periodic trends. periodic trend ~noting a property that is regularly repeating. like noting all...
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Periodic Trends
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Periodic trend ~noting a property that is regularly
repeating. Like noting all elements in group
18 are gases. Or metals in group 11 don’t readily
rust.
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How to tell what is more reactive
Most reactive metals are down and to the left (most metallic)
Most active metal is Fr then Cs then Ra
Most reactive nonmetals are up and to the right, excluding the noble gases
most active nonmetal is F then O then Cl
As you move towards the center of the table elements become less active.
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Least Reactive Elements Least Active elements are the
Noble Gases Far right column of periodic table
(group 18) They are also called the inert
gases
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What causes reactivity of elements
All atoms want to have a completely full valence shell (normally 8 electrons).
For the moment we will only concentrate on main group elements
Noble gases are already full. Elements that are really close,
desperately want to get there (halogens and alkali), and tend to be the most reactive.
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Gaining electrons
metals lose electrons, nonmetals gain electrons and metalloids can go either way is a loose rule.
Obviously the quickest way for something that has more than 4 electrons to get to 8 is to gain electrons (through chemical bonds).
halogens want to gain 1, oxygen group wants to gain 2, nitrogen group wants to gain 3.
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Losing Electrons Metals will gain a full valence shell
by losing electrons. (there is a full shell underneath
unless it is hydrogen) alkali will lose 1 electron, alkaline
earth will lose 2 etc.
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Atomic Radii
atomic radius- how big an atom is (radius- distance from center of atom to edge)
As you add an energy level it gets bigger
As you add more protons (higher atomic #), there is more attractive force so it gets smaller
Energy levels have a greater effect than protons
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Largest and smallest So start big get smaller across a
period, then get bigger as you drop down a period
The element with the smallest atom is…
helium The element with the largest atom
is francium
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Ionization Energy
Ion- atom (or molecule) with a charge
Ions are created when you add or remove electrons (protons can’t be added or removed)
Ionization Energy- the energy required to remove an electron from an atom
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Ionization energy levels Atoms that want to give electrons
have a low ionization energy (metals)
Atoms that want to take electrons have a high ionization energy (nonmetals)
The noble gases have an even higher ionization energy
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Trends in ionization energy As you move from left to right Elements have a higher ionization
energy As you move down Elements have a lower ionization
energy This is because the electrons are
further from the nucleus so they are not held as tightly
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Electron affinity electron affinity- the ability of an
atom to attract and hold an electron This is measured by the amount of
energy that is released when the atom gains an electron
When energy is released it is a negative number
This means the lower the number, the more it wants an electron
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Periodic trends in electron affinity
All noble gases have a positive electron affinity, meaning it takes energy to make an electron stay there
(just about) Everything else releases energy
Halogens have the lowest electron affinity (meaning they release the most energy)
Generally as you go down and to the left it increases
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Organization of the periodic table
Graphing of all of these trends helped with the modern organization of the periodic table
When you graph these properties and others (like boiling and melting point) you see similar patterns reoccurring.
When you put the reoccurring patterns on top of each other you have organized them by our groups
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The graph looks like
Atomic Radii
Atomic number
Ato
mic
Ra
dii
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