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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. Amount of heat needed to change a system by 1°C
specific heat
heat capacity
Bronsted-Lowry acid
Trigonal Bipyramidal

2. Hydroxides are soluble or insoluble?
-ous acid
carbonate
insoluble
Tetrahedral

3. Organic w/ -NH2
amine
s
high pressure - low temperature
blue

4. Expresses how the concentrations depend on time
Cation
triple bond
Integrated Rate Law
Kinetic Molecular Theory - for ideal gases

5. Color of Li (flame test)
Standard Temperature and Pressure
-oate
red
0

6. Boiling point - melting point - viscosity - vapor pressure - surface tension
effects of IMF
carbohydrates
Endothermic
flouride

7. Mass #
Electronegativity
s (fourth quantum number)
# protons + # neutrons
analyte

8. CN¹?
amine
oxide gas and water
cyanide
precipitate

9. Chemical composition of dry ice
solid CO2
% error
adhesion
cathode

10. AX4
Chemical Kinetics
tetrahedral
1/2mv²
paramagnetic

11. If Q>Ksp
Solubility Product (Ksp)
a precipitate forms
Cg=kPg
Specific Heat Capacity

12. (organics) two carbons
Negative work value; work done by system
Bond Order
eth-
Bonding Pairs

13. Passage of gas through tiny orifice
endless
Effusion
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
Law of Multiple Proportions

14. 96 -485 C/mol e-
Open System
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Boltzmann distribution
Faraday

15. Experimental yield/theoretical yieldx100
% yield
Tetrahedral
rate gas A/rate gas B = square root (mm A/ mm B)
Law of Definite Proportion

16. Gain of electrons - decrease in oxidation #
1.38x10?²³J/K
reduction
Cg=kPg
Nernst Equation

17. Variable for orientation of orbital (-1 through +1)
m (third quantum number)
strong acid strong base rxn
1.38x10?²³J/K
Speed of light

18. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
octahedral
Heisenberg Uncertainty Principle
complex ions
Molecular

19. AP doesn't deal with ...-order reaction - don't pick it!
Monoprotic
third
Electronegativity
Reaction Quotient (Q)

20. R in instances that pertain to energy
square planar
Integrated First-Order Rate Law
Chemical Bonds
8.314 J/K mol

21. Mole Fraction
Arrhenius Base
X of a = moles a/total moles
work
1st law of thermodynamics

22. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Acid + Base --> Salt + Water
condensation
supercritical fluid
Polar Covalent

23. Point at which vapor pressure=air pressure above
critical point
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
boiling point
charge

24. Spectrum of light when an electron drops to energy level n=2
trigonal pyramidal
Thermochemistry
wavelength
Balmer Series

25. Osmotic pressure formula
Law of Conservation of Energy
third
pi=(nRT)/v
l (second quantum number)

26. q cal = ?
Endothermic
Molarity
Equilibrium constant
CAT

27. [A]0/2k
-one
Zero-Order Half Life
Scientific Method
sublimation

28. Substances that form H+ when dissolved in water; proton donors
Valence Electrons(assigned)
Percent Yield
high pressure - low temperature
Acids

29. Releases/gives off heat (negative value)
Antibonding Molecular Orbital
AH
heat of vaporization
Exothermic

30. Like dissolves...
like
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Solute
q

31. Half cell in which oxidation occurs
Principal Quantum Number
anode
zero
96500

32. BrO3¹?
bromate
Lone Pair
sublimation
chromate

33. # bonding e- - # antibonding e-/2
trigonal bipyramidal
Molar Mass of Element/ Total Molar Mass %
Bond Order
Reaction Quotient (Q)

34. The likelihood that a rxn will occur "by itself"
spontaneity
Bases
Alpha Particles-
seesaw

35. Newton's Second Law
tetrahedral
Force = mass x acceleration
Theoretical yield
Hydrogen bonding

36. Formula used when diluting stock solution (to find amount of water or stock needed)
Closed System
d orbitals
Thermochemistry
M1V1=M2V2

37. Energy needed to break a bond
adhesion
bond energy
lambda
CAT

38. Oxidation # of Ions
charge
r1/r2
3rd law of thermodynamics
Matter

39. Energy (definition)
Reducing Agent
force x distance = work done
ionic
A Roman numeral

40. l=1
H
p
Solute
P1V1/N1T1=P2V2/N2T2

41. AX3
trigonal planar
sulfite
Radioactivity
0.0826Latm/Kmol

42. Specific heat of water
4.184
Q<K
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
3.0x108m/s

43. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Reaction Quotient (Q)
system
Pauli Exclusion Principle
Quantum Model

44. Point at which the titrated solution changes color
melting point
Normality
end point
-ol

45. Tools NEEDED for dilution
Volume Metric Flask & Pipet
f
Antibonding Molecular Orbital
mol Fraction

46. #NAME?
E
Anion
Dalton's Law of Partial Pressures
Pi Bond

47. Mass/volume
Density
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Molecular Orbitals (MOs)
melting

48. K
p
P of a =(X of a)(total pressure)
Equilibrium constant
n (first quantum number)

49. (# of lone pair e-)+1/2(# of shared e-)
Valence Electrons(assigned)
Van't Hoff factor
t-shape
System

50. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Kinetic Molecular Theory - for ideal gases
ammonium
nitrate
strong acids