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What Is the Formula of the Ionic Compound Expected to Form Between the Elements I and Ca?

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3.4 Ions and Ionic Compounds

Learning Objectives

  1. Know how ions form.
  2. Learn the characteristic charges that ions have.
  3. Construct a proper formula for an ionic compound.
  4. Generate a proper name for an ionic compound.

So far, nosotros take discussed elements and compounds that are electrically neutral. They take the same number of electrons as protons, so the negative charges of the electrons is balanced by the positive charges of the protons. However, this is not always the case. Electrons can motion from one atom to another; when they do, species with overall electric charges are formed. Such species are called ionsA species with an overall electrical accuse. . Species with overall positive charges are termed cationsA species with an overall positive charge. , while species with overall negative charges are called anionsA species with an overall negative charge. . Remember that ions are formed only when electrons move from one cantlet to another; a proton never moves from ane atom to some other. Compounds formed from positive and negative ions are called ionic compoundsA chemical compound formed from positive and negative ions. .

Individual atoms can gain or lose electrons. When they do, they go monatomic ions. When atoms proceeds or lose electrons, they usually gain or lose a characteristic number of electrons and so take on a feature overall accuse. Table 3.half-dozen "Monatomic Ions of Diverse Charges" lists some mutual ions in terms of how many electrons they lose (making cations) or gain (making anions). There are several things to observe nigh the ions in Table 3.half dozen "Monatomic Ions of Various Charges". First, each element that forms cations is a metal, except for one (hydrogen), while each chemical element that forms anions is a nonmetal. This is really one of the chemical properties of metals and nonmetals: metals tend to form cations, while nonmetals tend to form anions. 2nd, most atoms grade ions of a single feature accuse. When sodium atoms class ions, they always class a 1+ charge, never a 2+ or iii+ or even 1− accuse. Thus, if yous commit the data in Table 3.6 "Monatomic Ions of Various Charges" to memory, yous volition always know what charges nigh atoms form. (In Chapter nine "Chemic Bonds", we will hash out why atoms form the charges they exercise.)

Table iii.6 Monatomic Ions of Various Charges

Ions formed by losing a single electron H+
Na+
1000+
Rb+
Ag+
Au+
Ions formed by losing two electrons Mgii+
Ca2+
Sr2+
Fe2+
Coii+
Ni2+
Cu2+
Zn2+
Sn2+
Hgtwo+
Atomic number 82two+
Ions formed by losing three electrons Sc3+
Fe3+
Co3+
Ni3+
Au3+
Al3+
Cr3+
Ions formed by losing iv electrons Ti4+
Sn4+
Pb4+
Ions formed by gaining a unmarried electron F−
Cl−
Br−
I−
Ions formed by gaining two electrons O2−
Southward2−
Seii−
Ions formed past gaining three electrons N3−
P3−

3rd, there are some exceptions to the previous indicate. A few elements, all metals, can class more than than one possible charge. For case, fe atoms can course 2+ cations or iii+ cations. Cobalt is another element that can class more than one possible charged ion (2+ and 3+), while lead can class 2+ or iv+ cations. Unfortunately, at that place is footling understanding which two charges a metal atom may take, and so it is best to just memorize the possible charges a particular chemical element can take.

Note the convention for indicating an ion. The magnitude of the charge is listed every bit a right superscript side by side to the symbol of the element. If the charge is a single positive or negative one, the number 1 is not written; if the magnitude of the charge is greater than ane, and so the number is written before the + or − sign. An element symbol without a charge written next to it is causeless to be the uncharged cantlet.

Naming an ion is straightforward. For a cation, simply apply the proper noun of the element and add together the word ion (or if you want to be more than specific, add cation) after the element's name. Then Na+ is the sodium ion; Ca2+ is the calcium ion. If the chemical element has more than one possible charge, the value of the charge comes after the element name and before the word ion. Thus, Fe2+ is the iron two ion, while Fe3+ is the fe 3 ion. In print, we use roman numerals in parentheses to correspond the charge on the ion, so these two iron ions would be represented as the fe(2) cation and the atomic number 26(3) cation, respectively.

