Naming Simple Compounds Ionic Compounds
Ionic compounds
• consist of positive and negative ions.
• have attractions called ionic bonds between positively and negatively charged ions.
• have high melting and boiling points.
• are solid at room temperature.
Copyright © Houghton Mifflin Company. All rights reserved. 2–2 Salt is An Ionic Compound
Sodium chloride or “table salt” is an example of an ionic compound.
Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–3 Naming Ionic Compounds with Two Elements
To name a compound that contains two elements,
• identify the cation and anion. • name the cation first followed by the name of the anion.
Copyright © Houghton Mifflin Company. All rights reserved. 2–4 Binary Ionic Compounds Type (I)
An ionic formula
• consists of positively and negatively charged ions.
• is neutral.
• has charge balance. total positive charge = total negative charge
The symbol of the metal is written first followed by the symbol of the nonmetal.
Copyright © Houghton Mifflin Company. All rights reserved. 2–5 Charge Balance In MgCl2
In MgCl2, • a Mg atom loses two valence electrons.
• two Cl atoms each gain one electron.
• subscripts indicate the number of ions needed to give charge balance.
Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–6 Charge Balance in Na2S
In Na2S. • two Na atoms lose one valence electron each.
• one S atom gains two electrons.
• subscripts show the number of ions needed to give Copyright © 2005 by Pearson Education, Inc. charge balance. Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–7 Guide to Writing Formulas from the Name
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Copyright © Houghton Mifflin Company. All rights reserved. 2–8 Writing Ionic Formulas from Charges
Charge balance is used to write the formula for sodium nitride, a compound containing Na+ and N3−.
Na+ + 3− 3Na+N =Na3N Na+
3(+1) + 1(3-) = 0
Copyright © Houghton Mifflin Company. All rights reserved. 2–9 The balance of charges in Aluminum Oxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–10 Formula from Ionic Charges
Write the ionic formula of the compound with Ba2+ and Cl−.
• Write the symbols of the ions. Ba2+ Cl− • Balance the charges. Ba2+ Cl− two Cl- needed Cl− • Write the ionic formula using a subscript 2 for two chloride ions that give charge balance.
BaCl2
Copyright © Houghton Mifflin Company. All rights reserved. 2–11 Learning Check
Select the correct formula for each of the following ionic compounds.
A. Na+ and S2-
1) NaS 2) Na2S3) NaS2
B. Al3+ and Cl-
1) AlCl3 2) AlCl 3) Al3Cl
C. Mg2+ and N3-
1) MgN 2) Mg2N3 3) Mg3N2
Copyright © Houghton Mifflin Company. All rights reserved. 2–12 Solution
A. Na+ and S2-
2) Na2S check: 2Na+ + S2- = 2(1+) + 1(2-) = 0
B. Al3+ and Cl-
1) AlCl3 check: Al3+ + Cl- = (3+) + 3(1-) = 0
C. Mg2+ and N3-
3) Mg3N2 check: 2Mg2+ +2N3- = 2(3+) + 2(3-) = 0
Copyright © Houghton Mifflin Company. All rights reserved. 2–13 Useful relationships from the periodic table
Copyright © Houghton Mifflin Company. All rights reserved. 2–14 Names of Some Common Ions
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Copyright © Houghton Mifflin Company. All rights reserved. 2–15 Examples of Ionic Compounds with Two Elements
Formula Ions Name cation anion NaCl Na+ Cl- sodium chloride + 2- K2SKS potassium sulfide MgO Mg2+ O2- magnesium oxide 2+ - CaI2 Ca I calcium iodide 3+ 2- Al2O3 Al O aluminum oxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–16 Learning Check
Write the formulas and names for compounds of the following ions: Br− S2− N3−
Na+
Al3+
Copyright © Houghton Mifflin Company. All rights reserved. 2–17 Solution
Br− S2− N3−
NaBr Na2S Na3N sodium sodium sodium Na+ bromide sulfide nitride
AlBr3 Al2S3 AlN aluminum aluminum aluminum bromide sulfide nitride Al3+
Copyright © Houghton Mifflin Company. All rights reserved. 2–18 Binary Ionic Compounds (Type II) Transition Metals form Positive Ions
Most transition metals and Group 4(14) metals form 2 or more positive ions.
