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Test your basic knowledge |
AP Chemistry
Start Test
Study First
Subjects
:
science
,
ap
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
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study here
.
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. Kinetic Energy of an individual particle formula
s (fourth quantum number)
M = square root (3RT/mm)
8.314 J/K mol
yellow
2. H?+NH3?NH4
specific heat
Molal FP Depression Constant
p orbitals
Strong acid weak base rxn
3. 90°&120° - dsp^3
Ideal Gas Law
Trigonal Bipyramidal
s
Boltzmann distribution
4. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Resonance
sulfate
Zero-Order Rate Law
Bronsted-Lowry Acid
5. Energy needed to vaporize a mole of a liquid
?Hvap
Molecule
nu
methoxy-
6. Oxidation # of Halogens
-1
heat of fusion
paramagnetic
Adding
7. q H2O = ?
msAT
q/moles
p
X of a = moles a/total moles
8. The actual amount of product produced in an experiment
Antibonding Molecular Orbital
Naming Binary Ionic Compounds
experimental yield
0
9. Happens at lines in phase change charts
Integrated Second-Order Rate Law
equilibrium
lambda
tetrahedral
10. As protons are added to the nucleus - electrons are similarly added
Aufbau Principle
Transition metals
Reaction Quotient (Q)
# protons + # neutrons
11. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
ammonium
Hydrogen bonding
alkyne
End Point
12. Rate of Diffusion/Effusion formula
Average KE = 1/2(mass)(average speed of all particles)
square planar
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Enthalpy of Solution
13. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
rate law
not spontaneous
Standard Temperature and Pressure
trigonal bipyramidal
14. If Q<Ksp
Bronsted-Lowry Acid
System
triple point
no precipitate forms
15. Variable for spin of electron (+.5 or -.5)
equilibrium
q/moles
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
s (fourth quantum number)
16. [A] vs. time is a ...-order reaction
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
zero
1st law of thermodynamics
red
17. Polyatomic Ions (bonding)
perchlorate
Covalently w/in themselves - Ionicly bonded w/ each other
deposition
Bonding Pairs
18. Oxoacid solution (such as HSO4-) forms...
Alkaline earth metals
Quantum Numbers
blue
oxide gas and water
19. AX3E
H
trigonal pyramidal
Aufbau Principle
square planar
20. An equilibrium expression
methods of increasing rate
Solubility Product (Ksp)
-one
vapor pressure
21. Raoult's Law - relations between vapor pressure and concentrations
Acids
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
P1= X1P1°
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
22. Atoms with the same number of protons but a different number of neutrons
moles solute/kg solvent
l (second quantum number)
blue
Isotopes
23. R in ideal gas law
Root Mean Square Velocity
Heat Capacity (C)
0.0821 atm L/mol K
Constant Pressure
24. Oxidation # of Hydrogen
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
# protons + # neutrons
p
+1 - except if bonded to Alkali Metal -1
25. The measurement of heat changes
Law of Multiple Proportions
Calorimetry
Cation
Percent Yield
26. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
pent-
Amount of atoms present
chlorate
27. Melting
-(P)(Change in V)
fusion
-one
but-
28. Energy involved in gaining an electron to become a negative ion
electron affinity
p
alkyne
Metalliods
29. A weak acid that changes color at or near the equivalence point
spontaneous
precipitate
oxide gas and water
indicator
30. 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
trigonal bipyramidal
Manometer
blue-violet
supercritical fluid
31. Mols A/ total mols - XA
carbonate
deposition
mol Fraction
Net Ionic Equation
32. In a given atom no two electrons can have the same set of four quantum numbers
Angular Momentum Quantum Number
Pauli Exclusion Principle
dec-
msAT
33. Pairs of electrons localized on an atom
like
Lone Pair
% yield
Resonance
34. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
Polar Covalent
double bond
Hydrogen bonding
35. Similar to atomic orbitals - except between molecules
Molecular Orbitals (MOs)
sulfide
square pyramidal
Effusion
36. Unit of electrical potential; J/C
Volt
Linear
moles of solute/ L of solution
chloride
37. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
Anode
freezing
Buffer
38. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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39. Heat needed to change 1 g of substance to 1°C
not spontaneous
Equivalence Point
specific heat
see-saw
40. l=1
0
Reducing Agent
p
Hess's Law
41. Theoretical yield-experimental yield/theoretical yieldx100
% error
solid CO2
5% rule
0
42. H?+OH??H2O
Atomic Mass Unit
activation energy
strong acid strong base rxn
indicator
43. Wavelength symbol
Monoprotic
0.512°C
lambda
Bases
44. Mol of solute/kg of solvent
endless
Molality
Graham's Law
square pyramidal
45. Increase Volume
wavelength
sublimation
endothermic
Increase Temperature
46. SO3²?
conjugate base
AE= AH - RTAn
sulfite
bromate
47. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
Calorimeter
eth-
log[H+]
spontaneous
48. Loss of electrons - increase in oxidation #
LE Model
oxidation
Thermochemistry
First-Order Rate Law
49. Solid to gas
Chemical Bonds
sublimation
Cell Potential (Ecell)
Aufbau Principle
50. These orbitals are diagonal
Theoretical yield
d orbitals
London dispersion forces
Delta H or Enthalpy Change
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