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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. Carboxylic acid ending
condensation
oxidation
-oic acid
paramagnetic

2. K
Valence Electrons(assigned)
Manometer
?Tb= kb x molality
Equilibrium constant

3. Amount of heat needed to change a system by 1°C
zero
heat capacity
1st law of thermodynamics
deposition

4. (organics) one carbon
Molality
rate gas A/rate gas B = square root (mm A/ mm B)
titrant buret
meth-

5. Ptotal=P1+P2+P3+...

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6. frequency symbol
Ampere
nu
weak acid strong base rxn
n (first quantum number)

7. If anion ends in -ate - acid name ends in...
perchlorate
-ic acid
deposition
System

8. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Law of Conservation of Mass
Reducing Agent
Second-Order Half Life
Temperature

9. ln[A] vs. time is a ...-order reaction
first
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
q
Q<K

10. Only contains ions that change in reaction
Manometer
Buffer
Radioactivity
Net Ionic Equation

11. Volume of gas @STP
Alpha Particles-
Effusion
22.4L
conjugate base

12. 90° - d^2sp^3
Octahedral
PV=nRT
boiling point
green/yellow

13. l=0
s
2nd law of thermodynamics
Normality
t-shape

14. 109.5° - sp^3
Specific Heat (s)
AE= AH - RTAn
supercritical fluid
Tetrahedral

15. Ideal Gas Law Formula
% error
hydro-ic acid
PV=nRT
Balmer Series

16. Color of Cs (flame test)
blue
22.4L
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Ideal Gas Law

17. Coffee Cup Calorimeter
Effusion
titrant buret
Constant Pressure
M1V1=M2V2

18. IMF that occurs with FON
Hydrogen bonding
Hund's Rule
5% rule
Second-Order Half Life

19. A measure of randomness or disorder
Tetrahedral
equilibrium
entropy
1/2mv²

20. Diatomic Molecules
red
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
electron affinity
dichromate

21. Mixing of gases
-(P)(Change in V)
Diffusion
Zero-Order Rate Law
prop-

22. #NAME?
Trigonal Planar
E
Formal Charge
chloride

23. AX3E2
s orbitals
square pyramidal
Law of Multiple Proportions
T-shape

24. The total energy of the universe is constant - all systems tend towards minimum energy
1st law of thermodynamics
Arrhenius Acid
bent
dichromate

25. Formula used when diluting stock solution (to find amount of water or stock needed)
chlorate
M1V1=M2V2
Ampere
Bronsted-Lowry Base

26. (organics) six carbons
Dipole Moment
Quantum Numbers
hex-
Radioactivity

27. As protons are added to the nucleus - electrons are similarly added
3/2RT
Pressure
1.38x10?²³J/K
Aufbau Principle

28. (N) number of equivalents per liter of solution
tetrahedral
Bond Order
Normality
Surroundings

29. Instrument used to measure the pressure of atmospheric gas
heat of vaporization
Integrated Zero-Order Rate Law
Barometer
d

30. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change

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31. SO3²?
green/yellow
p orbitals
reduction
sulfite

32. =vM2/M1
Law of Definite Proportion
Quantum Model
r1/r2
red

33. The rest of the universe (in thermodynamics)
Arrhenius acid
surroundings
dec-
adiabatic

34. Symbol for Total Heat absorbed or released
q
Cathode
Hydrogen bonding
London dispersion forces

35. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
AE= AH - RTAn
activation energy
red
hydrolysis

36. How to Balance a Redox Equation
methoxy-
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
Allotrope
hydroxide

37. Electrons in a hydrogen atom move around the nucleus only in circular orbits
End Point
E
-(P)(Change in V)
Quantum Model

38. These orbitals are diagonal
d orbitals
Kinetic Molecular Theory - for ideal gases
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
% error

39. Amount of product produced when limiting reactant is used up
condensation
Theoretical yield
yellow --> green
a precipitate forms

40. Newton's Second Law
vapor pressure
London dispersion forces
2nd law of thermodynamics
Force = mass x acceleration

41. ln[A]=-kt + ln[A]0
Principal Quantum Number
Integrated First-Order Rate Law
Antibonding Molecular Orbital
1.86°C

42. SO4²?
Arrhenius Base
sulfate
freezing
Linear

43. Anions or cations as needed to produce a compound with non net charge
Hydrogen bonding
Counterions
l (second quantum number)
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

44. 760mmHg/Torr
acid
hex-
titrant buret
1atm=?mmHg/Torr

45. CrO4²?
chromate
strong bases
mol
analyte

46. Type of system in which the energy may escape - but the mass is conserved
Overall Reaction Order
Transition metals
different # of neutrons
Closed System

47. 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)
3.0x108m/s
trigonal pyramidal
Ionic Compounds
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

48. Each orbital can hold two e?s each w/ opposite spins
Endothermic
fusion
Pauli Exclusion Principle
Isotopes

49. Color of Ba (flame test)
1.86°C
green/yellow
Law of Conservation of Mass
Increase Temperature

50. A monoatomic anion is named by taking...
Exothermic
Its root and adding -ide
hept-
n (first quantum number)