For a monatomic anion, use the stem of the chemical element name and append the suffix -ide to it, and then add together ion. This is similar to how we named molecular compounds. Thus, Cl− is the chloride ion, and North3− is the nitride ion.

Case 6

Name each species.

  1. O2−
  2. Co
  3. Cotwo+

Solution

  1. This species has a 2− charge on it, so it is an anion. Anions are named using the stem of the element name with the suffix -ide added. This is the oxide anion.
  2. Because this species has no charge, it is an atom in its elemental form. This is cobalt.
  3. In this case, there is a 2+ charge on the atom, so it is a cation. We note from Table 3.vi "Monatomic Ions of Various Charges" that cobalt cations can have two possible charges, and then the proper name of the ion must specify which charge the ion has. This is the cobalt(Two) cation.

Exam Yourself

Name each species.

  1. P3−
  2. Sr2+

Answers

  1. the phosphide anion
  2. the strontium cation

Chemic formulas for ionic compounds are called ionic formulasThe chemical formula for an ionic compound. . A proper ionic formula has a cation and an anion in information technology; an ionic chemical compound is never formed between two cations only or ii anions only. The key to writing proper ionic formulas is simple: the full positive accuse must balance the total negative accuse. Because the charges on the ions are feature, sometimes we have to have more one of a cation or an anion to rest the overall positive and negative charges. It is conventional to use the lowest ratio of ions that are needed to remainder the charges.

For instance, consider the ionic compound betwixt Na+ and Cl−. Each ion has a single charge, one positive and one negative, so we demand only one ion of each to residual the overall charge. When writing the ionic formula, we follow two additional conventions: (1) write the formula for the cation first and the formula for the anion next, but (2) practise not write the charges on the ions. Thus, for the chemical compound between Na+ and Cl−, we have the ionic formula NaCl (Figure 3.5 "NaCl = Tabular array Salt"). The formula NaiiCl2 also has balanced charges, only the convention is to use the lowest ratio of ions, which would exist one of each. (Remember from our conventions for writing formulas that we don't write a 1 subscript if there is just one cantlet of a particular element present.) For the ionic compound between magnesium cations (Mgii+) and oxide anions (Oii−), again we need simply i of each ion to balance the charges. By convention, the formula is MgO.

For the ionic compound betwixt Mgii+ ions and Cl− ions, nosotros now consider the fact that the charges have different magnitudes, 2+ on the magnesium ion and 1− on the chloride ion. To residuum the charges with the lowest number of ions possible, we need to have two chloride ions to remainder the charge on the ane magnesium ion. Rather than write the formula MgClCl, nosotros combine the two chloride ions and write it with a 2 subscript: MgClii.

What is the formula MgCl2 telling us? There are 2 chloride ions in the formula. Although chlorine equally an element is a diatomic molecule, Clii, elemental chlorine is non part of this ionic compound. The chlorine is in the form of a negatively charged ion, non the neutral element. The 2 subscript is in the ionic formula because nosotros need ii Cl− ions to balance the charge on 1 Mg2+ ion.

Example vii

Write the proper ionic formula for each of the two given ions.

  1. Catwo+ and Cl−
  2. Al3+ and F−
  3. Al3+ and O2−

Solution

  1. We need ii Cl− ions to balance the charge on one Ca2+ ion, so the proper ionic formula is CaCl2.
  2. Nosotros demand three F− ions to balance the charge on the Althree+ ion, so the proper ionic formula is AlF3.
  3. With Al3+ and O2−, note that neither charge is a perfect multiple of the other. This means we have to go to a least common multiple, which in this case volition exist six. To go a total of 6+, we need two Althree+ ions; to become half dozen−, we need three O2− ions. Hence the proper ionic formula is Al2O3.

Test Yourself

Write the proper ionic formulas for each of the two given ions.

