States of Matter and Kinetic Theory
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Questions and Answers

What happens to the solubility of a substance as temperature increases?

  • Solubility only increases for gases
  • Solubility decreases for all substances
  • Solubility generally increases (correct)
  • Solubility remains constant

    • A solvent is a substance that dissolves in another substance.

    False

    What is the term used to describe a solution where no more solute can dissolve?

    saturated solution

    As the temperature increases, the solubility of solid substances generally __________.

    <p>increases</p> Signup and view all the answers

    What occurs during oxidation?

    <p>Gain of oxygen</p> Signup and view all the answers

    Metals that can be extracted by reduction with carbon include aluminum.

    <p>False</p> Signup and view all the answers

    What is the main source of aluminum ore?

    <p>Bauxite</p> Signup and view all the answers

    The reaction that occurs during the extraction of iron includes coke as a __________ agent.

    <p>reducing</p> Signup and view all the answers

    Match the extracted metals to their extraction methods:

    <p>Aluminum = Electrolysis Zinc = Reduction Iron = Blast furnace Sodium = Electrolysis</p> Signup and view all the answers

    Which of the following metals is more active than carbon?

    <p>Aluminum</p> Signup and view all the answers

    Weak metals like copper can undergo reactions with steam.

    <p>False</p> Signup and view all the answers

    Name one compound that can be used in displacement reactions.

    <p>Copper Sulphate</p> Signup and view all the answers

    What process occurs when gas particles cool and transition to a liquid?

    <p>Condensation</p> Signup and view all the answers

    A mixture cannot be separated by physical processes.

    <p>False</p> Signup and view all the answers

    What is the process called when a solid changes directly to a gas?

    <p>Sublimation</p> Signup and view all the answers

    A pure substance has a definite melting point and __________.

    <p>boiling point</p> Signup and view all the answers

    Match the following processes with their definitions:

    <p>Evaporation = Transition from liquid to gas Condensation = Transition from gas to liquid Sublimation = Transition from solid to gas Diffusion = Spreading of particles from high to low concentration</p> Signup and view all the answers

    Which of these statements is true about impurities in a substance?

    <p>They lower the melting point of the substance.</p> Signup and view all the answers

    All solid substances will melt into liquids before changing into gases.

    <p>False</p> Signup and view all the answers

    What can increase the rate of diffusion?

    <p>Increase in temperature</p> Signup and view all the answers

    Which of the following salts are soluble?

    <p>Silver Nitrate</p> Signup and view all the answers

    All sulfate salts are soluble regardless of their composition.

    <p>False</p> Signup and view all the answers

    What is the formula for the nitrate ion?

    <p>NO3-1</p> Signup and view all the answers

    Group 7 salts are soluble except when they are combined with _____ or _____ which make them solid.

    <p>Ag, Pb</p> Signup and view all the answers

    Match the following ions with their valency:

    <p>Ammonium = +1 Sulfate = -2 Nitrate = -1 Carbonate = -2</p> Signup and view all the answers

    Which of the following statements regarding insoluble salts is true?

    <p>Carbonates are insoluble except with group 1 or ammonium.</p> Signup and view all the answers

    The formula for a molecule of chlorine gas is Cl.

    <p>False</p> Signup and view all the answers

    What should be done to write the formula for an ionic compound?

    <p>Swap valences</p> Signup and view all the answers

    What is the primary characteristic of strong acids?

    <p>Completely ionized</p> Signup and view all the answers

    Weak acids fully ionize in solution.

    <p>False</p> Signup and view all the answers

    What is formed when an acid reacts with a base?

    <p>salt and water</p> Signup and view all the answers

    The pH range of weak acids is __________.

    <p>4-6</p> Signup and view all the answers

    Match the following indicators with their corresponding pH results:

    <p>Litmus Solution = Red for acid, Blue for base Methyl Orange = Red in acid, Yellow in neutral/alkaline Phenol Phtalein = Colorless in acid, Pink in base Universal Indicator = Violet in strong base, Dark Red in strong acid</p> Signup and view all the answers

    Which of the following describes a base?

