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. r=k
square pyramidal
Zero-Order Rate Law
Electron Spin Quantum Number
activation energy

2. J/°Cmol or J/Kmol
cohesion
trigonal bipyramidal
Molar Heat Capacity
entropy (S)

3. Negative enthalpy - heat flows into surroundings
1.38x10?²³J/K
Pi Bond
exothermic
Le Chatelier's Principle

4. H?+NH3?NH4
mol
entropy
Strong acid weak base rxn
Tetrahedral

5. In covalent bonds - prefixes are used to tell...
Amount of atoms present
indicator
Volt
entropy

6. Chemical composition of dry ice
Open System
solid CO2
rate law
Joule

7. Bomb Calorimeter
Zero-Order Half Life
Oxidizing Agent
Constant Volume
% yield

8. When ____ significant digits - round answer to least decimal place
Bond Order
p
Net Ionic Equation
Adding

9. A solution used in titrations whose concentration is known
violet
work
(moles of products that are gasses) - (moles of reactants that are gasses)
standard solution

10. In a given atom no two electrons can have the same set of four quantum numbers
Arrhenius base
viscosity
trigonal bipyramidal
Pauli Exclusion Principle

11. Proton acceptors - must have an unshared pair of e?s
Bronsted-Lowry base
Overall Reaction Order
system
Manometer

12. Cl¹?
chloride
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
E
wavelength

13. Arrhenius equation
Calorimetry
Aufbau Principle
blue-green
k=Ae^(-Ea/RT)

14. Elements in groups 3-12
Reaction Quotient (Q)
Temperature
bent
Transition metals

15. Different form of same element
moles solute/kg solvent
weak acid strong base rxn
1/2mv²
allotrope

16. q H2O = ?
endless
msAT
hex-
0.0826Latm/Kmol

17. A measure of randomness or disorder
Open System
entropy
Finding Empirical Formulas
bond energy

18. Each orbital can hold two e?s each w/ opposite spins
Force = mass x acceleration
Pauli Exclusion Principle
permanganate
second

19. q cal = ?
0 degrees C - 1 atm
Atomic Mass Unit
CAT
rate gas A/rate gas B = square root (mm A/ mm B)

20. % yield
actual yield/theoretical yield x 100%
Arrhenius equation
Cg=kPg
Reducing Agent

21. Proton donors
A Roman numeral
not spontaneous
Bronsted-Lowry acid
flouride

22. Force acting over distance
rate gas A/rate gas B = square root (mm A/ mm B)
Second-Order Half Life
no precipitate forms
Work

23. Releases/gives off heat (negative value)
Exothermic
geometric isomers
p orbitals
Galvanic Cell

24. Amount of gravitational force exerted on an object
Weight
Integrated Second-Order Rate Law
sulfite
condensation

25. AX5
Thermochemistry
trigonal bipyramidal
carbonate
adhesion

26. Point at which solid?liquid occurs
eth-
0 degrees C - 1 atm
e-
melting point

27. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
Reaction Quotient (Q)
oxalate
C + 273

28. 0°C and 1 atm
Integrated Second-Order Rate Law
Heisenberg Uncertainty Principle
STP
Galvanic Cell

29. Planck's constant - used to calculate energy w/frequency
effects of IMF
6.63x10?³4Js
condensation
-oate

30. R=
Reaction Quotient (Q)
0.0826Latm/Kmol
Angular Momentum Quantum Number
alkene

31. High-energy light
Gamma Ray-
equilibrium
heat of vaporization
purple --> pink

32. Half-life equation
e-
end point
permanent gases
N=N.(0.5)^time/time half-life

33. Oxidation # of Polyatomic Ions
oct-
charge
Decrease Volume and Increase Temperature
Transition metals

34. If anion ends in -ide - acid name ends in
hydro-ic acid
activation energy
-al
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

35. Determined by the formula h/m(in kg)v - (v=velocity)
wavelength
triple bond
0 degrees C - 1 atm
v3kT/m

36. Moles of solute/volume of soln(L)
freezing
Molarity
Weight
reduction agent

37. Solid to liquid
surroundings
Principal Quantum Number
melting
# protons (atom is defined by this)

38. C=2.9979*10^8 m/s
Speed of light
Endothermic
Closed System
Thermochemistry

39. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
mol Fraction
Bond enthalpy
State Functions
8.314 J/K mol

40. If heat capacity isn't mentioned - you can assume that q of cal is = ?
0
Nodes
5% rule
-one

41. Amount of heat needed to change a system by 1°C
oct-
anode
heat capacity
red

42. Temperature-pressure combination at which solid - liquid - and gas states appear
triple point
Heisenberg Uncertainty Principle
purple --> pink
Bronsted-Lowry Acid

43. IMF that exists in polar molecules
Ligand
Mass
Dipole-dipole forces
Electronegativity

44. Color of K (flame test)
CAT
purple
Octahedral
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

45. AX5E
?Tf= kf x molality
AE = q + w
octahedral
square pyramidal

46. Speed of light - C
3.0x108m/s
oxide
charge
Pauli Exclusion Principle

47. How to Balance a Redox Equation
Law of Multiple Proportions
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
0
base

48. OIL RIG
square planar
-al
heat of vaporization
Oxidation is Loss Reduction is Gain

49. Donates a single H+ Ion (... other prefixes also)
Specific Heat Capacity
conjugate base
Monoprotic
Bond enthalpy

50. O²?
triple bond
charge
Gamma Ray-
oxide