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Science 10

Science 10. Unit 1: energy and matter in chemical Change. Chapter 1: Atoms, Elements, and Compounds. 1.1 investigating and working with chemicals.

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Science 10

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  1. Science 10 Unit 1: energy and matter in chemical Change

  2. Chapter 1: Atoms, Elements, and Compounds 1.1 investigating and working with chemicals

  3. Modern Chemistry has a recent history dating back to the late 1700s. However, chemical properties and uses have been known to different civilizations for thousands of years: bluffton.edu

  4. North American Aboriginal Peoples • Tanning leathers • Herbal medicines chinesemedicineadvisor.com uwlax.edu

  5. Ancient Egypt • Embalming and mummification minnesota.publicradio.org

  6. Ancient Rome, Greece, Persia • Metal working for armour • Dyes for art and paint vector-clip-art.com en.wikipedia.org archive.worldhistoria.com

  7. Material Data Safety Sheets (MSDS) • Even natural chemicals must be handled properly to ensure safety. Each chemical today has a Material Safety Data Sheet (MSDS) to inform you of its physical properties (melting point, boiling point, odour) and hazards and instructions for handling and storing it safely.

  8. Workplace Hazardous Materials Information System (WHMIS) WHMIS identifies eight classes of hazards: • Hazardous Materials are covered by the Workplace Hazardous Materials Information System (WHMIS) which informs workers about the chemicals they work with in three ways: • Controlled products must have informative labels in both English and French on their containers • Each controlled product must have an MSDS • Workers must complete an education program that the employer provides

  9. Classifying Matter

  10. Practice Problems pg. 10 #1-4

  11. Chapter 1: Atoms, Elements, and Compounds 1.2 developing atomic theories

  12. From Ancient Greece to today… www.telegraph.co.uk www.universetoday.com 

  13. Assignment • Create a chart that follows the development of the Atomic Model throughout history. You can use the chart below to get started:

  14. John Dalton’s Atom The Billiard Ball Model • All matter is made up of small particles called atoms • Atoms cannot be created, destroyed, or divided into smaller particles • All atoms of the same element are identical in mass and size but different in mass and size to atoms of other elements • Compounds are formed when atoms of different elements combine in fixed or definite proportions • Chemical reactions change the way atoms are grouped but the atoms do not change thewallmachine.com

  15. The Cathode Ray Tube (CRT) • A gas discharge tube contains gas at a low pressure. • When electricity is run through it, a ray is formed and light is produced across the tube. www.xtimeline.com

  16. J.J. Thomson (1856-1950) • J.J. Thomson determined that the ‘ray’ in the Cathode Ray Tube was made up of a stream of negatively charged particles • He added charged plates to bend the cathode rays. • Based on the radius of the path, he determined that the mass of the particle was much less than that of an atom and that the negatively charged particle was a unique particle – the electron. cnx.org

  17. The Raisin-Bun or Plum-Pudding Model • Since these negatively charged electrons appeared to be present in all samples of matter, Thomson proposed that every atom contained electrons. • Since most matter was neutrally charged, there must also be a positively charged part of the atom. • Thomson thus proposed a positively charged sphere with many negatively charged electrons present on the surface of the sphere. www.nobelprize.org

  18. Ernest Rutherford (1871-1937) • Rutherford conducted his gold foil experiment to further examine the structure of atoms • He directed strongly positive alpha particles towards a thin layer of gold foil. • Most of the particles passed straight through, however some were deflected and even bounced back. www.rsc.org

  19. Protons and a Nucleus • Since most of the particles passed straight through, Rutherford concluded most of the atom is empty space • Since some of the particles reflected and deflected there must be a dense, massive nucleus to each atom. He determined that this was positively charged, made up of protons • The negatively charged electrons must orbit around the positively charged nucleus much like planets orbit the sun. www.iun.edu

  20. The Discovery of the Neutron • The Hydrogen atom is made up of 1 proton and 1 electron • Rutherford hypothesized that the next biggest atom, helium, would be 2 protons and 2 electrons. Therefore it should have a mass that is twice that of hydrogen. • Helium is 4 times more massive than hydrogen. • The neutron was discovered as a neutrally charged particle in the nucleus that has the same mass as a proton en.wikipedia.org

  21. Niels Bohr (1885-1962) • According to physical theory, the electrons orbiting the nucleus, should be losing energy in the form of light or radio waves. Losing energy would mean that the electron would come out of orbit and crash into the nucleus. This does not happen. • When electrical energy is applied to gases, they do emit light – a specific colour of light for each gas. Each colour corresponds to a specific wavelength of light or a specific energy. Rutherford’s model did not explain this, but Bohr’s did. en.wikipedia.org

  22. Energy Levels • Electrons in an atom have certain allowed energies that enable the atom to remain stable – energy levels. • Electrons can only move from one of these allowed energy levels to another – they cannot exist between them. • In order to jump from one level to the next they will absorb a specific amount of energy (jumping up a level), or emit a specific amount of energy (falling back down a level) library.thinkquest.org

  23. Our Working Model of the Atom… • Nucleons (protons and neutrons) make up the nucleus of an atom and electrons fill the space around the nucleus.

