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The base-emitter junctions of a transistor is
The current carries in a PNP transistor is
A transistor has
+5
Gravitation Handwritten Notes
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+8Oscillation Handwritten Notes
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β
Solids in different categories based on the nature of intermolecular forces operating in them:
π
Potassium sulphate β Ionic bond is formed,wherein potassium loses electrons & sulphate gains electrons
π
Tin β Tin can form two ions Sn 2+ or Sn4+ now depending on what form it is in and what other element it is bonding with then only the type of bonding will be known
π
Benzene β it is comprise of sp2 hybridized carbon atoms which makes covalent bond with each other by mutual sharing &pairing of electrons
π
Urea β Polar molecular solid & they mostly forms hydrogen bond with other atoms
π
Ammonia β covalently bonded polar compound formed by mutual sharing & pairing of electrons between nitrogen & three hydrogen atoms
π
Water β covalently bonded polar compound formed by mutual sharing of electrons between oxygen & hydrogen atoms
π
Zinc sulphide β it exist in the form of crystals & makes coordination bond
π
Graphite β it consist of carbon atoms & have covalent bond between them forming a 2-D (flat, planar etc.) network, which in itself is strong. These planes are then held together by London Forces, which are very weak.
π
Rubidium β Metallic bond is formed by rubidium because it is a metal.Metallic bond is hydrid of covalent bond & ionic bond
π
Argon β Non-polar molecular solid
π
Silicon carbide β Covalent or network solid
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 < SiH4 < GeH4 < 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 > BiΜ202
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 > SeO3 > 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
During simple harmonic motion of a body, the energy at the extreme positions is
Let Lβ and Le be the orbital angular momentum of an electron in the first and second excited states of hydrogen atom, respectively. According to the Bohr's model, the ratio Lβ: Lβ is:
Which one of the following electrons in the ground state will have least amount ofenergy?
The work done when 1 mole of a gas expands reversibly and Isothermally from
pressure of 5 atm to 1 atm at 300 K is (Given log 5-0.6989 and R-8.314 JK mol)
One mole of sugar is dissolved in three moles of water at 298 K. The relative lowering of vapourpressure is
Reduction can be done by
Matte is a mixture of
What's the ideal temperature in Roasting used?
Which gas is primarily released in Calcination?
Which gas is primarily released in roasting ?
Maximum covalency of first member of each group is ____ .
