Periodic Table Trends
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Transcript of Periodic Table Trends
![Page 1: Periodic Table Trends](https://reader035.fdocuments.in/reader035/viewer/2022062517/568136a6550346895d9e47e4/html5/thumbnails/1.jpg)
Periodic Table Trends
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• Dmitri Mendeleev arranged the elements in 1870 according to atomic mass and used the arrangements to predict the properties of missing elements.
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• The modern periodic table is arranged in order of increasing atomic number.
• The atomic number is the total number of protons in the nucleus.
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• Groups are vertical columns on the periodic table.
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• Periods are horizontal rows on the periodic table.
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• Three classes of elements are metals, nonmetals, and metalloids.
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Metals
• Metals are shiny, malleable (hammered into sheets), ductile (drawn into wires), solid at room temperature, and good conductors of electricity.
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Nonmetals• Nonmetals are poor conductors of electricity,
often gases at room temperature, and brittle if solid.
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Metalloids• Metalloids have some properties of metals
and nonmetals.• http://www.youtube.com/watch?v=CxjNGisjGi0
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• Group 1A - alkali metals (ex. Lithium)• Group 2A - alkaline earth metals (ex. Calcium)
• Group 7A – halogens (ex. Bromine)• Group 8A - noble gases (ex. Radon)
• Groups 1A through 7A - representative elements• Group B - transition metals (ex. Cobalt)
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Atomic Size
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The atomic radius increases from top to bottom in a group in the periodic table.
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As you move down a group in the periodic table, atomic size generally increases.
• WHY?• Adding more protons, neutrons and electrons
makes for larger atoms.
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The atomic radius decreases from left to right across a period in the periodic table.
• WHY?• Stronger pull on electrons to nucleus.
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• List the symbols for sodium, sulfur, and cesium in order of increasing atomic radii.
• Sulfur, Sodium, Cesium
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Ions and Ionization
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• Ions form when electrons enter or leave atoms.
• The charge of a cation is positive. Cations are smaller than the original atom.
• An anion has a negative charge. Anions are larger than the original atom.
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• Removing one electron from an atom results in the formation of an ion with a 1+ charge.
• Adding one electron to an atom results in the formation of an ion with a 1- charge.
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• Ionization energy - energy required to move an electron out of an atom
• Ionization energy decreases from top to bottom and increases from left to right on the periodic table.
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Among Na, K, and Cs, which element has the lowest ionization energy?
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• Cesium (Cs)
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Which is larger, K or K+?
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• K
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Which is smaller, Li, Li+, F, or F- ?
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• Li+
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Electronegativity
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• Electronegativity is the ability of an atom in a compound to attract electrons.
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• Electronegativity values tend to decrease from top to bottom and increase from left to right.
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• Which element in each pair has a higher electronegativity value?
• Mg or Ne • Mg
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• Which element in each pair has a higher electronegativity value?
• Cl or F• F
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• Which element in each pair has a higher electronegativity value?
• C or N• N
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• Which element in each pair has a higher electronegativity value?
• As or Ca• Ca
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• Cs has one of the lowest electronegativity values.
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Valence (outer) electrons may be transferred from one atom to
another.
Group Valence elctrons Resulting charge
1A Lose 1 1+
2A Lose 2 2+
3A Lose 3 3+
5A Gain3 3-
6A Gain 2 2-
7A Gain 1 1-
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• What charge would Na likely have in a compound? _______
• 1+• What charge would Mg likely have in a
compound? _______• 2+• What charge would Al likely have in a
compound? _______• 3+
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• What charge would O likely have in a compound? _______
• 2-• What charge would F likely have in a
compound? _______ • 1-
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