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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 elementary particle with 0 charge and mass about equal to a proton
Equlibrium constant
Reaction order
Strong acid
Neutron
2. Small discrete increments of energy.
Solute
quanta
Avagadros number
Ground state
3. 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
Hydrogen bonding
Collision theory of chemical Kinetics
percent composition
Atomic weight
4. Named after their cation and anion
bond length
heisenberg uncertainty principle
ionic cmpound
Normality
5. The maximum amount of product that can be produced from a given amount of reactant
Ground state
Diprotic Base
theoretical yield
Lewis structure
6. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Dispersion Forces
Intermolecular forces
atomic theory
7. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
pI
Reaction mechanism
hydrogen bonding
8. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
percent composition
Solute
Neutron
9. 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
Lewis structure
redox reaction
Titration
Amphoteric
10. A horizontal row of elements in the periodic table
Activation energy
Ionization energy
atomic emission spectrum
Period
11. 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
Concentration
Azeotrope
Disproportionation
Net ionic equation
12. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
quanta
Chemical Kinetics
Lewis acid base reaction
Dipole
13. In a solution - the substance that dissolves in the solvent
Reaction order
Solute
Disproportionation
Planck's Constant
14. 2.18 x 10^-18 J/electron
Le chateliers Principle
polymer
effective nuclear charge
Rydberg constant
15. (chemistry) a substance that changes color to indicate the presence of some ion or substance
s orbital
Octet Rule
solvation
indicator
16. A subdivision of an energy level in an atom. They are divided into orbitals.
Effusion
Planck's Constant
Period
subshell
17. 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
Diffusion
Nucleus
Equilibrium
Disproportionation
18. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
quantum numbers
Octet Rule
Combination Reaction
heisenberg uncertainty principle
19. Sum of the protons and neutrons in an element often denoted by the letter A
empirical formula
Amphoteric
Principle quantum number
Mass number
20. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
solvation
Decomposition reaction
Charles and Gay Lussac's Law
21. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Redox Half Reaction
Dipole Dipole interaction
Conjugate acids and Bases
s orbital
22. 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
Magnetic quantum number
atomic emission spectrum
Formal Charge
Ion dipole interactions
23. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
VSEPR
Noble gases
Solubility Product Constant
24. 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
redox reaction
Ionization energy
Formula weight
Halogens
25. 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.
quanta
atomic radius
Group 6A
Effective nuclear charge
26. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
s orbital
Diffusion
amorphous solid
27. 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
single displacement reaction
Period
The bohr model
Graham's Law
28. 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
Azeotrope
electrolysis
London forces
29. 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
Rate law
azimuthal quantum number
Resonance structure
electron affinity
30. 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
Nonpolar covalent bond
Decomposition reaction
Spin quantum number
VSEPR
31. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Bronsted - Lowry definition
Pauli exclusion principle
Equlibrium constant
quantum
32. Simplest whole # ration of atoms in a compound
sigma bond
Emperical Formula
transition elements
Group 3A
33. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Reaction mechanism
Emperical Formula
atomic theory
subshell
34. 5 valence electrons -3 ions - Nitride N
Lewis structure
electromagnetic energy of photons emmited from electrons at ground state
Group 5A
Chemical Kinetics
35. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
Percent yield
Arrhenius Definition
Noble gases
36. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
The bohr model
Planck's Constant
Mass number
effective nuclear charge
37. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
heisenberg uncertainty principle
Reaction order
Octet Rule
Group 5A
38. 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
Electronegativity
Decomposition reaction
heisenberg uncertainty principle
Acid dissociation constant
39. 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
Common ion effect
Solubility Product Constant
Bronsted Lowry
40. Slightly less reactive than alkali metals - comprise group II
Ion product
Disproportionation
Percent yield
Alkaline earths
41. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Spin quantum number
Electronegativity
Bronsted Lowry
42. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
quanta
amorphous solid
STP
molecular weight
43. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
solvation
Solution equilibrium
transition elements
Network covalent
44. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Triple point
heisenberg uncertainty principle
Proton
atomic emission spectrum
45. A reaction in which atoms of one element take the place of atoms of another element in a compound
Lyman series
electromagnetic energy of photons emmited from electrons at ground state
single displacement reaction
Combination Reaction
46. 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
Ionization energy
Resonance structure
Solution equilibrium
solvation
47. 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.
Triple point
Disproportionation
Henderson Hasselbalch Equation
The bohr model
48. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Ion
Azeotrope
polymer
Rate law
49. A reaction in which atoms of one element take the place of atoms of another element in a compound
Molar solubility
single displacement reaction
Buffer
quantum
50. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
quantum numbers
Pauli exclusion principle
atomic radius
periodic trends