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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. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
ionic cmpound
Formula weight
pI
Electrolyte
2. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Planck's Constant
electrolysis
actinide series
3. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Henderson Hasselbalch Equation
Nucleus
Concentration
quantum
4. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
Ion
Combination Reaction
heisenberg uncertainty principle
5. Numbers that specify the properties of atomic orbitals and of their electrons
pi bonds
angular momentum in the bohr model
Group 4A
quantum numbers
6. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
amorphous solid
redox reaction
Pauli exclusion principle
Ion dipole interactions
7. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Ground state
Charles and Gay Lussac's Law
Strong acid
pi bonds
8. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Decomposition reaction
Arrhenius Definition
Molarity
quantum
9. An ionic compound that resists changes in its pH
Triple point
theoretical yield
Buffer
Reaction order
10. Named after their cation and anion
ionic cmpound
Henderson Hasselbalch Equation
Network covalent
Formal Charge
11. 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
Balmer series
ionic cmpound
Neutron
12. The lowest allowable energy state of an atom
atomic radius
Ground state
The bohr model
Combination Reaction
13. A definite stable energy that a physical system can have
Equivalence point
Group 4A
energy state
percent composition
14. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Solution equilibrium
Activation energy
Lyman series
quantum numbers
15. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Resonance structure
Dipole
Rydberg constant
molecular weight
16. A substance that - when dissolved in water - results in a solution that can conduct electricity
Le chateliers Principle
electrolysis
Rydberg constant
Electrolyte
17. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Aqueous Solution
Triple point
Dispersion Forces
bond length
18. Slightly less reactive than alkali metals - comprise group II
hydrogen bonding
Alkaline earths
Molality
lewis base
19. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
s orbital
Nucleus
Network covalent
Decomposition reaction
20. Elements in the middle of the periodic table - in groups 3-12.
Ion
Formal Charge
transition elements
Lewis acid base reaction
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
Emperical Formula
Solute
Balmer series
22. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
quantum
Solvent
Bronsted Lowry
Common ion effect
23. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Atomic weight
Rydberg constant
effective nuclear charge
actinide series
24. A subdivision of an energy level in an atom. They are divided into orbitals.
Bronsted Lowry
subshell
atomic theory
Henry's Law
25. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
pH
atomic theory
The bohr model
Electrolyte
26. 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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27. The process by which one or more substances change to produce one or more different substances
Effective nuclear charge
chemical reaction
energy state
quantum numbers
28. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
atomic emission spectrum
Buffer
Triple point
29. A solution in which water is the solvent
amorphous solid
Aqueous Solution
Combination Reaction
Lewis acid base reaction
30. The percent by mass of each element in a compound
lathanide series
Lewis acid base reaction
percent composition
theoretical yield
31. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
Nonpolar covalent bond
Percent yield
sigma bond
Group 7A
32. 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
Combination Reaction
s orbital
angular momentum in the bohr model
transition elements
33. 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.
Group 2A
Equivalence point
amorphous solid
Period
34. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
ionic cmpound
atomic radius
Molar solubility
Noble gases
35. E=hc/?
Group 5A
Nonpolar covalent bond
electromagnetic energy of photons emmited from electrons at ground state
Group 7A
36. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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37. 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
Acid dissociation constant
Solution equilibrium
compound
hydrogen bonding
38. Having characteristics of both an acid and a base and capable of reacting as either
pi bonds
Period
bond length
Amphoteric
39. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Effusion
polymer
Formula weight
Acid dissociation constant
40. 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.
electron affinity
Disproportionation
Lyman series
Solubility Product Constant
41. 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-
Emperical Formula
Decomposition reaction
Water dissociation Constant
Ion
42. Gram equivalent weight of solute per liter of solution - often denoted by N.
Net ionic equation
Normality
Phase diagram
Effusion
43. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
atomic radius
electrolysis
STP
44. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Formula weight
redox reaction
hydrogen bonding
d orbital
45. 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
d orbital
Alkaline earths
Azeotrope
Hydrogen bonding
46. 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.
Aqueous Solution
Ion product
energy state
Group 5A
47. The process of decomposing a chemical compound by the passage of an electric current.
Dispersion Forces
Solution equilibrium
electrolysis
redox reaction
48. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
quantum numbers
Covalent Bond
Ion
empirical formula
49. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
lathanide series
Reaction order
Nonpolar covalent bond
Decomposition reaction
50. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Percent yield
Molecular orbital
Reaction mechanism