Presentation is loading. Please wait.

Presentation is loading. Please wait.

Chapter 6 Chemical Nomenclature

Similar presentations


Presentation on theme: "Chapter 6 Chemical Nomenclature"— Presentation transcript:

1 Chapter 6 Chemical Nomenclature

2 Metals, Nonmetals and Metalloids
The stair-step line in the periodic table separates metals from nonmetals. Elements bordering this line are metalloids

3 Formulas of Elements For most elements, the smallest independent particle is an atom. The formula of the element is the elemental symbol. Element Formula Helium He Lithium Li

4 Seven elements form stable diatomic molecules
Formulas of Elements Seven elements form stable diatomic molecules

5 Compounds of Two Nonmetals
Binary Molecular Compound A compound formed by two nonmetals or a metalloid and a nonmetal.

6 Compounds of Two Nonmetals
Naming Binary Molecular Compounds The first word is the name of the first element. A prefix is used to indicate the number of atoms. The second word is the name of the second element, changed to end in –ide.

7 Compounds of Two Nonmetals
Number prefixes used in chemical names Number Prefix Number Prefix 1 mono hexa- 2 di hepta- 3 tri octa- 4 tetra nona- 5 penta deca-

8 Compounds of Two Nonmetals
Write the name of N2O5. N = nitrogen; 2 = di The first word is dinitrogen O = oxygen, Change oxygen to end in -ide: oxide; 5 = penta The second word is pentoxide (the letter a in prefixes is omitted if the resulting word sounds better) dinitrogen pentoxide

9 Compounds of Two Nonmetals
Write the formula of nitrogen trifluoride. No prefix on the first word, so mono- is implied = 1 atom. The symbol of nitrogen is N. Tri- prefix on the second word = 3 atoms. -fluoride is an “-ide modified” fluorine = F. NF3

10 Compounds of Two Nonmetals
Two compounds are so common they are always called by their traditional names: H2O is water NH3 is ammonia

11 Ions, Cations, Anions Ion Charged particle formed when a neutral atom
or molecule loses or gains electrons. Cation Positively charged ion. Anion Negatively charged ion.

12 Ions formed by One Element
The charge on a main-group (U.S. A group) ion corresponds to its group number: Group 1A 2A 3A 5A 6A 7A Charge – 2– 1–

13 Ions Formed by One Element

14 Ions Formed by One Element
Name of a monatomic cation Name of element, followed by the word ion. Name of a monatomic anion Name of element changed to end in -ide,

15 Ions Formed by One Element
What is the formula of a sodium ion? Na+

16 Ions Formed by One Element
What are the name and formula of the ion formed from a chlorine atom? Cl– Change the name chlorine to end in –ide. Chloride ion

17 Ions Formed by One Element
Many transition elements (U.S. B groups) form multiple ions. The charge is shown by a Roman numeral enclosed in parentheses. Cr2+ is the chromium(II) ion Cr3+ is the chromium(III) ion

18 Ions Formed by One Element
Some transition element ions always occur with only one charge Zn2+ is zinc ion Ag+ is silver ion Ni2+ nickel ion Special Case Hg22+ is called mercury(I) ion.

19 Cations

20 Anions

21 H3O+ is called hydronium ion.
Acids and Their Anions Acid Molecular compound that reacts with water to produce a hydrated hydrogen ion and an anion. Ionization of hydrochloric acid HCl H2O + HCl → H3O+ + Cl– H3O+ is called hydronium ion.

