SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
1st law of thermodynamics
methods of increasing rate
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
soluble
2. Connects the 2 half cells in a voltaic cell
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
salt bridge
Weight
P1= X1P1°
3. OH¹?
increasing
Temperature
hydroxide
allotrope
4. C=2.9979*10^8 m/s
Speed of light
Normality
Angular Momentum Quantum Number
Bronsted-Lowry Acid
5. ?H when 1 mol of bonds is broken in the gaseous state
Zero-Order Rate Law
Bond enthalpy
C=(mass)(specific heat)
Arrhenius Acid
6. How to Find an Empirical Formula Given Grams
mol
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
base
Bronsted-Lowry Acid
7. 96 -485 C/mol e-
see-saw
rate gas A/rate gas B = square root (mm A/ mm B)
Solution
Faraday
8. Universal IMF for nonpolar molecules
octahedral
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
London dispersion forces
sublimation
9. Ionizes to produce H+ ions
C + 273
Galvanic Cell
Alkali metals
Arrhenius Acid
10. AX5E
square pyramidal
violet
system
Thermochemistry
11. Mole Fraction
X of a = moles a/total moles
-one
oxidizing agent
red/orange
12. Ester suffix
are
-oate
Alkaline earth metals
end point
13. Energy needed to break a bond
indicator
Second-Order Half Life
Scientific Method
bond energy
14. Group 1 metals
Alkali metals
Theoretical yield
Molar Mass of Element/ Total Molar Mass %
0
15. Raising heat - adding catalyst - heighten concentration - bigger surface area
hydroxide
?Tf= kf x molality
1atm=?mmHg/Torr
methods of increasing rate
16. All forms of energy except for heat
bent
sublimation
work
Atmospheric Pressure
17. I¹?
Volume Metric Flask & Pipet
iodide
conjugate acid
H
18. Each orbital can hold two e?s each w/ opposite spins
Matter
Pauli Exclusion Principle
A Roman numeral
salt bridge
19. AX2E - AX2E2
Cation
Calorimeter
bent
Integrated First-Order Rate Law
20. Resistance to flow
viscosity
Beta Particles-
-one
AE= AH - RTAn
21. Actual Yield/Theoretical Yield*100%
4.184
1.86°C
Cation
Percent Yield
22. l=2
d
6.63x10?³4Js
red
Gamma Ray-
23. Temperature-pressure combination at which solid - liquid - and gas states appear
complex ions
melting point
triple point
Buffered Solution
24. Oxidation # of Polyatomic Ions
bromate
nitrate
0
charge
25. The total energy of the universe is constant - all systems tend towards minimum energy
Cg=kPg
1st law of thermodynamics
1/2mv²
Hybridization
26. Atoms combine in fixed whole # ratios
Trigonal Planar
Law of Multiple Proportions
g solute/g solvent x 100
Amino-
27. Cl¹?
Naming Binary Ionic Compounds
trigonal planar
bond energy
chloride
28. Peak of energy diagram
Transition metals
Calorimeter
activated complex (transition state)
hydrolysis
29. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
30. Oxidation # of Halogens
London dispersion forces
phosphate - sulfide - carbonate - sulfate
-1
charge
31. The mixing of native atomic orbitals to form special orbitals for bonding
Hybridization
Density
Trigonal Bipyramidal
Buffered Solution
32. Kinetic Energy per mol
Cg=kPg
t-shape
Effusion
3/2RT
33. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
96500
endless
Finding Empirical Formulas
experimental yield
34. Carbon - hydrogen - oxygen compounds
carbohydrates
period
r1/r2
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
35. 180° - sp
Linear
0
STP
0
36. Gain of electrons - decrease in oxidation #
reduction
Law of Conservation of Mass
charge
indicator
37. Expresses how the concentrations depend on time
geometric isomers
Integrated Rate Law
l (second quantum number)
deposition
38. (organics) double-bonded compound
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
paramagnetic
single bond
alkene
39. Thickness
Naming Binary Ionic Compounds
Pi Bond
viscosity
Weight
40. The energy required to raise 1 g of substance 1 degree C
force x distance = work done
Specific Heat (s)
boiling point
Balmer Series
41. An element with several different forms - each with different properties (i.e. graphite & diamond)
methoxy-
increasing
1/2mv²
Allotrope
42. Bomb Calorimeter
see-saw
Nernst Equation
Constant Volume
blue-violet
43. 760mmHg/Torr
oxidizing agent
red
Electron Spin Quantum Number
1atm=?mmHg/Torr
44. Point at which vapor pressure=air pressure above
# protons + # neutrons
H
viscosity
boiling point
45. In ideal gas law problem - when it says "atmospheric" ...
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Pressure of H2O must be Subtracted
-ous acid
Exothermic
46. Proton donors
Bronsted-Lowry acid
seesaw
Le Chatelier's Principle
alcohol
47. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Dalton's Law
Acid + Base --> Salt + Water
q
viscosity
48. AX3E2
?Tf= kf x molality
t-shape
?Tb= kb x molality
moles solute/kg solvent
49. Half cell in which reduction occurs
system
Allotrope
Galvanic Cell
cathode
50. ... compounds are most conductive
red/orange
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
ionic
Law of Multiple Proportions