Summer Review for Students Entering AP Chemistry 2017

Throughout the school year, we will be reviewing and deepening our understanding of the Big Ideas of Chemistry. We will challenge each other to think critically, apply hands-on lab knowledge, and analyze experimental and theoretical data. While this will be a rigorous course, we will also have some fun gaining a greater appreciation for the chemistry of the world around us.

Attached are selected review topics for summer. These are concepts covered in honors/on level chemistry that will be needed at the beginning of AP chemistry. First and foremost, practice naming and formula writing, including memorizing the selected polyatomic ions listed in the review materials. These are necessary throughout the year! To get a head start, there are also optional topics with practice problems and video tutorials which we will cover at the beginning of the year (atomic structure, balancing equations and mole conversions).

Have a safe, fun, and refreshing summer! We’re looking forward to an amazing year in AP chemistry!

Name: ______

AP Chemistry Need to Know

Naming/Formula Writing:

  1. Valence Electrons

Using the Periodic Table:

  • The number of valence electrons an element has is determined by its location on the periodic table
  • The numbers listed in bold up top are the number of valence electrons for each group.
  • The only exception to the rule is helium. It only has 2 valence electrons while the rest of the group has 8.
  • Valence electrons do not apply to the D-Block elements!

Practice: How many valence electrons do these elements have?

  1. Mg: ______
  2. P:

  1. Ar:
  2. Al:

  1. I:
  2. H:

  1. Determining Charges
  2. Elements lose or gain electrons and become cations/anions in order to have noble gas/full shell configurations (more stable)
  3. Charges are easy to determine for the s and p block elements
  4. The following almost ALWAYS take the following charges when they exist as IONS:
  5. Group 1 (lithium, etc) = +1
  6. Group 2 (beryllium, etc) = +2
  7. Group 3 (aluminum, etc) = +3
  8. Group 4 (carbon, etc) = +/- 4 (usually doesn’t take charge)
  9. Group 5 (nitrogen, etc) = -3
  10. Group 6 (oxygen, etc) = -2
  11. Group 7 (fluorine, etc) = -1
  12. Group 8 (noble gases) = NO CHARGES!
  13. Transition metals and “other metals” (lead, tin…) are not predictable because they can take different charges (because of the D-Electrons)
  14. Ex: Fe2+, Fe3+
  15. Must be given their charge or determine it from the roman numeral in the name or based on its chemical formula
  16. Iron (II) chloride = Fe2+
  17. FeCl2 = Fe2+
  18. Don’t stress about memorizing these. You’ll get better at knowing common ones as the year goes on.
  1. Polyatomic Ions
  2. Ions made of more than one atom
  3. Try to memorize these this summer. Make sure you also memorize the charge. You will need to know these the entire year in chemistry.

Memorize:

Formula / Name
Ammonium / NH4+
Acetate / C2H3O2-
Bicarbonate / HCO3-
Carbonate / CO32-
Hyperchlorite / ClO1-
Chlorite / ClO2 1-
Chlorate / ClO3 1-
Perchlorate / ClO4 1-
Nitrite / NO2 1-
Nitrate / NO3 1-
Permanganate / MnO41-
Peroxide / O22- (not all O2 are peroxides)
Phosphate / PO43-
Sulfite / SO32-
Sulfate / SO42-
  1. Naming Ionic Compounds
  2. Ionic compounds are cation and anion (usually a metal and nonmetal or metal and polyatomic ion)
  3. Watch out for any compound with NH4+ because it ALWAYS acts as a METAL
  4. Held together by attractive (columbic) forces
  5. Writing Formulas for Ionic Compounds
  6. The cation and anion charges must cancel out for a sum total of zero.
  7. Remember to use parentheses around the polyatomic ions.
  8. Naming/Formula Writing Covalent Compounds
  9. Covalent compounds are nonmetals (or semimetals) that SHARE electrons forming a bond
  10. **The first element list only needs a prefix if it is more than 1. The second element ALWAYS needs a prefix (dihydrogen monoxide)
  11. Prefixes:

1 / mono-
(only use on 2nd element in compound)
2 / di-
3 / tri-
4 / tetra-
5 / penta-
6 / hexa-
  1. Video Tutorials for Naming and Formula Writing:

Note: There are several tutorials listed here that cover the same content, but have very different styles. Video tutorials are excellent ways to review for tests or to preview content throughout the year. Now is a great time to see which sites offer a style that fits YOU best!

