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Chapter 1 – 3 The Foundations

Chapter 1 – 3 The Foundations. There are two fundamental concepts for chemistry Matter is composed of various types of atoms On substance changes to another by reorganizing the way the atoms are attached to each other. Qualitative Versus Quantitative.

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Chapter 1 – 3 The Foundations

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  1. Chapter 1 – 3The Foundations • There are two fundamental concepts for chemistry • Matter is composed of various types of atoms • On substance changes to another by reorganizing the way the atoms are attached to each other.

  2. Qualitative Versus Quantitative

  3. Units of measureall measurements have 2 things!?What are they?

  4. Volume – SI derived unit for volume is cubic meter (m3) 1 cm3 = (1 x 10-2 m)3 = 1 x 10-6 m3 1 dm3 = (1 x 10-1 m)3 = 1 x 10-3 m3 1 L = 1000 mL = 1000 cm3 = 1 dm3 1 mL = 1 cm3 1 L = 1 dm3

  5. 1 m 1 m 1 m 1 m 100 cm 100 cm 100 cm 100 cm 3 Units to a Power • How many m3 is 1500 cm3? 1500 cm3 1500 cm3 =15 m3

  6. Uncertainty • All measurements have some degree of uncertainty. • The certain numbers and the uncertain numbers in a measurement are called the significant figures of a measurement.

  7. Precision vs. Accuracy Accuracy – how close a measurement is with the true value Precision - how close a set of measurements are to each other

  8. Uncertainty

  9. Significant figures & Dimensional Analysis • Science fiction often uses nautical analogies to describe space travel. If the starship U.S.S. Enterprise is traveling at warp factor 1.71, what is its speed in knots? • Warp 1.71 = 5.00 times the speed of light • speed of light = 3.00 x 108 m/s • 1 knot = 2000 yd/h exactly What is an exact number?

  10. Classifying matter3 states…what are they?What do we know about them?

  11. Methods of separating mixtures • Only a physical change- no new matter • Filtration- separate solids from liquids with a barrier • Distillation- separates because of different boiling points • Heat mixture • Catch vapor in cooled area • Chromatography-different substances are attracted to paper or gel, so they move at different speeds up the paper

  12. Distillation

  13. Chapter 2 – Atoms, Molecules, and Ions HISTORY • Robert Boyle was the first “chemist”: • Performed quantitative experiments • Lavosier – father or modern chemistry

  14. THREE IMPORTANT LAWS • Law of conservation of mass (Lavoisier): • Mass is neither created nor destroyed • Law of definite proportion (Proust): • A given compound always contains exactly the same proportion of elements by mass

  15. …the third law • Law of multiple proportions (Dalton): • When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers • Dalton could not deduce absolute formulas, but found that each element consisted of a certain type of atom and that compounds were formed from specific combinations of atoms.

  16. What do you know about Dalton? Which of the following statements regarding Dalton’s atomic theory are still believed to be true? • Elements are made of tiny particles called atoms. • All atoms of a given element are identical. • A given compound always has the same relative numbers and types of atoms. IV. Chemical reactions change the way atoms are bound together. Atoms are thus changed!

  17. Gay-Lussac/Avogadro & gases • Gay-Lussac measured (under same conditions of T and P) the volumes of gases that reacted with each other. • Avogadro’s Hypothesis: • At the same T and P, equal volumes of different gases contain the same number of particles

  18. JJ Thompson • Postulated the existence of electrons using cathode-ray tubes • Determined the charge-to-mass ratio of an electron • The atom must also contain positive particles that balance exactly the negative charge carried by the electrons

  19. Millikan • Performed experiments involving charged oil drops • Determined the magnitude of the electron charge • Calculated the mass of the electron

  20. Rutherford • Explained the nuclear atom • Atom has a dense center of positive charge called the nucleus • Electrons travel around the nucleus at a relatively large distance

  21. The modern atom • The atom contains: • Electrons – foundin the electron cloud region; negative charge (1/2000 the size of a proton or neutron) • Protons – found in the nucleus; positive charge equal in magnitude to the electron’s negative charge • Neutrons– found in the nucleus; no charge; virtually same mass as a proton

  22. The nucleus is: • Small compared with the overall size of the atom • Extremely dense; accounts for almost all of the atom’s mass “If the atom is the Houston Astrodome, then the nucleus is a marble on the 50-yard line.”

  23. Atomic informationWhich is which?What does this mean? • Z and A • Atomic number • Mass number • Isotopes…what are they?

  24. Bonds! • Forces that hold atoms together in compounds • Ionic Bonds: • Bonds form due to force of attraction between oppositely charged ions • Ion – atom or group of atoms that has a net positive or negative charge • Cation– positive ion; lost electron(s) • Anion – negative ion; gained electron(s) • Polyatomic ions---memorize them!!!!!

  25. More bonds! • Covalent Bonds: • Bonds form between atoms by sharing electrons • Resulting collection of atoms is called a molecule • Molecules can be represented in various ways. Some may or may not indicate the shape of the molecule. (shapes come in chapter 8)

  26. Formulas and Models

  27. The periodic table • KNOW… • Locations of metals, nonmetals, metalloids • Group names • Most common ionic charge • Trends

  28. Naming compoundsIonic AND molecular: What’s the difference? • MgO • MnO • KMnO4 • NH4NO3 • Hg2Cl2 • Cr2O3 • KClO4 • NaClO3 • CaS • K2S • AlPO4 • CO2 • CO • CCl4 • N2O4 • XeF6 • N4O4 • P2O10

  29. Now write formulas • Sodium sulfite • calcium iodide • Lead (II) oxide • Lead (IV) oxide • Mercury (I) sulfide • Barium chromate • Aluminum hydrogen sulfate • Cerium (IV) nitrite • Sulfur dioxide • diflourine monoxide • nitrogen trichloride • diphosphoruspentoxide

  30. Try this! Which of the following compounds is named incorrectly? • KNO3 potassium nitrate • TiO2 titanium(II) oxide • Sn(OH)4 tin(IV) hydroxide • PBr5 phosphorus pentabromide • CaCrO4 calcium chromate

  31. Acids • Learn the rules or MEMORIZE!! • Substances that produce an H+ when dissolved in water. • Two types • Oxyacids • Non oxyacids

  32. Oxyacids • If the formula has oxygen in it • write the name of the anion, but change • ate to -ic acid • ite to -ous acid • H2CrO4 • HMnO4 • HNO2

  33. Non oxyacids • If the acid doesn’t have oxygen • add the prefix hydro- • change the suffix -ide to -ic acid • HCl • H2S • HCN

  34. Now write formulas • hydrofluoric acid • acetic acid • carbonic acid • phosphoric acid • chlorous acid • Hydroiodic acid • Nitrous acid

  35. CuSO4 CuSO4•5H2O Hydrates are compounds that have a specific number of water molecules attached to them. barium chloride dihydrate BaCl2•2H2O lithium chloride monohydrate LiCl•H2O MgSO4•7H2O magnesium sulfate heptahydrate Sr(NO3)2 •4H2O strontium nitrate tetrahydrate

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