Chapter 4 & 10 Notes

Inorganic Nomenclature:

IUPAC (International Union of Pure and Applied Chemistry) is the universally adopted system LEARN THESE SYSTEMS!!!

1. Binary Ionic Compounds

2. Pseudobinary Ionic Compounds

3. Binary Covalent Compounds

4. Binary Acids

5. Ternary Acids

6. Ternary salts

7. Ternary acid salts

Monatomic Ions

· Charges when a metal is combined with a nonmetal or a polyatomic anion

Group 1A = +1

Group 2A = +2

Group 3A = +3

Group 5A = -3

Group 6A = -2

Group 7A = -1

· Many transition metals have variable oxidation states

1. Binary Ionic Compounds

· Binary compound contains 2 different elements and the name has 2 words

1^st word: Name of the metal

2^nd word: Name of the nonmetal with ending changed to ide

Name the following:

KCl

Rb₂S

Al₂Se₃

Ca₃P₂

· Transition metals with more than one oxidation state, the oxidation state is specified in the name using roman numerals

Name the following:

Cu₂O

Fe₂S₃

Au₂S

PtCl₂

· Transition metal with only 1 oxidation state, the oxidation state is not specifie

Name the following:

AgCl

Zn₃N₂

CdS

2. Pseudobinary Ionic Compounds

· These contain more than two elements

· One or both of the words is a polyatomic ion

1^st word: Name of metal or polyatomic cation

2^nd word: Name of nonmetal or polyatomic anion

(Ending on 2^nd word is changed to ide only if it is a nonmetal, not if it is a polyatomic ion)

Partial List of Polyatomic Ions

Name	Formula	Name	Formula
hydroxide ion	OH^-	carbonate ion	CO₃^2-
cyanide ion	CN^-	sulfate ion	SO₄^2-
thiocyanate ion	SCN^-	sulfite ion	SO₃^2-
chromate ion	CrO₄^2-	phosphate ion	PO₄^3-
dichromate ion	Cr₂O₇^2-	oxylate ion	C₂O₄^2-
permanganate ion	MnO₄^-	thiosulfate ion	S₂O₃^2-
ammonium ion	NH₄⁺	hydronium ion	H₃O⁺
acetate ion	CH₃COO^-	hypochlorite ion	ClO^-
chlorate ion	ClO₃^-	chlorite ion	ClO₂^-
bromate ion	BrO₃^-	nitrate ion	NO₃^-
iodate ion	IO₃^-	nitrite ion	NO₂^-

Name the following :

NaOH

NH₄SCN

CuCN

CuSO₄

K₂S₂O₃

CaC₂O₄

3. Covalent Binary Compounds

· These contain 2 different nonmetals

1^st word : Name of nonmetal with prefix

2^nd word : Name of nonmetal with prefix and the ending

changed to ide

· Because nonmetals have such variable oxidation states, the oxidation state is specified for both elements using prefixes

Prefixes for Covalent Binary Compounds

Number	Prefix	Number	Prefix
1	mono	6	hexa
2	di	7	hepta
3	tri	8	octa
4	tetra	9	nona
5	penta	10	deca

· Mono is usually omitted except with CO

Name the following:

PCl₃ IF₅

PCl₅ HCl_(g)

Cl₂O₇ HBr_(g)

I₄O₉ HCN_(g)

NO₂ H₂S_(g)

N₂O₄ S₂F₁₀

NaH

4. Binary Acids

· The mono, di, tri, etc… prefixes are never used with acids

· These acids consist of hydrogen + a more electronegative atom

1^st word: Name of element or polyatomic ion with hydro

prefix and the ending changed to ic

2^nd word: acid

Name the following:

HCl_(aq)

HBr_(aq)

HCN_(aq)

H₂S_(aq)

5. Ternary Acids

· Also known as oxyacids, because they contain oxygen

· These acids consist of hydrogen + oxygen + a more electronegative element

· Again, the mono, di, and tri, etc… prefixes are never used

Common Ternary “ic” Acids

Formula	Name
HClO₃	chloric acid
HBrO₃	bromic acid
HIO₃	iodic acid
HNO₃	nitric acid
H₂CO₃	carbonic acid
H₂SO₄	sulfuric acid
H₃PO₄	phosphoric acid

