Unit 3 Part 1 Atomic Structure
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Transcript of Unit 3 Part 1 Atomic Structure
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Unit 3 Part 1Atomic Structure
ICPMr. Patel
SWHS
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Topic OutlineLearn Major ElementsThe Atom Subatomic Particles Modern Atomic Theory Organizing the ElementsPeriodic TableClassifying ElementsAtomic Models
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Defining the AtomAtom – the smallest particle of an
element that retains its identityCan not see with naked eyeNanoscale (10-9 m)Seen with scanning
tunneling electronmicroscope
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DemocritusDemocritus was a Greek to first
come up with idea of an atom.
His belief: atoms were indivisible and indestructible. = WRONG!
Atom comes from “atmos” - indivisible
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Dalton’s Atomic Theory2000 yrs later, John Dalton used
scientific method to transform Democritus’s idea into a scientific theory
Dalton put his conclusions together into his Atomic Theory (4 parts)
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Dalton’s Atomic Theory1. All elements are composed of
indivisible atoms.
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Dalton’s Atomic Theory2. Atoms of the same element are
identical. Atoms of different elements are different
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Dalton’s Atomic Theory3. Atoms of different elements can
chemically combine in whole number ratios.
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Dalton’s Atomic Theory4. Atoms of one element can never be
changed to another element
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The ElectronParticle with negative charge
Discovered by J.J. Thomson
Used cathode ray (electron) beam and a magnet/charged plate.
Millikan found the charge and mass
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The Proton and NeutronAn atom is electrically neutral
If there is a negative particle then there must be positive particle
Proton – particle with positive charge
Chadwick discovered neutron – neutral charge
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Thomson’s Atomic ModelElectrons distributed in a sea of
positive chargePlum Pudding Model
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Rutherford’s Gold Foil Experiment
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Rutherford’s Atomic ModelThe nucleus is the central part of the
atom containing protons and neutronsPositive chargeMost of the mass
Electrons are located outside the nucleusNegative chargeMost of the volume
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Atomic Number An element is defined only by the
number of protons it contains
Atomic Number – number of protons
Number of protons = number of electronFor a neutral element
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Identify the number of Protons1. Zinc (Zn)
2. Iron (Fe)
3. Carbon (C)
4. Uranium (U)
1. 30
2. 26
3. 6
4. 92
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Mass NumberNucleus contains most of the mass
Mass Number – total protons and neutrons
Number of neutron = Mass # – Atomic #
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Identify # of Subatomic Particles1. Lithium
(MN = 7)
2. Nitrogen(MN = 14)
3. Fluorine(MN = 19)
**MN = Mass Number
1. 3 p+ , 3 e-, 4 n0
2. 7 p+ , 7 e-, 7 n0
3. 9 p+ , 9 e-, 10 n0
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Differences in Particle NumberDifferent element: different number of
protons
Ions – same number of proton, different number of electrons
Isotope – same number of proton, different number of neutronsDifferent Mass Numbers
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Two Notations for AtomsNuclear Notation
Write the element symbolOn left side, superscript = Mass NumberOn left side, subscript = Atomic Number
Isotope –Hyphen NotationWrite full name of elementOn right side, put a dashOn right side put Mass Number after dash
Hydrogen - 3
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Ex: Three isotopes of oxygen are oxygen-16, oxygen-17, and oxygen-18. Write the
nuclear symbol for each.
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Ex: Three isotopes of chromium are chromium-50, chromium-52, and chromium-53. How many neutrons are in each isotope?
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Ex: Calculate the number of neutrons for 99
42Mo.
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Atomic MassAtomic Mass Unit (amu) – one-twelfth of
the mass of the carbon-12 atom
Different isotopes have different amu (mass) and abundance (percentage of total)
Atomic Mass – weighted average mass of the naturally occurring atoms.Isotope MassIsotope Abundance
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Atomic MassBecause abundance is considered, the
most abundant isotope is typically the one with a mass number closest to the atomic mass.
Example, Boron occurs as Boron-10 and Boron-11. Periodic Table tells us Born has atomic mass of 10.81 amu.Boron-11 must be more
abundant