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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. Oxidation # of Ions
Atomic Mass Unit
+1 - except if bonded to Alkali Metal -1
1 atm = 760 mmHg = 101.3 kPa
charge

2. Measure of the average kinetic energy of all the particles in a substance
System
Temperature
3rd law of thermodynamics
v3RT/M(in kg)

3. The measurement of heat changes
Calorimetry
square pyramidal
Electron Spin Quantum Number
Decrease Volume and Increase Temperature

4. Where reduction occurs
but-
Cg=kPg
Specific Heat Capacity
Cathode

5. Connects the 2 half cells in a voltaic cell
salt bridge
cathode
q
r1/r2

6. Electron pairs found in the space between the atoms
Bonding Pairs
X of a = moles a/total moles
sulfate
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

7. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Polar Covalent
insoluble
ammonium
Bond enthalpy

8. A given compound always has exactly the same proportion of elements by mass
4.184
s orbitals
Dalton's Law of Partial Pressures
Law of Definite Proportion

9. ClO3²?
strong acids
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
Metalliods
chlorate

10. ... compounds are most conductive
ionic
complex ions
yellow --> green
% yield

11. Only contains ions that change in reaction
Net Ionic Equation
activated complex (transition state)
Amount of atoms present
-(q of H2O + q of cal)

12. Substances that form OH- when dissolved in water; proton acceptors
force x distance = work done
Bases
3.0x108m/s
a precipitate forms

13. Ionizes to produce H+ ions
msAT
P1= X1P1°
salt bridge
Arrhenius Acid

14. Significant Digits of Conversion Factors
allotrope
reduction agent
Law of Multiple Proportions
endless

15. When n=4 ->2 - color=
Pauli Exclusion Principle
octahedral
Pressure
blue-green

16. Formula used when diluting stock solution (to find amount of water or stock needed)
Standard Temperature and Pressure
Equilibrium Expression
M1V1=M2V2
boiling point

17. Osmotic pressure formula
square planar
acetate
pi=(nRT)/v
not spontaneous

18. All cations are soluble with sulfate EXCEPT
weak acid strong base rxn
equivalence point
Reaction Quotient (Q)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

19. # bonding e- - # antibonding e-/2
Bond Order
Radioactivity
Calorimeter
Integrated Second-Order Rate Law

20. Organic w/ -O-
ether
Solution
Equivalence Point
Alkali metals

21. #NAME?
chlorate
Molar Mass of Element/ Total Molar Mass %
triple bond
E

22. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
End Point
Osmotic Pressure
X of a = moles a/total moles
LE Model

23. (organics) four carbons
but-
Electron Spin Quantum Number
Integrated Zero-Order Rate Law
Second-Order Rate Law

24. Metal oxide + H20 ->
trigonal planar
First-Order Rate Law
Angular Momentum Quantum Number
base

25. Change that occurs at constant temperature
isothermal
AE= AH - RTAn
Amino-
Bronsted-Lowry Base

26. The total energy of the universe is constant - all systems tend towards minimum energy
Buffered Solution
hydro-ic acid
allotrope
1st law of thermodynamics

27. Energy involved in gaining an electron to become a negative ion
weak acid strong base rxn
electron affinity
Arrhenius base
Buffered Solution

28. n+m (these are orders of reactants)
violet
Overall Reaction Order
Equilibrium Expression
Hydrogen bonding

29. Anything occupying space and with mass
Matter
Temperature
triple point
AE = q + w

30. Average speed of gas
v3RT/M(in kg)
catalyst
second
Bond Energy

31. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
supercritical fluid
entropy
Equivalence Point
Faraday

32. 109.5° - sp^3
Tetrahedral
Bronsted-Lowry Acid
Law of Conservation of Mass
different # of neutrons

33. (organics) double-bonded compound
Adding
r1/r2
isothermal
alkene

34. Freezing point depression formula
Open System
Arrhenius acid
solid CO2
?Tf= kf x molality

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

36. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Zero-Order Half Life
red/orange
Ionic Compounds
Dipole-dipole forces

37. Isotope
Acids
different # of neutrons
red/orange
melting

38. Point where acid completely neutralizes base
Cg=kPg
analyte
equivalence point
indicator

39. Verticals on the periodic table
group
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
London dispersion forces
Radioactivity

40. Faraday's constant
Galvanic Cell
96500
Buffer
Hund's Rule

41. Electron (symbol)
Antibonding Molecular Orbital
e-
lambda
Ideal Gas Law

42. Oxidation # of Compounds
0
Bronsted-Lowry Acid
3/2RT
Dalton's Law of Partial Pressures

43. IMF that occurs with FON
Hydrogen bonding
are not
Cathode
Hund's Rule

44. Speed per molecule of gas
0.0821 atm L/mol K
Beta Particles-
3/2RT
v3kT/m

45. Boltzmann constant - used in calculating speed of gas per molecule
LeChatelier's Principle
1.38x10?²³J/K
3rd law of thermodynamics
heat of vaporization

46. Weakest IMFs - found in all molecules
moles of solute/ L of solution
conjugate acid
sublimation
London dispersion forces

47. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
Buffer
Pauli Exclusion Principle
f

48. AX3
specific heat
trigonal planar
1/2mv²
Negative work value; work done by system

49. q cal = ?
precipitate
CAT
excess reactant
solid CO2

50. Theoretical yield-experimental yield/theoretical yieldx100
double bond
% error
Amphoteric
wavelength