Zn2+,Ag+, and Cd2+ form only one ion.
Copyright © Houghton Mifflin Company. All rights reserved. 2–19 Metals that form more than One Cation
The name of metals with two or more positive ions (cations) use a Roman numeral to identify ionic charge.
Lead Pb2+ lead(II) Pb4+ lead(IV)
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Copyright © Houghton Mifflin Company. All rights reserved. 2–20 Naming Ionic Compounds with Variable Charge Metals
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Copyright © Houghton Mifflin Company. All rights reserved. 2–21 Naming Variable Charge Metals
Transition metals with two different ions use a Roman numeral after the name of the metal to indicate ionic charge.
Copyright © Houghton Mifflin Company. All rights reserved. 2–22 Naming FeCl2
To name FeCl2 1. Determine the charge of the cation using the charge of the anion (Cl-). Fe ion + 2 Cl- = Fe ion + 2- = 0 Fe ion = 2+ 2. Name the cation by the element name and add a Roman numeral in parenthesis to show its charge. Fe2+ = iron(II) 3. Write the anion with an ide ending.
FeCl2 = iron(II) chloride
Copyright © Houghton Mifflin Company. All rights reserved. 2–23 Naming Cr2O3
To name Cr2O3 1. Determine the charge of cation from the anion (O2-). 2 Cr ions + 3 O2- = 0 2 Cr ions + 3 (2-) = 0 2 Cr ions - 6 = 0 2 Cr ions = +6 Cr ion = 3+ = Cr3+ 2. Name the cation by the element name and add a Roman numeral in parenthesis to show its charge. Cr3+ = chromium(III) 3. Write the anion with an ide ending.
chromium(III) oxide = Cr2O3
Copyright © Houghton Mifflin Company. All rights reserved. 2–24 Learning Check
Select the correct name for each.
A. Fe2S3 1) iron sulfide 2) iron(II) sulfide 3) iron(III) sulfide
B. CuO 1) copper oxide 2) copper(I) oxide 3) copper(II) oxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–25 Solution
Select the correct name for each.
A. Fe2S3 3) iron (III) sulfide Fe3+ S2-
B. CuO 3) copper (II) oxide Cu2+ O2-
Copyright © Houghton Mifflin Company. All rights reserved. 2–26 Binary Compounds with Polyatomic Ions
A polyatomic ion • is a group of atoms. • has an overall ionic charge.
Some examples of polyatomic ions are + − NH4 ammonium OH hydroxide − − NO3 nitrate NO2 nitrite 2− 3− CO3 carbonate PO4 phosphate − HCO3 hydrogen carbonate (bicarbonate)
Copyright © Houghton Mifflin Company. All rights reserved. 2–27 Some Compounds with Polyatomic Ions
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Copyright © Houghton Mifflin Company. All rights reserved. 2–28 Copyright © Houghton Mifflin Company. All rights reserved. 2–29 Some Names of Polyatomic Ions
The names of common polyatomic anions • end in ate. − 3− NO3 nitrate PO4 phosphate • with one oxygen less end in ite. − 3− NO2 nitrite PO3 phosphite • with hydrogen attached use the prefix hydrogen (or bi). − HCO3 hydrogen carbonate (bicarbonate) − HSO3 hydrogen sulfite (bisulfite)
Copyright © Houghton Mifflin Company. All rights reserved. 2–30 Names and Formulas of Common Polyatomic Ions
oxyanions
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Copyright © Houghton Mifflin Company. All rights reserved. 2–31 Names and Formulas of Common Polyatomic Ions
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Copyright © Houghton Mifflin Company. All rights reserved. 2–32 Naming Compounds with Polyatomic Ions
• The positive ion is named first followed by the name of the polyatomic ion.
NaNO3 sodium nitrate
K2SO4 potassium sulfate
Fe(HCO3)3 iron(III) bicarbonate or iron(III) hydrogen carbonate
(NH4)3PO3 ammonium phosphite
Copyright © Houghton Mifflin Company. All rights reserved. 2–33 Formation of Ionic Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–34 Some Compounds with Polyatomic Ions
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Copyright © Houghton Mifflin Company. All rights reserved. 2–35 Learning Check
Match each formula with the correct name.
