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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. AX2 - AX2E3
Second-Order Rate Law
linear
hydroxide
Osmotic Pressure
2. Happens at lines in phase change charts
perchlorate
equilibrium
q/moles
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
3. Variable for energy of e- - goes from 1 -2 -3 on up
Density
Buffered Solution
n (first quantum number)
Angular Momentum Quantum Number
4. A molecule having a center of positive charge and a center of negative charge
Barometer
Dipole Moment
d
linear
5. O²?
Electronegativity
supercritical fluid
oxide
Faraday
6. (organics) double-bonded compound
LeChatelier's Principle
Hybridization
alkene
Heat Capacity (C)
7. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
3/2RT
London Dispersion Forces
vapor pressure
Calorimetry
8. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
are
Polar Covalent
Van't Hoff factor
Exothermic
9. Change in Energy (AE) = ? (in terms of work)
Enthalpy of Solution
AE = q + w
Reaction Quotient (Q)
Negative work value; work done by system
10. Atoms combine in fixed whole # ratios
Law of Multiple Proportions
Standard Temperature and Pressure
group
LE Model
11. Substances that form H+ when dissolved in water; proton donors
Acids
Quantum Model
Graham's Law
system
12. If Q>Ksp
Heat
Buffered Solution
a precipitate forms
alkene
13. Coffee Cup Calorimeter
Alpha Particles-
Constant Pressure
acetate
London dispersion forces
14. Anything occupying space and with mass
complex ions
soluble
supercritical fluid
Matter
15. In a given atom no two electrons can have the same set of four quantum numbers
adhesion
Hydrogen bonding
First-Order Half Life
Pauli Exclusion Principle
16. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
-2 - with peroxide -1
Colligative properties
0.0826Latm/Kmol
Joule
17. Raoult's Law - relations between vapor pressure and concentrations
freezing
State Functions
P1= X1P1°
chlorite
18. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Effusion
1.38x10?²³J/K
CAT
Ionic Compounds
19. Peak of energy diagram
-(q of H2O + q of cal)
allotrope
activated complex (transition state)
AE= AH - RTAn
20. An element with several different forms - each with different properties (i.e. graphite & diamond)
yellow
oxidation
chlorate
Allotrope
21. Ideal Gas Law Formula
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
carbonate
PV=nRT
Colligative properties
22. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
Effusion
STP
1.38x10?²³J/K
23. 120° - sp^2
Trigonal Planar
Arrhenius Acid
alkane
Atomic Mass Unit
24. 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)
d
Molecular Compounds
p orbitals
adiabatic
25. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
s orbitals
-al
Law of Multiple Proportions
Bases
26. Point where acid completely neutralizes base
equivalence point
0.512°C
First-Order Rate Law
Electron Spin Quantum Number
27. H?+OH??H2O
0.512°C
strong acid strong base rxn
8.314 J/K mol
purple
28. Increase Volume
Gamma Ray-
Increase Temperature
rate
Standard Temperature and Pressure
29. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
iodide
freezing
0
30. Boiling point elevation formula
Adding
square planar
Tetrahedral
?Tb= kb x molality
31. =vM2/M1
Bronsted-Lowry Acid
Scientific Method
Law of Conservation of Mass
r1/r2
32. Puts H? into solution
Its element
?Tb= kb x molality
like
Arrhenius acid
33. Two molecules with identical connectivity but different geometries
geometric isomers
chlorite
insoluble
Endothermic
34. Melting
Second-Order Rate Law
Molality
fusion
Pauli Exclusion Principle
35. Pure metal or metal hydride + H20 ->
wavelength
Anion
base and hydrogen gas
single bond
36. Mass/volume
Hydrogen bonding
Endothermic
Density
hydro-ic acid
37. Similar to atomic orbitals - except between molecules
Cg=kPg
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
Strong acid weak base rxn
Molecular Orbitals (MOs)
38. If anion ends in -ite - acid name ends in...
entropy (S)
Ionic Compounds
-ous acid
methods of increasing rate
39. Liquid to gas
spontaneous
v3RT/M(in kg)
vaporization
n (first quantum number)
40. Volume of gas @STP
22.4L
m (third quantum number)
boiling point
0
41. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Positive work value; work done on system
Metalliods
Formal Charge
Kinetic Molecular Theory - for ideal gases
42. (N) number of equivalents per liter of solution
1st law of thermodynamics
alcohol
Normality
Specific Heat (s)
43. Substance in which something is dissolved in a solution (higher [ ])
anode
Solvent
ammonium
hydro-ic acid
44. l=3
v3RT/M(in kg)
g solute/g solvent x 100
blue-violet
f
45. For significant digits - trailing zeros _____ significant
are
condensation
Q>K
Zero-Order Half Life
46. Energy needed to vaporize a mole of a liquid
1atm=?mmHg/Torr
blue-green
?Hvap
chromate
47. OH¹?
hydroxide
Hydrogen bonding
seesaw
Magnetic Quantum Number (ml)
48. 1 sigma bond
Allotrope
single bond
Hund's Rule
5% rule
49. [A] vs. time is a ...-order reaction
zero
yellow --> green
Anode
Solution
50. Aldehyde suffix
-al
Gamma Ray-
?Hvap
adhesion