Test your basic knowledge |

AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. Composition Formula
Delta H or Enthalpy Change
base
Molar Mass of Element/ Total Molar Mass %
ammonium

2. Speed of light - C
3.0x108m/s
permanent gases
ionic
8.314 J/K mol

3. R in instances that pertain to energy
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Isolated System
C=(mass)(specific heat)
8.314 J/K mol

4. Ptotal=P1+P2+P3+...

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

5. ... compounds are most conductive
First-Order Half Life
Integrated Rate Law
ionic
precipitate

6. Color of K (flame test)
triple point
endless
hydroxide
purple

7. For colligative properties for electrolytes - the # of mols of ions/ mols of solute

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

8. pH=
0
log[H+]
Density
Formal Charge

9. Idea Gas Law (actual rules)
conjugate acid
viscosity
are not
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions

10. r=k[A]
eth-
Scientific Method
First-Order Rate Law
weak acid strong base rxn

11. A monoatomic cation takes name from...
m (third quantum number)
-al
Its element
period

12. # bonding e- - # antibonding e-/2
Bond Order
Tetrahedral
Equilibrium constant
Chemical Bonds

13. Donates a single H+ Ion (... other prefixes also)
Monoprotic
Bonding Pairs
System
pi=(nRT)/v

14. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Atomic Mass Unit
Law of Definite Proportion
Cg=kPg

15. Describe various properties of one orbital
Lone Pair
Limiting reactant
Molar Heat Capacity
Quantum Numbers

16. Oxidation # of Polyatomic Ions
charge
vapor pressure
Diffusion
double bond

17. (A) - C/s
Ampere
dec-
sulfite
Standard Temperature and Pressure

18. 1/[A]=kt + 1/[A]0
-2 - with peroxide -1
Reducing Agent
Integrated Second-Order Rate Law
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

19. Amine prefix
Monoprotic
8.31J/Kmol
Amino-
-ol

20. Boltzmann constant - used in calculating speed of gas per molecule
Integrated Rate Law
wavelength
1.38x10?²³J/K
paramagnetic

21. r=k[A]^2
acetate
actual yield/theoretical yield x 100%
Second-Order Rate Law
isothermal

22. The part of the universe one is focused upon (in thermodynamics)
Valence Electrons(assigned)
specific heat
system
Theoretical yield

23. Where oxidation occurs
1.38x10?²³J/K
LE Model
96500
Anode

24. (organics) triple-bonded compound
alkyne
Angular Momentum Quantum Number
rate
Colligative properties

25. Mols A/ total mols - XA
mol Fraction
Dipole Moment
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
increasing

26. S²?
Amphoteric
Quantum Model
sulfide
-(P)(Change in V)

27. The heat changed in a chemical reaction.
s (fourth quantum number)
Molarity
1atm=?mmHg/Torr
Thermochemistry

28. O²?
Net Ionic Equation
Naming Binary Ionic Compounds
Law of Multiple Proportions
oxide

29. Cl¹?
chloride
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
8.31J/Kmol
reduction

30. 6.022x10^23
# protons + # neutrons
mol
First-Order Rate Law
Bases

31. AX2E - AX2E2
bent
# protons + # neutrons
Osmotic Pressure
charge

32. When gas compresses ...
Theoretical yield
Positive work value; work done on system
sublimation
log[H+]

33. 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
Integrated First-Order Rate Law
are not
end point
LE Model

34. negative ion
system
p+
Anion
Chemical Bonds

35. Half-life equation
N=N.(0.5)^time/time half-life
dec-
Bond enthalpy
moles solute/kg solvent

36. Osmotic pressure formula
pi=(nRT)/v
0
standard solution
-oic acid

37. Driving force of the electrons
hydrolysis
square pyramidal
Cell Potential (Ecell)
Molality

38. As protons are added to the nucleus - electrons are similarly added
Law of Conservation of Mass
Aufbau Principle
A Roman numeral
sulfate

39. Kinetic Energy of an individual particle formula
M = square root (3RT/mm)
1 atm
Cg=kPg
# protons (atom is defined by this)

40. AX2 - AX2E3
Ag+ - Pb2+ - Hg2+
moles of solute/ L of solution
linear
8.31J/Kmol

41. Dirrect Method Formula
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Chemical Bonds
3rd law of thermodynamics
Joule

42. 96 -485 C/mol e-
Faraday
Reducing Agent
Cell Potential (Ecell)
Boltzmann distribution

43. SO3²?
insoluble
sulfite
1/2mv²
Density

44. AX6
condensation
Molal FP Depression Constant
octahedral
Exothermic

45. (msubs) Can only be +1/2 or -1/2
?Hvap
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Electron Spin Quantum Number
allotrope

46. The reactant that is being reduced - brings about oxidation
oxidizing agent
Manometer
hydrolysis
Limiting reactant

47. How to Find a Weighted Average
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
0
Beta Particles-
cathode

48. The driving force for a spontaneous is an increase in entropy of the universe
m (third quantum number)
bond energy
Entropy (S)
Electronegativity

49. Color of Li (flame test)
red
Pressure
Exothermic
Electronegativity

50. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Law of Multiple Proportions
Dalton's Law of Partial Pressures
Diffusion
Hydrogen bonding