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. When gas expands ...
Integrated Zero-Order Rate Law
solid CO2
Root Mean Square Velocity
Negative work value; work done by system

2. U(rms)=(3RT/M)^1/2
insoluble
q/moles
Root Mean Square Velocity
electron affinity

3. r=k[A]^2
Second-Order Rate Law
like
oxide gas and water
Acid + Base --> Salt + Water

4. Osmotic pressure formula
pi=(nRT)/v
strong acids
Heat
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

5. Ketone suffix
-one
anode
standard solution
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

6. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
Temperature
ammonium
C=(mass)(specific heat)

7. Oxoacid solution (such as HSO4-) forms...
viscosity
condensation
Naming Binary Ionic Compounds
oxide gas and water

8. These orbitals are diagonal
d orbitals
heat capacity
Temperature
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

9. Isotope
1.86°C
C + 273
Radioactivity
different # of neutrons

10. ?T=k*m(solute)
-(P)(Change in V)
First-Order Half Life
Ionic
Molal BP Elevation Constant

11. Point at which solid?liquid occurs
Standard Temperature and Pressure
nu
Alkaline earth metals
melting point

12. An equilibrium expression
Solubility Product (Ksp)
Hund's Rule
Exothermic
reduction

13. These orbitals are perpendicular
Delta H or Enthalpy Change
entropy (S)
mol Fraction
p orbitals

14. A device used to measure Delta H
Temperature
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Calorimeter
Covalently w/in themselves - Ionicly bonded w/ each other

15. Resistance to flow
Oxidizing Agent
triple bond
Acid + Base --> Salt + Water
viscosity

16. STP
Buffer
experimental yield
Amino-
0 degrees C - 1 atm

17. Heat capacity formula
Electronegativity
oxidizing agent
alkyne
C=(mass)(specific heat)

18. (organics) single-bonded compound
alkane
Solute
Dipole-dipole forces
First-Order Half Life

19. Point at which vapor pressure=air pressure above
Antibonding Molecular Orbital
endothermic
0
boiling point

20. l=2
3rd law of thermodynamics
Specific Heat (s)
d
Bond Order

21. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Trigonal Planar
Dalton's Law of Partial Pressures
Quantum Model
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

22. This MUST be determined experimentally
red
amine
rate law
London Dispersion Forces

23. Oxidation # of free elements
r1/r2
Anode
Amphoteric
0

24. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
voltaic cells
like
Endothermic
Acid + Base --> Salt + Water

25. Negative enthalpy - heat flows into surroundings
96500
exothermic
sublimation
trigonal pyramidal

26. 760mmHg/Torr
strong acid strong base rxn
1atm=?mmHg/Torr
State Functions
linear

27. F¹?
Allotrope
reduction agent
Aufbau Principle
flouride

28. SI unit of energy; Kg*m^2/s^2
Dalton's Law
Heat Capacity (C)
Joule
% yield

29. Force acting over distance
m (third quantum number)
different # of neutrons
r1/r2
Work

30. ?H when 1 mol of bonds is broken in the gaseous state
Bond enthalpy
weak acid strong base rxn
methoxy-
-oic acid

31. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Integrated Zero-Order Rate Law
London Dispersion Forces
sublimation
Q<K

32. [A]0/2k
Zero-Order Half Life
perchlorate
catalyst
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

33. AX4
Negative work value; work done by system
k=Ae^(-Ea/RT)
tetrahedral
v3kT/m

34. Energy can't be created nor destroyed
Solvent
Law of Conservation of Energy
Integrated First-Order Rate Law
8.314 J/K mol

35. Electron (symbol)
Colligative properties
analyte
e-
Acid Dissociation Constant

36. # bonding e- - # antibonding e-/2
Bond Order
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Hund's Rule
Polar Covalent

37. Symbol for Total Heat absorbed or released
State Functions
pi=(nRT)/v
analyte
q

38. Cation first - anion second
Naming Binary Ionic Compounds
AH
red
PV=nRT

39. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals

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

40. Higher in energy than the atomic orbitals of which it is composed
hydrocarbons
Alkaline earth metals
Antibonding Molecular Orbital
Naming Binary Ionic Compounds

41. AX3E
blue-green
Law of Definite Proportion
p
trigonal pyramidal

42. Mass #
s (fourth quantum number)
hydro-ic acid
Octahedral
# protons + # neutrons

43. Lowers activation energy
Solution
prop-
Strong acid weak base rxn
catalyst

44. Universal IMF for nonpolar molecules
melting
p+
London dispersion forces
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

45. Elements on staircase on periodic table
+1 - except if bonded to Alkali Metal -1
high pressure - low temperature
trigonal bipyramidal
Metalliods

46. Color of Cs (flame test)
blue
trigonal bipyramidal
d orbitals
alkane

47. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
msAT
Magnetic Quantum Number (ml)
X of a = moles a/total moles
solid CO2

48. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Volume Metric Flask & Pipet
charge
Barometer

49. Change without heat transfer between the system and its surroundings
chlorite
moles of solute/ L of solution
1/2mv²
adiabatic

50. Color of K (flame test)
P1= X1P1°
N=N.(0.5)^time/time half-life
purple
Volt