LEARN TECH ||ethiopia ®

🔥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 <Ga > In <TI 🔴 12. Reactivity= C<Si< Ge < Sn <Pb 🔴 13. Metallic character= C< Si < Ge < Sn < Pb 🔴 14. Acidic character of the oxides= Co2 > 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 > Bi‌202 🔴 21. Acidic strength of oxides of nitrogen= N2O < NO <N2O3 <N2O4 < N2O5 🔴 22. Basic nature/ bond angle/ thermal stability and dipole moment of hydrides= NH3 > PH3 > AsH3 > SbH3 > BiH3 🔴 23. Stability of trihalides of nitrogen= NF3 > NCl3 > NBr3 🔴 24.Lewis base strength= NF3 <NCl3 <NBr3 < NI3 🔴 25. Ease of hydrolysis of trichlorides= NCl3 > 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 <ICl <HIO4 🔴 50. Increasing thermal stability= HOCl < HOClO < HOClO2 < HOClO3 @Entranceprepare

Questions on chemistry grade 11 unit 2 1. Who proposed the concept of the atom as an indivisible particle? a) John Dalton b) J.J. Thomson c) Ernest Rutherford d) Niels Bohr 2. Which experiment led to the discovery of the electron? a) Millikan's oil drop experiment b) Rutherford's gold foil experiment c) Thomson's cathode ray tube experiment d) Bohr's hydrogen spectrum experiment. 3. Which subatomic particle is responsible for the majority of the mass of an atom? a) proton b) electron c) neutron d) nucleus 4. What is the charge and relative mass of a neutron? a) charge: +1, mass: 1 amu b) charge: -1, mass: 1 amu c) charge: 0, mass: 1 amu d) charge: 0, mass: 0 amu 5. Which of the following electromagnetic radiations has the highest energy? a) radio waves b) microwaves c) visible light d) gamma rays 6. What does the principal quantum number (n) represent in the quantum mechanical model of the atom? a) shape of the orbital b) orientation of the orbital c) distance from the nucleus d) spin of the electron 7. What is the maximum number of electrons that can occupy the 2p subshell? a) 2 b) 4 c) 6 d) 8 8. Which of the following elements has the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶? a) carbon b) silicon c) argon d) calcium 9. Which principle states that no two electrons in an atom can have the same set of four quantum numbers? a) Aufbau principle b) Pauli exclusion principle c) Hund's rule d) Heisenberg uncertainty principle 10. Which of the following elements has the highest electronegativity value? a) lithium b) carbon c) oxygen d) fluorine 11. Which of the following elements is an alkaline earth metal? a) sodium b) magnesium c) chlorine d) nitrogen 12. Which of the following elements is a halogen? a) helium b) neon c) fluorine d) argon 13. Which of the following elements has the largest atomic radius? a) lithium b) carbon c) nitrogen d) fluorine 14. Which of the following elements has the highest ionization energy? a) sodium b) magnesium c) chlorine d) potassium 15. Which of the following elements is a transition metal? a) copper b) helium c) nitrogen d) argon 16. Which of the following elements is a noble gas? a) lithium b) carbon c) neon d) fluorine 17. Which of the following elements is a metalloid? a) sodium b) carbon c) oxygen d) fluorine 18. Which of the following elements has the highest melting point? a) sodium b) magnesium c) chlorine d) tungsten 19. Which of the following elements is a lanthanide? a) iodine b) uranium c) neodymium d) zinc 20. Which of the following elements is a synthetic element? a) hydrogen b) carbon c) plutonium d) oxygen 21. Which of the following quantum numbers describes the shape of an atomic orbital? a) principal quantum number (n) b) azimuthal quantum number (l) c) magnetic quantum number (ml) d) spin quantum number (ms) 22. What is the maximum number of orbitals in the p subshell? a) 1 b) 2 c) 3 d) 4 23. How many electrons can occupy the 3d subshell? a) 2 b) 6 c) 10 d) 14 24. Which of the following quantum numbers describes the orientation of an atomic orbital? a) principal quantum number (n) b) azimuthal quantum number (l) c) magnetic quantum number (ml) d) spin quantum number (ms) 25. What is the maximum number of electrons that can occupy the 4th energy level? a) 8 b) 18 c) 32 d) 50 መልሶቹን ሞክሩ ተወያዩባቸው መልስ ይለቀቃል

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