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AP Chemistry

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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. In covalent bonds - prefixes are used to tell...
Amount of atoms present
Linear
Arrhenius base
reduction

2. AX3E2
T-shape
s (fourth quantum number)
Colligative properties
specific heat

3. The total energy of the universe is constant - all systems tend towards minimum energy
experimental yield
Bond Energy
Molality
1st law of thermodynamics

4. 180 - sp
?Tb= kb x molality
oxalate
Graham's Law
Linear

5. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
heat of fusion
strong acids
End Point
Gamma Ray-

6. Color of Li (flame test)
no precipitate forms
red
s (fourth quantum number)
nitrate

7. ClO3?
chlorate
Anode
Atomic Mass Unit
Q>K

8. Absorbs/takes in heat (positive value)
Metalliods
Trigonal Planar
Amphoteric
Endothermic

9. Liquid to gas
vaporization
M = square root (3RT/mm)
Exothermic
Kinetic Molecular Theory - for ideal gases

10. How to Balance a Redox Equation
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
sulfate
l (second quantum number)
square pyramidal

11. Elements which have unpaired electrons and highly affected by magnetic fields
Law of Conservation of Energy
Acids
Tetrahedral
paramagnetic

12. (msubs) Can only be +1/2 or -1/2
Electron Spin Quantum Number
State Functions
Standard Temperature and Pressure
n0

13. Raising heat - adding catalyst - heighten concentration - bigger surface area
4.184
s (fourth quantum number)
T-shape
methods of increasing rate

14. Variable for orientation of orbital (-1 through +1)
force x distance = work done
rate
m (third quantum number)
1atm=?Pa

15. J/Cmol or J/Kmol
oxidation
activation energy
Molar Heat Capacity
Q<K

16. Solid to gas
Its element
sublimation
Mass
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

17. Variable for energy of e- - goes from 1 -2 -3 on up
solid CO2
n (first quantum number)
0.0821 atm L/mol K
geometric isomers

18. (organics) nine carbons
non-
Gamma Ray-
Integrated Rate Law
Pauli Exclusion Principle

19. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Ionic Compounds
d orbitals
k=Ae^(-Ea/RT)
single bond

20. Has values 1 -2 -3 -...; tells energy levels
alcohol
bromate
Principal Quantum Number
-oic acid

21. Dalton's Law of Partial Pressures (to find partial pressure formula)
cohesion
P of a =(X of a)(total pressure)
A Roman numeral
Hess's Law

22. Ionizes to produce H+ ions
1.86C
end point
red/orange
Arrhenius Acid

23. Point at which liquid?gas occurs
Multiplying
boiling point
p
-one

24. Phase change from solid to gas
sublimation
condensation
0.0821 atm L/mol K
nitrate

25. kf of water
1.86C
P1V1/N1T1=P2V2/N2T2
Acid Dissociation Constant
Electron Spin Quantum Number

26. J/Cg or J/Kg
Specific Heat Capacity
N=N.(0.5)^time/time half-life
methoxy-
Positive work value; work done on system

27. These orbitals are perpendicular
p orbitals
Dipole Moment
v3kT/m
Molecular

28. Significant Digits of Conversion Factors
second
endless
conjugate base
Alpha Particles-

29. In a given atom no two electrons can have the same set of four quantum numbers
Tetrahedral
Pauli Exclusion Principle
Beta Particles-
standard solution

30. frequency symbol
cyanide
nu
Arrhenius Acid
Temperature

31. H+ Acceptor
chlorite
Its root and adding -ide
Bronsted-Lowry Base
P of a =(X of a)(total pressure)

32. r=k
Manometer
Zero-Order Rate Law
reduction
Heat Capacity (C)

33. Organic w/ -NH2
no precipitate forms
Magnetic Quantum Number (ml)
Trigonal Bipyramidal
amine

34. Color of Ba (flame test)
s (fourth quantum number)
Entropy (S)
green/yellow
square planar

35. 760mmHg/Torr
Chemical Kinetics
1atm=?mmHg/Torr
alkane
Bronsted-Lowry acid

36. All forms of energy except for heat
d
work
Amphoteric
sulfide

37. To find activation energy use the...
excess reactant
AE = q + w
specific heat
Arrhenius equation

38. (organics) seven carbons
m (third quantum number)
allotrope
different # of neutrons
hept-

39. Arrhenius equation
k=Ae^(-Ea/RT)
freezing
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Isotopes

40. 6.022x10^23
Acid Dissociation Constant
Principal Quantum Number
mol
8.314 J/K mol

41. Pressure Units/Conversions
Integrated First-Order Rate Law
First-Order Rate Law
1 atm = 760 mmHg = 101.3 kPa
critical point

42. Symbol for Enthalpy
Molal FP Depression Constant
H
Weight
Amphoteric

43. (organics) double-bonded compound
alkene
green/yellow
chlorate
Delta H or Enthalpy Change

44. Energy needed to vaporize a mole of a liquid
permanganate
?Hvap
Principal Quantum Number
C=(mass)(specific heat)

45. Peak of energy diagram
1st law of thermodynamics
oxalate
activated complex (transition state)
Bond Energy

46. Nonmetal oxide + H2O ->
acid
octahedral
third
2nd law of thermodynamics

47. A given compound always has exactly the same proportion of elements by mass
hept-
Molecular
?Tf= kf x molality
Law of Definite Proportion

48. Energy (definition)
force x distance = work done
red/orange
Boltzmann distribution
specific heat

49. 2+ charge
sublimation
Alpha Particles-
critical point
Normality

50. Liquid to solid
square pyramidal
red
Hund's Rule
freezing

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