Chemistry Midterm Review Sheet

  1. Your exam is scheduled for:
  2. Your exam should take the two-hour period. Please, bring reading material in case you finish early. You will not be allowed to leave the room.
  3. Your exam is divided into 2 parts. The first part will be multiple choice. The second part will contain the following:
  4. Naming lab equipment
  5. Setting up and interpreting a graph
  6. Find the gram-atomic mass *NOTE: see moles
  7. Orbital notation of atoms
  8. Moles: find # of moles, # grams in x amount of moles, # of molecules or atoms *NOTE: see Avogadro’s #
  9. Using the formulas to determine calories, wavelength, frequency, energy of electromagnetic radiation: ΔH = cmΔT, c = * f & E = h* f *NOTE: know the value of c (speed of electromagnetic radiation aka light)

IV.Below the major concepts in each chapter we covered is outlined. Use the list as a study guide. Keep in mind that additional things may have been added and removed from each chapter, so use your notes as your primary source of reference.

V.I am available period 1A, 4, 5, & 8A-C. Additionally, I am here every morning by 7:00 (except A days) and stay until 3:15. So, if you have questions or want a study session, all you have to do is ask! I want to help. I thrive on it.

VI.There will be 3 periods designated for review. You will be given two review packets and we will possibly play a review game if there is time. BE SURE TO USE THIS REVIEW SHEET PRIOR TO THE ALOTTED REVIEW TIME, SO THAT YOU CAN ASK ANY BURNING QUESTIONS THAT ARISE OR CLEAR UP ANY UNCERTAINITIES.

VII.You will be allowed one note card. I will provide it. You will NOT be allowed to put on any additional information.


Chapter 1

  • Significant figures: How many?, multiplying, dividing, adding, & subtracting, rounding
  • Density: calculate (D = m/v), units (g/cm3 or g/ml)
  • Metric system: basic metric units, metric conversions
  • Scientific notation
  • Water: boil and freezing point (C & K), temp. at which water is most dense
  • Percent error

Chapter 2

  • Mixtures, compounds, elements: define, distinguish between, examples
  • Heterogeneous vs. homogenous: define, distinguish between, examples
  • Chemical & physical changes: examples, evidence
  • Catalyst: define & how would it look on a graph (hint: activation energy)
  • Energy: 3 types, categorize a type of energy into 1 of 3 types
  • Calorie problems: cal = c*m*T, c = 1 cal/gC
  • Convert calories  Joules
  • Convert C K
  • Define temperature in terms of kinetic energy
  • Temperature vs. heat
  • Endothermic vs. exothermic
  • Locate metals, nonmetals, & metalloids on periodic table
  • Decipher the state of matter (solid, liquid, gas) of an element at room temperature by looking at the periodic table
  • Precipitate

Chapter 3

  • 3 main particles in atom, their charges & location in the atom
  • Define atom
  • 3 types of radiation in nuclear reactions, characteristics, & symbols
  • Nuclear equations
  • Isotopes of the same element: how are they the same & how are they different?
  • Atomic number
  • Atomic mass (mass #) = #p+#n
  • Gold foil experiment
  • Determine #p, #n, #e- from element symbol:
  • Discuss the evolution of the atom model *hint: plum pudding vs. Rutherford model vs. electron cloud
  • Identify an elements gram-atomic mass (GAM) *NOTE: see moles
  • Band of Stability *NOTE: see stable vs. unstable nuclei
  • Find the gram-atomic mass *NOTE: see moles
  • Moles: find # of moles, # grams in x amount of moles, # of molecules or atoms (Avogadro’s # = 6.02 x 1023)

Chapter 4

  • Electromagnetic spectrum: define & list (in order) the wavelengths
  • Electromagnetic radiation: speed, wavelength, frequency
  • Electromagnetic radiation equations: c = λ * ν (c = 3.00 x 108 m/s);

E = h * ν (h = 6.63 x 10-34)

  • Electron configuration
  • Principal energy level: tell # of e- in each, when it is filled, maximum # of e- it can hold
  • Sublevels: # per principal energy level, how to tell when filled, maximum e- per sublevel
  • Orbital: # per sublevel, 2 e- per orbital
  • Bohr atom: how do e- move between energy levels
  • E- cloud
  • Photons
  • Shape of s and p orbitals
  • Possibilities for e- spin
  • Emission of energy (hint: electrons drop down a “level”)
  • Bright-line spectrum: what is it, what causes it
  • Orbital notation: # of e- paired, # of e- unpaired

Chapter 5

  • Periodic trends: atomic radius, ionization energy, electronegativity
  • Define: atomic radius, ionization energy, electronegativity
  • Locate on periodic table: alkali metals, alkaline earth metals, halogens, noble gases
  • Groups/Families vs. Periods: identify elements within NOTE: # of period indicates # of principal energy levels i.e. all the elements in period 2 have 2 principal energy levels
  • Mendeleev
  • Transition elements: where are they located on the periodic table & which sublevel is being filled
  • Elements in same groups have similar properties—why? (hint: same e- dot structures)
  • How are elements arranged in the modern periodic table
  • Most active metal and nonmetal

Reference Material (see the “Chemistry Reference Station” behind bench 1 & 2 for the following handouts)

  • Lab equipment
  • Metric cheat sheet
  • Sig fig rule & sig fig rules for math
  • Periodic trends
  • Electronegativities, ionization energy, electron affinity
  • Bonding concept map
  • Shapes of molecules

Miscellaneous

  • Any graphs asked on exams, are fair game for the midterm (hint: if you had trouble with the periodic table graph from that exam, make sure you ask me for help!)
  • Experimental questions i.e. given data/situation and answer questions about experiment
  • Reading a graduated cylinder
  • Reading a balance
  • Lab equipment!
  • Symbols for elements!

THIS IS NOT IMPOSSIBLE IF YOU STUDY!

YOU CAN DO IT!