AP TS DSC SA - PHYSICAL SCIENCE
METALS AND NON METALS
Physical Properties of Metals and Non-metals, Chemical Properties of Metals and Non-metals, Uses of Metals and Non-metals, Examples of metals and non-metals, Reactivity order of metals.
Here are questions and answers covering the physical and chemical properties, uses, examples, and reactivity of metals and non-metals.
1. Physical Properties of Metals
Q1. What are some common physical properties of metals?
A1. Metals generally have high melting and boiling points, good electrical and thermal conductivity, malleability, ductility, and a shiny luster.
Q2. Why are metals good conductors of electricity?
A2. Metals are good conductors of electricity because they have free-moving delocalized electrons that can carry electrical charge through the metal.
Q3. How does the density of metals compare to non-metals?
A3. Metals generally have higher densities compared to non-metals due to their closely packed atomic structure and heavier atomic masses.
Q4. What property allows metals to be hammered into thin sheets?
A4. The property that allows metals to be hammered into thin sheets is malleability, which means metals can be deformed under compressive stress without breaking.
Q5. Which metal is known for its high density and is used in the production of heavy machinery?
A5. Lead is known for its high density and is used in applications such as batteries and radiation shielding.
2. Physical Properties of Non-Metals
Q6. What are some common physical properties of non-metals?
A6. Non-metals typically have lower melting and boiling points, poor electrical and thermal conductivity, and are not malleable or ductile. They can be gases, liquids, or solids at room temperature.
Q7. How does the appearance of non-metals compare to metals?
A7. Non-metals usually lack the shiny luster characteristic of metals and can appear dull or colorless. They may be transparent (e.g., gases) or colored (e.g., iodine crystals).
Q8. Why are non-metals poor conductors of electricity?
A8. Non-metals are poor conductors of electricity because they lack free-moving electrons or ions that can carry electrical charge.
Q9. Give an example of a non-metal that is a good conductor of electricity.
A9. Graphite, a form of carbon, is a non-metal that is a good conductor of electricity due to its delocalized electrons in its structure.
Q10. What is the state of non-metals like nitrogen and oxygen at room temperature?
A10. Nitrogen and oxygen are gases at room temperature.
3. Chemical Properties of Metals
Q11. How do metals generally react with acids?
A11. Metals generally react with acids to produce a salt and hydrogen gas. For example, zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas.
Q12. What happens when a metal reacts with oxygen?
A12. When a metal reacts with oxygen, it typically forms a metal oxide. For example, iron reacts with oxygen to form iron(III) oxide (rust).
Q13. Why are metals considered to be good reducing agents?
A13. Metals are considered good reducing agents because they easily lose electrons (are oxidized) during chemical reactions, which can reduce other substances.
Q14. What is the reactivity trend of metals in the periodic table?
A14. In general, metals become more reactive as you move down a group in the periodic table and less reactive as you move from left to right across a period.
Q15. Give an example of a metal that reacts violently with water.
A15. Sodium reacts violently with water to produce sodium hydroxide and hydrogen gas.
4. Chemical Properties of Non-Metals
Q16. How do non-metals generally react with metals?
A16. Non-metals generally react with metals to form ionic compounds. For example, chlorine reacts with sodium to form sodium chloride.
Q17. What happens when a non-metal reacts with oxygen?
A17. When a non-metal reacts with oxygen, it typically forms a non-metal oxide, which can be acidic. For example, sulfur reacts with oxygen to form sulfur dioxide.
Q18. How do non-metals generally react with bases?
A18. Non-metals generally do not react with bases. However, some non-metal oxides can react with bases to form salts and water.
Q19. Which non-metal is known for its ability to form multiple allotropes?
A19. Carbon is known for its ability to form multiple allotropes, including diamond, graphite, and graphene.
Q20. How do non-metals generally react with acids?
A20. Non-metals generally do not react with acids. However, non-metal oxides can react with acids to form salts and water.
5. Uses of Metals
Q21. What is aluminum commonly used for?
A21. Aluminum is commonly used in the manufacturing of lightweight materials such as airplane parts, cans, and foil.
Q22. What are the primary uses of iron?
A22. Iron is primarily used in the production of steel, which is used in construction, automotive, and machinery industries.
Q23. How is copper used in electrical applications?
A23. Copper is used in electrical applications due to its excellent conductivity, and it is commonly used for electrical wiring and components.
Q24. What is platinum used for in catalytic converters?
A24. Platinum is used as a catalyst in catalytic converters to help convert harmful gases from automobile exhaust into less harmful substances.
