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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. 0.00°C - 1 atm
boiling point
Equivalence Point
Standard Temperature and Pressure
Finding Empirical Formulas
2. Matter can't be created nor destroyed
critical point
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Law of Conservation of Mass
3. Electron pairs found in the space between the atoms
Bonding Pairs
mol
chloride
London Dispersion Forces
4. A monoatomic cation takes name from...
Its element
Integrated First-Order Rate Law
Law of Definite Proportion
Enthalpy of Solution
5. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
t-shape
Dalton's Law
Cg=kPg
yellow --> green
6. Amine prefix
Amino-
Alpha Particles-
P of a =(X of a)(total pressure)
Dipole Moment
7. 120° - sp^2
96500
Molecular Compounds
8.31J/Kmol
Trigonal Planar
8. 6.022x10^23
soluble
mol
r1/r2
oct-
9. E?s fill the lowest energy orbital first - then work their way up
-oate
Aufbau Principle
ammonium
Pauli Exclusion Principle
10. Mass/volume
Isolated System
k=Ae^(-Ea/RT)
Density
carbonate
11. 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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12. Gain of electrons - decrease in oxidation #
Allotrope
reduction
N=N.(0.5)^time/time half-life
Law of Conservation of Mass
13. Atomic #
Pi Bond
g solute/g solvent x 100
# protons (atom is defined by this)
(moles of products that are gasses) - (moles of reactants that are gasses)
14. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Equivalence Point
Theory of Relativity
Amount of atoms present
Colligative properties
15. Significant Digits of counted things
strong bases
iodide
Cathode
endless
16. A solution that resists a change in pH - contains both a weak acid and its conjugate base
ammonium
Bonding Pairs
Ampere
Buffer
17. H?+NH3?NH4
Equivalence Point
Strong acid weak base rxn
geometric isomers
g solute/g solvent x 100
18. Driving force of the electrons
p
?Tb= kb x molality
endless
Cell Potential (Ecell)
19. When ____ significant digits - round answer to least decimal place
methoxy-
Adding
Entropy (S)
?Hvap
20. Spectrum of light when an electron drops to energy level n=2
electron affinity
spontaneity
Quantum Mechanical Model
Balmer Series
21. 90° - d^2sp^3
Octahedral
square pyramidal
weak acid strong base rxn
% error
22. Elements which have all electrons paired and relatively unaffected by magnetic fields
diamagnetic
geometric isomers
dichromate
q
23. AX6
Boltzmann distribution
octahedral
trigonal bipyramidal
0 degrees C - 1 atm
24. Boiling point - melting point - viscosity - vapor pressure - surface tension
STP
chromate
Volt
effects of IMF
25. (organics) double-bonded compound
red/orange
alkene
acetate
msAT
26. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
pi=(nRT)/v
Thermochemistry
Finding Empirical Formulas
boiling point
27. H+ Acceptor
trigonal pyramidal
zero
vaporization
Bronsted-Lowry Base
28. Larger molecules which have higher mass and therefore electron density have stronger...
London dispersion forces
entropy
Matter
Molecular
29. Faraday's constant
red/orange
experimental yield
96500
1.38x10?²³J/K
30. The rest of the universe (in thermodynamics)
insoluble
surroundings
moles of solute/ L of solution
0.512°C
31. pH=
LE Model
log[H+]
force x distance = work done
Metalliods
32. The reactant in the reduction reaction that forces the oxidation reaction to occur
Open System
base and hydrogen gas
Alkali metals
Oxidizing Agent
33. Theoretical yield-experimental yield/theoretical yieldx100
melting
% error
isothermal
Finding Empirical Formulas
34. Temperature-pressure combination at which solid - liquid - and gas states appear
Cg=kPg
triple point
critical point
Law of Conservation of Mass
35. Mol/kg of solvent - used in calculating colligative properties
Speed of light
Molality
Quantum Mechanical Model
System
36. Rate of Diffusion/Effusion formula
Specific Heat (s)
heat of fusion
Cation
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
37. Carbon & hydrogen compounds
3.0x108m/s
octahedral
hydrocarbons
Effusion
38. % yield
actual yield/theoretical yield x 100%
Acid Dissociation Constant
Nernst Equation
PV=nRT
39. A device used to measure Delta H
sublimation
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Calorimeter
fusion
40. Heat capacity formula
soluble
C=(mass)(specific heat)
Colligative properties
endless
41. Oxoacid solution (such as HSO4-) forms...
oxide gas and water
0.0821 atm L/mol K
heat of vaporization
Aufbau Principle
42. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
strong acids
P of a =(X of a)(total pressure)
excess reactant
1.38x10?²³J/K
43. 760mmHg/Torr
Equilibrium Expression
Pauli Exclusion Principle
1atm=?mmHg/Torr
Density
44. 180° - sp
Linear
log[H+]
Equilibrium Expression
ionic
45. Variable for type of orbital
-one
nu
dichromate
l (second quantum number)
46. Puts OH? into solution
Arrhenius base
l (second quantum number)
lambda
entropy (S)
47. Molecules' tendency to stick to one another
Valence Electrons(assigned)
0.0826Latm/Kmol
voltaic cells
cohesion
48. Everything in the universe that is not defined by you as part of the system
s
Buffer
Solute
Surroundings
49. Connects the 2 half cells in a voltaic cell
conjugate acid
salt bridge
electron affinity
third
50. Molecules' tendency to stick to the container
rate gas A/rate gas B = square root (mm A/ mm B)
London dispersion forces
insoluble
adhesion