chapter 7 chemical compounds & chemical...
TRANSCRIPT
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CHAPTER 7CHEMICAL COMPOUNDS & CHEMICAL FORMULAS
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CHEMICAL NAMES & FORMULAS
• Most everyday chemical compounds are given common names.
• But, these names don’t tell us about the chemical composition of the chemicals.
• Nomenclature systems allow for us to use the most accurate name for chemicals.
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SIGNIFICANCE OF A FORMULA
• Recall: A chemical formula tells us what number of atoms and what kind of atoms are in a chemical compound.
• Examples
• Octane (C8H18) a molecular compound
• Aluminum sulfate, Al2(SO4)3 an ionic compound
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MONATOMIC IONS
• Recall: Cations have very low ionization energies [energies needed to lose an electron], while anions have very high electron affinities [energy needed to add an electron].
• The goal for elements is to reach a noble-gas configuration. Noble-gas configuration = STABILITY
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MONATOMIC CATIONS
• Members of Group 1 tend to lose 1 electron in order to get back to a noble-gas configuration. This results in a 1+ charge.
• Members of Group 2 lose 2 electrons in order to get back to a noble-gas configuration. This results in a 2+ charge.
• Members of Group 13 lose 3 electrons to get to a noble-gas configuration, resulting in a 3+ charge.
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MONATOMIC ANIONS
• Starting with Group 15, elements begin to gain electrons in order to reach noble-gas configuration.
• Group 15 = 3- charge [gain of 3 electrons]
• Group 16 = 2- charge [gain of 2 electrons]
• Group 17 = 1- charge [gain of an electron]
• There are some elements on the periodic table that can have multiple charges (positive), see the transition metals in the middle of the PT.
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NAMING MONATOMIC IONS
• When naming cations, the name of the cation is the same as the metal’s name.
• When naming anions, the name of the anion is changed by adding the suffix –ide.
• When an element can have multiple charges, we must use the Stock system. The Stock system uses Roman numerals in parenthesis to indicate the charge of the cation.
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THE NOTORIOUS B.I .C (BINARY IONIC COMPOUND)
• Binary ionic compounds are compounds composed of 2 different elements.
• As a general rule, the total + charge must equal the total – charge.
• When writing the formulas for BICs, follow the following steps.
• 1. Write ions side by side with cation first.
• 2. Criss-cross charge to make subscripts.
• 3. Check to see if subscripts are in lowest terms.
• Remember, + must = -!
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WRITING CHEMICAL FORMULAS PRACTICE
• Write the formula of the binary ionic compound that will result between the following elements:
• 1. zinc and sulfur
• 2. aluminum and phosphorus
• 3. strontium and chlorine
• 4. barium and oxygen
• 5. sodium and nitrogen
• 6. lithium and iodine
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NAMING BICS
• When naming BICs, we name the cation (metal) first, then the anion (nonmetal).
• Examples:
• 1. Sr3N2
• 2. AgCl
• 3. NaI
• 4. CaO
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NAMING BICS PRACTICE
• Name the following BICs indicated by the following formulas:
• 1. AgBr
• 2. ZnO
• 3. CaBr2
• 4. MgO
• 5. AlP
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NAMING BICS USING STOCK SYSTEM PRACTICE
• Name the following BICs according to the Stock system:
• 1. CuO
• 2. SnS
• 3. Fe2O3
• 4. FeO
• 5. PbCl2
• 6. VO
• 7. V3P4
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POLYATOMIC IONS
• Polyatomic ions are ions that are composed of more than one type of atom.
• Almost all polyatomic ions are negatively charged, except the ammonium ion [NH4+].
• A majority of polyatomic ions are called oxyanions. Oxyanions are polyatomic ions that contain oxygen.
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NOMENCLATURE OF POLYATOMIC IONS
• We can make several different polyatomic ions from the same two elements.
• Ex. N & O
• Nitrite = NO2-
• Nitrate = NO3-
• The suffix –ite goes with the anion with the lower number of oxygen atoms.
• The suffix –ate goes with the anion with the higher number of oxygen atoms.
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NOMENCLATURE OF POLYATOMIC IONS (CONTINUED)
• Sometimes, we may have to use prefixes when we have more than 2 possible anions.
• Ex. Chlorine & oxygen
• ClO4- = perchlorate
• ClO3- = chlorate
• ClO2- = chlorite
• ClO- = hypochlorite
• The prefix per- is used for the highest number of oxygen atoms; whereas, the prefix hypo- is used for the lowest number of oxygen atoms.
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WRITING FORMULAS USING POLYATOMIC IONS
• When writing formulas for compounds using polyatomic ions, we follow the same steps as BICs.
• 1. Write ions side by side—cation first!
• 2. Criss-cross charges to make subscripts.*
• 3. Check to see if subscripts are in lowest terms.
• *There is only a slight difference: If we criss-cross and the subscript for the polyatomic ion is greater than one, then we must put the polyatomic ion in parentheses.
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WRITING FORMULAS PRACTICE
• Write formulas for the following ionic compounds:
• 1. lithium nitrate
• 2. copper (II) sulfate
• 3. potassium perchlorate
• 4. ammonium chloride
• 5. lead (IV) phosphate
• 6. tin (IV) oxalate
• 7. ammonium carbonate
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NAMING COMPOUNDS USING POLYATOMICS
• When naming ionic compounds using polyatomic ions, the rules are the same.
• Cation goes first, followed by anion.
• We don’t have to change the ending of the polyatomic since the majority of them are anions.
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NAMING COMPOUNDS PRACTICE
• Give the names of the following ionic compounds:
• 1. NaCH3COO
• 2. SrCO3
• 3. Ba3(PO4)2
• 4. AgNO3
• 5. Cu(ClO4)2
• 6. Al2(SO4)3
• 7. KCN
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BINARY MOLECULAR COMPOUNDS (BMCS)
• Different from BICs—contain 2 nonmetal atoms
• Nomenclature system uses Greek numerical prefixes
• PREFIXES *Use mono- only for second word
1 mono-*
2 di-
3 tri-
4 tetra-
5 penta-
6 hexa-
7 hepta-
8 octa-
9 nona-
10 deca-
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NAMING BINARY MOLECULAR COMPOUNDS
General Formula for Naming BMCs
Prefix* (if more than 1) Element name Prefix Root name of
element -ide
Less electronegative element More electronegative element
Order for less electronegative element: C, P, N, H, S, I, Br, Cl, O, F
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NAMING BMCS• Name the following binary molecular compound
P4O10
Tetra - + phosphorusDeca-‐ + ox-‐ + -‐ide
Drop the a from the prefix
tetraphosphorus decoxide
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NAMING BMCS PRACTICE
• Give the names of the following binary molecular compounds:
• 1. SO3
• 2. CO2
• 3. N2O5
• 4. As2O5
• 5. PBr5
• 6. SF6
• 7. ICl3
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WRITING BMCS FORMULAS PRACTICE
• Write the formulas for the following compounds:
• 1. oxygen difluoride
• 2. carbon tetraiodide
• 3. phosphorus trichloride
• 4. dinitrogen monoxide
• 5. disilicon hexabromide
• 6. diphosphorus trioxide
• 7. disulfur dichloride