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Periodic Trends
Description
Chemistry (Periodicity) Mind Map on Periodic Trends, created by cole.t75 on 28/02/2013.
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chemistry
periodicity
chemistry
periodicity
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cole.t75
, updated more than 1 year ago
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cole.t75
over 11 years ago
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Periodic Trends
Electronegativity
Annotations:
[Image: http://www.chemguide.co.uk/atoms/bonding/pteneg.GIF]
Electronegativity is a relative measure of attraction that an atom has for a shared pair of electrons when it covalently bonded with another atom
As size of an atom increases, the electronegativity decreases
The three most electronegative elements are F, N, and O
Ionic Radius
Annotations:
[Image: http://upload.wikimedia.org/wikipedia/commons/thumb/9/9f/Atomic_%26_ionic_radii.svg/300px-Atomic_%26_ionic_radii.svg.png]
Positive ions are cations negative ions are anions
Cations
Fewer electrons than protons
Therefore they are smaller than parent electron
Across the period, ions contain the same number of electrons
Anions
More electrons than protons
Therefore larger than parent atom
Proton number increases across the period
First Ionization Energy
Annotations:
[Image: http://mcat-review.org/ionization-energy.gif]
First ionization energy is the energy required to remove one electron from an atom in its gaseous state
The value decreases down the group as the outer electron is further from the nucleus so less energy will be required to remove it
Generally the values increase across the period
Tthe extra electrons are filling the same energy level and the extra protons in the nucleus attract this energy level closer - harder to remove
Atomic Radius
Annotations:
[Image: http://www.iun.edu/~cpanhd/C101webnotes/modern-atomic-theory/images/atomic-radii.jpg]
Atomic Radius is the distance from the outermost electron and the nucleus, this can never be exactly known
As you go down the group, the outermost electron has more energy - Group 1
The electrons closer to the nucleus have a greater pull on them
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