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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. Has values 1 -2 -3 -...; tells energy levels
Exothermic
Principal Quantum Number
s (fourth quantum number)
methods of increasing rate
2. 90°&120° - dsp^3
acetate
a precipitate forms
Balmer Series
Trigonal Bipyramidal
3. Electron (symbol)
e-
Bond Energy
Covalently w/in themselves - Ionicly bonded w/ each other
8.31J/Kmol
4. AX2E - AX2E2
pi=(nRT)/v
Allotrope
bent
Aufbau Principle
5. A solution used in titrations whose concentration is known
Bronsted-Lowry Base
standard solution
Cation
Isolated System
6. AX5E
square pyramidal
1/2mv²
experimental yield
Solubility Product (Ksp)
7. Osmotic pressure=MRT
Osmotic Pressure
boiling point
conjugate base
Second-Order Half Life
8. Carboxylic acid ending
Amino-
Pauli Exclusion Principle
-oic acid
analyte
9. ln[A] vs. time is a ...-order reaction
3rd law of thermodynamics
first
triple bond
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
10. 0°C and 1 atm
STP
Bond Order
rate gas A/rate gas B = square root (mm A/ mm B)
e-
11. When n=4 ->2 - color=
blue-green
q
Acid + Base --> Salt + Water
3.0x108m/s
12. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
v3RT/M(in kg)
Magnetic Quantum Number (ml)
vaporization
13. Cation first - anion second
-ol
Arrhenius Acid
Naming Binary Ionic Compounds
lambda
14. Equation to find Ea from reaction rate constants at two different temperatures
Formal Charge
Solute
Balmer Series
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
15. q H2O = ?
0
Hydrogen bonding
msAT
LeChatelier's Principle
16. The rest of the universe (in thermodynamics)
Bases
Molality
surroundings
Alkali metals
17. Boltzmann constant - used in calculating speed of gas per molecule
supercritical fluid
1.38x10?²³J/K
bent
entropy (S)
18. Like dissolves...
force x distance = work done
like
Heat
Molar Mass of Element/ Total Molar Mass %
19. Amount of gravitational force exerted on an object
insoluble
Weight
square pyramidal
Atmospheric Pressure
20. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
melting
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
Anion
strong acids
21. Electrons in a hydrogen atom move around the nucleus only in circular orbits
oxalate
red
Quantum Model
v3RT/M(in kg)
22. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equilibrium constant
Buffer
activated complex (transition state)
Equivalence Point
23. Organic w/ -OH group
Tetrahedral
1 atm = 760 mmHg = 101.3 kPa
alcohol
tetrahedral
24. If Q<Ksp
Faraday
but-
no precipitate forms
0
25. Atomic #
Amount of atoms present
# protons (atom is defined by this)
Bonding Pairs
voltaic cells
26. Occupies the space above and below a sigma bond
hydrolysis
Second-Order Half Life
Pi Bond
square planar
27. Calculation from K to C
activated complex (transition state)
Solubility Product (Ksp)
C + 273
octahedral
28. When _____ significant digits - round answer to least significant digit
Multiplying
Anode
sublimation
Open System
29. Ether prefix
cohesion
Resonance
methoxy-
base and hydrogen gas
30. A single substance that may be an acid or a base (i.e. water)
Covalently w/in themselves - Ionicly bonded w/ each other
Amphoteric
Amino-
yellow
31. Pairs of electrons localized on an atom
Calorimetry
Lone Pair
-1
0
32. The reactant in the oxidizing reaction that forces the reduction reaction to occur
system
chloride
g solute/g solvent x 100
Reducing Agent
33. Releases/gives off heat (negative value)
First-Order Half Life
square planar
like
Exothermic
34. SI unit of energy; Kg*m^2/s^2
are not
weak acid strong base rxn
Joule
Hess's Law
35. Unusually strong dipole forces found when H is bonded to N - O - or F
purple
3/2RT
Molality
Hydrogen bonding
36. Moles of solute/volume of soln(L)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Molarity
endless
Bonding Pairs
37. OH¹?
hydroxide
Arrhenius Base
activated complex (transition state)
Ionic
38. A device used to measure Delta H
Calorimeter
mol
Decrease Volume and Increase Temperature
Force = mass x acceleration
39. C2O4²?
Law of Multiple Proportions
oxalate
Ampere
1.86°C
40. Substances that form H+ when dissolved in water; proton donors
conjugate base
Acids
anode
condensation
41. The transfer of energy between two objects due to temperature difference
Heat
P1= X1P1°
increasing
Molal FP Depression Constant
42. Heat capacity formula
Cathode
Second-Order Half Life
C=(mass)(specific heat)
p
43. Isotope
acid
T-shape
different # of neutrons
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
44. Type of system in which nothing is transfered (no mass or energy); ideal
endless
Isolated System
oxidizing agent
Octahedral
45. Color of Ba (flame test)
oxidizing agent
green/yellow
CAT
Q>K
46. l=0
seesaw
s
Hybridization
Chemical Bonds
47. Mass reactants= mass products
Principal Quantum Number
Law of Conservation of Mass
London Dispersion Forces
chromate
48. Absorbs/takes in heat (positive value)
Arrhenius acid
Resonance
Solvent
Endothermic
49. Horizontals on the periodic table
0
period
1 atm
-oate
50. Oxidation # of free elements
Diffusion
AE= AH - RTAn
0
nu