Main Group Chemistry Exercise 1 Welcome to your Main Group Chemistry Exercise 1 today May 8, 2024 Name Email 1. What name is appropriate for the Group 18 element? Rare gases Inert gases Noble gases Non-reactive gases 2. The most abundant element in nature in Group 18 is Helium Argon Krypton Xenon 3. The effective nuclear charge of the element, He and Ne are ... and ... respectively. +2, +4 +2, +6 +2, +8 +4, +6 4. The boiling point of Helium is 2.4 K 4.2 K 2 K 3 K 5. Among the elements in Group 18, which element has the highest ionization energy? Xe Ne He Ar 6. Unless ________ is applied, ________ does not ________ at any temperature. and Helium 7. The study of matter at low temperature and the ability to flow without viscosity are ______ and ______ cryogenics, superfluidity superfluidity, viscosity cryogenics, viscosity low temperature, superfluidity 8. Among the following elements, which one exhibits the phenomenon of emitting white light when an electric current flows through it? Neon (Ne) Krypton (Kr) Argon (Ar) Helium (He) 9. Under which condition of temperature and pressure does the reaction Xe(g) + 2F2 → XeF4(g) occur favorably? 300°C and 1 atm 300°C and 6 atm 600°C and 6 atm 600°C and 1 atm 10. Despite the high relative abundance of H2 in nature, free H2 is only little because ________. H2 is light H2 is diatomic H2 atoms are held by Van der Waals forces H2 is chemically inert 11. The classification of hydrogen in Group 1 is primarily attributed to ________. its propensity to lose an electron its propensity to gain an electron its propensity to share an electron its atomic structure 12. How do the ions formed by hydrogen differ from the ions formed by Group 1 elements? Hydrogen ions exist as both liquid and gas, unlike the ions of Group 1 elements. Hydrogen ions exist as only gases, unlike the ions of Group 1 elements. Hydrogen ions exist as both liquid and gas, similar to the ions of Group 1 elements. Hydrogen ions exist as neither liquid nor gas, unlike the ions of Group 1 elements. 13. How do the characteristics of Group 1 elements and H2 at room temperature differ? Group 1 elements are highly reactive and electropositive, while H2 is relatively inert. Group 1 elements are inert and electropositive, while H2 is highly reactive. Group 1 elements are electropositive, inert, and highly reactive, unlike H2. Group 1 elements are highly reactive, while H2 is electropositive and inert 14. Which of the following elements is commonly used as a tracer? Hydrogen Tritium Iodine Carbon 15. The differences in the boiling points of H2O and D2O are primarily influenced by The polarity of the molecules. The strength of the hydrogen bonding interactions. The mass difference between hydrogen and deuterium isotopes. The strength of the covalent bond within the water molecules. 16. The term used to describe hydrogen at the moment of its preparation is ________. Atomic hydrogen Nascent hydrogen Nuclear hydrogen Reactive hydrogen 17. The production of atomic hydrogen can be achieved through ________. The reaction between metals and water Electron bombardment The reaction between coke and water Photodissociation of water molecules 18. In an equilibrium state, the distribution of ortho and para forms of hydrogen is characterized by ________ 25% ortho and 75% para 75% ortho and 25% para 50% ortho and 50% para 60% ortho and 40% para 19. In the industrial preparation of hydrogen through the steam reforming process, the catalyst used is ________. Ni at 1000°C Cu at 1000°C Cu at 400°C Pt at 800°C 20. Aluminium with a +3 oxidation state could be extracted from Bauxite (___________) and _________ (______), while the last member of Group IV, ______ with ____ and ____ oxidation states has Galena (_____) as its ore. Al2O3, Cryolite (Na3AlF6), Tin, +2, +4, PbS Al(OH)3, Halite (NaCl), Carbon, +3, +5, ZnS