > NBr3
π΄ 24.Lewis base strength=
NF3 <NCl3 <NBr3 < NI3
π΄ 25. Ease of hydrolysis of trichlorides=
NCl3 > PCI3 > AsCl3 > SbCl3 > BiCl3
π΄ 26. Lewis acid strength of trihalides of P, As, and Sb=
PCl3 > ASCl3 > SbCl3
π΄ 27. Lewis acid strength among phosphorus trihalides
PF3 > PCl3 > PBr3 > PI3
π΄ 28. Melting and boiling point of hydrides=
H2O > H2Te > H2Se >H2S
π΄ 29. Volatility of hydrides=
H2O < H2Te < H2Se < H2S
π΄ 30. Reducing nature of hydrides=
H2S < H2Se < H2Te
π΄ 31. Covalent character of hydrides=
H2O < H2S < H2Se < H2Te
π΄ 32. The acidic character of oxides (elements in the same oxidation state)=
SO2 > SeO2 > TeO2 > PoO2
SO3 > SeO3Β > TeO3
π΄ 33. Acidic character of oxide of a particular element (e.g. S)=
SO < SO2 < SO3
SO2 > TeO2 > SeO2 > PoO2
π΄ 34. Bond energy of halogens=
Cl2 > Br2 > F2 > I2
π΄ 35. Solubility of halogen in water =
F2 > Cl2 > Br2 > I2
π΄ 36. Oxidising power=
F2 > Cl2 > Br2 > I2
π΄ 37. Enthalpy of hydration of X ion=
F- > Cl- > Br- >I-
π΄ 38. Reactivity of halogens:=
F> Cl> Br > I
π΄ 39. Ionic character of M-X bond in halides
= M-F > M-Cl > MBr > M-I
π΄ 40. Reducing character of X ion:=
I- > Br- > Cl- > F-
π΄ 41. Acidic strength of halogen acids=
HI > HBr > HCI > HF
π΄ 42. Reducing property of hydrogen halides
= HF < HCL < HBr < HI
π΄ 43. Oxidising power of oxides of chlorine
= Cl2O > ClO2 > Cl206 > Cl2O7
π΄ 44. Decreasing ionic size=
02- > F- > Na+ > Mg2+
π΄ 45. Increasing acidic property=
Na2O3 < MgO < ZnO< P205
π΄ 46. Increasing bond length=
N2 <02 < F2 < CL2
π΄ 47. Increasing size=
Ca2+ < Cl- < S2-
π΄ 48. Increasing acid strength=
HClO < HClO2 < HClO3 < HClO4
π΄ 49. Increasing oxidation number of iodine=
HI< I2 <ICl <HIO4
π΄ 50. Increasing thermal stability=
HOCl < HOClO < HOClO2 < HOClO3
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π₯Increasings or Decreasing Orderπ₯
π΄ 01. Melting point=
Li > Na > K > Rb > Cs
π΄ 02. Colour of the flame=
Li-Red, Na-Golden, K-Violet, Rb-Red, Cs-Blue, Ca-Brick red, Sr-Blood red, Ba-Apple green
π΄ 03. Stability of hydrides =
LiH > NaH > KH > RbH> CsH
π΄ 04. Basic nature of hydroxides=
LIOH < NaOH < KOH < RbOH < CsOH
π΄ 05. Hydration energy=
Li> Na > K> Rb > Cs
π΄ 06. Reducing character=
Li > Cs > Rb > K > Na
π΄ 07. Stability of +3 oxidation state=
B> Al > Ga > In > T1
π΄ 08. Stability of +1 oxidation state= Ga < In < TI
π΄ 09. Basic nature of the oxides and hydroxides=
B< Al< Ga < In < TI
π΄ 10. Relative strength of Lewis acid= BF3 < BCl3 < BBr3 < BI3
π΄ 11. Ionisation energy=
B> Al <Ga > In <TI
π΄ 12. Reactivity=
C<Si< Ge < Sn <Pb
π΄ 13. Metallic character=
