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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. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Effusion
Reaction mechanism
electromagnetic energy of photons emmited from electrons at ground state
sigma bond
2. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
gram equivalent weight
theoretical yield
Lewis definition
3. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Common ion effect
Solution equilibrium
Nonpolar covalent bond
redox reaction
4. PH of a molecule at which it contains no net electric charge - isoelectric point.
Alkaline earths
Ion
pI
Solution equilibrium
5. 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.
Intermolecular forces
Mass number
Redox Half Reaction
Pauli exclusion principle
6. Redox reaction - in which the same species is both oxidized and reduced.
atomic radius
Noble gases
Disproportionation
s orbital
7. 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
Dipole Dipole interaction
indicator
Atomic weight
Spin quantum number
8. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
quanta
atomic radius
Combination Reaction
Bronsted - Lowry definition
9. 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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10. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
azimuthal quantum number
percent composition
Dipole Dipole interaction
molecular weight
11. In a solution - the substance that dissolves in the solvent
Bronsted Lowry
Solute
Pauli exclusion principle
Halogens
12. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Covalent Bond
Ion dipole interactions
Strong acid
Network covalent
13. 5 valence electrons -3 ions - Nitride N
Magnetic quantum number
Theoretical yield
Group 5A
Solution equilibrium
14. A reaction in which atoms of one element take the place of atoms of another element in a compound
subshell
electromagnetic energy of photons emmited from electrons at ground state
Diprotic Base
single displacement reaction
15. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
crystalline solid
Group 7A
Equivalence point
16. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Henry's Law
atomic emission spectrum
Decomposition reaction
redox reaction
17. 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.
Network covalent
Effective nuclear charge
indicator
Group 6A
18. An elementary particle with 0 charge and mass about equal to a proton
heisenberg uncertainty principle
Neutron
chemical reaction
solvation
19. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Solution equilibrium
Atomic absorption Spectra
physical reaction
Chemical Kinetics
20. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Dipole
Raoult's Law
Effusion
Resonance structure
21. 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
Molarity
energy state
bond energy
22. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Theoretical yield
Redox Half Reaction
pI
decomposition reaction
23. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Rate determining step
Equilibrium
actinide series
Mass number
24. 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
Resonance structure
quantum
Alkaline earths
Rate determining step
25. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Group 6A
Le chateliers Principle
Hydrogen bonding
Reaction mechanism
26. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Graham's Law
Conjugate acids and Bases
hydrogen bonding
d orbital
27. The slowest elementary step which is the limit for the rate of the other steps
Lewis structure
Electronegativity
Collision theory of chemical Kinetics
Rate determining step
28. 5 different orbitals shaped like clover leaves and max electrons is 10
Equivalence point
periodic trends
d orbital
Lewis structure
29. The process of decomposing a chemical compound by the passage of an electric current.
quanta
Rate determining step
electrolysis
law of constant composition
30. 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
Arrhenius Definition
Neutralization reaction
Half equivalence point
quantum
31. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
d orbital
Acid dissociation constant
Dipole
32. Having characteristics of both an acid and a base and capable of reacting as either
Neutron
Amphoteric
STP
law of constant composition
33. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Azeotrope
Decomposition reaction
indicator
Ground state
34. A substance that - when dissolved in water - results in a solution that can conduct electricity
Planck's Constant
Ion
Lyman series
Electrolyte
35. A horizontal row of elements in the periodic table
Period
Network covalent
electron affinity
Noble gases
36. Acids defined as electron - pair acceptors and bases as electron - pair donors.
pH
amorphous solid
Lewis definition
Redox Half Reaction
37. 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
solvation
Molar solubility
Ground state
Solution equilibrium
38. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Equlibrium constant
Acid dissociation constant
Phase diagram
Equilibrium
39. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Water dissociation Constant
s orbital
Equilibrium
Balmer series
40. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
single displacement reaction
Neutron
d orbital
41. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
periodic trends
Solvent
Nonpolar covalent bond
Molar solubility
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.
Percent yield
Molecular orbital
atomic emission spectrum
pH
43. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Lewis structure
Concentration
empirical formula
Reaction mechanism
44. Substance in which a solute is dissolved to form a solution
Solvent
Colligative properties
Azeotrope
Formal Charge
45. A solution in which water is the solvent
Nonpolar covalent bond
pi bonds
Aqueous Solution
Vapor pressure
46. The percent by mass of each element in a compound
Water dissociation Constant
Atomic absorption Spectra
actinide series
percent composition
47. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Group 6A
Group 4A
effective nuclear charge
gram equivalent weight
48. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
pH
Titration
Rydberg constant
49. Numbers that specify the properties of atomic orbitals and of their electrons
Lewis acid base reaction
quantum numbers
Reaction mechanism
Ground state
50. 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
Formal Charge
Triple point
Ionization energy
Emperical Formula