Naming and Writing Formulas for Molecular Compounds 93 Section Review

Chapter 4. Chemical Nomenclature

4.3 Nomenclature of Simple Ionic and Molecular Compounds

Learning Objectives

By the end of this module, y'all will exist able to:

• Derive names for common types of inorganic compounds and simple molecular compounds using a systematic arroyo

Nomenclature, a collection of rules for naming things, is important in science and in many other situations. This module describes an approach that is used to name simple ionic and molecular compounds, such equally NaCl, CaCO₃, and N₂O₄. The simplest of these are binary compounds, those containing simply two elements, but nosotros will also consider how to name ionic compounds containing polyatomic ions, and one specific, very important class of compounds known as acids – subsequent chapters in this text will focus on these compounds in great detail. We will limit our attending hither to inorganic compounds, compounds that are equanimous principally of elements other than carbon, and will follow the nomenclature guidelines proposed by IUPAC. The rules for organic compounds, in which carbon is the principle element, will be treated in a later chapter on organic chemical science.

Nomenclature of Ionic Compounds

To proper name an inorganic compound, nosotros need to consider the answers to several questions. First, is the compound ionic or molecular? If the compound is ionic, does the metallic grade ions of but one type (fixed accuse) or more than one type (variable charge)? Are the ions monatomic or polyatomic? If the compound is molecular, does it contain hydrogen? If so, does information technology as well contain oxygen? From the answers nosotros derive, we place the chemical compound in an advisable category and then name information technology accordingly.

Compounds Containing Merely Monatomic Ions

The name of a binary compound containing monatomic ions consists of the name of the cation (the name of the metallic) followed by the name of the anion (the proper noun of the nonmetallic element with its ending replaced by the suffix –ide). Some examples are given in Table 1.

NaCl, sodium chloride	Na2O, sodium oxide
KBr, potassium bromide	CdS, cadmium sulfide
CaI2, calcium iodide	MgiiiNtwo, magnesium nitride
CsF, cesium fluoride	Ca3Pii, calcium phosphide
LiCl, lithium chloride	AlivC3, aluminum carbide
Table i. Names of Some Ionic Compounds

Compounds Containing Polyatomic Ions

Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, except there is no need to modify to an –ide ending, since the suffix is already present in the name of the anion. Examples are shown in Table 2.  See Tabular array 1 in Chapter 4.ii Ionic and Molecular Compounds for the listing of common polyatomic ions.

KCtwoH3O2, potassium acetate	(NH4)Cl, ammonium chloride
NaHCO3, sodium bicarbonate	CaSO4, calcium sulfate
Al2(COthree)3, aluminum carbonate	Mg3(PO4)2, magnesium phosphate
Table 2. Names of Some Polyatomic Ionic Compounds

Case one

Proper noun the following ionic compounds:

a)  NaCl           b) AlBr₃          c)  BaH_ii

Solution

a)  Identify the cation and anion.
Na is a Group 1 metal, and thus it forms the cation Na⁺, called "sodium" ion.
Cl is a nonmetal, and forms the anion Cl^–, chloride.  Thus, NaCl = sodium chloride.

b)  AlBr₃consists of aluminum and bromine; nosotros call it aluminum bromide.

c)  BaH_twois called barium hydride.

Test Yourself

Proper noun the following ionic compounds:

      a)  Al₂Due south_three          b) ZnS            c)  MgI₂

Answers

a) aluminum sulfide         b) zinc sulfide         c) magnesium iodide

Compounds Containing a Metal Ion with a Variable Charge

Most of the transition metals tin form two or more cations with unlike charges. Compounds of these metals with nonmetals are named with the aforementioned method as compounds in the first category, except the charge of the metallic ion is specified by a Roman numeral in parentheses later the name of the metal. The charge of the metallic ion is determined from the formula of the chemical compound and the charge of the anion. For example, consider binary ionic compounds of iron and chlorine. Fe typically exhibits a charge of either 2+ or 3+ (see Figure 2 in Chapter 4.ii Ionic and Molecular Compounds), and the two corresponding compound formulas are FeCl₂ and FeCl₃. The simplest name, "iron chloride," will, in this case, be ambiguous, as it does not distinguish betwixt these ii compounds. In cases similar this, the charge of the metal ion is included as a Roman numeral in parentheses immediately following the metallic name. These two compounds are then unambiguously named iron(Two) chloride and iron(3) chloride, respectively. Other examples are provided in Table 4.