C< Si < Ge < Sn < Pb
π΄ 14. Acidic character of the oxides=
Co2 > SiO2 > Ge02 > SnO2 > PbO2
π΄ 15. Reducing nature of hydrides=
CH4 < SiH4Β < GeH4Β < SnH4 < PbH4
π΄ 16. Thermal stability of tetrahalides=
CCl4> SiCl4> GeCl4> SnCl4 > PbCl4
π΄ 17. Oxidising character of M+4 species=
GeCl4 < SnCl4 < PbCl4
π΄ 18. Ease of hydrolysis of tetrahalides=
SiCl4 < GeCl4 < SnCl4 < PbCI4
π΄ 19. Acidic strength of trioxides=
N203 > P2O3 > As2O3
π΄ 20. Acidic strength of pentoxides=
N2O2 > P2O2> As202 > Sb2O2 > Biβ202
π΄ 21. Acidic strength of oxides of nitrogen=
N2O < NO <N2O3 <N2O4 < N2O5
π΄ 22. Basic nature/ bond angle/ thermal stability and dipole moment of hydrides=
NH3 > PH3 > AsH3 > SbH3 > BiH3
π΄ 23. Stability of trihalides of nitrogen=
NF3 > NCl3 > NBr3
π΄ 24.Lewis base strength=
NF3 <NCl3 <NBr3 < NI3
π΄ 25. Ease of hydrolysis of trichlorides=
NCl3 > PCI3 > AsCl3 > SbCl3 > BiCl3
π΄ 26. Lewis acid strength of trihalides of P, As, and Sb=
PCl3 > ASCl3 > SbCl3
π΄ 27. Lewis acid strength among phosphorus trihalides
PF3 > PCl3 > PBr3 > PI3
π΄ 28. Melting and boiling point of hydrides=
H2O > H2Te > H2Se >H2S
π΄ 29. Volatility of hydrides=
H2O < H2Te < H2Se < H2S
π΄ 30. Reducing nature of hydrides=
H2S < H2Se < H2Te
π΄ 31. Covalent character of hydrides=
H2O < H2S < H2Se < H2Te
π΄ 32. The acidic character of oxides (elements in the same oxidation state)=
SO2 > SeO2 > TeO2 > PoO2
SO3 > SeO3Β > TeO3
π΄ 33. Acidic character of oxide of a particular element (e.g. S)=
SO < SO2 < SO3
SO2 > TeO2 > SeO2 > PoO2
π΄ 34. Bond energy of halogens=
Cl2 > Br2 > F2 > I2
π΄ 35. Solubility of halogen in water =
F2 > Cl2 > Br2 > I2
π΄ 36. Oxidising power=
F2 > Cl2 > Br2 > I2
π΄ 37. Enthalpy of hydration of X ion=
F- > Cl- > Br- >I-
π΄ 38. Reactivity of halogens:=
F> Cl> Br > I
π΄ 39. Ionic character of M-X bond in halides
= M-F > M-Cl > MBr > M-I
π΄ 40. Reducing character of X ion:=
I- > Br- > Cl- > F-
π΄ 41. Acidic strength of halogen acids=
HI > HBr > HCI > HF
π΄ 42. Reducing property of hydrogen halides
= HF < HCL < HBr < HI
π΄ 43. Oxidising power of oxides of chlorine
= Cl2O > ClO2 > Cl206 > Cl2O7
π΄ 44. Decreasing ionic size=
02- > F- > Na+ > Mg2+
π΄ 45. Increasing acidic property=
Na2O3 < MgO < ZnO< P205
π΄ 46. Increasing bond length=
N2 <02 < F2 < CL2
π΄ 47. Increasing size=
Ca2+ < Cl- < S2-
π΄ 48. Increasing acid strength=
HClO < HClO2 < HClO3 < HClO4
π΄ 49. Increasing oxidation number of iodine=
HI< I2 <ICl <HIO4
π΄ 50. Increasing thermal stability=
HOCl < HOClO < HOClO2 < HOClO3
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