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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 process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
mole
Equivalence point
Aqueous Solution
Effusion
2. 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
Spin quantum number
molecule
Magnetic quantum number
Lewis acid base reaction
3. 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.
Magnetic quantum number
Rydberg constant
Combination Reaction
atomic radius
4. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
Net ionic equation
Ion
redox reaction
5. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
bond length
subshell
empirical formula
Water dissociation Constant
6. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
heisenberg uncertainty principle
Common ion effect
Ion
s orbital
7. 5 different orbitals shaped like clover leaves and max electrons is 10
Bronsted - Lowry definition
Molarity
d orbital
theoretical yield
8. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Noble gases
Diffusion
Reaction mechanism
Effective nuclear charge
9. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Percent composition
polymer
Le chateliers Principle
10. An atom or group of atoms that has a positive or negative charge
Ion
Combination Reaction
Equlibrium constant
crystalline solid
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
Equivalence point
pH
Solvent
Spin quantum number
12. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Collision theory of chemical Kinetics
Group 3A
periodic trends
13. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
physical reaction
Reaction order
Combination Reaction
Noble gases
14. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
transition elements
STP
single displacement reaction
Group 7A
15. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
empirical formula
Buffer
Formal Charge
Collision theory of chemical Kinetics
16. Property of the elements that can be predicted from the arrangement of the periodic table
Ion dipole interactions
Lewis structure
periodic trends
Buffer
17. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Avagadros number
Ground state
Combination Reaction
Half equivalence point
18. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
atomic radius
atomic radius
Group 1A
Ionic Bond
19. A reaction in which atoms of one element take the place of atoms of another element in a compound
Ion
electron affinity
single displacement reaction
Graham's Law
20. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Bronsted - Lowry definition
pi bonds
Dipole
Colligative properties
21. (chemistry) p(otential of) H(ydrogen)
subshell
pH
Aqueous Solution
Intermolecular forces
22. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
mole
crystalline solid
Equilibrium
The bohr model
23. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Aqueous Solution
London forces
Formula weight
24. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Colligative properties
Vapor pressure
Group 2A
Activation energy
25. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
Amphoteric
Phase diagram
Net ionic equation
26. Sum of the protons and neutrons in an element often denoted by the letter A
bond length
Mass number
Strong acid
Dipole
27. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Ground state
und's rule
lathanide series
28. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Bronsted Lowry
Rydberg constant
Neutralization reaction
heisenberg uncertainty principle
29. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Diprotic Base
compound
molecular weight
Group 7A
30. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Strong acid
Nonpolar covalent bond
Group 1A
Common ion effect
31. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Halogens
Dipole Dipole interaction
decomposition reaction
32. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
STP
Reaction mechanism
redox reaction
Group 3A
33. 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
Group 6A
compound
s orbital
Rydberg constant
34. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Mass number
Decomposition reaction
Conjugate acids and Bases
Net ionic equation
35. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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36. 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
lewis base
Water dissociation Constant
Group 5A
37. 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
Azeotrope
Proton
Dispersion Forces
gram equivalent weight
38. 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
Decomposition reaction
und's rule
s orbital
Hydrogen bonding
39. Two or more atoms held together by covalent bonds
molecule
Equlibrium constant
Molecular orbital
heisenberg uncertainty principle
40. 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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41. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
azimuthal quantum number
actinide series
Percent yield
42. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Azeotrope
Raoult's Law
Avagadros number
Molecular orbital
43. Numbers that specify the properties of atomic orbitals and of their electrons
Reaction order
gram equivalent weight
quantum numbers
Atomic weight
44. A reaction where a compound does Not change its molecular structure.
Nucleus
empirical formula
physical reaction
Acid dissociation constant
45. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Atomic absorption Spectra
Group 4A
Half equivalence point
46. Chalcogens - - Oxide O
Group 6A
Bronsted Lowry
Avagadros number
Lewis structure
47. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
pi bonds
Covalent Bond
Equlibrium constant
Network covalent
48. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
single displacement reaction
Disproportionation
Mass number
solvation
49. The slowest elementary step which is the limit for the rate of the other steps
Group 4A
Rate determining step
polymer
Effective nuclear charge
50. 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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