Naming inorganic compounds

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Naming inorganic compounds

NAMING INORGANIC COMPOUNDS

Inorganic compounds are often classified as ionic and covalent. The method for naming these compounds is slightly different. We will first look at naming ionic compounds and then covalent compounds.

Naming Ionic Compounds

To name ionic compounds you have to recognize that the compound is ionic. An ionic compound consists of the combination of metal and nonmetal elements. You also need to know which metal ions form only one possible ion. The elements in groups IA, IIA, and IIIA (except Tl), can only form one ion. The charge of the ion is the same as the group number. For monoatomic nonmetal ions, take the group number and subtract eight, i.e., oxide ion is -2 since oxygen is in group VIA, so 6 - 8 gives -2 for the ion charge. The polyatomic ions must be memorized. You should know the formula and the charge for a select number of these ions. Refer to any general chemistry text for a table of polyatomic ions which are of common use. Armed with this knowledge, let's look at naming some ionic compounds.

1. Name the cation (usually the metal ion) using the same name as the element. If the metal forms only one ion, a Stock number (Roman numeral) is not needed. For elements forming more than one ion, use the Stock number (a Roman numeral) following the element name. Do not put a space between the metal name and the Stock number. The Stock number is the same as the charge of the ion. For example, Na+, would be named as sodium ion, since sodium can only form a +1 ion. On the other hand, Cu2+, would be called copper(II) ion since copper can form both a +1 and a +2 ion.

2. If the anion is monoatomic, take the first syllable (sometimes two syllables) of the element name and use the prefix -ide. So O2- becomes oxide, Cl- becomes chloride, etc. Where more than one syllable of the element name is needed is usually obvious: I- is iodide, Se2- is selenide, etc. If the anion is polyatomic, use the name of the polyatomic ion. These ion names must be memorized. So, SO42- is sulfate, NO3- is nitrate, etc.

3. The cation is always named first, followed by the anion.

4. Unless you are starting a sentence, names of compounds are not capitalized.

Here are some examples for you to try. The correct names are found at the end of the tutorial:

1. NaBr ______________________________

2. CaSO4 _____________________________

3. K2S _______________________________

4. Ni(NO3)2 ___________________________

5. Mg3N2______________________________

6. Fe2(CO3)3 ___________________________

7. Cr2O3 ______________________________

8. Ti(ClO4)4 ____________________________

9. AlCl3 _______________________________

10. PbC2O4 ____________________________

Naming Binary Covalent Compounds

Naming covalent compounds is easier than ionic compounds. To indicate how many of an element is present, prefixes are used:

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

1. Name the first element in the compound as the element. If more than one of that element is found in the formula, use the appropriate prefix. Note that mono is never used as a prefix for the first element, when only one of that element is present.

2. Name the second element using the appropriate prefix to indicate how many and the -ide suffix at the end of the name, just as if the element were a monoatomic ion. If the element begins with a vowel, and the prefix ends with the letter a, drop the letter a in the prefix.

Here are some examples for you try. The correct names are given at the end of the tutorial:

1. CO _______________________________

2. CO2 ______________________________

3. S2F6 ______________________________

4. P4O10 _____________________________

5. N2O4 _____________________________

6. NCl3 ______________________________

7. PBr5 ______________________________

8. SiS2 _______________________________

9. N2F4 ______________________________

10. SeBr2 _________________________________

Naming Acids

1. Some acids are formed by the addition of hydrogen ions, (H+), to a monatomic anion. To name an acid which contains a monatomic anion, drop the start the name with hydro, drop the -ide ending of the anion and add the suffix, -ic acid. For example, HBr is hydrobromic acid.

2. Oxyacids contain polyatomic anions such as nitrite, carbonate, etc. To namean acid with an anion ending with the -ite suffix, drop the -ite suffix and add the suffix, -ous acid. For example, HNO2 , would be name as nitrous acid. To name an acid with an anion ending with the -ate suffix, drop the -ate suffix and add the suffix, -ic acid. For example, H2CO3 , would be named carbonic acid.

