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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. Universal IMF for nonpolar molecules
-(P)(Change in V)
bond energy
Monoprotic
London dispersion forces
2. Point at which vapor pressure=air pressure above
Isotopes
precipitate
Sigma Bond
boiling point
3. A molecule having a center of positive charge and a center of negative charge
?Tb= kb x molality
sublimation
Dipole Moment
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
4. AX2E - AX2E2
bent
meth-
?Tb= kb x molality
nitrate
5. Determined by the formula h/m(in kg)v - (v=velocity)
Decrease Volume and Increase Temperature
Integrated Second-Order Rate Law
wavelength
C=(mass)(specific heat)
6. Boiling point elevation formula
?Tb= kb x molality
are
LeChatelier's Principle
Bond enthalpy
7. #NAME?
Standard Temperature and Pressure
E
Scientific Method
Heat Capacity (C)
8. Releases/gives off heat (negative value)
Exothermic
octahedral
square pyramidal
-al
9. 1/[A]=kt + 1/[A]0
Integrated Second-Order Rate Law
methods of increasing rate
trigonal bipyramidal
Specific Heat Capacity
10. If anion ends in -ite - acid name ends in...
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
-ous acid
% yield
Molarity
11. 1 sigma bond - 1 pi bond
double bond
seesaw
conjugate base
standard solution
12. 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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13. 6.022x10^23
mol
A Roman numeral
Acid + Base --> Salt + Water
First-Order Rate Law
14. .69/k
First-Order Half Life
trigonal bipyramidal
Amino-
A Roman numeral
15. In covalent bonds - prefixes are used to tell...
hydrocarbons
Amount of atoms present
Oxidation is Loss Reduction is Gain
Ligand
16. l=3
conjugate acid
Oxidation is Loss Reduction is Gain
f
deposition
17. NO3¹?
cyanide
sublimation
Second-Order Half Life
nitrate
18. High-energy light
Gamma Ray-
Speed of light
ionic
e-
19. Oxidation # of Halogens
critical point
Atomic Mass Unit
A Roman numeral
-1
20. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
Hydrogen bonding
Alkali metals
supercritical fluid
21. ClO4¹?
catalyst
are
vapor pressure
perchlorate
22. Chemical composition of dry ice
(moles of products that are gasses) - (moles of reactants that are gasses)
solid CO2
alcohol
Closed System
23. Raising heat - adding catalyst - heighten concentration - bigger surface area
AH
M = square root (3RT/mm)
methods of increasing rate
Dipole Moment
24. A measure of randomness or disorder
titrant buret
entropy
alkyne
linear
25. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
endothermic
Manometer
Sigma Bond
Work
26. ?Hsoln=?H1+?H2+?H3+...
Enthalpy of Solution
activation energy
Law of Multiple Proportions
Limiting reactant
27. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Molecular Orbitals (MOs)
Temperature
heat capacity
Magnetic Quantum Number (ml)
28. CO3²?
deposition
carbonate
Molal BP Elevation Constant
1atm=?Pa
29. Kinetic Energy of an individual particle formula
M = square root (3RT/mm)
msAT
Calorimetry
purple --> pink
30. 90°&120° - dsp^3
Standard Temperature and Pressure
eth-
Trigonal Bipyramidal
Bases
31. AX3E
trigonal pyramidal
Quantum Mechanical Model
equivalence point
Entropy (S)
32. Weakest IMFs - found in all molecules
dec-
Joule
London dispersion forces
% yield
33. Measure of the average kinetic energy of all the particles in a substance
State Functions
Temperature
vaporization
heat capacity
34. SO3²?
8.314 J/K mol
equilibrium
hex-
sulfite
35. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
soluble
LE Model
alkene
Dalton's Law of Partial Pressures
36. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Dalton's Law
Quantum Model
sulfide
excess reactant
37. q H2O = ?
Specific Heat (s)
msAT
1 atm = 760 mmHg = 101.3 kPa
Theoretical yield
38. Expresses how the concentrations depend on time
Integrated Rate Law
charge
hydroxide
0.0826Latm/Kmol
39. Molecules' tendency to stick to one another
bent
weak acid strong base rxn
van't Hoff Factor
cohesion
40. E=mc^2
p orbitals
0
0
Theory of Relativity
41. kb of water
Equilibrium constant
0.512°C
Theory of Relativity
m (third quantum number)
42. r=k
Equilibrium constant
Zero-Order Rate Law
standard solution
-2 - with peroxide -1
43. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Molecular Compounds
exothermic
LE Model
London Dispersion Forces
44. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Molar Heat Capacity
strong acids
Molecular Compounds
precipitate
45. Heat capacity formula
C=(mass)(specific heat)
-ic acid
P1= X1P1°
Integrated First-Order Rate Law
46. x can be ignored when % ionization is <5%
Arrhenius Acid
5% rule
indicator
Electronegativity
47. H?+NH3?NH4
p
Strong acid weak base rxn
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
First-Order Rate Law
48. Amine prefix
Amino-
isothermal
Specific Heat (s)
Molal FP Depression Constant
49. Color of Ca (flame test)
red/orange
solid CO2
Decrease Volume and Increase Temperature
Acid + Base --> Salt + Water
50. Mols A/ total mols - XA
Integrated Second-Order Rate Law
mol Fraction
methoxy-
Surroundings