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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. Boiling point elevation formula
not spontaneous
?Tb= kb x molality
Adding
Law of Conservation of Energy

2. Has values from 0 to (n-1); tells shape of atomic orbitals
Arrhenius acid
Angular Momentum Quantum Number
Integrated Second-Order Rate Law
0.0821 atm L/mol K

3. 120° - sp^2
Allotrope
Trigonal Planar
activated complex (transition state)
Integrated First-Order Rate Law

4. Formula used when diluting stock solution (to find amount of water or stock needed)
H
M1V1=M2V2
rate gas A/rate gas B = square root (mm A/ mm B)
Ag+ - Pb2+ - Hg2+

5. For significant digits - trailing zeros _____ significant
are
salt bridge
square pyramidal
4.184

6. Non-Ideal Gas Conditions
g solute/g solvent x 100
high pressure - low temperature
-ol
Lone Pair

7. I=moles of particles/moles of solute dissolved

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8. (organics) nine carbons
non-
0
Anode
Alkaline earth metals

9. Unusually strong dipole forces found when H is bonded to N - O - or F
alkane
Hydrogen bonding
Formal Charge
Graham's Law

10. How to Find an Empirical Formula Given Grams
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
log[H+]
Its root and adding -ide
triple bond

11. l=3
fusion
Molecular Orbitals (MOs)
f
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

12. Amine prefix
Anion
Amino-
oxalate
# protons (atom is defined by this)

13. O²?
oxide
heat of vaporization
Principal Quantum Number
Faraday

14. Molecules' tendency to stick to one another
Pauli Exclusion Principle
Anion
base and hydrogen gas
cohesion

15. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
Ideal Gas Law
Buffered Solution
Nernst Equation

16. What is defined by you taken from the whole universe
blue
v3RT/M(in kg)
London dispersion forces
System

17. C2H3O2¹?
Reaction Quotient (Q)
% yield
1.38x10?²³J/K
acetate

18. 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)
k=Ae^(-Ea/RT)
# protons (atom is defined by this)
State Functions
+1 - except if bonded to Alkali Metal -1

19. AX4
tetrahedral
violet
Allotrope
Van't Hoff factor

20. Oxidation # of Ions
0
1 atm = 760 mmHg = 101.3 kPa
charge
red/orange

21. Mixing of gases
Diffusion
End Point
Percent Yield
0

22. Connects the 2 half cells in a voltaic cell
salt bridge
flouride
reduction
Calorimetry

23. Electrons in a hydrogen atom move around the nucleus only in circular orbits
adhesion
rate law
tetrahedral
Quantum Model

24. Kinetic Energy is proportional to ______
diamagnetic
Calorimetry
Boltzmann distribution
Temperature

25. Mass/volume
oxide gas and water
Isolated System
Density
electrolyte

26. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Reaction Quotient (Q)
yellow --> green
0
Heat

27. A given compound always has exactly the same proportion of elements by mass
single bond
Law of Definite Proportion
Transition metals
Ionic Compounds

28. Measure of the average kinetic energy of all the particles in a substance
Acids
Temperature
Joule
Law of Conservation of Energy

29. Symbol for Total Heat absorbed or released
hydrolysis
q
Dalton's Law
P1= X1P1°

30. SI unit of energy; Kg*m^2/s^2
alkene
Nernst Equation
Joule
Molecular Compounds

31. CN¹?
vapor pressure
ammonium
cyanide
6.63x10?³4Js

32. Chemical composition of dry ice
M1V1=M2V2
solid CO2
Molecule
Its element

33. ln[A] vs. time is a ...-order reaction
Heisenberg Uncertainty Principle
Trigonal Bipyramidal
Integrated First-Order Rate Law
first

34. Mass reactants= mass products
Law of Conservation of Mass
London Dispersion Forces
1 atm
System

35. pH=
Osmotic Pressure
t-shape
Chemical Bonds
log[H+]

36. Unit of electrical potential; J/C
Calorimetry
PV=nRT
Volt
0 degrees C - 1 atm

37. R=
0.0826Latm/Kmol
entropy (S)
different # of neutrons
8.314 J/K mol

38. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium

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39. Peak of energy diagram
Work
Oxidizing Agent
activated complex (transition state)
Molecular Orbitals (MOs)

40. AX5E
A Roman numeral
Acid + Base --> Salt + Water
square pyramidal
Integrated First-Order Rate Law

41. IMF that exists in polar molecules
trigonal pyramidal
Solute
freezing
Dipole-dipole forces

42. Loss of electrons - increase in oxidation #
Density
van't Hoff Factor
Isolated System
oxidation

43. Cl¹?
Law of Multiple Proportions
chloride
triple bond
Ampere

44. Atoms with the same number of protons but a different number of neutrons
endless
different # of neutrons
Isotopes
(moles of products that are gasses) - (moles of reactants that are gasses)

45. Like dissolves...
Principal Quantum Number
cohesion
first
like

46. 180° - sp
Linear
Van't Hoff factor
Dalton's Law
Beta Particles-

47. AX3
Bronsted-Lowry Base
trigonal planar
Galvanic Cell
weak acid strong base rxn

48. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Graham's Law
1st law of thermodynamics
Cg=kPg
-oic acid

49. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
insoluble
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Polar Covalent
entropy

50. l=0
London dispersion forces
Chemical Bonds
Amino-
s