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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. A device in which chemical energy is changed to electrical energy
Galvanic Cell
-ic acid
chlorite
e-
2. Ketone suffix
hept-
Gamma Ray-
k=Ae^(-Ea/RT)
-one
3. Organic w/ -NH2
amine
Constant Pressure
AE= AH - RTAn
are
4. Ability of an atom in a molecule to attract shared electrons to itself
exothermic
Molar Mass of Element/ Total Molar Mass %
Electronegativity
phosphate
5. 2 or more covalently bonded atoms
deposition
Molecule
excess reactant
Normality
6. Gain of electrons - decrease in oxidation #
reduction
8.314 J/K mol
4.184
Nodes
7. Delta H (AH) = ?
different # of neutrons
q/moles
Speed of light
trigonal bipyramidal
8. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Pauli Exclusion Principle
paramagnetic
yellow --> green
freezing
9. Different form of same element
Root Mean Square Velocity
allotrope
alkene
v3kT/m
10. Mass percent
weak acid strong base rxn
Density
Molecule
g solute/g solvent x 100
11. Oxidation # of Oxygen
sulfide
-2 - with peroxide -1
Q>K
zero
12. Increase Pressure
l (second quantum number)
Molar Heat Capacity
Decrease Volume and Increase Temperature
Law of Conservation of Mass
13. If needed - indicate charge of metal(cation) by...
spontaneity
single bond
A Roman numeral
Cell Potential (Ecell)
14. 1 sigma bond - 2 pi bonds
triple bond
oxidizing agent
First-Order Rate Law
nu
15. H+ Acceptor
Bronsted-Lowry Base
f
spontaneous
Alkali metals
16. [A]=-kt + [A]0
Delta H or Enthalpy Change
Second-Order Rate Law
Integrated Zero-Order Rate Law
Constant Volume
17. Mass #
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
# protons + # neutrons
alcohol
cathode
18. % yield
analyte
actual yield/theoretical yield x 100%
Angular Momentum Quantum Number
red
19. Measure of the average kinetic energy of all the particles in a substance
Temperature
red
Molar Heat Capacity
s orbitals
20. Heat required to raise the system 1°C
high pressure - low temperature
supercritical fluid
heat capacity
oxidation
21. Force per unit area
alcohol
X of a = moles a/total moles
Pressure
oxide gas and water
22. Matter can't be created nor destroyed
Law of Conservation of Mass
Van't Hoff factor
soluble
adhesion
23. When n=4 ->2 - color=
heat capacity
blue-green
charge
0.0826Latm/Kmol
24. 109.5° - sp^3
Tetrahedral
Specific Heat Capacity
Molality
van't Hoff Factor
25. =vM2/M1
Ionic
solid CO2
r1/r2
Molecular Orbitals (MOs)
26. 1 sigma bond - 1 pi bond
double bond
A Roman numeral
isothermal
dichromate
27. A solution that resists a change in its pH
heat capacity
Buffered Solution
Solution
cyanide
28. Where oxidation occurs
square pyramidal
Arrhenius acid
yellow --> green
Anode
29. 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
Increase Temperature
green/yellow
Boltzmann distribution
Finding Empirical Formulas
30. High-speed electrons
Temperature
Overall Reaction Order
State Functions
Beta Particles-
31. Universal IMF for nonpolar molecules
System
London dispersion forces
Heat
-ic acid
32. Amount of gravitational force exerted on an object
t-shape
Bond enthalpy
Weight
entropy
33. 1 sigma bond
single bond
melting point
ammonium
but-
34. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
AH
Normality
voltaic cells
red/orange
35. U(rms)=(3RT/M)^1/2
q
hydroxide
Root Mean Square Velocity
experimental yield
36. Describe various properties of one orbital
Overall Reaction Order
Quantum Numbers
Ampere
0 degrees C - 1 atm
37. 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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38. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
cathode
diamagnetic
dichromate
Magnetic Quantum Number (ml)
39. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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40. Similar to atomic orbitals - except between molecules
period
Molecular Orbitals (MOs)
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
oct-
41. 120° - sp^2
Bronsted-Lowry Base
Gamma Ray-
Trigonal Planar
Graham's Law
42. A solid or gas that can be formed when 2 or more aqueous reactants come together
precipitate
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
chloride
hydroxide
43. Proton (symbol)
Normality
Covalently w/in themselves - Ionicly bonded w/ each other
p+
Atomic Mass Unit
44. Cl¹?
flouride
chloride
Constant Pressure
1st law of thermodynamics
45. AX4E2
square planar
Overall Reaction Order
96500
flouride
46. Color of Cs (flame test)
octahedral
l (second quantum number)
blue
Matter
47. ClO4¹?
Molecular Compounds
activation energy
perchlorate
isothermal
48. PV=nRT
paramagnetic
E
Closed System
Ideal Gas Law
49. Metal oxide + H20 ->
base
1 atm = 760 mmHg = 101.3 kPa
Pauli Exclusion Principle
Limiting reactant
50. Driving force of the electrons
Transition metals
Cell Potential (Ecell)
lambda
Barometer