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6.3 summery-Deema Aldawood, image, image, image, image - Coggle Diagram
6.3 summery-Deema Aldawood
atomic radius
Atomic size is one such periodic trend. The sizes of atoms are influenced by electron configuration.
for metals, atomic radius is half the distance between adjacent nuclei in a crystal of the element
for elements that occur as molecules the atomic radius is half the distance between nuclei of identical atoms,
atomic radius decrease from left to right across a period caused by increasing atomic charge, the principal energy level (n) in a period remains the same, and valence electrons are not shielded because electrons are added in between. Increase as you move down a group as there is more energy levels which means less attraction between nucleus and valence electrons
ionic radius
Atoms can gain or lose one or more electrons to form ions.
Because electrons are negatively charged, atoms that gain or lose electrons acquire a net charge.
Both increase in size moving down a group
a positive ion is always smaller than an atom
The loss of a valence electron can leave an empty outer orbital resulting in a small radius.
Electrostatic repulsion decreases allowing the electrons to be pulled closer to the radius. They decrease from left to right group (15-18)(ore negative charge more repulsion)
A negative ion is always larger that an atom
When atoms gain electrons, they can become larger because the addition of an electron increases electrostatic repulsion.They decrease from left to right
ionization energy
Ionization energy is defined as the energy required to remove an electron from a gaseous atom. Is the energy required to move the first electron.
Atoms with low ionization energy values are likely to form positive ions
Atoms with high ionization energy values are likely to form negative ions
Removing the second electron requires more energy and is called the second ionization energy. Each successive ionization requires more energy, but it is not a steady increase
The increase in ionization energy shows that atoms hold onto their inner core electrons much more strongly than they hold onto their valence electrons.
electronrgativity
The electronegativity of an element indicates its relative ability to attract electrons in a chemical bond. Decrease down a group and increase from left to right across a period. Noble gas(18/8A) do not have electronegativity values they are stable.
