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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. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Neutron
Phase diagram
Magnetic quantum number
Intermolecular forces
2. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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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.
Bronsted Lowry
Molecular orbital
solvation
compound
4. PH of a molecule at which it contains no net electric charge - isoelectric point.
molecule
pI
Covalent Bond
redox reaction
5. A solid made up of particles that are not arranged in a regular pattern.
electrolysis
Theoretical yield
Emperical Formula
amorphous solid
6. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Neutralization reaction
Lewis acid base reaction
Solvent
Formula weight
7. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Rate law
effective nuclear charge
Electrolyte
Henderson Hasselbalch Equation
8. The lowest allowable energy state of an atom
Principle quantum number
Proton
Ground state
Molecular orbital
9. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Diprotic Base
Combination Reaction
Lewis structure
Rydberg constant
10. A base that can accept two moles of H+ per mole of itself (ex: SO4
energy state
Magnetic quantum number
Net ionic equation
Diprotic Base
11. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Lewis acid base reaction
Rate law
Water dissociation Constant
12. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Common ion effect
Diffusion
Group 7A
Collision theory of chemical Kinetics
13. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Resonance structure
Percent yield
Group 3A
14. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
quantum numbers
Reaction order
quanta
Conjugate acids and Bases
15. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
London forces
angular momentum in the bohr model
Molality
Triple point
16. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Magnetic quantum number
polymer
Balmer series
Atomic weight
17. Small discrete increments of energy.
Resonance structure
hydrogen bonding
Neutron
quanta
18. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Equlibrium constant
pi bonds
Le chateliers Principle
Dipole Dipole interaction
19. 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
Formal Charge
Alkaline earths
Reaction order
atomic radius
20. 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
Disproportionation
Proton
Atomic weight
21. 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
Charles and Gay Lussac's Law
Hydrogen bonding
Concentration
Group 1A
22. 5 different orbitals shaped like clover leaves and max electrons is 10
Formula weight
d orbital
Dipole Dipole interaction
Ionic Bond
23. An ionic compound that resists changes in its pH
Group 1A
Buffer
Strong acid
Group 6A
24. 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
Percent yield
Avagadros number
Alkaline earths
25. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
Activation energy
ionic cmpound
Neutralization reaction
26. An elementary particle with 0 charge and mass about equal to a proton
pI
polymer
Neutron
molecule
27. 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.
Henderson Hasselbalch Equation
Formal Charge
Triple point
decomposition reaction
28. 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
Ionization energy
Mass number
theoretical yield
Aqueous Solution
29. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
Diffusion
Amphoteric
azimuthal quantum number
30. Tells you how much solute is present compared to the amount of solvent
The bohr model
Concentration
und's rule
Conjugate acids and Bases
31. Sum of the protons and neutrons in an element often denoted by the letter A
Amphoteric
Mass number
electron affinity
Disproportionation
32. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Activation energy
Diffusion
Octet Rule
Free radical
33. The process by which one or more substances change to produce one or more different substances
Strong acid
percent composition
chemical reaction
Ion product
34. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
Normality
single displacement reaction
London forces
35. 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.
Solution equilibrium
Solubility Product Constant
molecular weight
lathanide series
36. A reaction where a compound does Not change its molecular structure.
actinide series
physical reaction
Vapor pressure
Conjugate acids and Bases
37. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Effusion
Equivalence point
pH
38. 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.
Le chateliers Principle
azimuthal quantum number
The bohr model
Ion product
39. A reaction in which atoms of one element take the place of atoms of another element in a compound
Mass number
lewis base
Collision theory of chemical Kinetics
single displacement reaction
40. The maximum amount of product that can be produced from a given amount of reactant
atomic theory
energy state
subshell
theoretical yield
41. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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42. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Diffusion
energy state
Chemical Kinetics
Intermolecular forces
43. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
azimuthal quantum number
The bohr model
effective nuclear charge
Noble gases
44. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
empirical formula
quanta
The bohr model
Decomposition reaction
45. 2.18 x 10^-18 J/electron
Rydberg constant
theoretical yield
Spin quantum number
Acid dissociation constant
46. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
atomic radius
Rate determining step
solvation
Group 6A
47. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Activation energy
electromagnetic energy of photons emmited from electrons at ground state
Diffusion
Group 3A
48. An atom or group of atoms that has a positive or negative charge
Solution equilibrium
Vapor pressure
angular momentum in the bohr model
Ion
49. Slightly less reactive than alkali metals - comprise group II
Pauli exclusion principle
Avagadros number
crystalline solid
Alkaline earths
50. 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
theoretical yield
Theoretical yield
Covalent Bond
Resonance structure