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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. C=2.9979*10^8 m/s
Cation
third
Net Ionic Equation
Speed of light
2. A homogeneous mixture with 1 phase
surroundings
-oate
third
Solution
3. Matter can't be created nor destroyed
carbonate
p+
Cation
Law of Conservation of Mass
4. High-speed electrons
Beta Particles-
dichromate
Molar Heat Capacity
reduction agent
5. Point at which the titrated solution changes color
critical point
chlorate
end point
8.314 J/K mol
6. Tools NEEDED for dilution
Antibonding Molecular Orbital
Volume Metric Flask & Pipet
Work
Heisenberg Uncertainty Principle
7. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Constant Pressure
Electronegativity
critical point
strong acids
8. q cal = ?
CAT
base and hydrogen gas
ammonium
Increase Temperature
9. Where there are no electrons
reduction agent
Nodes
Dipole-dipole forces
oxidation
10. Variable for orientation of orbital (-1 through +1)
hydrolysis
m (third quantum number)
Law of Multiple Proportions
yellow --> green
11. Driving force of the electrons
Cell Potential (Ecell)
acetate
carbonate
Bronsted-Lowry base
12. #NAME?
Hess's Law
n0
E
isothermal
13. AX5
sulfite
trigonal bipyramidal
conjugate acid
Reducing Agent
14. ?T=k*m(solute)
Arrhenius Acid
Molal BP Elevation Constant
P1V1/N1T1=P2V2/N2T2
weak acid strong base rxn
15. Anions or cations as needed to produce a compound with non net charge
Cathode
v3RT/M(in kg)
nitrate
Counterions
16. Kinetic Energy per mol
3/2RT
octahedral
Allotrope
trigonal bipyramidal
17. Oxidation # of Polyatomic Ions
charge
Speed of light
Equilibrium Expression
Pauli Exclusion Principle
18. 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
Bond Order
base
Finding Empirical Formulas
Reducing Agent
19. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
1 atm = 760 mmHg = 101.3 kPa
rate
zero
Q>K
20. Has values 1 -2 -3 -...; tells energy levels
Principal Quantum Number
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
LeChatelier's Principle
p orbitals
21. Cl¹?
Molarity
chloride
triple bond
Boltzmann distribution
22. J/°Cg or J/Kg
-ol
perchlorate
Specific Heat Capacity
Heat Capacity (C)
23. We cannot simultaneously determine an atom's exact path or location
0.0821 atm L/mol K
Temperature
First-Order Rate Law
Heisenberg Uncertainty Principle
24. Organic w/ -O-
ether
red
LE Model
96500
25. Ionizes to produce OH- Ions
Arrhenius Base
n0
bent
Hydrogen bonding
26. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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27. CO3²?
work
carbonate
Hydrogen bonding
boiling point
28. Energy required for liquid?gas
Beta Particles-
2nd law of thermodynamics
chlorate
heat of vaporization
29. Substance being dissolved in a solution (lower [ ])
solid CO2
Solute
melting point
-1
30. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
Molecular Compounds
activated complex (transition state)
Open System
Exothermic
31. r=k[A]^2
Density
Cathode
Second-Order Rate Law
Increase Temperature
32. NO3¹?
nitrate
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Molecular Compounds
Increase Temperature
33. Electron pairs found in the space between the atoms
Heisenberg Uncertainty Principle
group
Bonding Pairs
carbohydrates
34. [A]0/2k
soluble
Zero-Order Half Life
# protons + # neutrons
single bond
35. The minimum energy that molecules must possess for collisions to be effective - Ea
Bronsted-Lowry Base
phosphate - sulfide - carbonate - sulfate
sublimation
activation energy
36. Equation to find Ea from reaction rate constants at two different temperatures
linear
vaporization
P1= X1P1°
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
37. Expresses how the concentrations depend on time
Negative work value; work done by system
End Point
Integrated Rate Law
chlorate
38. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Hund's Rule
vapor pressure
Reducing Agent
msAT
39. Symbol for the heat absorbed or lost molecularly (PER MOLE)
hydro-ic acid
group
Work
AH
40. Half cell in which reduction occurs
8.314 J/K mol
Dalton's Law of Partial Pressures
cathode
Endothermic
41. Color of Ba (flame test)
trigonal bipyramidal
Anode
green/yellow
insoluble
42. BrO3¹?
spontaneity
n (first quantum number)
Alpha Particles-
bromate
43. When _____ significant digits - round answer to least significant digit
Pi Bond
condensation
triple bond
Multiplying
44. Absorbs/takes in heat (positive value)
1st law of thermodynamics
Endothermic
Galvanic Cell
Integrated Zero-Order Rate Law
45. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
hydrolysis
t-shape
Nernst Equation
0
46. Actual Yield/Theoretical Yield*100%
Percent Yield
specific heat
End Point
s (fourth quantum number)
47. Point at which solid?liquid occurs
alkene
increasing
melting point
0
48. Different form of same element
Bonding Pairs
allotrope
but-
London dispersion forces
49. A measure of randomness or disorder
square pyramidal
P of a =(X of a)(total pressure)
yellow --> green
entropy
50. (organics) triple-bonded compound
insoluble
actual yield/theoretical yield x 100%
sulfide
alkyne
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