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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. (organics) three carbons
bromate
prop-
pent-
precipitate
2. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
but-
P1= X1P1°
square pyramidal
3. Determined by the formula h/m(in kg)v - (v=velocity)
C=(mass)(specific heat)
wavelength
viscosity
Aufbau Principle
4. Coffee Cup Calorimeter
geometric isomers
6.63x10?³4Js
Constant Pressure
k=Ae^(-Ea/RT)
5. The driving force for a spontaneous is an increase in entropy of the universe
T-shape
lambda
Molar Mass of Element/ Total Molar Mass %
Entropy (S)
6. ClO4¹?
charge
perchlorate
bromate
Ligand
7. A monoatomic cation takes name from...
adhesion
red/orange
Its element
Negative work value; work done by system
8. (organics) seven carbons
Strong acid weak base rxn
hept-
rate
seesaw
9. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
Atomic Mass Unit
Volume Metric Flask & Pipet
-ic acid
10. Instrument used to measure the pressure of atmospheric gas
3/2RT
C + 273
van't Hoff Factor
Barometer
11. Energy involved in gaining an electron to become a negative ion
electron affinity
melting point
Molal FP Depression Constant
Bond Energy
12. Elements which have unpaired electrons and highly affected by magnetic fields
spontaneous
solid CO2
Molecule
paramagnetic
13. 1 sigma bond - 1 pi bond
soluble
are not
van't Hoff Factor
double bond
14. If anion ends in -ate - acid name ends in...
dec-
-ic acid
C=(mass)(specific heat)
anode
15. The reactant that is being reduced - brings about oxidation
oxidizing agent
Antibonding Molecular Orbital
alkyne
-ol
16. (N) number of equivalents per liter of solution
pi=(nRT)/v
Endothermic
Normality
isothermal
17. How to Find a Weighted Average
+1 - except if bonded to Alkali Metal -1
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Bronsted-Lowry Base
moles solute/kg solvent
18. Moles of solute/volume of soln(L)
system
Arrhenius Acid
Molarity
Molal BP Elevation Constant
19. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
1atm=?Pa
Quantum Mechanical Model
spontaneous
deposition
20. Proton acceptors - must have an unshared pair of e?s
bond energy
rate
endothermic
Bronsted-Lowry base
21. Equation to find Ea from reaction rate constants at two different temperatures
d
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Matter
Cathode
22. Force that holds atoms together
Amount of atoms present
0
Quantum Numbers
Chemical Bonds
23. A weak acid that changes color at or near the equivalence point
indicator
Arrhenius Acid
freezing
Pauli Exclusion Principle
24. x can be ignored when % ionization is <5%
London dispersion forces
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Specific Heat (s)
5% rule
25. Measure of the change in enthalpy
Anode
Delta H or Enthalpy Change
v3kT/m
3/2RT
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
4.184
0.0826Latm/Kmol
Volume Metric Flask & Pipet
Finding Empirical Formulas
27. Group 1 metals
Alkali metals
nitrate
State Functions
acetate
28. Ptotal=P1+P2+P3+...
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29. AX4
LeChatelier's Principle
violet
tetrahedral
methods of increasing rate
30. Amount of product produced when limiting reactant is used up
-(q of H2O + q of cal)
voltaic cells
strong bases
Theoretical yield
31. Color of K (flame test)
purple
nu
k=Ae^(-Ea/RT)
Negative work value; work done by system
32. Color of Ca (flame test)
Principal Quantum Number
sulfate
1atm=?Pa
red/orange
33. (organics) single-bonded compound
Bonding Pairs
moles of solute/ L of solution
M1V1=M2V2
alkane
34. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
Trigonal Bipyramidal
precipitate
mol Fraction
35. E?s fill the lowest energy orbital first - then work their way up
are
Aufbau Principle
Adding
Alpha Particles-
36. F¹?
Principal Quantum Number
Law of Definite Proportion
flouride
Isolated System
37. Nonmetal oxide + H2O ->
Law of Multiple Proportions
violet
1/2mv²
acid
38. Unit of electrical potential; J/C
Second-Order Rate Law
Solute
Volt
Chemical Kinetics
39. R=
-(P)(Change in V)
8.31J/Kmol
N=N.(0.5)^time/time half-life
Exothermic
40. Energy needed to break a bond
Pauli Exclusion Principle
bond energy
P of a =(X of a)(total pressure)
salt bridge
41. R in instances that pertain to energy
condensation
8.314 J/K mol
voltaic cells
% error
42. Speed of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm A/ mm B)
q
period
square pyramidal
43. 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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44. Positive ion
Increase Temperature
Cation
Octahedral
Nodes
45. High-energy light
Weight
oxidation
Gamma Ray-
AE = q + w
46. Involves quantum numbers
Hydrogen bonding
Quantum Mechanical Model
tetrahedral
viscosity
47. I=moles of particles/moles of solute dissolved
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48. Pairs of electrons localized on an atom
Lone Pair
Overall Reaction Order
allotrope
equivalence point
49. 96 -485 C/mol e-
Oxidizing Agent
Faraday
Solvent
Dalton's Law of Partial Pressures
50. Point where acid completely neutralizes base
Bond Energy
equivalence point
insoluble
chloride