Atomic radius: Difference between revisions

From Citizendium
Jump to navigation Jump to search
imported>David Yamakuchi
m (New page: {{subpages}} Our quantum mechanical description of an atom suggests a very broad region for finding the electron. It is difficult to define a sharp boundary f...)
 
imported>David Yamakuchi
mNo edit summary
 
Line 2: Line 2:
Our [[quantum mechanics|quantum mechanical]] description of an [[atom]] suggests a very broad region for finding the [[electron]]. It is difficult to define a sharp boundary for distance between the electrons in any particular atom and the nucleus. So some approximations are made in determining this parameter.<ref>http://intro.chem.okstate.edu/1314F00/Lecture/Chapter7/Lec111300.html</ref>
Our [[quantum mechanics|quantum mechanical]] description of an [[atom]] suggests a very broad region for finding the [[electron]]. It is difficult to define a sharp boundary for distance between the electrons in any particular atom and the nucleus. So some approximations are made in determining this parameter.<ref>http://intro.chem.okstate.edu/1314F00/Lecture/Chapter7/Lec111300.html</ref>


After collecting large amounts of data generally accepted atomic radii are known for most elements in the [[Periodic Table of Elements|periodic table]].  Atomic radius decreases from left to right across a period.  It is believed tis is due to stronger attractive forces in atoms (as you go from left to right) between the opposite charges in the [[nucleus]] and [[electron cloud]] cause the atom to be 'sucked' together a little tighter.  Atomic radius increases as you go down a group.  There is typically a significant jump in the size of the [[nucleus]] ([[protons]] + [[neutrons]]) each time you move from period to period down a group.
== Empirically measured atomic radii ==
 
After collecting large amounts of data generally accepted atomic radii are known for most elements in the [[Periodic Table of Elements|periodic table]].  Atomic radius decreases from left to right across a period.  It is believed this is due to stronger attractive forces in atoms (as you go from left to right) between the opposite charges in the [[nucleus]] and [[electron cloud]] cause the atom to be 'sucked' together a little tighter.  Atomic radius increases as you go down a group.  There is typically a significant jump in the size of the nucleus ([[protons]] + [[neutrons]]) each time you move from period to period down a group.


<references/>
<references/>

Latest revision as of 00:22, 3 April 2008

This article is a stub and thus not approved.
Main Article
Discussion
Related Articles  [?]
Bibliography  [?]
External Links  [?]
Citable Version  [?]
Catalogs [?]
 
This editable Main Article is under development and subject to a disclaimer.

Our quantum mechanical description of an atom suggests a very broad region for finding the electron. It is difficult to define a sharp boundary for distance between the electrons in any particular atom and the nucleus. So some approximations are made in determining this parameter.[1]

Empirically measured atomic radii

After collecting large amounts of data generally accepted atomic radii are known for most elements in the periodic table. Atomic radius decreases from left to right across a period. It is believed this is due to stronger attractive forces in atoms (as you go from left to right) between the opposite charges in the nucleus and electron cloud cause the atom to be 'sucked' together a little tighter. Atomic radius increases as you go down a group. There is typically a significant jump in the size of the nucleus (protons + neutrons) each time you move from period to period down a group.