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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.
If you are not ready to take this test, you can
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. Experimental yield/theoretical yieldx100
Gamma Ray-
triple bond
Oxidizing Agent
% yield
2. NO3¹?
chloride
nitrate
viscosity
Linear
3. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
Molar Mass of Element/ Total Molar Mass %
hydrolysis
Theoretical yield
trigonal pyramidal
4. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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5. Driving force of the electrons
fusion
Its root and adding -ide
# protons + # neutrons
Cell Potential (Ecell)
6. ln[A]=-kt + ln[A]0
1st law of thermodynamics
Theory of Relativity
surroundings
Integrated First-Order Rate Law
7. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
melting
strong acids
Molar Mass of Element/ Total Molar Mass %
anode
8. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Arrhenius equation
Equilibrium Expression
rate law
red
9. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
Ampere
Second-Order Rate Law
Speed of light
10. Substances w/ critical temperatures below 25°C
Equilibrium Expression
permanent gases
equivalence point
Dalton's Law of Partial Pressures
11. Increase Pressure
0.0821 atm L/mol K
Decrease Volume and Increase Temperature
Sigma Bond
First-Order Rate Law
12. Change in Energy (AE) = ? (in terms of work)
Multiplying
cohesion
AE = q + w
End Point
13. Mixing of gases
Diffusion
Amphoteric
sulfide
# protons + # neutrons
14. Phase change from solid to gas
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
square pyramidal
sublimation
Acids
15. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
phosphate
Resonance
Trigonal Planar
Valence Electrons(assigned)
16. R in ideal gas law
0.0821 atm L/mol K
Solubility Product (Ksp)
rate
a precipitate forms
17. Molarity (M)
moles of solute/ L of solution
boiling point
Trigonal Bipyramidal
k=Ae^(-Ea/RT)
18. Point where acid completely neutralizes base
bent
spontaneity
equivalence point
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
19. Group 2 metals
Alkaline earth metals
Buffered Solution
?Hvap
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
20. Heat needed to change 1 g of substance to 1°C
State Functions
specific heat
Overall Reaction Order
1.38x10?²³J/K
21. Lowers activation energy
d orbitals
catalyst
freezing
Positive work value; work done on system
22. SI unit of energy; Kg*m^2/s^2
Law of Multiple Proportions
Integrated Rate Law
Joule
Constant Pressure
23. Half cell in which reduction occurs
Work
cathode
trigonal bipyramidal
Naming Binary Ionic Compounds
24. A device in which chemical energy is changed to electrical energy
Molal BP Elevation Constant
Galvanic Cell
Hybridization
Q>K
25. Force per unit area
Heat
pi=(nRT)/v
Pressure
Pauli Exclusion Principle
26. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
Amount of atoms present
pent-
Zero-Order Rate Law
27. Bomb Calorimeter
Acids
Naming Binary Ionic Compounds
reduction
Constant Volume
28. Positive enthalpy - heat flows into system
viscosity
Root Mean Square Velocity
endothermic
oxalate
29. 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
0.0821 atm L/mol K
Bond Order
boiling point
30. Gas to solid
Equilibrium constant
London dispersion forces
electron affinity
deposition
31. Osmotic pressure=MRT
conjugate base
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
phosphate
Osmotic Pressure
32. Effusion of a gas is inversely proportional to the square root of the molar mass
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33. When gas expands ...
Dalton's Law
Atmospheric Pressure
pi=(nRT)/v
Negative work value; work done by system
34. When n=5 ->2 - color=
blue-violet
excess reactant
London dispersion forces
paramagnetic
35. Change without heat transfer between the system and its surroundings
Q<K
adiabatic
oxidizing agent
Limiting reactant
36. AX3E
trigonal pyramidal
-1
mol Fraction
Hydrogen bonding
37. What is defined by you taken from the whole universe
1.38x10?²³J/K
Dipole-dipole forces
System
nitrate
38. 760mmHg/Torr
Mass
% error
1atm=?mmHg/Torr
precipitate
39. 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
1 atm
chlorate
supercritical fluid
purple
40. Faraday's constant
strong acids
equivalence point
96500
Work
41. Osmotic pressure formula
Van't Hoff factor
pi=(nRT)/v
2nd law of thermodynamics
third
42. Variable for energy of e- - goes from 1 -2 -3 on up
Trigonal Planar
n (first quantum number)
Closed System
square pyramidal
43. C2O4²?
oxalate
oct-
Chemical Kinetics
Normality
44. H+ Acceptor
Bronsted-Lowry Base
experimental yield
hept-
Alpha Particles-
45. Change that occurs at constant temperature
Entropy (S)
Specific Heat Capacity
PV=nRT
isothermal
46. Reverse rxn occurs when
tetrahedral
eth-
Q>K
Electronegativity
47. AX3
system
trigonal planar
P1= X1P1°
iodide
48. Higher in energy than the atomic orbitals of which it is composed
Antibonding Molecular Orbital
Integrated Rate Law
bond energy
Acid + Base --> Salt + Water
49. Energy needed to break a bond
bond energy
isothermal
q
Pauli Exclusion Principle
50. Involves quantum numbers
8.314 J/K mol
Quantum Mechanical Model
d orbitals
M = square root (3RT/mm)