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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. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Network covalent
Covalent Bond
Reaction mechanism
2. 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
Solubility Product Constant
Conjugate acids and Bases
Electrolyte
Ionic Bond
3. Simplest whole # ration of atoms in a compound
Lewis definition
Emperical Formula
Dipole
Half equivalence point
4. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Acid dissociation constant
Reaction order
Halogens
compound
5. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
und's rule
gram equivalent weight
sigma bond
6. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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7. (chemistry) p(otential of) H(ydrogen)
Reaction order
pH
Aqueous Solution
Vapor pressure
8. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
electrolysis
Hydrogen bonding
Strong acid
pi bonds
9. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Group 4A
decomposition reaction
und's rule
energy state
10. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
compound
sigma bond
Molar solubility
Formal Charge
11. 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.
Free radical
Activation energy
lathanide series
Atomic absorption Spectra
12. 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
Combination Reaction
Spin quantum number
Equivalence point
atomic radius
13. Elements in the middle of the periodic table - in groups 3-12.
Electrolyte
Conjugate acids and Bases
transition elements
Solution equilibrium
14. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
representative elements
pI
Balmer series
Molecular orbital
15. 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.
bond energy
Atomic absorption Spectra
Theoretical yield
VSEPR
16. 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.
empirical formula
Henderson Hasselbalch Equation
Group 1A
d orbital
17. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
actinide series
angular momentum in the bohr model
London forces
quantum numbers
18. 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
d orbital
bond energy
Colligative properties
Formula weight
19. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
angular momentum in the bohr model
bond length
lewis base
Reaction mechanism
20. Slightly less reactive than alkali metals - comprise group II
Atomic weight
Concentration
Alkaline earths
pi bonds
21. 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
Nonpolar covalent bond
theoretical yield
London forces
Ion
22. 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.
d orbital
atomic radius
Raoult's Law
Ion product
23. 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.
Dipole Dipole interaction
Atomic weight
Ion product
single displacement reaction
24. Small discrete increments of energy.
quanta
Hydrogen bonding
Effective nuclear charge
Disproportionation
25. PH of a molecule at which it contains no net electric charge - isoelectric point.
subshell
Group 5A
crystalline solid
pI
26. A solid made up of particles that are not arranged in a regular pattern.
Magnetic quantum number
Noble gases
amorphous solid
Covalent Bond
27. The Percent by mass of each element in a compound.
Activation energy
Electronegativity
Avagadros number
Percent composition
28. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Le chateliers Principle
Hydrogen bonding
Lewis definition
Atomic absorption Spectra
29. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Decomposition reaction
Diprotic Base
Solvent
Free radical
30. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Neutron
Rate determining step
Solute
Avagadros number
31. Rare earth element group (elements 58-71)
Pauli exclusion principle
lathanide series
Buffer
Atomic absorption Spectra
32. 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
Reaction mechanism
Rate determining step
Emperical Formula
33. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Rydberg constant
Ion
Avagadros number
Reaction mechanism
34. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Principle quantum number
azimuthal quantum number
Solvent
sigma bond
35. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Solubility Product Constant
Equilibrium
Rate law
Reaction order
36. Named after their cation and anion
ionic cmpound
electron affinity
Pauli exclusion principle
Diffusion
37. 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.
Solubility Product Constant
Balmer series
Raoult's Law
STP
38. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Solution equilibrium
Activation energy
Covalent Bond
Nonpolar covalent bond
39. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
energy state
atomic emission spectrum
Azeotrope
40. Having characteristics of both an acid and a base and capable of reacting as either
Effective nuclear charge
Proton
pH
Amphoteric
41. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Solution equilibrium
Arrhenius Definition
Avagadros number
Atomic absorption Spectra
42. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
quantum
Dipole Dipole interaction
Water dissociation Constant
Group 6A
43. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Molecular orbital
Bronsted Lowry
und's rule
energy state
44. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
pI
Diprotic Base
Effusion
Collision theory of chemical Kinetics
45. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Graham's Law
Diffusion
molecular weight
pI
46. The slowest elementary step which is the limit for the rate of the other steps
Equilibrium
Rate determining step
Charles and Gay Lussac's Law
Free radical
47. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
empirical formula
hydrogen bonding
Neutralization reaction
Diprotic Base
48. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Group 2A
Group 5A
London forces
49. 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
Arrhenius Definition
quantum numbers
Electronegativity
50. The maximum amount of product that can be produced from a given amount of reactant
Disproportionation
bond energy
Percent composition
theoretical yield