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Science 10

Science 10. Properties of Matter (A1.0). Classification of Matter (A2.0). Energy and Matter in Chemical Change. Chemical Reactions (A3.0). A1.0 Properties of Matter. Lab Safety. Properties of Matter. Theories of Matter. Lab Safety. Lab safety contract and rules

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Science 10

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  1. Science 10 Properties of Matter (A1.0) Classification of Matter (A2.0) Energy and Matter in Chemical Change Chemical Reactions (A3.0)

  2. A1.0 Properties of Matter Lab Safety Properties of Matter Theories of Matter

  3. Lab Safety • Lab safety contract and rules • Safety hazard symbols identify dangerous materials in household products • WHMIS symbols identify dangerous materials in the workplace or school • MSDS are detailed information sheets about dangerous materials

  4. Properties of Matter • Matter: anything that takes up space (solid, liquid, gas or plasma) • Chemical: any pure substance or mixture of pure substances • Physical Property: an observable characteristic of matter including colour, texture, hardness, malleability, ductility, boiling point and melting point

  5. Properties of Matter • Chemical Property: a description of how a substance reacts when exposed to another substance • Pure Substance: a substance that has fixed properties and cannot easily be separated into its components

  6. Properties of Matter • Element: a pure substance made up of only one type of atom • Compound: a pure substance made up or more than one type of element • Mixture: a combination of two or more pure substances • Mechanical Mixture: a mixture in which the pure substances are distinct (heterogeneous)

  7. Properties of Matter • Solution: a mixture in which the pure substances are not distinct (homogeneous) • Solute: the substance dissolved • Solvent: the substance that dissolves the solute • A chemical reaction occurs when a substance reacts to form new substances

  8. Properties of Matter • Evidence of a chemical reaction may include: • A change in state, melting point, colour or density • A change in temperature • Formation of a gas (bubbles) or a precipitate (solid particles in a previously clear solution) • Chemical reactions must obey the law of conservation of mass

  9. Theories of Matter • Historical use of chemistry has included • Food Chemistry Heating and freezing Salting Fermentation • Metallurgy Annealing, ores and alloys • Alchemy Ancient “science”

  10. Theories of Matter • An atom is the smallest particle of an element that retains the properties of the element • Atomic theory has evolved over the years: • Dalton: billiard ball model • Thompson: plum pudding model • Rutherford: nuclear model • Bohr: energy level model • Quantum: electron cloud model

  11. A2.0 Classification of Matter The Periodic Table and Atomic Structure Naming Ionic and Molecular Compounds Properties of Ionic and molecular Compounds Acids and Bases Our Chemical Society

  12. The Periodic Table and Atomic Structure • All known elements are grouped according to physical and chemical properties • Information contained in the Periodic Table includes: • Element Symbol • Element Name • Period Number • Family Number

  13. The Periodic Table and Atomic Structure • Atomic Number • Other information • Atomic mass • SATP State • Metal/Non-metal/Metalloid • A Bohr model illustrates the relative locations of the protons, neutrons and electrons of an atom

  14. The Periodic Table and Atomic Structure • A valence electron is an electron that is in the highest energy level of an atom • A Lewis diagram depicts the valence electrons in an atom • The Rule of Octets states that atoms bond in such a way as to have a full valence level

  15. Naming Ionic and Molecular Compounds • Ionic compounds are formed when a metal donates one or more electrons to a non-metal • The metal becomes a positively charged ion (cation) while the non-metal becomes a negatively charged ion (anion) • Positive ions attract negative ions to form a stable crystal lattice

  16. Naming Ionic and Molecular Compounds • Naming binary ionic compounds: • Name the cation first by using the element’s name • Name the anion second by using the first part of the element name and changing the ending to “ide” • Include the state of matter

  17. Naming Ionic and Molecular Compounds • Writing formulas of binary ionic compounds: • Identify the anion and cation • Determine the total charges needed to balance • Note the ratio of cations to anions • Use subscripts to write the formula

  18. Naming Ionic and Molecular Compounds • Naming multivalent ionic compounds: • Identify the anion • Use the charge of the anion to determine which version of the cation to use • Write the name of the cation with a roman numeral to indicate which version is used • Write the name of the anion and change the ending to “ide” • Include the state of matter

