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Electronic Configuration

Terms

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Hund's Rule
In p, d, and f orbital, first one electron fills each orbital and then pairing takes place
ionization energy
energy required to remove an electron from an atom
Aubuau Principal
Electrons occups lowest energy level
periods
the name gived to rows in periodic tables
electronegativity
the ability of an atom to attract the electrons of another atom towards istelf in a chemical bond
Atomic number
the modern periodic table of elements is arranged by this.
atomic radius
defined as half the distance between nuclei of identical atoms that are chemically bonded together
cation
formed when an atom looses electrons
Mendeleev's proposition
The chemical and physical properties of the elements increased gradually and suddenly changed at distinct steps, or periods
francium
has the lowest ionization energy
covalent bond
when the difference between the electronegativity of two atoms is less than 1.67
Drastic shift
occurs in chemical properties from left to right
shielding
represents the number of shells between the valence electron and the nulceus
silver metal solid at room temperature
sodium & lithium
periodic law
states that when elements are arranged in an order of increasing atomic number, they show a periodic repetition in their chemical and physical properties
Pauli's Exclusion Principle
Orbital can only hold two electrons, which should both have opposite spin
Stable nonmetals
oxygen, fluroine, and neon
ionic bond
when the difference between the electronegativity of two atoms is equal to or greater than 1.67
ionization energy
required to remove an electron from an atom
groups
the name given to coloumns in periodic tables
anion
when an atom gains electrons
electro negativity
ability of an atom to attract electrons from another atome involved in a bond
Henry Moseley
responsible for arranging the periodic so that an elements atomic number increased from left to right
1869
Year when Mendeleev first proposed chemical elements
fluorine
the most electronegatice element on the periodic table

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