Chemistry: Matter and Particle Theory
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Questions and Answers

What is the mass number of an atom with 12 protons and 14 neutrons?

  • 12
  • 14
  • 28
  • 26 (correct)

    • The Bohr-Rutherford model of the atom depicts electrons orbiting the nucleus in circular paths.

    True (A)

    What is the main difference between a cation and an anion?

    A cation is a positively charged ion formed by losing electrons, while an anion is a negatively charged ion formed by gaining electrons.

    The ______ rule states that atoms tend to gain or lose electrons to achieve a full valence orbital of 8 electrons.

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

    Match the following terms with their corresponding definitions:

    <p>Valence electrons = Electrons in the outermost orbital involved in chemical reactions Alkali metals = Group 1 elements Halogens = Group 17 elements Noble gases = Group 18 elements, known for their stability due to full valence orbitals Ionic bond = Attraction between oppositely charged ions that holds ionic compounds together</p> Signup and view all the answers

    Which of the following elements tends to gain electrons in chemical reactions?

    <p>Oxygen (O) (D)</p> Signup and view all the answers

    Ionic compounds generally dissolve in water, forming electrolytes.

    <p>True (A)</p> Signup and view all the answers

    Explain the concept of the criss-cross method for determining ionic formulas.

    <p>The criss-cross method involves exchanging the numerical values of the charges of the ions to determine the subscripts in the ionic formula.</p> Signup and view all the answers

    The ionic compound formed between potassium and bromine is called ______.

    <p>potassium bromide</p> Signup and view all the answers

    What is the general pattern for a double displacement reaction?

    <p>AB + CD -----&gt; AD + CB (C)</p> Signup and view all the answers

    A single displacement reaction involves the reaction of one compound and one element.

    <p>True (A)</p> Signup and view all the answers

    What is the name of the process where a hydrocarbon reacts rapidly with oxygen, producing carbon dioxide, water, and energy?

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

    The presence of limited oxygen during combustion leads to ______ combustion, which produces carbon monoxide and soot.

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

    Which of the following is NOT a product of incomplete combustion of hydrocarbons?

    <p>Nitrogen dioxide (NO2) (D)</p> Signup and view all the answers

    What is the chemical formula for methane?

    <p>CH4</p> Signup and view all the answers

    Carbon monoxide is a colorless, odorless, and toxic gas produced by complete combustion.

    <p>False (B)</p> Signup and view all the answers

    Match the following terms with their correct definitions:

    <p>Corrosion = The breakdown of a metal due to chemical reactions with the environment Rusting = Corrosion specific to iron-containing metals Galvanizing = A method of preventing corrosion by coating steel with zinc Electrolyte = A substance that conducts electricity when dissolved in water Protective coating = A layer applied to a material to prevent corrosion</p> Signup and view all the answers

    Which of the following is NOT a method for preventing corrosion?

    <p>Applying heat to the metal surface (A)</p> Signup and view all the answers

    Acids release ______ ions when dissolved in water, giving them their acidic properties.

    <p>H+</p> Signup and view all the answers

    What is the chemical formula for hydrochloric acid?

    <p>HCl (A)</p> Signup and view all the answers

    Acids taste bitter and react with metals to produce hydrogen gas.

    <p>False (B)</p> Signup and view all the answers

    What is the chemical formula for carbon dioxide?

    <p>CO2</p> Signup and view all the answers

    Acids react with carbonates to produce ______ gas.

    <p>carbon dioxide</p> Signup and view all the answers

    The combustion of hydrogen is a decomposition reaction.

    <p>False (B)</p> Signup and view all the answers

    What is the chemical formula for aluminum oxide?

    <p>Al2O3</p> Signup and view all the answers

    Which of the following is a pro of using hydrogen gas as an energy source?

    <p>Burns cleanly (B)</p> Signup and view all the answers

    What is the primary method of distinguishing between a pure substance and a mixture?

    <p>Types of particles (C)</p> Signup and view all the answers

    Particles in matter move slower at higher temperatures.

    <p>False (B)</p> Signup and view all the answers

    What are the three subatomic particles found in an atom?

    <p>Proton, Electron, Neutron</p> Signup and view all the answers

    The number of protons in an atom is known as its ___ number.

