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Comparing Ionic, Metallic and Covalent Bonds
characteristics of ionic, metallic and covalent bonds and compounds. One side has the characteristic; the other side has the bond/compound type
Has an empirical formula
Has a molecular formula
Held together by electrostatic force
Has high melting point
Has high boiling point
Good conductor of heat and electricity
metals lose electrons and form cations
non-metals gain electrons and form anions
Metal and Non-metal combines
form giant crystalline lattice solids
formed from non-metals only
held together by mutual attraction for electrons
Have molecular formulas
Have low melting points
Have low boiling points
Non-aqueous solutions do NOT conduct electricity
formed from metals
cations held together by sea of mobile valence electrons
form compact arrangement and orderly patterned crystals
Water is a common example
sodium chloride (table salt) is a common example
sugar is a common example
Compound may be solid, liquid or gas at room temperature.