Q25. What is the significance of gold in electronics?
A25. Gold is used in electronics due to its excellent corrosion resistance and conductivity, making it ideal for high-quality connectors and circuitry.
6. Uses of Non-Metals
Q26. What are some common uses of sulfur?
A26. Sulfur is used in the manufacture of sulfuric acid, fertilizers, and as a fungicide and disinfectant.
Q27. How is chlorine used in water treatment?
A27. Chlorine is used to disinfect and purify water by killing bacteria and other microorganisms.
Q28. What are the industrial applications of nitrogen?
A28. Nitrogen is used in the production of ammonia for fertilizers, as a refrigerant, and as an inert atmosphere in industrial processes.
Q29. How is helium utilized in scientific research?
A29. Helium is used as a coolant in cryogenics, especially in superconducting magnets, and in various scientific research applications due to its low boiling point.
Q30. What are the primary uses of carbon?
A30. Carbon is used in various forms, including graphite for batteries and lubricants, activated carbon for filtration, and carbon fibers for high-strength materials.
7. Examples of Metals
Q31. Name a metal that is liquid at room temperature.
A31. Mercury is the only metal that is liquid at room temperature.
Q32. Which metal is known for its use in dental alloys?
A32. Silver is commonly used in dental alloys for its durability and resistance to corrosion.
Q33. What metal is used in the production of stainless steel?
A33. Chromium is used in the production of stainless steel to enhance its corrosion resistance.
Q34. Name a metal that is highly resistant to corrosion and used in aerospace applications.
A34. Titanium is highly resistant to corrosion and is used in aerospace applications due to its strength-to-weight ratio.
Q35. Which metal is used in the production of electrical contacts and connectors?
A35. Silver is used in the production of electrical contacts and connectors due to its superior conductivity.
8. Examples of Non-Metals
Q36. Name a non-metal that is essential for human respiration.
A36. Oxygen is essential for human respiration.
Q37. What non-metal is used in the production of phosphoric acid?
A37. Phosphorus is used in the production of phosphoric acid and fertilizers.
Q38. Which non-metal is a major component of proteins and nucleic acids?
A38. Nitrogen is a major component of proteins and nucleic acids.
Q39. Name a non-metal that is commonly used in the production of bleach.
A39. Chlorine is commonly used in the production of bleach.
Q40. Which non-metal is found in all organic compounds?
A40. Carbon is found in all organic compounds.
9. Reactivity Order of Metals
Q41. What is the general reactivity trend of metals as you move down a group in the periodic table?
A41. The reactivity of metals generally increases as you move down a group in the periodic table.
Q42. Which metal is more reactive: sodium or magnesium?
A42. Sodium is more reactive than magnesium.
Q43. How does the reactivity of alkali metals compare to that of alkaline earth metals?
A43. Alkali metals (Group 1) are more reactive than alkaline earth metals (Group 2).
Q44. What is the reactivity of copper compared to zinc?
A44. Copper is less reactive than zinc.
Q45. Arrange the following metals in order of increasing reactivity: iron, calcium, potassium, and zinc.
A45. The order of increasing reactivity is: iron < zinc < calcium < potassium.
10. Additional Advanced Questions
Q46. Explain why alkali metals are highly reactive.
A46. Alkali metals are highly reactive because they have a single electron in their outermost shell, which they readily lose to achieve a stable noble gas configuration.
Q47. How does the reactivity of transition metals compare to that of alkali metals?
A47. Transition metals are generally less reactive than alkali metals. They have more electrons in their d-orbitals, which makes them less likely to lose electrons compared to alkali metals.
Q48. What is the effect of the atomic radius on the reactivity of metals?
A48. As the atomic radius increases, the reactivity of metals generally increases because the outer electrons are further from the nucleus and more easily lost.
Q49. How does the presence of oxide layers affect the reactivity of metals?
A49. The presence of oxide layers can protect metals from further oxidation and corrosion, reducing their reactivity. For example, aluminum forms a protective oxide layer that prevents further oxidation.
Q50. Why do non-metals like fluorine and chlorine exhibit high reactivity?
A50. Non-metals like fluorine and chlorine exhibit high reactivity because they have high electronegativity and readily gain electrons to achieve a stable noble gas configuration.
Q51. What is the role of non-metals in the formation of covalent bonds?
A51. Non-metals play a crucial role in forming covalent bonds by sharing electrons with other non-metals to achieve full outer electron shells.
Q52. Explain why noble gases are generally non-reactive.
A52. Noble gases are generally non-reactive because they have full outer electron shells, making them stable and less likely to gain or lose electrons.