22 The Acids of Chlorine and Their Anions
Acids and Their Anions The Acids of Chlorine and Their Anions # of O atoms Acid prefix Anion prefix Compared with and/or suffix and/or suffix -ic acid and -ate anion (Example) (Example) One more per ic per- -ate HClO4 (perchloric) (perchlorate) Same ic ate HClO3 (chloric) (chlorate) One fewer ous ite HClO2 (chlorous) (chlorite) Two fewer hypo- -ous hypo- -ite HClO (hypochlorous) (hypochlorite) No oxygen hydro- -ic ide HCl (hydrochloric) (chloride)

23 The names and formulas of following acids should be memorized
Acids and Their Anions The names and formulas of following acids should be memorized Acid Ionization Equation Ion Name Chloric acid HClO H+ + ClO3– Chlorate ion Nitric acid HNO H+ + NO3– Nitrate ion Sulfuric acid H2SO H+ + SO42– Sulfate ion Carbonic acid H2CO H+ + CO32– Carbonate ion Phosphoric acid H3PO H+ + PO43– Phosphate ion

24 Step-by-Step Acid Anion Nomenclature
Acid Anions Step-by-Step Acid Anion Nomenclature H3PO4 phosphoric acid H2PO4– dihydrogen phosphate ion HPO42– hydrogen phosphate ion PO43– phosphate ion

25 Acids and Their Anions

26 Formulas of Ionic Compounds
A compound made up of ions. The formula unit must have an equal number of positive and negative charges.

27 Formulas of Ionic Compounds
Formula of the cation, followed by the formula of the anion. (omit the charges). Subscripts are used to show the number of each ion in the formula unit. (sum of charges must equal to zero) Omit the subscript if only one ion is needed. Enclose formula of the polyatomic ion in parentheses and place the subscript after the closing parentheses.

28 Formulas of Ionic Compounds
What is the formula of magnesium chloride? Magnesium is in Group 2A, so its ion is Mg2+. Chlorine is in Group 7A, so its ion is Cl–. Two 1– ions are needed to balance the 2+ ion. MgCl2.

29 Formulas of Ionic Compounds
What is the formula of barium nitrate? Barium cation is Ba2+ Nitrate anion is NO3– Nitrate ion must be enclosed in parentheses Ba(NO3)2

30 Memorize the following common and important ions:
Other Acids and Ions Memorize the following common and important ions: Hydroxide ion OH– Ammonium ion NH4+

31 Names of Ionic Compounds
Example: Write the name of Zn(NO3)2. Solution: 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. To name the ion, the -ic ending changes to -ate: nitrate ion. Zinc nitrate

32 Names of Ionic Compounds
How to Write the Name of an Ionic Compound Write the name of the cation. Write the name of the anion.

33 Names of Ionic Compounds
Write the name of CoCl2. There is more than one common charge for cobalt ions. We will have to use the anion to determine this charge. Chlorine is in Group 7A, so the charge on the ion is 1–: Cl–. The name of the anion is changed to end in -ide: chloride ion. Two 1– ions require a 2+ ion to balance the charge: cobalt(II) ion. Cobalt(II) chloride

34 Hydrates Hydrate A solid compound that includes water molecules as part of its crystal structure.

35 Water of crystallization
Hydrates Water of crystallization Water molecules that are part of the crystal structure in a hydrate. Anhydrous compound An ionic compound without water.

36 Hydrates Formulas of Hydrated Compounds
Formula of ionic compound, followed by the number of water molecules, separated by a dot. Example: Copper (II) sulfate pentahydrate CuSO4 • 5 H2O There are five water molecules for every formula unit of copper (II) sulfate.

37 Hydrates Names of Hydrated Compounds
Use the prefixes for naming binary molecular compounds to indicate the number of water molecules associated with each formula unit of the anhydrous compound. Example: MgSO4 • 7 H2O Magnesium sulfate heptahydrate

38 Hydrates Example: What is the formula of iron(III) sulfate nonahydrate? Solution: Iron(III) ion is Fe3+. Sulfuric acid is H2SO4, so sulfate ion is SO42–. Nona- is the prefix for 9. -hydrate refers to water of hydration, H2O. 2 × 3+ balances 3 × 2–. Fe2(SO4)3 • 9 H2O

39 Homework Homework for chapter 6:
3, 5, 9, 13,15, 19, 21, 23, 25, 33, 35, 39, 41,43, 45, 47, 49 Fill the tables 6-13, 6-14, 6-15 and 6-16


Download ppt "Chapter 6 Chemical Nomenclature"

Similar presentations


Ads by Google