periodic table trends. arrangement of the elements in order of their atomic numbers so that elements...
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Periodic Table Trends
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• Arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group
•What is it?
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• Group: vertical column of periodic table• Period: horizontal row of periodic table• Valence Electrons: electrons that occupy the highest energy level
• Up to 8• Atoms want to have full valence shell
• Ion: atom that has gained or lost an electron• Cation: atom loses electron; has + charge• Anion: atom gains electron: has - charge
• Important Terms
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• Silvery appearance• Can be cut by knife• Highly reactive with water• Usually not found in nature as a pure element• Always forms cations with +1 charge
• NOTE: Hydrogen, even though it is listed in group one, is NOT an alkali metal
• Alkali metals•Group 1
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• Similar to alkali metals, but harder, denser, and stronger
• Also not usually found in nature as a pure element• Always forms cations with +2 charge
• Alkaline-earth metals•Group 2
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• Good conductors of electricity• High luster• Less reactive than alkali and alkaline-earth metals
• Some do not easily form compounds!• Forms cations with varying charges
• Transition metals•Groups 3-12
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• Most reactive non-metals• React with metals to form salts• Always form anions with -1 Charge
• Halogens•Group 17
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• All electron shells full• Little to no chemical reactivity• Always has neutral charge
• Noble Gases•Group 18
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• Do not easily fit in any particular group, so these elements are usually separated in it’s own area on the periodic table
• All actinides are radioactive• Only 4 are found naturally
•Lanthanides and Actinides
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• Distance from the nucleus to the outer edge of electron cloud
• Increases as you go read down the group• Decreases as you read across the period
• Why?
• Atomic radiiPeriodic Properties
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• Distance from the nucleus to the outer edge of electron cloud after an atom has gained or lost an electron
• Groups 1-13 form cations (+)• Groups 15-17 form anions (-)
• Increase as you go read down the group• Cationic radii decrease as you read across the period• Anionic radii increase as you read across the period
• Why?
• Ionic radii
Periodic Properties
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• The energy needed to remove an electron from an atom
• Decreases as you read down a group• Increases as you read across a period
• Why?
• Ionization energyPeriodic Properties
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• Energy change that occurs when an electron is gained by a neutral atom
• Represented as a negative number• Decreases slightly as you read down a group• Greatly increases as you read across a period
• Why?
• Electron AffinityPeriodic Properties
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• The ability of an atom to attract an electron; only a property of atoms in compounds
• Decreases as you read down a group• Increases as you read across a period
• Why?
• ElectronegativityPeriodic Properties