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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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1. Formula used when diluting stock solution (to find amount of water or stock needed)
square pyramidal
M1V1=M2V2
actual yield/theoretical yield x 100%
salt bridge

2. Energy required to break a bond
Bond Energy
excess reactant
Acid + Base --> Salt + Water
Bronsted-Lowry base

3. What is defined by you taken from the whole universe
System
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
indicator
T-shape

4. Actual Yield/Theoretical Yield*100%
charge
Joule
Bronsted-Lowry acid
Percent Yield

5. Higher in energy than the atomic orbitals of which it is composed
Heat Capacity (C)
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Cg=kPg
Antibonding Molecular Orbital

6. Cl¹?
chloride
force x distance = work done
Calorimetry
Molecular Orbitals (MOs)

7. Color of Li (flame test)
strong acid strong base rxn
red
conjugate acid
X of a = moles a/total moles

8. Different form of same element
London dispersion forces
allotrope
-ic acid
actual yield/theoretical yield x 100%

9. H?+NH3?NH4
Negative work value; work done by system
Bronsted-Lowry acid
Hydrogen bonding
Strong acid weak base rxn

10. If anion ends in -ate - acid name ends in...
permanent gases
First-Order Half Life
-ic acid
22.4L

11. (organics) nine carbons
Aufbau Principle
excess reactant
non-
conjugate acid

12. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
Balmer Series
Exothermic
fusion

13. Color of Ca (flame test)
red/orange
Alkali metals
melting
Bonding Pairs

14. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
insoluble
electrolyte
flouride
Pauli Exclusion Principle

15. kf of water
insoluble
1.86°C
Isotopes
-ic acid

16. H+ Acceptor
Buffered Solution
Bronsted-Lowry Base
Constant Pressure
Resonance

17. Atoms combine in fixed whole # ratios
LE Model
rate law
high pressure - low temperature
Law of Multiple Proportions

18. Metal oxide + H20 ->
methoxy-
Anion
Molecular
base

19. Diatomic Molecules
Cg=kPg
AE= AH - RTAn
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
X of a = moles a/total moles

20. (organics) three carbons
2nd law of thermodynamics
period
P1= X1P1°
prop-

21. 101 -325 Pa
different # of neutrons
square planar
1atm=?Pa
supercritical fluid

22. AX3
LE Model
trigonal planar
s (fourth quantum number)
eth-

23. How to Balance a Redox Equation
heat of fusion
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
Chemical Bonds
Quantum Numbers

24. The actual amount of product produced in an experiment
Sigma Bond
insoluble
experimental yield
adiabatic

25. The chemical formed when an acid donates a proton
8.31J/Kmol
conjugate base
permanganate
-one

26. PV=nRT
Q<K
Ideal Gas Law
Molecular Compounds
triple point

27. Energy required for liquid?gas
electron affinity
rate
heat of vaporization
?Hvap

28. For significant digits - trailing zeros _____ significant
Thermochemistry
v3RT/M(in kg)
bent
are

29. 760mmHg/Torr
geometric isomers
bond energy
Molecular
1atm=?mmHg/Torr

30. Reverse rxn occurs when
system
carbonate
1 atm = 760 mmHg = 101.3 kPa
Q>K

31. Where there are no electrons
Nodes
square planar
0.512°C
Specific Heat (s)

32. R=
8.31J/Kmol
Weight
supercritical fluid
Surroundings

33. Ionizes to produce H+ ions
iodide
purple --> pink
Open System
Arrhenius Acid

34. Average speed of gas
Magnetic Quantum Number (ml)
Arrhenius Base
Closed System
v3RT/M(in kg)

35. Two molecules with identical connectivity but different geometries
p
geometric isomers
blue-violet
Bronsted-Lowry Acid

36. AX5
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
zero
adiabatic
trigonal bipyramidal

37. Molarity (M)
AE= AH - RTAn
?Hvap
moles of solute/ L of solution
are

38. 90° - d^2sp^3
oxide gas and water
C=(mass)(specific heat)
Octahedral
Bronsted-Lowry base

39. Driving force of the electrons
Cell Potential (Ecell)
mol
1st law of thermodynamics
Polar Covalent

40. The total entropy is always increasing - all systems tend towards maximum entropy
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
alkyne
-ic acid
2nd law of thermodynamics

41. U(rms)=(3RT/M)^1/2
Polar Covalent
Integrated First-Order Rate Law
0.512°C
Root Mean Square Velocity

42. Electrons in a hydrogen atom move around the nucleus only in circular orbits
v3kT/m
Barometer
Quantum Model
Average KE = 1/2(mass)(average speed of all particles)

43. Energy (definition)
phosphate
force x distance = work done
rate law
+1 - except if bonded to Alkali Metal -1

44. Moles of solute/volume of soln(L)
Effusion
Bond Energy
Molarity
vapor pressure

45. Heat required to raise the system 1°C
oxide
n (first quantum number)
Dalton's Law of Partial Pressures
heat capacity

46. An equilibrium expression
+1 - except if bonded to Alkali Metal -1
supercritical fluid
charge
Solubility Product (Ksp)

47. Variable for spin of electron (+.5 or -.5)
Heat Capacity (C)
supercritical fluid
AE= AH - RTAn
s (fourth quantum number)

48. SI unit of energy; Kg*m^2/s^2
pi=(nRT)/v
H
entropy (S)
Joule

49. Puts H? into solution
dichromate
0
Arrhenius acid
tetrahedral

50. Solution in flask being titrated
Dalton's Law
sulfate
1.38x10?²³J/K
analyte

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AP Chemistry

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