3. The oxyacids of the Group VII elements (halogens) have more complex names because there are four different possible oxyanions. The -ite/ous acid and -ate/ic acid changes still apply, the only difference is the additional prefixes of hypo- or per- are carried along in both the anion and the acid name.

Here is an example using chlorine as the halogen:

ClO- is hypochlorite ion; the corresponding acid name is hypochlorous acid, HClO.

ClO2- is chorite ion; the corresponding acid name is chlorous acid, HClO2.

ClO3- is chlorate ion; the corresponding acid name is chloric acid, HClO3.

ClO4- is perchlorate ion; the corresponding acid name is perchloric acid, HClO4.

Answers to problems in naming ionic compounds:

1. sodium bromide

2. calcium sulfate

3. potassium sulfide

4. nickel(II) nitrate

5. magnesium nitride

6. iron(III) carbonate

7. chromium(III) oxide

8. titanium(IV) perchlorate

9. aluminum chloride

10. lead(II) oxalate

Answers to naming binary compounds:

1. carbon monoxide

2. carbon dioxide

3. disulfur hexafluoride

4. tetraphosphorus decoxide

5. dinitrogen tetroxide

6. nitrogen trichloride

7. phosphorus pentabromide

8. silicon disulfide

9. dinitrogen tetrafluoride

10. selenium dibromide

© Copyright, 2001, L. Ladon. Permission is granted to use and duplicate these materials for non-profit educational use, under the following conditions: No changes or modifications will be made without written permission from the author. Copyright registration marks and author acknowledgement must be retained intact.

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Naming inorganic compounds

NAMING INORGANIC COMPOUNDS

Introduction

A primary control in chemical experiments is knowing the identity of the initial substances. This knowledge can be communicated by the name of the substances and labels on reagent containers. The following sections describe systematic names for simple inorganic compounds. These systematic names can be assigned from the chemical formula, and then the name communicates the chemical formula.

Binary Covalent Compounds

Covalent compounds can be operationally defined as compounds that do not conduct electricity when pure and in the liquid state. These compounds, with few exceptions, are composed of nonmetal elements only. Binary covalent compounds are composed of two nonmetal elements, and the name for the compound is constructed from the chemical formula in the following manner:

Prefix + name of 1st element Prefix + stem of 2nd element + ide

The stem of an element is formed by dropping the last syllable of the element's name. Prefixes are assigned by the number of atoms of each element in the formula, and the prefix corresponding to a given number of atoms can be found Table 1. The prefix "mon" is dropped with the exception of carbon monoxide, and the suffix "ide" is used with all two element compounds. Carbon dioxide is a familiar example of a systematic name. The name tells us what elements compose carbon dioxide, the number of atoms of each element, and hence the chemical formula of carbon dioxide. Note, a compound that appeared on the Internet was dihydrogen oxide, what is the formula of this compound? The following examples may help you answer this question.

Example 1--What is the formula of sulfur hexafluoride?

The elements composing the compound are S and F. Also the prefix hex says there are 6 F atoms so the formula is SF₆.

Example 2--Please name the compound N₂O₄?

The name is dinitrogen tetroxide.

Table 1--Prefixes for number of atoms

Number of atoms	Prefix
1	mon
2	di
3	tri
4	tetra or tetr*
5	penta or pent*
6	hexa or hex*

*The first spelling is used if the stem of the element begins with a consonant and the second spelling if the stem of the element begins with a vowel.

