Chemistry Class Quiz: Mixtures and Reactions
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Questions and Answers

What is the purpose of centrifugation in the separation of mixtures?

  • To directly combine components of the mixture
  • To crystallize components at a higher temperature
  • To speed up the setting process of a precipitate (correct)
  • To increase the temperature in the mixture

    • Which property classification is dependent on mass?

  • Density
  • Volume (correct)
  • Color
  • Melting Point

    • An example of a physical change is:

  • Rust formation on iron
  • Baking bread
  • Burning wood
  • Dissolving sugar in water (correct)

    • Which of the following is an indication of a chemical change?

    <p>Emission of light</p> Signup and view all the answers

    What type of reaction is represented by the equation AB + C ---- AC + B?

    <p>Single Displacement Reaction</p> Signup and view all the answers

    During which process is heat absorbed or liberated?

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

    What is the product of saponification?

    <p>Soap and glycerol</p> Signup and view all the answers

    Which of the following is NOT a type of chemical reaction?

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

    Which of the following elements is produced artificially?

    <p>Technetium (Tc)</p> Signup and view all the answers

    What is the common feature of liquids at room temperature?

    <p>They have indefinite shape but definite volume.</p> Signup and view all the answers

    What determines the solubility of a substance in a solvent?

    <p>'Like dissolves like' principle.</p> Signup and view all the answers

    Which group contains alkaline metals?

    <p>Group I A</p> Signup and view all the answers

    What is the primary distinction between mass and weight?

    <p>Mass does not change with gravity, while weight does.</p> Signup and view all the answers

    Which of the following best describes a compound?

    <p>A substance where two or more elements are chemically combined.</p> Signup and view all the answers

    Which statement is true about an unsaturated solution?

    <p>It contains less solute than the saturated solution.</p> Signup and view all the answers

    What effect does temperature have on gas solubility?

    <p>Increasing temperature decreases gas solubility.</p> Signup and view all the answers

    What characterizes a mixture in relation to its components?

    <p>Components maintain their individual chemical properties.</p> Signup and view all the answers

    How is weight calculated according to the given information?

    <p>Weight = mass x acceleration due to gravity</p> Signup and view all the answers

    What type of solution contains more solute than can be dissolved in it?

    <p>Supersaturated solution</p> Signup and view all the answers

    Which block of the periodic table do transition metals occupy?

    <p>D block</p> Signup and view all the answers

    Which of the following correctly defines matter?

    <p>Anything that occupies space and has mass.</p> Signup and view all the answers

    What is the most abundant state of matter in the universe?

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

    Which of the following describes a colloid?

    <p>Particles that are evenly suspended but not broken down to molecular size</p> Signup and view all the answers

    What physical phenomena most strongly affects plasma?

    <p>Magnetic Field</p> Signup and view all the answers

    Which process separates components of a mixture based on differences in density?

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

    What is an example of a homogeneous mixture?

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

    Which is the correct conversion formula to find Celsius from Fahrenheit?

    <p>C = 5/9 (F - 32)</p> Signup and view all the answers

    What distinguishes a suspension from a solution?

    <p>Suspension contains insoluble solids, solutions do not</p> Signup and view all the answers

    Which state of matter is associated with high enthalpy?

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

    How does increasing pressure affect the solubility of a gas?

    <p>It increases the solubility of gases.</p> Signup and view all the answers

    What is the effect of decreasing particle size on solubility?

    <p>It increases solubility due to greater surface area.</p> Signup and view all the answers

    What is the common ion effect?

    <p>It decreases solubility of certain compounds due to the presence of a common ion.</p> Signup and view all the answers

    Which intermolecular force is primarily responsible for attraction between polar molecules?

    <p>Hydrogen bonds.</p> Signup and view all the answers

    Which of the following statements about intramolecular forces is correct?

    <p>Covalent bonds can be both polar and nonpolar.</p> Signup and view all the answers

    What characterizes colligative properties?

    <p>They depend on the total number of solute particles in a solution.</p> Signup and view all the answers

    Which intermolecular force involves a charged ion and a polar molecule?

    <p>Ion-dipole forces.</p> Signup and view all the answers

    What is meant by 'salting in' and 'salting out' in terms of solubility?

    <p>Salting out refers to the presence of salts decreasing solubility, while salting in refers to salts increasing solubility.</p> Signup and view all the answers

    What effect does the addition of a non-volatile solute have on the vapor pressure of a liquid?

    <p>It lowers the vapor pressure of the liquid.</p> Signup and view all the answers

    How does the boiling point of a solution compare to that of its pure solvent?