Transition metal Ionic Chemical compound	Name
FeCliii	atomic number 26(3) chloride
Hg2O	mercury(I) oxide
HgO	mercury(II) oxide
Cu3(PO4)two	copper(II) phosphate
Tabular array 4. Names of Some Transition Metal Ionic Compounds

An old naming convention used the suffixes –ic and –ous to designate metals with college and lower charges, respectively: Iron(Three) chloride, FeCl_three, can be chosen chosen ferric chloride, and iron(II) chloride, FeCl₂, is as well known equally ferrous chloride.  This older naming convention remains in use by some segments of manufacture. For example, you may come across the words stannous fluoride on a tube of toothpaste. This represents the formula SnF₂, which is as well named tin can(2) fluoride following the more current convention. The other fluoride of tin can is SnF_iv, is now named tin(Four) fluoride simply is however oftentimes referred to as stannic fluoride.  Knowing both convention remains important.

Element	Common Ions	Common Names for Ions
Cu	Cu+/Cutwo+	cuprous/cupric
Fe	Iron2+/Fe3+	ferrous/ferric
Co	Co2+/Co3+	cobaltous/cobaltic
Cr	Crtwo+/Cr3+	chromous/chromic
Sn	Sn2+/Sn4+	stannous/stannic
Atomic number 82	Pb2+/Pb4+	plumbous/plumbic
Hg	Hgtwo 2+/Hg2+	mercurous/mercuric
Table five. Common Names for Some Metal Ions with Variable Charges

Example ii

Name each species.

a) O²⁻b) Co         c) Co²⁺

Solution

a) This species has a 2− accuse on information technology, then information technology is an anion. Anions are named using the stalk of the element name with the suffix -ide added. This is the oxide anion.

b) Because this species has no charge, information technology is an cantlet in its elemental form. This is cobalt.

c) In this case, there is a 2+ charge on the atom, so it is a cation. Nosotros note from Figure 2 in Chapter four.2 Ionic and Molecular Compounds), that cobalt cations can accept two possible charges, so the name of the ion must specify which charge the ion has. This is the cobalt(II) cation.

Exam Yourself

Proper noun each species: P³⁻and Sr²⁺

Answers

the phosphide anion and the strontium cation

Instance 3

Name the post-obit ionic compounds:

a) SnBr_four         b) CoCl₃          c)  Fe₂O₃

Solution

a)   Start, identify the charge on the cation (Sn).

Because Br has a charge of –1, we know that Sn must have a charge of +4.

                  0 = 1(10) + 4(-1)                       x = +4         Therefore SnBr₄=  can(Four) bromide

b)  Cl adopts a charge of –one

                  0 = one(10) + 3(-one)                       x = +iii         Therefore CoCl₃= cobalt(III) chloride

c)  O adopts a charge of –2

                  0 = two(x) + three(-ii)                       x = +3         Therefore Fe₂O₃= iron(Iii) oxide

Test Yourself

Proper noun the following ionic compounds:

      a)  HgO            b)  PbCl₄          c) PbS           d) Sc_twoO₃ e) AgCl

Answers

a) mercury(Two) oxide         b) lead(IV) chloride         c) lead(Ii) sulphide

d) scandium oxide         e) silver chloride

Example 4

Proper name the post-obit ionic compounds:

a) Iron₂Due south_threeb) CuSe         c) GaN         d) CrCl₃eastward) Ti₂(And so₄)₃ f) Co₂O₃         yard) CaCl₂         h) AlF₃

Solution
The anions in these compounds take a fixed negative accuse (S²⁻, Se²⁻ , N^three−, Cl⁻, SO₄ ⁱⁱ⁻, O⁻ⁱⁱ, and F⁻), and the compounds must exist neutral. Considering the metal ions in questions a) to f) accept a variable charge, we must effigy out the charge of the metal ion by ensuring that the full number of positive charges in each compound must equal the total number of negative charges.  Therefore the positive ions must be Fe³⁺, Cu²⁺, Ga³⁺, Cr³⁺, Ti³⁺ and Co³⁺. These charges are used in the names of the metallic ions:

a) atomic number 26(Iii) sulfide                     b) copper(II) selenide           c) gallium(Three) nitride

d) chromium(Three) chloride         e) titanium(III) sulfate          f) cobalt(Three) oxide

In questions k) and h) the metal ions do not have a variable accuse, therefore

thousand) Using the names of the ions, this ionic compound is named calcium chloride. It is non calcium(Ii) chloride because calcium forms only one cation when it forms an ion, and it has a characteristic charge of 2+.

h)The name of this ionic chemical compound is aluminum fluoride.

