Download - Unit 7.2 Ionic Bonding
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Warm Up:
1. How many moles are contained in 6.0 g of carbon?
2. When two chemicals are mixed together in a beaker that is sitting in an ice water bath, the ice in the water melts as the chemicals react. Is the reaction exothermic or endothermic? Explain your reasoning.
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Ions and Ionic Bonding• One way for atoms to reach stability is by either losing or gaining electrons.
• When this occurs an ion is formed.
• Ion – an atom that has a charge.
• Occurs when the number of protons is unequal to the number of electrons.
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Cations• Whenever atoms lose electrons they form
cations.
• Cations are positively charged atoms.
• Metals tend to form cations.
• Example:
– Sodium
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Anions• Whenever atoms gain electrons they form
anions.
• Anions are negatively charged atoms.
• Nonmetals tend to form anions.
• Example:– Chlorine (Cl)
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We can use the periodic table to predict
the type of ion an atom will form.
Group Number Type of Ion Formed
1 +1
2 +2
13 +3
15 -3
16 -2
17 -1
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What Do You Think?
1. What charge would Lithium make?
2. What charge would sulfur make?
3. Neon?
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Ionic Bonding• Ionic bonding involves the transfer of
electrons from one atom to another.
• We can use electron dots to show how ionic bonds are formed.
• Example: – Na and Cl
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• Opposite charges serve as the glue that holds
the atoms together in the bond.
• Ionic bonds are extremely strong chemical bonds.
• Ionic bonds usually involve a combination of a metal with a nonmetal.
– By definition, an ionic bond is made when the electronegativity difference between atoms is greater than 1.7
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Illustrating Ionic Bonding in Compounds• Use electron dots to demonstrate how
calcium (Ca) and bromine (Br) form a stable compound by ionic bonding. Give the chemical formula for the compound formed.
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Polyatomic Ions can act as anions!
•Group of covalently bonded atoms that has a charge. (a charged molecule)
•Example: SO4-2 (sulfate ion)
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Writing Formulas and Naming Chemical Compounds
• There are two types of chemical compounds:
– ionic compounds– covalent (molecular) compounds
• Ionic Compounds are composed of a cation and an anion.
– cations – positively charged ion (metals)
– anions – negatively charged ion (nonmetals)
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Monoatomic Ions• Cations
– For monatomic cations, the name of the ion is the name of the element.
– examples:
Na+ = sodium ion
Mg2+ = magnesium ion
Al3+ = aluminum ion
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– Some metals are able to form more than one stable ion (polyvalent)
• usually transition elements• example: copper • forms Cu2+ and Cu+
• use Roman numerals to distinguish charge
• copper (II) and copper (I)
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• Anions– Monoatomic anions are named by dropping the
ending of the element and replacing with the suffix “-ide”.
– examples:
Cl- = chloride ion
O2- = oxide ion
N3- = nitride ion
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Naming Binary Ionic Compounds
• The nomenclature, or naming system, or binary ionic compounds involves combining the names of the compound’s positive and negative ions.
• The name of the cation is given first, followed by the name of the anion:– example: Al2O3 — aluminum oxide
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Independent practice
1. What is the formula and name for Sodium and Oxygen?
2. What would the formula and name be for potassium and sulfur?
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The Stock System of Nomenclature
Write the formula and give the name for the compound formed by the ions Cr3+ and F–.
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Independent Practice
1. Give the formula for Chromium (II) Fluoride.
2. What is the name of Fe2O3?
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Compounds Containing Polyatomic Ions
• Many common polyatomic ions are negatively charged and oxyanions— polyatomic ions that contain oxygen.
• Some elements can combine with oxygen to form more than one type of oxyanion.– example: nitrogen can form or .−
3NO
nitrate nitrite
• The name of the ion with the greater number of oxygen atoms ends in -ate. The name of the ion with the smaller number of oxygen atoms ends in -ite.
2NO−
3NO−2NO−
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• Some elements can form more than two types of oxyanions.– example: chlorine can form , ,
or .
• In this case, an anion that has one fewer oxygen atom than the -ite anion has is given the prefix hypo-.
• An anion that has one more oxygen atom than the -ate anion has is given the prefix per-.
hypochlorite chlorite chlorate perchlorate
ClO−2ClO−
3ClO−4ClO−
ClO−2ClO−
3ClO−
4ClO−
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Give the formula for…
1. Potassium Chlorate
2. Hydrogen Sulfite
3. Tin(IV) sulfate.
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Closure
• What is one thing you learned today?
• What is one thing we need more practice on?