Metals and Non-metals Overview
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Metals and Non-metals Overview

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Questions and Answers

What can be inferred about the solubility of ionic compounds in different solvents based on the observed results?

Ionic compounds are generally soluble in water but insoluble in non-polar solvents like kerosene and petrol.

Explain the relationship between the ionic nature of compounds and their melting points.

Ionic compounds have high melting points due to the strong electrostatic forces between positively and negatively charged ions.

How does the electrical conductivity test reveal the properties of ionic compounds in solution?

When dissolved in water, ionic compounds dissociate into ions, which allows the solution to conduct electricity.

Describe the typical physical state and brittleness of ionic compounds.

<p>Ionic compounds are typically solid and brittle due to the rigid structure of the ionic lattice.</p> Signup and view all the answers

What is the significance of the melting and boiling points of ionic compounds, based on the provided data?

<p>The high melting and boiling points indicate that a substantial amount of energy is needed to break the ionic bonds.</p> Signup and view all the answers

Explain why the extraction of metals often requires high temperatures in the process.

<p>Most metals have high melting points, requiring significant heat to separate them from their ores effectively.</p> Signup and view all the answers

Discuss the solubility differences between ionic and non-ionic compounds.

<p>Ionic compounds typically dissolve in polar solvents like water, while non-ionic compounds may not due to lack of charged particles.</p> Signup and view all the answers

What are the general physical properties of ionic compounds regarding electrical conductivity?

<p>Ionic compounds conduct electricity when dissolved in water or molten, as their ions are free to move.</p> Signup and view all the answers

Compare the melting and boiling points of metals with non-metals based on their general properties.

<p>Metals usually have high melting and boiling points, while most non-metals are gases or have low melting points.</p> Signup and view all the answers

What role does the allotrope of carbon play in distinguishing it from typical non-metals?

<p>Carbon exists in allotropes such as diamond and graphite, exhibiting properties like high hardness and electrical conductivity.</p> Signup and view all the answers

Study Notes

Metals and Non-metals

  • Elements are classified as metals or non-metals based on properties.
  • Metals have various uses in daily life, including cooking utensils.
  • Non-metals also have numerous uses, such as in everyday items and in the manufacturing process.
  • Physical properties, like lustre, are used to distinguish between metals and non-metals.

Physical Properties of Metals

  • Metallic Lustre: Metals (in pure form) have a shiny surface.
  • Hardness: Metals are generally hard, but hardness varies between different metals.
  • Malleability: Some metals can be beaten into thin sheets.
  • Ductility: Some metals can be drawn into thin wires.
  • Conductivity: Metals are good conductors of heat and electricity.
  • Sonority: Metals produce a sound when struck.
  • Melting and Boiling Points: Metals generally have high melting and boiling points.

Activities

  • Activity 3.1: Observe the appearance of iron, copper, aluminum and magnesium samples, and their appearance after cleaning them with sandpaper. Metals exhibit a shining surface (metallic lustre).
  • Activity 3.2: Try cutting small pieces of iron, copper, aluminum, and magnesium with a knife and observe the results. Use caution when handling sodium. Note the ability or inability to cut the metals. Observe sodium's reaction.
  • Activity 3.3: Strike pieces of iron, zinc, lead, and copper on a block to observe their behavior and the resulting changes in shape. Record this change.
  • Activity 3.4: List metals used to make wires, demonstrating their ductility.
  • Activity 3.5: Heat a metal wire to observe its response to heat and its properties like melting and conductivity. Does the metal melt?
  • Activity 3.6: Set up an electrical circuit with a metal sample to determine if it is a conductor of electricity. Does the bulb glow?
  • Activity 3.7: Collect samples of carbon (coal or graphite), sulfur, and iodine to investigate their properties—compare and contrast them with metals.
  • Activity 3.8: Burn magnesium ribbon and sulfur powder, observe the results, and determine if the products are acidic or basic.
  • Activity 3.9: Burn different metals in air to see how they react with oxygen. Determine the colors of the flame and the products in different reactions. Observe the metals’ reactions under different conditions
  • Activity 3.10: Investigate reactions of different metals with cold water. Determine which metals react with cold water, and arrange them by their reactivity in increasing order. Note if any metals produce fire with water.
  • Activity 3.11: Investigate reactions of various metals with dilute hydrochloric acid to see how the metals react in different conditions. Note the highest temperature and relative reactivity.
  • Activity 3.12: Observe the reaction between copper wire in iron sulfate solution and iron nail in copper sulfate solution. Determine if displacement reaction occurs. Identify the more reactive metal.

Chemical Properties of Metals

  • Reaction with Oxygen: Most metals react with oxygen to form metal oxides.
  • Reaction with Water: Some metals react violently with cold water, and others react with hot water or steam.
  • Reaction with Acids: Most metals react with dilute acids to produce hydrogen gas, and a corresponding salt. Some metals don't react.
  • Reactivity Series: This arranges metals based on their reactivity according to their reactions with acids and water, and how they displace other metals.
    • High reactivity metals strongly react with water and acids.
    • Low reactivity metals minimally react with water and acids.
  • Displacement Reaction: A more reactive metal can displace a less reactive metal from its salt solution.

Ionic Compounds

  • Physical Nature: Ionic compounds are usually solids, hard, and often brittle.
  • Melting and Boiling Points: Ionic compounds usually have high melting and boiling points.
  • Solubility: Many ionic compounds dissolve in water but not in other solvents.
  • Electrical Conductivity: Ionic compounds conduct electricity when melted or dissolved in water. (In solid state, they don't).

Corrosion

  • Rusting: Iron reacts with moist air (water vapor and oxygen) to form rust (iron oxide).
  • Conditions for rusting include the presence of both oxygen and water.
  • Prevention of Corrosion: Methods include painting, oiling, greasing, galvanizing and alloying.

Extraction of Metals

  • Ores: Minerals that contain high concentrations of a metal.
  • Gangue: Impurities in ores that must be removed.
  • Methods for extracting metals: Methods vary based on a metal's reactivity in a reactivity series.
    • Calcination
    • Roasting
    • Reduction
    • Electrolysis

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Metals and Non-Metals PDF

Description

This quiz explores the classification of elements into metals and non-metals according to their physical properties. Engage with various activities that highlight the characteristics and applications of these elements in daily life and industry. Test your understanding of key concepts like metallic lustre and conductivity.

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