    <p>It is higher than the boiling point of the pure solvent.</p> Signup and view all the answers

    What is the definition of freezing point depression?

    <p>The temperature at which a solution has a lower freezing point than the pure solvent.</p> Signup and view all the answers

    What is osmosis?

    <p>The movement of water from high to low concentration through a semi-permeable membrane.</p> Signup and view all the answers

    In osmosis, what change occurs in a hypertonic solution?

    <p>Cells shrink or undergo crenation.</p> Signup and view all the answers

    What does Boyle's Law describe?

    <p>The relationship between pressure and volume of a gas at a constant temperature.</p> Signup and view all the answers

    What is the ideal gas law equation?

    <p>PV = nRT</p> Signup and view all the answers

    Which of the following describes Gay-Lussac's Law?

    <p>P1/T1 = P2/T2</p> Signup and view all the answers

    Study Notes

    Module 1: General Chemistry

    • Chemistry is the study of matter
    • Matter is anything that occupies space and has mass
    • Mass refers to the amount of matter present in a material or object

    Classification of Matter

    • Element - simplest form, one component
    • Compound - two or more elements (chemically combined)
    • Mixture - two or more substances (not chemically combined)

    States of Matter

    • Solid: Definite shape and size, definite volume, vibration
    • Liquid: Indefinite shape, definite volume (assumes the shape of the container), gliding motion
    • Gas: Indefinite shape and volume, constant random motion

    Units of Measurement

    • Length - Meter (m)
    • Mass - Kilograms (kg)
    • Time - Seconds (sec)
    • Temperature - Kelvin (K)

    Classification of Mixtures

    • Homogeneous: One phase (e.g., solutions)
    • Heterogeneous: Two or more phases (e.g., suspensions, colloids)
      • Solution: uniform mixture (solute + solvent)
      • Suspension: coarse mixture (finely divided solid materials dispersed in a liquid)
      • Colloid: particle of solute not broken down to the size of molecules

    Process of Separating Components of Mixtures

    • Decantation - difference in specific gravity/density
    • Distillation - evaporation and condensation
    • Evaporation - separation by evaporation
    • Magnetic Separation
    • Filtration

    Continuation of Mixture Separation Process

    • Sorting
    • Centrifugation - speed up the setting process of a precipitate
    • Fractional Crystallization - lowering the temperature to separate based on differences in solute affinity
    • Chromatography - separating based on differences in solute affinity

    Properties of Matter

    • Intrinsic: Intensive property, independent of mass/amount (e.g., density, specific gravity, melting point, viscosity, temperature, color)
    • Extrinsic: Extensive property, dependent on mass (e.g., weight, volume, pressure, heat content, length, mass/cot, entropy, enthalpy, electrical resistance)

    Changes that Matter Undergoes

    • Physical Change: Change in phase (e.g., sublimation, deposition)
    • Chemical Change: Change in both intrinsic and extrinsic properties (e.g., evolution of gas, formation of precipitate, emission of light, generation of electricity, production of mechanical energy, absorption/liberation of heat)

    Types of Chemical Reactions

    • Combination/Synthesis - A + B → AB
    • Decomposition/Analysis - AB → A + B
    • Single Displacement/Single Replacement - AB + C → AC + B
    • Double Displacement - AB + CD → AC + BD
      • Neutralization: Acid + Base → Salt + Water

    Processes Involved in Chemical Change

    • Oxidation - + oxygen
    • Reduction - oxygen or + hydrogen
    • Neutralization - Acid + Base → Salt + Water
    • Hydrolysis - Water + Salt → Acid + Base
    • Saponification - Alkali + Fat → Soap + Glycerol
    • Fermentation - Organic substances + Microbes → Alcohol

    Nuclear Change

    • Nuclear Fission - splitting of a heavy atom
    • Nuclear Fusion - union of two light atoms to form a bigger molecule

    Atomic Structure

    • Protons = electrons = atomic number
    • Neutrons= mass number - atomic number
    • Electrons= protons - charge
    • Mass number = protons + neutrons

    General Principles in Electron Configuration

    • Pauli's Exclusion Principle - no two electron shall have the same set of quantum numbers. Each atomic orbital can only accommodate 2 electrons.
    • Heisenberg's Uncertainty Principle - impossible to simultaneously determine the electron momentum and position.
    • Aufbau's Building Up Principle - lower energy levels are filled up first.
    • Hund's Rule of Maximum Multiplicity - orbitals are filled singly before pairing up.

