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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. Positive ion
vaporization
Trigonal Bipyramidal
Bond enthalpy
Cation
2. The heat changed in a chemical reaction.
Thermochemistry
Ampere
Gamma Ray-
Atmospheric Pressure
3. A given compound always has exactly the same proportion of elements by mass
-ic acid
Law of Definite Proportion
Arrhenius equation
hept-
4. Peak of energy diagram
Weight
activated complex (transition state)
second
moles solute/kg solvent
5. What is defined by you taken from the whole universe
System
-ous acid
heat capacity
red
6. These orbitals are diagonal
Chemical Bonds
moles of solute/ L of solution
Adding
d orbitals
7. I¹?
Bond Energy
alkyne
iodide
Amino-
8. Substances w/ critical temperatures below 25°C
paramagnetic
Polar Covalent
oxide
permanent gases
9. Point at which solid?liquid occurs
melting point
n0
v3RT/M(in kg)
Monoprotic
10. MnO4¹?
permanganate
catalyst
Cg=kPg
allotrope
11. The amount of energy/heat required to raise some substance 1 degree C
2nd law of thermodynamics
Electronegativity
?Tb= kb x molality
Heat Capacity (C)
12. (organics) three carbons
prop-
Amount of atoms present
oxidizing agent
reduction
13. Solid to gas
sublimation
Pressure
Solute
adiabatic
14. Organic reaction in which two functional groups come together - resulting in the release of water
condensation
s
octahedral
hydro-ic acid
15. AX2E - AX2E2
boiling point
Law of Conservation of Mass
bent
(moles of products that are gasses) - (moles of reactants that are gasses)
16. SI unit of energy; Kg*m^2/s^2
activated complex (transition state)
Molar Heat Capacity
Joule
Isotopes
17. Everything in the universe that is not defined by you as part of the system
Surroundings
Valence Electrons(assigned)
Transition metals
Mass
18. A monoatomic anion is named by taking...
Temperature
Colligative properties
Its root and adding -ide
Resonance
19. Mols A/ total mols - XA
spontaneous
Pauli Exclusion Principle
mol Fraction
endothermic
20. Thickness
Effusion
alkene
Allotrope
viscosity
21. BrO3¹?
bromate
Scientific Method
Law of Conservation of Mass
Mass
22. The driving force for a spontaneous is an increase in entropy of the universe
London dispersion forces
Heisenberg Uncertainty Principle
Entropy (S)
dichromate
23. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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24. Does the same as equilibrium expression - except it uses initial concentrations
Reaction Quotient (Q)
Chemical Kinetics
viscosity
Allotrope
25. Speed per molecule of gas
8.314 J/K mol
Diffusion
v3kT/m
Q<K
26. Mass percent
g solute/g solvent x 100
non-
Covalently w/in themselves - Ionicly bonded w/ each other
Alkaline earth metals
27. AX4E
Integrated First-Order Rate Law
see-saw
Its root and adding -ide
force x distance = work done
28. negative ion
Alkaline earth metals
moles of solute/ L of solution
dichromate
Anion
29. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Mass
0
Work
Valence Electrons(assigned)
30. neutron (symbol)
Positive work value; work done on system
Solubility Product (Ksp)
Arrhenius acid
n0
31. x can be ignored when % ionization is <5%
5% rule
Isotopes
msAT
base and hydrogen gas
32. (organics) five carbons
pent-
d
indicator
green/yellow
33. An equilibrium expression
Solubility Product (Ksp)
red/orange
methoxy-
Mass
34. Amount of gravitational force exerted on an object
Weight
alkyne
endless
Solution
35. S²?
increasing
Bonding Pairs
freezing
sulfide
36. The reactant that is being reduced - brings about oxidation
1/2mv²
oxidizing agent
period
square pyramidal
37. AX3E2
insoluble
Arrhenius base
oxidation
t-shape
38. E?s fill the lowest energy orbital first - then work their way up
electron affinity
C=(mass)(specific heat)
Aufbau Principle
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
39. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
2nd law of thermodynamics
a precipitate forms
salt bridge
40. Lowers activation energy
acid
endothermic
catalyst
equilibrium
41. Temperature-pressure point after which gas can no longer form liquid
high pressure - low temperature
critical point
rate
-ous acid
42. Nonmetal oxide + H2O ->
acid
trigonal planar
# protons (atom is defined by this)
spontaneity
43. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Acids
Acid + Base --> Salt + Water
allotrope
Nodes
44. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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45. Substance in which something is dissolved in a solution (higher [ ])
Oxidizing Agent
strong acid strong base rxn
Delta H or Enthalpy Change
Solvent
46. Within a sublevel - place one e? per orbital before pairing them
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47. Type of system in which the energy and mass may leave or enter
chromate
Counterions
Endothermic
Open System
48. Ionizes to produce H+ ions
Specific Heat Capacity
square planar
paramagnetic
Arrhenius Acid
49. ?Hsoln=?H1+?H2+?H3+...
Molarity
Enthalpy of Solution
Pressure
Speed of light
50. A solution that resists a change in its pH
Buffered Solution
Hess's Law
Quantum Mechanical Model
freezing