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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. OH¹?
rate
hydroxide
yellow --> green
isothermal
2. Oxidation # of Ions
Colligative properties
chlorate
Alkali metals
charge
3. H + donor
# protons (atom is defined by this)
Bronsted-Lowry Acid
ether
equilibrium
4. Energy needed to break a bond
Electron Spin Quantum Number
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
bond energy
Hybridization
5. Variable for energy of e- - goes from 1 -2 -3 on up
n (first quantum number)
electrolyte
Alkaline earth metals
Normality
6. Happens at lines in phase change charts
square pyramidal
msAT
q/moles
equilibrium
7. ln[A]=-kt + ln[A]0
-1
Integrated First-Order Rate Law
Q>K
increasing
8. Substance being dissolved in a solution (lower [ ])
prop-
Molarity
Closed System
Solute
9. Liquid to solid
specific heat
# protons + # neutrons
indicator
freezing
10. AX3E
Thermochemistry
trigonal pyramidal
Pressure of H2O must be Subtracted
dichromate
11. Heat required to raise the system 1°C
1 atm = 760 mmHg = 101.3 kPa
Isolated System
heat capacity
Chemical Bonds
12. IMF that occurs with FON
carbonate
allotrope
Hydrogen bonding
mol
13. Phase change from solid to gas
Metalliods
sublimation
phosphate
Manometer
14. ln[A] vs. time is a ...-order reaction
-ol
first
Density
permanent gases
15. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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16. 180° - sp
r1/r2
P1V1/N1T1=P2V2/N2T2
cyanide
Linear
17. Cation first - anion second
hydro-ic acid
Theory of Relativity
Atmospheric Pressure
Naming Binary Ionic Compounds
18. If needed - indicate charge of metal(cation) by...
dichromate
A Roman numeral
Solubility Product (Ksp)
system
19. Involves quantum numbers
group
PV=nRT
Quantum Mechanical Model
Hund's Rule
20. The heat changed in a chemical reaction.
Thermochemistry
mol
methoxy-
Balmer Series
21. Point at which vapor pressure=air pressure above
Anion
boiling point
Heat Capacity (C)
-oic acid
22. Atomic #
# protons (atom is defined by this)
Molal BP Elevation Constant
Adding
Temperature
23. (organics) one carbon
meth-
sulfate
base
Multiplying
24. (organics) ten carbons
Density
dec-
Speed of light
Molality
25. The reactant in the reduction reaction that forces the oxidation reaction to occur
e-
Oxidizing Agent
Quantum Mechanical Model
work
26. R=
Quantum Mechanical Model
0.0826Latm/Kmol
analyte
n0
27. Change in Energy = ? (in terms of constant pressure; for gasses)
lambda
anode
AE= AH - RTAn
square planar
28. Idea Gas Law (actual rules)
l (second quantum number)
Bond enthalpy
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
red
29. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Lone Pair
melting
Chemical Kinetics
Integrated Zero-Order Rate Law
30. Measure of the average kinetic energy of all the particles in a substance
Isolated System
Temperature
chlorite
E
31. Force per unit area
Colligative properties
Pressure
Pi Bond
indicator
32. Kinetic Energy of an individual particle formula
M = square root (3RT/mm)
charge
cyanide
precipitate
33. A method of investigation involving observation and theory to test scientific hypotheses
96500
Cg=kPg
Scientific Method
moles of solute/ L of solution
34. A monoatomic anion is named by taking...
Graham's Law
reduction agent
Its root and adding -ide
E
35. Increase Pressure
trigonal bipyramidal
Decrease Volume and Increase Temperature
cyanide
chloride
36. A given compound always has exactly the same proportion of elements by mass
Oxidizing Agent
2nd law of thermodynamics
charge
Law of Definite Proportion
37. ClO3²?
weak acid strong base rxn
chlorate
hept-
Bonding Pairs
38. Change in Energy (AE) = ? (in terms of work)
Bond Order
AE = q + w
mol
base and hydrogen gas
39. Organic w/ -NH2
heat capacity
g solute/g solvent x 100
n (first quantum number)
amine
40. This MUST be determined experimentally
exothermic
rate law
sulfide
H
41. A device in which chemical energy is changed to electrical energy
Oxidation is Loss Reduction is Gain
Galvanic Cell
Speed of light
Integrated Zero-Order Rate Law
42. Mass percent
g solute/g solvent x 100
end point
Entropy (S)
1/2mv²
43. K
isothermal
Equilibrium constant
yellow
Covalently w/in themselves - Ionicly bonded w/ each other
44. Type of system in which the energy and mass may leave or enter
Standard Temperature and Pressure
Open System
rate law
Arrhenius Acid
45. Elements on staircase on periodic table
Molality
entropy (S)
effects of IMF
Metalliods
46. Mol of solute/kg of solvent
m (third quantum number)
% yield
Bronsted-Lowry acid
Molality
47. The reactant that is being oxidized - brings about reduction
Trigonal Bipyramidal
Integrated Rate Law
reduction agent
Pi Bond
48. Where there are no electrons
actual yield/theoretical yield x 100%
Nodes
4.184
voltaic cells
49. Negative enthalpy - heat flows into surroundings
Reducing Agent
Nernst Equation
exothermic
second
50. Connects the 2 half cells in a voltaic cell
red/orange
Heat Capacity (C)
Atmospheric Pressure
salt bridge