Science 10 Chemistry Flashcards

Lab Safety

• Rules, Protection, Clean Up: Core aspects of lab safety.

• WHMIS: Info on hazardous materials.

  • Symbols

  • Biohazard: Threat to living organisms.

  • Corrosive: Damages substances.

  • Flammable: Easily ignited.

  • Compressed Gas: High pressure, dangerous if released.

  • Oxidizing Material: Contributes to combustion.

  • Poisonous (Immediate): Toxic effects after exposure.

  • Dangerous Reactive: Rapid, uncontrolled reaction.

  • Toxic (Long Term): Adverse effects after repeated exposure.

Properties of Matter

• Physical Properties

  • Boiling Point: Liquid to gas.

  • Melting Point: Solid to liquid.

  • Colour: Visual attribute.

  • State: Solid, liquid, gas.

  • Solubility: Dissolves in solvent.

  • Conductivity: Conducts electricity/heat.

  • Magnetic: Attracted to magnetic field.

  • Ductility: Drawn into wire.

• Chemical Properties

  • Flammable: Ability to burn.

  • Reaction with Water: Interaction with water.

  • Reaction with Acids: Interaction with acids.

  • Reaction with Heat: Changes when heated.

• Seperation Methods- Physical
  - Filter: Solids from liquids.
  - Decant: Pouring off liquid.
  - Distillation: Separating liquids by boiling points.
  - Magnet: Separating magnetic substances.
  - Picking: Manual separation.

  • Chemical

    • Electrolysis: Electricity to decompose.

    • Reactions: Chemical reactions to separate.

Matter

• Pure Substances

  • Elements: One type of atom.

  • Compounds: Two or more elements bonded.

• Mixtures

  • Homogeneous: Uniform composition.

  • Heterogeneous: Non-uniform composition.

  • Mechanical Mixture: Easily visible components.

  • Suspension: Large particles, settle over time.

  • Colloids: Particles between solution and suspension size.

  • Solutions: Substance dissolved in another.

Evidence of Chemical Reaction

• Precipitate: Solid forms from solution.

• Gas Formed: Gas production.

• Colour Change: Change in colour.

• Change in Temperature: Increase or decrease in temperature.

Periodic Table

• Arrangement

  • Groups/Families (Vertical): Similar chemical properties.

  • Periods (Horizontal): Increasing atomic number.

  • Metals: Shiny, conductive, malleable.

  • Nonmetals: Lack metallic properties.

  • Alkali Metals: Group 1, highly reactive.

  • Alkaline Earth Metals: Group 2, reactive.

  • Transition Metals: d-block elements.

  • Halogens: Group 17, highly reactive nonmetals.

  • Noble Gases: Group 18, stable and unreactive.

Atomic Theory

• Nucleus

  • Protons

    • Charge: +1

    • Mass: 1 \text{ amu } (1 \text{ g/mol})

    • Number of Protons = Atomic Number

  • Neutron

    • Charge: 0

    • Mass: 1 \text{ amu } (1 \text{g/mol})

    • Number of Neutrons = Atomic Mass – Protons

• Outside Nucleus

  • Electrons

    • Charge: -1

    • Mass: 0 \text{ amu }

    • Number of Electrons = Protons

Isotopes

• Have different number of neutrons.

Ions

• Metals lose electrons: cations (+).

• Non-metals gain electrons: anions (-).

• Achieve full valence shell like noble gases.

• Shell capacities: 1st = 2, 2nd = 8, 3rd = 8…

Compounds

• Ionic

  • Metals transfer electrons to non-metals.

  • Properties:

    • Solids

    • Dissociate in solution

    • Conduct electricity in solution

• Molecular

  • Non-metals share electrons.

  • Properties:

    • Solid, Liquid, or Gas

    • May dissolve

    • Do not conduct electricity

Naming Compounds

• Metal, NH_4^+ , or H^+?

  • Yes = Ionic

    • Name positive then negative.

    • Transition metal: Roman numeral = charge.

    • Balance charges for formula; subscript for quantity.

    • 2nd element ends in -ide.

  • No = Molecular

    • Prefixes indicate atom quantity in name and formula.

• H^+ = Acid

Acid/Base

• Acids

  • Conduct electricity

  • Sour

  • pH < 7

  • Blue litmus turns red

• Bases

  • Ionic Naming

  • Often have OH^-

  • Bitter

  • Slippery

  • pH > 7

  • Red litmus turns blue

Solubility of Ionic Compounds

• Solubility > 0.1 mol/L: Group 1, ClO3^-, CF3^-, NH4^+, NO3^-, CH_3COO^-, Br^-, I^-

• Solubility < 0.1 mol/L: SO4^{2-}, Cl^-, ClO4^-, PO4^{3-}, OH^-, S^{2-}, CO3^{2-}

• Most: Group 1, NH_4^+, Sr^{2+}, Ba^{2+}, Tl^+

• None: Ag^+, Ca^{2+}, Pb^{2+}, Hg^{2+}, Cu^{2+}, Ra^{2+}

Molecular Compounds

• Prefixes: Memorize 1-10 (mono to deca).

• Molecular Elements: Memorize H2, N2, O2, F2, Cl2, Br2, I2, O3, P4, S8

• Common Compounds: Memorize H2O, H2O2, NH3, C{12}H{22}O{11}, C6H{12}O6, CH4, C3H8, CH3OH, C2H5OH

Chemical Reactions

• Law of Conservation of Mass: Matter is neither created nor destroyed.

• Atoms entering a reaction must exit in equal quantity.

• Chemical Equations: Reactants ========> Products

Balancing Equations

1. Correct formulas.

2. List elements on both sides.

3. Count atoms of each element.

4. Balance using coefficients.

5. Recheck until balanced.

Types of Reactions

1. Formation: A + B \rightarrow AB

2. Decomposition: AB \rightarrow A + B

3. Single Replacement: A + BC \rightarrow AC + B or A + BC \rightarrow C + BA

4. Double Replacement: AB + CD \rightarrow AD + CB

5. Hydrocarbon Combustion: CxHy + O2 \rightarrow CO2 + H_2O