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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 reaction in which atoms of one element take the place of atoms of another element in a compound
Henry's Law
pi bonds
single displacement reaction
Balmer series
2. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Neutron
Decomposition reaction
percent composition
crystalline solid
3. The percent by mass of each element in a compound
Aqueous Solution
Reaction order
percent composition
Planck's Constant
4. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
azimuthal quantum number
quantum numbers
Percent composition
5. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Theoretical yield
Principle quantum number
Formula weight
Spin quantum number
6. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Aqueous Solution
polymer
VSEPR
solvation
7. The area of chemistry that is concerned with reaction rates and reaction mechanisms
bond length
transition elements
Graham's Law
Chemical Kinetics
8. A base that can accept two moles of H+ per mole of itself (ex: SO4
Theoretical yield
Free radical
Diprotic Base
Group 5A
9. 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
Group 2A
Redox Half Reaction
Covalent Bond
Group 7A
10. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
decomposition reaction
Pauli exclusion principle
Theoretical yield
11. Elements in the middle of the periodic table - in groups 3-12.
Percent yield
transition elements
Water dissociation Constant
pI
12. Common definition of acids as proton (H+) donors and bases as proton acceptors
compound
Raoult's Law
Bronsted - Lowry definition
Titration
13. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
Solution equilibrium
Group 2A
Theoretical yield
quantum numbers
14. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Ionization energy
Bronsted - Lowry definition
physical reaction
redox reaction
15. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Noble gases
Lewis structure
Molality
und's rule
16. A reaction in which atoms of one element take the place of atoms of another element in a compound
Theoretical yield
single displacement reaction
s orbital
Conjugate acids and Bases
17. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Ion product
redox reaction
Le chateliers Principle
The bohr model
18. 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
Henderson Hasselbalch Equation
Group 2A
The bohr model
Equivalence point
19. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
redox reaction
Combination Reaction
Reaction order
electromagnetic energy of photons emmited from electrons at ground state
20. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
The bohr model
polymer
Solubility Product Constant
21. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Percent composition
Combination Reaction
Group 7A
und's rule
22. 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
Equlibrium constant
Effective nuclear charge
Nucleus
quantum
23. 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
solvation
Water dissociation Constant
representative elements
Buffer
24. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Molecular orbital
atomic radius
Rydberg constant
decomposition reaction
25. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Dispersion Forces
amorphous solid
azimuthal quantum number
26. E=hc/?
Net ionic equation
s orbital
redox reaction
electromagnetic energy of photons emmited from electrons at ground state
27. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Lewis acid base reaction
electron configuration
Charles and Gay Lussac's Law
pi bonds
28. 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
Neutralization reaction
hydrogen bonding
Octet Rule
Solvent
29. 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
Hydrogen bonding
Formal Charge
physical reaction
Molar solubility
30. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
law of constant composition
Buffer
percent composition
31. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
Pauli exclusion principle
quanta
Emperical Formula
32. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Neutralization reaction
quanta
Diffusion
polymer
33. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Reaction order
Avagadros number
single displacement reaction
34. 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.
single displacement reaction
Principle quantum number
mole
Aqueous Solution
35. 5 different orbitals shaped like clover leaves and max electrons is 10
Reaction mechanism
amorphous solid
Dipole
d orbital
36. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Solubility Product Constant
Molecular orbital
Noble gases
heisenberg uncertainty principle
37. Simplest whole # ration of atoms in a compound
angular momentum in the bohr model
Emperical Formula
molecule
London forces
38. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
single displacement reaction
electron configuration
quantum numbers
Molality
39. In a solution - the substance that dissolves in the solvent
pi bonds
Solute
redox reaction
energy state
40. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
law of constant composition
Period
gram equivalent weight
lewis base
41. A solution in which water is the solvent
Buffer
Resonance structure
Diffusion
Aqueous Solution
42. 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.
Chemical Kinetics
Bronsted Lowry
Equivalence point
gram equivalent weight
43. 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.
Group 3A
Redox Half Reaction
Dipole Dipole interaction
Acid dissociation constant
44. 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
Henry's Law
Bronsted Lowry
Spin quantum number
VSEPR
45. 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-
lathanide series
Water dissociation Constant
Equilibrium
Acid dissociation constant
46. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
und's rule
Conjugate acids and Bases
quantum numbers
Combination Reaction
47. 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
Azeotrope
Disproportionation
hydrogen bonding
Formula weight
48. 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.
bond energy
Effective nuclear charge
Solubility Product Constant
Rate law
49. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
electromagnetic energy of photons emmited from electrons at ground state
single displacement reaction
Strong acid
Formal Charge
50. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Noble gases
Raoult's Law
Ionization energy
Collision theory of chemical Kinetics