  1. (Crash Course Chemistry #11: “How to Speak Chemistrian”)
  2. (Khan Academy: Ions)
  3. (Practice Quiz: Predicting Charge on Ions)
  4. (Khan Academy: Common polyatomic Ions)
  5. (Khan Academy: Naming Ionic Compounds)
  6. (Khan Academy: Compounds and Molecules Article)
  7. (Practice Quiz: Naming ionic compounds)
  8. (Practice Quiz: Writing Ionic Formulas)
  9. ionic naming -- weird formatting when you enter the names – see instructions on the top)
  10. (practice quizzes for covalent naming – scroll down the page)
  11. (Bozeman Science: Naming Part 1)
  12. (Bozeman Science: Naming Part 2)
  1. PRACTICE Naming/Formula Writing Ionic and Covalent Mixed

You should be able to do these in AP chemistry with ONLY a periodic table.

Don’t forget roman numerals as needed.

  1. Name:

CrO3______

Cu2O______

CO______

K3N______

Fe(CN)3______

N2O4______

Ca(OH)2______

PBr3______

P2O5______

NaNO3______

CCl4______

AlCl3______

Ni2S3______

B2H6______

  1. Write the formula:

Iodine pentafluoride______

Lithium phosphide______

aluminum hydroxide______

iron (II) chloride______

calcium fluoride______

nitrogen trifluoride______

magnesium phosphate______

sodium acetate______

AP Chemistry: Looking Ahead (Optional Topics)

These are topics we will be covering during class at the beginning of the year. I’ve outlined them for you just in case you want to get ahead. Please do not stress if you need help on these – we’ll have time to review.

Great Websites:

Khan Academy: Chemistry

Bozeman Science Chemistry

Crash Course Chemistry

Atomic Structure

  1. The Atom
  2. Protons have a mass in AMU of ONE and a charge of +1. Protons are found inside the nucleus.
  3. Electrons have a mass in AMU of ZERO and a charge of -1. Electrons are found in orbitals outside of the nucleus.
  4. Neutrons have a mass in AMU of ONE and a charge of 0. Neutrons are found inside the nucleus.
  5. Atomic Numbers

Website Resources:

PLAY: (don’t worry about nucleons!)

  1. Isotopes = same number of protons, different number of neutrons therefore different mass numbers (also different levels of nuclear stability)
  2. Ions (cations/anions) = same number of protons, lost or gained electrons
  3. Mass Number = THIS IS EQUAL TO THE NUMBER OF PROTONS + NEUTRONS in a given isotope. ALWAYS A WHOLE NUMBER!!!
  4. Average Atomic Mass = Average of all the isotopes mass and % abundance, what you find on the periodic table, will not usually be a whole number.
  5. Standard Notation: atomic numberE
  6. # of protons = atomic number
  7. # of electrons = atomic number – charge
  8. # of neutrons = mass number – protons

Standard Formatting / Mass / #
Protons / #
Electrons / #
Neutrons / Charge / Cation, anion or neutral
28 / 28 / 32
19 / 9 / 10
64Zn+1
108 / 47
51V
2 / 2 / 2
16 / 18 / 32
47 / 46 / 60
64Zn
127I1-
107Ag

Chemical Equations:

  1. Balancing Chemical Equations
    Website tutorial:

Practice:

More Practice:

  1. I have a feeling you are already excellent at this 
  2. I balance combustion reactions a special way: C first, H next and I leave the O for last! – saves a lot of time
  3. How are coefficients different than subscripts?

Mole Conversions

  1. Mole Calculations

Great Practice:

  1. 1 mole = molar mass (use the periodic table – each element/compound is different)
  2. 1 mole = 6.02 x 1023 atoms/molecules/formula units
  3. Atoms are for elements
  4. Molecules are for covalent compounds
  5. Formula units are for ionic compounds (to go from formula units to atoms multiply by the number of atoms in the compound!)
  6. 1 mole = 22.4 L of a GAS at STP (1atm and 25oC or 1atm and 0oC)
  7. Practice:
  8. How many formula units of CuCl2 are in 2.5g? How many atoms?
  9. How many moles of hydrogen gas are in 3L at STP?
  10. How many grams are in 4.2 x 10-5 moles of MgCO3?