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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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1. Heat needed to change 1 g of substance to 1°C
zero
Allotrope
N=N.(0.5)^time/time half-life
specific heat

2. Molecules' tendency to stick to one another
Specific Heat (s)
cohesion
First-Order Rate Law
Hydrogen bonding

3. Substances that form H+ when dissolved in water; proton donors
d
Acids
Colligative properties
blue-green

4. Universal IMF for nonpolar molecules
London dispersion forces
actual yield/theoretical yield x 100%
STP
Q<K

5. How to Find an Empirical Formula Given Percentages
t-shape
oxalate
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Covalently w/in themselves - Ionicly bonded w/ each other

6. 1/[A]=kt + 1/[A]0
red
-one
Integrated Second-Order Rate Law
AE= AH - RTAn

7. Tools NEEDED for dilution
Volume Metric Flask & Pipet
octahedral
adhesion
Isotopes

8. Temperature-pressure point after which gas can no longer form liquid
critical point
Bronsted-Lowry Acid
p+
Dalton's Law of Partial Pressures

9. Pure metal or metal hydride + H20 ->
1 atm = 760 mmHg = 101.3 kPa
base and hydrogen gas
increasing
Valence Electrons(assigned)

10. Increase Volume
Increase Temperature
Decrease Volume and Increase Temperature
g solute/g solvent x 100
Calorimetry

11. Only contains ions that change in reaction
Counterions
1atm=?Pa
Net Ionic Equation
are

12. Experimental yield/theoretical yieldx100
Bronsted-Lowry base
% yield
wavelength
soluble

13. Heat capacity formula
solid CO2
C=(mass)(specific heat)
Hybridization
analyte

14. Equation to find Ea from reaction rate constants at two different temperatures
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
end point
log[H+]
rate gas A/rate gas B = square root (mm A/ mm B)

15. (N) number of equivalents per liter of solution
Normality
Integrated Zero-Order Rate Law
double bond
mol

16. Ionizes to produce OH- Ions
lambda
Arrhenius Base
Acid + Base --> Salt + Water
Quantum Mechanical Model

17. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Trigonal Bipyramidal
Valence Electrons(assigned)
a precipitate forms
Equilibrium Expression

18. [A]0/2k
Zero-Order Half Life
Normality
blue-violet
1 atm = 760 mmHg = 101.3 kPa

19. STP
0 degrees C - 1 atm
Metalliods
Atmospheric Pressure
single bond

20. Oxidation # of Compounds
oxalate
0
T-shape
Strong acid weak base rxn

21. Within a sublevel - place one e? per orbital before pairing them

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22. E?s fill the lowest energy orbital first - then work their way up
dec-
moles solute/kg solvent
Matter
Aufbau Principle

23. Expresses how the concentrations depend on time
Standard Temperature and Pressure
London dispersion forces
Cell Potential (Ecell)
Integrated Rate Law

24. Point at which vapor pressure=air pressure above
pi=(nRT)/v
Electron Spin Quantum Number
boiling point
Bonding Pairs

25. Speed per molecule of gas
freezing
zero
v3kT/m
Law of Conservation of Energy

26. Ecell= E°cell -RT/nF x lnQ
moles of solute/ L of solution
Nernst Equation
carbohydrates
Van't Hoff factor

27. (organics) four carbons
but-
Hund's Rule
hex-
Open System

28. (organics) nine carbons
reduction agent
non-
London dispersion forces
Integrated First-Order Rate Law

29. AX5
N=N.(0.5)^time/time half-life
red
nitrite
trigonal bipyramidal

30. S²?
oxide
Effusion
m (third quantum number)
sulfide

31. (A) - C/s
Adding
C=(mass)(specific heat)
Ampere
cyanide

32. Composition Formula
Molar Mass of Element/ Total Molar Mass %
% yield
Quantum Numbers
v3kT/m

33. kf of water
System
insoluble
Solution
1.86°C

34. NO3¹?
Nernst Equation
complex ions
oxide
nitrate

35. The mixing of native atomic orbitals to form special orbitals for bonding
Bond Order
Barometer
Hybridization
s (fourth quantum number)

36. r=k
X of a = moles a/total moles
mol Fraction
Zero-Order Rate Law
-oate

37. CN¹?
octahedral
3/2RT
bromate
cyanide

38. Ideal Gas Law Formula
Principal Quantum Number
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
PV=nRT
Surroundings

39. Mol/L - concentration of a solution
cathode
Molecular Orbitals (MOs)
a precipitate forms
Molarity

40. ClO2¹?
Faraday
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Solute
chlorite

41. AX5
Arrhenius acid
pi=(nRT)/v
group
trigonal bipyramidal

42. Energy required to break a bond
adhesion
wavelength
Bond Energy
-2 - with peroxide -1

43. 96 -485 C/mol e-
Osmotic Pressure
Faraday
Standard Temperature and Pressure
X of a = moles a/total moles

44. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
hydrolysis
Cg=kPg
d orbitals
Chemical Kinetics

45. Coffee Cup Calorimeter
triple bond
carbonate
Constant Pressure
q/moles

46. Boltzmann constant - used in calculating speed of gas per molecule
1.38x10?²³J/K
Valence Electrons(assigned)
0.0826Latm/Kmol
Decrease Volume and Increase Temperature

47. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
endothermic
oxide
Molecular
Quantum Mechanical Model

48. OH¹?
alkyne
k=Ae^(-Ea/RT)
hydroxide
1/2mv²

49. High-speed electrons
End Point
octahedral
Beta Particles-
First-Order Half Life

50. Symbol for Total Heat absorbed or released
Solute
log[H+]
q
Ideal Gas Law