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CHAPTER 3 Atoms: The Building Blocks of Matter CHEMISTRY.

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Presentation on theme: "CHAPTER 3 Atoms: The Building Blocks of Matter CHEMISTRY."— Presentation transcript:

1 CHAPTER 3 Atoms: The Building Blocks of Matter CHEMISTRY

2 Foundations of Atomic Theory  History –Greek  Democritus – “atom” – could not be divided anymore  Aristotle and Plato - argued – s  Natural Philosophers –Experimentation – balances – quantitative measurements  Atom –Comes from Greek  “a” – not  “tomos” – cutting  indivisible

3 Foundations of Atomic Theory  Chemical Reaction –Transformation of substances into one or more new substances –Chemical change  Law of Conservation of Mass –Mass is neither created nor destroyed in ordinary chemical reactions –http://search.msn.com/video/results.aspx?q=l aw+of+conservation+of+mass&docid= &FORM=VIVR3 aw+of+conservation+of+mass&docid= &FORM=VIVR3http://search.msn.com/video/results.aspx?q=l aw+of+conservation+of+mass&docid= &FORM=VIVR3  Law of Definite Proportions –A chemical compound contains the same elements in exactly the same proportions by mass regardless of size of sample –Ex – H 2 O, CO 2

4 Foundations of Atomic Theory  Law of Multiple Proportions –If two or more compounds are composed of the same 2 elements, the masses can be expressed as ratios of small whole numbers

5 Dalton’s Atomic Theory  John Dalton  English School Teacher  1803

6 Dalton’s Atomic Theory  5 Points in his 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 cannot be subdivided, created, or destroyed –Atoms of different elements combine in simple whole number ratios to form compounds –In chemical reactions, atoms are combined, separated, or rearranged

7 Dalton’s Atomic Theory

8 Modern Atomic Theory  There have been some changes since Dalton’s Theory  Important concepts of modern theory –All matter is composed of atoms –Atoms of one element differ in properties from atoms of another element

9 Structure of the Atom  Atom – smallest particle of an element that can exist alone –Two regions of an atom  Nucleus –Center of atom –Protons and neutrons  Electron “cloud” –Area surrounding nucleus containing electrons

10 Discovery of the electron  Symbol  e -  Cathode ray tubes –Vacuum tube containing an electron gun (a source of electrons) and a fluorescent screen, with internal or external means to accelerate and deflect the electron beam, used to form images in the form of light emitted from the fluorescent screen. –Used in TV, computer monitors

11 Discovery of the electron  Charge and mass of the electron –JJ Thomson – 1897  Discovered the electron  1907 Nobel Prize in Physics  structure-electrons-video.htm structure-electrons-video.htm structure-electrons-video.htm  Did experiments with CRT – –Found that the charge to mass ration was always the same ration was always the same

12 Discovery of the atomic nucleus  Ernest Rutherford – 1908  Gold Foil Experiment

13 Composition of the nucleus  Protons –Positive charge 806-atomic-structure-the-nucleus- video.htm 806-atomic-structure-the-nucleus- video.htm 806-atomic-structure-the-nucleus- video.htm  Neutrons –Neutral charge 07-atomic-structure-neutrons-video.htm 07-atomic-structure-neutrons-video.htm

14 Forces in Nucleus  Nuclear forces –Forces that hold nuclear particles together –Binds protons and neutrons into the atomic nucleus

15 Sizes of Atoms  8-size-of-atoms-matter-video.htm 8-size-of-atoms-matter-video.htm 8-size-of-atoms-matter-video.htm

16 Summary

17 Counting Atoms  Atomic Number –Symbol  Z –Number of protons in nucleus –The number of protons determines identity of the element!!

18 Counting Atoms  Isotopes –Atoms of the same element with varying number of neutrons –Nuclide – general term for any isotope of any element –Mass Number – total number of protons + neutrons

19 Counting Atoms  The isotope of hydrogen –Protium – one proton only; 1e - –Deuterium – one proton, one neutron, one electron –Tritium – one proton, two neutrons, one electron; radioactive –http://www.citycollegiate.com/isotopeso fhydrogen.htm fhydrogen.htmhttp://www.citycollegiate.com/isotopeso fhydrogen.htm

20 Counting Atoms  Designating Isotopes –Hyphen notation  Name-mass #  Uranium-235  Ex – Neon with 12 neutrons? –Nuclear Symbol Notation  MN AN Element symbol  3 1 H  U How many p,n,e - in chlorine-37?

21 Relative Atomic Mass  Relative scale –Standard –Way to compare –Carbon-12  All others compared to Carbon-12  Atomic mass unit –amu –Approximate mass of a proton or a neutron

22 Average Atomic Mass  Weighted average of the atomic masses for all known isotopes –Calculating average atomic mass:

23 Relating mass to the number of atoms  “Particle” – a generic term  Mole – SI unit for amount of substance, counting unit –Symbol – mol –Avogadro’s number  6.02 x – number of particles in 1mol of substance –Molar mass  Mass of 1mol of substance = atomic mass

24 Calculating Molar Mass  H 2 O  CO 2  C 6 H 12 O 6

25 Conversions  Gram  Mole  Mole  Gram  Mole  Particle  Particle  Mole  Gram  Particle  Particle  Gram

26 Conversions  Gram  Mole; Mole  Gram

27 Conversions  Mole  Particle; Particle  Mole

28 Conversions  Gram  Particle; Particle  Gram


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