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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. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Solute
lewis base
Atomic absorption Spectra
Titration
2. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Conjugate acids and Bases
Pauli exclusion principle
periodic trends
Intermolecular forces
3. An ionic compound that resists changes in its pH
electron configuration
Molar solubility
Group 2A
Buffer
4. 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
Theoretical yield
Halogens
Magnetic quantum number
Triple point
5. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
Half equivalence point
Lewis definition
electron configuration
6. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Collision theory of chemical Kinetics
amorphous solid
Equilibrium
energy state
7. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
molecular weight
Redox Half Reaction
Reaction order
Electronegativity
8. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
indicator
Arrhenius Definition
Common ion effect
ionic cmpound
9. 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
Molar solubility
Formula weight
Henry's Law
Proton
10. The percent by mass of each element in a compound
quantum numbers
percent composition
Resonance structure
Formula weight
11. 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.
Ion
Henderson Hasselbalch Equation
Rate determining step
Conjugate acids and Bases
12. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Free radical
solvation
Phase diagram
Intermolecular forces
13. E=hc/?
quanta
electromagnetic energy of photons emmited from electrons at ground state
transition elements
amorphous solid
14. 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
Henry's Law
Group 7A
Bronsted - Lowry definition
Neutron
15. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Decomposition reaction
effective nuclear charge
heisenberg uncertainty principle
16. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Concentration
Disproportionation
electron affinity
pi bonds
17. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
The bohr model
Dipole
Buffer
Reaction mechanism
18. 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
molecular weight
Molar solubility
representative elements
theoretical yield
19. Substance in which a solute is dissolved to form a solution
Net ionic equation
Solvent
Theoretical yield
Lyman series
20. 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
Dipole
Buffer
Acid dissociation constant
Group 1A
21. Two or more atoms held together by covalent bonds
atomic emission spectrum
molecule
Ground state
single displacement reaction
22. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Avagadros number
lewis base
Solution equilibrium
solvation
23. 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
azimuthal quantum number
quantum
Reaction order
Atomic weight
24. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
electromagnetic energy of photons emmited from electrons at ground state
Neutron
electron affinity
Collision theory of chemical Kinetics
25. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Dispersion Forces
quanta
atomic radius
electron configuration
26. The slowest elementary step which is the limit for the rate of the other steps
law of constant composition
empirical formula
Rate determining step
Halogens
27. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
quanta
Halogens
polymer
mole
28. 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
Charles and Gay Lussac's Law
Colligative properties
polymer
The bohr model
29. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Lewis definition
Colligative properties
amorphous solid
Covalent Bond
30. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Buffer
d orbital
hydrogen bonding
31. Elements in the middle of the periodic table - in groups 3-12.
Mass number
transition elements
subshell
chemical reaction
32. 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
Percent composition
decomposition reaction
Collision theory of chemical Kinetics
33. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
pi bonds
Decomposition reaction
quanta
redox reaction
34. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Colligative properties
Dispersion Forces
Bronsted Lowry
Formula weight
35. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Solute
Covalent Bond
Water dissociation Constant
Henderson Hasselbalch Equation
36. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
lewis base
solvation
Effusion
Rate law
37. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
solvation
Le chateliers Principle
Alkaline earths
amorphous solid
38. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Group 7A
Nonpolar covalent bond
electron configuration
39. The lowest allowable energy state of an atom
Ion product
effective nuclear charge
Resonance structure
Ground state
40. PH of a molecule at which it contains no net electric charge - isoelectric point.
und's rule
lathanide series
The bohr model
pI
41. 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.
Principle quantum number
Theoretical yield
transition elements
Solution equilibrium
42. 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
Pauli exclusion principle
quantum
Group 2A
Formal Charge
43. Any sample of a given compound will contain the same elements in the identical mass ratio.
Period
law of constant composition
Redox Half Reaction
chemical reaction
44. Having characteristics of both an acid and a base and capable of reacting as either
Arrhenius Definition
redox reaction
Amphoteric
Molality
45. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Effective nuclear charge
pI
Ionic Bond
compound
46. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Rydberg constant
Dipole
Ion dipole interactions
Henderson Hasselbalch Equation
47. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Spin quantum number
Titration
single displacement reaction
48. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Percent yield
Group 2A
s orbital
Group 6A
49. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Reaction order
Emperical Formula
Dipole Dipole interaction
Percent yield
50. The average distance between the nuclei of two bonded atoms
bond length
Percent yield
Planck's Constant
atomic radius