Atomic Structure Chapter 4 Development of the Atom
- Slides: 88
Atomic Structure Chapter 4
Development of the Atom
The Hellenic Market Fire ~~ Water Earth Air
The Greeks History of the Atom • Not the history of atom, but the idea of the atom • In 400 B. C the Greeks tried to understand matter (chemicals) and broke them down into earth, wind, fire, and water. ~ ~ • Democritus and Leucippus Greek philosophers
Mental Experiment – Atoms Exist • Looked at beach • Made of sand • Cut sand - smaller sand Smallest possible piece? q Atomos - not to be cut q
Greek Model Democritus • Greek philosopher • Idea of ‘democracy’ • Idea of ‘atomos’ – Atomos = ‘indivisible’ – ‘Atom’ is derived • No experiments to support idea Democritus’s model of atom No protons, electrons, or neutrons Solid and INDESTRUCTABLE
Four Element Theory FIRE • Plato was an atomist • Thought all matter was composed of 4 elements: – – – Earth (cool, heavy) Water (wet) Fire (hot) Air (light) Ether (close to heaven) Hot AIR Dry EARTH ‘MATTER’ Wet Cold WATER Relation of the four elements and the four qualities Blend these “elements” in different proportions to get all substances
Some Early Ideas on Matter Anaxagoras (Greek, born 500 B. C. ) – Suggested every substance had its own kind of “seeds” that clustered together to make the substance, much as our atoms cluster to make molecules. Empedocles (Greek, born in Sicily, 490 B. C. ) – Suggested there were only four basic seeds – earth, air, fire, and water. The elementary substances (atoms to us) combined in various ways to make everything. Democritus (Greek, born 460 B. C. ) – Actually proposed the word atom (indivisible) because he believed that all matter consisted of such tiny units with voids between, an idea quite similar to our own beliefs. It was rejected by Aristotle and thus lost for 2000 years. Aristotle (Greek, born 384 B. C. ) – Added the idea of “qualities” – heat, cold, dryness, moisture – as basic elements which combined as shown in the diagram (previous page). Hot + dry made fire; hot + wet made air, and so on. O’Connor Davis, Mac. Nab, Mc. Clellan, CHEMISTRY Experiments and Principles 1982, page 26,
Who Was Right? • • California WEB Greek society was slave based Beneath famous to work with hands did not experiment Greeks settled disagreements by argument Aristotle was more famous He won! His ideas carried through middle ages. Alchemists change lead to gold
Alchemy • After that chemistry was ruled by alchemy. • They believed that they could take any cheap metals and turn them into gold. • Alchemists were almost like magicians. – Elixirs, physical immortality
Alchemy Alchemical symbols for substances… . . . . GOLD SILVER COPPER IRON SAND transmutation: changing one substance into another D In ordinary chemistry, we cannot transmute elements.
Contributions of alchemists: Information about elements - the elements mercury, sulfur, and antimony were discovered - properties of some elements Develop lab apparatus / procedures / experimental techniques - alchemists learned how to prepare acids. - developed several alloys - new glassware
Alchemists’ Contributions • The elements mercury, sulfur, and antimony were discovered. • Alchemists learned how to prepare acids. • Develop lab apparatus / procedures • How to make some alloys • Properties of some elements
Timeline Greeks (Democratus ~450 BC) Discontinuous theory of matter 400 BC Greeks (Aristotle ~350 BC)) Continuous theory of matter ALCHEMY 300 AD 1000 Issac Newton (1642 - 1727) 2000 American Independence (1776)
Dalton Model of the Atom Late 1700’s - John Dalton- England Teacher- summarized results of his experiments and those of other’s Combined ideas of elements with that of atoms in Dalton’s Atomic Theory
Foundations of Atomic Theory Law of Conservation of Mass is neither destroyed nor created during ordinary chemical reactions. Law of Definite Proportions The fact that a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound. Law of Multiple Proportions If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first elements is always a ratio of small whole numbers.
Conservation of Atoms 2 H 2 + O 2 2 H 2 O John Dalton H H 2 H O 2 + H 2 H O H 2 O H H 4 atoms hydrogen 2 atoms oxygen Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3 rd Edition, 1990, page 204 4 atoms hydrogen 2 atoms oxygen
Legos are Similar to Atoms H 2 H H H O + O O 2 O H H H Legos can be taken apart and built into many different things. Atoms can be rearranged into different substances.