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

    Match the gas with its corresponding test result:

    <p>Carbon Dioxide (CO2) = Turns clear limewater to cloudy Oxygen Gas (O2) = Fire relights with glowing splint Hydrogen gas = Explosion with a 'pop' sound</p> Signup and view all the answers

    Which of the following is NOT a sign of a chemical change?

    <p>Change in state (A)</p> Signup and view all the answers

    Isotopes have the same number of protons but a different number of neutrons.

    <p>True (A)</p> Signup and view all the answers

    The ability of a substance to conduct electricity is classified as a ___ property.

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

    What is the primary reaction that occurs when sulfur dioxide is released into the atmosphere?

    <p>2SO2(g) + O2(g) ----&gt; 2SO3(g) (C)</p> Signup and view all the answers

    Nitrogen oxides are primarily produced from farming and food production.

    <p>False (B)</p> Signup and view all the answers

    What does a coefficient in a chemical equation represent?

    <p>The number of particles needed for the reaction (A)</p> Signup and view all the answers

    What is the pH range suitable for growing beans?

    <p>7-10</p> Signup and view all the answers

    The buffering capacity of soil is affected by the presence of __________.

    <p>CaCO3</p> Signup and view all the answers

    In a chemical equation, the subscript can be changed to balance the equation.

    <p>False (B)</p> Signup and view all the answers

    What is the general pattern for a synthesis reaction?

    <p>A + B --&gt; AB</p> Signup and view all the answers

    Match the following sources of nitrogen oxides with their percentage contribution:

    <p>Road transportation = 22% Non-road transportation = 29% Industry = 36% Power generation = 10%</p> Signup and view all the answers

    The type of reaction where two compounds swap bonding partners is called a ______ reaction.

    <p>double displacement</p> Signup and view all the answers

    Which of the following impacts on the environment is associated with increased acidity?

    <p>Weakens trees (B)</p> Signup and view all the answers

    What is the main reason acids are good conductors of electricity when dissolved in water?

    <p>They produce ions. (A)</p> Signup and view all the answers

    Match the following types of reactions with their general patterns:

    <p>Synthesis Reaction = A + B --&gt; AB Decomposition Reaction = AB --&gt; A + B Single Displacement = AB + C --&gt; CB + A Double Displacement = AB + CD --&gt; AC + BD</p> Signup and view all the answers

    Over 50% of sulfur dioxide in Ontario originates from Canada itself.

    <p>False (B)</p> Signup and view all the answers

    Which example represents a decomposition reaction?

    <p>2H2O2 --&gt; O2 + 2H2O (C)</p> Signup and view all the answers

    A strong acid has a higher pH value than a weak acid.

    <p>False (B)</p> Signup and view all the answers

    What economic impacts are caused by increased acidity in the environment?

    <p>Higher costs for farming, lumber, and fishing.</p> Signup and view all the answers

    What type of acid is HCl(aq)?

    <p>Binary acid</p> Signup and view all the answers

    Two elements can completely swap their positions in a double displacement reaction.

    <p>True (A)</p> Signup and view all the answers

    The formula for sulfuric acid is __________.

    <p>H2SO4</p> Signup and view all the answers

    What is the purpose of setting up a chart when balancing a chemical equation?

    <p>To show the number of each element for reactants and products.</p> Signup and view all the answers

    During balancing, coefficients multiply the total number of ______ in a compound.

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

    Match the following acids to their corresponding names:

    <p>HCl = Hydrochloric acid H2SO4 = Sulfuric acid HNO3 = Nitric acid HF = Hydrofluoric acid</p> Signup and view all the answers

    What is produced when bases dissolve in water?

    <p>OH- ions (A)</p> Signup and view all the answers

    Identify a characteristic of a balanced equation.

    <p>Atoms are equal on both sides of the equation (C)</p> Signup and view all the answers

    Phenolphthalein turns pink in acidic solutions.

    <p>False (B)</p> Signup and view all the answers

    Which ion is a characteristic of acidic solutions?

    <p>H+</p> Signup and view all the answers

    The pH scale ranges from __________ to __________.

    <p>0, 14</p> Signup and view all the answers

    What happens to water's H+ and OH- ion concentration when a base is added?

    <p>OH- concentration increases. (D)</p> Signup and view all the answers

    Which of the following represents a molecular compound?

    <p>H2O (D)</p> Signup and view all the answers

    All transition metals can form multiple oxidation states.

    <p>False (B)</p> Signup and view all the answers

    What is the chemical formula for ammonium?

