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. Different form of same element
allotrope
Density
base
strong acids

2. Negative enthalpy - heat flows into surroundings
exothermic
insoluble
supercritical fluid
Closed System

3. Osmotic pressure=MRT
blue
Osmotic Pressure
oxide gas and water
Zero-Order Half Life

4. Thickness
Molal BP Elevation Constant
sulfate
viscosity
group

5. Ability of an atom in a molecule to attract shared electrons to itself
Negative work value; work done by system
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
diamagnetic
Electronegativity

6. Where oxidation occurs
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Anode
P1V1/N1T1=P2V2/N2T2
reduction agent

7. PO4³?
q
C + 273
phosphate
Naming Binary Ionic Compounds

8. Energy required for liquid?gas
Enthalpy of Solution
Formal Charge
Hydrogen bonding
heat of vaporization

9. Delta H (AH) = ?
d orbitals
q/moles
moles solute/kg solvent
red

10. AX5E
alkene
square pyramidal
rate
(moles of products that are gasses) - (moles of reactants that are gasses)

11. The measurement of heat changes
Law of Conservation of Energy
equilibrium
Calorimetry
0

12. STP
square pyramidal
1st law of thermodynamics
bromate
0 degrees C - 1 atm

13. I¹?
P1= X1P1°
iodide
Gamma Ray-
tetrahedral

14. ?T=k*m(solute)
Quantum Model
Colligative properties
Molal BP Elevation Constant
Integrated Second-Order Rate Law

15. The reactant that is being reduced - brings about oxidation
Scientific Method
acid
single bond
oxidizing agent

16. (# of lone pair e-)+1/2(# of shared e-)
STP
yellow
oxidation
Valence Electrons(assigned)

17. Symbol for Total Heat absorbed or released
q
critical point
Polar Covalent
are

18. (msubs) Can only be +1/2 or -1/2
f
Electron Spin Quantum Number
-(q of H2O + q of cal)
Cell Potential (Ecell)

19. Ka=[products]^m/[reactants]^n
Anode
Bronsted-Lowry Base
Acid Dissociation Constant
permanganate

20. Chemical composition of dry ice
solid CO2
Alkali metals
Hund's Rule
Pauli Exclusion Principle

21. Substances that form OH- when dissolved in water; proton acceptors
pent-
methods of increasing rate
Bases
Ionic

22. (organics) single-bonded compound
triple point
alkane
-ol
amine

23. For colligative properties for electrolytes - the # of mols of ions/ mols of solute

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

24. Change without heat transfer between the system and its surroundings
adiabatic
log[H+]
reduction
Quantum Numbers

25. A solution used in titrations whose concentration is known
Molecular Compounds
-(q of H2O + q of cal)
standard solution
First-Order Rate Law

26. When gas compresses ...
Le Chatelier's Principle
Second-Order Rate Law
Positive work value; work done on system
red

27. Cl¹?
chloride
Enthalpy of Solution
alkane
nitrate

28. (organics) one carbon
1/2mv²
Enthalpy of Solution
Bronsted-Lowry Acid
meth-

29. AX6
Trigonal Bipyramidal
octahedral
ammonium
Constant Volume

30. A solution that resists a change in its pH
hept-
dichromate
Buffered Solution
Heisenberg Uncertainty Principle

31. Kinetic Energy per molecule
STP
1/2mv²
Arrhenius equation
Entropy (S)

32. 0°C and 1 atm
% error
reduction
linear
STP

33. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
LeChatelier's Principle
-ous acid
standard solution

34. AX2 - AX2E3
melting
linear
+1 - except if bonded to Alkali Metal -1
violet

35. kb of water
0.512°C
A Roman numeral
sublimation
titrant buret

36. How to Balance a Redox Equation
Boltzmann distribution
Weight
d orbitals
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

37. (organics) nine carbons
Cathode
group
purple
non-

38. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Alkaline earth metals
heat of fusion
work
Acid + Base --> Salt + Water

39. Rate of Diffusion/Effusion formula
surroundings
Hydrogen bonding
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Density

40. If heat capacity isn't mentioned - you can assume that q of cal is = ?
pent-
0
square planar
AE = q + w

41. Where reduction occurs
Cathode
Root Mean Square Velocity
-ous acid
Pressure of H2O must be Subtracted

42. C=2.9979*10^8 m/s
Octahedral
Speed of light
triple point
sublimation

43. Mol of solute/kg of solvent
P1V1/N1T1=P2V2/N2T2
Molality
base
nitrate

44. F¹?
linear
lambda
Graham's Law
flouride

45. 109.5° - sp^3
Tetrahedral
Ampere
m (third quantum number)
0

46. Oxidation # of Hydrogen
Amino-
+1 - except if bonded to Alkali Metal -1
sublimation
carbonate

47. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
force x distance = work done
Alkali metals
Graham's Law
Boltzmann distribution

48. When ____ significant digits - round answer to least decimal place
viscosity
Adding
Osmotic Pressure
linear

49. negative ion
oct-
X of a = moles a/total moles
Anion
square planar

50. Color of Li (flame test)
red
msAT
Aufbau Principle
square planar