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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. In covalent bonds - prefixes are used to tell...
permanent gases
Principal Quantum Number
Amount of atoms present
hex-

2. The heat changed in a chemical reaction.
1.38x10?²³J/K
Thermochemistry
methoxy-
Linear

3. Forward rxn occurs when
linear
heat capacity
alcohol
Q<K

4. Amount of product produced when limiting reactant is used up
electron affinity
Theoretical yield
nitrate
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

5. 1 sigma bond - 1 pi bond
double bond
Open System
Overall Reaction Order
green/yellow

6. R in instances that pertain to energy
Q<K
Chemical Kinetics
Weight
8.314 J/K mol

7. Symbol for Enthalpy
diamagnetic
Counterions
H
Atomic Mass Unit

8. AX2 - AX2E3
purple --> pink
entropy (S)
Bonding Pairs
linear

9. Mass percent
entropy (S)
supercritical fluid
g solute/g solvent x 100
Constant Pressure

10. Moles of solute/volume of soln(L)
fusion
Solubility Product (Ksp)
Molarity
tetrahedral

11. All cations are soluble with bromide - chloride and iodide EXCEPT
3/2RT
hept-
Entropy (S)
Ag+ - Pb2+ - Hg2+

12. Molarity (M)
moles of solute/ L of solution
Alpha Particles-
?Hvap
soluble

13. An equilibrium expression
Solubility Product (Ksp)
C=(mass)(specific heat)
group
voltaic cells

14. 2+ charge
condensation
bent
Osmotic Pressure
Alpha Particles-

15. kb of water
0.512°C
Arrhenius Acid
T-shape
Root Mean Square Velocity

16. Newton's Second Law
Force = mass x acceleration
melting
blue-green
PV=nRT

17. H+ Acceptor
Bond enthalpy
electrolyte
Bronsted-Lowry Base
Finding Empirical Formulas

18. Variable for type of orbital
l (second quantum number)
d orbitals
Trigonal Planar
Amino-

19. Oxidation # of Halogens
Radioactivity
sulfide
-1
heat of fusion

20. l=2
d
Trigonal Bipyramidal
Q<K
Open System

21. 6.022x10^23
mol
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
-ous acid
Its element

22. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
see-saw
p
Cg=kPg
phosphate - sulfide - carbonate - sulfate

23. AX3E2
-one
cyanide
adiabatic
t-shape

24. Change without heat transfer between the system and its surroundings
hex-
0
Principal Quantum Number
adiabatic

25. The actual amount of product produced in an experiment
experimental yield
amine
Alpha Particles-
excess reactant

26. Idea Gas Law (actual rules)
System
seesaw
Molar Heat Capacity
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

27. F¹?
Hess's Law
third
flouride
effects of IMF

28. Instrument used to measure the pressure of atmospheric gas
Enthalpy of Solution
Barometer
square pyramidal
freezing

29. Mol/kg of solvent - used in calculating colligative properties
period
Ampere
Molality
permanganate

30. Molecules' tendency to stick to the container
Angular Momentum Quantum Number
adhesion
are not
exothermic

31. Amine prefix
Decrease Volume and Increase Temperature
Pauli Exclusion Principle
sulfate
Amino-

32. When n=5 ->2 - color=
blue-violet
8.314 J/K mol
Bond Order
q/moles

33. S²?
conjugate base
ether
trigonal pyramidal
sulfide

34. Substances w/ critical temperatures below 25°C
Gamma Ray-
melting point
deposition
permanent gases

35. A device in which chemical energy is changed to electrical energy
electrolyte
activation energy
-al
Galvanic Cell

36. The chemical formed when a base accepts a proton
charge
g solute/g solvent x 100
rate gas A/rate gas B = square root (mm A/ mm B)
conjugate acid

37. Faraday's constant
linear
Alkali metals
chloride
96500

38. MnO4¹?
Covalently w/in themselves - Ionicly bonded w/ each other
p orbitals
permanganate
Dipole-dipole forces

39. NO2¹?
nitrite
Hydrogen bonding
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Bond enthalpy

40. Lowers activation energy
strong acid strong base rxn
vaporization
catalyst
insoluble

41. Organic w/ -NH2
high pressure - low temperature
phosphate
Boltzmann distribution
amine

42. Average speed of gas
v3RT/M(in kg)
Heat Capacity (C)
Molality
Heat

43. Point at which vapor pressure=air pressure above
reduction agent
actual yield/theoretical yield x 100%
boiling point
Angular Momentum Quantum Number

44. Kinetic Energy per mol
Second-Order Rate Law
Formal Charge
3/2RT
strong acids

45. How to Balance a Redox Equation
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
s orbitals
g solute/g solvent x 100
Calorimetry

46. Boiling point - melting point - viscosity - vapor pressure - surface tension
analyte
End Point
Surroundings
effects of IMF

47. ... compounds are most conductive
96500
ionic
trigonal bipyramidal
Graham's Law

48. The total entropy is always increasing - all systems tend towards maximum entropy
2nd law of thermodynamics
red
strong acid strong base rxn
Covalently w/in themselves - Ionicly bonded w/ each other

49. Describe various properties of one orbital
London dispersion forces
Integrated First-Order Rate Law
oxidizing agent
Quantum Numbers

50. H + donor
carbohydrates
Tetrahedral
Bronsted-Lowry Acid
q

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AP Chemistry

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