Binary Ionic Compounds

Ionic compounds are operationally defined as compounds that conduct electricity when pure and in the liquid state. All ionic compounds are solids at room temperature and with a few exceptions composed of a metal and nonmetal elements. When the metal is a group IA element, group II A element, or aluminum, the name is assigned using the form:

metal stem of nonmetal element + ide

This system does not use prefixes and assumes a knowledge of the law of electrical neutrality, the octet rule, and ionic theory. Ionic theory states that ionic compounds are composed of positive and negative ions formed by the transfer of valence electrons between atoms or molecules. The attraction between the oppositely charged ions bonds the ions together in the solid state. In the liquid state the electrical attraction is much weaker, and the ions are mobile. This explains why ionic compounds conduct electricity only in the liquid state. Electrical neutrality requires the total positive and negative charge on the ions be equal and that no valence electrons are lost or gained by the transfer of electrons between atoms and molecules. The octet rule is used to assign changes on the ions composing a compound, and states that group IA and IIA elements and aluminum loose their valence electron while nonmetals gain electrons until the total number of valence electron is eight. The following examples illustrate the naming system and the chemical principles.

Example 1- The mineral fluorite has the chemical formula CaF₂ . What is fluorite's systematic name?

The names of the elements composing fluorite are

calcium and fluorine.

The last syllable of fluorine is changed to ide and the name is calcium fluoride.

Example 2- What is the chemical formula of cesium sulfide?

The compound is composed of cesium and sulfur. From the Periodic Table and the Octet Rule, we have

Cs has 1 valence e^– loses 1 e^–

S has 6 valence e^– gains 2 e^–.

To make electrons lost equal electrons gained, two cesium atoms lose electrons so we have

2 Cs have 2 valance e^– loose 2 e^–

S has 6 valance e^– gains 2 e^–

and the formula of cesium sulfide is Cs₂S. Note the ions composing cesium sulfide are Cs⁺ and S^2–.

There are many other examples of metal elements, and these metals are called transition metals (elements in columns headed with a B), inner transition metals (metals in block separated from Periodic Table), or post-transition metals (all Group IIIA--VIA metals except aluminum). A property common to all of these metals is the formation of stable ions with different charges depending on the conditions under which the ion is formed. For ionic compounds with these metals, the systematic name is:

metal(Roman numeral) stem of nonmetal + ide.

The Roman numeral equals the charge on the metal ion. The following examples show how the names in these compounds are assigned and used to determine the chemical formula from the name.

Example 1--The color of ruby and sapphire is due to a small quantity of Cr₂O₃ in these gem stones. What is the systematic name of Cr₂O₃?

The charge on the "B" metal is determined from the nonmetal. From the periodic table and the octet rule

O has 6 valence e^– gains 2

and for the compound

3 O have 18 valence e^– and gained 6.

Since electrons lost equals electrons gained, the chemical formula says

2 Cr have lost 6 e^–

and then

Cr has lost 3 e^–.

The name of the compound is Chromium(III) oxide.

Example 2--The compound Lead(IV) oxide is used in car batteries. What is the chemical formula of Lead(IV) oxide?

Pb has lost 4 e^– (from Lead(IV))

O has 6 valence e^– gains 2 e^– (from Periodic Tale and Octet rule)

To make electrons lost equal electrons gained, multiply O by two

Pb has lost 4 e^–

2 O have 12 valence e^– gain 4 e^–.

The chemical formula is PbO₂.

Ionic compounds with Polyatomic or Complex ions

Polyatomic or Complex ions are examples of molecules that have lost or gained valence electrons. The names of ionic compounds with negative complex ions end in "ite" or "ate" with a few exceptions. The most common exceptions are compounds which contain the following complex ions:

OH^– hydroxide ion

CN^– cyanide ion

O₂^2– peroxide ion.

The names of compounds with these ions consist of the metal and the anion. For example, the poison NaCN has the name sodium cyanide.

Many complex ions have the general formula NMO_m^n–, and the names of ionic compounds containing these ions are constructed in the manner:

metal stem of nonmetal + ate or ite.

The "ate" ion always has one more O atom than the "ite" ion. For example SO₄^2– is sulfate ion and SO₃^2– is sulfite ion. For a specific nonmetal, knowing the charge and number of oxygen atoms in the "ate" ion is sufficient to remember the formula and charge in the "ite" ion. Table 2 lists six "ate" ions and these are best memorized. The formulas of other ions can be derived from these ions and periodic law. In writing formulas with complex ions, multiple complex ions are enclosed in parenthesis but single complex ions are not enclosed in parenthesis. Some examples illustrating the names of compounds with complex ions follow.

