Naming ii smart

Unit 7Nomenclature IIHow to get the formula from the

name

Binary covalent compounds are compounds with two (2) nonmetals (Ex. CO, SF6, P2O5).

Binary Covalent Compounds


Determining the formula: Identify the elements in the compound. Confirm they are both nonmetals. Use the prefix to tell how many atoms of each element there are in the compound.

mono = 1 • di = 2 • tri = 3 • tetra = 4 • penta = 5

hexa = 6 • hepta = 7 • octo = 8 • nona = 9 • deca = 10


Determining the formula: To indicate how many atoms of each element are in the formula, use subscripts.

Example: carbon dioxide has1 carbon and 2 oxygens = C1O2 = CO2

(carbon’s 1 subscript is understood)




Practice: selenium tetrafluoride __________________________________ octaphosphorus pentabromide__________________________________ heptanitrogen hexachloride__________________________________ iodine trifluoride__________________________________



Acids

Acid - a compound that produces hydrogen ions, (H+) when dissolved in water. An acid will always end in the word "acid"! Also, an acid formula will always begin with hydrogen!

Acids

Finding the formula of an acid1) What kind of acid is it?

a. If it begins with “hydro”, it is binary, meaning hydrogen bound to a nonmetal.

b. If it does not begin with “hydro”, it is ternary, meaning hydrogen bound to a polyatomic ion.

Acids

Finding the formula of an acid2) Find the formula of a binary acid!

a. First, identify the nonmetal from the root of the word before acid.

Example: Hydrochloric Acidthe nonmetal is

chlorine.

Acids


b. Then, find the oxidation number of hydrogen (always 1+) and the nonmetal and write them as superscripts of each ion. This makes a cation(+) and an anion(–)

Example: H+1

Cl–1

Acids


c. Next, CRISS-CROSS the number of each oxidation number (NOT the charge!) down to the subscript of the opposite ion to indicate how many atoms you have of each ion in the compound.

Example:

H+1

Cl–1

= H1 Cl1

Acids


d. Reduce subscripts to lowest whole number ratio.

Example HCl(1 subscripts are understood)

Acids


Practice: Hydrochloric Acid_________________________________ Hydroselenic Acid_________________________________ Hydroiodic Acid_________________________________

Acids

Finding the formula of an acid3) Find the formula of a Ternary Acid!

a. Identify the polyatomic ion.i. If it ends in “-ous” acid,

change the end to “-ite”, look up on polyatomic ion list.

ii. If it ends in “-ic” acid, change the end to “-ate”, look up on polyatomic ion list.

Acids


b. Write the oxidation numbers of H and the polyatomic anion as superscripts

c. Criss cross the numbers only (not the charge!)

d. Reduce subscripts to lowest whole number ratio.

SAME AS

BINARY ACIDS

Acids


Practice: Chlorous Acid____________________________________ Sulfuric Acid____________________________________ Perchloric Acid____________________________________

Ionic Compounds

Ionic Compounds are made of a metal and a nonmetal (KCl, NaCl, NaI, CaCl2, BeF2).

Ionic Compounds

Determining the Formula of an Ionic Compound1) Identify the elements that make up the compound

a. The first term, the metal, is the cation (+) and will look the same as it does on the periodic table.

b. The second term, the nonmetal, is the anion (–) and its ending has been changed to"-ide”. Determine the element name from the root of the word.

Ionic Compounds

Determining the Formula of an Ionic Compound2) Form the cation and anion by looking at oxidation numbers.

3) Use the criss-cross method to form the compound.

4) Reduce subscripts to lowest whole numbers.

Ionic Compounds

Practice: sodium chloride ____________________________________________

magnesium fluoride ____________________________________________

aluminum iodide____________________________________________

calcium sulfide____________________________________________

Compounds withPolyatomic Ions

Polyatomic ions are groups of covalently bonded atoms that function as ions.

Compounds w/Polyatomic Ions

Determining the Formula:1) Identify the first term, the cation (+), and the second term, the anion (–)

a. the cation, anion, or BOTH may be polyatomic ions.

2) Form the cation and anion by looking at oxidation numbers.



Compounds w/Polyatomic Ions

Practice: Sodium cyanide________________________________

Aluminum nitrite________________________________

Ammonium silicate________________________________

Ionic Compounds w/ Transition Metals

Transition metals are the d block on the periodic table!


Determining the Formula from the Name:1) Identify the transition metal and the anion.

2) Form the cation and anion by finding the oxidation numbers of the ions.

a. transition metal - the Roman numeral

b. anion - periodic table groups or polyatomic ions




Practice: tin (IV) iodide__________________

mercury (II) sulfide______________

iron (III) oxide__________________

nickel (III) sulfate________________

chromium (VI) phosphate__________

Compounds w/Polyatomic IonsIon Name Ion Name

HCO3- hydrogen carbonate

CO32- carbonate

CN- cyanide CrO42-

chromate

C2H3O2-

acetate Cr2O72-

dichromate

ClO- hypochlorite SiO32- silicate

ClO2- chlorite SO32- sulfite

ClO3- chlorate SO42- sulfate

ClO4- perchlorate PO33- phosphite

MnO4- permanganate PO43- phosphate

NO2- nitrite NO3- nitrate

NH4+ ammonium OH- hydroxide

Business

Naming ii smart