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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. Consists of a complex ion - a transition metal with attached ligands - and counterions
0
Delta H or Enthalpy Change
Coordination Compound
q

2. Ionizes to produce OH- Ions
Zero-Order Rate Law
Arrhenius Base
red
endothermic

3. STP
phosphate - sulfide - carbonate - sulfate
Equilibrium Expression
96500
0 degrees C - 1 atm

4. Ketone suffix
Aufbau Principle
excess reactant
-one
Cg=kPg

5. AX3E2
Integrated Second-Order Rate Law
violet
T-shape
flouride

6. r=k[A]^2
Finding Empirical Formulas
bent
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Second-Order Rate Law

7. 760mmHg/Torr
iodide
Zero-Order Rate Law
1atm=?mmHg/Torr
t-shape

8. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
AE= AH - RTAn
hydrolysis
p
Polar Covalent

9. Proton acceptors - must have an unshared pair of e?s
Its element
nu
Bronsted-Lowry base
Bonding Pairs

10. When gas expands ...
Heisenberg Uncertainty Principle
Negative work value; work done by system
hept-
London dispersion forces

11. The weighted average of all the isotopes that an atom can have (in g/mol)
Isolated System
Atomic Mass Unit
Bond Order
moles of solute/ L of solution

12. A measure of resistance of an object to a change in its state of motion
reduction agent
Mass
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Zero-Order Half Life

13. 6.022x10^23
Manometer
mol
1 atm = 760 mmHg = 101.3 kPa
LeChatelier's Principle

14. Electrons in a hydrogen atom move around the nucleus only in circular orbits
base and hydrogen gas
Graham's Law
Quantum Model
1 atm

15. Energy needed to vaporize a mole of a liquid
hydrocarbons
1.86°C
permanent gases
?Hvap

16. Temperature-pressure combination at which solid - liquid - and gas states appear
triple point
London dispersion forces
red
Effusion

17. NH4¹?
Normality
ammonium
-2 - with peroxide -1
AH

18. Gas to liquid
Chemical Kinetics
C + 273
alkene
condensation

19. Chemical composition of dry ice
solid CO2
end point
0.512°C
Acid Dissociation Constant

20. (organics) two carbons
weak acid strong base rxn
Entropy (S)
eth-
Q>K

21. #NAME?
E
exothermic
Magnetic Quantum Number (ml)
oxidation

22. pH=
log[H+]
Graham's Law
Van't Hoff factor
nitrite

23. ClO3²?
zero
Oxidation is Loss Reduction is Gain
chlorate
Quantum Numbers

24. Metal oxide + H20 ->
Law of Multiple Proportions
spontaneity
like
base

25. Half-life equation
Work
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
sulfate
N=N.(0.5)^time/time half-life

26. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
Coordination Compound
pi=(nRT)/v
third

27. Moles of solute/volume of soln(L)
Molarity
Integrated Zero-Order Rate Law
endless
log[H+]

28. SO3²?
Integrated Second-Order Rate Law
endothermic
1 atm = 760 mmHg = 101.3 kPa
sulfite

29. Equation to find Ea from reaction rate constants at two different temperatures
Osmotic Pressure
Temperature
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
E

30. All cations are soluble with sulfate EXCEPT
Speed of light
Effusion
Galvanic Cell
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

31. Atomic #
T-shape
octahedral
Sigma Bond
# protons (atom is defined by this)

32. AX4
Increase Temperature
Temperature
tetrahedral
X of a = moles a/total moles

33. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
effects of IMF
Acid + Base --> Salt + Water
Principal Quantum Number
Zero-Order Half Life

34. The actual amount of product produced in an experiment
Effusion
Trigonal Planar
Molecular
experimental yield

35. Kinetic Energy per molecule
1/2mv²
heat of vaporization
viscosity
entropy

36. Unit of electrical potential; J/C
Solvent
pent-
viscosity
Volt

37. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
charge
spontaneity
Formal Charge
complex ions

38. Pure metal or metal hydride + H20 ->
base and hydrogen gas
cyanide
C + 273
square planar

39. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Allotrope
Hund's Rule
Entropy (S)
LE Model

40. Forward rxn occurs when
second
Q<K
deposition
double bond

41. Solid to gas
n0
sulfate
sublimation
Bond enthalpy

42. Spontaneous emission of radiation
Radioactivity
are not
Ligand
-ic acid

43. K
-ol
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Equilibrium constant
endless

44. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Decrease Volume and Increase Temperature
Equivalence Point
Acid + Base --> Salt + Water
oxalate

45. When _____ significant digits - round answer to least significant digit
Multiplying
Solvent
diamagnetic
Equilibrium Expression

46. Energy can't be created nor destroyed
Law of Conservation of Energy
spontaneous
Increase Temperature
Oxidation is Loss Reduction is Gain

47. Loss of electrons - increase in oxidation #
oxidation
Cathode
chlorite
1atm=?mmHg/Torr

48. Variable for energy of e- - goes from 1 -2 -3 on up
double bond
n (first quantum number)
CAT
permanganate

49. Ester suffix
bond energy
-oate
-ic acid
red/orange

50. Tools NEEDED for dilution
activated complex (transition state)
condensation
Pressure of H2O must be Subtracted
Volume Metric Flask & Pipet