Unit 2: Molecular and Ionic Compound Structure and Properties

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