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Gifted Chemistry – Week 13
Monday Chrome Book Activity
TuesdayStudent Presentations: Covalent Bonds; Notes & Guided Practice: Covalent Nomenclature
Wednesday
Lab: Naming Covalent Molecules
Thursday
Quiz: Ionic & Covalent Formulas & Nomenclature;Notes: Lewis Dot Structures for Covalent Molecules
Friday Begin Test Review (Test on Tuesday)Two Quia due on Sunday at 11:59 pmWeek 13: 8-1 and 8-2 & Week 13: Mixed Review
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Most Missed Quia – Week 12
Write the formula for the ionic compound created fromaluminum and carbonate
Al2(CO3)3
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Most Missed Quia – Week 12
Write the formula for the ionic compound created fromcalcium and chlorate
Ca(ClO3)2
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Most Missed Quia – Week 12
Name this compound: Be(ClO2)2
Beryllium DichloriteBeryllium(II) Chlorideberyllium(II) chlorite
beryllium chlorite
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Ionic Bonds
• Transferring electrons from one atom to another in order to complete an octet of valence electrons
• Groups 1 and 2 lose electrons…become positive cations
• Chalogens and Halogens gain electrons…become negative anions
• Metal + nonmetal salt• Metal + oxygen oxide
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Ionic Bonds
• Formula Writing– Balance charges– Use parentheses, when necessary
Calcium hydroxide Lithium iodate
Ca(OH)2 LiIO3
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Ionic Bonds
• Formula Writing– Balance charges– Use parentheses, when necessary
Ammonium sulfate potassium carbonate
(NH4)2SO4 K2CO3
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Ionic Bonds – Which one is correct?
(Ca) OH2
(NH4)3PO4
(Fe+2)2(PO3)3
Ca (OH)2
NH12PO4
(Fe+2)3(PO3)2
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Ionic Bonds
• Compound Naming– Cations first; anions second– Use roman numerals for transition
metals
Fe(NO2)3
Sn(CO3)2
iron (III) nitrite
tin (IV) carbonate
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Properties of Ionic Compounds
• Ionic bonds produce unique physical structures
• Atoms are highly organized with consistent spacing and a uniform pattern
• Crystal lattice – a 3D arrangement of particles
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Properties of Ionic Compounds
1. ConductivityIonic solids do not conduct electricity.Melted ionic solids or ionic solids dissolved in a solution will conduct electricity (electrolytes).
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Properties of Ionic Compounds
2. High melting points and high boiling points.Ionic bonds are very strong and require a lot of energy to break apart.
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Ionic Bonds and Energy
Formation of ionic bonds is always exothermic.
Lattice energy – energy required to separate the ions in an ionic compound
Smaller ions have greater lattice energies.Larger charges also have greater lattice energies.
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1
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Naming Covalently Bonded Molecules
A binary covalent compound is composed of two different nonmetal elements. There are four rules on naming these molecules.
Rule 1. The element with the lower group number
is written first in the name; the element with the higher group number is written second in the name.
Exception: when the compound contains oxygen and a halogen, the name of the halogen is the first word in the name.
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Rule 2. If both elements are in the same group, the element with the higher period number is written first in the name.
Rule 3. The second element in the name is named as if it were an anion, i.e., by adding the suffix -ide to the name of the element.
Naming Covalently Bonded Molecules
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Rule 4. Greek prefixes are used to indicate the number of atoms of each nonmetal element in the chemical formula for the compound.
Naming Covalently Bonded Molecules
Prefix Meaning Prefix Meaning
Mono- 1 Hexa- 6
di- 2 Hepta- 7
tri- 3 Octa- 8
Tetra- 4 Nona- 9
Penta- 5 Deca- 10
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Practice:
1) SbCl3
2) S2Cl2
3) BF3
4) P4O6
5) Se4S10
Naming Covalently Bonded Molecules
6) phosphorus trichloride7) selenium tetrafluoride8) carbon tetrabromide9) sulfur trioxide10) tetraphosphorus
hexaoxide
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Covalent Bond Review
Covalent bond – chemical bond that occurs when valence electrons are shared, not transferred
Molecule – product of a covalent bond
Usually occurs between nonmetals and elements that are close to each other on the periodic table
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Covalent Bond Nomenclature Lab
Use your device to download a free dice rolling app
11 Undeca12 Dodeca
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Lewis Dot Structure
CH4
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Lewis Dot Structure
NH3
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1) chlorine monoxide
2) oxygen difluoride
3) boron monophosphide
4) dinitrogen monoxide
5) nitrogen trifluoride
6) sulfur tetrachloride
7) xenon trioxide
8) carbon dioxide
9) diphosphorous pentoxide
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Diatomic Molecules
Two atoms of the same element share electrons in order to form a stable molecule
Seven naturally occurring diatomic moleculesH2 O2 F2 Br2 I2 N2 Cl2
“Hof Brincl”
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Diatomic Molecules
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Diatomic Molecules
More stable than single H atoms due to
full shell
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Diatomic Molecules
• When only one pair of electrons is shared, it is a single covalent bond.
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Single Bonds
• Draw the Lewis Dot Structure for WaterH2O
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Single Bonds
• Draw the Lewis Dot Structure for AmmoniaNH3
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Single Bonds
• Draw the Lewis Dot Structure for MethaneCH4
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Single Bonds
• Draw the Lewis Dot Structure for MethaneCH4
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Double Bonds
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Double Bonds
• Draw the Lewis Dot Structure for carbon dioxide CO2
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Triple Bonds
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Triple Bonds
• Draw the Lewis Dot Structure for acetylene C2H2
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