Example 1--Phosphate rock has the chemical formula Ca₃(PO₄)₂. What is the systematic name of phosphate rock?

The names of the component elements excluding oxygen are

calcium phosphorous

and since PO₄ is the formula of phosphate ion the name is calcium phosphate.

Example 2--A preservative has the name sodium nitrite. What is the chemical formula of the preservative?

Nitrite ion refers to the ion NO₂^– which has gained 1 e^–

Na has 1 valence e^– loses 1 e^–.

Since electrons lost equals electrons gained, the chemical formula is NaNO₂.

Example 3--What is the charge on the complex ion in the compound Na₂C₂O₄?

The charge is determined from the "A" metal

Na has 1 valence e^– loses 1 e^–

and since the formula has 2 Na ions, the number of electrons lost is

2 Na have 2 valence e^– lose 2 e^–.

and electrical neutrality requires that

C₂O₄^n– gains 2 e^–.

The charge is –2 (C₂O₄^2–).

Table 2--Names and formulas of common oxyanions

Ion	Name
CO₃^2–	carbonate ion
NO₃^–	nitrate ion
SiO₄^4–	silicate ion
PO₄^3–	phosphate ion
SO₄^2–	sulfate ion
ClO₃^–	chlorate ion

Acids

Acids are operationally defined as compounds that form sour tasting solutions, turn blue litmus paper pink, have a pH less than 7, and chemically react with bases to neutralize acid and base properties. Theoretically acids donate hydrogen ions (H⁺) and produce hydronium ion (H₃O⁺) in water. The formulas of these compounds are written with acid hydrogen first. For example, H₂SO₄ is the chemical formula of sulfuric acid and indicates two acidic H. The systematic name of a binary acid, H_nX where X is a nonmetal element, is assigned using the format

Hydro + stem of nonmetal element + ic acid.

The chemical formula of a binary acid can be determined from the name by determining the charge predicted by the octet rule for the nonmetal element and then balancing this charge with the appropriate number of hydrogen ions. Examples 1 and 2 below illustrate the application of these rules.

Oxyacids are another common group of acids, and the chemical formulas for these compounds have the form H_nNMO_m. The name of an oxyacid has the form

stem of nonmetal + ous or ic acid.

For a specific nonmetal, the ous acid always has one less oxygen than the ic acid. The correct ending can be selected by treating the acid as an ionic compound composed of hydrogen ions (H⁺) and a complex ion, applying electrical neutrality to assign the charge on the complex ion, naming the complex ion, and then changing the ite ending to ous acid or the ate ending to ic acid. The procedure is reversed to determine the chemical formula from the systematic name. Also, the system can be extended to less or more oxygens by adding the prefix hypo to the ous acid for one less oxygen and the prefix hyper to the ic acid for one more oxygen. Examples 3 and 4 illustrate the systematic naming of oxyacids.

Example 1--H₂S is a foul smelling gas that forms an acidic solution when dissolved in water. What is the acid name of H₂S?

The compound is a binary acid and the name is

hydrosulfuric acid.

Example 2--Hydrofluoric acid is used to etch glass. What is the chemical formula of hydrofluoric acid?

The nonmetal is fluorine and the the octet rule predicts

F has 7 valence e^–- gains 1 e^–; F^–

H has lost 1 e-; H⁺

The chemical formula is HF.

Example 3--One of the acids found in acid rain has the chemical formula H₂SO₃. What is the name of this acid?

The acid has two acidic H hence

2 H have lost 2 e^–; 2 H⁺

SO₃ has gained 2 e^–; SO₃²^-.

The name of the complex ion is sulfite ion, and the name of the acid is sulfurous acid.

Example 4--Carbonic acid is present in all carbonated beverages. What is the chemical formula of carbonic acid?

