Organic Chemistry Topics 10 & 20 Chapter 22 PART 1: Naming Organic Compounds.
Naming Simple Compounds - Chemistry - California State University
Transcript of Naming Simple Compounds - Chemistry - California State University
Naming Simple Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–2
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.
Ionic Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–3
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. 2–4
Naming Ionic Compounds with Two Elements
To name a compound that contains two elements,
• identify the cationand anion.
• name the cation first followed by the name of the anion.
Copyright © Houghton Mifflin Company. All rights reserved. 2–5
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.
Binary Ionic Compounds Type (I)
Copyright © Houghton Mifflin Company. All rights reserved. 2–6
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. 2–7
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 charge balance.
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–8
Guide to Writing Formulas from the Name
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–9
Writing Ionic Formulas from Charges
Charge balance is used to write the formula forsodium nitride, a compound containing Na+ and N3−.
Na+
3 Na+ + N3− = Na3NNa+
3(+1) + 1(3-) = 0
Copyright © Houghton Mifflin Company. All rights reserved. 2–10
The balance of charges in Aluminum Oxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–11
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
Formula from Ionic Charges
Copyright © Houghton Mifflin Company. All rights reserved. 2–12
Select the correct formula for each of the following ionic compounds.
A. Na+ and S2-
1) NaS 2) Na2S 3) NaS2
B. Al3+ and Cl-
1) AlCl3 2) AlCl 3) Al3Cl
C. Mg2+ and N3-
1) MgN 2) Mg2N3 3) Mg3N2
Learning Check
Copyright © Houghton Mifflin Company. All rights reserved. 2–13
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
Solution
Copyright © Houghton Mifflin Company. All rights reserved. 2–14
Useful relationships from the periodic table
Copyright © Houghton Mifflin Company. All rights reserved. 2–15
Names of Some Common Ions
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–16
Formula Ions Namecation anion
NaCl Na+ Cl- sodium chloride
K2S K+ S2- potassium sulfide
MgO Mg2+ O2- magnesium oxide
CaI2 Ca2+ I- calcium iodide
Al2O3 Al3+ O2- aluminum oxide
Examples of Ionic Compounds with Two Elements
Copyright © Houghton Mifflin Company. All rights reserved. 2–17
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. 2–18
Solution
Br− S2− N3−
Na+
Al3+
NaBrsodium bromide
Na2Ssodium sulfide
Na3Nsodium nitride
AlBr3
aluminum bromide
Al2S3
aluminum sulfide
AlNaluminum nitride
Copyright © Houghton Mifflin Company. All rights reserved. 2–19
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. 2–20
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.
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Lead Pb2+ lead(II)Pb4+ lead(IV)
Copyright © Houghton Mifflin Company. All rights reserved. 2–21
Naming Ionic Compounds with Variable Charge Metals
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–22
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. 2–23
Naming FeCl2
To name FeCl21. Determine the charge of the cation using the charge
of the anion (Cl-).Fe ion + 2 Cl- = Fe ion + 2- = 0Fe ion = 2+
2. Name the cation by the element name and add aRoman 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. 2–24
Naming Cr2O3
To name Cr2O31. Determine the charge of cation from the anion (O2-).
2 Cr ions + 3 O2- = 02 Cr ions + 3 (2-) = 0 2 Cr ions - 6 = 02 Cr ions = +6 Cr ion = 3+ = Cr3+
2. Name the cation by the element name and add aRoman 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. 2–25
Learning Check
Select the correct name for each.A. Fe2S3
1) iron sulfide2) iron(II) sulfide3) iron(III) sulfide
B. CuO1) copper oxide2) copper(I) oxide 3) copper(II) oxide
Copyright © Houghton Mifflin Company. All rights reserved. 2–26
Solution
Select the correct name for each.A. Fe2S3
3) iron (III) sulfide Fe3+ S2-
B. CuO3) copper (II) oxide Cu2+ O2-
Copyright © Houghton Mifflin Company. All rights reserved. 2–27
A polyatomic ion• is a group of atoms. • has an overall ionic charge.
Some examples of polyatomic ions areNH4
+ ammonium OH− hydroxide
NO3− nitrate NO2
− nitrite
CO32− carbonate PO4
3− phosphateHCO3
− hydrogen carbonate(bicarbonate)
Binary Compounds with Polyatomic Ions
Copyright © Houghton Mifflin Company. All rights reserved. 2–28
Some Compounds with Polyatomic Ions
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–29
Copyright © Houghton Mifflin Company. All rights reserved. 2–30
The names of common polyatomic anions
• end in ate.
NO3− nitrate PO4
3− phosphate• with one oxygen less end in ite.
NO2− nitrite PO3
3− phosphite• with hydrogen attached use the prefix hydrogen (or bi).
HCO3− hydrogen carbonate (bicarbonate)
HSO3− hydrogen sulfite (bisulfite)
Some Names of Polyatomic Ions
Copyright © Houghton Mifflin Company. All rights reserved. 2–31
Names and Formulas of Common Polyatomic Ions
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
oxyanions
Copyright © Houghton Mifflin Company. All rights reserved. 2–32
Names and Formulas of Common Polyatomic Ions
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–33
• 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
Naming Compounds with Polyatomic Ions
Copyright © Houghton Mifflin Company. All rights reserved. 2–34
Formation of Ionic Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–35
Some Compounds with Polyatomic Ions
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–36
Match each formula with the correct name.