Test Yourself

Write the formulas of the post-obit ionic compounds:

a) chromium(Iii) phosphide        b) mercury(II) sulfide         c) manganese(II) phosphate

d) copper(I) oxide         e) chromium(VI) fluoride

Answers

a) CrP         b) HgS        c) Mn₃(PO_iv)_iid) Cu₂O         due east) CrF₆

Erin Brockovich and Chromium Contamination

In the early 1990s, legal file clerk Erin Brockovich (Effigy 1) discovered a loftier rate of serious illnesses in the pocket-size town of Hinckley, California. Her investigation eventually linked the illnesses to groundwater contaminated past Cr(VI) used by Pacific Gas & Electrical (PG&East) to fight corrosion in a nearby natural gas pipeline. As dramatized in the film Erin Brokovich (for which Julia Roberts won an Oscar), Erin and lawyer Edward Masry sued PG&E for contaminating the water near Hinckley in 1993. The settlement they won in 1996—$333 million—was the largest corporeality always awarded for a straight-activeness lawsuit in the U.s. at that time.

Figure 1. (a) Erin Brockovich constitute that Cr(Vi), used past PG&E, had contaminated the Hinckley, California, water supply. (b) The Cr(Six) ion is ofttimes nowadays in water as the polyatomic ions chromate, CrO₄ ²⁻ (left), and dichromate, Cr_iiO₇ ²⁻ (correct).

Chromium compounds are widely used in industry, such as for chrome plating, in dye-making, as preservatives, and to foreclose corrosion in cooling belfry h2o, as occurred near Hinckley. In the environs, chromium exists primarily in either the Cr(3) or Cr(VI) forms. Cr(Three), an ingredient of many vitamin and nutritional supplements, forms compounds that are not very soluble in water, and it has low toxicity. But Cr(Vi) is much more than toxic and forms compounds that are reasonably soluble in h2o. Exposure to small-scale amounts of Cr(Six) can lead to damage of the respiratory, gastrointestinal, and immune systems, as well as the kidneys, liver, blood, and pare.

Despite cleanup efforts, Cr(6) groundwater contagion remains a problem in Hinckley and other locations across the earth. A 2010 report by the Ecology Working Group found that of 35 US cities tested, 31 had higher levels of Cr(Six) in their tap h2o than the public wellness goal of 0.02 parts per billion ready by the California Environmental Protection Agency.

Example 5

Write the proper formula and requite the proper name for each ionic compound formed between the two listed ions.

a) NH₄ ⁺ and S²⁻b) Alⁱⁱⁱ⁺ and PO_four ⁱⁱⁱ⁻c) Fe²⁺ and PO₄ ³⁻

Solution

a) Because the ammonium ion has a one+ charge and the sulfide ion has a 2− accuse, we need two ammonium ions to balance the charge on a single sulfide ion. Enclosing the formula for the ammonium ion in parentheses, nosotros have (NH_four)₂S. The compound's proper name is ammonium sulfide.

b) Because the ions have the aforementioned magnitude of accuse, nosotros demand only one of each to residual the charges. The formula is AlPO_iv, and the name of the compound is aluminum phosphate.

c) Neither charge is an exact multiple of the other, and then we take to go to the least common multiple of 6. To get half-dozen+, we need three atomic number 26(II) ions, and to get six−, we demand 2 phosphate ions. The proper formula is Fe₃(PO_iv)₂, and the compound's proper name is atomic number 26(2) phosphate.

Examination Yourself

Write the proper formula and give the name for each ionic compound formed between the two listed ions.

a) NH_iv ⁺ and PO₄ ^three−b) Co³⁺ and NO₂ ⁻

Answers

a) (NH₄)₃PO₄, ammonium phosphate          b) Co(NO₂)₃, cobalt(Iii) nitrite

Ionic Compounds in Your Cabinets

Every day you meet and use a large number of ionic compounds. Some of these compounds, where they are establish, and what they are used for are listed in Tabular array 3. Look at the label or ingredients list on the various products that you use during the next few days, and see if you run into whatever of those in this tabular array, or discover other ionic compounds that you lot could now proper noun or write every bit a formula.

