Download - Lattice Energy
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Lattice Energy
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Properties affected by bond strength
• melting/boiling point (stronger bonds = higher melting/boiling point)
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Properties affected by bond strength
• melting/boiling point (stronger bonds = higher melting point/boiling point)
• hardness (stronger bonds = harder crystals)
![Page 4: Lattice Energy](https://reader036.vdocuments.site/reader036/viewer/2022081723/568159a4550346895dc6fe4f/html5/thumbnails/4.jpg)
Properties affected by bond strength
• melting/boiling point (stronger bonds = higher melting point/boiling point)
• hardness (stronger bonds = harder crystals)• odor (stronger bonds = weaker odor)
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Properties affected by bond strength
• melting/boiling point (stronger bonds = higher melting point/boiling point)
• hardness (stronger bonds = harder crystals)• odor (stronger bonds = weaker odor)• state at room temperature (stronger bonds
are more likely to be solids)
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Bond formation
• Whenever a new bond forms, energy is released. The stronger the bond, the more energy that is released.
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Bond formation
• Whenever a new bond forms, energy is released. The stronger the bond, the more energy that is released.
• For ionic bonds, this energy is called lattice energy.
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Bond formation
• Whenever a new bond forms, energy is released. The stronger the bond, the more energy that is released.
• For ionic bonds, this energy is called lattice energy.
• Higher lattice energy values correspond to stronger bonds.
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Bond formation• Whenever a new bond forms, energy is
released. The stronger the bond, the more energy that is released.
• For ionic bonds, this energy is called lattice energy.
• Higher lattice energy values correspond to stronger bonds.
• The amount of energy released when a bond forms is identical to the amount of energy required to break the bond.
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Predicting lattice energy
• Two factors will determine the lattice energy for ionic compounds.
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Predicting lattice energy
• Two factors will determine the lattice energy for ionic compounds.– Bigger charges produce higher lattice energies (2+
and 2- produce stronger bonds than 1+ and 1-)
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Predicting lattice energy
• Two factors will determine the lattice energy for ionic compounds.– Bigger charges produce higher lattice energies (2+
and 2- produce stronger bonds than 1+ and 1-)– Fewer energy levels result in greater lattice
energies (LiF will have a greater lattice energy than NaCl)
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Predicting lattice energy
• Two factors will determine the lattice energy for ionic compounds.– Bigger charges produce higher lattice energies (2+
and 2- produce stronger bonds than 1+ and 1-)– Fewer energy levels result in greater lattice
energies (LiF will have a greater lattice energy than NaCl)
– Charge is by far the bigger factor and should always be compared first!!!
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Which compound will have the greatest lattice energy, MgS or LiF?
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Which compound will have the greatest lattice energy, MgS or LiF?
• Magnitude of charge is the first thing we should look at.
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Which compound will have the greatest lattice energy, MgS or LiF?
• Magnitude of charge is the first thing we should look at.– magnesium (2+ charge), sulfide (2- charge)
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Which compound will have the greatest lattice energy, MgS or LiF?
• Magnitude of charge is the first thing we should look at.– magnesium (2+ charge), sulfide (2- charge) – lithium (1+ charge), fluoride (1- charge)
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Which compound will have the greatest lattice energy, MgS or LiF?
• Magnitude of charge is the first thing we should look at.– magnesium (2+ charge), sulfide (2- charge) – lithium (1+ charge), fluoride (1- charge)
– MgS has the greater individual charges, so MgS has the greater lattice energy.
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Which compound will have a lower melting point, Na2S or BeO?
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Which compound will have a lower melting point, Na2S or BeO?
• A lower melting point means we need to select the compound with the lower lattice energy. We check the charges first.
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Which compound will have a lower melting point, Na2S or BeO?
• A lower melting point means we need to select the compound with the lower lattice energy. We check the charges first.– sodium (1+), sulfide (2-)
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Which compound will have a lower melting point, Na2S or BeO?
• A lower melting point means we need to select the compound with the lower lattice energy. We check the charges first.– sodium (1+), sulfide (2-)– beryllium (2+), oxide (2-)
![Page 23: Lattice Energy](https://reader036.vdocuments.site/reader036/viewer/2022081723/568159a4550346895dc6fe4f/html5/thumbnails/23.jpg)
Which compound will have a lower melting point, Na2S or BeO?
• A lower melting point means we need to select the compound with the lower lattice energy. We check the charges first.– sodium (1+), sulfide (2-)– beryllium (2+), oxide (2-)
– sodium sulfide has smaller individual charges, so it has the lower melting point.
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Which compound has harder crystals, CaCl2 or MgCl2?
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Which compound has harder crystals, CaCl2 or MgCl2?
• Harder crystals require a higher lattice energy. First, check the charges.
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Which compound has harder crystals, CaCl2 or MgCl2?
• Harder crystals require a higher lattice energy. First, check the charges.– calcium (2+), chloride (1-)
![Page 27: Lattice Energy](https://reader036.vdocuments.site/reader036/viewer/2022081723/568159a4550346895dc6fe4f/html5/thumbnails/27.jpg)
Which compound has harder crystals, CaCl2 or MgCl2?
• Harder crystals require a higher lattice energy. First, check the charges.– calcium (2+), chloride (1-)– magnesium (2+), chloride (1-)
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Which compound has harder crystals, CaCl2 or MgCl2?
• Harder crystals require a higher lattice energy. First, check the charges.– calcium (2+), chloride (1-)– magnesium (2+), chloride (1-)– the charges are the same, so we need to see
which ions have fewer energy levels.
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Which compound has harder crystals, CaCl2 or MgCl2?
– the charges are the same, so we need to see which ions have fewer energy levels.
– calcium (4), chloride (3)
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Which compound has harder crystals, CaCl2 or MgCl2?
– the charges are the same, so we need to see which ions have fewer energy levels.
– calcium (4), chloride (3)– magnesium (3), chloride (3)
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Which compound has harder crystals, CaCl2 or MgCl2?
– the charges are the same, so we need to see which ions have fewer energy levels.
– calcium (4), chloride (3)– magnesium (3), chloride (3)– fewer energy levels give MgCl2 the higher lattice
energy and therefore, the harder crystals.
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Which compound has the lower boiling point, AgNO3 or K2SO4?
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Which compound has the lower boiling point, AgNO3 or K2SO4?
• Lower boiling point means a lower lattice energy.
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Which compound has the lower boiling point, AgNO3 or K2SO4?
• Lower boiling point means a lower lattice energy.– silver (1+), nitrate (1-)
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Which compound has the lower boiling point, AgNO3 or K2SO4?
• Lower boiling point means a lower lattice energy.– silver (1+), nitrate (1-)– potassium (1+), sulfate (2-)
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Which compound has the lower boiling point, AgNO3 or K2SO4?
• Lower boiling point means a lower lattice energy.– silver (1+), nitrate (1-)– potassium (1+), sulfate (2-)– Charges indicate a lower lattice energy for AgNO3.
Lower lattice energy means a lower boiling point.