C2.2 Chemical Families 1. Mention the physical properties of Alkali metals Alkali metals have a shiny metallic luster when cut which quickly tarnishes as it reacts with the surrounding air.Alkali metals are soft and easy to cutAlkali metals have low melting and boiling pointsAll of the above 2. Does the electron affinity decrease as the size of the atoms increases in Halogen hence the reactivity decreases down the group? {Fluorine reacts more than iodine} True or False TRUEFALSEMaybeNone 3. Mention the characteristics of Halogens The atomic radii increase down the groupThe ionic radii increase down the groupAn increase in the number of occupied energy levels.All of the above 4. Does the ionization energy decrease as you go down the group of alkali metals? FALSEMaybeTRUENone 5. The elements in group 1 of the periodic table are called Alkali metals True or False TRUEFALSEMaybeNone 6. Mention the uses of noble gas Argon is used in light bulbs to provide an inert environment to prevent oxidationArgon is used as an insulator in arch-weldingNeon gas is used in street and advertisement lightAll of the above 7. What is the name of the minimum energy required to remove an electron from the outermost energy level of an atom in the gaseous state? Ionic radiusAtomic radiusIonization energy None of the mentioned 8. Mention the Electrical physical properties of elements in period 3 Some such as Sodium, Magnesium, and Aluminum conduct electricity due to the presence of delocalized electronsSome do not conduct electricity such as Phosphorous, Sulphur, and chlorine which are molecules are lack delocalized electronsSome like Silicon are semi-conductorsAll of the above 9. The atomic radius of Halogen atom is less than the ionic radius of halogen ion e.g. Chlorine atom and Chlorine ion True or False TRUEFALSEMaybeNone 10. The elements in group 8 of the periodic table are called HalogensAlkaline metalsAlkaline earth metalsNoble gases 11. Which of the following is not an example of alkali metal? CalciumLithiumSodiumPotassium 12. Explain why the melting and boiling points decrease down the group of alkali metals Due to the weakening of the forces holding the atoms togetherAs the atomic radius increases as you go down the group the forces of attraction between the atoms weakenBoth A and B None of the mentioned 13. Mention the physical properties of noble gases Are colorless monoatomic gasesTheir atomic radius increases down the group due to the increase in the number of energy levelsHave a low melting and boiling points due to weak inter-atomic forces of attraction between atomsAll of the above 14. Which of the following doesn’t belong to alkaline earth metals? MagnesumBerylliumCalciumSodium 15. Explain why there is an increase in reactivity as you go down the alkali metal group from Lithium to Potassium Due to the ease of losing valence electrons increases down the group as the atomic radius increasesThe most reactive metal which is Potassium its outermost electron is easily removed during a reactionThe atomic radius decreases as you go down the groupBoth A and B 16. Mention the chemical properties of Alkaline earth metals They react in the air to form Metal oxides and react with water to form alkaline solution and hydrogen gas.Magnesium reacts with steam to give Magnesium oxide and hydrogen gasAlkaline earth metals react with chlorine to give out Metal chloride (Magnesium Chloride and Calcium chloride).All of the above 17. Mention the chemical properties of alkali metals Alkali metals react with water to form alkaline solutions and hydrogen gasAlkali metals react with chlorine gas to form metal chlorides.Alkali metals react with oxygen to form a baseBoth A and B 18. Mention the characteristics of Noble gases Their outermost energy level is full with Helium (2) duplet and the rest have (8) octetNeither gain nor lose electronsThey are stable and non-reactiveAll of the above 19. In Alkali metals, the electrons in the outermost energy level move randomly throughout the metallic structure and are said to be delocalized? TRUEFALSEMaybeNone 20. How many alkali metal ions is needed to combine one oxide ion? 1324 21. Mention the uses of Halogens and their compounds Chlorine is used to make bleaches used in paper pulp.Chlorine is added to water to kill micro-organismsFluorine is used to manufacture hydrogen fluoride used to engrave words or picturesAll of the above 22. Explain why Halogen melting and boiling point level increase as you go down the group? {Iodine has high melting and boiling point than Fluorine} Presence of delocalized electronsIntermolecular forces increase with the increase in the size of the molecules Force of attraction decreases with the size of the moleculesNone of the mentioned 23. What is the name of the energy released as an ion is formed in