Ionic Compound	Use
NaCl, sodium chloride	ordinary table salt
KI, potassium iodide	added to "iodized" common salt for thyroid wellness
NaF, sodium fluoride	ingredient in toothpaste
NaHCOthree, sodium bicarbonate	baking soda; used in cooking (and as antacid)
Na2COthree, sodium carbonate	washing soda; used in cleaning agents
NaOCl, sodium hypochlorite	active ingredient in household bleach
CaCO3 calcium carbonate	ingredient in antacids
Mg(OH)two, magnesium hydroxide	ingredient in antacids
Al(OH)3, aluminum hydroxide	ingredient in antacids
NaOH, sodium hydroxide	lye; used as drain cleaner
K3POfour, potassium phosphate	food additive (many purposes)
MgSO4, magnesium sulfate	added to purified h2o
Na2HPO4, sodium hydrogen phosphate	anti-caking agent; used in powdered products
Na2And then3, sodium sulfite	preservative
Table 3. Everyday Ionic Compounds

Classification of Molecular (Covalent) Compounds

The bonding characteristics of inorganic molecular compounds are different from ionic compounds, and they are named using a different organization as well. The charges of cations and anions dictate their ratios in ionic compounds, so specifying the names of the ions provides sufficient information to make up one's mind chemic formulas. Still, because covalent bonding allows for significant variation in the combination ratios of the atoms in a molecule, the names for molecular compounds must explicitly identify these ratios.

Compounds Composed of 2 Elements

When two nonmetallic elements course a molecular compound, several combination ratios are ofttimes possible. For case, carbon and oxygen can form the compounds CO and CO₂. Since these are different substances with different properties, they cannot both accept the same name (they cannot both exist chosen carbon oxide). To deal with this situation, nosotros use a naming method that is somewhat like to that used for ionic compounds, but with added prefixes to specify the numbers of atoms of each element. The name of the more metal element (the 1 further to the left and/or bottom of the periodic table) is start, followed by the proper name of the more than nonmetallic element (the one farther to the right and/or top) with its ending inverse to the suffix –ide. The numbers of atoms of each chemical element are designated past the Greek prefixes shown in Table half-dozen.

Number	Prefix	Number	Prefix
ane (sometimes omitted)	mono-	half dozen	hexa-
2	di-	7	hepta-
3	tri-	eight	octa-
iv	tetra-	9	nona-
v	penta-	ten	deca-
Table 6. Nomenclature Prefixes

When only one atom of the showtime chemical element is nowadays, the prefix mono– is usually deleted from that part. Thus, CO is named carbon monoxide, and CO₂ is called carbon dioxide. When two vowels are adjacent, the a in the Greek prefix is ordinarily dropped. Some other examples are shown in Tabular array seven.

Compound	Name	Compound	Proper name
Thenii	sulfur dioxide	BClthree	boron trichloride
So3	sulfur trioxide	SF6	sulfur hexafluoride
NOtwo	nitrogen dioxide	PF5	phosphorus pentafluoride
N2Ofour	dinitrogen tetroxide	P4O10	tetraphosphorus decaoxide
Due north2O5	dinitrogen pentoxide	IFvii	iodine heptafluoride
Tabular array 7. Names of Some Molecular Compounds Composed of Two Elements

There are a few common names that you will encounter equally you keep your study of chemistry. For example, although NO is often called nitric oxide, its proper name is nitrogen monoxide. Similarly, N₂O is known as nitrous oxide even though our rules would specify the proper name dinitrogen monoxide. (And H₂O is usually called water, not dihydrogen monoxide.) You should commit to retention the common names of compounds every bit yous come across them.

Example 6

Name the post-obit covalent compounds:

a) SF_vib) North₂O₃c) Cl₂O₇d) P₄O₆ east) PF₃ f) CO         k) Se_iiBr_two

Solution
Because these compounds consist solely of nonmetals, they are molecular compounds, therefore according to the rules, we utilise prefixes to designate the number of atoms of each element:

a) sulfur hexafluoride                    b) dinitrogen trioxide              c) dichloride heptoxide

d) tetraphosphorus hexoxide         e) phosphorus trifluoride         f) carbon monoxide (non carbon monooxide)

g) diselenium dibromide

Examination Yourself
Write the formulas for the post-obit compounds:

a) phosphorus pentachloride          b) dinitrogen monoxide         c) iodine heptafluoride

d) carbon tetrachloride                   eastward) disulfur difluoride              f) iodine pentabromide

Answers

a) PCl₅b) N_iiO         c) IF₇d) CCl₄ e) S₂F₂f) IBr₅

The following website provides practice with naming chemical compounds and writing chemical formulas. You can choose binary, polyatomic, and variable charge ionic compounds, besides as molecular compounds.

