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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. Boiling point elevation formula
?Tb= kb x molality
3.0x108m/s
Normality
bromate
2. A method of investigation involving observation and theory to test scientific hypotheses
Scientific Method
First-Order Rate Law
reduction
Closed System
3. 0.00°C - 1 atm
second
Standard Temperature and Pressure
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
dichromate
4. Speed of light - C
3.0x108m/s
Molal FP Depression Constant
allotrope
supercritical fluid
5. Temperature-pressure point after which gas can no longer form liquid
Delta H or Enthalpy Change
1 atm
critical point
Second-Order Half Life
6. Molecules' tendency to stick to one another
cohesion
Boltzmann distribution
strong acids
nitrate
7. Point at which solid?liquid occurs
-ic acid
Second-Order Half Life
AE= AH - RTAn
melting point
8. Generally insoluble anions (names)
vaporization
Finding Empirical Formulas
phosphate - sulfide - carbonate - sulfate
Scientific Method
9. Entropy in the universe is always...
E
PV=nRT
hept-
increasing
10. 2 or more covalently bonded atoms
Amino-
Diffusion
Molecule
Linear
11. Like dissolves...
5% rule
like
Manometer
trigonal bipyramidal
12. Similar to atomic orbitals - except between molecules
viscosity
Molecular Orbitals (MOs)
M1V1=M2V2
alkyne
13. Color of Cs (flame test)
blue
hydrocarbons
System
State Functions
14. Instrument used to measure the pressure of atmospheric gas
CAT
specific heat
Metalliods
Barometer
15. Color of Li (flame test)
red
Hydrogen bonding
pi=(nRT)/v
lambda
16. A homogeneous mixture with 1 phase
alcohol
Bond Order
Polar Covalent
Solution
17. Energy can't be created nor destroyed
q/moles
1 atm = 760 mmHg = 101.3 kPa
Law of Conservation of Energy
red
18. Force that holds atoms together
Chemical Bonds
2nd law of thermodynamics
Bond enthalpy
bent
19. Isotope
acetate
H
surroundings
different # of neutrons
20. Bomb Calorimeter
triple point
strong bases
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Constant Volume
21. Group 1 and heavier Group 2 bases
Arrhenius Base
Octahedral
permanganate
strong bases
22. Oxidation # of Halogens
Anion
-1
Joule
Entropy (S)
23. The chemical formed when an acid donates a proton
AE= AH - RTAn
conjugate base
Temperature
3/2RT
24. OIL RIG
Oxidation is Loss Reduction is Gain
Cation
Hydrogen bonding
charge
25. AH of formation for a substance in its stablest form (how it is found in nature)
Ionic Compounds
0
1.86°C
Arrhenius acid
26. Freezing point depression formula
?Tf= kf x molality
Thermochemistry
Bronsted-Lowry Acid
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
27. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
supercritical fluid
yellow --> green
permanganate
force x distance = work done
28. 1 sigma bond - 1 pi bond
violet
5% rule
double bond
dec-
29. Anions or cations as needed to produce a compound with non net charge
Manometer
Counterions
6.63x10?³4Js
heat of fusion
30. Organic w/ -OH group
Limiting reactant
End Point
pent-
alcohol
31. For significant digits - leading zeros ____ significant
-(q of H2O + q of cal)
paramagnetic
viscosity
are not
32. If anion ends in -ide - acid name ends in
hydro-ic acid
Effusion
surroundings
voltaic cells
33. Where reduction occurs
Cathode
?Tb= kb x molality
Molal FP Depression Constant
boiling point
34. Type of system in which the energy may escape - but the mass is conserved
meth-
trigonal bipyramidal
Closed System
CAT
35. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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36. Type of system in which the energy and mass may leave or enter
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Open System
force x distance = work done
Transition metals
37. F¹?
Pressure
flouride
soluble
Endothermic
38. Work = ?
-(P)(Change in V)
wavelength
-one
Constant Volume
39. Color of Ba (flame test)
Bonding Pairs
-2 - with peroxide -1
Colligative properties
green/yellow
40. Spontaneous emission of radiation
are not
Mass
X of a = moles a/total moles
Radioactivity
41. 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)
f
Molecular Compounds
g solute/g solvent x 100
Electronegativity
42. Two molecules with identical connectivity but different geometries
Law of Conservation of Mass
allotrope
Alkali metals
geometric isomers
43. High-speed electrons
Boltzmann distribution
Beta Particles-
bromate
Molar Heat Capacity
44. Has values from 0 to (n-1); tells shape of atomic orbitals
(moles of products that are gasses) - (moles of reactants that are gasses)
Angular Momentum Quantum Number
Hess's Law
Bonding Pairs
45. Actual Yield/Theoretical Yield*100%
Ideal Gas Law
0
Dalton's Law of Partial Pressures
Percent Yield
46. J/°Cg or J/Kg
-one
standard solution
log[H+]
Specific Heat Capacity
47. Idea Gas Law (actual rules)
Sigma Bond
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
Molarity
Gamma Ray-
48. Coffee Cup Calorimeter
boiling point
ammonium
Constant Pressure
Tetrahedral
49. The reactant that is being reduced - brings about oxidation
spontaneous
endothermic
oxidizing agent
purple
50. neutron (symbol)
yellow --> green
London Dispersion Forces
cohesion
n0