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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. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Ionization energy
Dipole Dipole interaction
Phase diagram
Group 5A
2. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Triple point
Equlibrium constant
atomic theory
Net ionic equation
3. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Alkaline earths
atomic radius
Avagadros number
4. A horizontal row of elements in the periodic table
Dispersion Forces
Ion product
pH
Period
5. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
atomic emission spectrum
The bohr model
Colligative properties
Formal Charge
6. 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
Spin quantum number
Halogens
Atomic weight
7. An elementary particle with 0 charge and mass about equal to a proton
Electrolyte
Henderson Hasselbalch Equation
Activation energy
Neutron
8. (chemistry) p(otential of) H(ydrogen)
pH
Nonpolar covalent bond
Bronsted - Lowry definition
Activation energy
9. 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.
Conjugate acids and Bases
Phase diagram
Effective nuclear charge
Group 3A
10. A solid made up of particles that are not arranged in a regular pattern.
Ion dipole interactions
amorphous solid
Pauli exclusion principle
Planck's Constant
11. Common definition of acids as proton (H+) donors and bases as proton acceptors
actinide series
Water dissociation Constant
theoretical yield
Bronsted - Lowry definition
12. The Percent by mass of each element in a compound.
crystalline solid
Combination Reaction
Percent composition
Strong acid
13. 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.
effective nuclear charge
azimuthal quantum number
bond length
atomic radius
14. A reaction in which atoms of one element take the place of atoms of another element in a compound
Colligative properties
single displacement reaction
gram equivalent weight
Activation energy
15. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Mass number
quantum numbers
The bohr model
16. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Azeotrope
sigma bond
solvation
Electronegativity
17. Small discrete increments of energy.
quanta
Equivalence point
Group 7A
molecular weight
18. A subdivision of an energy level in an atom. They are divided into orbitals.
Aqueous Solution
subshell
atomic radius
electrolysis
19. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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20. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
ionic cmpound
Colligative properties
quantum
law of constant composition
21. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Graham's Law
atomic radius
compound
22. Simplest whole # ration of atoms in a compound
Emperical Formula
Disproportionation
Strong acid
Pauli exclusion principle
23. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Ion dipole interactions
Principle quantum number
amorphous solid
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.
Ion product
Neutron
azimuthal quantum number
Concentration
25. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Equlibrium constant
Percent yield
Group 1A
Combination Reaction
26. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Group 5A
polymer
periodic trends
Group 7A
27. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
pi bonds
Covalent Bond
Rate law
empirical formula
28. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Le chateliers Principle
actinide series
VSEPR
Diffusion
29. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Molality
Charles and Gay Lussac's Law
Phase diagram
Diffusion
30. 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
Resonance structure
Halogens
Emperical Formula
Half equivalence point
31. Any sample of a given compound will contain the same elements in the identical mass ratio.
Group 2A
law of constant composition
Noble gases
heisenberg uncertainty principle
32. A dynamic condition in which two opposing changes occur at equal rates in a closed system
subshell
Ground state
Equilibrium
single displacement reaction
33. An ionic compound that resists changes in its pH
Buffer
Molecular orbital
Dipole
Percent yield
34. 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
Concentration
Molecular orbital
chemical reaction
35. Rare earth element group (elements 58-71)
lathanide series
law of constant composition
bond length
Lewis structure
36. 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
lathanide series
Equivalence point
Reaction mechanism
hydrogen bonding
37. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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38. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
actinide series
indicator
Decomposition reaction
39. Elements in the middle of the periodic table - in groups 3-12.
atomic theory
transition elements
STP
Emperical Formula
40. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
representative elements
Network covalent
molecular weight
electron configuration
41. 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
Disproportionation
redox reaction
Percent yield
subshell
42. 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-
chemical reaction
Water dissociation Constant
Ion dipole interactions
Halogens
43. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Period
atomic radius
mole
44. 2.18 x 10^-18 J/electron
representative elements
Hydrogen bonding
Rydberg constant
Equivalence point
45. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Henderson Hasselbalch Equation
Nonpolar covalent bond
redox reaction
Rydberg constant
46. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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47. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
Ionic Bond
Avagadros number
Percent composition
azimuthal quantum number
48. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Nucleus
Common ion effect
lathanide series
Hydrogen bonding
49. 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
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50. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Dipole Dipole interaction
Octet Rule
Bronsted - Lowry definition
Pauli exclusion principle