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ionic bonding naming

QuestionAnswer
Compound definition Any combination of 2 or moredifferent elements
Binary Compound Any combination of two different elements, ex NaCl
Ternary Compounds Any combination of three different elements, ex: KCLO3
Endothermic Energy is required to break a chemical bond. Energy is the reactant. Surrounding area loses heat. End product is more potential energy.
Exothermic Energy is released when a chemical bond is formed. Energy is the product. Surrounding area gains heat. End product is less potential energy.
Ionic bonding Between metal and non-metal (ex: NaCl) where there is a larger difference in electronegativity values. Electrons transfer from M to NM. Results in + and - ions
Properties of ionic compounds Hard, high melting point, cannot conduct electricity as a solid, can conduct electricity as a liquid OR in an aqueous solution
IUPAC naming system Name of the metal, then root name of non-metal with ending of -ide
Oxidation Number identify how many electrons are either lost, gained or shared by an atom or ion as the result of a chemical reaction
Roman numerals are used for what? Only when the metal has more than one possible charge, tells you the charge of the metal ion (Ex: iron (II) is Fe2+)
Group 1 has what oxidation number +1
Group 2 has what oxidation number +2
In compounds, fluorine has what oxidation number -1
Elements other than fluorine in group 17 have what -1 if they are the most electronegative
Hydrogen has what oxidation number +1 in compounds unless with a metal then it is -1
Oxygen has what oxidation number -2 in compounds, +2 with F and -1 in peroxide ion
An ionic compound that contains a polyatomic ion has what Both ionic and covalent bonding (EX: CaCO3)
Metallic Bonding Occurs in a pure metallic element (ex, Cu) Positively charged ions surrounded by a “sea of mobile electrons” Attraction between kernels (+) and electrons (-)
Can metals dissolve in water No, not soluble
Created by: markoii
 

 



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