A system of names used in a science. The key to learning such a system ...
Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third
Edition ...
Chapter 6
Section 6.1
Chemical Nomenclature
Introduction to Nomenclature
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Nomenclature: A system of names used in a science.
The key to learning such a system is to minimize memorization and develop an understanding of a systematic procedure for naming chemical compounds.
Section 6.2 Formulas of Elements
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Goal 1
In Chapter 5 you learned the symbols of 35 elements. In this chapter you will learn the chemical formulas of those elements.
Given a name or formula of an element in Figure 5.9, write the other.
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Molecule: The tiniest independent particle of a pure substance.
For most elements, the smallest independent particle is a single atom. Their formula is the elemental symbol. Examples Element
Formula
Helium Lithium
He Li
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Seven elements form diatomic molecules under normal conditions Di- means two The smallest particle of these elements is two atoms that are chemically attached to each other The chemical formula of a diatomic molecule is the elemental symbol followed by a subscript of 2 Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
7 elements occur in nature as diatomic (two-atom) molecules: the formula of hydrogen is H2 the formula of nitrogen is N2 the formula of oxygen is O2 the formula of fluorine is F2 the formula of chlorine is Cl2 the formula of bromine is Br2 the formula of iodine is I2
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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He Some other elements commonly form polyatomic (many-atom) molecules. However, their natural molecular form varies, so we will write their formulas as if they were monatomic (one-atom) species. This will not affect calculations involving these elements.
Element
Formula
carbon phosphorus sulfur
C P S
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2
Cl2
S or S8
P or P4
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Section 6.3 C or C60
Compounds Made from Two Nonmetals
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Goal 2
Goal 3
Given the name or formula of a binary molecular compound, write the other.
Given the name or the formula of water, write the other; given the name or the formula of ammonia, write the other.
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The stair-step line in the periodic table separates elements on the left that are metals from elements on the right that are nonmetals. Several elements bordering on this line are metalloids or semimetals.
Compounds formed by two nonmetals or a metalloid and a nonmetal are called binary molecular compounds.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Naming binary molecular compounds: 1. The first word is the name of the first element in the compound, modified with a prefix to indicate the number of atoms of that element in the molecule. 2. The second word is the name of the second element in the compound, changed to end in -ide, modified with a prefix to indicate the number of atoms of that element in the molecule.
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1
mono-
Examples:
2
di-
3
tri-
Write the name of I2O5. 2 = di-
4
tetra-
I = iodine
5
penta-
first word is diiodine
6
hexa-
5 = penta-
7
hepta-
O = oxygen
8
octa-
change 2nd word to end in -ide = oxide
9
nona-
second word is pentoxide
10
deca-
Answer: diiodine pentoxide
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Write the formula of nitrogen trifluoride.
Two important exceptions to the binary molecular compound nomenclature rules:
No prefix on first word = mono- is implied: 1 The symbol of nitrogen is N 2nd word prefix tri- = 3
H2O is water
-fluoride is an “-ide modified” fluorine = F Answer: NF3
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NH3 is ammonia
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Goal 4 Section 6.4 Names and Formulas of Ions Formed by One Element Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Given the name or formula of an ion in Figure 6.3, write the other.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Ion: Charged particle formed when a neutral atom or molecule loses or gains electrons Cation: Positively-charged ion. Formed when a neutral atom or molecule loses one or more electrons.
Figure 6.3
Anion: Negatively-charged ion. Formed when a neutral atom or molecule gains one or more electrons.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Monatomic ion: Ion formed from a single (mono-) atom
Name of a monatomic cation: Name of element, followed by the word ion
Formula of a monatomic ion: Elemental symbol followed by superscript size of charge and sign of charge (if the size of the charge is 1, the 1 is omitted)
Name of a monatomic anion: Name of element changed to end in -ide, followed by the word ion
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The charge on a main-group (U.S. A group) ion corresponds to its group number:
Group
1A
2A
3A
5A
6A
7A
Charge
1+
2+
3+
3–
2–
1–
Examples: What is the the formula of sodium ion? Sodium is in Group 1A, so its ion has a 1+ charge We write the symbol of the element, followed by the charge in superscript, omitting the 1 Na+
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
What is are the name and formula of the ion formed from a sulfur atom?
