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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. Energy (definition)
not spontaneous
chlorate
force x distance = work done
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
2. Increase Volume
purple --> pink
critical point
Equivalence Point
Increase Temperature
3. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Bronsted-Lowry base
Chemical Kinetics
double bond
Law of Multiple Proportions
4. A measure of randomness or disorder
entropy
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
trigonal bipyramidal
period
5. The reactant in the reduction reaction that forces the oxidation reaction to occur
Endothermic
seesaw
Oxidizing Agent
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
6. ClO3²?
chlorate
eth-
Delta H or Enthalpy Change
Molecule
7. H + donor
Chemical Bonds
melting
Bronsted-Lowry Acid
m (third quantum number)
8. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
fusion
weak acid strong base rxn
London dispersion forces
9. These orbitals are diagonal
entropy (S)
vaporization
titrant buret
d orbitals
10. Ether prefix
methoxy-
Quantum Mechanical Model
nitrite
Law of Definite Proportion
11. All _________ compounds are electrolytes
anode
1.86°C
Ionic
P of a =(X of a)(total pressure)
12. Effusion of a gas is inversely proportional to the square root of the molar mass
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13. H?+NH3?NH4
paramagnetic
Strong acid weak base rxn
Bases
carbonate
14. Heat needed to change 1 g of substance to 1°C
Adding
methods of increasing rate
specific heat
Integrated Zero-Order Rate Law
15. Electrons in a hydrogen atom move around the nucleus only in circular orbits
0
insoluble
Quantum Model
Amphoteric
16. AH of formation for a substance in its stablest form (how it is found in nature)
alcohol
like
viscosity
0
17. An element with several different forms - each with different properties (i.e. graphite & diamond)
heat capacity
nitrite
Beta Particles-
Allotrope
18. Atoms combine in fixed whole # ratios
-ol
Law of Multiple Proportions
prop-
log[H+]
19. Symbol for Enthalpy
v3kT/m
Increase Temperature
Net Ionic Equation
H
20. Spontaneous emission of radiation
acid
meth-
Its root and adding -ide
Radioactivity
21. neutron (symbol)
single bond
n0
London dispersion forces
heat of fusion
22. #NAME?
moles solute/kg solvent
E
C + 273
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
23. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
State Functions
Ligand
Endothermic
hept-
24. For significant digits - trailing zeros _____ significant
are
fusion
charge
Zero-Order Rate Law
25. Donates a single H+ Ion (... other prefixes also)
Multiplying
Monoprotic
exothermic
chloride
26. AX5E
Angular Momentum Quantum Number
yellow --> green
square pyramidal
Cation
27. Force acting over distance
prop-
Amphoteric
Work
CAT
28. Elements on staircase on periodic table
0
% yield
Metalliods
Cation
29. The chemical formed when a base accepts a proton
conjugate acid
square pyramidal
v3RT/M(in kg)
paramagnetic
30. Ability of an atom in a molecule to attract shared electrons to itself
period
-ic acid
Electronegativity
prop-
31. (organics) five carbons
soluble
C=(mass)(specific heat)
Polar Covalent
pent-
32. K
Equilibrium constant
square planar
1/2mv²
base
33. ClO2¹?
square pyramidal
N=N.(0.5)^time/time half-life
chlorite
purple
34. Faraday's constant
96500
surroundings
A Roman numeral
Tetrahedral
35. Mixing of gases
Root Mean Square Velocity
condensation
adhesion
Diffusion
36. PO4³?
0
phosphate
Endothermic
Colligative properties
37. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Buffer
Its element
Reducing Agent
condensation
38. Verticals on the periodic table
oxidizing agent
methods of increasing rate
group
-oic acid
39. Elements which have all electrons paired and relatively unaffected by magnetic fields
Beta Particles-
Q>K
diamagnetic
paramagnetic
40. 120° - sp^2
Galvanic Cell
oct-
Trigonal Planar
d orbitals
41. Delta H (AH) = ?
Hund's Rule
Electronegativity
Solubility Product (Ksp)
q/moles
42. Bomb Calorimeter
Constant Volume
viscosity
ammonium
oxidizing agent
43. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
First-Order Half Life
Decrease Volume and Increase Temperature
22.4L
44. Substances that form OH- when dissolved in water; proton acceptors
Anode
C=(mass)(specific heat)
Bases
alcohol
45. Isotope
Limiting reactant
Alpha Particles-
E
different # of neutrons
46. Temperature-pressure combination at which solid - liquid - and gas states appear
nitrate
supercritical fluid
Specific Heat (s)
triple point
47. All cations are soluble with sulfate EXCEPT
deposition
precipitate
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
flouride
48. When n=6 ->2 - color=
permanganate
Acids
violet
sulfite
49. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
strong acids
electrolyte
(moles of products that are gasses) - (moles of reactants that are gasses)
Dalton's Law of Partial Pressures
50. The total energy of the universe is constant - all systems tend towards minimum energy
insoluble
d orbitals
1st law of thermodynamics
Decrease Volume and Increase Temperature
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