  24. Nuclear Notation • Isotopes – atoms made up of the same number of protons, but different number of neutrons • The atomic number is the number of protons and identifies the atom • The mass number is the total number of protons and neutrons • An atom has a neutral charge so there are equal numbers of protons and electrons in every atom • Ex. 11H - mass number is top, atomic number is bottom There is one proton, zero neutrons, and one electron. The name is hydrogen - 1

  25. Homework: pg. 23 #5-8, pg.24 #2, 4

  26. Chapter 2: Names, Formulas, and Properties 2.1 Chemical Names and formulas

  27. International Union of Pure and Applied Chemistry (IUPAC) • Founded in 1919, IUPAC developed a systematic method to name chemicals according to their composition. • The systematic name allows us to determine the chemical formula and predict some of its properties.

  28. Binary Compounds • Compounds that are made up of two elements are called binary compounds. • The names of binary compounds almost always end with the suffix “-ide”. commons.wikimedia.org

  29. Binary Molecular Compounds • A binary molecular compound forms when two non-metallic elements come together and form a covalent bond (sharing electrons). • Example – dihydrogen monoxide – fatal if inhaled montessorimuddle.org

  30. Rules for Naming Binary Molecular Compounds • 1. The first element in the name and formula is usually the one that is furthest to the left on the periodic table. • 2. The suffix “-ide” is attached to the name of the second element. • 3. Prefixes are used to indicate how many atoms of each type are present in one molecule of the compound. ths.talawanda.net

  31. Examples: • NO • N2O • NO2 • N2O3 • N2O4 • N2O5 • Practice Problems pg. 44 #1-4

  32. Names and Formulas for Binary Ionic Compounds • A binary ionic compound is composed of ions of one metal element and ions of one non-metal element joined by ionic bonds. elmhurst.edu

  33. Rules for writing names and formulas: • Ex. An ionic compound is made between calcium and fluorine. • The name is calcium fluoride • The formula is CaF2 • The first element in the name and formula is the metal. • The second element is the non-metal. The suffix “-ide” is attached to the name. • The chemical formula shows the simplest whole number ratio of each type of ion in the compound. *The names of ionic compounds DO NOT contain prefixes* en.wikipedia.org

  34. Example: Predict the formula of Lithium Oxide Solution: • Identify the type of compound – metal & non-metal therefore ionic • Determine the charges on the ions – Li1+ and O2- • The compound must be electrically neutral. Therefore it will take two lithium ions to balance with one oxide ion. • The formula is Li2O

  35. Practice Problems: pg. 45 #5-8

  36. Cation Charges • Many of the transition metals (elements in groups 3-12) are able to form more than one type of cation. • Ex. Nickel can form Ni2+ or Ni3+ • Ex. Copper can form Cu+ and Cu2+ • If you are given the formula of an ionic compound you can determine the charge on the cation. en.wikipedia.org

  37. Example: Which copper cation, Cu+ or Cu2+, is in CuCl2 Solution: • Begin by writing out the two ions involved. Chloride is always a Cl1- and the copper could be either Cu+ or Cu2+ • The compound must be electrically neutral. If there are two Cl1- ions then the single copper must be a 2+ charge. • Therefore the cation is Cu2+

  38. Practice Problems: pg. 46 #9, 10

  39. Naming Cations Using the Stock System • When writing the name of an ionic compound that consists of a transition element that could be different charges, the charge on the cation is written in parentheses, as a Roman numeral after the name of the metal. • Example: Cu2+ is copper (II)

  40. Example: Write the chemical formula for copper(II) oxide Solution: • The copper cation is named copper(II) and therefore is Cu2+ • The oxide anion is always O2- • The compound must be electrically neutral so the charges must cancel. • Therefore, one copper(II) ion will combine with one oxide ion. • The formula is CuO

  41. Practice Problems: pg. 47 #11-12

  42. Homework: Investigation 2-A

  43. Compounds Containing Polyatomic Ions • Many ionic compounds are not binary because they are made up of one or both ions containing more than one type of atoms – polyatomic ions. • Polyatomic ions are made of covalent bonds that as a group have a collective positive or negative charge. www.fccj.us

  44. Example: What is the formula of ammonium sulfide?

  45. Example: What is the name of CuCO3

  46. Practice Problems: pg. 52 #13-16

  47. Families of Polyatomic Anions • Ex. Nitrate, nitrite or sulfate, sulfite • Patterns exist: • In each family, the anion ending with “-ate” serves as a reference point. The other anions are named according to the number of oxygen atoms in their formula, in relation to the reference anion. • Compared with an “__-ate” anion, an “___-ite” anion has one less oxygen in its formula 4. Compared with an “____-ate” anion, a “hypo___ite” has two less oxygen atoms in its formulas 5. Compared with an “____-ate” anion, a “per_____ate” has one more oxygen atom in its formula.

  48. Practice Problems: pg. 53 #17-19

  49. Hydrogen Compounds • Hydrogen is a non-metal even though it appears on the left side of the periodic table. • Therefore, these hydrogen compounds are molecular but they do not use prefixes • Common examples are on Table 2.5 on pg. 54 in textbook. • Homework: pg. 55 #1-6

  50. Chapter 2: Names, Formulas, and Properties 2.2 Explaining properties of substances

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