t he periodic table
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T he Periodic Table. Twelve elements have been known since ancient times. What do you think they are? (Name them, use your periodic table to help you.). T he Periodic Table. Twelve elements have been known since ancient times. What do you think they are? - PowerPoint PPT PresentationTRANSCRIPT
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The Periodic Table
Twelve elements have been known since ancient times. What do you think they are?(Name them, use your periodic table to help you.)
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The Periodic Table
Twelve elements have been known since ancient times. What do you think they are?(Name them, use your periodic table to help you.)carbon, sulfur, iron, copper, arsenic, silver, tin, antimony, gold, mercury, lead, bismuth
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The Periodic Table
Why do you think these particular elements have been known for so long, while most elements were not discovered until the 1800s and 1900s?
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Overview of the Periodic Table
Metals Metalloids Nonmetals Noble gases
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Overview of the Periodic Table
Metals Metalloids Nonmetals Noble gases
1. excellent heat conductor2. excellent electrical conductor3. lustrous (shiny)4. malleable, ductile5. silvery-gray, except Cu and Au6. solids at room T, except Hg
Some properties of metals, some properties of nonmetals1. moderate electrical conductivity2. appearance – more like metals – lustrous, silvery-gray3. brittle like nonmetals4. solids at room T
1. poor heat conductors
2. poor electrical conductors
3. not lustrous4. brittle5. variety of
colors6. gases or brittle
solids at room T
1. extremely unreactive – “inert”
2. rarely form compounds with other elements
3. colorless, odorless gases at room T
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Trends of the Periodic Table “periodic” = repeating pattern
Overall theme = electrons’ positions relative to each other and the nucleus determine the following properties:
4. Electron configuration5. Ionic radius
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Electron Configuration
Compare the charges on the ion list with the positionof the element in the periodic table
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Electron Configuration
• Noble gas configuration = [core] e-’s
• ‘Outer’ electrons = valence e-’s
• Elements of groups 1A-8A have valence e-’s in s and p orbitals
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Periodic Trends
The position of a valence electron and the ability to remove it from an atom are related to
• the number of protons in the nucleus
• the extent to which the valence electron is shielded from the positively-charged nucleus by the negatively-charged core electrons
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Isoelectronic Series
= a group of ions and atoms that have the same electron configuration
1. Draw the electron configuration of each of the following elements.
2. What ions will they form?
3. When ions, how many electrons does each have? How many protons?
4. Predict the relative diameters of the members of this isoelectronic
series.
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Isoelectronic Series Element Electron
configIon Ion
# e-’sIon # p+
OFNeNaMg
Prediction: smallest to largest:
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Isoelectronic Series Element Electron
configIon Ion
# e-’sIon # p+
O 1s22s22p4 1s22s22p6
O2- 10 e- 8 p+
F 1s22s22p5 1s22s22p6
F- 10 e- 9 p+
Ne 1s22s22p6 1s22s22p6
Ne 10 e- 10 p+
Na 1s22s22p63s1
1s22s22p6 Na+ 10 e- 11 p+
Mg 1s22s22p63s2
1s22s22p6 Mg2+ 10 e- 12 p+
Prediction: smallest to largest: Mg2+ < Na+ < Ne < F-< O2-
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Reminder: Atomic Radius
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Ionic Radius
• Cations (+) smaller than original atom– remove e-’s greater pull from
nucleus
• Anions (-) larger than original atom– Increased repulsion swells the shell
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Ionic Radius
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Ionic Radius1. In this table of ionic radii, how is the charge of the ions of elements in groups
1A-4A related to the group number?