Q53. How does the ionization energy of non-metals compare to metals?
A53. Non-metals generally have higher ionization energies compared to metals because they have more electrons in their valence shell and are less willing to lose electrons.
Q54. What is the significance of the reactivity series of metals in predicting displacement reactions?
A54. The reactivity series helps predict which metals will displace others in single displacement reactions. A more reactive metal will displace a less reactive metal from its compound.
Q55. How does the presence of multiple oxidation states in transition metals affect their chemical behavior?
A55. The presence of multiple oxidation states in transition metals allows them to participate in various chemical reactions and form different compounds with varying properties.
Here are additional questions and answers covering more detailed aspects of metals and non-metals, their properties, and uses:
11. Detailed Physical Properties of Metals
Q56. What physical property of metals contributes to their use in making jewelry?
A56. The shiny luster of metals contributes to their use in making jewelry, as it provides a visually appealing surface.
Q57. Why are metals generally used in construction materials?
A57. Metals are used in construction materials due to their strength, durability, and ability to withstand high stresses and loads.
Q58. How does the malleability of metals benefit their use in manufacturing?
A58. Malleability allows metals to be shaped into various forms without breaking, making them useful for manufacturing items such as sheets, foils, and components.
Q59. What is the significance of the high melting and boiling points of metals?
A59. The high melting and boiling points of metals make them suitable for high-temperature applications, such as in machinery and industrial processes.
Q60. How does the thermal conductivity of metals affect their use in heat exchangers?
A60. The high thermal conductivity of metals allows efficient heat transfer, making them ideal for use in heat exchangers and cooling systems.
12. Detailed Physical Properties of Non-Metals
Q61. Why are non-metals typically poor conductors of heat?
A61. Non-metals are poor conductors of heat because they lack free-moving electrons or ions to transfer thermal energy efficiently.
Q62. How does the brittleness of non-metals affect their use in manufacturing?
A62. The brittleness of non-metals means they can break or shatter under stress, limiting their use in applications where flexibility and durability are required.
Q63. What role does the low density of non-metals play in their applications?
A63. The low density of non-metals, such as gases and certain solids, makes them useful for applications where weight is a critical factor, such as in lightweight materials and packaging.
Q64. How do the colors of non-metallic substances, like iodine and bromine, influence their uses?
A64. The colors of non-metallic substances, such as iodine (purple) and bromine (red-brown), can be used for identification and in applications such as dyes and indicators.
Q65. Why are non-metals like oxygen and nitrogen used in cryogenic applications?
A65. Non-metals like oxygen and nitrogen are used in cryogenic applications due to their low boiling points, which allow them to be stored and transported in liquid form for various industrial processes.
13. Detailed Chemical Properties of Metals
Q66. How do metals typically react with halogens?
A66. Metals react with halogens to form metal halides. For example, sodium reacts with chlorine to form sodium chloride.
Q67. What is the role of metal oxides in rusting?
A67. Metal oxides, such as iron(III) oxide (rust), form when metals react with oxygen and moisture, leading to corrosion and deterioration of the metal.
Q68. How do metals react with water at different temperatures?
A68. Metals react with water at different rates depending on temperature. Alkali metals react vigorously with cold water, while less reactive metals like iron may react more slowly or require higher temperatures.
Q69. What is the general trend in the reactivity of transition metals with acids?
A69. Transition metals generally show less reactivity with acids compared to alkali metals. They may react slowly or require specific conditions to react.
Q70. How do metal-carbonate reactions vary among different metals?
A70. Metals react with carbonates to form metal oxides, carbon dioxide, and water. The reactivity varies, with some metals reacting more readily than others. For example, calcium carbonate decomposes easily when heated.
14. Detailed Chemical Properties of Non-Metals
Q71. How do non-metals form acidic oxides?
A71. Non-metals form acidic oxides when they react with oxygen. These oxides dissolve in water to form acids. For example, sulfur dioxide reacts with water to form sulfurous acid.
Q72. What is the reaction between a non-metal oxide and a base?
A72. Non-metal oxides react with bases to form salts and water. For instance, carbon dioxide reacts with sodium hydroxide to form sodium carbonate and water.
Q73. How do non-metals participate in redox reactions?
A73. Non-metals participate in redox reactions by gaining electrons (reduction) and forming negative ions or oxides. For example, chlorine gains electrons to form chloride ions.
Q74. What is the reactivity of nitrogen with other elements?
A74. Nitrogen is relatively unreactive due to the strong triple bond in N₂. However, it can react with metals under high temperatures to form nitrides, such as with lithium to form lithium nitride.