AlCl3, Fluorite (CaF2), Silicon, +2, +4, FeS2 Al2S3, Calcite (CaCO3), Lead, +1, +3, CuFeS2 21. Non-metallic elements: ________ conducts electricity due to the presence of ____________; _____________ fluoresce to give green faint light when burnt in air; __________ is a liquid substance, and ________ is inert at room temperature due to the presence of high __________ and __________ and then the absence of ____________ in it. The electronegativity of these elements in decreasing order is _____________. Graphite, delocalized pi electrons, Phosphorus, Bromine, ionization energy, electron affinity, noble gases, P > Br > C Diamond, free valence electrons, Chlorine, Mercury, atomic radius, ionization energy, hydrogen, Cl > Hg > C Silicon, mobile ions, Oxygen, Sulfur, electronegativity, electron affinity, transition metals, Si > S > O Carbon, localized pi bonds, Fluorine, Bromine, ionization energy, electron affinity, halogens, F > Br > C 22. S + O2 → SO2. Replacing S with P in the above reaction will give a product of ______ and in excess O2 gives _____ (name, ______________________). PO2, Phosphorus dioxide (Phosphorus(IV) oxide) P2O3, Phosphorus trioxide (Phosphorus(III) oxide) PO4, Phosphorus tetraoxide (Phosphorus(IV) oxide) P4O6, Phosphorus hexoxide (Phosphorus(VI) oxide) 23. The elements belonging to Groups 6 and 7 are commonly referred to as _________ and ___________ respectively. They have the ability to form binary compounds with various elements on the Periodic table. For instance, when the second member element of each group reacts with Tin, the resulting compounds are _________, __________, ___________, and ___________. Halogens, Chalcogens, SnF2, SnCl2, SnBr2, SnI2 Alkali metals, Alkaline earth metals, SnO, SnS, SnSe, SnTe Transition metals, Noble gases, SnO2, SnS2, SnSe2, SnTe2 Lanthanides, Actinides, SnO3, SnS3, SnSe3, SnTe3 24. Phenomena: ________ undergoes passivity when reacting with acid, forming a _________ layer. _________ demonstrates catenation due to its _________ being equal to or greater than 2, and its tendency to form stronger _________ bonds with its own atoms rather than with other atoms. In Group III, _________ ionizes to produce a monovalent ion because of its _________ being significantly high. Among the fluorides of alkali metals, all are soluble in aqueous solutions except for _________. Furthermore, _________ shares similar chemical characteristics with __________. Copper, oxide, Oxygen, atomic radius, metallic, Gallium, electron affinity, Potassium, Rubidium Iron, oxide, Nitrogen, electronegativity, ionic, Indium, electron configuration, Cesium, Francium Aluminum, protective, Carbon, valence, covalent, Boron, ionization energy, Lithium, Sodium Chromium, passivation, Sulfur, electron configuration, metallic, Aluminum, atomic radius, Francium, Radium 25. i) Sn(CO3)2(s) → SnO2 (s) + 2CO2(g), ii) 4Bi(NO3)3 → 2Bi2O3(s) + 12NO2(g) + 3O2 (g) Based on the given reactions, the acidic oxides are _______ and ________; the basic oxide is _______; and the amphoteric oxide is _______. Furthermore, when limestone is heated, it produces P (an acidic oxide) and Q (a basic oxide). Q can react with silica to form R (IUPAC name: ______________________). Similarly, Q can combine with carbon disulphide to yield S (IUPAC name: _______________________). The reaction equations are as follows: SnO2, Bi2O3, CO2, Bi2O3, P (carbon dioxide), Q (calcium oxide), Silicon dioxide, R (calcium silicate), Q (calcium oxide), Carbon disulphide, S (calcium carbide) SnO2, Bi2O3, CO2, Bi2O3, P (carbon monoxide), Q (calcium carbonate), Silicon dioxide, R (calcium silicate), Q (calcium carbonate), Carbon disulphide, S (calcium carbonate) CO2, O2, SnO2, Bi2O3, P (carbon dioxide), Q (calcium oxide), Silicon dioxide, R (calcium silicate), Q (calcium oxide), Carbon disulphide, S (calcium