Binary Acids

Some compounds containing hydrogen are members of an important class of substances known as acids, and these compounds take interesting chemic backdrop. The chemistry of these compounds is explored in more than detail in later capacity of this text, but for now, it will suffice to annotation that many acids release hydrogen ions, H⁺, when dissolved in water.  To indicate that something is dissolved in water, we will apply the phase label (aq) next to a chemical formula (where aq stands for "aqueous," a word that describes something dissolved in water).  To denote this distinct chemical belongings, a mixture of water with an acid is given a proper noun derived from the compound's name. If the chemical compound is a binary acid (comprised of hydrogen and one other nonmetallic element):

1. The give-and-take "hydrogen" is changed to the prefix hydro-
2. The other nonmetallic element name is modified past adding the suffix –ic
3. The word "acid" is added every bit a 2nd discussion

For case, when the gas HCl (hydrogen chloride) is dissolved in water, the solution is called hydrochloric acid. Several other examples of this nomenclature are shown in Table eight.

Proper noun of Gas	Name of Acid
HF(g), hydrogen fluoride	HF(aq), hydrofluoric acid
HCl(one thousand), hydrogen chloride	HCl(aq), hydrochloric acid
HBr(1000), hydrogen bromide	HBr(aq), hydrobromic acid
Hello(thousand), hydrogen iodide	HI(aq), hydroiodic acid
H2S(yard), hydrogen sulfide	H2South(aq), hydrosulfuric acid
HCN(k), hydrogen cyanide	HCN(aq), hydrocyanic acid
Table viii. Names of Some Simple Acids

Oxyacids

Many compounds containing three or more elements (such as organic compounds or coordination compounds) are subject to specialized nomenclature rules that you will learn after. However, we will briefly talk over the important compounds known as oxyacids, compounds that incorporate hydrogen, oxygen, and at least one other element, and are bonded in such a style as to impart acidic properties to the compound (y'all will learn the details of this in a later chapter). Typical oxyacids consist of hydrogen combined with a polyatomic, oxygen-containing ion. To name oxyacids:

1. Omit "hydrogen"
2. Start with the root name of the anion
3. Supervene upon –ate with –ic, or –ite with –ous
4. Add together "acid"

For example, consider H₂CO₃ (which you lot might be tempted to call "hydrogen carbonate"). To name this correctly, "hydrogen" is omitted; the –ate of carbonate is replace with –ic; and acid is added—so its name is carbonic acrid. Other examples are given in Tabular array 9. In that location are some exceptions to the general naming method (due east.chiliad., H₂And so₄ is chosen sulfuric acrid, not sulfic acid, and H₂SO₃ is sulfurous, not sulfous, acrid).

Formula	Anion Name	Acid Name
HC2H3Otwo	acetate	acetic acrid
HNO3	nitrate	nitric acid
HNO2	nitrite	nitrous acrid
HClO4	perchlorate	perchloric acid
HClO 3	chlorate	chloric acid
HClO ii	chlorite	chlorous acid
HClO	hypochlorite	hypochlorous acid
H2CO3	carbonate	carbonic acrid
HtwoAnd theniv	sulfate	sulfuric acid
HtwoSO3	sulfite	sulfurous acid
HiiiPO4	phosphate	phosphoric acid
HthreePO3	phosphite	phosphorous acid
H2CrO4	chromate	chromic acid
Table 9. Names of Common Oxyacids

Example 7

Name each acrid without consulting the tables.

a) HBr(aq)         b) H₂SO₄c)  HF(m)         d)  HCN(aq)         e) H₂South(aq)

Solution

a) As an aqueous binary acid, the acid'due south name is hydro- + stem proper name +-ic acrid. Considering this acid contains a bromine atom, the name is hydrobromic acrid.

b) Considering this acid is derived from the sulfate ion, the name of the acid is the stalk of the anion proper name +-ic acid. The proper name of this acrid is sulfuric acrid.

c) Because HF(thou) is in gaseous form, nosotros name it hydrogen fluoride.

d)  HCN(aq) contains the polyatomic ion cyanide. The root is "cyan", thus HCN(aq) = hydrocyanic acid.

eastward)  H₂S(aq) contains the ion sulfide. In this example, nonetheless, the root takes a slightly unlike course of "sulfur" (the same as the element proper name). Thus H₂S(aq) = hydrosulfuric acid.