halogen? Ionization energyElectron affinity CationAnion 24. Which of the following statement describes the characteristics of alkaline earth metals? It has two electrons in the outermost energy levelIts atomic radius increases as you go down the groupIts ionic radius reduces as you go down the groupAll of the above 25. Explain why is the ionic radius of an alkali metal is less than its atomic radius An alkali metal forms an ion by losing the single electron from the outermost energy level.The resulting ion {cation} has one less occupied energy level than the alkali atomThe ionic radius is nearer to the nucleus than the atomBoth A and B 26. Explain why are alkali metals are good conductors of heat and electricity Presence of delocalized (free) electrons Absence of free electronsPresence of mobile atomsNone of the mentioned 27. Which of the following is not a noble gas? HeliumNeonArgonChlorine 28. Mention the uses of alkali metals and their compounds Lithium compounds are used in the manufacture of mobile phone dry cellsSodium chloride is used as a food additive.Molten sodium is used as a reducing agent in the extraction of titaniumAll of the above 29. The elements in Group 2 of the periodic table are called? Alkali metals Form two'sAlkaline earth metalsNone of the mentioned 30. Mention the physical properties of Halogens Fluorine and chlorine are gaseous at room temperature while bromine is brown liquid and iodine a shiny dark grey solidThe solubility of halogens in water decreases down the groupHalogens are non-conductors of heat and electricityAll of the above 31. Explain why Halogens cannot conduct heat and electricity Absence of delocalized electrons Presence of delocalized electronsAbsence of mobile atomsNone of the mentioned 32. Which among the following element is not among Period 3? SodiumPotassiumMagnessiumAluminium 33. Mention the examples of Halogens FluorineChlorineBromineAll of the above 34. Mention the chemical properties of Halogens It reacts with metals to form Metal chloride ( salt)It reacts with water to form an acid.Chlorine + water + Hydrochloric acid + Chloric (I) acidAll of the above 35. Mention the uses of Alkaline earth metals and their compounds Magnesium is used in the manufacture of magnesium hydroxide which is used as anti-acid medicine.Calcium carbonate is used in the extraction of iron.Magnesium oxide is used in the lining of furnaces.All of the above 36. Non-metals in Group 7 are called AlkaliAlkaline earth metalsHalogensNone 37. Why is the atomic radius of halogen atom less than the ionic radius of halogen ion? Halogen atom gains an electron in the outermost energy level to become an ionHalogen atom loses an electron in the outermost energy level to become an ionHalogen atom loses all the electron in the outermost electron to become an ionNone of the mentioned 38. Explain why atomic radii of the alkali metals increase down the group Each alkali metal has one more occupied energy level than the preceding member in the group Alkali metals have one valence electron in the outermost energy levelAlkali metals lose an electron to form a positively charged ionNone of the mentioned. 39. Mention the physical properties of elements in period 3 The atomic radii decrease across the period from left to right of the periodic tableHigh melting and boiling points of aluminum compared to metals sodium and magnesiumThe high melting point of silicon compared to non-metals Phosphorous and ChlorineAll of the above 40. Define Atomic Radius? The distance between the center of the nucleus of an atom and the innermost energy level occupied by an electron(sThe distance between the nucleus and the outermost energy levelThe distance between the center of the nucleus of an atom and the outermost energy level occupied by an electron(s).None of the mentioned 41. Due to their reactivity alkali metals are not found as free electrons rather as combined elements FALSEMaybeTRUENone 42. Explain why the ionization energy decreases as you go down the group of alkali metals Increase in the atomic size as you down the grouphe decrease in the force of attraction between the positive nucleus and the negative outermost electron.Increase in the atomic radius as you go down the groupAll of the above 43. Mention the physical properties of Alkaline earth metals When alkaline earth metal is polished it acquires a metallic luster and you must polish it before an experiment in order to remove the thin oxide layer which forms on the surfaceThey are good conductors of electricity and have high melting and boiling pointsThey are brittle (calcium) and ductile (magnesium) hence hard to cut with a knifeAll of the above Loading...
In Alkali metals, the electrons in the outermost energy level move randomly throughout the metallic structure and are said to be delocalized?
