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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. Happens at lines in phase change charts
Amino-
Hess's Law
Molecule
equilibrium

2. R=
Specific Heat (s)
Isotopes
0.0826Latm/Kmol
g solute/g solvent x 100

3. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
prop-
Electron Spin Quantum Number
Hund's Rule

4. Organic w/ -NH2
trigonal planar
Mass
amine
Solute

5. Elements which have all electrons paired and relatively unaffected by magnetic fields
k=Ae^(-Ea/RT)
diamagnetic
mol
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

6. Different form of same element
0
allotrope
Constant Volume
double bond

7. If needed - indicate charge of metal(cation) by...
A Roman numeral
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Molecular Compounds
Acid Dissociation Constant

8. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
excess reactant
strong acids
Oxidizing Agent
Law of Definite Proportion

9. Calculation from K to C
C + 273
analyte
Zero-Order Half Life
Atomic Mass Unit

10. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
rate
reduction
violet
State Functions

11. Only contains ions that change in reaction
high pressure - low temperature
Buffered Solution
Net Ionic Equation
Principal Quantum Number

12. Osmotic pressure formula
Dipole-dipole forces
pi=(nRT)/v
square pyramidal
Finding Empirical Formulas

13. Solid to liquid
Angular Momentum Quantum Number
Molecular Orbitals (MOs)
melting
base and hydrogen gas

14. Cation first - anion second
Weight
-(P)(Change in V)
iodide
Naming Binary Ionic Compounds

15. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
1 atm = 760 mmHg = 101.3 kPa
M = square root (3RT/mm)
Manometer
endless

16. ?T=k*m(solute)
geometric isomers
Molal FP Depression Constant
Coordination Compound
complex ions

17. Variable for type of orbital
-ic acid
l (second quantum number)
Antibonding Molecular Orbital
linear

18. The line running between the atoms
Pressure
Sigma Bond
Galvanic Cell
perchlorate

19. A solution used in titrations whose concentration is known
fusion
0.512°C
Pressure
standard solution

20. Mass #
non-
# protons + # neutrons
but-
Arrhenius Base

21. Mass percent
period
Ampere
Hund's Rule
g solute/g solvent x 100

22. Negative enthalpy - heat flows into surroundings
exothermic
End Point
Graham's Law
Dalton's Law of Partial Pressures

23. Variable for orientation of orbital (-1 through +1)
m (third quantum number)
condensation
Oxidation is Loss Reduction is Gain
Van't Hoff factor

24. A molecule having a center of positive charge and a center of negative charge
critical point
base and hydrogen gas
Finding Empirical Formulas
Dipole Moment

25. The chemical formed when a base accepts a proton
nu
conjugate acid
reduction
Speed of light

26. Symbol for Total Heat absorbed or released
Molal FP Depression Constant
methoxy-
q
Bronsted-Lowry base

27. (N) number of equivalents per liter of solution
Normality
geometric isomers
mol
-oic acid

28. Ideal Gas Law Formula
oxidation
p orbitals
wavelength
PV=nRT

29. Matter can't be created nor destroyed
Molar Mass of Element/ Total Molar Mass %
Law of Conservation of Mass
endless
nitrate

30. When gas expands ...
v3RT/M(in kg)
96500
Negative work value; work done by system
Alkali metals

31. 1 sigma bond - 1 pi bond
3.0x108m/s
red
M = square root (3RT/mm)
double bond

32. l=2
d
blue
conjugate acid
Alkali metals

33. Color of Na (flame test)
Polar Covalent
yellow
Oxidation is Loss Reduction is Gain
force x distance = work done

34. Point where acid completely neutralizes base
equivalence point
Isotopes
alkyne
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

35. Forward rxn occurs when
Q<K
rate gas A/rate gas B = square root (mm A/ mm B)
precipitate
London dispersion forces

36. Substance being dissolved in a solution (lower [ ])
Integrated Zero-Order Rate Law
System
chlorate
Solute

37. Polyatomic Ions (bonding)
Dalton's Law
cyanide
Covalently w/in themselves - Ionicly bonded w/ each other
Volume Metric Flask & Pipet

38. A solution that resists a change in pH - contains both a weak acid and its conjugate base
p orbitals
Open System
endless
Buffer

39. 109.5° - sp^3
square pyramidal
Tetrahedral
van't Hoff Factor
P1= X1P1°

40. Half-life equation
Quantum Numbers
Q<K
Faraday
N=N.(0.5)^time/time half-life

41. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
Quantum Model
Second-Order Rate Law
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

42. Change in Energy = ? (in terms of constant pressure; for gasses)
activation energy
Magnetic Quantum Number (ml)
AE= AH - RTAn
boiling point

43. A device in which chemical energy is changed to electrical energy
Amount of atoms present
Galvanic Cell
Alkali metals
Scientific Method

44. AX6
prop-
Hydrogen bonding
octahedral
?Tb= kb x molality

45. NO3¹?
activation energy
solid CO2
nitrate
Increase Temperature

46. Ester suffix
Acids
Integrated First-Order Rate Law
-oate
activation energy

47. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Ligand
Hund's Rule
Solubility Product (Ksp)
Formal Charge

48. U(rms)=(3RT/M)^1/2
Root Mean Square Velocity
different # of neutrons
iodide
oxidizing agent

49. Carboxylic acid ending
not spontaneous
Pauli Exclusion Principle
1 atm
-oic acid

50. (organics) triple-bonded compound
s orbitals
STP
alkyne
1.38x10?²³J/K