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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.
Reaction mechanism
Arrhenius Definition
Formula weight
Collision theory of chemical Kinetics
2. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Phase diagram
bond energy
Magnetic quantum number
Atomic weight
3. 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
heisenberg uncertainty principle
solvation
compound
4. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
d orbital
electron configuration
actinide series
5. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Free radical
Collision theory of chemical Kinetics
bond length
Combination Reaction
6. 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
Molarity
representative elements
Molality
bond length
7. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Group 7A
redox reaction
Redox Half Reaction
Molecular orbital
8. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
bond length
Aqueous Solution
atomic emission spectrum
Effective nuclear charge
9. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Ionization energy
Solubility Product Constant
Electronegativity
Diffusion
10. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Bronsted Lowry
Group 7A
Group 2A
bond length
11. Rare earth element group (elements 58-71)
Neutralization reaction
lathanide series
Ion product
Dipole
12. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
d orbital
Molecular orbital
Theoretical yield
energy state
13. 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
Ionic Bond
Balmer series
Hydrogen bonding
Activation energy
14. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Conjugate acids and Bases
atomic theory
Dispersion Forces
molecule
15. An atom or group of atoms that has a positive or negative charge
s orbital
quanta
effective nuclear charge
Ion
16. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
molecule
molecular weight
lewis base
17. 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
pi bonds
Formal Charge
Ionization energy
Effusion
18. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
electromagnetic energy of photons emmited from electrons at ground state
Theoretical yield
azimuthal quantum number
19. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Principle quantum number
sigma bond
Free radical
lewis base
20. The lowest allowable energy state of an atom
Electrolyte
Ground state
Molality
molecule
21. The maximum amount of product that can be produced from a given amount of reactant
Emperical Formula
Dipole Dipole interaction
theoretical yield
Molar solubility
22. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Diprotic Base
single displacement reaction
Resonance structure
23. Small discrete increments of energy.
Half equivalence point
Effusion
quanta
heisenberg uncertainty principle
24. 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.
atomic emission spectrum
Ion product
Normality
quanta
25. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
atomic emission spectrum
decomposition reaction
Ionic Bond
26. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
redox reaction
Reaction mechanism
pH
Octet Rule
27. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
Ion dipole interactions
Aqueous Solution
representative elements
28. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
lewis base
Henderson Hasselbalch Equation
Azeotrope
29. A base that can accept two moles of H+ per mole of itself (ex: SO4
Lewis structure
Diprotic Base
Free radical
effective nuclear charge
30. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
Reaction order
crystalline solid
quantum
31. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Planck's Constant
Solute
Henderson Hasselbalch Equation
actinide series
32. The percent by mass of each element in a compound
polymer
mole
Triple point
percent composition
33. 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
molecular weight
angular momentum in the bohr model
Redox Half Reaction
34. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Planck's Constant
quantum
Concentration
heisenberg uncertainty principle
35. The process by which one or more substances change to produce one or more different substances
Combination Reaction
chemical reaction
Colligative properties
compound
36. Numbers that specify the properties of atomic orbitals and of their electrons
atomic theory
quantum numbers
electron configuration
Water dissociation Constant
37. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
quantum
actinide series
Colligative properties
empirical formula
38. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Concentration
molecule
Titration
heisenberg uncertainty principle
39. Redox reaction - in which the same species is both oxidized and reduced.
Atomic absorption Spectra
Equilibrium
Disproportionation
Octet Rule
40. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
atomic emission spectrum
redox reaction
Nonpolar covalent bond
Noble gases
41. In a solution - the substance that dissolves in the solvent
Solute
Dipole Dipole interaction
chemical reaction
Emperical Formula
42. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Ion
percent composition
Halogens
molecule
43. 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
Lewis structure
gram equivalent weight
Net ionic equation
London forces
44. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
redox reaction
Net ionic equation
angular momentum in the bohr model
transition elements
45. 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
Equivalence point
Colligative properties
electron configuration
angular momentum in the bohr model
46. Substance in which a solute is dissolved to form a solution
Chemical Kinetics
Colligative properties
pi bonds
Solvent
47. Gram equivalent weight of solute per liter of solution - often denoted by N.
Disproportionation
Normality
Ground state
Net ionic equation
48. A reaction where a compound does Not change its molecular structure.
Henderson Hasselbalch Equation
Equivalence point
physical reaction
Phase diagram
49. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
bond length
Emperical Formula
Chemical Kinetics
Group 4A
50. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Equilibrium
Dispersion Forces
Group 7A