Test Yourself

Name each acid.

a) HF(aq)         b) HNO_iic) HClO₄       d) H₂SO₄e) H_iiCrO₄(aq)          f)  H₃PO₄(aq)      g) HClO(aq)

Answers

a) hydrofluoric acid         b) nitrous acid         c) perchloric acid         d) sulphuric acid         eastward) chromic acid

f) phosphoric acid         grand) hypochlorous acid

All acids have some like properties. For example, acids have a sour gustatory modality; in fact, the sour gustatory modality of some of our foods, such every bit citrus fruits and vinegar, is caused by the presence of acids in food. Many acids react with some metal elements to grade metal ions and elemental hydrogen. Acids brand certain establish pigments alter colors; indeed, the ripening of some fruits and vegetables is acquired by the formation or destruction of excess acrid in the found. In a later on chapter, we will explore the chemical behaviour of acids.

Acids are very prevalent in the world around us. We have already mentioned that citrus fruits contain acid; amidst other compounds, they contain citric acid, H_iiiC₆H₅O₇(aq). Oxalic acid, H₂C₂O_four(aq), is plant in spinach and other green leafy vegetables. Muriatic acid not only is found in the tummy (tummy acid) but also can be bought in hardware stores equally a cleaner for concrete and masonry. Phosphoric acid is an ingredient in some soft drinks.

Sodium in Your Food

The element sodium, at least in its ionic form as Na⁺, is a necessary nutrient for humans to live. In fact, the human body is approximately 0.15% sodium, with the boilerplate person having one-twentieth to i-10th of a kilogram in their body at any given time, mostly in fluids outside cells and in other actual fluids.

Sodium is likewise present in our nutrition. The common table salt nosotros apply on our foods is an ionic sodium compound. Many processed foods likewise comprise significant amounts of sodium added to them as a diverseness of ionic compounds. Why are sodium compounds used so much? Usually sodium compounds are inexpensive, but, more importantly, virtually ionic sodium compounds deliquesce easily. This allows candy nutrient manufacturers to add together sodium-containing substances to food mixtures and know that the compound volition deliquesce and distribute evenly throughout the food. Simple ionic compounds such as sodium nitrite (NaNO₂) are added to cured meats, such as bacon and cafeteria-manner meats, while a compound chosen sodium benzoate is added to many packaged foods as a preservative. Tabular array 10 "Some Sodium Compounds Added to Food" is a partial list of some sodium additives used in nutrient. Some of them you may recognize after reading this chapter. Others you may non recognize, but they are all ionic sodium compounds with some negatively charged ion also present.

Sodium Compound	Apply in Nutrient
Sodium acetate	preservative, acidity regulator
Sodium adipate	food acid
Sodium alginate	thickener, vegetable glue, stabilizer, gelling amanuensis, emulsifier
Sodium aluminum phosphate	acidity regulator, emulsifier
Sodium aluminosilicate	anticaking agent
Sodium ascorbate	antioxidant
Sodium benzoate	preservative
Sodium bicarbonate	mineral salt
Sodium bisulfite	preservative, antioxidant
Sodium carbonate	mineral salt
Sodium carboxymethylcellulose	emulsifier
Sodium citrates	food acid
Sodium dehydroacetate	preservative
Sodium erythorbate	antioxidant
Sodium erythorbin	antioxidant
Sodium ethyl para-hydroxybenzoate	preservative
Sodium ferrocyanide	anticaking agent
Sodium formate	preservative
Sodium fumarate	food acid
Sodium gluconate	stabilizer
Sodium hydrogen acetate	preservative, acidity regulator
Sodium hydroxide	mineral salt
Sodium lactate	food acid
Sodium malate	food acid
Sodium metabisulfite	preservative, antioxidant, bleaching agent
Sodium methyl para-hydroxybenzoate	preservative
Sodium nitrate	preservative, color fixative
Sodium nitrite	preservative, color fixative
Sodium orthophenyl phenol	preservative
Sodium propionate	preservative
Sodium propyl para-hydroxybenzoate	preservative
Sodium sorbate	preservative
Sodium stearoyl lactylate	emulsifier
Sodium succinates	acerbity regulator, flavour enhancer
Sodium salts of fatty acids	emulsifier, stabilizer, anticaking agent
Sodium sulfite	mineral salt, preservative, antioxidant
Sodium sulfite	preservative, antioxidant
Sodium tartrate	food acid
Sodium tetraborate	preservative

Tabular array 10. Some Sodium Compounds Added to Food

The use of then many sodium compounds in prepared and candy foods has alarmed some physicians and nutritionists. They argue that the boilerplate person consumes also much sodium from his or her nutrition. The average person needs simply about 500 mg of sodium every day; most people swallow more than this—upwardly to 10 times as much. Some studies have implicated increased sodium intake with high claret pressure level; newer studies advise that the link is questionable. However, at that place has been a button to reduce the amount of sodium nearly people ingest every twenty-four hour period: avoid candy and manufactured foods, read labels on packaged foods (which include an indication of the sodium content), don't oversalt foods, and use other herbs and spices too common salt in cooking.