  1. Feii+ and Due south2−
  2. Ironiii+ and S2−

Answers

  1. FeS
  2. Fe2S3

Naming ionic compounds is simple: combine the proper name of the cation and the name of the anion, in both cases omitting the word ion. Practice not utilise numerical prefixes if there is more than i ion necessary to balance the charges. NaCl is sodium chloride, a combination of the name of the cation (sodium) and the anion (chloride). MgO is magnesium oxide. MgClii is magnesium chloride—not magnesium dichloride.

In naming ionic compounds whose cations can take more than than one possible charge, nosotros must also include the accuse, in parentheses and in roman numerals, equally part of the name. Hence FeS is atomic number 26(Two) sulfide, while Fe2Siii is iron(Three) sulfide. Again, no numerical prefixes announced in the name. The number of ions in the formula is dictated by the need to balance the positive and negative charges.

Example viii

Name each ionic compound.

  1. CaCltwo
  2. AlFiii
  3. Co2Oiii

Solution

  1. Using the names of the ions, this ionic chemical compound is named calcium chloride. It is not calcium(II) chloride considering calcium forms just one cation when it forms an ion, and it has a characteristic charge of two+.
  2. The name of this ionic compound is aluminum fluoride.
  3. We know that cobalt can accept more than one possible charge; we merely need to decide what information technology is. Oxide ever has a 2− charge, so with three oxide ions, we have a full negative accuse of 6−. This means that the two cobalt ions have to contribute half dozen+, which for two cobalt ions ways that each one is 3+. Therefore, the name for this ionic compound is cobalt(III) oxide.

Examination Yourself

Name each ionic compound.

  1. Sc2O3
  2. AgCl

Answers

  1. scandium oxide
  2. silver chloride

How exercise you know whether a formula—and past extension, a name—is for a molecular chemical compound or for an ionic compound? Molecular compounds form between nonmetals and nonmetals, while ionic compounds form between metals and nonmetals. The periodic table (Figure 3.2 "A Simple Periodic Table") tin be used to determine which elements are metals and nonmetals.

There also exists a group of ions that contain more than one atom. These are chosen polyatomic ionsAn ion that contains more than one atom. . Table 3.7 "Common Polyatomic Ions" lists the formulas, charges, and names of some common polyatomic ions. Only i of them, the ammonium ion, is a cation; the rest are anions. Most of them also comprise oxygen atoms, so sometimes they are referred to as oxyanions. Some of them, such as nitrate and nitrite, and sulfate and sulfite, take very similar formulas and names, so care must exist taken to get the formulas and names correct. Note that the -ite polyatomic ion has one less oxygen atom in its formula than the -ate ion but with the aforementioned ionic charge.

Table three.7 Common Polyatomic Ions

Proper name Formula and Charge Proper noun Formula and Charge
ammonium NH4 + hydroxide OH−
acetate C2HthreeOii −, or CHiiiCOO− nitrate NO3 −
bicarbonate (hydrogen carbonate) HCO3 − nitrite NO2 −
bisulfate (hydrogen sulfate) HSOiv − peroxide O2 2−
carbonate COthree 2− perchlorate ClO4 −
chlorate ClO3 − phosphate PO4 3−
chromate CrO4 ii− sulfate SO4 2−
cyanide CN− sulfite SO3 2−
dichromate Cr2Ovii two− triiodide Iiii −

The naming of ionic compounds that contain polyatomic ions follows the same rules as the naming for other ionic compounds: simply combine the proper noun of the cation and the name of the anion. Practice not utilize numerical prefixes in the proper noun if in that location is more than than ane polyatomic ion; the merely exception to this is if the proper noun of the ion itself contains a numerical prefix, such as dichromate or triiodide.

Writing the formulas of ionic compounds has one of import divergence. If more than one polyatomic ion is needed to rest the overall accuse in the formula, enclose the formula of the polyatomic ion in parentheses and write the proper numerical subscript to the right and outside the parentheses. Thus, the formula between calcium ions, Ca2+, and nitrate ions, NOthree −, is properly written Ca(NO3)2, not CaNO32 or Can2O6. Use parentheses where required. The name of this ionic compound is simply calcium nitrate.

