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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. 6.022x10^23
purple --> pink
p
Delta H or Enthalpy Change
mol

2. Energy can't be created nor destroyed
Magnetic Quantum Number (ml)
Law of Conservation of Energy
Hess's Law
Amount of atoms present

3. When n=3 ->2 - color=
red
Alkaline earth metals
Specific Heat (s)
H

4. When _____ significant digits - round answer to least significant digit
Multiplying
Acids
zero
oxalate

5. Change in Energy = ? (in terms of constant pressure; for gasses)
Dalton's Law
Molecular Orbitals (MOs)
Atomic Mass Unit
AE= AH - RTAn

6. S²?
Hess's Law
Bond Order
sulfide
activation energy

7. J/°Cmol or J/Kmol
Specific Heat (s)
Enthalpy of Solution
Molar Heat Capacity
indicator

8. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
melting
yellow
Radioactivity

9. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Formal Charge
Increase Temperature
hydrolysis
Alpha Particles-

10. Weakest IMFs - found in all molecules
Temperature
Adding
permanent gases
London dispersion forces

11. Faraday's constant
msAT
96500
P1= X1P1°
Cell Potential (Ecell)

12. A monoatomic cation takes name from...
Bronsted-Lowry Acid
Second-Order Half Life
Its element
system

13. x can be ignored when % ionization is <5%
Equilibrium constant
strong acids
v3kT/m
5% rule

14. Rate of Diffusion/Effusion formula
LeChatelier's Principle
amine
Hydrogen bonding
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

15. Volume of gas @STP
Atomic Mass Unit
Quantum Model
22.4L
heat of fusion

16. The chemical formed when a base accepts a proton
conjugate acid
bent
Molality
Endothermic

17. AX4
tetrahedral
Increase Temperature
Buffer
second

18. neutron (symbol)
n0
Alkaline earth metals
Force = mass x acceleration
Enthalpy of Solution

19. Ester suffix
-oate
8.31J/Kmol
different # of neutrons
AH

20. I¹?
s orbitals
Overall Reaction Order
iodide
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

21. Variable for type of orbital
experimental yield
l (second quantum number)
catalyst
non-

22. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Amphoteric
1/2mv²
Molality

23. R=
permanganate
pi=(nRT)/v
Pauli Exclusion Principle
0.0826Latm/Kmol

24. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
blue
second
Bronsted-Lowry base
Acid + Base --> Salt + Water

25. Boiling point - melting point - viscosity - vapor pressure - surface tension
effects of IMF
Allotrope
Covalently w/in themselves - Ionicly bonded w/ each other
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

26. (organics) nine carbons
yellow --> green
non-
endless
Chemical Kinetics

27. ClO2¹?
Molal BP Elevation Constant
zero
charge
chlorite

28. The reactant that is being reduced - brings about oxidation
oxidizing agent
Ionic Compounds
0.0826Latm/Kmol
-ic acid

29. negative ion
Anion
boiling point
Bronsted-Lowry Acid
sulfide

30. A measure of resistance of an object to a change in its state of motion
Q>K
blue-violet
Mass
yellow --> green

31. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
exothermic
zero
Equivalence Point
LE Model

32. How to Find an Empirical Formula Given Grams
AE= AH - RTAn
Molecule
square planar
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

33. Cation first - anion second
Naming Binary Ionic Compounds
sublimation
zero
hydrolysis

34. Oxidation # of Ions
charge
not spontaneous
% error
viscosity

35. Actual Yield/Theoretical Yield*100%
Percent Yield
Buffer
charge
Bond enthalpy

36. High-speed electrons
Beta Particles-
Alkaline earth metals
red
Pi Bond

37. Entropy in the universe is always...
insoluble
increasing
Thermochemistry
red/orange

38. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Solution
5% rule
trigonal pyramidal
soluble

39. Occupies the space above and below a sigma bond
0.512°C
Hydrogen bonding
Pi Bond
Force = mass x acceleration

40. Energy required for liquid?gas
tetrahedral
Transition metals
heat of vaporization
0

41. All forms of energy except for heat
1.86°C
P1V1/N1T1=P2V2/N2T2
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
work

42. (organics) triple-bonded compound
charge
alkyne
t-shape
analyte

43. Ability of an atom in a molecule to attract shared electrons to itself
p
% error
prop-
Electronegativity

44. AX4E2
square planar
Cg=kPg
1atm=?mmHg/Torr
Principal Quantum Number

45. Group 1 and heavier Group 2 bases
1 atm = 760 mmHg = 101.3 kPa
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
strong bases
k=Ae^(-Ea/RT)

46. Bomb Calorimeter
X of a = moles a/total moles
Constant Volume
Cell Potential (Ecell)
paramagnetic

47. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
% error
Chemical Kinetics
Bond enthalpy
bromate

48. Symbol for Enthalpy
rate law
H
standard solution
eth-

49. Ionizes to produce H+ ions
Arrhenius Acid
Trigonal Planar
Trigonal Bipyramidal
Tetrahedral

50. CO3²?
equilibrium
carbonate
different # of neutrons
Multiplying