1 / 36

Chemistry SOL Review by Anne Mooring (Jamestown High School, Williamsburg VA, 2006)

Chemistry SOL Review by Anne Mooring (Jamestown High School, Williamsburg VA, 2006). Part 3: Nomenclature, Chemical Formulas and Reactions Types of Compounds (Ionic vs. Molecular) Naming Compounds and Writing Formulas Molecular and Empirical Formulas Reaction Types

tam
Télécharger la présentation

Chemistry SOL Review by Anne Mooring (Jamestown High School, Williamsburg VA, 2006)

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemistry SOL Reviewby Anne Mooring (Jamestown High School, Williamsburg VA, 2006) • Part 3: Nomenclature, Chemical Formulas and Reactions • Types of Compounds (Ionic vs. Molecular) • Naming Compounds and Writing Formulas • Molecular and Empirical Formulas • Reaction Types • Balancing Chemical Equations • Drawing Lewis Structures and Predicting Geometric Shapes • Reaction Rates and Kinetics • Use the SOL periodic table. http://www.pen.k12.va.us/VDOE/Assessment/Manipulatives/PTE.pdf This section represents 16/50 of the SOL questions

  2. Non-metals above the staircase Metals below the staircase

  3. Non-metals above the staircase Metals below the staircase The yellow shaded metals can take on multiple charges/oxidation states (except Zn, Ag, and Cd).

  4. Chemistry SOL Review—Nomenclature, Formulas and Reactions Types of Compounds (Ionic vs. Molecular) Ionic compounds form from metals and non-metals (across the tracks) and transfer electrons between elements. You figure out the formula for an ionic compound by criss-crossing charges to subscripts and reducing subscripts if possible. Ca2+ and F1- form ___________ Li1+ and PO43- form____________ Pb4+ and S2- form ________ Mn2+ and ClO3-1 form _________

  5. Chemistry SOL Review—Nomenclature, Formulas and Reactions Types of Compounds (Ionic vs. Molecular) Ionic compounds form from metals and non-metals (across the tracks) and transfer electrons between elements. You figure out the formula for an ionic compound by criss-crossing charges to subscripts and reducing subscripts if possible. Ca2+ and F1- form CaF2 Li1+ and PO43- form Li3PO4 Pb4+ and S2- form Pb2S4 which reduces to PbS2 Mn2+ and ClO3-1 form Mn(ClO3)2

  6. Chemistry SOL Review—Nomenclature, Formulas and Reactions Naming Ionic Compounds • Write the name of the cation. • If the anion is an element, change its ending to -ide; if the anion is a polyatomic ion, simply write the name of the polyatomic ion. • If the cation can have more than one possible charge, write the charge as a Roman numeral in parentheses. Name the following compounds CaF2 _________________________ Li3PO4 __________________________ PbS2 _____________________________ Mn(ClO3)2 ______________________________

  7. Chemistry SOL Review—Nomenclature, Formulas and Reactions Naming Ionic Compounds • Write the name of the cation. • If the anion is an element, change its ending to -ide; if the anion is a polyatomic ion, simply write the name of the polyatomic ion. • If the cation can have more than one possible charge, write the charge as a Roman numeral in parentheses. Name the following compounds CaF2 Calcium fluoride Li3PO4Lithium phosphate PbS2 Lead (IV) sufide Mn(ClO3)2 Manganese (II) chlorate

  8. Chemistry SOL Review—Nomenclature, Formulas and Reactions Molecular Compounds • Molecular compounds are composed of two non-metals (above the staircase) • Indicate # of each atom using prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca) • The first element does not use mono if there’s only one. • Examples: • OF2 is named oxygen diflouride • N2O is named dinitrogen monoxide • You try: • NO2 ___________________________ • P2O4 ____________________________

  9. Chemistry SOL Review—Nomenclature, Formulas and Reactions Molecular Compounds • Molecular compounds are composed of two non-metals (above the staircase) • Indicate # of each atom using prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca) • The first element does not use mono if there’s only one. • Examples: • OF2 is named oxygen diflouride • N2O is named dinitrogen monoxide • You try: • NO2nitrogen dioxide • P2O4diphosphorus tetroxide

  10. Molecular and Empirical Formulas Molecular Formulas provide the true number of atoms in a compound Empirical formulas give the ratio of the elements found in a compound Structural formulas show how the atoms are connected.

