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Chapter 7
Ionic Compounds and Metals
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ION FORMATIONSection 7.1
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Chemical Bonds
A chemical bond is the force that holds two atoms together.
• Can form by the attraction between the positive nucleus of one atom and the negative electrons of another
• Can form between positive and negative ions
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Valence Electrons
• Electrons in the outermost principal energy level
• Shown in the electron dot structures
• Octet rule – atoms will gain, lose or share electrons to obtain 8 valence electrons
• The valence electrons determine the bonding properties of the atom
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Positive Ion Formation
• A positively charged ion is called a cation.
• Positive ions are formed when an atom loses one or more valence electrons
• Metals make positive ions
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Negative Ion Formation
• A negatively charged ion is called an anion.
• Negative ions are formed when an atom gains one or more electrons in its valence shell.
• Nonmetals make negative ions.
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IONIC BONDS AND IONIC COMPOUNDS
Section 7.2
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Formation of an Ionic Bond
• An ionic bond is the electrostatic force that holds oppositely charged particles together in an ionic compound
• Compounds that contain ionic bonds are called ionic compounds.
• Ionic compounds are formed between metals (+ charge) and nonmetals (- charge).
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Binary Ionic Compounds
• Contain a metallic cation and a nonmetallic anion.
• Formation of Binary Ionic Compounds– Electron(s) is/are transferred from metal to
nonmetal – Metal becomes positive, nonmetal becomes
negative– Opposite charges attract
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Properties of Ionic Compounds
• Take the structure of a crystal lattice – Many units of positive and negative ions stick together
in a three-dimensional geometric arrangement
• Can conduct electricity when dissolved in water (they are electrolytes and break into ions when dissolved in water), but not in solid form
• Melting point, boiling point and hardness depend upon how strongly the ions are attracted to each other
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NAMES AND FORMULAS FOR IONIC COMPOUNDS
Section 7.3
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Formulas for Ionic Compounds
• Monatomic ions are one-atom ions– Examples: Mg2+ , Br-
• Oxidation numbers are the charges on ions– Note: some elements have multiple oxidation
states – you will have a periodic table to tell this
• Binary ionic compounds are made of two monatomic ions (one positive, one negative)
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Formulas for Binary Ionic Compounds
• Symbol for cation is written first, anion second
• Subscripts tell the number of atoms of each element
• What are the following compounds made of?– CaF2 1 calcium, 2 fluorine
– Na2S 2 sodium, 1 sulfur
– NaCl 1 sodium, 1 chlorine
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Naming Binary Ionic Compounds
• Name the cation first• Name the anion second with –ide at the end
• Examples– CaF2 calcium fluoride
– Na2S sodium sulfide
– NaCl sodium chloride
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Try Naming a few moreBinary Ionic Compounds
• K2O potassium oxide
• Al2S3 aluminum sulfide
• Na3N sodium nitride
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What if the cation has more than one oxidation state?
• You tell which ion was used by putting a Roman Numeral after the name of the cation
• Example:– CuS• We know S was -2 (that’s the only one it makes)• If there is only one atom of each element, the Cu must
have been +2• So, the name is written as Copper (II) sulfide [the “II”
indicates the charge]• Make sure, especially with transition elements, that you are
checking the oxidation states
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Writing Formulas for Binary Ionic Compounds
• Look up the charges for each element• For a compound to form, the total charge
must balance out to zero (positive charges must equal negative charges)
• Example:– Sodium bromide• Na is +1, Br is -1• Only need one of each to balance• Formula is NaBr
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Try writing some more formulasBinary Ionic Compounds
• Potassium Iodide KI
• Aluminum bromide AlBr3
• Magnesium chloride MgCl2
• Cesium nitride Cs3N
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Formulas for Polyatomic Ionic Compounds
• Polyatomic ions are ions that are made up of more than one atom
• You will have a chart for these and do not have to memorize them.
• Examples:– SO4
2- = sulfate
– CN- = cyanide– NH4
+ = ammonium
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Naming Polyatomic Ionic Compounds
• Name the cation first, anion second• Name the polyatomic as is – don’t change its
name at all
• Examples:– Ca3(PO4)2 calcium phosphate
– Mg(CN)2 magnesium cyanide
– NH4Cl ammonium chloride
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Now you try naming Polyatomic Ionic Compounds
• NaNO3 sodium nitrate
• Ca(ClO3)2 calcium chlorate
• Al2(CO3)3 aluminum carbonate
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Writing formulas for Polyatomic Ionic Compounds
• Same as binary ionic compounds EXCEPT you may not change anything in the polyatomic ion formula
• Put them in a “bubble” and put subscripts outside that bubble
• Example:– Calcium Nitrate
• Ions are Ca2+ and NO3-
• Formula will be Ca(NO3)2
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Now you try writing formulas forPolyatomic Ionic Compounds
• Sodium hydroxide NaOH
• Copper (II) nitrate Cu(NO3)2
• Silver chromate Ag2CrO4
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METALLIC BONDS AND THEPROPERTIES OF METALS
Section 7.4
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Metallic Bonds
• The electron sea model proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a “sea” of electrons
• Since the electrons are free to move, they are called delocalized electrons
• A metallic bond is the attraction of a metallic cation for delocalized electrons
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Properties of Metals(revisited)
• Moderately high melting points• High boiling points• Malleable, ductile, durable• Conduct heat and electricity well• Transition metals are harder/stronger than
alkali metals because the transition metals have more delocalized electrons