Chapter 6 The Periodic Table and Periodic Law. Historical Timeline Development of the Periodic...
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Transcript of Chapter 6 The Periodic Table and Periodic Law. Historical Timeline Development of the Periodic...
![Page 1: Chapter 6 The Periodic Table and Periodic Law. Historical Timeline Development of the Periodic Table.](https://reader036.fdocuments.net/reader036/viewer/2022081421/5697c0101a28abf838ccaef3/html5/thumbnails/1.jpg)
Chapter 6Chapter 6
The Periodic Table and Periodic Law
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Historical Timeline Development of the
Periodic Table
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Thursday and Friday
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6.1 Development of the Periodic Table
• Late 1790s
• Antoine Lavoisier
• compiled a list of all elements known at the time- 23 elements
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• 1800s- invention of electricity, development of spectrometer, and industrial revolution led to explosion in the number of known elements
• By 1870 there were 70 known elements
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• 1864• John Newlands • created law of octaves, which
means that properties repeat every 8th element
• Law doesn’t work for all elements
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• 1869
• Meyer and Mendeleev demonstrated a connection between atomic mass and elemental properties
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• 1869
• Mendeleev organized 1st periodic table by atomic mass and left blank spaces where undiscovered elements should go- not completely correct
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•1913• Moseley arranged elements
according to atomic number• Periodic Law – the periodic
repetition of chemical and physical properties of elements when they are arranged by increasing atomic number
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The Modern Periodic Table• Consists of boxes containing
element name, symbol, atomic number, and atomic mass
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Friday• We will finish the historical timeline of the periodic
table• We will color the two main sections of the periodic
table:• Representative elements• Transition elements• We will color in the metals and the nonmetals and
the metalloids
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• Representative Elements- main group of periodic table (1,2, and 13-18), s and p block; represent a wide range of chemical and physical properties
• Transition Elements- groups 3-12
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Classifying the Elements• Metals- elements that are
generally shiny, solids at room temperature, good conductors of heat and electricity, malleable (able to be pounded into thin sheets), and ductile (drawn into wires)
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• Nonmetals- generally gases or brittle, dull-looking solids; poor conductors of electricity
• Metalloids- elements with physical and chemical properties of both metals and nonmetals
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Monday• We will make a foldable over the different types of
groups in the periodic table
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The Families of the modern Periodic Table
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• Alkali Metals- Group 1A (1)
• Alkaline Earth Metals- Group 2A (2)
• Both groups are chemically reactive
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• Transition Metals- Group B elements (d block)
• Inner Transition Metals- (f block)
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• Halogens- Group 7A (17); highly reactive
• Noble Gases- Group 8A (18); extremely unreactive
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Classifying the Elements• S-block elements
–groups 1A and 2A
–Holds a maximum of two electrons
• P-block elements group 3A through 8A, or 13-18
Holds a maximum of 6 electrons
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• d-block elements– contains transition metals
– largest block– holds maximum of 10 electrons
• f-block elements– contains inner transition metals
– lanthanide and actinide series
– holds maximum of 14 electrons
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Tuesday - Exploration Activity• Lab over the periodic trends of the Periodic
Table
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Wednesday• We will do trends on the periodic table• Compare our notes to he lab from Tuesday
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6.3 Periodic Trends• Atomic Radius
generally increases from right to left and increases from top to bottom of the periodic table
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• Adaptive Curriculum Clip
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Atomic Size
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•Ionic Radius- positive ions decrease from left to right until group 3A (13), then negative ions decrease until 8A (18); generally increases from top to bottom
•Ion- atom or bonded group of atoms that has a positive or negative charge
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Cation –positively charged ion (lost electron)–Will decrease radius because of loss of outer energy level–Are in groups 1-13
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Anions–negatively charged ion (gained
electron)–will increase radius because
protons “pulling in” are the same and with extra electrons they repel each other and spread out
–groups 14-18
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Atomic and Ionic radius follow the
same trend!!
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Ionization Energy
• energy required to remove an electron from a gaseous atom
• generally decreases from right to left and decreases from top to bottom
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Electronegativity• indicates the relative ability of its
atoms to attract electrons in a chemical bond
• decreases from right to left and decreases from top to bottom
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Follows the same trend as electronegativity!!
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Thursday• We will finish our lab• We will finish our review and check it in
class
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Friday• We will test on Friday