Nomenclature
First things First….
 There are 3 main types of Compounds...
 Covalent
 Ionic
 Metallic
Ionic Compounds
 Ionic bonds are between Cations/anions
 In these bonds, the cation, metal, and anion,
nonmetal, do not share the electrons…instead, the
metal gives its electron to the nonmetal and the non
metal takes it.
Ionic
 To go from word form to written chemical formula
(letter form) we must use the charges.
Ionic
 To name these compounds, the metal keeps its
original name and the nonmetal changes its ending
from “ine” to “ide”
Ex: NaCl Sodium chloride
Ionic
 In order for this compound to be neutral, the charge
of the cations must equal the anions.
 Ex: BeF2 Beryllium Fluoride
 TiBr3
 Mn2(SO3)3
 Lithium Iodide
 Cobalt (III) Oxide
 Vanadium (IV) Carbonate
Ionic Compounds
 Although they ionic compounds are formed from
ions, these compounds are electronically neutral.
 Most ionic compounds are crystalline solids at room
temperature and have high melting points
 Chemical formula-the kinds and numbers of atoms in the
smallest representative unit of a substance.
 Formula unit-the lowest whole-number ratio of ions in an ionic
compound.
Ionic Compounds
 Octet Rule: in forming compounds, atoms tend to
achieve the electron configuration of a noble gas.
Octet is a set of 8.
 Therefore when an ionic compound bonds, the cation
will loose their outer electron and achieve noble gas
configuration in the lower energy level where as
anions achieve it in the current energy level by
gaining electrons.
Acids and bases
 For acids of of elements, hydro is added to the
beginning of the element and the ending is changed
to “ic”
 Ex: H2S Hydrosulfuric acid
 HCl Hydrochloric acid
Acids and Bases
 For acids containing polyatomic ions….
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Acids ending in ate change the ending to ic
Acids ending in ite change the ending to ous
Hydro will not be used in this case
Ex: H2SO4 sulfuric acid
HNO3
H3PO4
Sulfurous acid
Covalent
 A covalent bond occurs between two nonmetals.
 In these bonds, the elements in those bonds share
their electrons.
 There is a specific way that these compounds are
named.
Covalent
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In a covalent bond elements use a prefix to show the
number of atoms, shown by the subsript bonded in a
particular compound.
1-mono
 6-hexa
2-di
 7-hepta
3-tri
 8-octa
4-tetra
 9-nona
5-penta
 10-deca
Covalent
 To use these prefixes, we add them to the front of
the element
Ex: H2O The prefix for hydrogen would be
dihydrogen and oxygen would be monoxide
 The exception is if there is one one first element in the
name, there is no need to add a prefix
Ex: CO the C would have no prefix.
it would be carbon monoxide
Covalent
 The second half of naming a compound is the ending
 Change the ending on the second element to “ide”
 Ex: H2O would be dihydrogen monoxide
 CF4 would be carbon tetrafluoride
 Practice time!!!!!
Bonding of Covalent Bonds
 Use lewis dot structures and the octet rule to show
the bonding of a covalent bond.