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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. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Henry's Law
Solubility Product Constant
Effusion
Collision theory of chemical Kinetics
2. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Decomposition reaction
Solute
redox reaction
3. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Buffer
physical reaction
Ion product
Equilibrium
4. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Decomposition reaction
Rydberg constant
Magnetic quantum number
Spin quantum number
5. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
azimuthal quantum number
Diffusion
Reaction order
Octet Rule
6. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
7. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
lathanide series
Half equivalence point
Equlibrium constant
Halogens
8. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Colligative properties
Diprotic Base
Group 3A
sigma bond
9. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Equlibrium constant
Phase diagram
Combination Reaction
Triple point
10. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
Diprotic Base
Electrolyte
Rate law
11. A solid made up of particles that are not arranged in a regular pattern.
Rate determining step
amorphous solid
compound
indicator
12. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Net ionic equation
Lewis definition
Phase diagram
Raoult's Law
13. Gram equivalent weight of solute per liter of solution - often denoted by N.
heisenberg uncertainty principle
Normality
Molarity
Combination Reaction
14. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
15. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Atomic weight
Percent yield
Covalent Bond
16. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
chemical reaction
Network covalent
azimuthal quantum number
Lyman series
17. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
lewis base
Effective nuclear charge
Diprotic Base
Water dissociation Constant
18. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Triple point
Strong acid
Raoult's Law
Nonpolar covalent bond
19. 5 valence electrons -3 ions - Nitride N
Group 5A
Mass number
Titration
Henderson Hasselbalch Equation
20. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
Atomic absorption Spectra
compound
Lewis structure
21. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Molar solubility
Neutron
bond length
actinide series
22. Elements in the middle of the periodic table - in groups 3-12.
physical reaction
Octet Rule
Solvent
transition elements
23. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
law of constant composition
quantum
Group 3A
Triple point
24. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
Redox Half Reaction
Electrolyte
pH
25. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Solubility Product Constant
Triple point
Ground state
lewis base
26. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Molecular orbital
Group 7A
empirical formula
Period
27. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
Henderson Hasselbalch Equation
Aqueous Solution
Resonance structure
Ion
28. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
mole
Free radical
Group 3A
Triple point
29. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Ground state
Conjugate acids and Bases
Le chateliers Principle
30. Rare earth element group (elements 58-71)
lathanide series
VSEPR
molecular weight
mole
31. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
s orbital
Principle quantum number
Le chateliers Principle
Equilibrium
32. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Ionic Bond
Balmer series
pi bonds
Titration
33. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Noble gases
crystalline solid
Electronegativity
34. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Group 3A
pi bonds
chemical reaction
Resonance structure
35. Chalcogens - - Oxide O
Rate law
Spin quantum number
Group 6A
mole
36. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Free radical
polymer
percent composition
Strong acid
37. A definite stable energy that a physical system can have
Colligative properties
energy state
Redox Half Reaction
Group 4A
38. A reaction where a compound does Not change its molecular structure.
Proton
Neutron
redox reaction
physical reaction
39. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Octet Rule
Rate determining step
indicator
Half equivalence point
40. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Ion
Percent yield
Chemical Kinetics
Rydberg constant
41. 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
Neutralization reaction
bond length
London forces
Formula weight
42. Tells you how much solute is present compared to the amount of solvent
Concentration
Octet Rule
Amphoteric
Lewis structure
43. E=hc/?
Molar solubility
electromagnetic energy of photons emmited from electrons at ground state
Free radical
Aqueous Solution
44. Any sample of a given compound will contain the same elements in the identical mass ratio.
Effective nuclear charge
law of constant composition
Solvent
Percent composition
45. Slightly less reactive than alkali metals - comprise group II
Rydberg constant
Effusion
Alkaline earths
chemical reaction
46. The process by which one or more substances change to produce one or more different substances
subshell
chemical reaction
Effusion
Solubility Product Constant
47. Simplest whole # ration of atoms in a compound
Solubility Product Constant
Octet Rule
Emperical Formula
representative elements
48. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
quanta
Intermolecular forces
electron configuration
Lewis acid base reaction
49. In a solution - the substance that dissolves in the solvent
Molar solubility
Solute
Effusion
Theoretical yield
50. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Equilibrium
Le chateliers Principle
Vapor pressure