    <p>NH4^+</p> Signup and view all the answers

    The polyatomic ion carbonate is represented by the formula ______.

    <p>CO3^2-</p> Signup and view all the answers

    Match the following molecular compounds with their correct names:

    <p>CO = Carbon monoxide SF6 = Sulfur hexafluoride N2O4 = Dinitrogen tetroxide PCl5 = Phosphorus pentachloride</p> Signup and view all the answers

    What is the proper name for the compound NaNO2?

    <p>Sodium Nitrite (C)</p> Signup and view all the answers

    Diatomic molecules consist of two atoms of the same element.

    <p>True (A)</p> Signup and view all the answers

    What do reaction arrows signify in a chemical equation?

    <p>They indicate the conversion of reactants to products.</p> Signup and view all the answers

    The formula for calcium nitrate is ______.

    <p>Ca(NO3)2</p> Signup and view all the answers

    Match the following types of chemical equations:

    <p>Word equation = Uses chemical names Chemical equation = Uses chemical formulas Skeletal equation = Without coefficients Balanced equation = With coefficients</p> Signup and view all the answers

    Which of the following is a diatomic element?

    <p>Fluorine (A)</p> Signup and view all the answers

    Ionic compounds form between non-metals only.

    <p>False (B)</p> Signup and view all the answers

    What prefix indicates three atoms in molecular compound naming?

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

    The correct name for N2O5 is ______.

    <p>Dinitrogen pentoxide</p> Signup and view all the answers

    What happens during a chemical reaction?

    <p>Substances are converted into different substances. (C)</p> Signup and view all the answers

    Study Notes

    Particle Theory

    • All matter is composed of tiny particles.
    • Particles are constantly moving.
    • Particle movement increases with temperature.
    • Particles attract each other.
    • Each pure substance has unique particles.

    Matter Categories

    • Matter is categorized as either pure substances or mixtures.
    • Pure substances are further categorized as elements or compounds.
    • Mixtures can be heterogeneous or homogeneous.

    Physical Properties

    • Clarity
    • Temperature
    • Density
    • Malleability
    • Luster
    • Ductility
    • Color
    • Conductivity
    • State (solid, liquid, gas)
    • Hardness
    • Melting/boiling point
    • Taste
    • Odor
    • Solubility
    • Texture

    Chemical Properties

    • How a substance reacts with other substances.
    • Reaction with acid
    • Combustibility (reaction with oxygen)

    Chemical and Physical Changes

    • Physical change: The substance remains the same.
      • Examples: changes of state, dissolving.
    • Chemical change: A new substance is formed.

    Signs of a Chemical Change

    • Precipitate (solid formed from two solutions)
    • Bubbles/gas/odor
    • Change in color
    • Heat and/or light
    • Usually hard to reverse.

    Gas Tests

    • Physical properties often insufficient to identify gases.
    • Specific gas tests are used.
    Gas Test Result
    Carbon Dioxide Limewater Turns clear solution cloudy
    Oxygen Glowing splint Fire relights
    Hydrogen Flaming splint Explosion with a "pop" sound

    Atomic Structure

    • Proton: Found in the nucleus, +1 charge.
    • Electron: Found in orbitals, -1 charge.
    • Neutron: Found in the nucleus, 0 charge.
    • Atomic number (Z): Number of protons, defines the element.
    • Mass number: Number of protons and neutrons.
    • Isotopes: Atoms of the same element with different numbers of neutrons.
    • Normally, number of protons equals number of electrons.
    • Neutrons: Hold the nucleus together with the strong nuclear force.
    • Unstable nuclei result from too many or too few neutrons.
    • Radioactive atoms result from unstable nuclei.

    Bohr-Rutherford Model

    • Orbitals are rings.
    • First orbital holds 2 electrons.
    • Second orbital holds 8 electrons.
    • Third orbital holds 8 electrons (but can hold 18).

    Valence Electrons

    • Valence electrons are in the outer orbital.
    • Valence electrons determine chemical reactivity.
    • Atoms react to achieve a full valence orbital (octet rule).
    • Atoms with <4 valence electrons tend to lose electrons.
    • Atoms with >4 valence electrons tend to gain electrons.
    • Atoms with 4 valence electrons can either gain or lose electrons.
    • Group numbers correspond to the number of valence electrons (except transition metals).

