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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. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Equilibrium Expression
rate gas A/rate gas B = square root (mm A/ mm B)
Quantum Model
oct-
2. CN¹?
Ligand
soluble
Electronegativity
cyanide
3. The line running between the atoms
Arrhenius equation
Normality
Sigma Bond
Standard Temperature and Pressure
4. Oxidation # of Polyatomic Ions
charge
ammonium
strong bases
see-saw
5. Point at which solid?liquid occurs
melting point
London Dispersion Forces
Galvanic Cell
Constant Volume
6. High-energy light
Average KE = 1/2(mass)(average speed of all particles)
Integrated Zero-Order Rate Law
8.31J/Kmol
Gamma Ray-
7. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
AE = q + w
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Specific Heat (s)
8. Heat capacity formula
Bronsted-Lowry Base
van't Hoff Factor
Specific Heat Capacity
C=(mass)(specific heat)
9. A molecule having a center of positive charge and a center of negative charge
Dipole Moment
p
Nernst Equation
-oic acid
10. Mass percent
Atmospheric Pressure
Equivalence Point
Surroundings
g solute/g solvent x 100
11. 101 -325 Pa
pent-
Bases
AE= AH - RTAn
1atm=?Pa
12. Elements which have all electrons paired and relatively unaffected by magnetic fields
diamagnetic
Theoretical yield
1.86°C
1/2mv²
13. Similar to atomic orbitals - except between molecules
blue-violet
Constant Volume
but-
Molecular Orbitals (MOs)
14. Gas to solid
d
p orbitals
deposition
1.86°C
15. 1 sigma bond - 1 pi bond
entropy (S)
double bond
Metalliods
0
16. Atoms combine in fixed whole # ratios
a precipitate forms
Law of Multiple Proportions
oxide
Constant Pressure
17. ClO4¹?
perchlorate
Buffered Solution
activated complex (transition state)
sulfate
18. A monoatomic cation takes name from...
ionic
Its element
p+
methods of increasing rate
19. We cannot simultaneously determine an atom's exact path or location
Heisenberg Uncertainty Principle
Hybridization
Atomic Mass Unit
linear
20. (organics) four carbons
but-
Graham's Law
melting
Bronsted-Lowry base
21. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
rate
Bases
Resonance
22. (N) number of equivalents per liter of solution
supercritical fluid
flouride
Normality
work
23. Oxoacid solution (such as HSO4-) forms...
phosphate - sulfide - carbonate - sulfate
Buffered Solution
oxide gas and water
indicator
24. AX4E
see-saw
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
?Hvap
Molality
25. Point where acid completely neutralizes base
equivalence point
Nodes
dec-
alkyne
26. STP
0 degrees C - 1 atm
ionic
s
% error
27. Variable for type of orbital
X of a = moles a/total moles
moles solute/kg solvent
l (second quantum number)
Calorimeter
28. Substance being dissolved in a solution (lower [ ])
Solute
isothermal
Molar Mass of Element/ Total Molar Mass %
Heat Capacity (C)
29. Pairs of electrons localized on an atom
Lone Pair
Molarity
boiling point
square planar
30. Gain of electrons - decrease in oxidation #
specific heat
Density
rate law
reduction
31. Elements in groups 3-12
Transition metals
nitrite
chromate
Anion
32. Molality =
Manometer
Specific Heat Capacity
moles solute/kg solvent
hydro-ic acid
33. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
red
Manometer
Atomic Mass Unit
Root Mean Square Velocity
34. Mass/volume
Density
phosphate - sulfide - carbonate - sulfate
Heat
trigonal planar
35. The mixing of native atomic orbitals to form special orbitals for bonding
0.0821 atm L/mol K
Chemical Kinetics
Hybridization
surroundings
36. If anion ends in -ide - acid name ends in
Bronsted-Lowry Acid
hydro-ic acid
hydroxide
seesaw
37. When gas compresses ...
Positive work value; work done on system
Decrease Volume and Increase Temperature
Dalton's Law
Aufbau Principle
38. Boiling point elevation formula
first
?Tb= kb x molality
phosphate
% yield
39. A solution that resists a change in its pH
Buffered Solution
Balmer Series
Manometer
specific heat
40. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Limiting reactant
not spontaneous
Pressure
0
41. Passage of gas through tiny orifice
methods of increasing rate
Effusion
-(P)(Change in V)
5% rule
42. (organics) six carbons
viscosity
hex-
indicator
Integrated Zero-Order Rate Law
43. Phase change from solid to gas
sublimation
meth-
trigonal bipyramidal
Metalliods
44. Amount of product produced when limiting reactant is used up
Solution
zero
strong acid strong base rxn
Theoretical yield
45. An equilibrium expression
reduction
Solubility Product (Ksp)
Specific Heat Capacity
msAT
46. Positive enthalpy - heat flows into system
Molecule
f
nu
endothermic
47. Planck's constant - used to calculate energy w/frequency
State Functions
Ligand
Metalliods
6.63x10?³4Js
48. Absorbs/takes in heat (positive value)
Endothermic
Hess's Law
cohesion
high pressure - low temperature
49. CO3²?
log[H+]
double bond
Barometer
carbonate
50. Ketone suffix
force x distance = work done
Colligative properties
-one
trigonal bipyramidal