    Fundamental Chemistry Laws

    • Law of Conservation of Mass/Matter - Mass/Matter cannot be created or destroyed
    • Law of Definite/Constant Proportions - Chemical compounds always contain the exact proportion of elements in fixed ratios by mass
    • Law of Multiple Proportions
    • Law of combining weights

    Useful Trivias SA Board Exam

    • 3 most abundant elements - O, Si, Al
    • 1st element produced artificially - Tc= technetos
    • Rarest element - At = Astatin
    • Liquid at room temperature - Hg/Br

    The Periodic Table of Elements

    • (Provides a table of elements with organization by properties)

    Family A & B Elements

    • Family A: Representative elements arranged in the S and P blocks
    • Family B: Transition Elements arranged in the D and F Blocks
      • D block - Transition metals
      • F block - Lanthanides/Actinides
    • Atomic Radius
    • lonization Energy
    • Electron Affinity
    • Nonmetallic character
    • Metallic Character

    Kinematic Molecular Theory

    • Explains the phases of matter based on the movement of molecules/ions/atoms
      • Solid
      • Liquid
      • Gas

    Solutions

    • Homogeneous mixture of two or more substances (single phase)
      • Saturated- maximum solute
      • Unsaturated - less solute
      • Supersaturated - more solute than solvent

    Factors Affecting Solubility

    • Nature of Solute and Solvent ("like dissolves like")
    • Temperature
      • Exothermic - solubility decreases with increasing temperature
      • Endothermic - solubility increases with increasing temperature
    • Pressure (for gases only) - solubility increases with increasing pressure
    • Particle Size/Surface Area - increased surface area leads to increased solubility
    • Presence of Salts (salting out/ in)- presence of salt decreases/increases solubility with common ion effect

    Forces of Attraction

    • Intramolecular Forces (within molecules)
      • Ionic - electron transfer
      • Covalent - electron sharing (polar/nonpolar)
    • Intermolecular Forces (between molecules)
    • Van der Waals forces
      • Keesom - dipole-dipole
      • Debye - dipole-induced dipole
      • London Dispersion Forces- induced dipole-induced dipole
      • Ion-dipole
      • Hydrogen Bond

    Physical Properties of Systems

    • Additive Property- depends on the sum (molecular weight)
    • Constitutive Property- depends on type/arrangement (optical rotation)
    • Colligative Property- depends on the number of solute particles (e.g., vapor pressure lowering, boiling point elevation, freezing point depression. osmotic pressure)

    Colligative Properties

    • Vapor Pressure Lowering
    • Boiling Point Elevation
    • Freezing Point Depression
    • Osmotic Pressure

    Gas Laws

    • Boyle's/Mariotte Law - P1V1 = P2V2
    • Charles Law - V1/T1 = V2/T2
    • Gay-Lussac's Law - P1/T1 = P2/T2
    • Combined Gas Law - P1V1/T1 = P2V2/T2
    • Ideal Gas Law
    • Avogadro's Law - V1/n1 = V2/n2
    • Dalton's Law of Partial Pressures - Pt = P1 + P2 + P3
    • Graham's Law - Rate diffusion = 1/(square root of density)
    • Fick's 1st Law

    Acids and Bases

    • Electrolytes (good conductors)
      • Strong electrolytes
      • Weak electrolytes
    • Non-Electrolytes (do not conduct electricity)
    • Acid-Base Theories (Arrhenius, Bronsted-Lowry, Lewis, Pearson's HSAB)
    • Acids (taste sour. pH<7, turn litmus paper red)
    • Bases (taste bitter, pH>7, turn litmus paper blue)
    • Acid-Base Concepts (Pearson's HSAB)

    Buffers

    • Resist pH changes when acids or bases are added
    • Consist of a weak acid and its conjugate base or weak base and its conjugate acid
    • Henderson-Hasselbalch Equation
    • Buffer Capacity

    Thermochemistry

    • Heat (q) - energy transfer due to temperature difference
    • Work (w) - energy transfer between a system and its surroundings (compression/expansion of gas)
    • Internal Energy (U)
    • Enthalpy (H) - energy of a reaction
    • Entropy (S) - degree of disorderliness
    • Heat Capacity (c)
    • Specific Heat
    • Endothermic - absorbs heat, positive heat value
    • Exothermic - releases heat, negative heat value
    • Thermodynamically Spontaneous reactions: -H and +S; otherwise -H and -S
    • Le Chatelier's Principle - a system in equilibrium will shift to relieve stress

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    Description

    Test your knowledge of fundamental chemistry concepts, including the properties of mixtures, physical and chemical changes, and the classification of reactions. This quiz covers essential topics such as saponification, solubility, and the characteristics of elements and compounds.

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