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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. HF+ OH??H2O
weak acid strong base rxn
deposition
Negative work value; work done by system
prop-

2. When n=5 ->2 - color=
blue-violet
Hund's Rule
nitrate
0

3. Mole Fraction
chlorate
X of a = moles a/total moles
Cell Potential (Ecell)
P1= X1P1°

4. Pressure Units/Conversions
1 atm = 760 mmHg = 101.3 kPa
indicator
Octahedral
wavelength

5. Proton (symbol)
Alkaline earth metals
p+
melting
1 atm = 760 mmHg = 101.3 kPa

6. Arrhenius equation
k=Ae^(-Ea/RT)
4.184
alkane
Scientific Method

7. Raoult's Law - relations between vapor pressure and concentrations
Dipole-dipole forces
P1= X1P1°
exothermic
force x distance = work done

8. Oxoacid solution (such as HSO4-) forms...
-one
nitrite
oxide gas and water
Graham's Law

9. ?Hsoln=?H1+?H2+?H3+...
triple point
# protons + # neutrons
Enthalpy of Solution
96500

10. Substance that - when dissolved - is conductive
linear
electrolyte
Polar Covalent
Theory of Relativity

11. Osmotic pressure=MRT
Transition metals
surroundings
Osmotic Pressure
-al

12. CO3²?
carbonate
mol Fraction
Amount of atoms present
d orbitals

13. H + donor
octahedral
Bronsted-Lowry Acid
8.314 J/K mol
heat of vaporization

14. Polyatomic Ions (bonding)
Dipole Moment
Covalently w/in themselves - Ionicly bonded w/ each other
1 atm = 760 mmHg = 101.3 kPa
Molality

15. Measure of the average kinetic energy of all the particles in a substance
see-saw
van't Hoff Factor
precipitate
Temperature

16. Cr2O7²?
carbohydrates
Integrated Zero-Order Rate Law
specific heat
dichromate

17. Point at which liquid?gas occurs
square planar
boiling point
Angular Momentum Quantum Number
Its root and adding -ide

18. Energy (definition)
Entropy (S)
Limiting reactant
force x distance = work done
Solvent

19. Mass/volume
Density
heat of vaporization
0
blue

20. Puts H? into solution
q/moles
Octahedral
zero
Arrhenius acid

21. Phase change from solid to gas
0.512°C
Balmer Series
equilibrium
sublimation

22. Hydroxides are soluble or insoluble?
Reaction Quotient (Q)
% yield
Le Chatelier's Principle
insoluble

23. Significant Digits of counted things
t-shape
charge
Quantum Mechanical Model
endless

24. (N) number of equivalents per liter of solution
carbonate
adhesion
Normality
6.63x10?³4Js

25. l=2
Molecular
d
Diffusion
Integrated First-Order Rate Law

26. F¹?
London dispersion forces
flouride
melting point
sulfate

27. Type of system in which the energy may escape - but the mass is conserved
Pi Bond
Closed System
red/orange
-one

28. Freezing point depression formula
dichromate
Quantum Mechanical Model
?Tf= kf x molality
Dalton's Law of Partial Pressures

29. A monoatomic cation takes name from...
Its element
Calorimeter
amine
Chemical Bonds

30. A method of investigation involving observation and theory to test scientific hypotheses
Ampere
effects of IMF
Its root and adding -ide
Scientific Method

31. Different form of same element
P1= X1P1°
sublimation
cathode
allotrope

32. The total energy of the universe is constant - all systems tend towards minimum energy
Decrease Volume and Increase Temperature
Integrated Rate Law
1.86°C
1st law of thermodynamics

33. (organics) single-bonded compound
alkane
Anion
Speed of light
Galvanic Cell

34. Force per unit area
Hund's Rule
Pressure
hydro-ic acid
entropy

35. Only contains ions that change in reaction
Net Ionic Equation
Molarity
specific heat
Its root and adding -ide

36. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
Cg=kPg
+1 - except if bonded to Alkali Metal -1
Diffusion

37. (organics) triple-bonded compound
pi=(nRT)/v
alkyne
square planar
mol Fraction

38. Oxidation # of Polyatomic Ions
charge
Integrated Rate Law
Q<K
group

39. Speed of Diffusion/Effusion formula
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
electron affinity
iodide
rate gas A/rate gas B = square root (mm A/ mm B)

40. Expresses how the concentrations depend on time
violet
Integrated Rate Law
London dispersion forces
weak acid strong base rxn

41. Energy required to break a bond
Bronsted-Lowry Base
hydrocarbons
1st law of thermodynamics
Bond Energy

42. (organics) ten carbons
q
hydrocarbons
dec-
Principal Quantum Number

43. AX2E - AX2E2
Percent Yield
lambda
bent
nitrite

44. Raising heat - adding catalyst - heighten concentration - bigger surface area
charge
Nernst Equation
methods of increasing rate
Arrhenius Base

45. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Equilibrium Expression
0.0826Latm/Kmol
electron affinity
Pauli Exclusion Principle

46. Colors of Reaction when (MnO4 -) --> (Mn2+)
Law of Conservation of Energy
purple --> pink
Gamma Ray-
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

47. Increase Volume
Increase Temperature
Finding Empirical Formulas
r1/r2
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

48. Energy can't be created nor destroyed
Law of Conservation of Energy
perchlorate
A Roman numeral
green/yellow

49. 1 sigma bond - 2 pi bonds
triple bond
chlorite
like
2nd law of thermodynamics

50. A monoatomic anion is named by taking...
Bronsted-Lowry acid
Anode
Nernst Equation
Its root and adding -ide