Naming Chemical Compounds

• First part: The name of the metal ion is the same as its element name. Use a roman numeral in parenthesis to indicate charge if variable.
• Space: A space separates the name of the cation from the name of the anion;
• Second part: The name of the nonmetal ion is obtained by using the first syllable of its element name followed by ide. If polyatomic, use appropriate suffix (ate or ite) and prefix (per or hypo).
• Subscripts: do not affect the name
• 

A Roman numeral that is equal to the ionic charge is placed in parentheses immediately after the name of the metal.

A group of covalently bonded nonmetal atoms that has an overall charge. Most are nonmetals such as P, S, C, or N covalently bonded to O atoms.

True. Exception: NH4+

True

• Cation is written first: usually a metal
• Anion is written second: usually a nonmetal

• ate: suffix for most polyatomic ions
• per: add prefix if 1 more O atom than -ate
• ite: suffix if one less O atom than -ate
• hypo: add prefix if 1 less O atom than -ite
• Exceptions: hydroxide (OH-) and cyanide (CN-) ions

• ClO4-: perchlorate
• ClO3-: chlorate
• ClO2-: chlorite
• ClO-: hypochlorite

If it is a transition element, except for zinc, cadmium, or silver, you need to use its ionic charge as a Roman numeral as part of its name. The ionic charge balances the negative charge of the anions.

• True
• 

True: except for zinc (Zn2+), cadmium (Cd2+) and silver (Ag+)

True: for example lead, tin, and bismuth

True: Fluorine, Clorine, Bromine, Iodine

• Bismuth (Bi): (III) and (V)
• Chromium (Cr): (II) and (III)
• Cobalt (Co): (II) and (III)
• Copper (Cu): (I) and (II)
• Gold (Au): (I) and (III)
• Iron (Fe): (II) and (III)
• Lead (Pb): (II) and (IV)
• Manganese (Mn): (II) and (III)
• Mercury (Hg): (I)-see note and (II)
• Nickel (Ni): (II) and (III)
• Tin (Sn): (II) and (IV)

Note: Hg(I) ions form an ion pair with a 2+ charge

• First nonmetal: named by its element
• Second nonmetal: named using the first syllable of its element name, followed by ide.
• Subscripts: use a prefix to indicate the number of atoms of an element
• 

• 1: mono (optional)
• 2: di
• 3: tri
• 4: tetra
• 5: penta
• 6: hexa
• 7: hepta
• 8: octa
• 9: nona
• 10: deca

acidus: Latin for "sour" (e.g., vinegar and lemons)

• Arrhenius: When dissolved in water, acids produce hydrogen ions (H+) and bases dissociate into hydroxide ions (OH-) and cations
• Brønsted-Lowry: acids can donate a hydrogen ion (H+); bases can accept one (need not contain OH- ions)
• Litmus paper: red
• Phenolphthalein: colorless

• Pronounced: fee-nol-thay-lean
• Phenolphthalein: C20H14O4
• Shorthand: HIn or phph

True: The negative ion may be a nonmetal anion or a polyatomic ion.

False: it bonds to water to form a hydronium ion, H30+

• Typical Arrhenius bases are named as hydroxides
• NaOH: sodium hydroxide (most common Arrhenius base)
• KOH: potassium hydroxide
• Ba(OH)2: barium hydroxide
• Ca(OH)2: Calcium hydroxide
• Al(OH)3: aluminum hydroxide

• Nonmetal anion: hydro is used before the name of the nonmetal anion with its ide ending changed to ic acid
• Polyatomic anion: ate is changed to ic acid or ite to ous acid
• Example 1: HCl is hydrochloric acid
• Example 2: HClO3 is chloric acid, HClO2 is chlorous acid

True: The name of its polyatomic anion ends in ate.

• Molecules or ions related by the loss and gain of one H+
• Example 1: HF (acid) donates a proton to F- (conjugate base)
• Example 2: H2O (base) gains a proton from H3O+ (conjugate acid)

True: its behavior depends on the other reactant

Substances that can act as either an acid or a base in water

• -ic acids: HF, HCl, HBr, HI, HCN, HNO3, H2SO4 (sulfuric), H2CO3 (carbonic), HC2H3O2 (acetic), H3PO4 (phosporic)
• -ous acids: HNO2 (nitous), H2SO3 (sulfurous), H3PO3 (phosphorous)
• 

• The acid donates a proton and the base accepts it
• After donating a proton the acid becomes its conjugate base
• After accepting a proton the base becomes its conjugate base
• One pair occurs in the each direction
•