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Atomic Structure & Periodic Table Introduction
Physical Science
JPHancock
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The Atom
• Basic building block of all matter• Elements on periodic table are
represented as one neutral atom• Chemical symbols are abbreviated
ways of representing elements– C, H, N, O – Na, Cl, Ne, Cu– NaCl, H2O, CO2
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Parts of the Atom
• Protons= (+) charge• Neutrons= (0) charge• Electrons= (-) charge• Quarks= smallest particles arranged in
groups of threes to make p+, e-, or n0
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History of the Atomic Model
Aristotle 350BC
•Matter made up of earth, air, fire, and water
Democrit
us 400 BC
•Matter cannot be divided indefinately.
•“atomos = uncuttable”
Dalton
1803
•“Billard Ball Model” Atom solid and undivisible
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Thomso
n 1904
•“Plum Pudding Model” – a (+)sphere with (-) particles embedded
Rutherford 1911
•Most of the mass in a (+) nucleus surrounded by (-) electrons
Bohr
1913
•(+) protons & neutral neutrons in nucleus
•e- are in shells and can jump to higher levels with energy
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Rutherford Experiment
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Electron Cloud Model-1926
• “Probability Cloud”• Electrons orbit the
nucleus in energy levels or orbits.
• Why is it considered a “probability cloud”?
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EVOLUTION OF ATOM
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PERIODIC TABLE
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• The number of neutrons = mass number –atomic number
• In a neutral atom the number of e- and number of p+ are equal
• Every atom of the same element has the same number of protons
• MASS NUMBER =ATOMIC MASS
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ISOTOPES
• Atoms of the same element with different numbers of neutrons
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Atomic Mass Units• Do we now know how much atoms
really weigh, in pounds or grams?
• Yes, but we don't normally use those units for measuring the mass of an atom. It's much more convenient to use something called the atomic mass unit, or amu.
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Using AMU is simplier!
• One gram is about 600,000,000,000,000,000,000,000 amu (that's 600 sextillion, or a 6 followed by 23 zeros). A pound is just shy of 300 septillion amu--that is, 300,000,000,000,000,000,000,000,000. (26 zeros there.)
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Periodic Table
• 1869 Dmitri Mendeleev arranged the elements in order of their increasing atomic masses
• He discovered a pattern and was able to give rise to the modern
periodic table
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Mendeleev’s Periodic Table
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PERIODIC LAW
• The properties of elements are a periodic function of their atomic number– The properties change in a repeated
pattern as we move across or down the periodic table
– Elements are arranged by changes in physical and chemical properties
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MODERN PERIODIC TABLE
• 1913 Henry G.J. Moseley• Arranged the periodic table based on
increasing atomic numbers
• PERIODS or Series –horizontal rows 1-7• GROUPS or Families-vertical columns
1-18 with similar properties
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Properties of Groups
• Elements of same group have same # valence electrons– Valence electrons- are the e- in the
outermost energy level– Important role in chemical reactivity– Electrons closer to the nucleus have lower
energy than those farther away
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Properties of Series
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Ionization Energy
• Amount of energy needed to remove the outer electrons
• As you move right to left the radius of the nucleus increases meaning the size(distance) between the nucleus and electrons is greater
• As you move left to right the radius decreases meaning the electrons are valence electrons closer to the nucleus, held tighter and require more energy to remove
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Atomic Radii
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Electron Dot Diagrams
• Used to represent valence electrons in bonding