SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Dipole
Group 7A
Buffer
mole
2. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Theoretical yield
Colligative properties
Group 4A
3. The lowest allowable energy state of an atom
Ground state
Aqueous Solution
Ionization energy
Ion dipole interactions
4. Slightly less reactive than alkali metals - comprise group II
Ionization energy
Alkaline earths
actinide series
Bronsted Lowry
5. Redox reaction - in which the same species is both oxidized and reduced.
Arrhenius Definition
Nonpolar covalent bond
Ion
Disproportionation
6. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
energy state
transition elements
theoretical yield
Octet Rule
7. 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.
mole
Henderson Hasselbalch Equation
Mass number
Ion product
8. 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.
Diprotic Base
Solubility Product Constant
Planck's Constant
Group 3A
9. 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
Vapor pressure
atomic emission spectrum
hydrogen bonding
bond energy
10. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Azeotrope
Dipole Dipole interaction
Atomic weight
representative elements
11. 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
transition elements
redox reaction
Intermolecular forces
12. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Reaction mechanism
Free radical
Bronsted Lowry
Equlibrium constant
13. Tells you how much solute is present compared to the amount of solvent
azimuthal quantum number
Concentration
Ion
Rate law
14. 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
The bohr model
Decomposition reaction
Percent yield
pH
15. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Rate determining step
Half equivalence point
quantum numbers
Atomic weight
16. Small discrete increments of energy.
Triple point
Disproportionation
Rate law
quanta
17. Substance in which a solute is dissolved to form a solution
Solvent
Decomposition reaction
theoretical yield
Electrolyte
18. 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
heisenberg uncertainty principle
pI
Lewis definition
Ionization energy
19. Chalcogens - - Oxide O
Raoult's Law
Group 6A
Atomic absorption Spectra
Acid dissociation constant
20. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Lewis structure
Molar solubility
Molarity
lewis base
21. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Ionization energy
Chemical Kinetics
Atomic weight
und's rule
22. A subdivision of an energy level in an atom. They are divided into orbitals.
polymer
Effusion
Group 2A
subshell
23. 5 valence electrons -3 ions - Nitride N
solvation
quantum numbers
Group 5A
Principle quantum number
24. The average distance between the nuclei of two bonded atoms
compound
Covalent Bond
physical reaction
bond length
25. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Buffer
percent composition
electron affinity
26. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
subshell
s orbital
Phase diagram
Le chateliers Principle
27. The process by which one or more substances change to produce one or more different substances
azimuthal quantum number
Spin quantum number
chemical reaction
Equilibrium
28. A reaction in which atoms of one element take the place of atoms of another element in a compound
Amphoteric
single displacement reaction
Octet Rule
Strong acid
29. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Combination Reaction
electron configuration
Emperical Formula
30. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Noble gases
Rate law
theoretical yield
31. 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.
ionic cmpound
VSEPR
Raoult's Law
electron affinity
32. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
redox reaction
ionic cmpound
redox reaction
33. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
crystalline solid
Ion
Network covalent
Acid dissociation constant
34. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Ground state
angular momentum in the bohr model
Amphoteric
polymer
35. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher
Free radical
Formal Charge
electron configuration
Formula weight
36. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
atomic radius
Azeotrope
Octet Rule
Triple point
37. A solution in which water is the solvent
Ionic Bond
Equivalence point
Aqueous Solution
Formula weight
38. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Triple point
energy state
Ion
Net ionic equation
39. 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.
London forces
Rate determining step
Nonpolar covalent bond
VSEPR
40. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
41. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Half equivalence point
Spin quantum number
Rydberg constant
42. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
Ground state
Group 4A
Molar solubility
43. The slowest elementary step which is the limit for the rate of the other steps
Planck's Constant
Rate determining step
heisenberg uncertainty principle
pH
44. 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
Titration
pi bonds
Net ionic equation
law of constant composition
45. Named after their cation and anion
Dispersion Forces
ionic cmpound
energy state
Colligative properties
46. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
hydrogen bonding
bond length
s orbital
single displacement reaction
47. Simplest whole # ration of atoms in a compound
Emperical Formula
bond energy
Bronsted Lowry
electron affinity
48. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
49. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Ion product
effective nuclear charge
VSEPR
Pauli exclusion principle
50. 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
Spin quantum number
Lewis definition
Dipole Dipole interaction
atomic radius