Trends on the Periodic Table

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I see you are not up to date on your periodic trends

I scoff in your general direction! Look at that row! It's so last season.

Periodic Trends

• tendencies of certain elemental characteristics to increase or decrease as one progresses along a row or column of the periodic table of elements
• there are several trends that you must be able to describe to be trendy within this circle!
• metallic properties
• atomic radius
• ionization energy
• electronegativity
• reactivity
• ion charge
• melting/boiling point
• density

Metallic Properties

• properties change from metallic to non-metallic from left to right
• become more metallic going down a family in the periodic table

Atomic Radius

• Decrease going across row from left to right
• Increase going down a group
• as the number of protons in the nucleus of the atom increases, there is a greater force of attraction for the electrons in the shell and the distance between the electrons and nuclease decrease

Reactivity

• metals and non-metals show different trends
• when the metals move down and right it is more reactive
• when non-metals move left and up it is more reactive

Ion Charge

•  element charges depend on their group

Melting Point and Boiling Point

• elements in the centre of the table have the highest melting point
• noble gases have the lowest melting point
• start from the left and moving right; melting point increases until the middle of the table

Ionization Energy

• the energy needed to completely remove an electron from an atom
• increases going up and to the right
• all noble gases have ionization energy
• helium has the highest ionization energy and francium has the lowest
• opposite trend from the atomic radius
• measured in KJ/mol
• can have 1st ionization energy, 2nd ionization energy
• refer to the removal of more than one electron

Electronegativity

• refer to how much atoms want to gain electrons
• same trend as ionization energy
• tendency of an atom to attract electrons from a neighboring atom
• if atom has high EN
• strongly attract electrons and may completely remove them
• also strong attracted to own valence electrons=harder to remove
• if atom has low EN
• little tendency to remove electron from neighbor
• also has small attraction to own electrons
• low ionization energy=easily removable

VOILA! NOW AREN'T YOU ALL FANTABOULOUS READERS?!

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