Chemistry books

2021-06-28 10:58:15 INORGANIC IN SHOTS

Increasings or Decreasing Order

01. Melting point=
Li > Na > K > Rb > Cs

02. Colour of the flame=
Li-Red, Na-Golden, K-Violet, Rb-Red, Cs-Blue, Ca-Brick red, Sr-Blood red, Ba-Apple green

03. Stability of hydrides =
LiH > NaH > KH > RbH> CsH

04. Basic nature of hydroxides=
LIOH < NaOH < KOH < RbOH < CsOH

05. Hydration energy=
Li> Na > K> Rb > Cs

06.) Reducing character=
Li > Cs > Rb > K > Na

07. Stability of +3 oxidation state=
B> Al > Ga > In > T1

08. Stability of +1 oxidation state= Ga < In < TI

09. Basic nature of the oxides and hydroxides=
B< Al< Ga < In < TI

10. Relative strength of Lewis acid= BF3 < BCl3 < BBr3 < BI3

11. Ionisation energy=
B> Al In SiO2 > Ge02 > SnO2 > PbO2

15. Reducing nature of hydrides=
CH4 < SiH4 < GeH4 < SnH4 < PbH4

16. Thermal stability of tetrahalides=
CCl4> SiCl4> GeCl4> SnCl4 > PbCl4

17. Oxidising character of M+4 species=
GeCl4 < SnCl4 < PbCl4

18. Ease of hydrolysis of tetrahalides=
SiCl4 < GeCl4 < SnCl4 < PbCI4

19. Acidic strength of trioxides=
N203 > P2O3 > As2O3

20. Acidic strength of pentoxides=
N2O2 > P2O2> As202 > Sb2O2 > Bi̟202

21) Acidic strength of oxides of nitrogen=
N2O < NO PH3 > AsH3 > SbH3 > BiH3

23. Stability of trihalides of nitrogen=
NF3 > NCl3 > NBr3

24.Lewis base strength=
NF3 PCI3 > AsCl3 > SbCl3 > BiCl3

26.Lewis acid strength of trihalides of P, As, and Sb=
PCl3 > ASCl3 > SbCl3

27. Lewis acid strength among phosphorus trihalides
PF3 > PCl3 > PBr3 > PI3

(28) Melting and boiling point of hydrides=
H2O > H2Te > H2Se >H2S

29. Volatility of hydrides=
H2O < H2Te < H2Se < H2S

30. Reducing nature of hydrides=
H2S < H2Se < H2Te

31. Covalent character of hydrides=
H2O < H2S < H2Se < H2Te

32. The acidic character of oxides (elements in the same oxidation state)=
SO2 > SeO2 > TeO2 > PoO2
SO3 > SeO3 > TeO3

33. Acidic character of oxide of a particular element (e.g. S)=
SO < SO2 < SO3
SO2 > TeO2 > SeO2 > PoO2

34. Bond energy of halogens=
Cl2 > Br2 > F2 > I2

35. Solubility of halogen in water =
F2 > Cl2 > Br2 > I2

36. Oxidising power=
F2 > Cl2 > Br2 > I2

37. Enthalpy of hydration of X ion=
F- > Cl- > Br- >I-

38. Reactivity of halogens:=
F> Cl> Br > I

39. Ionic character of M-X bond in halides
= M-F > M-Cl > MBr > M-I

40. Reducing character of X ion:=
I- > Br- > Cl- > F-

41. Acidic strength of halogen acids=
HI > HBr > HCI > HF

42 Reducing property of hydrogen halides
= HF < HCL < HBr < HI

43. Oxidising power of oxides of chlorine
= Cl2O > ClO2 > Cl206 > Cl2O7

44. Decreasing ionic size=
02- > F- > Na+ > Mg2+

45 Increasing acidic property=
Na2O3 < MgO < ZnO< P205

46 Increasing bond length=
N2 <02 < F2 < CL2

47 Increasing size=
Ca2+ < Cl- < S2-

48 Increasing acid strength=
HClO < HClO2 < HClO3 < HClO4

49 Increasing oxidation number of iodine=
HI< I2


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2021-06-28 08:12:55 Teaching tips

Encourage students to draw diagrams as part of their introduction to VSEPR theory and molecular shape. Whiteboards can support formative assessment either by the teacher or peers.

Explicitly use dot-and-cross diagrams to support the analytical processing involved in VSEPR. These diagrammatic representations can be a more helpful way to count electrons.

Model sketching 3D representations of predicted molecular geometries for students with weaker visuospatial abilities by showing how to draw dash-wedge representations. This will reinforce mental visualisation before introducing VSEPR theory.

Use visual guides to support students with high visuospatial ability. These students might favour imagistic approaches, but need to be able to apply accurate geometric terminology to 3D diagrams to meet exam requirements.

Analyse students’ sketches to provide insight into their visuospatial and analytical thinking. The process of sketching itself can be valuable in supporting deeper learning. Bear in mind that apparently accurate drawings may not reflect a solid conceptual understanding.

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2021-06-28 08:12:36 5 tips for teaching VSEPR theory Open / Comment

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