Key Concepts and Summary

Chemists use nomenclature rules to clearly proper name compounds. Ionic and molecular compounds are named using somewhat-unlike methods. Binary ionic compounds typically consist of a metal and a nonmetal. The name of the metal is written commencement, followed by the name of the nonmetal with its ending changed to –ide. For example, 1000_iiO is called potassium oxide. If the metallic tin class ions with different charges, a Roman numeral in parentheses follows the name of the metal to specify its charge. Thus, FeCl₂ is iron(II) chloride and FeCl₃ is iron(III) chloride. Some compounds contain polyatomic ions; the names of mutual polyatomic ions should be memorized. Molecular compounds can form compounds with different ratios of their elements, and then prefixes are used to specify the numbers of atoms of each element in a molecule of the compound. Examples include SF_{half dozen}, sulfur hexafluoride, and N₂O₄, dinitrogen tetroxide. Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix hydro-, changing the –ide suffix to –ic, and adding "acrid;" HCl is hydrochloric acid. Oxyacids are named by changing the ending of the anion to –ic, and calculation "acrid;" H₂CO₃ is carbonic acid.

Figure three. Flowchart illustrating the thought process involved in naming simple ionic and covalent compounds and the rules needed to follow.

Activity

Brand yourself a stack of pocket-sized sized Qcards.  On one side accept the name of an ionic compound (e.g. sodium hydroxide) and on the other side have its chemical formula (e.yard. NaOH).  Use every case plant in this chapter – including those in the exercises.  Then use these Qcards to quiz yourself.

Exercises

i.  Requite the formula and name for each ionic compound formed between the two listed ions.

a)  Mg²⁺ and Cl⁻b)  Atomic number 26²⁺ and Oⁱⁱ⁻c)  Fe³⁺ and Oⁱⁱ⁻

2.  Give the formula and name for each ionic chemical compound formed between the ii listed ions.

a)  Cu²⁺ and F⁻b)  Ca²⁺ and O²⁻c)  K⁺ and P^three−

3.  Give the formula and proper noun for each ionic compound formed between the two listed ions.

a)  K⁺ and SO₄ ⁱⁱ⁻b)  NH₄ ⁺ and S²⁻c)  NH₄ ⁺ and PO₄ ³⁻

4.  Requite the formula and name for each ionic compound formed between the two listed ions.

a)  Pb⁴⁺ and SO_iv ²⁻b)  Na⁺ and I₃ ⁻c)  Li⁺ and Cr₂O_vii ²⁻

v.  Give the formula and name for each ionic compound formed betwixt the two listed ions.

a)  Ag⁺ and SO₃ ^two−b)  Na⁺ and HCO₃ ⁻c)  Feⁱⁱⁱ⁺ and ClO_iii ⁻

6. .Which of these formulas represent molecules? State how many atoms are in each molecule.

a)  Feb)  PCl_iii c)  P₄ d)  Ar

vii.  What is the difference between CO and Co?

viii.  Give the proper formula for each diatomic element.

ix.  What is the stem of fluorine used in molecule names? CF _iv is ane instance.

10.  Give the name for each molecule.

a)  PF₃ b)  TeCl₂ c)  N₂O₃

11.  Give the proper proper noun for each molecule.

a)  XeF₂ b)  O₂F_two c)  SF_{half dozen}

12.  Give the name for each molecule.

a)  N₂Ob)  N₂O₄ c)  N_twoO_v

13.  Give the proper formula for each name.

a)  dinitrogen pentoxideb)  tetraboron tricarbidec)  phosphorus pentachloride

14.  Give the proper formula for each proper name.

a)  dioxygen dichlorideb)  dinitrogen trisulfidec)  xenon tetrafluoride

15.  Give the proper formula for each name.

a)  iodine trifluorideb)  xenon trioxidec)  disulfur decafluoride

16. Requite the formula for each acrid.

a)  perchloric acrid         b)  hydroiodic acid

17. Proper name each acid.

a)  HF(aq)         b)  HNO₃(aq)         c)  H_iiC_iiO_iv(aq)

18. Proper name the following compounds:

a) CsCl         b) BaO         c) K₂S         d) BeCl_iieast) HBr         f) AlF_iii