· Other ternary acids differ from these by the number of oxygens they have

1^st word : Determined systematically using the

rules in the table below

2^nd word: acid

Naming Ternary Acids from “ic” Acids

# oxygens compared to “ic” acid	Name Change
+ 1	per prefix
-1	ic à ous
-2	ic à hypo--ous

Name the following:

HBrO_4(aq)

HNO₂ _(aq)

H₃PO_2(aq)

HIO_2(aq)

HClO_(aq)

6. Ternary Salts

· Result from replacement the acidic hydrogens in ternary acids with another cation

· Naming is like other ionic compounds

1^st word: Name of metal or polyatomic cation

2^nd word: Name of the polyatomic anion (acid derivative)

“ic” acid becomes à ate ending on acid derivative

“ous” acid becomes à ite ending on acid derivative

Name the following:

Na₂CO₃

(NH₄)₂SO₃

KIO

LiClO₄

Au(NO₃)₃

7. Ternary Acid Salts

· Results from replacement of only some of the acidic hydrogens in ternary acids with another cation

· Endings are like ternary salts

1^st word: Name of metal or polyatomic cation

2^nd word: Hydrogen

3^rd word: Name of the polyatomic anion (acid derivative)

“ic” acid becomes à ate ending on acid derivative

“ous” acid becomes à ite ending on acid derivative

NaHCO₃

NaHSO₄

K₂HPO₃

KH₂PO₃

· Note: the last 2 are distinguished by placing a prefix on H, not on potassium

Introduction to Aqueous Solutions

Strong Electrolytes

· Form lots of ions in aq solution ( ~ 100 %)

· Good conductors

Weak Electrolytes

· Form few ions in aq solution ( < 5 %)

· Poor conductors

Nonelectrolytes

· Form no ions in aq solution

· Nonconductors

Ion formation in Ionic Compounds:

· The process is called dissociation

Ion formation in Covalent Compounds:

· The process is called ionization

Acids

· Arrhenius definition says substances that produce H⁺ ions, hydrogen ions, or protons, when dissolved in water

monoprotic acids

diprotic acids

triprotic acids

Strong acids

· Strong electrolytes

· Form 100% ions in aq solution

· This non-reversible rxn goes to completion

· Single arrow forward

7 Strong Acids:

HCl _(aq) hydrochloric acid

HBr_(aq) hydrobromic acid

HI _(aq) hydroiodic acid

HNO₃ _(aq)nitric acid

H₂SO₄ _(aq)sulfuric acid

HClO_3
(aq)chloric acid

HClO_4
(aq)perchloric acid

Weak acids

· Weak electrolytes

· Form < 5% ions in aq solution

· This reversible rxn does not go to completion

· Double arrow forward and reverse

· All organic acids are weak, and the H is written at the end, not at the beginning as with inorganic acids (CH₃COOH, acetic acid

and C₆H₅COOH, benzoic acid)

Bases

· Arrhenius definition says substances that produce OH^-ions, hydroxide ions, when dissolved in aq solution

Strong bases

· Strong electrolytes

· Form 100% ions in aq solution

· This non-reversible rxn goes to completion

· Single arrow forward

8 strong, soluble bases:

LiOH CsOH

NaOH Ca(OH)₂

KOH Sr(OH)₂

RbOH Ba(OH)₂

Weak bases

· Weak electrolytes

· Form < 5% ions in aq solution

· This reversible rxn does not go to completion

· Double arrow forward and reverse

· Ammonia is the only weak base we will consider

· Most weak bases which are soluble, are salts

Insoluble bases

· Do not dissolve in water and therefore do not react

Salts

· Ionic compounds whose cations come from bases and whose anions come from acids

· If salts are soluble, they are strong electrolytes

· Determine the solubility from the solubility table handout

General Types of Reactions

I. Combination Reactions

· More than one reactant to form a single product

A. Element + Element à Compound

B. Compound + Element à Compound

C. Compound + Compound à Compound

II. Decomposition Reactions

· Single reactant to form more than one product

A. Compound à Element + Element

B. Compound à Compound + Element

C. Compound à Compound + Compound

III. Oxidation/Reduction Reactions (redox)

· Reactions that result in a change of oxidation numbers by transfer of electrons

· Before we continue we need to discuss oxidation numbers in more detail:

