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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. Substances that form OH- when dissolved in water; proton acceptors
Bases
are
Dipole Moment
bent

2. Speed of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm A/ mm B)
second
ammonium
Ionic Compounds

3. Has values 1 -2 -3 -...; tells energy levels
triple bond
Principal Quantum Number
boiling point
Limiting reactant

4. How to Find an Empirical Formula Given Grams
moles solute/kg solvent
22.4L
non-
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

5. The minimum energy that molecules must possess for collisions to be effective - Ea
Weight
entropy (S)
activation energy
rate gas A/rate gas B = square root (mm A/ mm B)

6. Determined by the formula h/m(in kg)v - (v=velocity)
electrolyte
wavelength
boiling point
Bronsted-Lowry acid

7. Energy needed to break a bond
bond energy
strong acids
oxalate
1.86°C

8. What is defined by you taken from the whole universe
ammonium
Theoretical yield
System
hydroxide

9. Amount of gravitational force exerted on an object
diamagnetic
Weight
Equivalence Point
Law of Multiple Proportions

10. Moles of solute/volume of soln(L)
Aufbau Principle
Molarity
2nd law of thermodynamics
square planar

11. Variable for orientation of orbital (-1 through +1)
trigonal pyramidal
m (third quantum number)
Exothermic
Aufbau Principle

12. C=2.9979*10^8 m/s
Speed of light
Trigonal Bipyramidal
lambda
Law of Multiple Proportions

13. Planck's constant - used to calculate energy w/frequency
supercritical fluid
viscosity
6.63x10?³4Js
Isolated System

14. (organics) five carbons
weak acid strong base rxn
pent-
m (third quantum number)
Arrhenius equation

15. H?+OH??H2O
yellow --> green
Pressure of H2O must be Subtracted
strong acid strong base rxn
Molarity

16. Reactant which doesn't get used up completely in a chemical reaction
Electronegativity
Ag+ - Pb2+ - Hg2+
excess reactant
supercritical fluid

17. Substances w/ critical temperatures below 25°C
q
Polar Covalent
permanent gases
Calorimetry

18. A weak acid that changes color at or near the equivalence point
indicator
adiabatic
# protons (atom is defined by this)
6.63x10?³4Js

19. (organics) nine carbons
Cation
purple
non-
M1V1=M2V2

20. A monoatomic cation takes name from...
AE = q + w
Its element
Colligative properties
cathode

21. Type of system in which nothing is transfered (no mass or energy); ideal
charge
Bronsted-Lowry Base
Isolated System
0

22. CO3²?
purple
conjugate base
d orbitals
carbonate

23. Ptotal=Pa+Pb+Pc....

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24. When n=4 ->2 - color=
3rd law of thermodynamics
-one
blue-green
Molecular Orbitals (MOs)

25. AX5E
third
linear
square pyramidal
Molarity

26. Point at which solid?liquid occurs
indicator
supercritical fluid
condensation
melting point

27. 2+ charge
violet
Zero-Order Rate Law
Alpha Particles-
square pyramidal

28. Passage of gas through tiny orifice
Effusion
spontaneity
Ideal Gas Law
cathode

29. Amine prefix
Amino-
London dispersion forces
Theory of Relativity
red

30. Atoms combine in fixed whole # ratios
Alkaline earth metals
Law of Multiple Proportions
Atomic Mass Unit
are

31. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
bond energy
methoxy-
Polar Covalent
voltaic cells

32. Occupies the space above and below a sigma bond
Bonding Pairs
excess reactant
p orbitals
Pi Bond

33. A given compound always has exactly the same proportion of elements by mass
methods of increasing rate
Law of Definite Proportion
yellow --> green
like

34. The total entropy is always increasing - all systems tend towards maximum entropy
First-Order Rate Law
London dispersion forces
2nd law of thermodynamics
spontaneous

35. 2 or more covalently bonded atoms
pi=(nRT)/v
Density
E
Molecule

36. Color of Sr (flame test)
C=(mass)(specific heat)
1atm=?Pa
are
red

37. PV=nRT
0
Ideal Gas Law
?Tf= kf x molality
e-

38. A monoatomic anion is named by taking...
System
Its root and adding -ide
8.314 J/K mol
strong acid strong base rxn

39. (organics) eight carbons
Molality
Principal Quantum Number
allotrope
oct-

40. Electron (symbol)
Buffered Solution
e-
Standard Temperature and Pressure
yellow

41. 760mmHg/Torr
1atm=?mmHg/Torr
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
1st law of thermodynamics
reduction agent

42. Liquid to gas
Hydrogen bonding
vaporization
M1V1=M2V2
C=(mass)(specific heat)

43. Wavelength symbol
lambda
blue-green
Law of Conservation of Mass
Formal Charge

44. The mixing of native atomic orbitals to form special orbitals for bonding
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Hybridization
Its root and adding -ide
Hund's Rule

45. Puts H? into solution
oxalate
Arrhenius acid
Cg=kPg
Dipole Moment

46. Expresses how the concentrations depend on time
Overall Reaction Order
Atomic Mass Unit
Integrated Rate Law
base and hydrogen gas

47. Oxidation # of Hydrogen
carbonate
+1 - except if bonded to Alkali Metal -1
P1= X1P1°
Aufbau Principle

48. The reactant that is being reduced - brings about oxidation
rate gas A/rate gas B = square root (mm A/ mm B)
Quantum Model
LE Model
oxidizing agent

49. Ionizes to produce H+ ions
viscosity
AE= AH - RTAn
Arrhenius Acid
Lone Pair

50. The energy required to raise 1 g of substance 1 degree C
nitrate
strong bases
Specific Heat (s)
non-