Gifted Chemistry – Week 13 Monday Chrome Book Activity Tuesday Student 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 pm Week 13: 8-1 and 8-2 & Week 13: Mixed Review

Most Missed Quia – Week 12 Write the formula for the ionic compound created from aluminum and carbonate Al2(CO3)3

Most Missed Quia – Week 12 Ca(ClO3)2  Write the formula for the ionic compound created from calcium and chlorate  Ca(ClO3)2

Most Missed Quia – Week 12 beryllium chlorite Name this compound: Be(ClO2)2  Beryllium Dichlorite Beryllium(II) Chloride beryllium(II) chlorite beryllium chlorite

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

Ionic Bonds Ca(OH)2 LiIO3 Formula Writing Balance charges Use parentheses, when necessary Calcium hydroxide Lithium iodate Ca(OH)2 LiIO3

Ionic Bonds (NH4)2SO4 K2CO3 Formula Writing Balance charges Use parentheses, when necessary Ammonium sulfate potassium carbonate (NH4)2SO4 K2CO3

Ionic Bonds – Which one is correct? (Ca) OH2 (NH4)3PO4 (Fe+2)2(PO3)3 Ca (OH)2 NH12PO4 (Fe+2)3(PO3)2

Ionic Bonds iron (III) nitrite tin (IV) carbonate Compound Naming Cations first; anions second Use roman numerals for transition metals Fe(NO2)3 Sn(CO3)2 iron (III) nitrite tin (IV) carbonate

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

Properties of Ionic Compounds Conductivity Ionic solids do not conduct electricity. Melted ionic solids or ionic solids dissolved in a solution will conduct electricity (electrolytes).

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.

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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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.

Naming Covalently Bonded Molecules 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 Rule 4. Greek prefixes are used to indicate the number of atoms of each nonmetal element in the chemical formula for the compound. Prefix Meaning Mono- 1 Hexa- 6 di- 2 Hepta- 7 tri- 3 Octa- 8 Tetra- 4 Nona- 9 Penta- 5 Deca- 10

Naming Covalently Bonded Molecules Practice: SbCl3 S2Cl2 BF3 P4O6 Se4S10 phosphorus trichloride selenium tetrafluoride carbon tetrabromide sulfur trioxide tetraphosphorus hexaoxide

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

Covalent Bond Nomenclature Lab Use your device to download a free dice rolling app Undeca Dodeca

Lewis Dot Structure CH4

Lewis Dot Structure NH3

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

Diatomic Molecules Two atoms of the same element share electrons in order to form a stable molecule Seven naturally occurring diatomic molecules H2 O2 F2 Br2 I2 N2 Cl2 “Hof Brincl”

Diatomic Molecules

More stable than single H atoms due to full shell Diatomic Molecules More stable than single H atoms due to full shell

Diatomic Molecules When only one pair of electrons is shared, it is a single covalent bond.

Single Bonds Draw the Lewis Dot Structure for Water H2O

Single Bonds Draw the Lewis Dot Structure for Ammonia NH3

Single Bonds Draw the Lewis Dot Structure for Methane CH4

Single Bonds Draw the Lewis Dot Structure for Methane CH4

Double Bonds

Double Bonds Draw the Lewis Dot Structure for carbon dioxide CO2

Triple Bonds

Triple Bonds Draw the Lewis Dot Structure for acetylene C2H2

Quiz Review: Dot and Mixed Nomenclature

Quiz Review: Dot and Mixed Nomenclature

Quiz Review: Dot and Mixed Nomenclature Kahoot.it You must enter your real name Scores will be part of your classwork grade for today. Quiz Review: Dot and Mixed Nomenclature