Example 9

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

  1. NH4 + and S2−
  2. Aliii+ and PO4 3−
  3. Fe2+ and PO4 3−

Solution

  1. Because the ammonium ion has a 1+ charge and the sulfide ion has a 2− accuse, we demand ii ammonium ions to balance the charge on a single sulfide ion. Enclosing the formula for the ammonium ion in parentheses, we have (NH4)iiS. The chemical compound'southward name is ammonium sulfide.
  2. Because the ions have the same magnitude of accuse, nosotros demand only one of each to remainder the charges. The formula is AlPO4, and the name of the compound is aluminum phosphate.
  3. Neither charge is an verbal multiple of the other, so we have to go to the to the lowest degree common multiple of half dozen. To get half dozen+, we need three iron(II) ions, and to become 6−, we need ii phosphate ions. The proper formula is Fe3(POiv)two, and the compound's name is iron(II) phosphate.

Test Yourself

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

  1. NH4 + and POiv 3−
  2. Co3+ and NO2 −

Answers

  1. (NHfour)iiiPOiv, ammonium phosphate
  2. Co(NOii)3, cobalt(III) nitrite

Nutrient and Drink App: Sodium in Your Food

The chemical element sodium, at least in its ionic form as Na+, is a necessary nutrient for humans to alive. In fact, the human being torso is approximately 0.fifteen% sodium, with the boilerplate person having i-twentieth to ane-10th of a kilogram in their torso at whatsoever given fourth dimension, generally in fluids exterior cells and in other bodily fluids.

Sodium is also nowadays in our diet. The common table table salt we utilise on our foods is an ionic sodium compound. Many processed foods also incorporate significant amounts of sodium added to them every bit a variety of ionic compounds. Why are sodium compounds used then much? Unremarkably sodium compounds are inexpensive, but, more importantly, most ionic sodium compounds dissolve easily. This allows processed nutrient manufacturers to add sodium-containing substances to food mixtures and know that the compound volition deliquesce and distribute evenly throughout the food. Unproblematic ionic compounds such every bit sodium nitrite (NaNOtwo) are added to cured meats, such equally bacon and deli-style meats, while a compound called sodium benzoate is added to many packaged foods as a preservative. Tabular array 3.viii "Some Sodium Compounds Added to Food" is a fractional list of some sodium additives used in nutrient. Some of them y'all may recognize afterward reading this chapter. Others you may non recognize, but they are all ionic sodium compounds with some negatively charged ion also present.

Table 3.8 Some Sodium Compounds Added to Food

Sodium Chemical compound Use in Nutrient
Sodium acetate preservative, acidity regulator
Sodium adipate food acid
Sodium alginate thickener, vegetable gum, stabilizer, gelling agent, 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 acrid
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, acerbity regulator
Sodium hydroxide mineral salt
Sodium lactate food acid
Sodium malate nutrient acid
Sodium metabisulfite preservative, antioxidant, bleaching agent
Sodium methyl para-hydroxybenzoate preservative
Sodium nitrate preservative, color fixative
Sodium nitrite preservative, colour fixative
Sodium orthophenyl phenol preservative
Sodium propionate preservative
Sodium propyl para-hydroxybenzoate preservative
Sodium sorbate preservative
Sodium stearoyl lactylate emulsifier
Sodium succinates acidity regulator, flavor enhancer
Sodium salts of fatty acids emulsifier, stabilizer, anticaking amanuensis
Sodium sulfite mineral salt, preservative, antioxidant
Sodium sulfite preservative, antioxidant
Sodium tartrate nutrient acid
Sodium tetraborate preservative

The employ of so many sodium compounds in prepared and candy foods has alarmed some physicians and nutritionists. They argue that the average person consumes too much sodium from his or her nutrition. The average person needs only about 500 mg of sodium every day; most people consume more than this—up to 10 times every bit much. Some studies have implicated increased sodium intake with loftier claret pressure; newer studies advise that the link is questionable. However, at that place has been a push to reduce the amount of sodium most people ingest every twenty-four hour period: avoid processed 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 besides salt in cooking.

