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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. An element with several different forms - each with different properties (i.e. graphite & diamond)
Buffer
Allotrope
pent-
-2 - with peroxide -1
2. All _________ compounds are electrolytes
rate gas A/rate gas B = square root (mm A/ mm B)
Surroundings
Anion
Ionic
3. Kinetic Energy per molecule
1/2mv²
pent-
sublimation
prop-
4. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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5. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
voltaic cells
-(P)(Change in V)
% yield
adhesion
6. C2O4²?
Increase Temperature
increasing
msAT
oxalate
7. Anything occupying space and with mass
charge
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
hydrolysis
Matter
8. Spontaneous emission of radiation
Trigonal Bipyramidal
lambda
Radioactivity
heat capacity
9. Lowers activation energy
catalyst
Antibonding Molecular Orbital
viscosity
Cg=kPg
10. AX3
Solvent
viscosity
trigonal planar
Law of Multiple Proportions
11. (organics) five carbons
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
pent-
melting point
cohesion
12. O²?
oxide
entropy (S)
Net Ionic Equation
ammonium
13. A single substance that may be an acid or a base (i.e. water)
Lone Pair
Reducing Agent
Amphoteric
Overall Reaction Order
14. 109.5° - sp^3
Tetrahedral
Overall Reaction Order
acid
1/2mv²
15. Ionizes to produce OH- Ions
moles solute/kg solvent
Arrhenius acid
Arrhenius Base
s orbitals
16. Cation first - anion second
Its element
-ol
are not
Naming Binary Ionic Compounds
17. Carbon & hydrogen compounds
heat of fusion
hydrocarbons
melting
excess reactant
18. ?T=k*m(solute)
Buffered Solution
Molal BP Elevation Constant
dichromate
increasing
19. Color of Li (flame test)
red
weak acid strong base rxn
sulfite
nitrate
20. l=0
phosphate
s
salt bridge
ammonium
21. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Molecule
Boltzmann distribution
1.86°C
P1= X1P1°
22. Has values 1 -2 -3 -...; tells energy levels
moles of solute/ L of solution
Kinetic Molecular Theory - for ideal gases
Principal Quantum Number
are
23. Type of system in which nothing is transfered (no mass or energy); ideal
Oxidizing Agent
Isolated System
Bond enthalpy
Dipole-dipole forces
24. Spectrum of light when an electron drops to energy level n=2
Heat Capacity (C)
Balmer Series
bond energy
Linear
25. (organics) single-bonded compound
alkane
Nodes
Law of Multiple Proportions
Delta H or Enthalpy Change
26. Solid to liquid
Aufbau Principle
Bond Order
melting
a precipitate forms
27. How to Find an Empirical Formula Given Percentages
isothermal
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
a precipitate forms
endless
28. S²?
alkane
-al
spontaneous
sulfide
29. SO4²?
adiabatic
melting point
p
sulfate
30. A molecule having a center of positive charge and a center of negative charge
Dipole Moment
Pressure of H2O must be Subtracted
Buffered Solution
Closed System
31. Matter can't be created nor destroyed
n0
Hydrogen bonding
wavelength
Law of Conservation of Mass
32. These orbitals are diagonal
Joule
red
Electronegativity
d orbitals
33. Where oxidation occurs
melting
s orbitals
dec-
Anode
34. l=1
third
solid CO2
p
red
35. Phase change from gas to solid
deposition
Magnetic Quantum Number (ml)
phosphate - sulfide - carbonate - sulfate
AE = q + w
36. Gas to solid
seesaw
Q>K
excess reactant
deposition
37. Heat capacity formula
Calorimeter
C=(mass)(specific heat)
Law of Multiple Proportions
sulfite
38. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
Solubility Product (Ksp)
Solute
?Tb= kb x molality
supercritical fluid
39. Tools NEEDED for dilution
Molar Mass of Element/ Total Molar Mass %
Volume Metric Flask & Pipet
Its element
-1
40. Measure of the average kinetic energy of all the particles in a substance
Temperature
perchlorate
Q<K
hydrolysis
41. Verticals on the periodic table
Formal Charge
Anion
group
Aufbau Principle
42. These orbitals are perpendicular
p orbitals
insoluble
Hydrogen bonding
Transition metals
43. The weighted average of all the isotopes that an atom can have (in g/mol)
paramagnetic
Second-Order Half Life
Atomic Mass Unit
methods of increasing rate
44. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
diamagnetic
nitrate
red/orange
45. Elements in groups 3-12
spontaneous
Transition metals
1st law of thermodynamics
Molecular
46. Organic w/ -O-
Quantum Model
ether
96500
Hybridization
47. Color of K (flame test)
AE = q + w
purple
meth-
charge
48. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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49. Energy involved in gaining an electron to become a negative ion
Law of Multiple Proportions
boiling point
Dipole Moment
electron affinity
50. AX5E
q/moles
adhesion
Acid + Base --> Salt + Water
square pyramidal