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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. The energy required to break a chemical bond and form neutral isolated atoms
Proton
bond energy
gram equivalent weight
Lewis acid base reaction
2. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
ionic cmpound
Molar solubility
Net ionic equation
Molecular orbital
3. 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.
theoretical yield
Group 6A
Effective nuclear charge
Concentration
4. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
mole
Molecular orbital
empirical formula
decomposition reaction
5. 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
ionic cmpound
Atomic weight
Acid dissociation constant
Percent yield
6. 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
Aqueous Solution
Spin quantum number
Arrhenius Definition
Strong acid
7. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Half equivalence point
theoretical yield
redox reaction
London forces
8. Named after their cation and anion
Solubility Product Constant
ionic cmpound
theoretical yield
Mass number
9. 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
Reaction order
Octet Rule
decomposition reaction
10. A horizontal row of elements in the periodic table
Effective nuclear charge
Chemical Kinetics
Period
Neutron
11. A solid made up of particles that are not arranged in a regular pattern.
Group 6A
lathanide series
Ion
amorphous solid
12. 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
pi bonds
London forces
hydrogen bonding
Intermolecular forces
13. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Lyman series
Ion product
sigma bond
Noble gases
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.
hydrogen bonding
Lyman series
Noble gases
Dipole
15. 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
Decomposition reaction
Electrolyte
s orbital
Equivalence point
16. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
solvation
Magnetic quantum number
quantum
quantum numbers
17. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
law of constant composition
Magnetic quantum number
d orbital
18. Small discrete increments of energy.
quanta
azimuthal quantum number
pi bonds
electrolysis
19. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Theoretical yield
Lewis acid base reaction
energy state
Solution equilibrium
20. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Group 5A
Molar solubility
crystalline solid
21. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Henry's Law
angular momentum in the bohr model
Covalent Bond
22. A base that can accept two moles of H+ per mole of itself (ex: SO4
Balmer series
Diprotic Base
molecular weight
Planck's Constant
23. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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24. 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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25. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
polymer
sigma bond
bond length
Water dissociation Constant
26. 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.
s orbital
Equivalence point
Magnetic quantum number
Group 7A
27. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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28. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Electronegativity
Dispersion Forces
azimuthal quantum number
Effusion
29. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
atomic radius
polymer
Ion product
30. The average distance between the nuclei of two bonded atoms
Intermolecular forces
bond length
Lyman series
Rydberg constant
31. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Equlibrium constant
atomic theory
Effusion
Combination Reaction
32. 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
Raoult's Law
sigma bond
empirical formula
Titration
33. The percent by mass of each element in a compound
percent composition
electron configuration
Ground state
Network covalent
34. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Pauli exclusion principle
chemical reaction
Chemical Kinetics
35. 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
London forces
amorphous solid
Pauli exclusion principle
energy state
36. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Vapor pressure
quantum
electron affinity
Chemical Kinetics
37. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Nonpolar covalent bond
crystalline solid
Bronsted Lowry
Diprotic Base
38. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
decomposition reaction
Henry's Law
Equivalence point
39. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Arrhenius Definition
gram equivalent weight
polymer
Halogens
40. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Dispersion Forces
Ion
Electrolyte
Atomic weight
41. Rare earth element group (elements 58-71)
Ionic Bond
Dispersion Forces
Alkaline earths
lathanide series
42. 2.18 x 10^-18 J/electron
Group 3A
Amphoteric
Rydberg constant
Lyman series
43. A substance that - when dissolved in water - results in a solution that can conduct electricity
Common ion effect
Alkaline earths
Electrolyte
single displacement reaction
44. In a solution - the substance that dissolves in the solvent
indicator
electrolysis
Magnetic quantum number
Solute
45. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
percent composition
Dipole Dipole interaction
Proton
Phase diagram
46. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Henderson Hasselbalch Equation
Molarity
molecular weight
pi bonds
47. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
theoretical yield
Amphoteric
pi bonds
sigma bond
48. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
Formula weight
Arrhenius Definition
transition elements
49. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
periodic trends
Diffusion
Collision theory of chemical Kinetics
Ionization energy
50. 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.
Solubility Product Constant
Percent composition
decomposition reaction
bond energy