Law of Multiple Proportions John Dalton (1766 – 1844) If two elements form more than one compound, the ratio of the second element that combines with 1 gram of the first element in each is a simple whole number. e. g. H 2 O & H 2 O 2 water hydrogen peroxide Ratio of oxygen is 1: 2 (an exact ratio)
Daltons Atomic Theory • Dalton stated that elements consisted of tiny particles called atoms • He also called the elements pure substances because all atoms of an element were identical and that in particular they had the same mass.
Dalton’s Theory Continued • He also said the reason why elements differed from one another was that atoms of each element had different masses. • He also said that compounds consisted of atoms of different elements combined together. • Dalton's model was that the atoms were tiny, indivisible, indestructible particles and that each one had a certain mass, size, and chemical behavior that was determined by what kind of element they were.
Dalton’s Symbols John Dalton 1808
Daltons’ Models of Atoms Carbon dioxide, CO 2 Water, H 2 O Methane, CH 4
Dalton’s Atomic Theory 1. All matter is made of tiny indivisible particles called atoms. 2. Atoms of the same element are identical, those of different atoms are different. 3. Atoms of different elements combine in whole number ratios to form compounds 4. Chemical reactions involve the rearrangement of atoms. No new atoms are created or destroyed. California WEB
Dalton’s Atomic Theory 1. All matter consists of tiny particles. Dalton, like the Greeks, called these particles “atoms”. 2. Atoms of one element can neither be subdivided nor changed into atoms of any other element. 3. Atoms can neither be created nor destroyed. 4. All atoms of the same element are identical in mass, size, and other properties. 5. Atoms of one element differ in mass and other properties from atoms of other elements. 6. In compounds, atoms of different elements combine in simple, whole number ratios.
Structure of Atoms • Scientist began to wonder what an atom was like. • Was it solid throughout with no internal structure or was it made up of smaller, subatomic particles? • It was not until the late 1800’s that evidence became available that atoms were composed of smaller parts.
Thomson Model of the Atom J. J. Thomson - English physicist. 1897 Made a piece of equipment called a cathode ray tube. It is a vacuum tube - all the air has been pumped out.
A Cathode Ray Tube Source of Electrical Potential Stream of negative particles (electrons) Metal Plate Gas-filled glass tube Zumdahl, De. Coste, World of Chemistry 2002, page 58 Metal plate
A Cathode Ray Tube Zumdahl, De. Coste, World of Chemistry 2002, page 58
Thomson’s Experiment - voltage source vacuum tube metal disks +
Thomson’s Experiment - voltage source vacuum tube metal disks +
Thomson’s Experiment ON - OFF voltage source + Passing an electric current makes a beam appear to move from the negative to the positive end
Thomson’s Experiment ON - OFF voltage source +
Thomson’s Experiment ON - OFF voltage source + + By adding an electric field… he found that the moving pieces were negative.
The Effect of an Electric Field on Cathode Rays Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3 rd Edition, 1990, page 118
J. J. Thomson • He proved that atoms of any element can be made to emit tiny negative particles. • From this he concluded that ALL atoms must contain these negative particles. • He knew that atoms did not have a net negative charge and so there must be something balancing the negative charge. J. J. Thomson
Thomson • In 1910 proposed the Plum Pudding model – Negative electrons were embedded into a positively charged spherical cloud. Zumdahl, De. Coste, World of Chemistry 2002, page 56 Spherical cloud of Positive charge Electrons
Plum-Pudding Model Zumdahl, De. Coste, World of Chemistry 2002, page 56
Thomson Model of the Atom • J. J. Thomson discovered the electron and knew that electrons could be emitted from matter (1897). • William Thomson proposed that atoms consist of small, negative electrons embedded in a massive, positive sphere. • The electrons were like currants in a plum pudding. • This is called the ‘plum pudding’ model of the atom. electrons
Thomson’s Model • Found the electron • Couldn’t find positive (for a while) • Said the atom was like plum pudding • A bunch of positive stuff, with the electrons able to be removed - - -
Rutherford Model of the Atom