Q75. How do non-metal halides behave in water?
A75. Non-metal halides, such as hydrogen chloride (HCl), dissolve in water to form acidic solutions. For example, HCl forms hydrochloric acid when dissolved in water.
15. Detailed Uses of Metals
Q76. Why is gold used in electronics beyond its conductivity?
A76. Gold is used in electronics not only for its conductivity but also for its resistance to corrosion and tarnish, ensuring reliable and long-lasting connections.
Q77. How does the use of titanium benefit the aerospace industry?
A77. Titanium is used in the aerospace industry due to its high strength-to-weight ratio, corrosion resistance, and ability to withstand high temperatures, making it ideal for aircraft and spacecraft components.
Q78. What are the applications of zinc in everyday products?
A78. Zinc is used in everyday products such as galvanized steel (for corrosion protection), batteries, and as a dietary supplement.
Q79. How is magnesium used in the automotive industry?
A79. Magnesium is used in the automotive industry to produce lightweight components, such as wheels and engine parts, to improve fuel efficiency and performance.
Q80. What role does silver play in photography?
A80. Silver halides, such as silver bromide, are used in photographic film and paper for their light-sensitive properties, crucial for capturing images.
16. Detailed Uses of Non-Metals
Q81. How does chlorine contribute to public health?
A81. Chlorine is used to disinfect drinking water and swimming pools, killing bacteria and other pathogens to ensure water safety and prevent disease.
Q82. What is the significance of nitrogen in fertilizers?
A82. Nitrogen is a key component of fertilizers, such as ammonium nitrate and urea, which enhance plant growth by providing essential nutrients.
Q83. How is carbon used in environmental applications?
A83. Carbon, in the form of activated carbon, is used in environmental applications for water and air purification, as it adsorbs contaminants and pollutants.
Q84. What are the applications of fluorine in industrial processes?
A84. Fluorine is used in the production of fluorinated compounds, such as refrigerants, Teflon coatings, and in uranium processing for nuclear fuel.
Q85. How is sulfur used in the manufacture of rubber?
A85. Sulfur is used in the vulcanization process of rubber to improve its elasticity, strength, and durability, making it suitable for tires and other rubber products.
17. Reactivity Series and Trends
Q86. How does the reactivity series predict the outcome of a displacement reaction?
A86. The reactivity series predicts that a more reactive metal will displace a less reactive metal from its compound in a displacement reaction. For example, zinc will displace copper from copper sulfate.
Q87. What factors influence the position of metals in the reactivity series?
A87. The position of metals in the reactivity series is influenced by their ability to lose electrons and form positive ions, as well as their reactions with water, acids, and oxygen.
Q88. How does the reactivity of alkali metals compare with alkaline earth metals in terms of reactivity with water?
A88. Alkali metals are more reactive with water compared to alkaline earth metals. For example, sodium reacts vigorously with water, while calcium reacts less violently.
Q89. Why does the reactivity of metals increase down a group in the periodic table?
A89. The reactivity of metals increases down a group because the outer electrons are further from the nucleus, making them easier to lose and react more readily.
Q90. How does the reactivity of transition metals compare to that of group 1 and group 2 metals?
A90. Transition metals are generally less reactive compared to group 1 and group 2 metals. They have more electrons to lose and form various oxidation states, making them less reactive overall.
18. Advanced Topics
Q91. How does the concept of electronegativity relate to the formation of ionic and covalent bonds?
A91. Electronegativity is a measure of an atom's ability to attract electrons. In ionic bonds, a large difference in electronegativity between metals and non-metals leads to electron transfer, while in covalent bonds, similar electronegativities lead to electron sharing.
Q92. What is the significance of the octet rule in chemical bonding?
A92. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight electrons in their outer shell, similar to noble gases.
Q93. How does the VSEPR theory explain the shape of molecules?
A93. The Valence Shell Electron Pair Repulsion (VSEPR) theory explains that the shape of a molecule is determined by the repulsion between electron pairs around a central atom, which arranges the pairs to minimize repulsion and maximize distance.
Q94. What is hybridization, and how does it affect molecular geometry?
A94. Hybridization is the mixing of atomic orbitals to form new hybrid orbitals, which affects molecular geometry by determining the arrangement of bonds and lone pairs around the central atom.
Q95. How do the principles of quantum mechanics contribute to our understanding of atomic structure?
A95. Quantum mechanics provides a framework for understanding atomic structure by describing electron behavior through quantum numbers, wave functions, and probability distributions, leading to the modern model of electron orbitals and energy levels.
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