Periodic Trends
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Transcript of Periodic Trends
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Periodic Trends
Still all about + and – charges!
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Which of the following atoms is the largest?
A. MgB. CaC. SrD. How the fluorine should I know?
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Which of the following atoms is the largest?
A. MgB. AlC. Cl
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Periodic for a Reason
It is a “periodic” table because of the “periodic trends” that make it up.
We saw that the electron configurations are periodic (s-block, p-block, d-block, etc.) and I suggested that the Chemistry associated with the atoms followed the electron configuration.
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Other Periodic Properties
Electron configuration isn’t the only periodic trend in the table.
The other important trends are all rationalizable based on the most important trend – atomic size!
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Atomic Size
Suppose we want to compare the atomic radius of two atoms on the periodic table, for example Na and K.
Which would you think is bigger?
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What does an atom look like?
Bohr Model
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The Bohr Model
Nucleusp
p p nn
nn
e-
e-e-
So, what determines the size of the atom?
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The size is determined by…
…where the last electron lies.
So, which is bigger Na or K?
K – it is Na with a whole extra shell of electrons!
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Na vs. K
Na: 1s22s22p63s1
K: 1s22s22p63s23p64s1
This is a general trend. As you go down a column in the periodic table, the atomic radius increases.
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What about the rows?
Suppose I ask the same question about Na and Mg; which is larger?
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Na vs. Mg
Na: 1s22s22p63s1
Mg: 1s22s22p63s2
Does this help us any?
They have the same valence shell (n=3). The same highest orbital (3s).
Does this mean they are the same size?
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Those pesky charges
What are the differences between Na and Mg?
One extra electron One extra proton
Does that help?
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The Bohr Model - Na
11 p
12 nfull
e-full
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The Bohr Model - Mg
12 p
12 nfull
e-full e-
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The Bohr Model – Na vs. Mg
12 p12 nfull
e-full e-
11 p
12 nfulle-
full
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Na vs. Mg
Same outer shell of the electrons (- charge).
More + charges in nucleus.
What do you think happens?
Mg is actually slightly smaller than Na due to the extra + charge in the nucleus pulling the – electrons in closer!
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Periodic Trend – atomic radius
This pair of observations describes the general trend of atomic size:
Larger as you go down a column (large effect)
Smaller as you go across the row (small effect)
Note: There are exceptions due to special cases (1/2 full orbitals, etc.)
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Rank from Largest to smallest
A. Sn, In, Ga, AsB. In Sn As GaC. In Sn Ga AsD. In Ga Sn As
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Periodic Trend – atomic radius
Both of these trends are related to the charged species:
Larger as you go down a column (more electron shells – adding layers)
Smaller as you go across the row (stronger attraction between more + protons and the outer electrons)
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Other Trends
Understanding the trend in atomic radius and keeping the charge issues in mind make it easy to understand and predict some other periodic trends.
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Ionization Energy
Ionization energy is the amount of energy required to remove an electron from an atom:
Na + energy Na+ + e-
(You simply raise the electron from n=valence to n=∞)
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Ionization Energy
Na + energy Na+ + e-
If you are going to remove an electron, what is the relevant issue?
Charge – what a surprise!
What Charge?
The nuclear charge! - At least in part
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Na vs. Mg
Compare the Ionization Energy of Na to that of Mg.
Which do you think would be larger?
Na or Mg
Why?
They have the same outer orbital, but Mg has a larger nuclear charge (sound familiar) – Mg should have the larger ionization energy!
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Larger Ionization Energy
A. SodiumB. MagnesiumC. I have no frigging idea
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Na vs. K
Compare Na to K, what is relevant?
K is bigger than Na – why?
Because K has more shells and larger radius. Electrons are farther from nucleus.
Same argument for ionization energy. Electron, farther away, less attracted to nucleus, smaller ionization energy!
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Ionization Energy vs. Atomic Radius
It is the same arguments, with the same results.
Ionization energy has a trend that tracks the radius. Smaller atoms, larger ionization energy!
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Electron Affinity
Electron Affinity is complementary to ionization energy. Rather than give up an electron, the atom receives it:
Na + e- → Na-
What will determine if an atom wants an electron?
Attraction for the nucleus – so electron affinity will also track atomic radius
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Electron Affinity
Na vs. K
K will have a smaller electron affinity – K is larger, a new electron is farther away, less attracted to nucleus
Na vs. Mg
Na will have a smaller electron affinity – same radius, smaller charge, less attraction for the electron.
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Electronegativity
Electronegativity is the ability of an atom to attract electrons to itself. (Kind of like electron affinity, but on a different scale)
Electronegativity is important in predicting whether a bond is ionic or covalent.
Electronegativity will have the same trend as electron affinity.