A. MgS 1) magnesium sulfite MgSO3 2) magnesium sulfateMgSO4 3) magnesium sulfide
B. Ca(ClO3)2 1) calcium chlorateCaCl2 2) calcium chloriteCa(ClO2)2 3) calcium chloride
Learning Check
Copyright © Houghton Mifflin Company. All rights reserved. 2–37
Match each formula with the correct name:
A. MgS 3) magnesium sulfideMgSO3 1) magnesium sulfite MgSO4 2) magnesium sulfate
B. Ca(ClO3)2 1) calcium chlorateCaCl2 3) calcium chlorideCa(ClO2)2 2) calcium chlorite
Solution
Copyright © Houghton Mifflin Company. All rights reserved. 2–38
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. 2–39
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. 2–40
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− NaNO3
• with two or more polyatomic ions has the polyatomic ions in parentheses.
Mg2+ and 2NO3− Mg(NO3)2
subscript 2 for charge balance
Copyright © Houghton Mifflin Company. All rights reserved. 2–41
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)
Learning Check
Copyright © Houghton Mifflin Company. All rights reserved. 2–42
Select the correct formula for each.
A. aluminum nitrate 3) Al(NO3)3
B. copper(II) nitrate2) Cu(NO3)2
C. iron(III) hydroxide3) Fe(OH)3
D. tin(IV) hydroxide1) Sn(OH)4
Solution
Copyright © Houghton Mifflin Company. All rights reserved. 2–43
Learning Check
Write the correct formula for each.
A. potassium bromateB. calcium carbonateC. sodium phosphateD. iron(III) oxideE. iron(II) nitrite
Copyright © Houghton Mifflin Company. All rights reserved. 2–44
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. 2–45
Rules for Naming Ionic Compounds
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–46
Flowchart for Naming Ionic Compounds
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–47
Molecular vs. Ionic Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–48
Covalent Bonding
Copyright © Houghton Mifflin Company. All rights reserved. 2–49
QUESTIONHypochlorous 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. 2–50
QUESTIONWhich of the following provides the correct name for Ca(H2PO4)2?
1. Calcium dihydrogen phosphate2. Calcium (II) hydrogen phosphate3. Calcium di-dihydrogen phosphate4. Calcium (II) dihydrogen phosphate
Copyright © Houghton Mifflin Company. All rights reserved. 2–51
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).
Binary Covalent Compounds (Type III)
Copyright © Houghton Mifflin Company. All rights reserved. 2–52
Naming Covalent Compounds
To name covalent compounds
• STEP 1: Name the first nonmetal as an element.
• STEP 2: Name the second nonmetal with an ideending.
• STEP 3: Use prefixes to indicate the number of atoms (subscript) of each element.
Table 2.6
Copyright © Houghton Mifflin Company. All rights reserved. 2–53
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 sulfur trioxide
The subscript 1 (for S) or mono is understood.
Naming Covalent Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–54
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 tetraphosphorus trisulfide
Naming Covalent Compounds
Copyright © Houghton Mifflin Company. All rights reserved. 2–55
Formulas and Names of Some Covalent Compounds
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
Copyright © Houghton Mifflin Company. All rights reserved. 2–56
Select the correct name for each compound.A. SiCl4 1) silicon chloride
2) tetrasilicon chloride3) silicon tetrachloride
B. P2O5 1) phosphorus oxide2) phosphorus pentoxide3) diphosphorus pentoxide
C. Cl2O7 1) dichlorine heptoxide2) dichlorine oxide3) chlorine heptoxide
Learning Check
Copyright © Houghton Mifflin Company. All rights reserved. 2–57
Select the correct name for each compound.
A. SiCl4 3) silicon tetrachlorideB. P2O5 3) diphosphorus pentoxideC. Cl2O7 1) dichlorine heptoxide
Solution
Copyright © Houghton Mifflin Company. All rights reserved. 2–58
Write the name of each covalent compound.
CO _____________________
CO2 _____________________
PCl3 _____________________
CCl4 _____________________
N2O _____________________
Learning Check
Copyright © Houghton Mifflin Company. All rights reserved. 2–59
Write the name of each covalent compound.
CO carbon monoxide
CO2 carbon dioxide
PCl3 phosphorus trichloride
CCl4 carbon tetrachloride
N2O dinitrogen monoxide
Solution
Copyright © Houghton Mifflin Company. All rights reserved. 2–60
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 SSTEP 2: No prefix for carbon means 1 C
Prefix di = 2Formula: CS2
Guide to Writing Formulas
Copyright © Houghton Mifflin Company. All rights reserved. 2–61
Write the correct formula for each of the following.
A. phosphorus pentachloride
B. dinitrogen trioxide
C. sulfur hexafluoride
Learning Check
Copyright © Houghton Mifflin Company. All rights reserved. 2–62
Write the correct formula for each of the following.
A. phosphorus pentachloride1 P penta = 5 Cl PCl5
B. dinitrogen trioxidedi = 2 N tri = 3 O N2O3
C. sulfur hexafluoride
1 S hexa = 6 F SF6
Solution
Copyright © Houghton Mifflin Company. All rights reserved. 2–63
Learning Check
Identify each compound as ionic or covalent and give itscorrect name.
A. SO3
B. BaCl2C. (NH4)3PO4
D. Cu2CO3
E. N2O4
Copyright © Houghton Mifflin Company. All rights reserved. 2–64
Copyright © Houghton Mifflin Company. All rights reserved. 2–65
Binary Acids
If the anion does not contain oxygen:
HCl hydrogen chloride hydrochloric acid
HF hydrogen fluoride hydrofluoric acid
Acids produce H+ when dissolved in water.
They are compounds that ionize in water.
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. 2–66