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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. Universal IMF for nonpolar molecules
1/2mv²
Heisenberg Uncertainty Principle
Alkali metals
London dispersion forces
2. Force acting over distance
endothermic
Work
trigonal bipyramidal
Molarity
3. Energy required to break a bond
alkane
0.512°C
entropy (S)
Bond Energy
4. Occupies the space above and below a sigma bond
+1 - except if bonded to Alkali Metal -1
excess reactant
Pi Bond
acid
5. R in instances that pertain to energy
blue-violet
geometric isomers
H
8.314 J/K mol
6. Osmotic pressure formula
Calorimeter
pi=(nRT)/v
Molecular Orbitals (MOs)
First-Order Rate Law
7. R=
Molecular Orbitals (MOs)
actual yield/theoretical yield x 100%
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
8.31J/Kmol
8. A solution used in titrations whose concentration is known
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
standard solution
Solubility Product (Ksp)
Molar Mass of Element/ Total Molar Mass %
9. AX6
0
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
voltaic cells
octahedral
10. When n=5 ->2 - color=
blue-violet
nitrite
single bond
acid
11. 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
insoluble
supercritical fluid
Molal FP Depression Constant
Bonding Pairs
12. Where there are no electrons
d orbitals
hydro-ic acid
-oic acid
Nodes
13. Color of Ba (flame test)
deposition
3/2RT
Magnetic Quantum Number (ml)
green/yellow
14. Rate of Diffusion/Effusion formula
Heat
Amino-
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
ionic
15. Polyatomic Ions (bonding)
condensation
Covalently w/in themselves - Ionicly bonded w/ each other
a precipitate forms
Aufbau Principle
16. AX4E2
Quantum Mechanical Model
dichromate
square planar
no precipitate forms
17. PO4³?
a precipitate forms
Specific Heat Capacity
phosphate
supercritical fluid
18. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Hydrogen bonding
London Dispersion Forces
bond energy
Solute
19. J/°Cmol or J/Kmol
Lone Pair
oxide
P1V1/N1T1=P2V2/N2T2
Molar Heat Capacity
20. Color of Li (flame test)
nitrite
s (fourth quantum number)
Cell Potential (Ecell)
red
21. Atoms combine in fixed whole # ratios
1/2mv²
N=N.(0.5)^time/time half-life
hex-
Law of Multiple Proportions
22. #NAME?
Magnetic Quantum Number (ml)
E
force x distance = work done
sulfate
23. Group 1 metals
d orbitals
Alkali metals
chromate
vaporization
24. Mass reactants= mass products
acid
t-shape
Law of Conservation of Mass
-(P)(Change in V)
25. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
exothermic
LE Model
vapor pressure
-(P)(Change in V)
26. Half cell in which oxidation occurs
Heat Capacity (C)
Hybridization
anode
-al
27. Organic w/ -NH2
charge
-oic acid
amine
nitrate
28. As protons are added to the nucleus - electrons are similarly added
(moles of products that are gasses) - (moles of reactants that are gasses)
Thermochemistry
Pauli Exclusion Principle
Aufbau Principle
29. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Lone Pair
H
Magnetic Quantum Number (ml)
Bond enthalpy
30. (organics) seven carbons
State Functions
moles solute/kg solvent
phosphate - sulfide - carbonate - sulfate
hept-
31. Half-life equation
Arrhenius Base
Open System
N=N.(0.5)^time/time half-life
chlorate
32. AX4E
Le Chatelier's Principle
Faraday
Equivalence Point
see-saw
33. Mass #
hex-
paramagnetic
Normality
# protons + # neutrons
34. ClO2¹?
LE Model
Percent Yield
chlorite
entropy
35. H?+NH3?NH4
Strong acid weak base rxn
1atm=?Pa
Law of Conservation of Mass
Amphoteric
36. A given compound always has exactly the same proportion of elements by mass
Law of Conservation of Mass
Law of Definite Proportion
Negative work value; work done by system
P1V1/N1T1=P2V2/N2T2
37. Boiling point - melting point - viscosity - vapor pressure - surface tension
s
moles of solute/ L of solution
group
effects of IMF
38. Mass/volume
# protons + # neutrons
Density
oxalate
oxide gas and water
39. Symbol for Enthalpy
Polar Covalent
H
heat of vaporization
0.512°C
40. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
Law of Definite Proportion
Diffusion
green/yellow
41. Unusually strong dipole forces found when H is bonded to N - O - or F
square pyramidal
Hydrogen bonding
Volume Metric Flask & Pipet
Bases
42. SI unit of energy; Kg*m^2/s^2
end point
PV=nRT
Joule
surroundings
43. F¹?
ether
flouride
log[H+]
(moles of products that are gasses) - (moles of reactants that are gasses)
44. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Aufbau Principle
adhesion
Quantum Model
Law of Multiple Proportions
45. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Atmospheric Pressure
Anode
d
46. Reactant which doesn't get used up completely in a chemical reaction
single bond
excess reactant
cohesion
condensation
47. A monoatomic cation takes name from...
-1
-one
Its element
Effusion
48. Energy needed to break a bond
hydroxide
bond energy
viscosity
Volume Metric Flask & Pipet
49. Oxidation # of Compounds
triple bond
Volt
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
0
50. Organic w/ -OH group
alcohol
Dalton's Law of Partial Pressures
Pauli Exclusion Principle
Molality