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Chapter #3

Chapter #3 ATOMS: The Building Blocks of Matter. Chapter #3. Atoms: The Building Blocks of Matter. 3-1 Early Atomic Theory. Do Not need in notes. Atoms are so small they cannot be observed directly. Scientists could use only experimental data to help describe the atom.

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Chapter #3

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  1. Chapter #3 ATOMS: The Building Blocks of Matter Chapter #3 • Atoms: The Building Blocks of Matter

  2. 3-1 Early Atomic Theory Do Not need in notes • Atoms are so small they cannot be observed directly. Scientists could use only experimental data to help describe the atom. • Around 400 B.C., Democritus (a Greek philosopher) suggested that the world was made of two things - empty space and tiny particles called atoms. • During the 1800's, a French Chemist (Antoine Lavoisier) discovered that chemical "changes" occurring in a closed system - the mass after a chemical change equaled the mass before the chemical change. • He proposed that, in ordinary chemical reactions, matter can be changed in many ways, but it cannot be created or destroyed (Law of Conservation of Mass). • Work by another French Chemist, Joseph Proust, had observed that specific substances always contain elements in the same ratio by mass (Law of Definite Proportions.)

  3. Foundations of Atomic Theory • Law of Definite Proportions: The elements composing a compound are always found in the same ratio by mass. • Law of Multiple Proportions: The masses of one element that combine with a fixed amount of another element to form more than one compound are in the ratio of small whole numbers. Example CO, CO2

  4. For example: Oxygen can combine with Carbon to form Carbon Monoxide, CO, or form Carbon Dioxide, CO2. • Dalton was the founder of Atomic Theory.

  5. Dalton’s Atomic Theory • All matter is composed of extremely small particles called atoms. • Atoms of a given element are identical in size, mass and other properties; atoms of different elements differ in size, mass, and other properties. • Atoms cannot be subdivided, created, or destroyed. • Atoms of different elements combine in simple whole-number ratios to form chemical compounds. • In chemical reactions, atoms are combined, separated, or rearranged.

  6. Modern Atomic Theory • Element have a characteristic average mass which is unique to that element. • Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions. However, these changes CAN occur in nuclear reactions! • All matter is composed of atoms • Atoms of any one element differ in properties from atoms of another element

  7. Section 3-2 • Atom- the smallest particle of an element that retains the chemical properties of that element. • Nucleus- is the positively charges, dense central portion of the atom that contains nearly all of its mass but takes up only an insignificant fraction of its volume.

  8. Subatomic Particles

  9. The Atomic Scale • Most of the mass of the atom is in the nucleus (protons and neutrons) • Electrons are found outside of the nucleus (the electron cloud). e- have very tiny mass. • Most of the volume of the atom is empty space

  10. Drawing atoms • In the nucleus • Symbol • # of p+ • # of N • Outside the nucleus in the energy shells/level • electrons

  11. Famous Scientist

  12. Do NOT need in Notes Discovery of the Electron • In 1897, J.J. Thomson used a cathode ray tube to deduce the presence of a negatively charged particle. • Cathode ray tubes pass electricity through a gas that is contained at a very low pressure.

  13. Thomson was awarded the Nobel Prize in 1906 for his "discovery" of the first sub-atomic particle; the electron. This discovery strongly implied that Dalton was wrong and that the atom was not the smallest particle of matter. It looked as if the atom could be broken down into even smaller pieces, and to Thomson these smaller pieces were his negatively charged electrons. Do NOT need in NOTES

  14. Do NOT need in NOTES Conclusions from the Study of the Electron • Cathode rays have identical properties regardless of the element used to produce them. All elements must contain identically charged electrons. • Atoms are neutral, so there must be positive particles in the atom to balance the negative charge of the electrons • Electrons have so little mass that atoms must contain other particles that account for most of the mass

  15. Do NOT need in NOTES Thomson’s Atomic Model • Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “plum pudding” model.

