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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 30 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. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Emperical Formula
Electronegativity
Raoult's Law
2. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
3. Chalcogens - - Oxide O
Group 6A
single displacement reaction
Lewis acid base reaction
Ground state
4. 5 valence electrons -3 ions - Nitride N
Group 5A
Period
Dipole Dipole interaction
Spin quantum number
5. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Solute
Decomposition reaction
Hydrogen bonding
6. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
electrolysis
indicator
Atomic weight
7. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
single displacement reaction
Lyman series
Solubility Product Constant
quantum numbers
8. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
Group 1A
Ion dipole interactions
The bohr model
Rate determining step
9. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Neutralization reaction
Covalent Bond
periodic trends
gram equivalent weight
10. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Rate law
Diffusion
law of constant composition
empirical formula
11. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
ionic cmpound
Activation energy
Common ion effect
Vapor pressure
12. Slightly less reactive than alkali metals - comprise group II
Graham's Law
Alkaline earths
Molarity
Ion
13. The slowest elementary step which is the limit for the rate of the other steps
Titration
Triple point
Activation energy
Rate determining step
14. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
atomic theory
hydrogen bonding
Free radical
Period
15. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Concentration
Collision theory of chemical Kinetics
Noble gases
Ion dipole interactions
16. (chemistry) p(otential of) H(ydrogen)
Rydberg constant
pH
physical reaction
Neutralization reaction
17. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Reaction mechanism
London forces
Bronsted Lowry
18. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Strong acid
Buffer
redox reaction
19. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Ionization energy
electron affinity
Lewis structure
Water dissociation Constant
20. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
Reaction order
Molar solubility
percent composition
Atomic absorption Spectra
21. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Equivalence point
Graham's Law
Charles and Gay Lussac's Law
chemical reaction
22. The Percent by mass of each element in a compound.
Percent composition
Molecular orbital
Decomposition reaction
Atomic absorption Spectra
23. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
redox reaction
Ionic Bond
molecular weight
Strong acid
24. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
ionic cmpound
Formal Charge
Group 7A
STP
25. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
d orbital
Effusion
Halogens
Group 7A
26. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
Water dissociation Constant
Group 5A
Net ionic equation
Hydrogen bonding
27. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Rate determining step
Electronegativity
bond length
molecular weight
28. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
bond energy
Molecular orbital
Rate law
Group 6A
29. A base that can accept two moles of H+ per mole of itself (ex: SO4
Ionic Bond
indicator
Diprotic Base
Group 3A
30. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
azimuthal quantum number
Formula weight
Theoretical yield
31. Small discrete increments of energy.
Group 6A
Group 5A
quanta
Rydberg constant
32. Numbers that specify the properties of atomic orbitals and of their electrons
Magnetic quantum number
Theoretical yield
Nucleus
quantum numbers
33. An elementary particle with 0 charge and mass about equal to a proton
bond length
Magnetic quantum number
Neutron
Network covalent
34. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Resonance structure
Dipole
angular momentum in the bohr model
hydrogen bonding
35. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Dipole
compound
Effective nuclear charge
Group 2A
36. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
energy state
Mass number
bond energy
37. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
38. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
bond length
Neutralization reaction
Neutron
Molar solubility
39. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
lathanide series
Atomic absorption Spectra
Effusion
Normality
40. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Aqueous Solution
Lewis definition
amorphous solid
molecular weight
41. A reaction in which atoms of one element take the place of atoms of another element in a compound
Effusion
Buffer
Theoretical yield
single displacement reaction
42. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Planck's Constant
Ionic Bond
Reaction mechanism
Octet Rule
43. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Water dissociation Constant
Net ionic equation
Planck's Constant
empirical formula
44. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
atomic emission spectrum
Equlibrium constant
Titration
45. PH of a molecule at which it contains no net electric charge - isoelectric point.
Rydberg constant
Effusion
pI
Electrolyte
46. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Vapor pressure
pH
Bronsted Lowry
actinide series
47. Temperature is constant; effusion and temperature are proportional to the square root of their masses
48. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
effective nuclear charge
mole
single displacement reaction
49. The energy required to break a chemical bond and form neutral isolated atoms
Arrhenius Definition
Lewis definition
bond energy
Diffusion
50. A definite stable energy that a physical system can have
energy state
Ionization energy
Free radical
Solute