    <p>Proton acceptor</p> Signup and view all the answers

    Titration is the method used to prepare soluble salts from group I and ammonium.

    <p>True</p> Signup and view all the answers

    What occurs during the neutralization reaction between an acid and a base?

    <p>Proton transfer</p> Signup and view all the answers

    What is the first step in preparing a sample of copper sulfate from sulfuric acid and copper (II) oxide?

    <p>Add 25cm of sulfuric acid using a pipette</p> Signup and view all the answers

    The empirical formula represents the actual number of atoms in a molecule.

    <p>False</p> Signup and view all the answers

    What is the resulting insoluble salt formed when lead(II) nitrate reacts with sodium chloride?

    <p>Lead(II) chloride (PbCl2)</p> Signup and view all the answers

    To find the molecular formula from the empirical formula, we need to calculate the ______ factor.

    <p>enlargement</p> Signup and view all the answers

    Match the following chemical components with their corresponding roles or formulas:

    <p>Sulfuric Acid = H2SO4 Copper(II) Oxide = CuO Lead(II) Nitrate = Pb(NO3)2 Sodium Chloride = NaCl</p> Signup and view all the answers

    Which formula correctly represents percent yield?

    <p>(actual amount / theoretical amount) x 100</p> Signup and view all the answers

    In the preparation of insoluble salts, the solid formed can be separated by filtration.

    <p>True</p> Signup and view all the answers

    What is the molecular formula if the empirical formula is CH3 and its relative formula mass is 45?

    <p>C3H9</p> Signup and view all the answers

    Signup and view all the answers

    Study Notes

    State of Matter

    • Properties of Solids, Liquids, and Gases:
      • Compressibility: Solids are difficult to compress, liquids are difficult to compress, and gases are easy to compress.
      • Molecular Packing: Solids have very close packing, liquids have close packing, and gases have widely separated molecules.
      • Shape: Solids have a fixed shape, liquids take the shape of their container, and gases take the shape of their container.
      • Molecular Movement: Solids vibrate in their position, liquids move relatively freely to take the shape of the container, and gases move freely.
      • Attraction Force: Solids have very strong attraction force, liquids have relatively strong forces, and gases have very weak forces.
      • Diffusion: Solids diffuse very slowly, liquids diffuse slowly, and gases diffuse rapidly.

    The Kinetic Theory and Change of State

    • Kinetic Theory Points:

      • All matter is made up of tiny particles (atoms or molecules).
      • The particles are in constant motion.
      • The higher the temperature, the higher the average energy of the particles.

    • Change of States:

      • Melting (Solid to Liquid): When a solid is heated, particles gain kinetic energy, vibrate more, move apart, and the solid melts into a liquid. The melting point is the temperature at which this happens.
      • Boiling (Liquid to Gas): When a liquid is heated, particles gain more kinetic energy, move faster, and overcome attraction forces, escaping into the gaseous phase. This occurs at a constant temperature, the boiling point.
      • Condensation (Gas to Liquid): As gas particles cool, they lose kinetic energy, move slower, and eventually come together to form a liquid state.
      • Freezing (Liquid to Solid): As a liquid cools, particles lose kinetic energy, move more slowly, attraction forces become stronger, and the liquid becomes a solid.
      • Sublimation (Solid to Gas): Some solids change directly into a gas without becoming a liquid when heated. This is called sublimation.

    Comparison Between Compound and Mixture

    • Compound:
      • Formed of two or more elements in a fixed composition chemically bonded.
      • Made through a chemical reaction.
      • Cannot be separated by physical processes, a chemical reaction is required.
      • Has new properties different from its elements.
    • Mixture:
      • Formed of elements or compounds in any composition, not chemically bonded.
      • Made without a chemical reaction.
      • Components can be separated by physical processes.
      • Has the properties of its components.