Food labels include the amount of sodium per serving. This particular label shows that at that place are 75 mg of sodium in one serving of this particular nutrient item.

Key Takeaways

  • Ions form when atoms lose or gain electrons.
  • Ionic compounds have positive ions and negative ions.
  • Ionic formulas balance the total positive and negative charges.
  • Ionic compounds have a elementary system of naming.
  • Groups of atoms can have an overall accuse and brand ionic compounds.

Exercises

  1. Explain how cations form.

  2. Explain how anions form.

  3. Give the charge each atom takes when it forms an ion. If more than 1 charge is possible, list both.

    1. K
    2. O
    3. Co

  4. Give the charge each atom takes when it forms an ion. If more than one charge is possible, list both.

    1. Ca
    2. I
    3. Fe

  5. Give the charge each atom takes when it forms an ion. If more than than one accuse is possible, list both.

    1. Ag
    2. Au
    3. Br

  6. Give the accuse each atom takes when it forms an ion. If more than ane charge is possible, listing both.

    1. S
    2. Na
    3. H

  7. Name the ions from Practise 3.

  8. Name the ions from Practice iv.

  9. Proper noun the ions from Practice v.

  10. Name the ions from Exercise half dozen.

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

    1. Mg2+ and Cl−
    2. Atomic number 262+ and O2−
    3. Fe3+ and O2−

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

    1. 1000+ and S2−
    2. Ag+ and Br−
    3. Sr2+ and Due norththree−

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

    1. Cu2+ and F−
    2. Caii+ and O2−
    3. G+ and P3−

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

    1. Na+ and N3−
    2. Coii+ and I−
    3. Au3+ and S2−

  15. Requite the formula and proper noun for each ionic compound formed between the two listed ions.

    1. K+ and SOfour 2−
    2. NH4 + and Sii−
    3. NH4 + and PO4 3−

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

    1. Ca2+ and NO3 −
    2. Caii+ and NO2 −
    3. Scthree+ and CtwoH3O2 −

  17. Give the formula and proper name for each ionic compound formed between the 2 listed ions.

    1. Pbfour+ and So4 two−
    2. Na+ and Iiii −
    3. Li+ and Cr2Oseven 2−

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

    1. NHfour + and Norththree−
    2. Mg2+ and CO3 2−
    3. Al3+ and OH−

  19. Give the formula and name for each ionic compound formed between the two listed ions.

    1. Ag+ and SOiii 2−
    2. Na+ and HCOthree −
    3. Fe3+ and ClO3 −

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

    1. Rb+ and O2 2−
    2. Au3+ and HSO4 −
    3. Sr2+ and NO2 −

  21. What is the difference between So3 and And so3 ii−?

  22. What is the deviation between NO2 and NO2 −?

Answers

  1. Cations grade by losing electrons.

    1. 1+
    2. 2−
    3. two+, 3+
    1. ane+
    2. 1+, iii+
    3. 1−
    1. the potassium ion
    2. the oxide ion
    3. the cobalt(Ii) and cobalt(III) ions, respectively
    1. the silver ion
    2. the gold(I) and gold(III) ions, respectively
    3. the bromide ion
    1. magnesium chloride, MgCl2
    2. iron(II) oxide, FeO
    3. iron(Iii) oxide, FeiiO3
    1. copper(II) fluoride, CuF2
    2. calcium oxide, CaO
    3. potassium phosphide, K3P
    1. potassium sulfate, KtwoSOfour
    2. ammonium sulfide, (NHiv)iiS
    3. ammonium phosphate, (NH4)iiiPOiv
    1. lead(IV) sulfate, Pb(And then4)2
    2. sodium triiodide, NaIiii
    3. lithium dichromate, LitwoCrtwoOseven
    1. argent sulfite, Ag2SOiii
    2. sodium hydrogen carbonate, NaHCOthree
    3. iron(Three) chlorate, Fe(ClO3)3

  21. And so3 is sulfur trioxide, while SOthree ii− is the sulfite ion.

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Source: https://saylordotorg.github.io/text_introductory-chemistry/s07-04-ions-and-ionic-compounds.html

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