Coyle/Tang-Johnson Chemistry Study Guide Chapter 9 Study Guide TEST: Monday 1/10/11 9.1 Naming Ions Define the following terms: - monatomic ion - polyatomic ion 1. How can you figure out the charge of an ion using the periodic table? 2. How are the ions for transition metals different from the group A element ions? 3. What are the two ways you can name metal ions with more than one ionic charge? Give an example using Cu + and Cu 2+ . 4. Where can you find a list of common polyatomic ions? 1
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Coyle/Tang-Johnson Chemistry Study Guide
Chapter 9 Study GuideTEST: Monday 1/10/11
9.1 Naming Ions
Define the following terms:
- monatomic ion
- polyatomic ion
1. How can you figure out the charge of an ion using the periodic table?
2. How are the ions for transition metals different from the group A element ions?
3. What are the two ways you can name metal ions with more than one ionic charge? Give an example using Cu + and Cu 2+.
4. Where can you find a list of common polyatomic ions?
5. What do the names of most polyatomic ions end in?
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Coyle/Tang-Johnson Chemistry Study Guide
9.2 Naming and Writing Formulas for Ionic Compounds
1. To name a binary ionic compound, which ion must be named first?
2. How does the ending of the anion change from its element name when it is in a binary ionic compound? (ie. fluorine becomes:________________)
*** If you know the name of a binary ionic compound, you can use the criss-cross method to write its formula. Ex: Calcium bromide
Ca2+ and Br- (Use the periodic table to find the correct ions)
Ca2+ Br1- (Criss-cross the numerical value of the charge of each ion)
CaBr2 (Do not write the subscript 1, and do not write the charges)
*** Use the same method for metal ions with multiple charges Ex: Iron (III) oxide
Fe3+ and O2- (The roman numeral tells you which iron ion to use)
Fe3+ O2- (Criss-cross the numerical value of the charge of each ion)
Fe2O3
*** Use the same method for binary compounds with polyatomic ions.
Ex: Calcium nitrate (The –ate ending is a clue that it’s polyatomic)
Ca2+ and (NO3)1- (The negative 1 charge is for the entire polyatomic ion)
Ca2+ (NO3)1- (Criss-cross)
Ca(NO3)2 (Parentheses are needed around the entire nitrate ion because you need more than one of these polyatomic ions. )
*** Subscripts MUST be in the lowest whole number ratio possible ***
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9.3 Naming and Writing Formulas for Molecular Compounds
1. Memorize the following prefixes:
Prefix Mono- Di- Tri- Tetra- Penta- hexa Hepta- Octa- Nona- Deca-Number 1 2 3 4 5 6 7 8 9 10
*** To name binary molecular compounds,1. Check to see if the compound is made up of two nonmetals2. Name the elements in the order listed in the formula3. Use the correct prefix indicating the number of each atom 4. The second element’s suffix is –ide* Omit the prefix mono- if the formula contains only one atom of the first element.
Ex: N2O = dinitrogen monoxide CO = carbon monoxide
*** To write binary molecular compound formulas, use the prefixes in the name to tell you the subscript of each element in the formula.
Ex: dinitrogen tetroxide = N2O4 phosphorous pentachloride = PCl5
9.4 Naming and Writing Formulas for Acids and Bases
Define the following terms:
- acid (HnX)
- base
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*** An acid’s name depends on its anion (in HnX, X is the anion): See table 9.5 on p. 272 for a summary of rules
1. When the anion ends in –ide, the acid name begins with the prefix hydro-. The stem of the anion has the suffix –ic and is followed by the word acid.
Ex: HCl (X = chloride) hydrochloric acid H2S (X = sulfide) hydrosulfuric acid
2. When the anion ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by the word acid.
Ex: H2SO3 (X = sulfite) sulfurous acid
3. When the anion ends in –ate, the acid name is the stem of the anion with the suffix –ic, followed by the word acid.
Ex: HNO3 (X = nitrate) nitric acid
1. Name these acids:a) HNO2
b) HMnO4
c) HCNd) H2Se) HClO4
2. Write the formulas for these acids:a) carbonic acidb) sulfurous acid
*** Bases are names like ionic compounds: the name of the cation followed by the anion. Example: Al(OH)3 = Aluminum hydroxide
3. Name these bases:a) LiOHb) Pb(OH)2
c) Mg(OH)2
d) KOH
4. Write the formulas for these bases:a) iron (III) hydroxideb) strontium hydroxide
9.5 Laws Governing Formulas and Names
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Coyle/Tang-Johnson Chemistry Study Guide
Define the following terms:
- law of definite proportions
- law of multiple proportions
*** Calculating mass ratios ***1. Carbon reacts with oxygen to form two compounds. Compound A contains 2.41g of carbon for each 3.22g of oxygen. Compound B contains 6.71g of carbon for each 17.9g of oxygen. What is the lowest whole number mass ratio of carbon that combines with a given mass of oxygen? (See example 9.1 on p. 275)
2. Lead forms two compounds with oxygen. One contains 2.98g of lead and 0.461g of oxygen. The other contains 9.89g of lead and 0.763g of oxygen. For a given mass of oxygen, what is the lowest whole number mass ratio of lead in the two compounds?
Practice Naming Chemical Compounds:
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Coyle/Tang-Johnson Chemistry Study Guide
(from "Chemistry" Wilbraham, Staley, Matta & Waterman, 2005 Prentice Hall)
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Coyle/Tang-Johnson Chemistry Study Guide
From: http://www.miracosta.cc.ca.us/home/dlr/names2.htm
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Coyle/Tang-Johnson Chemistry Study Guide
Practice Writing Chemical Formulas:
(from "Chemistry" Wilbraham, Staley, Matta & Waterman, 2005 Prentice Hall)
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Coyle/Tang-Johnson Chemistry Study Guide
From: http://www.miracosta.cc.ca.us/home/dlr/names1.htm
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Coyle/Tang-Johnson Chemistry Study Guide
Mixed Practice:
From: http://www.miracosta.cc.ca.us/home/dlr/names3.htm
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