    Separation of Mixtures

    • Solid-Solid:
      • Salt and Sand: Dissolve salt in water, filter the mixture.
    • Solid-Liquid:
      • Insoluble Solid in Liquid: Use filtration.
      • Soluble Solid in Liquid: Use crystallization or distillation.
    • Mixture of Liquids:
      • Miscible Liquids: Use fractional distillation.
      • Immiscible Liquids: Use a separating funnel.

    Paper Chromatography

    • Used to separate mixtures of coloured materials.
    • A baseline is drawn on filter paper, a spot of the mixture is placed on the baseline.
    • The paper is placed in a beaker with a small amount of solvent.
    • The solvent rises up the paper, carrying the components of the mixture at different rates.
    • The separated components can be seen as spots on the paper.
    • Rf value (retention factor) is calculated to identify the components.

    Solubility

    • Definition: The amount of a substance (solute) that can dissolve in a given amount of solvent (usually water).
    • Factors Affecting Solubility:
      • Temperature: Solubility increases as temperature increases (for most solids).
      • Pressure: Solubility increases as pressure increases (for gases).
    • Solubility Curves: Graphs showing the relationship between the solubility of a substance and temperature.

    Solute and Solvent

    • Solute: The substance being dissolved.
    • Solvent: The substance doing the dissolving.

    Extraction of Metals

    • Different metals are extracted in different ways, depending on their reactivity.
    • Electrolysis: Used for highly reactive metals (e.g., aluminum).
    • Reduction: Used for less reactive metals (e.g., iron).

    Extraction of Iron

    • Iron is extracted from its ore by reducing it with carbon monoxide in a blast furnace.
      • Raw materials include iron ore, coke, limestone, and air.
      • The blast furnace produces molten iron that is further processed to make steel.

    Making Steel

    • Unwanted impurities are removed from molten iron to create steel.
    • Different types of steel exist (mild/low carbon, high carbon, stainless steel) based on carbon content and added elements.
    • Steel is stronger and more resistant to corrosion.

    Rusting of Iron

    • Rusting is an oxidation reaction of iron and oxygen in the presence of water.
    • Rust is hydrated iron(III) oxide.
    • Prevention methods include painting, oiling, and galvanizing.

    Acids and Bases

    • Acids: Proton donors (H+ ions). Sour taste, corrosive, turn blue litmus red.
    • Bases: Proton acceptors (OH- ions). Bitter taste, soapy feel, turned red litmus blue.
    • Neutralization: Reaction between an acid and a base to form a salt and water.
    • Indicators: Substances that change color depending on the pH of the solution.
    • pH scale measures acidity/basicity.
      • pH 1-3: Strong acid
      • pH 4-6: Weak acid
      • pH 7: Neutral
      • pH 8-14: Base

    Titration

    • Method to determine the concentration of an unknown acid or base solution using a known concentration of another reagent.
    • Done using a burette and an indicator.
    • A known amount of one solution dispensed from a burette to reach the endpoint (colour change of the indicator).
    • This point shows equal amounts of reactants, thus the unknown concentration can be calculated.

    Precipitation

    • Method to prepare insoluble salts by combining two or more soluble salts in a solution.
    • Insoluble salt formed precipitates.
    • This can be used to identify substances in a solution.

    Calculations

    • Moles:
      • Moles = Mass (g) / Mr
      • Moles = Concentration (mol/dm^3) x Volume (dm^3)
    • Empirical Formula: Ratio of elements in the simplest whole number form.
    • Molecular Formula: Actual number of atoms of each element in a compound.

    Percentage Yield

    • Percentage yield is a measure of the efficiency of a chemical reaction.
    • It is calculated by dividing the actual yield of a product by the theoretical yield (expected yield) of the product and multiplying by 100.

    Energy Changes

    • Exothermic Reactions: Release more energy than absorbed (energy out).
    • Endothermic Reactions: Absorb more energy than released (energy in).

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    EDEXCEL Chemistry Revision Notes PDF

    Description

    Test your knowledge on the properties of solids, liquids, and gases, as well as the principles of kinetic theory. This quiz covers key concepts such as compressibility, molecular movement, and state changes. Perfect for understanding the fundamental concepts in chemistry.

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