carbide) CO2, O2, SnO2, Bi2O3, P (carbon monoxide), Q (calcium carbonate), Silicon dioxide, R (calcium silicate), Q (calcium carbonate), Carbon disulphide, S (calcium carbonate) 26. The molecular formula of halide that: i) possesses a bridged dimer is _________; ii) forms a complex with ammonia is ______; iii) is a weak acid is _____; iv) is not prepared by direct combination but by substitution reaction is ______; v) are ammoniates are ___________ and ____________ . i) F2; ii) [Pd(NH3)4]Cl2; iii) H2SO4; iv) NaCl; v) [Cu(NH3)4]Cl2 and [Ag(NH3)2]Cl i) Br2; ii) [Fe(NH3)6]Cl3; iii) HBr; iv) ZnCl2; v) [Cr(NH3)6]Cl3 and [Co(NH3)6]Cl3 i) I2; ii) [Ag(NH3)2]Cl; iii) HCl; iv) MgCl2; v) [Ni(NH3)6]Cl2 and [Pt(NH3)4]Cl2 i) Cl2; ii) [Cu(NH3)4]Cl2; iii) HF; iv) AlCl3; v) [Cr(NH3)6]Cl3 and [Co(NH3)6]Cl3 27. Which of these elements is the first member of its group? And Chalcogens are: P and Salt formers S and Ore formers Se and Noble non-metals F and Inert gases 28. Which of these elements exhibit inert pair effect and which element is not a diatomic molecule? Cl and Oxygen F and Chlorine Bi and Nitrogen Se and Phosphorus 29. Which of these options correctly describes the groups 5, 6, and 7 elements and the general outer electronic configuration of group 16? Groups 5, 6, and 7 elements are also called elements of the s-block, and the general outer electronic configuration of group 16 is ns2 np6. Groups 5, 6, and 7 elements are also called elements of the d-block, and the general outer electronic configuration of group 16 is ns2 np5. Groups 5, 6, and 7 elements are also called elements of the p-block, and the general outer electronic configuration of group 16 is ns2 np4. Groups 5, 6, and 7 elements are also called elements of the f-block, and the general outer electronic configuration of group 16 is ns2 np3. 30. Which of these elements does not exist in free state naturally and could exist as a white solid? Nitrogen Phosphorus Oxygen Sulphur 31. Which of these elements could exist as a pale blue gas? Nitrogen Phosphorus Oxygen Sulphur 32. Which of the following substances does NOT contain sulphur? Zinc blende Silica Gypsum Iron pyrite 33. Which of the following is extracted using fractional distillation? Nitrogen and sulphur Nitrogen and oxygen Oxygen and hydrogen Nitrogen and hydrogen 34. What is the chemical formula of carnalite? KCl.MgCl2. 6H2O KCl.MgCl2. 4H2O KCl.MgCl2. 2H2O KCl.MgCl2 35. Among the following molecules, which one produces a greenish-yellow color? Selenium Chlorine Nitrogen Iodine 36. Arrange the following elements in increasing order of their atomic radii: F2, Cl2, Br2, I2 Cl2, F2, Br2, I2 F2, Br2, Cl2, I2 I2, Br2, Cl2, F2 37. Which of these compounds represents an oxide? NaOCl NaNO3 N2O4 NO2- 38. Among the following oxides, which one has the highest oxidation number? K2O ZnO Fe2O3 N2O5 39. Which compound among the following is a weak base and a precipitating agent? NH3 H2S HCl H2O 40. Which compound among the following is an effective solvent for ionic compounds, facilitates the hydration of ethene, and promotes the hydrolysis of C2H5OH? H2S HBr H2O HI 41. In the chemical equation FeY + 2HCl → FeCl2 + H2Y, what element is represented by the symbol Y? Nitrogen Phosphorus Sulphur Chlorine 42. Among the following options, which compound is the strongest acid, considering their related properties? H2O (water) - low ionization constant H2S (hydrogen sulfide) - limited ionization in water H2Se (hydrogen selenide) - slightly higher acidity than H2S H2Te (hydrogen telluride) - significant ionization in water 43. Among the following oxides, which one cannot react with both NaOH (sodium hydroxide) and HCl (hydrochloric acid)? N2O (nitrous oxide) P4O6 (phosphorus trioxide) TeO2 (tellurium dioxide) Bi2O3 (bismuth trioxide) 44. Which of the following compounds is the oxo-chlorate (I) acid? HOCl (hypochlorous acid) HClO2 (chlorous acid) HClO3 (chloric acid) HClO4 (perchloric acid) 45. Which of the following sequences represents the increasing order of disproportionation of hypohalites? [OI-], [OCl-], [OBr-] [OBr-], [OCl-], [OI-] [OCl-], [OBr-], [OI-] [OBr-], [OI-], [OCl-] 46. Which of the following substances does fluorine NOT react violently with? Oxygen Bismuth Nitrogen Xenon 47. Which of the following is NOT a hydride of nitrogen? Ammonia Hydrazine Hydroxonium Hydrogen azide 48. In which of the following substances does oxygen NOT occur naturally? Water Carbohydrate Hydrocarbon Proteins 49. Which of the following is the reason for the high boiling point of water? Presence of ionic bonding Presence of covalent bonding Presence of coordinate bonding Presence of hydrogen bonding 50. Which of the following compounds is not a hydride? H2O2 HCOOH N2H4 H2S 51. What is the correct electronic configuration of iodine? [Xe] 4d10 5s2 5p5 [Ar] 4d10 5s2 5p5 [Xe] 3d10 4s2 4p5 [Ar] 3d10 4s2 4p5 52. Which of the following elements does NOT exhibit variable oxidation states? N P O Cl 53. Which of the following elements exhibits the inert pair effect? As - Arsenic Te - Tellurium Cl - Chlorine S - Sulfur 54. Which of the following elements is a gaseous member of its group? P - Phosphorus S - Sulfur Br - Bromine N - Nitrogen 55. Which of the following elements is stored under water? Brown Bromine White Phosphorus Pale blue Ozone Yellow Sulphur 56. Which of the following groups of elements is monovalent? Alkali earth metal Pnictogen Chalcogen Halogen 57. Which of the following elements forms molecules? Aluminium Carbon Lead Gallium 58. Which of the following elements is found in trace quantities? Carbon (C) Germanium (Ge) Boron (B) Tin (Sn) 59. Which of the following elements exist in a free state naturally? Carbon (C) Aluminium (Al) Indium (In) Tin (Sn) 60. Which of the following elements can be extracted from cryolite? Cr (Chromium) and F (Fluorine) Al (Aluminium) and F (Fluorine) Na (Sodium) and F (Fluorine) Na (Sodium) and Al (Aluminium) 61. Which of the following options represents the correct electronic configuration of Mg2+? 1s² 2s² 2p⁶ 1s² 2s² 2p⁶ 3s¹ 1s² 2s² 2p⁶ 3s² 1s² 2s² 2p⁶ 3s² 3p¹ 62. Which of the following options represents the elements corresponding to the given general electronic configurations: ns1, ns2np2, ns2np5, and ns2np6? Ba (Barium), C (Carbon), Cl (Chlorine), and Ne (Neon) Rb (Rubidium), Ge (Germanium), F (Fluorine), and Ar (Argon) Li (Lithium), Si (Silicon), Se (Selenium), and I (Iodine) B (Boron), P (Phosphorus), O (Oxygen), and He (Helium) 63. Which of the following inert gases does not strictly adhere to the octet rule? He (Helium) Ar (Argon) Ne (Neon) Kr (Krypton) 64. Among the following compounds, which one is insoluble in aqueous solution? LiF (Lithium fluoride) NaF (Sodium fluoride) KF (Potassium fluoride) RbF (Rubidium fluoride) 65. Which of the following compounds will produce similar products to the reaction MgCO3 -> MgO + CO2? Rb2CO3 (Rubidium carbonate) K2CO3 (Potassium carbonate) Na2CO3 (Sodium carbonate) Li2CO3 (Lithium carbonate) 66. The Be2+ ion is hydrated in aqueous solution, forming [Be(H2O)4]2+ as it also happens with which of the following ions? Na+ Mg2+ Al3+ K+ 67. Limestone decomposes on heating to give which of the following compounds? CaO Na2O CO2 SO2 68. When magnesium oxide reacts with silica, the resulting compound is: Magnesium silicide Magnesium basilica Magnesium tetraoxosilicate (IV) Magnesium trioxosilicate (IV) 69. Potassium hydroxide reacts with ------------- to form a salt. CO N2O As2O5 H2O 70. The combination of chlorine and alkali metal will result in: RbCl GaCl MgCl2 SbCl3 Thank you for attempting Main Group Chemistry Exercise 1. Kindly share this link https://chemistreal.com/quiz/main-group-chemistry-exercise-1/