  16. Do NOT need in NOTES Rutherford’s Gold Foil Experiment • Alpha particles are helium nuclei • Particles were fired at a thin sheet of gold foil • Particle hits on the detecting screen (film) are recorded

  17. DO NOT Need in Notes Rutherford’s Findings • Most of the particles passed right through • A few particles were deflected • VERY FEW were greatly deflected • Conclusions: • The nucleus is small • The nucleus is dense • The nucleus is positively charged

  18. Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element. The number of protons = the number of electrons 6 C Carbon 12.011 Section 3-3

  19. Mass Number • Mass number is the number of protons and neutrons in the nucleus of an isotope. • Mass # = p+ + n • SOooo the number of Neutrons = • n= Mass # - p+

  20. Isotopes • Isotopes are atoms of the same element that have different masses. (number of neutrons)

  21. Nuclear Symbols 235 92 Mass number (p+ + n) Mass number (p+ + n) Element symbol Atomic number (# of p+) U 235 92

  22. Hyphen Notation Sodium-23 (23 is the mass #) Sooo… 23- 11 (atomic #) = 12 for the # of neutrons. 11 is the # of protons and electrons.

  23. Isotopes of H

  24. The Mole • 1 dozen =12 • 1 gross = 144 • 1 ream = 500 • 1 mole = 6.022 x 1023 • There are exactly 12 grams of carbon-12 in one mole of carbon-12.

  25. Calculations:Converting moles to grams • Given # of mole X ? g (look at periodic table)= g of 1 mole • How many grams of lithium are in 3.50 moles of lithium? • 3.50 mole X 6.941 g = 24.29 g Li 1 mol

  26. Calculations:Converting grams to moles • Given # of g X 1 mol = mol of g (look at periodic table) • How many moles of lithium are in 18.2 grams of lithium? • 18.2 g X 1 mol Li = 2.622 mol Li 6.941 g

  27. Avogadro’s Number • Is the number of particles in exactly one mole of a pure substance. • 6.022 x 1023 is called “Avogadro’s Number” in honor of the Italian chemist Amadeo Avogadro (1776-1855). I didn’t discover it. Its just named after me!

  28. Calculations:Converting Moles to Particles • Given # of mol x 6.022 x 1023 part= atoms 1 mol • How many atoms/particles/molecules of lithium are in 3.50 moles of lithium? • 3.50 mole X 6.022 x 1023 = 2.11 x 1024 atoms of Li 1 mol

  29. Calculations:Converting Particles to Moles • Given # of particles x 1 mole = mol 6.022 x 1023 • How many moles of lithium are there in 1.2044 x 1024 particles of Li? • 1.2044 x 1024 part x 1 mole = 2.0 mol Li 6.022 x 1023 part

  30. Calculations:Converting grams to particles • Given # of grams x 1 mol x 6.022 x 1023= particles ? g 1 mol • How many atoms/particles/molecules of lithium are in 18.2 g of lithium? • 18.2 g x 1 mol x 6.022 x 1023 = 1.58 x 1024 particle Li 6.941g 1 mol

  31. Calculations:Converting particles to grams • Given # of particles x 1 mol x ? g = g 6.022 x 1023 1 mol • How many grams are there in 8.02 x 1025 particles of lithium?

  32. Work Cited • “JJ Thomson”. Photo. July 28, 2006. http://www.sciencemuseum.org.uk/online/electron/section2/recording.asp • Cathode Ray Image and JJ Thomson Model. Image. July 28, 2006. http://www.brooklyn.cuny.edu/bc/ahp/LAD/C3/C3_Electrons.html • “Gold Foil Experiment”. Image. July 28, 2006. http://www.avon-chemistry.com/atom_lecture.html • “Rutherford”. Photo. July 28,2006. http://www.anthroposophie.net/bibliothek/nawi/physik/rutherford/bib_rutherford.htm • “Mole”. Photo. Aug 8, 2006. http://www.mwt.net/~bionorse/chemistry.htm

  33. “Hydrogen Isotopes”. Picture. August 4, 2006. www.sr.bham.ac.uk/xmm/atom.html • “Amedeo Avogadro”. avagadroc.jpg August 4, 2006. poohbah.cem.msu.edu/Portraits/PortraitsH... • “Uranium symbol”. Picture. August 4, 2006.www.webelements.com/webelements/scholar/... • Holt, Rinehart and Winston. Modern Chemistry. Harcourt Brace & Company. 1999. • “Atom Comic Cover”. Photo. Aug. 12, 2006. http://home.cfl.rr.com/fradford/Atom/Atom20.jpg

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