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Many transition elements (U.S. B groups) form multiple ions with different charges
Sulfur is in Group 6A, so it forms 2– ions; write the symbol of the element, followed by the charge in superscript:
All transition-element ions have a positive charge
S2–
To distinguish among the ions, the magnitude of the charge is included with its name:
A monatomic anion is named by changing the name of the element to end in -ide, followed by the word ion: sulfide ion
Cr2+ is chromium(II) ion Cr3+ is chromium(III) ion
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Three of the transition element ions almost always occur with only one charge, so chemists do not write the magnitude of the charge in their names:
The mercury(I) ion is a special case:
2+
Ni is nickel ion Zn2+ is zinc ion Ag+ is silver ion
it is a diatomic (two-atom) ion: Hg22+ It is named as if single atoms existed separately: mercury(I) ion
You must memorize their charges
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Example: What is the formula of copper(II) ion? What is the name of Zn2+?
The symbol for copper is Cu (II) indicates the 2+ ion Cu2+ The name of Zn is zinc Zinc has just one common charge, so its charge is not included in its name zinc ion Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Ionic compound: A combination of cations and anions that form a crystalline solid Must be electrically neutral
Section 6.8 Formulas of Ionic Compounds
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How to Write the Formula of an Ionic Compound Write the formula of the cation, followed by the formula of the anion, omitting the charges Insert subscripts to show the number of each ion needed in the formula unit to make the sum of the charges equal to zero with the fewest number of ions possible If only one ion is needed, omit the subscript If a polyatomic ion is needed more than once, enclose the formula of the ion in parentheses and place the subscript after the closing parenthesis
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Examples: What is the formula of magnesium chloride?
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Refer to this table for your Polyatomic ions. Some General Chemistry Courses will require you to memorize most of these. Be prepared to do that!!!
Magnesium ion is in Group 2A/2, so its formula is Mg2+ Chlorine is in Group 7A/17, so chloride ion is Cl– Two 1– ions are needed to balance the 2+ ion MgCl2
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What is the formula of barium nitrate? What is the formula of aluminum oxide? Aluminum is in Group 3A/13, so aluminum ion is Al3+ Oxygen in in Group 6A/16, so oxide ion is O2– The least common multiple of 2 and 3 is 6, so 2 x 3+ balances 3 x 2– Al2O3 Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Barium is in Group 2A/2, so barium ion is Mg2+ The formula of nitric acid is HNO3, so nitrate ion is what results when the H+ is removed, so it is a 1– ion, NO3– Two 1– ions are needed to balance the charge of the 2+ ion, and to retain the identity of the nitrate ion, enclose it in parentheses Ba(NO3)2 Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Goal 9 Section 6.9 Names of Ionic Compounds
Given the formula of an ionic compound made up of identifiable ions, write the name of the compound.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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How to Write the Name of an Ionic Compound
Examples: Write the name of the following compound: Zn(NO3)2
Write the name of the cation Write the name of the anion To name an ionic compound containing a metal that commonly is capable of having more than one ionic charge, the compound name includes the charge of that metal Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Zinc ion has only one common charge, 2+, so the magnitude of the charge is not included in its name: zinc ion NO3– comes from the memorized acid HNO3, nitric acid -ic changes to -ate: nitrate ion zinc nitrate Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Examples: Write the name of the following compound: CoCl2 Cobalt ion has more than one common charge Chlorine, Cl, is in Group 7A/17, so it forms a 1– ion that ends in -ide: chloride ion Two 1– ions means the positive charge must be 2+: cobalt(II) ion
Section 6.11 Summary of the Nomenclature System
cobalt(II) chloride Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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Section 6.12 Common Names of Chemicals
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Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
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