A. MgS 1) magnesium sulfite
MgSO3 2) magnesium sulfate
MgSO4 3) magnesium sulfide
B. Ca(ClO3)2 1) calcium chlorate
CaCl2 2) calcium chlorite
Ca(ClO2)2 3) calcium chloride
Copyright © Houghton Mifflin Company. All rights reserved. 2–36 Solution
Match each formula with the correct name:
A. MgS 3) magnesium sulfide
MgSO3 1) magnesium sulfite
MgSO4 2) magnesium sulfate
B. Ca(ClO3)2 1) calcium chlorate
CaCl2 3) calcium chloride
Ca(ClO2)2 2) calcium chlorite
Copyright © Houghton Mifflin Company. All rights reserved. 2–37 Learning Check
Name each of the following compounds:
A. Mg(NO3)2
B. Cu(ClO3)2
C. PbO2
D. Fe2(SO4)3
E. Ba3(PO3)2
Copyright © Houghton Mifflin Company. All rights reserved. 2–38 Solution
Name each of the following compounds:
A. Mg(NO3)2 magnesium nitrate
B. Cu(ClO3)2 copper(II) chlorate
C. PbO2 lead(IV) oxide
D. Fe2(SO4)3 iron(III) sulfate
E. Ba3(PO3)2 barium phosphite
Copyright © Houghton Mifflin Company. All rights reserved. 2–39 Writing Formulas with Polyatomic Ions
The formula of an ionic compound • containing a polyatomic ion must have a charge balance that equals zero (0). + − Na and NO3 Æ NaNO3
• with two or more polyatomic ions has the polyatomic ions in parentheses. 2+ − Mg and 2NO3 Æ Mg(NO3)2 subscript 2 for charge balance
Copyright © Houghton Mifflin Company. All rights reserved. 2–40 Learning Check
Select the correct formula for each. A. aluminum nitrate
1) AlNO3 2) Al(NO)3 3) Al(NO3)3 B. copper(II) nitrate
1) CuNO3 2) Cu(NO3)2 3) Cu2(NO3) C. iron(III) hydroxide
1) FeOH 2) Fe3OH 3) Fe(OH)3 D. tin(IV) hydroxide
1) Sn(OH)4 2) Sn(OH)2 3) Sn4(OH)
Copyright © Houghton Mifflin Company. All rights reserved. 2–41 Solution
Select the correct formula for each.
A. aluminum nitrate
3) Al(NO3)3 B. copper(II) nitrate
2) Cu(NO3)2 C. iron(III) hydroxide
3) Fe(OH)3 D. tin(IV) hydroxide
1) Sn(OH)4
Copyright © Houghton Mifflin Company. All rights reserved. 2–42 Learning Check
Write the correct formula for each.
A. potassium bromate B. calcium carbonate C. sodium phosphate D. iron(III) oxide E. iron(II) nitrite
Copyright © Houghton Mifflin Company. All rights reserved. 2–43 Solution
Write the correct formula for each.
A. potassium bromate KBrO3
B. calcium carbonate CaCO3
C. sodium phosphate Na3PO4
D. iron(III) oxide Fe2O3
E. iron(II) nitrite Fe(NO2)2
Copyright © Houghton Mifflin Company. All rights reserved. 2–44 Rules for Naming Ionic Compounds
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Copyright © Houghton Mifflin Company. All rights reserved. 2–45 Flowchart for Naming Ionic Compounds
Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings Copyright © Houghton Mifflin Company. All rights reserved. 2–46 Molecular vs. Ionic Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–47 Covalent Bonding
Copyright © Houghton Mifflin Company. All rights reserved. 2–48 QUESTION
Hypochlorous acid is related to the anion found in common household bleach. Which of the following is that common anion?
– 1. ClO4 – 2. ClO3 – 3. ClO2 4. ClO–
Copyright © Houghton Mifflin Company. All rights reserved. 2–49 QUESTION
Which of the following provides the correct name for
Ca(H2PO4)2?
1. Calcium dihydrogen phosphate 2. Calcium (II) hydrogen phosphate 3. Calcium di-dihydrogen phosphate 4. Calcium (II) dihydrogen phosphate
Copyright © Houghton Mifflin Company. All rights reserved. 2–50 Binary Covalent Compounds (Type III)
Covalent bonds form
• when atoms share electrons to complete octets.