The ic ending says the acid may be treated as composed of carbonate ion and hydrogen ion. The corresponding chemical formulas are

CO₃^2– has gained 2 e^–

H⁺ has lost 1 e^–,

and electrical neutrality says

CO₃^2– has gained 2 e^–

2 H⁺ have lost 2 e^–.

The chemical formula of carbonic acid is H₂CO₃.

Chemistry 1000 exercise on Inorganic Nomeclature

1. The correct scientific name for the mineral hematite, Fe2O3, is

a)iron oxide

b)iron(III) oxide

c)diiron trioxide

2. Please name the following

a)AsF3

b)Al2S3

c)TiO2

d)CoCl2

e)Cr(OH)3

3.Please write the formula for

a)Manganese(III) phosphite

b)Strontium fluoride

c)Sodium nitrate

d)Dinitrogen pentoxide

e)Potassium carbonate

4.Please write the chemical formula and charge for

a) sulfide ion

b) sulfate ion

Source : http://www.baruch.cuny.edu/wsas/academics/natural_science/chm_1000/inorg_nom.doc

Web site link: http://www.baruch.cuny.edu/wsas/academics/natural_science/chm_1000

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Naming inorganic compounds

NAMING INORGANIC COMPOUNDS

Memorize:
1) symbols and English names of elements
(see Periodic table, groups IA - VIIIA and IIIB - IB, the most important ones are listed in the table attached)

2) Latin names of elements
(from the names symbols of elements are derived)

3) names of common cations and anions
(see attached tables)

4) common names of selected compounds:

Formula	Systematic Name	Common Name	Use
NH₃	Hydrogen nitride	Ammonia	cleaner
CO₂	Carbon dioxide	Dry Ice (solid)	freezing substance
N₂O	Dinitrogen oxide	Laughing gas or nitrous oxide	anesthetic
NO	Nitrogen monoxide	Nitric oxide	biological active compound
CaCO₃	Calcium carbonate	Limestone	marble, chalk, make cement
NaCl	Sodium chloride	Table salt	seasoning
H₂O	Hydrogen oxide	Water	drinking, washing
H₂O₂	Hydrogen peroxide	Peroxide	antiseptic, bleaching agent
HCO₃^-	hydrogen carbonate	bicarbonate	blood buffering
NaHCO₃	Sodium hydrogen carbonate	(Baking) soda	antacid, fire extinguisher


Keep in mind the rules:
1) names of binary and ternary compounds are derived from the names of cations, anions and polyatomic ions
2) all binary compounds end in -ide
	e.g. CaO = Calcium oxide, H₂O₂ = Hydrogen peroxide, NaCl = Sodium chloride,
	HF (g) = Hydrogen fluoride (g = gas)

3) binary compounds composed of two nonmetals: Greek prefixes are used to indicate the number of atoms
of each element in the compound
	Greek prefixes:	mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-
		(1, 2, 3, 4, 5, 6, 7, 8, 9, 10)

	e.g. SO₂ = Sulfur dioxide, N₂O₅ = Dinitrogen pentoxide, CO = Carbon monoxide
	(when two vowels appear next to each other, the vowel of Greek prefix is dropped;
	the prefix mono- is never used for naming the first element of a compound)

4) binary compound composed of metal ion with fixed or variable oxidation numbers and nonmetal ion:
the metal ion is named by both the -ous / -ic suffix system and the Stock system (oxidation number
written in a parenthesis, it is prefered); no Greek prefixes are used

	e.g. CuCl₂ = Copper(II) chloride or cupric chloride (-ic means "a higher oxidation number")
	CuCl = Copper(I) chloride or cuprous chloride (-ous means "a lower oxidation number")
	(English name) (derived from Latin name of the cation)

	Fe₂O₃ = Iron(III) oxide or ferric oxide (-ic means "a higher oxidation number")
	FeO = Iron(II) oxide or ferrous oxide (-ous means "a lower oxidation number")
	The suffixes -ous and -ic do not mean the same oxidation numbers in naming of different
	compounds !!! However -ic always means higher and -ous lower oxidation state of a metal.

