1. 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

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

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

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

5. 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

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

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

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

9. 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

10. 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

11. 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).

12. 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.

13. 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.

14. 1

17. 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.

18. 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.

19. 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

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

21. 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

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

23. Lewis Dot Structure
CH4

24. Lewis Dot Structure
NH3

28. 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

29. 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”

30. Diatomic Molecules

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

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

33. Single Bonds
Draw the Lewis Dot Structure for Water
H2O

34. Single Bonds
Draw the Lewis Dot Structure for Ammonia
NH3

35. Single Bonds
Draw the Lewis Dot Structure for Methane
CH4

36. Single Bonds
Draw the Lewis Dot Structure for Methane
CH4

37. Double Bonds

38. Double Bonds
Draw the Lewis Dot Structure for
carbon dioxide CO2

39. Triple Bonds

40. Triple Bonds
Draw the Lewis Dot Structure for
acetylene C2H2

41. Quiz Review: Dot and Mixed Nomenclature

42. Quiz Review: Dot and Mixed Nomenclature

43. Quiz Review: Dot and Mixed Nomenclature
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Quiz Review: Dot and Mixed Nomenclature