Unit 2: Molecular and Ionic Compound Structure and Properties Flashcards
(23 cards)
Substitutional alloys
occur when metals of similar radii combine.
electrostatic force
The elements are held together by because the positively charged cation is attracted to the negatively charged anion.
Noble gases
can sometimes bond because of their empty d- orbital.
potential energy
When two atoms are too close, the is high, and the nuclei reset each other.
Covalent substances
never conduct electricity, including pure water.
Metals
can be made into alloys.
anion
To bond, the cation gives up the electron (s) entirely to the .
Ionic substances
can not conduct as solids because of the electrons stuck in the lattice structure.
Interstitial alloys
occur when there are two metals with vastly different radii combine.
Network covalent bonds
as solids are held together in a lattice of covalent bonds which makes them very hard, very high melting point and boiling point.
sea of electrons
the electron organization for metallic bonds
ionic bonds
formed when a metal and nonmetal bonds
metallic bonds
formed when two metals bond
molecular covalent bonds
formed when two nonmetals bond
network covalent bonds
solids held together in covalent bonds (mainly containing carbon or silicon).
resonance forms
different, equivalent forms of drawing the same molecule in a lewis dot structure
formal charge
the most likely version of a lewis dot structure to form
molecular geometry
the three dimensional structure or arrangement of atoms in a molecule; based on the number of lone pairs and bonds
linear molecular geometry
two electron pairs
trigonal planar geometry
three electron pairs
tetrahedral geometry
four electron pairs
trigonal bipyramidal geometry
five electron pairs
octahedral geometry
six electron pairs