5) ternary compounds are composed of hydrogen ion H⁺ (see below) and/or metal ion with fixed (e.g. Mg)
or variable (e.g. Fe) oxidation numbers, and a polyatomic ion (e.g. SO₃^2- or SO₄^2-)
	e.g. H₂SO₃ = Sulfurous acid / MgSO₃ = Magnesium sulfite (-ous / -ite) - sulfur is present as S⁴⁺
	H₂SO₄ = Sulfuric acid / MgSO₄ = Magnesium sulfate (-ic / -ate) - sulfur is present as S⁶⁺

	The suffix -ite is used for an anion with lower oxidation number of a central atom (see S),
	whereas the suffix -ate is for an anion having a higher oxidation state of the same central
	atom. If only one oxidation state of the central atom is possible the suffix -ate is used.

	a metal forming more cations (variable oxidation numbers)
	FeSO₄ = Iron(II) sulfate or Ferrous sulfate (iron is present as Fe²⁺)
	Fe₂(SO₄)₃ = Iron(III) sulfate or Ferric sulfate (iron is present as Fe³⁺)

6) hydrogen compounds that yield hydrogen ions in water solution are called acids
	*binary: HCl (l) = Hydrochloric acid* whereas HCl (g) = Hydrogen chloride !!! (l = liquid, g = gas)

	exception: HCN (l) = Hydrocyanic acid (prefix Hydro- although it is a ternary compound; it is
	an oxygen-free acid)

	ternary: H₂CO₃ = Carbonic acid (its anion = carbonate, so the suffix for acid must be -ic, see point 5)
	HNO₂ = Nitrous acid (its anion = nitrite, so the suffix for the acid must be -ous)

	HClO = Hypochlorous acid (anion = hypochlorite)		Cl¹⁺
	HClO₂ = Chlorous acid (anion = chlorite)		Cl³⁺
	HClO₃ = Chloric acid (anion = chlorate)		Cl⁵⁺
	HClO₄ = (Hy)perchloric acid (anion = perchlorate)		Cl⁷⁺

	The prefixes hypo- (= under) and per- (or hyper- = above) are used if more than two
	oxidation states are formed by a central atom (e.g. all halogens).

7) bases are substances that contain a metal ion and a hydroxide aion; the suffix: -ide
	e.g. NaOH = Sodium hydroxide, Fe(OH)₃ = Ferric hydoxide

8) salts are formed when one or more of the hydrogen ions of an acid is replaced by a cation
	e.g. NaH₂PO₄ = Sodium dihydrogen phosphate
	Na₃PO₄ = Trisodium phosphate

9) acid salts are salts that contain one or more hydrogen atoms bonded to the anion
	e.g. NaH₂PO₄ = Sodium dihydrogen phosphate

10) hydroxy salts are salts that contain one or more hydroxide ions together with their own anion
	e.g. Ca(OH)Cl = Calcium hydroxychloride

11) double salts are salts containing two different cations or anions
	e.g.KLiSO₄ = Potassium lithium sulfate
	Cu₃(CO₃)₂F₂ = Copper(II) carbonate fluoride

12) hydrates are salts containing one or more molecules of water bonded to their molecule
	e.g. CoCl₂ . 6 H₂O = Cobalt(II) chloride hexahydrate

13) thioacids or thiosalts are compounds in which one oxygen was replaced by sulfur atom
	e.g. H₂S₂O₃ = Thiosulfuric acid
	Na₂S₂O₃ = Sodium thiosulfate