    Periodic Table Groups

    • Group 1: Alkali Metals
    • Group 2: Alkaline Earth Metals
    • Groups 3-12: Transition Metals
    • Group 17: Halogens
    • Group 18: Noble Gases

    Lewis Diagrams

    • Element symbol in the center, dots for valence electrons.

    Ions

    • An ion is a charged atom (gained/lost electrons).
    • Cation: Positive ion (lost electrons).
    • Anion: Negative ion (gained electrons).
    • Elements tend to gain/lose electrons to achieve full valence shells.
    • Ion charge prediction based on group number (transition metals are exceptions).

    Naming Ions

    • Cations: Element name + "ion".
      • Example: Magnesium ion (Mg²⁺)
    • Anions: Element stem + "ide" + "ion".
      • Example: Chloride ion (Cl⁻)

    Ionic Compounds

    • Formed between metals and nonmetals.
    • Metals form cations, nonmetals form anions.
    • Ionic bond: Attraction between oppositely charged ions.
    • Ionic compounds tend to be hard, brittle, with high melting/boiling points.
    • Crystal structure.
    • Dissolving: Ions separate in water, water molecules surround them.
    • Electrolytes: Dissolve in water to form a solution that conducts electricity.

    Naming Ionic Compounds

    • Metal name followed by nonmetal name (with anion ending)
    • Transition metals use Roman numerals to show ion charge.

    Polyatomic Ions

    • Stable group of atoms acting as a single charged particle.
    • Example: Carbonate (CO³⁻²).
    • Many anions - use brackets for multiple polyatomics.

    Naming and Formulas of Ionic Compounds w/ Polyatomics

    • Element + polyatomic name
    • Polyatomics that have subscripts must use brackets - Example: Calcium Nitrate = Ca(NO₃)₂

    Molecular Compounds

    • Formed between two or more nonmetals.
    • Covalent bonds: Electrons are shared.
    • Lower melting/boiling points than ionic compounds.
    • Usually do not dissolve in water.
    • Generally do not conduct electricity.

    Diatomic Molecules

    • 7 diatomic elements: HOFBrINCl (Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen, Chlorine).

    Naming Molecular Compounds

    • Use prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa) to indicate numbers of atoms.
    • "Mono" not used for first element.
    • Examples: CO (Carbon monoxide), N₂O₅ (dinitrogen pentoxide).

    Chemical Reactions

    • Reactants → Products
    • Word equations vs. chemical equations (with coefficients).

    Balancing Chemical Equations

    • Use coefficients to ensure equal numbers of each atom on both sides of the equation.
    • Never change subscripts.
    • Follow steps to balance.

    Types of Chemical Reactions

    • Synthesis (combination): A + B → AB
    • Decomposition: AB → A + B
    • Single displacement: AB + C → AC + B
    • Double displacement: AB + CD → AD + CB

    Combustion & Corrosion

    • Combustion: Rapid reaction with oxygen, produces oxides & energy.
    • Incomplete combustion: Limited oxygen supply, produces soot (carbon) and carbon monoxide (CO).
    • Corrosion: Breakdown of a metal due to chemical reactions with environment.
    • Rusting: Specific type of corrosion affecting iron. Preventing corrosion: coatings, materials, galvanizing.
      • Coatings: Protecting the metal.

    Acids and Bases

    • Acids: Substance that releases H+ ions in water.

      • Taste: sour
      • Reaction with metals: Produce H₂ gas.
      • Reaction with carbonates: Produce CO₂ gas.
      • Often start with hydrogen.

    • Bases: Substances that release OH⁻ or CO₃²⁻ ions in water.

    • Taste: bitter

    • Conduct electricity when dissolved in water

    • Often contain hydroxide (OH⁻), or carbonate (CO₃²⁻)

    Naming Acids

    • Binary acids: Hydro + stem + "ic" acid (Ex: HCl → hydrochloric acid).
    • Oxyacids: Stem end + "ic" or "ous" (Ex: HNO₃ → nitric acid).

    pH Scale

    • pH measures acidity/basicity of a solution (concentration of H⁺ ions).
    • Low pH = strong acid, high pH = strong base.
    • pH 7 = neutral.
    • pH scale is logarithmic.

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    Explore the fundamental concepts of matter including particle theory, physical and chemical properties, and changes in substances. This quiz will test your knowledge on how matter is categorized and the characteristics that define it. Perfect for students studying chemistry principles.

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