• between two nonmetal atoms.
• between nonmetal atoms from Groups 4A(14), 5A(15), 6A(16), and 7A(17).
Copyright © Houghton Mifflin Company. All rights reserved. 2–51 Naming Covalent Compounds
To name covalent Table 2.6 compounds • STEP 1: Name the first nonmetal as an element. • STEP 2: Name the second nonmetal with an ide ending. • STEP 3: Use prefixes to indicate the number of atoms (subscript) of each element.
Copyright © Houghton Mifflin Company. All rights reserved. 2–52 Naming Covalent Compounds
What is the name of SO3?
1. The first nonmetal is S sulfur. 2. The second nonmetal is O named oxide. 3. The subscript 3 of O is shown as the prefix tri.
SO3 Æ sulfur trioxide
The subscript 1 (for S) or mono is understood.
Copyright © Houghton Mifflin Company. All rights reserved. 2–53 Naming Covalent Compounds
Name P4S3.
1. The first nonmetal P is phosphorus. 2. The second nonmetal S is sulfide. 3. The subscript 4 of P is shown as tetra. The subscript 3 of S is shown as tri.
P4S3 Æ tetraphosphorus trisulfide
Copyright © Houghton Mifflin Company. All rights reserved. 2–54 Formulas and Names of Some Covalent Compounds
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Copyright © Houghton Mifflin Company. All rights reserved. 2–55 Learning Check
Select the correct name for each compound.
A. SiCl4 1) silicon chloride 2) tetrasilicon chloride 3) silicon tetrachloride
B. P2O5 1) phosphorus oxide 2) phosphorus pentoxide 3) diphosphorus pentoxide
C. Cl2O7 1) dichlorine heptoxide 2) dichlorine oxide 3) chlorine heptoxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–56 Solution
Select the correct name for each compound.
A. SiCl4 3) silicon tetrachloride
B. P2O5 3) diphosphorus pentoxide
C. Cl2O7 1) dichlorine heptoxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–57 Learning Check
Write the name of each covalent compound.
CO ______
CO2 ______
PCl3 ______
CCl4 ______
N2O ______
Copyright © Houghton Mifflin Company. All rights reserved. 2–58 Solution
Write the name of each covalent compound.
CO carbon monoxide
CO2 carbon dioxide
PCl3 phosphorus trichloride
CCl4 carbon tetrachloride
N2O dinitrogen monoxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–59 Guide to Writing Formulas
The prefixes in the name are used to write the formula. STEP 1: Write the symbols in the order of the elements in the name. STEP 2: Write any prefixes as subscripts.
Example: Write the formula for carbon disulfide. STEP 1: Elements are C and S STEP 2: No prefix for carbon means 1 C Prefix di = 2
Formula: CS2
Copyright © Houghton Mifflin Company. All rights reserved. 2–60 Learning Check
Write the correct formula for each of the following.
A. phosphorus pentachloride
B. dinitrogen trioxide
C. sulfur hexafluoride
Copyright © Houghton Mifflin Company. All rights reserved. 2–61 Solution
Write the correct formula for each of the following.
A. phosphorus pentachloride
1 P penta = 5 Cl PCl5
B. dinitrogen trioxide
di = 2 N tri = 3 O N2O3
C. sulfur hexafluoride
1 S hexa = 6 F SF6
Copyright © Houghton Mifflin Company. All rights reserved. 2–62 Learning Check
Identify each compound as ionic or covalent and give its correct name.
A. SO3
B. BaCl2
C. (NH4)3PO4
D. Cu2CO3
E. N2O4
Copyright © Houghton Mifflin Company. All rights reserved. 2–63 Copyright © Houghton Mifflin Company. All rights reserved. 2–64 Binary Acids
Acids produce H+ when dissolved in water. They are compounds that ionize in water. If the anion does not contain oxygen:
HCl hydrogen chloride hydrochloric acid HF hydrogen fluoride hydrofluoric acid
If the anion contain oxygen
Anion ends in-ate, the suffix –ic is added to the root name. Anion ends in –ite, the suffix –ous.
Copyright © Houghton Mifflin Company. All rights reserved. 2–65 Copyright © Houghton Mifflin Company. All rights reserved. 2–66