Ernest Rutherford (1871 -1937) • Learned physics in J. J. Thomson’ lab. • Noticed that ‘alpha’ particles were sometime deflected by something in the air. • Gold-foil experiment
Rutherford’s Apparatus beam of alpha particles radioactive substance circular Zn. S - coated fluorescent screen gold foil Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3 rd Edition, 1990, page 120
Rutherford ‘Scattering’ • In 1909 Rutherford undertook a series of experiments • He fired a (alpha) particles at a very thin sample of gold foil • According to the Thomson model the a particles would only be slightly deflected • Rutherford discovered that they were deflected through large angles and could even be reflected straight back to the source Lead collimator Gold foil a particle source q
Rutherford’s Apparatus beam of alpha particles radioactive substance fluorescent screen circular - Zn. S coated gold foil Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3 rd Edition, 1990, page 120
Rutherford’s Experiment Zumdahl, De. Coste, World of Chemistry 2002, page 56
He Expected • The alpha particles to pass through without changing direction very much • Because • The positive charges were spread out evenly. Alone they were not enough to stop the alpha particles California WEB
What he expected… California WEB
What he got… California WEB
Interpreting the Observed Deflections. . beam of alpha particles . . . . gold foil Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3 rd Edition, 1990, page 120 . . . undeflected particles . . deflected particle
Results of foil experiment if plumpudding had been correct. Electrons scattered throughout - + - positive charges + + - Zumdahl, De. Coste, World of Chemistry 2002, page 57 - + -
Explanation of Alpha-Scattering Results Alpha particles Nucleus + - + + - - + - + - Plum-pudding atom Nuclear atom Thomson’s model Rutherford’s model
Density and the Atom • Since most of the particles went through, the atom was mostly empty. • Because the alpha rays were deflected so much, the positive pieces it was striking were heavy. • Small volume and big mass = big density • This small dense positive area is the nucleus California WEB
Rutherford’s Gold-Foil Experiment Conclusions: Atom is mostly empty space Nucleus has (+) charge Electrons float around nucleus Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3 rd Edition, 1990, page 120
The Rutherford Atom Zumdahl, De. Coste, World of Chemistry 2002, page 323
Millikan’s Oil Drop Experiment Calculated the charge of an electron.
Oil Drop Experiment oil droplets . . . . . . . . . . . . . . . . . . . . . oil atomizer . . . . . . . . . . . . . . . . . . Charged plate + Small hole Charged plate Telescope oil droplet under observation
Particles in the Atom
Other pieces • Proton – (Goldstein) positively charged pieces – 1840 times heavier than the electron • Neutron – (Chadwick) no charge but the same mass as a proton. • How were these pieces discovered? • Where are the pieces?
Discovery of the Neutron + + James Chadwick bombarded beryllium-9 with alpha particles, carbon-12 atoms were formed, and neutrons were emitted. Dorin, Demmin, Gabel, Chemistry The Study of Matter 3 rd Edition, page 764
Atomic Review • William Thomson’s "plum pudding" model, published in 1904, showed that the model did produce electron arrangements that were stable. • Thomson’s model was conclusively destroyed by Rutherford's 1911 nucleus paper. • We know that atoms have a net neutral charge and they have positive and negative parts.
Particles in the Atom Electrons (-) charge no mass located outside the nucleus 1 amu located inside the nucleus Protons (+) charge Neutron no charge
Subatomic particles Name Symbol Charge Relative mass Actual mass (g) Electron e- -1 Proton p+ +1 1 1. 67 x 10 -24 Neutron no 0 1 1. 67 x 10 -24 1/1840 9. 11 x 10 -28
Structure of the Atom There are two regions The nucleus • With protons and neutrons – Positive charge – Almost all the mass Orbitals – Most of the volume of an atom – The region where the electron can be found
Size of an atom • Atoms are incredibly tiny. • Measured in picometers (10 -12 meters) – Hydrogen atom, 32 pm radius • Nucleus tiny compared to atom – Radius of the nucleus near 10 -15 m. – Density near 1014 g/cm • IF the atom was the size of a stadium, the nucleus would be the size of a marble. California WEB
Review Models of the Atom
