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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 base that can accept two moles of H+ per mole of itself (ex: SO4
Charles and Gay Lussac's Law
Covalent Bond
Diprotic Base
lewis base
2. Rare earth element group (elements 58-71)
Rydberg constant
electron configuration
Mass number
lathanide series
3. 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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4. 2.18 x 10^-18 J/electron
Rydberg constant
law of constant composition
Molar solubility
Mass number
5. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
subshell
Mass number
Effective nuclear charge
6. 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
Halogens
Group 6A
7. 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
Bronsted Lowry
Ion product
azimuthal quantum number
Magnetic quantum number
8. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
azimuthal quantum number
Ionic Bond
atomic theory
quanta
9. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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10. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Network covalent
Noble gases
percent composition
Neutralization reaction
11. The process of decomposing a chemical compound by the passage of an electric current.
atomic emission spectrum
Lyman series
Balmer series
electrolysis
12. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
Network covalent
Charles and Gay Lussac's Law
Ground state
Azeotrope
13. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
ionic cmpound
angular momentum in the bohr model
empirical formula
gram equivalent weight
14. Elements in the middle of the periodic table - in groups 3-12.
redox reaction
atomic radius
subshell
transition elements
15. Gram equivalent weight of solute per liter of solution - often denoted by N.
mole
single displacement reaction
Pauli exclusion principle
Normality
16. 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
Acid dissociation constant
Disproportionation
quantum
Proton
17. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
Bronsted Lowry
Molality
Bronsted - Lowry definition
18. Sum of the protons and neutrons in an element often denoted by the letter A
quantum
Resonance structure
Mass number
atomic emission spectrum
19. The process by which one or more substances change to produce one or more different substances
Effective nuclear charge
theoretical yield
Hydrogen bonding
chemical reaction
20. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Pauli exclusion principle
Intermolecular forces
Arrhenius Definition
atomic radius
21. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Intermolecular forces
quantum
polymer
Equilibrium
22. 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.
electrolysis
Percent yield
Ion product
Bronsted Lowry
23. 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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24. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Henry's Law
Normality
Dipole
Free radical
25. 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
Diffusion
Group 4A
solvation
London forces
26. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Ionization energy
Halogens
Molar solubility
Ionic Bond
27. The average distance between the nuclei of two bonded atoms
Dispersion Forces
sigma bond
Ion product
bond length
28. 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.
Lewis definition
Henderson Hasselbalch Equation
subshell
law of constant composition
29. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Group 4A
und's rule
sigma bond
Atomic weight
30. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Electrolyte
Group 2A
Atomic weight
31. 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.
Effective nuclear charge
Molecular orbital
Dipole
Ion product
32. 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
Arrhenius Definition
Ion
Percent yield
33. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
amorphous solid
Network covalent
molecular weight
electron affinity
34. 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
Intermolecular forces
Conjugate acids and Bases
The bohr model
VSEPR
35. 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
Molarity
Pauli exclusion principle
Resonance structure
Disproportionation
36. (chemistry) p(otential of) H(ydrogen)
Nucleus
pH
lathanide series
Solution equilibrium
37. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
Equivalence point
Proton
VSEPR
Diffusion
38. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
The bohr model
hydrogen bonding
Half equivalence point
Formula weight
39. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Solution equilibrium
Formula weight
representative elements
40. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
Hydrogen bonding
Atomic absorption Spectra
Charles and Gay Lussac's Law
Network covalent
41. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Dispersion Forces
Proton
Molecular orbital
actinide series
42. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Percent yield
Diffusion
mole
effective nuclear charge
43. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Combination Reaction
Vapor pressure
Proton
Avagadros number
44. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Ionic Bond
Noble gases
Buffer
Le chateliers Principle
45. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
heisenberg uncertainty principle
Hydrogen bonding
molecular weight
Molarity
46. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Dipole
Ion
transition elements
Collision theory of chemical Kinetics
47. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
molecular weight
Amphoteric
Principle quantum number
Disproportionation
48. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Reaction mechanism
lathanide series
angular momentum in the bohr model
49. A subdivision of an energy level in an atom. They are divided into orbitals.
Solution equilibrium
Le chateliers Principle
subshell
Dipole Dipole interaction
50. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
electron configuration
representative elements
electrolysis
periodic trends