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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. Color of Ca (flame test)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
6.63x10?³4Js
purple --> pink
red/orange
2. Kinetic Energy per molecule
1/2mv²
Pressure of H2O must be Subtracted
s orbitals
period
3. 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)
system
Density
d
Kinetic Molecular Theory - for ideal gases
4. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
trigonal bipyramidal
carbonate
triple bond
5. Anions or cations as needed to produce a compound with non net charge
Counterions
Cell Potential (Ecell)
Nodes
entropy (S)
6. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Equilibrium Expression
group
bond energy
oct-
7. negative ion
Anion
Galvanic Cell
H
supercritical fluid
8. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
rate gas A/rate gas B = square root (mm A/ mm B)
State Functions
Oxidizing Agent
phosphate - sulfide - carbonate - sulfate
9. Heat needed to change 1 g of substance to 1°C
H
specific heat
-al
Arrhenius acid
10. Boiling point elevation formula
Arrhenius base
?Tb= kb x molality
Thermochemistry
hydrolysis
11. Symbol for Total Heat absorbed or released
entropy
dichromate
Counterions
q
12. Puts OH? into solution
Hydrogen bonding
Arrhenius base
experimental yield
Molarity
13. Cation first - anion second
work
trigonal planar
Arrhenius Acid
Naming Binary Ionic Compounds
14. Positive enthalpy - heat flows into system
Counterions
endless
Positive work value; work done on system
endothermic
15. I=moles of particles/moles of solute dissolved
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183
16. A measure of randomness or disorder
increasing
entropy
Quantum Mechanical Model
nitrite
17. Average Kinetic Energy Formula
p
first
amine
Average KE = 1/2(mass)(average speed of all particles)
18. Variable for spin of electron (+.5 or -.5)
Finding Empirical Formulas
s (fourth quantum number)
Kinetic Molecular Theory - for ideal gases
Atmospheric Pressure
19. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
Ag+ - Pb2+ - Hg2+
violet
square pyramidal
20. (N) number of equivalents per liter of solution
?Hvap
red/orange
Normality
Molarity
21. Wavelength symbol
lambda
Joule
0
Kinetic Molecular Theory - for ideal gases
22. Temperature-pressure point after which gas can no longer form liquid
second
(moles of products that are gasses) - (moles of reactants that are gasses)
critical point
dec-
23. PO4³?
phosphate
-one
deposition
Net Ionic Equation
24. AX5E
Integrated Second-Order Rate Law
A Roman numeral
square pyramidal
(moles of products that are gasses) - (moles of reactants that are gasses)
25. Significant Digits of Conversion Factors
Theoretical yield
endless
Resonance
Electron Spin Quantum Number
26. Oxidation # of Oxygen
critical point
Bronsted-Lowry Base
-2 - with peroxide -1
1atm=?Pa
27. The reactant in the reduction reaction that forces the oxidation reaction to occur
Chemical Kinetics
Oxidizing Agent
force x distance = work done
fusion
28. Freezing point depression formula
adiabatic
cyanide
meth-
?Tf= kf x molality
29. Significant Digits of counted things
Kinetic Molecular Theory - for ideal gases
Diffusion
permanganate
endless
30. Oxidation # of Hydrogen
Decrease Volume and Increase Temperature
+1 - except if bonded to Alkali Metal -1
Dipole Moment
Arrhenius acid
31. All _________ compounds are electrolytes
Ionic
0.0826Latm/Kmol
methoxy-
Its root and adding -ide
32. Phase change from solid to gas
Law of Multiple Proportions
deposition
sublimation
6.63x10?³4Js
33. C=2.9979*10^8 m/s
Speed of light
increasing
p+
Electronegativity
34. AX3E2
a precipitate forms
see-saw
T-shape
-ous acid
35. The total energy of the universe is constant - all systems tend towards minimum energy
Ionic Compounds
Bond Energy
insoluble
1st law of thermodynamics
36. Energy needed to break a bond
trigonal bipyramidal
Equilibrium Expression
3/2RT
bond energy
37. Solution used in titration
bond energy
1.38x10?²³J/K
Equilibrium constant
titrant buret
38. l=2
Arrhenius base
chromate
Negative work value; work done by system
d
39. AX5E
Covalently w/in themselves - Ionicly bonded w/ each other
oxidation
phosphate
square pyramidal
40. Elements in groups 3-12
Transition metals
acid
Integrated Rate Law
Electron Spin Quantum Number
41. Weakest IMFs - found in all molecules
ionic
Hybridization
London dispersion forces
Heat
42. The weighted average of all the isotopes that an atom can have (in g/mol)
octahedral
Integrated Zero-Order Rate Law
precipitate
Atomic Mass Unit
43. Color of Li (flame test)
0 degrees C - 1 atm
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
green/yellow
red
44. For significant digits - leading zeros ____ significant
Pauli Exclusion Principle
are not
v3kT/m
N=N.(0.5)^time/time half-life
45. Describe various properties of one orbital
moles solute/kg solvent
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Arrhenius Base
Quantum Numbers
46. Passage of gas through tiny orifice
Temperature
charge
Effusion
bent
47. Organic w/ -OH group
red
London dispersion forces
ionic
alcohol
48. Force acting over distance
Weight
actual yield/theoretical yield x 100%
Work
but-
49. Donates a single H+ Ion (... other prefixes also)
eth-
meth-
Monoprotic
e-
50. Melting
fusion
deposition
-(P)(Change in V)
Law of Conservation of Energy