3.2 Lecture 2008
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Transcript of 3.2 Lecture 2008
![Page 1: 3.2 Lecture 2008](https://reader036.fdocuments.us/reader036/viewer/2022081413/548297975806b501058b46f0/html5/thumbnails/1.jpg)
3.2 A Guided Tour of the Periodic Table
Pages 77 - 85
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Goal 1
Explain the relationship between the periodic table and the arrangement of electrons
within an atom.
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• Order based on number of protons
• Similar elements grouped together
• Similarities then occur in regular pattern
• Helps predict properties
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• Horizontal rows are called “periods”
• Can be used to determine electron arrangement
• Works up to element 20, Ca
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• Each horizontal row is an energy level
• Each square counts as an electron in that energy level
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Li has 3 electrons level 1 = 2e- level 2 = 1 e-
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N has 7 electrons Level 1 = __ Level 2 = __
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• Each vertical column is a Group
• Elements in a group have similar chemical properties
• Valence electrons 1, 2, 13-18
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Goal 2
Explain ion formation
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• Purpose of Ionization– Full outermost shell– Gain or lose valence electrons– Results in imbalanced electronic charge
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• Loss of electron yields “+” charge– Lose 1 electron 1+ charge– Lose 2 electrons 2+ charge– Lose 3 electrons 3+ charge
• Happens with small # of valence electrons
• Left-side of the periodic table– Which groups???
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• What will the charge be on the following ions?– H– Li– Ca– K– W
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• Gain of electrons yields “-” charge– Gain 1 electron 1- charge– Gain 2 electrons 2- charge– Gain 3 electrons 3- charge
• Happens with high # of valence electrons
• Which groups???
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• What will the charge be on the following ions?– F– Cl– S– P– N
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Goal 3
Use the periodic table to determine the number of protons, electrons, and
neutrons
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• Atomic number– Protons– Electrons
6 24
carbon12
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• Mass number– Protons + neutrons
6 24
carbon12
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• Protons = atomic number
• Electrons = atomic number
• Neutrons = mass number – atomic number
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Goal 4
Work with isotopes and average atomic mass
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• Isotopes– Same number of protons– Different number of neutrons– Chemical properties remain same– Mass number changes– Mass changes
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• Example – One atom of “Carbon”
• 6 protons• 6 neutrons• Atomic mass ~ 12
– One isotope atom of “Carbon – 14” • 6 protons• 8 neutrons !!!• Atomic mass ~ 14
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• How many neutrons are in the following isotopes?– Nitrogen -15– Sulfur – 35– Calcium – 45– Iodine - 131
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• The mass of atoms and isotopes
• Atomic mass unit1.0 amu = one proton = one neutron
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• Average atomic mass– Weighted average of isotopes– Nearest whole number indicates most
common isotope6 2
4
carbon12.011