Elements close to eachother on the periodic table display similar characteristics
There are 7 important periodic trends:
1) Reactivity2) Ion Charge
3) Melting Point
4) Atomic Radius5) Ionization Energy
6) Electronegativity
7) Density
1) REACTIVITY
- metals and non-metals shoe different trends
- the most reactive metal is Francium; the most reactive non-metal is Fluorine
-reactivity increases as you go down for metals and up for non-metals-Noble gases are very unreactive
2) ION CHARGES
- elements ion charges depend on their group (column)
3) MELTING POINT
- elements in the centre of the table have the highest melting point
- noble gases have the lowest melting points
- starting from the left and moving right, melting point increases (until the middle of the table, it then starts to decrease)
-an exception to this rule is Carbon. Carbon has a high melting point!
4) ATOMIC RADIUS
- radius decrease to the up and the right
- Helium has the smallest atomic radius
- Francium has the largest atomic radius
- ionization energy is the energy needed to completely remove an electron from an atom
- it increases going up and to the right
- all noble gases have high ionization energy- Helium has the highest I.E.
- Francium has the lowest I.E.
- opposite trend from atomic radius
-Quick note: think about why Ionization energy has the opposite trend of the Atomic radius. Since the atomic radius gets smaller when ionization energy increases, it tells us that when the shells are smaller, the energy needed to completely remove an electron is easier, therefore, electrons can leave their small atomic radius which is an increase in ionization energy.
-Quick note: think about why Ionization energy has the opposite trend of the Atomic radius. Since the atomic radius gets smaller when ionization energy increases, it tells us that when the shells are smaller, the energy needed to completely remove an electron is easier, therefore, electrons can leave their small atomic radius which is an increase in ionization energy.
6) ELECTRONEGATIVITY
- refers to how much atoms want to gain electrons- same trend as I.E.
7) DENSITY
...yet to be learned!
and our own pictures!
Post by: Adrienne Ross (with pictures from Ren Flores)
Great Help!
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keep doing what you are doing...! :)
this is pretty darn cool! :D
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ReplyDeleteQuick correction - you have the correct trend for ionization energy but your explanation is flawed. An increase in ionization energy corresponds to an increase in difficulty removing an electron from the outermost shell (recall that the definition of ionization energy is the energy required for removal). It opposes atomic radius because the smaller the radius, the stronger electrons are attracted to the nucleus and the harder it is to pull them away. Inner shells "shield" outer shells from the attractive force of the nucleus, so as atoms increase in size, ionization energy decreases.
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