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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. PO4³?
Polar Covalent
Radioactivity
phosphate
Atmospheric Pressure
2. Significant Digits of Conversion Factors
Arrhenius base
solid CO2
strong bases
endless
3. Color of Ba (flame test)
moles of solute/ L of solution
acetate
Arrhenius acid
green/yellow
4. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
like
surroundings
Specific Heat (s)
Formal Charge
5. Variable for type of orbital
p+
Pauli Exclusion Principle
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
l (second quantum number)
6. Carbon - hydrogen - oxygen compounds
T-shape
carbohydrates
f
Linear
7. If anion ends in -ate - acid name ends in...
Nernst Equation
square planar
-ic acid
k=Ae^(-Ea/RT)
8. A weak acid that changes color at or near the equivalence point
indicator
q
Percent Yield
red
9. Degree of disorder in a system
Van't Hoff factor
s
E
entropy (S)
10. Chemical composition of dry ice
solid CO2
square planar
C + 273
Temperature
11. Variable for energy of e- - goes from 1 -2 -3 on up
Integrated First-Order Rate Law
n (first quantum number)
Aufbau Principle
Solubility Product (Ksp)
12. 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)
P1= X1P1°
Ionic Compounds
experimental yield
double bond
13. (organics) double-bonded compound
alkene
m (third quantum number)
Beta Particles-
base
14. The reactant that is being oxidized - brings about reduction
?Tf= kf x molality
Integrated First-Order Rate Law
hydroxide
reduction agent
15. (organics) seven carbons
van't Hoff Factor
hept-
Acid Dissociation Constant
London Dispersion Forces
16. Universal IMF for nonpolar molecules
London dispersion forces
ammonium
Law of Definite Proportion
diamagnetic
17. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
indicator
Boltzmann distribution
Law of Definite Proportion
1st law of thermodynamics
18. CrO4²?
AE= AH - RTAn
chromate
Faraday
Hydrogen bonding
19. AX3E2
group
Solution
Bronsted-Lowry acid
t-shape
20. % yield
actual yield/theoretical yield x 100%
Molal BP Elevation Constant
Decrease Volume and Increase Temperature
Ionic Compounds
21. 2 or more covalently bonded atoms
electron affinity
Constant Volume
Acids
Molecule
22. AX3
trigonal planar
% yield
Magnetic Quantum Number (ml)
Bond Energy
23. Isotope
Bronsted-Lowry acid
System
f
different # of neutrons
24. Color of K (flame test)
purple
sublimation
t-shape
Formal Charge
25. Amount of gravitational force exerted on an object
Anion
Weight
critical point
Law of Multiple Proportions
26. Half cell in which reduction occurs
Speed of light
weak acid strong base rxn
96500
cathode
27. Elements in groups 3-12
Speed of light
entropy (S)
Transition metals
deposition
28. HF+ OH??H2O
Chemical Kinetics
weak acid strong base rxn
Quantum Mechanical Model
Magnetic Quantum Number (ml)
29. E=mc^2
electron affinity
alkane
Counterions
Theory of Relativity
30. Puts OH? into solution
Le Chatelier's Principle
Integrated Rate Law
Arrhenius base
# protons + # neutrons
31. Nonmetal oxide + H2O ->
3rd law of thermodynamics
0
deposition
acid
32. The mixing of native atomic orbitals to form special orbitals for bonding
-one
phosphate
purple --> pink
Hybridization
33. Everything in the universe that is not defined by you as part of the system
effects of IMF
Surroundings
Pressure
M = square root (3RT/mm)
34. Combined Gas Law Formula
Equivalence Point
Constant Pressure
Oxidation is Loss Reduction is Gain
P1V1/N1T1=P2V2/N2T2
35. l=3
-ous acid
f
Bond Order
Dalton's Law
36. Mass #
Molar Heat Capacity
Arrhenius base
activation energy
# protons + # neutrons
37. Each orbital can hold two e?s each w/ opposite spins
AH
Pauli Exclusion Principle
State Functions
Hybridization
38. A monoatomic anion is named by taking...
Molecule
Barometer
Oxidizing Agent
Its root and adding -ide
39. Kinetic Energy is proportional to ______
Temperature
Hund's Rule
k=Ae^(-Ea/RT)
violet
40. AX2 - AX2E3
Bond enthalpy
Anode
oct-
linear
41. Arrhenius equation
Integrated Zero-Order Rate Law
+1 - except if bonded to Alkali Metal -1
k=Ae^(-Ea/RT)
ionic
42. We cannot simultaneously determine an atom's exact path or location
Heat
Valence Electrons(assigned)
# protons (atom is defined by this)
Heisenberg Uncertainty Principle
43. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Resonance
square pyramidal
Molecular Compounds
Work
44. PV=nRT
London dispersion forces
Open System
n0
Ideal Gas Law
45. When ____ significant digits - round answer to least decimal place
Adding
Effusion
+1 - except if bonded to Alkali Metal -1
Bonding Pairs
46. r=k[A]^2
nitrate
Pressure of H2O must be Subtracted
Second-Order Rate Law
complex ions
47. Substance being dissolved in a solution (lower [ ])
Solute
purple --> pink
cathode
Quantum Numbers
48. Mixing of gases
Hess's Law
Diffusion
oxalate
p orbitals
49. Point at which the titrated solution changes color
end point
AH
1.38x10?²³J/K
s (fourth quantum number)
50. Heat needed to change 1 g of substance to 1°C
base
specific heat
Specific Heat Capacity
activated complex (transition state)