  19. Naming Ionic and Molecular Compounds • Writing the formulas of multivalent ionic compounds: • Identify the anion and cation • Determine which version of the cation is used • Determine the total charges needed to balance • Note the ratio of cations to anions • Use subscripts to write the formula

  20. Naming Ionic and Molecular Compounds • Naming polyatomic ionic compounds: • Identify the cation and write the element name • Identify the polyatomic anion and write its name • If necessary use a roman numeral to indicate which version of the cation is used • Include the state of matter

  21. Naming Ionic and Molecular Compounds • Writing the formulas of polyatomic ionic compounds: • Identify the cation and polyatomic anion • Determine the total charges needed to balance • Note the ratio of cations to anions • Place brackets around the anion if more than one is needed • Use subscripts to write the formula

  22. Naming Ionic and Molecular Compounds • Molecular compounds are formed when two non-metals share a pair of valence electrons • A covalent bond is a shared pair of electrons • The number of shared pairs of electrons determines the number of covalent bonds between two atoms

  23. Naming Ionic and Molecular Compounds • Molecular elements contain atoms of only one element • Molecular elements can be monatomic, diatomic and polyatomic • Binary molecular compounds that do not contain hydrogen can be named: • Use a prefix to indicate the number of the first element • Use a prefix to indicate the number of the second element and change the ending to “ide” • Include the state of matter

  24. Naming Ionic and Molecular Compounds • To write the formulas of binary molecular compounds: • Use the prefix of the first element to determine the number of that element • Use the prefix of the second element to determine the number of that element • Molecular compounds that contain hydrogen have unique names that must be memorized

  25. Properties of Ionic and Molecular Compounds • Ionic compounds: • Have a high melting point (solid at SATP) • Retain a crystal shape • Dissolve in water • Conduct electricity when dissolved • The solubility of ionic compounds can be predicted using a solubility table

  26. Properties of Ionic and Molecular Compounds • Molecular compounds: • Have low melting points (can be solid, liquid or gas at SATP) • Do not conduct electricity when dissolved • Water is a molecular compound with special properties including: • High boiling point • Low density as a solid • High polarity

  27. Acids and Bases • Acids: • Are aqueous compounds with that dissolve to form hydrogen ions • Have a pH level less than 7 • React with metals to make hydrogen gas • Taste sour • Can be neutralized with bases

  28. Acids and Bases • Bases: • Are aqueous compounds with that dissolve to form hydroxide ions • Have a pH level greater than 7 • Taste bitter • Feel slippery • Can be neutralized with acids

  29. Acids and Bases • An indicator is a chemical that changes colour depending on the pH of the solution to which it is added • Litmus paper is an indicator • A universal indicator is a mixture of indicators that can determine the precise pH of a solution

  30. Our Chemical Society • The use of industrial and household chemicals has risks • Environmental (example: CFC’s) • Health (Examples: alcohol, nicotine, benzene) • Several careers relate to chemistry • Food Technologist • Cosmetics Formulator • Petroleum Engineer

  31. Chemical Reactions Examples of Chemical Change Writing Chemical Equations Types of Chemical Reactions The mole

  32. Examples of Chemical Change • Different examples of chemical changes include • Reactions that form gases • Reactions that form solids • Exothermic reactions • Endothermic reactions • Biochemical reactions including photosynthesis and cellular respiration

  33. Examples of Chemical Change • Characteristics of chemical reactions include: • The production of new substances with new properties • The flow of energy • A change of state • The observance of the law of conservation of mass

  34. Writing Chemical Reactions • A word equation is a sentence that accurately describes a chemical change • A balanced chemical formula equation uses appropriate symbols to accurately describe a chemical change

  35. Types of Chemical Reactions • There are five types of chemicals reactions we will study • Formation (element + element  compound) • Decomposition (compound  element + element) • Hydrocarbon Combustion (hydrocarbon + oxygen gas  carbon dioxide gas + liquid water)

  36. Types of Chemical Reactions 4. Single Replacement (element + compound element + compound) 5. Double Replacement (compound + compound  compound + compound)

  37. The Mole • A mole is a quantity use in chemistry to measure elements and compounds • One mole equals 602 000 000 000 000 000 000 000 particles • Avogadro’s Number = 6.02 x 1023 • Molar mass is the mass of one mole of a substance • Number of moles = mass / molar mass

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