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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. The chemical formed when an acid donates a proton
Pauli Exclusion Principle
carbohydrates
Equilibrium constant
conjugate base
2. Ether prefix
methoxy-
0
s (fourth quantum number)
Bonding Pairs
3. A solid or gas that can be formed when 2 or more aqueous reactants come together
charge
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
precipitate
equivalence point
4. Proton (symbol)
p+
Trigonal Planar
square pyramidal
hydro-ic acid
5. Bomb Calorimeter
red
Theory of Relativity
square planar
Constant Volume
6. SI unit of energy; Kg*m^2/s^2
Bond Order
adhesion
Joule
oxalate
7. Unusually strong dipole forces found when H is bonded to N - O - or F
bromate
H
Hydrogen bonding
Oxidizing Agent
8. Entropy in the universe is always...
activation energy
increasing
reduction agent
Beta Particles-
9. Two molecules with identical connectivity but different geometries
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Entropy (S)
Isotopes
geometric isomers
10. frequency symbol
nu
bent
red
insoluble
11. Boiling point elevation formula
indicator
% yield
?Tb= kb x molality
pi=(nRT)/v
12. Energy (definition)
force x distance = work done
diamagnetic
A Roman numeral
AE= AH - RTAn
13. Releases/gives off heat (negative value)
Exothermic
Thermochemistry
permanganate
Nodes
14. Does the same as equilibrium expression - except it uses initial concentrations
p orbitals
electron affinity
Oxidation is Loss Reduction is Gain
Reaction Quotient (Q)
15. Point at which liquid?gas occurs
salt bridge
boiling point
Amino-
Surroundings
16. ?H when 1 mol of bonds is broken in the gaseous state
acid
msAT
Bond enthalpy
electron affinity
17. Organic w/ -O-
ether
Molar Mass of Element/ Total Molar Mass %
Amount of atoms present
Enthalpy of Solution
18. CN¹?
cyanide
A Roman numeral
second
Angular Momentum Quantum Number
19. A method of investigation involving observation and theory to test scientific hypotheses
Molal FP Depression Constant
base
Scientific Method
Atomic Mass Unit
20. Energy required for liquid?gas
1atm=?Pa
Bronsted-Lowry Acid
heat of vaporization
Zero-Order Half Life
21. Peak of energy diagram
activated complex (transition state)
Trigonal Bipyramidal
insoluble
Cg=kPg
22. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
nitrate
Law of Multiple Proportions
hydro-ic acid
voltaic cells
23. Color of Li (flame test)
heat capacity
boiling point
sulfite
red
24. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
0
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
State Functions
blue
25. Isotope
square planar
Temperature
Principal Quantum Number
different # of neutrons
26. OH¹?
Kinetic Molecular Theory - for ideal gases
hydroxide
base
precipitate
27. H?+NH3?NH4
actual yield/theoretical yield x 100%
v3kT/m
Strong acid weak base rxn
Amino-
28. Liquid to gas
Bronsted-Lowry acid
vaporization
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
s (fourth quantum number)
29. Planck's constant - used to calculate energy w/frequency
n0
6.63x10?³4Js
Molecular Compounds
no precipitate forms
30. OIL RIG
Oxidation is Loss Reduction is Gain
C + 273
r1/r2
system
31. AX3E
p orbitals
boiling point
trigonal pyramidal
Bronsted-Lowry Base
32. Color of Sr (flame test)
seesaw
red
Bond Order
C=(mass)(specific heat)
33. Mass/volume
5% rule
t-shape
Density
q
34. Substances that form OH- when dissolved in water; proton acceptors
base and hydrogen gas
Volume Metric Flask & Pipet
Bases
1.86°C
35. AX4E2
Multiplying
insoluble
Oxidizing Agent
square planar
36. Ending for alcohols
Ionic
-ol
third
Ionic Compounds
37. Has values 1 -2 -3 -...; tells energy levels
triple bond
v3kT/m
% yield
Principal Quantum Number
38. Idea Gas Law (actual rules)
insoluble
heat capacity
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
Polar Covalent
39. Equation to find Ea from reaction rate constants at two different temperatures
End Point
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Nernst Equation
Open System
40. The total energy of the universe is constant - all systems tend towards minimum energy
precipitate
Integrated Second-Order Rate Law
1st law of thermodynamics
no precipitate forms
41. I¹?
are
iodide
charge
P of a =(X of a)(total pressure)
42. NO3¹?
non-
nitrate
-2 - with peroxide -1
2nd law of thermodynamics
43. Amount of heat needed to change a system by 1°C
Oxidation is Loss Reduction is Gain
PV=nRT
heat capacity
electron affinity
44. If anion ends in -ite - acid name ends in...
r1/r2
-ous acid
Molecular
mol
45. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
endless
Metalliods
Alpha Particles-
Molecular
46. The part of the universe one is focused upon (in thermodynamics)
system
cathode
Its element
Equilibrium constant
47. Freezing point depression formula
electrolyte
Radioactivity
activation energy
?Tf= kf x molality
48. R in instances that pertain to energy
8.314 J/K mol
melting point
Molality
Colligative properties
49. When n=3 ->2 - color=
p orbitals
Galvanic Cell
red
cathode
50. Symbol for Enthalpy
Entropy (S)
H
zero
Second-Order Rate Law