Names of elements			Common metals and their cations

Symbol	Latin	English	Metal	Group	Common Cations	Cation Name
H	Hydrogenium	Hydrogen	Lithium	IA	1+	Lithium
Li	Lithium	Lithium	Sodium	IA	1+	Sodium
Na	Natrium	Sodium	Potassium	IA	1+	Potassium
K	Kalium	Potassium	Beryllium	IIA	2+	Beryllium
Be	Beryllium	Beryllium	Magnesium	IIA	2+	Magnesium
Mg	Magnesium	Magnesium	Calcium	IIA	2+	Calcium
Ca	Calcium	Calcium	Strontium	IIA	2+	Strontium
Sr	Strontium	Strontium	Barium	IIA	2+	Barium
Ba	Baryum	Barium	Aluminium	IIIA	3+	Aluminium
B	Borum	Boron	Tin	IVA	2+	Tin(II) or stannous
Al	Aluminium	Aluminium			4+	Tin(IV) or stannic
C	Carboneum	Carbon	Lead	IVA	2+	Lead(II) or plumbous
Si	Silicium	Silicon			4+	Lead(IV) or plumbic
Sn	Stannum	Tin	Bismuth	VA	3+	Bismuth
Pb	Plumbum	Lead	Iron	VIIIB	2+	Iron(II) or ferrous
N	Nitrogenium	Nitrogen			3+	Iron(III) or ferric
P	Phosphorus	Phosphorus	Cobalt	VIIIB	2+	Cobalt(II) or cobaltous
As	Arsenicum	Arsenic			3+	Cobalt(III) or cobaltic
Sb	Stibium	Antimony	Copper	IB	1+	Copper(I) or cuprous
Bi	Bismuthum	Bismuth			2+	Copper(II) or cupric
O	Oxygenium	Oxygen	Silver	IB	1+	Silver
S	Sulfur	Sulfur	Gold	IB	3+	Gold(III)
Se	Selenium	Selenium	Zinc	IIB	2+	Zinc
F	Fluorum	Fluorine	Cadmium	IIB	2+	Cadmium
Cl	Chlorum	Chlorine	Mercury	IIB	1+	Mercury(I) or Hydrargyrous
Br	Bromum	Bromine			2+	Mercury(II) or Hydrargyric
I	Iodium	Iodine
He	Helium	Helium	Common nonmetals and their anions (suffix -ide)
Ne	Neon	Neon
Ar	Argon	Argon	Nonmetal	Group	Anion	Anion Name
Kr	Krypton	Krypton	Fluorine	VIIA	1-	Fluoride
Xe	Xenon	Xenon	Chlorine	VIIA	1-	Chloride
Rn	Radon	Radon	Bromine	VIIA	1-	Bromide
Cr	Chromium	Chromium	Iodine	VIIA	1-	Iodide
Mo	Molybdaenum	Molybdenum	Hydrogen	IA	1-	Hydride
W	Wolframium	Tungsten	Nitrogen	VA	3-	Nitride
Mn	Manganum	Manganese	Phosphorus	VA	3-	Phosphide
Fe	Ferrum	Iron	Oxygen	VIA	2-	Oxide
Co	Cobaltum	Cobalt	Sulfur	VIA	2-	Sulfide
Ni	Niccolum	Nickel
Pt	Platinum	Platinum
Cu	Cuprum	Copper
Ag	Argentum	Silver
Au	Aurum	Gold
Zn	Zincum	Zinc
Cd	Cadmium	Cadmium
Hg	Hydrargyrum	Mercury

Common polyatomic cations

Formula	Cation Name
NH₄⁺	Ammonium
H₃0⁺	Hydronium

Common polyatomic anions

Formula	Anion Name
OH^-	Hydroxide
CN^-	Cyanide
CO₃^2-	Carbonate
NO₂^-	Nitrite
NO₃^-	Nitrate
PO₄^3-	Phosphate
SO₃^2-	Sulfite
SO₄^2-	Sulfate
CrO₄^2-	Chromate
MnO₄^-	Permanganate
ClO^-	Hypochlorite
ClO₂^-	Chlorite
ClO₃^-	Chlorate
ClO₄^-	Perchlorate

