AP Chemistry · Handsworth 2026–27
Before Day 1: Prerequisites
Dr. Ras Mulinta
Handsworth Secondary
A Chem 11 self-check
AP Chemistry is a full year of first-year university chemistry, it starts where Chemistry 11 left off and assumes those ideas are solid on Day 1. Work through this self-check over the summer. If a section feels shaky, that's exactly where an afternoon with your Chem 11 notes pays off. Everything here is straight from the BC Chemistry 11 curriculum.
Name:Block:Date:
A · The mole & conversions BC: the mole · dimensional analysis
Convert in any direction: mass ↔ moles ↔ particles (n = m/M, N = n·N_A, N_A = 6.022×10²³), molarity (c = n/V), and gas amounts. For gases, the general tool is PV = nRT; at STP (0 °C, 100 kPa) one mole of gas is 22.7 L.
Check yourself
How many molecules are in 36.0 g of water?
M(H₂O) = 18.02 g/mol → n = 36.0/18.02 = 2.00 mol → N = 2.00 × 6.022×10²³
= 1.20 × 10²⁴ molecules
B · Reaction stoichiometry BC: reactions · stoichiometric calculations
Use mole ratios from a balanced equation to find amounts of reactant or product, and identify the limiting reactant when reactions go to completion. Keep your significant figures.
Check yourself
For 2 H₂ + O₂ → 2 H₂O, how many moles of water form from 5.0 mol H₂ (excess O₂)?
5.0 mol H₂ × (2 mol H₂O / 2 mol H₂) = 5.0 mol H₂O
C · Atomic structure & isotopes BC: quantum model · the mole
Know protons, neutrons, electrons (how to count each in a neutral atom or ion) what an isotope is, and how to find the average atomic mass from percent abundances.
Check yourself
An element is 65% mass-134, 25% mass-135, 7% mass-136, 3% mass-137. Average atomic mass?
(0.65)(134) + (0.25)(135) + (0.07)(136) + (0.03)(137) = 87.1 + 33.75 + 9.52 + 4.11
= 134.5 amu
D · Electron configuration BC: quantum mechanical model · electron configuration
Write full and core ([noble-gas]) configurations for any element. Understand s, p, d, f subshells and the filling order: 1s 2s 2p 3s 3p 4s 3d 4p … (s holds 2, p 6, d 10).
Check yourself
Ground-state configuration of iron (Z = 26)?
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶ = [Ar] 4s² 3d⁶
E · The periodic table & trends BC: valence electrons · electronegativity
Know the typical charges of common ions, alkali (+1), alkaline-earth (+2), Al³⁺, Zn²⁺, Ag⁺, and the monatomic anions, and that transition metals can have more than one charge. Know the trends across & down the table for atomic radius, electronegativity, and ionization energy.
Check yourself
Order Na, Mg, Cl by increasing ionization energy.
Na < Mg < Cl (ionization energy rises left → right across a period)
F · Bonding & lab math BC: bonding by electronegativity · sig figs
Tell ionic from covalent using electronegativity, draw simple Lewis structures, and judge polarity. In the lab, be fluent with significant figures, scientific notation, and uncertainty.
Check yourself
Is the bond in HCl ionic or covalent, and is the molecule polar?
Polar covalent (ΔEN ≈ 0.9), the molecule is polar, with Cl the negative end.
If you want to go further
Re-memorize your common ions / polyatomic ions and the solubility rules, we use them constantly. For reading ahead, OpenStax Chemistry 2e (free) chapters 1–3 line up with our Unit 1.