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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. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Equilibrium
angular momentum in the bohr model
Neutron
electron configuration
2. Gram equivalent weight of solute per liter of solution - often denoted by N.
Rydberg constant
angular momentum in the bohr model
Molality
Normality
3. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Octet Rule
Activation energy
theoretical yield
Henderson Hasselbalch Equation
4. The percent by mass of each element in a compound
Effective nuclear charge
pi bonds
percent composition
Common ion effect
5. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
indicator
Collision theory of chemical Kinetics
actinide series
molecular weight
6. Slightly less reactive than alkali metals - comprise group II
Theoretical yield
Hydrogen bonding
crystalline solid
Alkaline earths
7. 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.
Group 7A
redox reaction
Redox Half Reaction
Solvent
8. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
Nucleus
Lewis acid base reaction
bond length
Intermolecular forces
9. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
STP
Ion product
Pauli exclusion principle
quanta
10. The slowest elementary step which is the limit for the rate of the other steps
atomic theory
Diprotic Base
Intermolecular forces
Rate determining step
11. Sum of the protons and neutrons in an element often denoted by the letter A
Covalent Bond
Ion
Mass number
quantum numbers
12. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Phase diagram
crystalline solid
Normality
13. Substance in which a solute is dissolved to form a solution
Magnetic quantum number
ionic cmpound
Solvent
Group 7A
14. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
atomic radius
Ground state
gram equivalent weight
15. 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-
Amphoteric
Avagadros number
Water dissociation Constant
Alkaline earths
16. 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
The bohr model
Ionization energy
Redox Half Reaction
empirical formula
17. The Percent by mass of each element in a compound.
Free radical
Group 6A
Percent composition
Dipole Dipole interaction
18. 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.
single displacement reaction
Group 3A
law of constant composition
bond length
19. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
effective nuclear charge
Solvent
amorphous solid
20. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Rydberg constant
Charles and Gay Lussac's Law
Magnetic quantum number
pi bonds
21. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Rate law
bond length
mole
electron affinity
22. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
atomic theory
Equivalence point
lathanide series
23. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Reaction order
Free radical
redox reaction
Buffer
24. Simplest whole # ration of atoms in a compound
Azeotrope
Theoretical yield
Emperical Formula
und's rule
25. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
decomposition reaction
Le chateliers Principle
Ionization energy
physical reaction
26. Rare earth element group (elements 58-71)
Collision theory of chemical Kinetics
Avagadros number
Atomic absorption Spectra
lathanide series
27. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Balmer series
Chemical Kinetics
Network covalent
Ion
28. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
chemical reaction
Free radical
Principle quantum number
Octet Rule
29. An ionic compound that resists changes in its pH
VSEPR
Molality
Buffer
Bronsted - Lowry definition
30. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
empirical formula
polymer
Octet Rule
representative elements
31. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Planck's Constant
The bohr model
solvation
Emperical Formula
32. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
33. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
pH
Vapor pressure
Azeotrope
Molecular orbital
34. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Solubility Product Constant
Rydberg constant
Formula weight
35. The lowest allowable energy state of an atom
mole
pH
Ground state
Group 4A
36. 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
Group 5A
azimuthal quantum number
Percent yield
Formal Charge
37. 2.18 x 10^-18 J/electron
Rydberg constant
Lewis definition
molecule
compound
38. 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
Atomic weight
Electronegativity
Molar solubility
39. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Diprotic Base
Atomic weight
pH
Water dissociation Constant
40. 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
Atomic weight
Rydberg constant
Colligative properties
Concentration
41. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Rate law
Reaction order
Group 1A
lewis base
42. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Le chateliers Principle
Collision theory of chemical Kinetics
Atomic absorption Spectra
Group 5A
43. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Ion product
Mass number
Net ionic equation
atomic emission spectrum
44. Common definition of acids as proton (H+) donors and bases as proton acceptors
Water dissociation Constant
mole
Effusion
Bronsted - Lowry definition
45. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
d orbital
Normality
Equlibrium constant
46. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Colligative properties
Atomic absorption Spectra
Reaction order
actinide series
47. 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
d orbital
Strong acid
Solvent
Equlibrium constant
48. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
polymer
quantum numbers
Electronegativity
49. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Le chateliers Principle
Dipole Dipole interaction
heisenberg uncertainty principle
polymer
50. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Bronsted - Lowry definition
Reaction mechanism
Proton
atomic radius