Suffixes in English and the related ones in Latin

	lower cation	higher cation	lower anion	higher anion
English	ous	ic	ite	ate
Latin	osi	i	is	as


	lower anion	related lower acid	higher anion	related higher acid
English	ite	ous	ate	ic
Latin	is	osum	as	icum


	binary compounds, hydroxides and CN^-
English	ide
Latin	idum

Source : http://old.lf3.cuni.cz/chemie/english/premedical_course/inorganic.doc

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Naming inorganic compounds

INORGANIC NOMENCLATURE

All chemical compounds can be classified into two categories: organic compounds and inorganic compounds. Both categories of compounds have different systems of naming rules.

Organic compounds are compounds based on carbon. Most carbon-containing compounds are classified as organic (exceptions: carbon dioxide, carbon monoxide, and carbonates). All other compounds are considered to be inorganic compounds, and we will be learning some of the rules for naming these compounds.

Binary Compounds: When The First Element is Monovalent

A binary compound is an inorganic compound that contains 2 elements.

This is the method you use when the first element in the compound is monovalent.

Rules for Writing a Name From a Formula

1. Write down the name of the first element in the chemical formula. This is the element with the lower electronegativity, and it is usually a metal.

2. Remove the ending on the name of the second element and replace it with “ide”.

Examples: KI potassium iodide

AlCl₃ aluminum chloride

Na₂S sodium sulfide

Try these: MgS

Ag₂O

CaCl₂

AlBr₃

Li₃P

Zn₃N₂

Rules for Writing a Formula From A Name

1. Write down the symbols for the two elements, in the order in which they appear in the name.

2. Place the valence of the first element (without the sign) above the first symbol.

3. Place the valence of the second element (without the sign) above the second symbol.

4. Write each valence as a subscript on the opposite element (the “criss-cross” rule).

5. If necessary, reduce the subscript numbers to the simplest ratio. (You do not need to write the number 1.)

Examples:

Rubidium nitride Rb¹ N³ à Rb₃N

Magnesium phosphide Mg²P³ à Mg₃P₂

Calcium oxide Ca²O² à Ca₂O₂ à CaO

Try these: Magnesium bromide

Potassium oxide

Beryllium fluoride

Calcium sulphide

Strontium chloride

Barium iodide

Magnesium hydride

Zinc oxide

Silver chloride

Cesium phosphide

PRACTICE

Give the correct formula for the following.

1. sodium sulfide 16. silver bromide

2. calcium phosphide 17. beryllium fluoride

3. hydrogen iodide 18. lithium bromide

4. magnesium hydride 19. potassium phosphide

5. barium oxide 20. aluminum hydride

6. barium chloride 21. lithium oxide

7. aluminum oxide 22. barium bromide

8. cadmium oxide 23. aluminum carbide

9. francium oxide 24. strontium nitride

10. potassium oxide 25. cadmium bromide

11. silver sulfide 26. magnesium carbide

12. zinc chloride 27. cesium nitride

13. calcium iodide 28. zinc nitride

14. rubidium fluoride 29. lithium selenide

15. calcium chloride 30. beryllium telluride

Give the correct name for the following.

1. NaCl 16. SrCl₂

2. MgO 17. Na₂O

3. CaO 18. K₃N

4. BBr₃ 19. Li₃P

5. MgS 20. BaF₂

6. CaCl₂ 21. MgI₂

7. AlBr₃ 22. K₂S

8. Rb₄C 23. SrO

9. Al₂O₃ 24. Al₂S₃

10. Li₂O 25. SrF₂

11. NaBr 26. Ag₂S

12. Be₃P₂ 27. RbI

13. BeF₂ 28. Al₂O₃

14. AlCl₃ 29. MgO

15. HCl 30. KBr

Source : http://taverner.wikispaces.com/file/view/INORGANIC+NOMENCLATURE.doc

Web site link: http://taverner.wikispaces.com

Google key word : Naming inorganic compounds file type : doc

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Binary Compounds: When The First Element is Monovalent

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