  11. Chemistry SOL Review—Nomenclature, Formulas and Reactions Types of Reactions • AX + B → BX + Y single replacement • AX + BY → AY + BX double replacement • AB → A + B decomposition • A + B → AB combination or synthesis • CxHy + O2 → CO2 + H2O combustion You identify each type H2SO4 + PbCl2 → HCl + PbSO4 Li + Cu(OH)2→ LiOH + Cu CH4 + O2→ CO2 + H2O NH3→ N2 + H2 H2O + O2→ H2O2

  12. Chemistry SOL Review—Nomenclature, Formulas and Reactions Types of Reactions • AX + B → BX + Y single replacement • AX + BY → AY + BX double replacement • AB → A + B decomposition • A + B → AB combination or synthesis • CxHy + O2 → CO2 + H2O combustion You identify each type H2SO4 + PbCl2 → HCl + PbSO4Double Replacement Li + Cu(OH)2→ LiOH + Cu Single Replacement CH4 + O2→ CO2 + H2O Combustion NH3→ N2 + H2 Decomposition H2O + O2→ H2O2Synthesis or combination

  13. Chemistry SOL Review—Nomenclature, Formulas and Reactions Balancing Equations Chemical Reactions should have the same number of atoms on each side to follow the Law of Conservation of Mass. Use coefficients (numbers in front) to balance the equations. ___Al + ___FeCl2 → ___AlCl3 +___Fe Count the number of atoms on each side and track the changes as you make them.

  14. Chemistry SOL Review—Nomenclature, Formulas and Reactions Balancing Equations Chemical Reactions should have the same number of atoms on each side to follow the Law of Conservation of Mass. Use coefficients (numbers in front) to balance the equations. ___Al + 3FeCl2 → ___AlCl3 +___Fe Count the number of atoms on each side and track the changes as you make them.

  15. Balancing Equations Chemical Reactions should have the same number of atoms on each side to follow the Law of Conservation of Mass. Use coefficients (numbers in front) to balance the equations. ___Al + 3FeCl2 → 2AlCl3 +___Fe Count the number of atoms on each side and track the changes as you make them.

  16. Balancing Equations Chemical Reactions should have the same number of atoms on each side to follow the Law of Conservation of Mass. Use coefficients (numbers in front) to balance the equations. 2Al + 3FeCl2 → 2AlCl3 +___Fe Count the number of atoms on each side and track the changes as you make them.

  17. Balancing Equations Chemical Reactions should have the same number of atoms on each side to follow the Law of Conservation of Mass. Use coefficients (numbers in front) to balance the equations. 2Al + 3FeCl2 → 2AlCl3 +3Fe Count the number of atoms on each side and track the changes as you make them.

  18. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound SO3 = 6 + 3(6)= 24 valence e-

  19. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds SO3 = 6 + 3(6)= 24 valence e-

  20. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule . SO3 = 6 + 3(6)= 24 valence e-

  21. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule Step 4: Place any remaining electrons on the central atom. SO3 = 6 + 3(6)= 24 valence e-

  22. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule Step 4: Place any remaining electrons on the central atom. Step 5: If the central atom does not have an octet, share pairs of electrons as bonds from outside atoms. SO3 = 6 + 3(6)= 24 valence e-

  23. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound PO33- = 5 + 3(6) + 3 = 26 valence e-

  24. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds PO33- = 5 + 3(6) + 3 = 26 valence e-

  25. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule PO33- = 5 + 3(6) + 3 = 26 valence e-

  26. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule Step 4: Place any remaining electrons on the central atom. PO33- = 5 + 3(6) + 3 = 26 valence e-

  27. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule Step 4: Place any remaining electrons on the central atom. Step 5: If the central atom does not have an octet, share pairs of electrons as bonds from outside atoms. PO33- = 5 + 3(6) + 3 = 26 valence e- Step 5 unnecessary

  28. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound CO2 = 4 + 2(6) + 16 valence e-

  29. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds CO2 = 4 + 2(6) + 16 valence e-

  30. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule CO2 = 4 + 2(6) + 16 valence e-

  31. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule Step 4: Place any remaining electrons on the central atom. CO2 = 4 + 2(6) + 16 valence e-

  32. Drawing Lewis Structures and Predicting Geometric Shapes Step 1: Count the number of valence electrons in the compound Step 2: Connect the atoms around the central atom by single bonds Step 3: Place remaining electrons on the outside atoms to fulfill octet rule Step 4: Place any remaining electrons on the central atom. Step 5: If the central atom does not have an octet, share pairs of electrons as bonds from outside atoms. CO2 = 4 + 2(6) + 16 valence e-

  33. Drawing Lewis Structures and Predicting Geometric Shapes VSEPR THEORY Valence Shell Electron Pair Repulsion Molecules adopt the shape that minimizes electron pair repulsions. The electron pairs/groups around the central atom get as far apart as possible. CO2 SO3 CH4

  34. Drawing Lewis Structures and Predicting Geometric Shapes Geometries for Four Electron Pairs Around a Central Atom

  35. Reaction Rates and Kinetics • Ways to speed up reactions: • Decrease particle size (grind the sample) • Increase heat • Add catalyst • Increase concentration of reagents

  36. References http://www.markrosengarten.com/ for New York Regent’s exam powerpoint.

More Related