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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
Subjects
:
mcat
,
science
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. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Redox Half Reaction
Triple point
electromagnetic energy of photons emmited from electrons at ground state
Collision theory of chemical Kinetics
2. 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
Group 1A
Equlibrium constant
Lewis structure
3. An atom or group of atoms that has a positive or negative charge
Bronsted - Lowry definition
Ion
Concentration
electron affinity
4. 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.
Atomic absorption Spectra
Acid dissociation constant
Ion
Activation energy
5. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Nucleus
Lewis acid base reaction
Graham's Law
Dipole
6. 5 different orbitals shaped like clover leaves and max electrons is 10
redox reaction
d orbital
Ion product
Chemical Kinetics
7. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
lathanide series
Group 7A
Ionic Bond
8. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
Group 6A
Covalent Bond
Spin quantum number
Water dissociation Constant
9. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
Covalent Bond
London forces
Group 7A
Dipole Dipole interaction
10. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
Equlibrium constant
Water dissociation Constant
decomposition reaction
atomic radius
11. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Spin quantum number
Rate law
London forces
empirical formula
12. The Percent by mass of each element in a compound.
Equlibrium constant
Water dissociation Constant
Percent composition
Buffer
13. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
molecule
Formal Charge
Atomic weight
14. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Ionic Bond
atomic theory
Equilibrium
15. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Azeotrope
Nucleus
quanta
16. A reaction in which atoms of one element take the place of atoms of another element in a compound
Principle quantum number
single displacement reaction
representative elements
Ion dipole interactions
17. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
Vapor pressure
Redox Half Reaction
Half equivalence point
18. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Molecular orbital
law of constant composition
Pauli exclusion principle
Hydrogen bonding
19. A solid made up of particles that are not arranged in a regular pattern.
Colligative properties
amorphous solid
electrolysis
Lyman series
20. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Group 3A
redox reaction
Free radical
redox reaction
21. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
single displacement reaction
molecular weight
atomic emission spectrum
Henderson Hasselbalch Equation
22. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Balmer series
Group 6A
Neutron
23. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Equlibrium constant
Collision theory of chemical Kinetics
Ionization energy
pi bonds
24. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
crystalline solid
Chemical Kinetics
Arrhenius Definition
25. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Amphoteric
Nucleus
compound
26. Chalcogens - - Oxide O
amorphous solid
Group 6A
bond length
Acid dissociation constant
27. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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28. Named after their cation and anion
empirical formula
Acid dissociation constant
compound
ionic cmpound
29. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Collision theory of chemical Kinetics
electron configuration
Group 4A
30. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
subshell
quantum numbers
Le chateliers Principle
Network covalent
31. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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32. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Nonpolar covalent bond
Magnetic quantum number
Henderson Hasselbalch Equation
Equlibrium constant
33. 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
Reaction order
Rate law
The bohr model
Reaction mechanism
34. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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35. Rare earth element group (elements 58-71)
Amphoteric
Group 7A
Collision theory of chemical Kinetics
lathanide series
36. A definite stable energy that a physical system can have
Atomic weight
Molecular orbital
physical reaction
energy state
37. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Dipole Dipole interaction
Aqueous Solution
actinide series
Ionization energy
38. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
atomic theory
Solute
Strong acid
Rate law
39. An elementary particle with 0 charge and mass about equal to a proton
Theoretical yield
Raoult's Law
electron configuration
Neutron
40. Redox reaction - in which the same species is both oxidized and reduced.
Solute
Disproportionation
Henderson Hasselbalch Equation
redox reaction
41. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
pi bonds
theoretical yield
Intermolecular forces
gram equivalent weight
42. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Percent composition
Electrolyte
Balmer series
43. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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44. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
electromagnetic energy of photons emmited from electrons at ground state
VSEPR
Phase diagram
Solvent
45. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Avagadros number
Ionic Bond
transition elements
46. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Arrhenius Definition
physical reaction
Water dissociation Constant
Solubility Product Constant
47. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
redox reaction
quantum
Colligative properties
Percent yield
48. In a solution - the substance that dissolves in the solvent
Solute
Activation energy
representative elements
Ion
49. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Redox Half Reaction
Planck's Constant
energy state
Molarity
50. The lowest allowable energy state of an atom
und's rule
Ground state
Amphoteric
Group 7A