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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. Molecules' tendency to stick to the container
adhesion
m (third quantum number)
Alkali metals
chlorite

2. 0°C and 1 atm
Specific Heat Capacity
Effusion
Molecular Orbitals (MOs)
STP

3. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
red/orange
are
Exothermic
Ligand

4. Gain of electrons - decrease in oxidation #
reduction
Anode
second
Equivalence Point

5. AX5E
square pyramidal
Bronsted-Lowry base
electron affinity
Monoprotic

6. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
n (first quantum number)
Formal Charge
purple
like

7. The heat changed in a chemical reaction.
Average KE = 1/2(mass)(average speed of all particles)
Thermochemistry
square planar
1 atm = 760 mmHg = 101.3 kPa

8. Organic w/ -OH group
Solubility Product (Ksp)
Bases
alcohol
square pyramidal

9. Volume of gas @STP
22.4L
Specific Heat (s)
Hund's Rule
Aufbau Principle

10. How to Find an Empirical Formula Given Grams
chlorite
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Average KE = 1/2(mass)(average speed of all particles)
a precipitate forms

11. Passage of gas through tiny orifice
M1V1=M2V2
Coordination Compound
Effusion
salt bridge

12. 120° - sp^2
Density
nitrite
diamagnetic
Trigonal Planar

13. Solid to liquid
Oxidation is Loss Reduction is Gain
melting
chlorite
octahedral

14. If anion ends in -ate - acid name ends in...
pent-
base
-ic acid
Second-Order Rate Law

15. Diatomic Molecules
adhesion
n (first quantum number)
entropy
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

16. When gas compresses ...
octahedral
violet
Positive work value; work done on system
flouride

17. Raising heat - adding catalyst - heighten concentration - bigger surface area
critical point
(moles of products that are gasses) - (moles of reactants that are gasses)
triple point
methods of increasing rate

18. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
-ic acid
heat capacity
Atmospheric Pressure
amine

19. In ideal gas law problem - when it says "atmospheric" ...
-oic acid
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Mass
Pressure of H2O must be Subtracted

20. Higher in energy than the atomic orbitals of which it is composed
Electron Spin Quantum Number
oxide
sulfite
Antibonding Molecular Orbital

21. SO3²?
sulfite
Linear
v3RT/M(in kg)
C=(mass)(specific heat)

22. A weak acid that changes color at or near the equivalence point
indicator
force x distance = work done
Negative work value; work done by system
conjugate base

23. Average Kinetic Energy Formula
Zero-Order Rate Law
Oxidizing Agent
methods of increasing rate
Average KE = 1/2(mass)(average speed of all particles)

24. Force acting over distance
strong acid strong base rxn
ether
reduction
Work

25. Substances that form H+ when dissolved in water; proton donors
Polar Covalent
Naming Binary Ionic Compounds
Acids
Density

26. 760mmHg/Torr
indicator
spontaneous
1atm=?mmHg/Torr
m (third quantum number)

27. Symbol for the heat absorbed or lost molecularly (PER MOLE)
Integrated Second-Order Rate Law
Specific Heat Capacity
AH
spontaneity

28. Positive ion
3/2RT
different # of neutrons
strong bases
Cation

29. H+ Acceptor
Bronsted-Lowry Base
Constant Pressure
Ionic
Acids

30. Generally insoluble anions (names)
Strong acid weak base rxn
Integrated Rate Law
oxide gas and water
phosphate - sulfide - carbonate - sulfate

31. Unit of electrical potential; J/C
deposition
E
Volt
Ampere

32. Phase change from solid to gas
Nernst Equation
ether
Molecule
sublimation

33. A device in which chemical energy is changed to electrical energy
Galvanic Cell
Beta Particles-
chromate
M = square root (3RT/mm)

34. Weakest IMFs - found in all molecules
Negative work value; work done by system
ammonium
Adding
London dispersion forces

35. Speed of light - C
3.0x108m/s
entropy (S)
Its element
Radioactivity

36. SI unit of energy; Kg*m^2/s^2
oxidation
Le Chatelier's Principle
Joule
Equilibrium constant

37. Average speed of gas
van't Hoff Factor
f
v3RT/M(in kg)
Manometer

38. OIL RIG
electrolyte
-2 - with peroxide -1
s (fourth quantum number)
Oxidation is Loss Reduction is Gain

39. Non-Ideal Gas Conditions
high pressure - low temperature
Aufbau Principle
end point
p

40. Amount of gravitational force exerted on an object
Weight
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Zero-Order Half Life
Coordination Compound

41. ... compounds are most conductive
ionic
Constant Pressure
cohesion
X of a = moles a/total moles

42. r=k[A]
Alkali metals
First-Order Rate Law
Molecular Compounds
4.184

43. Dalton's Law of Partial Pressures (to find partial pressure formula)
Endothermic
P of a =(X of a)(total pressure)
Molar Heat Capacity
green/yellow

44. Entropy in the universe is always...
square planar
T-shape
increasing
Hydrogen bonding

45. Dirrect Method Formula
Law of Conservation of Mass
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
(moles of products that are gasses) - (moles of reactants that are gasses)
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

46. Elements in groups 3-12
Transition metals
Thermochemistry
Closed System
precipitate

47. q H2O = ?
phosphate - sulfide - carbonate - sulfate
anode
octahedral
msAT

48. Degree of disorder in a system
entropy (S)
dichromate
Lone Pair
London dispersion forces

49. AX6
4.184
octahedral
STP
Scientific Method

50. (A) - C/s
Bronsted-Lowry acid
Polar Covalent
Integrated Second-Order Rate Law
Ampere