Oxidation Numbers (oxidation states)

· The number of electrons gained or lost when an atom or group of atoms

becomes ionized

General Rules for determining ox #:

Free elements or molecules: ox # = 0 (Fe, C, H₂, S₈ )

Monatomic ions : ox # = charge (Cl^‑,O^2-, Fe³⁺)

Polyatomic ions: ox # = charge (NH⁴⁺, SO₄^2-)

[this is actually the sum of the ox #’s on the individual atoms in the ion]

Neutral compounds: ox # = 0 (ZnSO₄, NaCl)
Many elements have ox #’s which apply to them in many cases:

Group IA = +1

Group IIA = +2

Group IIIA = +3

Group VA = -3

Group VIA = -2

Group VIIA = -1

H = +1

O = -2

· Sometimes these rules for ionic compounds apply with covalent molecules, and sometimes not.

Mnemonics for remembering REDOX:

OIL RIG Oxidation involves loss of electrons

Reduction involves gain of electrons

· Oxidations and Reductions always occur together, one species gains electrons and the other species loses electrons

· Let’s put together the two half reactions from above into a net ionic equation

Half-Reactions

· These are the oxidation and the reduction written out separately with the electrons included

· A reducing agent is oxidized, causing another substance to be reduced

· An oxidizing agent is reduced, causing another substance to be oxidized

A. Combustion

· Carbon/oxygen compounds or hydrocarbons burned in environmental oxygen

· A change in the oxidation number of C occurs

Reactions in Aqueous Solution:

· We will look at several types of reactions in aqueous solution in further detail

· Before we begin looking at these types of reactions in aqueous solution, we will look at how we will be analyzing them

Molecular equation

· Shows all the reactants and products in a balanced equation

· Formulas of compounds are written as if species are whole units

To write molecular equations, when only the reactants are given:

· Determine solubility or reactivity

· Write products

· Balance products using subscripts

· Balance eq using coefficients

Total ionic

· Shows compounds as they really exist, mostly or completely ionized or unionized, in aq solution

To write total ionic equations from molecular equations:

· Separate everything with _(aq) designation into ions, except weak acids and bases

Net ionic

· Shows just the species that actually participate in the reaction

To write net ionic equations from total ionic equations:

· Cancel all species which are exactly the same on the reactant and the product side of the arrow

· This is omission of the spectator ions

B. Displacement Reactions

· The first 3 types are based on the activity series

1. Type 1 Metal

A + BC à B + AC

[More active metal + salt of Less active metal] à

[Less active metal + salt of More active metal]

2. Type 2 Metal

A + HX à H_2(g) + AX

[Active metal + Nonoxidizing acid] à [Hydrogen + Salt of acid]

Nonoxidizing Acids: HCl and H₂SO₄

Active metal: any metal above H is the activity series

3. Type 3 Metal

A + H₂O à H_2(g) + AOH

[Active metal + Water à [Hydrogen + Salt of water]

· Must be one of the top 6 metals in the activity series to react with water

· It takes a metal with very low ionization energy to pick up the

OH^-from solution

· The total and the net ionic equations are combined

4 . Nonmetal

· In this case activity is based on the molecular weight

· The lighter halogen is the more reactive (active)

X + YZ à Y + XZ

[Active nonmetal + Salt of less active nonmetal] à

[Less active nonmetal + Salt of more active nonmetal]

IV. Metathesis Reactions (Double replacement)

· Means to transpose

· Positive and negative ions change partners to form new compounds with no change in oxidation numbers

AB + CD à AD + BC

A. Neutralization Reactions

· In most cases, the driving force is the combination of H⁺ and OH^- to form water

· This is always the case when both the acid and base are strong

acid + base à H₂0 + salt

1. Strong acid + Strong base:

2. Weak acid + Strong base:

3. Weak acid + Strong base:

B. Precipitation Reactions

· Formation of insoluble or slightly soluble solids are formed when 2 solutions containing soluble compounds are mixed

· The driving force is the strong attractions between cations and anions

· The solid, called a precipitate, separates from the solution

C. Gas-Formation Reactions

· Formation of insoluble or slightly soluble gases is the driving force

· The only common water soluble gases are HCl_(g) and NH_3(g)

Page Created by Anita Thurwachter

Last Updated 02/09/07