19. Write the formulas of the following compounds:

a) rubidium bromide         b) magnesium selenide         c) sodium oxide         d) calcium chloride

eastward) hydrogen fluoride         f) gallium phosphide         g) aluminum bromide         h) ammonium sulfate

20. Write the formulas of the following compounds:

a) chlorine dioxide         b) dinitrogen tetraoxide         c) potassium phosphide

d) silver(I) sulfide         e) aluminum nitride         f) silicon dioxide

21. Each of the post-obit compounds contains a metal that can showroom more than ane ionic charge. Name these compounds:

a) Cr_iiO₃b) FeCl₂c) CrO₃d) TiCl_foure) CoO         f) MoS₂

22. The following ionic compounds are found in common household products. Write the formulas for each compound:

a) potassium phosphate         b) copper(II) sulfate         c) calcium chloride

d) titanium dioxide         eastward) ammonium nitrate

f) sodium bisulfate (the common name for sodium hydrogen sulfate)

23. What are the IUPAC names of the following compounds?

a) manganese dioxide         b) mercurous chloride (Hg₂Cl₂)         c) ferric nitrate [Fe(NO_iii)₃]

d) titanium tetrachloride         eastward) cupric bromide (CuBr₂)

Answers

1. a)  magnesium chloride, MgCl₂ b)  fe(Two) oxide, FeOc)  iron(Iii) oxide, Atomic number 26₂O₃

2. a)  copper(II) fluoride, CuF₂ b)  calcium oxide, CaOc)  potassium phosphide, K₃P

three. a)  potassium sulfate, Thousand₂SO₄ b)  ammonium sulfide, (NH₄)₂Sc)  ammonium phosphate, (NH₄)₃PO₄

iv. a)  lead(IV) sulfate, Pb(So₄)_ii b)  sodium triiodide, NaI₃ c)  lithium dichromate, Li_twoCr₂O₇

five. a)  silver sulfite, Ag_twoSO₃ b)  sodium hydrogen carbonate, NaHCO₃ c)  iron(III) chlorate, Atomic number 26(ClO₃)_iii

6. a)  not a moleculeb)  a molecule; four atoms fullc)  a molecule; 4 atoms total

d)  not a molecule

vii. CO is a compound of carbon and oxygen; Co is the element cobalt.

viii. H₂, O₂, N₂, F₂, Cl₂, Br₂, I_ii

9.fluor-

10. a)  phosphorus trifluorideb)  tellurium dichloridec)  dinitrogen trioxide

xi. a)  xenon difluorideb)  dioxygen difluoridec)  sulfur hexafluoride

12. a)  dinitrogen monoxideb)  dinitrogen tetroxidec)  dinitrogen pentoxide

13. a)  North_twoO₅ b)  B_fourC_three c)  PCl₅

xiv. a)  O_twoCl₂ b)  N₂South_three c)  XeF₄

15. a)  IF₃ b)  XeO₃ c)  Southward₂F_ten

16.a)  HClO ₄ (aq) b)  HI(aq)

17. a)  hydrofluoric acid         b)  nitric acid         c)  oxalic acid

18. a) cesium chloride         b) barium oxide         c) potassium sulfide

d) beryllium chloride         e) hydrogen bromide         f) aluminum fluoride

xix. a) RbBr         b) MgSe         c) Na₂O         d) CaCl_iie) HF         f) GaP         thousand) AlBr₃h) (NH_four)₂And then_four

20. a) ClO₂b) North_twoO_ivc) G_threeP         d) Ag₂S         e) AlN         f) SiO₂

21. a) chromium(III) oxide         b) iron(2) chloride         c) chromium(6) oxide

d) titanium(IV) chloride         e) cobalt(Ii) oxide         f) molybdenum(IV) sulfide

22. a) 1000_threePO₄b) CuSO₄c) CaCl_twod) TiO_iieastward) NH_ivNO₃f) NaHSO₄

23. a) manganese(Iv) oxide         b) mercury(I) chloride         c) atomic number 26(III) nitrate

d) titanium(IV) chloride         e) copper(Ii) bromide

Glossary

binary acid:chemical compound that contains hydrogen and one other element, bonded in a way that imparts acidic backdrop to the chemical compound (ability to release H⁺ ions when dissolved in water)

binary chemical compound:chemical compound containing two different elements.

nomenclature:system of rules for naming objects of interest

oxyacid:chemical compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H⁺ ions when dissolved in water)

herzthiets.blogspot.com

Source: https://pressbooks.bccampus.ca/chem1114langaracollege/chapter/2-7-chemical-nomenclature/

Share this post