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Covalent CompoundsCovalent Compounds
Covalent BondsCovalent Bonds Atoms of two nonmetals combinedAtoms of two nonmetals combined Held together by sharing electrons Held together by sharing electrons
““co” means cooperate/shareco” means cooperate/share ““valent” refers to the valence electronsvalent” refers to the valence electrons
Atoms bonded with covalent bonds are called Atoms bonded with covalent bonds are called moleculesmolecules
Covalent moleculesCovalent molecules
Atoms with covalent Atoms with covalent bonds share electrons bonds share electrons to achieve an octet for to achieve an octet for
each of themeach of them Some elements exist Some elements exist
in nature as in nature as diatomic moleculesdiatomic molecules
= molecules that = molecules that contain two like contain two like
atomsatoms* Note the names* Note the names
Sharing Electrons Between Sharing Electrons Between Atoms of Different ElementsAtoms of Different Elements
The number of The number of electrons that an electrons that an atom shares and atom shares and the number of the number of covalent bonds it covalent bonds it forms are usually forms are usually equalequal to the to the number of number of electrons needed electrons needed to acquire a noble to acquire a noble gas arrangementgas arrangement
ExceptionsExceptions Although the nonmetals typically form octets,…
Some (P, S, Cl, Br, and I) can share more valence electrons and form stable valence shells of 10 or 12 electrons
1A 3A 4A 5A 6A 7AH
1 bond
B3 bonds
C4 bonds
N3 bonds
O 2 bonds
F1 bond
Si 4 bonds
P3 (or 5) bonds
S2 (4 or
6)bonds
Cl, Br, I1 (3 or
5)Bonds
Multiple Covalent BondsMultiple Covalent Bonds
In many covalent compounds, atoms may share 2 or 3 pairs of electrons to complete their octets
Double bond 2 pairs of e- shared Triple bond 3 pairs of e- shared C, O, N, and S are most likely to form
multiple bonds Atoms of hydrogen and the halogens do
not form double or triple bonds
Naming Covalent Naming Covalent CompoundsCompounds
1st nonmetal uses its elemental name
2nd nonmetal uses its elemental name with the –ide ending
Subscripts are expressed as prefixes placed in front of each name
Prefixes fornaming covalent
numbers used incompounds
1 Mono
2 Di
3 Tri
4 Tetra
5 Penta
6 Hexa
7 Hepta
8 Octa
9 Nona
10 Deca
The names of covalent compounds need prefixes because several different compounds can be formed from the same two nonmetals
Ex) carbon + oxygen can form CO (carbon monoxide) or CO2 (carbon dioxide)
In the name of a covalent compound, the prefix mono is usually omitted on the 1st atoms name
When the vowels o and o or a and o appear together, the first vowel is omitted
Practice naming covalent compounds
Name each of the following covalent compounds:a) NCl3 b) N2O4
Nitrogen trichloride Dinitrogen tetroxide
Write the formula of sulfur dichloride.SCl2
Naming and Writing FormulasNaming Binary Molecular Compounds
The prefix tells how many atoms of each element are present in each molecule of the compound
Carbon Monoxide vs. Carbon Dioxide
Mono- indicates one oxygen
Di- indicates two oxygens
Naming and Writing FormulasGuidelines for Naming
1) Confirm the compound is a molecular compound (2 nonmetals)
2) Omit mono- when the the formula contains only one of the first element in the name
3) Add -ide to the second element in the formula
Guidelines for Formula Writing
1) Use the prefixes in the name to tell you the subscripts in the formula
Naming and Writing FormulasPractice
Write the name of these molecular compounds:
a) NCl3
b) BCl3
c) NI3
d) SO3
e) N2H4
f) N2O3
Naming and Writing FormulasPractice
Write the formulas for these binary molecular compounds:
a) Phosphorus pentachloride
b) Iodine heptafluoride
c) Chlorine trifluoride
d) Iodine dioxide
e) Carbon tetrabromide
f) Diphosphorus trioxide
Summary of naming rulesSummary of naming rulesBinary Compounds (may be ionic or covalent)
State the 1st element, followed by the 2nd element with an –ide ending
If 1st element is
a metal = ionic compoundnonmetal = covalent compound
Ionic compounds Is the 1st able to form more than one ion? …
…if so, use Roman numerals to indicate charge
Compounds with polyatomic ions use –ate or –ite endings (determined by # of oxygens)
* Exception NH4+ written 1st
Covalent compounds Prefixes are needed to show # of atoms of each
nonmetal in the formula
Organic CompoundsOrganic Compounds