Models of the Atom Dalton’s Greek model (400 (1803) B. C. ) Thomson’s plum-pudding model (1897) Bohr’s model (1913) Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3 rd Edition, 1990, page 125 Rutherford’s model (1909) Charge-cloud model (present)
Counting the Pieces Atomic Number = number of protons # of protons determines kind of atom Atomic Number = number of electrons in a neutral atom Mass Number = the number of protons + neutrons California WEB
Symbols Contain the symbol of the element, the mass number and the atomic number # protons + # neutrons mass number # protons Mass number Atomic number X
Symbols • Find the – number of protons = 9 + – number of neutrons = 10 – number of electrons = 9 – Atomic number = 9 – Mass number = 19 19 9 F
Symbols Find the – number of protons = 35 – number of neutrons = 45 – number of electrons = 35 – Atomic number = 35 – Mass number = 80 80 35 Br
Symbols Find the – number of protons – number of neutrons – number of electrons – Atomic number – Mass number 23 11 Na Sodium atom
Symbols Find the – number of protons = 11 – number of neutrons = 12 – number of electrons = 10 – Atomic number = 11 – Mass number = 23 23 11 Na Sodium ion 1+
Symbols If an element has an atomic number of 23 and a mass number of 51 what is the – number of protons = 23 – number of neutrons = 28 – number of electrons = 23 – Complete symbol 51 23 V
Symbols If an element has 60 protons and 144 neutrons what is the = 60 – Atomic number = 204 – Mass number – number of electrons = 60 – Complete symbol 204 60 Nd
Symbols If a neutral atom of an element has 78 electrons and 117 neutrons what is the – Atomic number – Mass number – number of protons – Complete symbol
Isotopes
Isotopes Dalton was wrong. Atoms of the same element can have different numbers of neutrons different mass numbers called isotopes C-12 California WEB vs. C-14
Isotopes of Magnesium 24 12 Atomic symbol 25 12 Mg 26 12 Mg Mg Number of protons 12 12 12 Number of electrons 12 12 12 24 Mass number Number of neutrons Isotope Notation Timberlake, Chemistry 7 th Edition, page 64 12 25 13 Mg-24 26 14 Mg-25 Mg-26
Naming Isotopes • Put the mass number after the name of the element • carbon- 12 • carbon -14 • uranium-235 California WEB
Isotopes of Hydrogen • Protium (H-1) 1 proton, 0 neutrons, 1 electron Most abundant isotope • Deuterium (H-2) 1 proton, 1 neutron, 1 electron Used in “heavy water” • Tritium (H-3) 1 proton, 2 neutrons, 1 electron radioactive
Isotopes of Three Common Elements Mass (amu) Fractional Abundance 12 12 (exactly) 99. 89% C 13 13. 003 1. 11% 35 17 Cl 35 34. 969 75. 53% 37 17 Cl 37 36. 966 24. 47% Si Si 30 Si 14 28 29 30 27. 977 28. 976 29. 974 92. 21% 4. 70% 3. 09% Mass Element Carbon Chlorine Silicon Symbol Number 12 6 C 13 6 28 14 29 14 Le. May Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 110 Average Atomic Mass 12. 01 35. 45 28. 09
Atomic Mass • • • How heavy is an atom of oxygen? There are different kinds of oxygen atoms. More concerned with average atomic mass. Based on abundance of each element in nature. Don’t use grams because the numbers would be too small California WEB
Measuring Atomic Mass • Unit is the Atomic Mass Unit (amu) • One twelfth the mass of a carbon-12 atom. • Each isotope has its own atomic mass we need the average from percent abundance. California WEB
Calculating averages • You have five rocks, four with a mass of 50 g, and one with a mass of 60 g. What is the average mass of the rocks? • Total mass = (4 x 50) + (1 x 60) = 260 g • Average mass = (4 x 50) + (1 x 60) = 260 g 5 5 • Average mass = 4 x 50 + 1 x 60 = 260 g 5 5 5 California WEB
Calculating averages • Average mass = 4 x 50 + 1 x 60 = 260 g 5 5 5 • Average mass =. 8 x 50 +. 2 x 60 • 80% of the rocks were 50 grams • 20% of the rocks were 60 grams • Average = % as decimal x mass + California WEB
Atomic Mass Calculate the atomic mass of copper if copper has two isotopes. 69. 1% has a mass of 62. 93 amu and the rest has a mass of 64. 93 amu. California WEB
Atomic Mass Magnesium has three isotopes. 78. 99% magnesium 24 with a mass of 23. 9850 amu, 10. 00% magnesium 25 with a mass of 24. 9858 amu, and the rest magnesium 26 with a mass of 25. 9826 amu. What is the atomic mass of magnesium? If not told otherwise, the mass of the isotope is the mass number in amu. California WEB Isotope Percent Abundance Mass Mg-24 78. 99 23. 9850 18. 94575 Mg-25 10. 00 24. 9585 2. 49585 Mg-26 11. 01 25. 9826 2. 86068 24. 304 amu
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