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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. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Phase diagram
Arrhenius Definition
STP
Half equivalence point
2. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Molar solubility
Magnetic quantum number
bond energy
3. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Pauli exclusion principle
Diffusion
Ion product
4. The lowest allowable energy state of an atom
Rydberg constant
Proton
Ground state
Half equivalence point
5. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Conjugate acids and Bases
Theoretical yield
London forces
6. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Acid dissociation constant
quantum
Ionic Bond
Ion product
7. Slightly less reactive than alkali metals - comprise group II
empirical formula
Effusion
Alkaline earths
Vapor pressure
8. The percent by mass of each element in a compound
Hydrogen bonding
percent composition
Resonance structure
redox reaction
9. Two or more atoms held together by covalent bonds
molecule
Arrhenius Definition
atomic radius
quanta
10. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Acid dissociation constant
Reaction mechanism
Net ionic equation
Conjugate acids and Bases
11. 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.
Atomic absorption Spectra
subshell
gram equivalent weight
Concentration
12. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Rate determining step
effective nuclear charge
Halogens
13. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Planck's Constant
redox reaction
Network covalent
Combination Reaction
14. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Molarity
Triple point
molecular weight
Solubility Product Constant
15. 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
Electrolyte
Triple point
Proton
Group 6A
16. 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
Lewis definition
Diffusion
Mass number
Ionization energy
17. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
electron affinity
Avagadros number
Activation energy
Atomic weight
18. A definite stable energy that a physical system can have
Decomposition reaction
Group 5A
energy state
Formal Charge
19. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Group 1A
Henderson Hasselbalch Equation
Planck's Constant
Intermolecular forces
20. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
effective nuclear charge
Common ion effect
theoretical yield
Ion
21. In a solution - the substance that dissolves in the solvent
heisenberg uncertainty principle
Water dissociation Constant
amorphous solid
Solute
22. Chalcogens - - Oxide O
Group 6A
Vapor pressure
Solvent
Bronsted - Lowry definition
23. A horizontal row of elements in the periodic table
Period
Decomposition reaction
chemical reaction
redox reaction
24. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Magnetic quantum number
Lewis definition
electromagnetic energy of photons emmited from electrons at ground state
atomic emission spectrum
25. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Activation energy
transition elements
Group 7A
26. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
quantum
Redox Half Reaction
Molarity
Formula weight
27. An ionic compound that resists changes in its pH
Neutron
Noble gases
Solubility Product Constant
Buffer
28. 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
Solvent
Halogens
Reaction mechanism
29. 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
single displacement reaction
Rate determining step
Resonance structure
law of constant composition
30. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
atomic radius
Collision theory of chemical Kinetics
STP
Avagadros number
31. 5 valence electrons -3 ions - Nitride N
energy state
Group 5A
chemical reaction
Strong acid
32. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
molecule
physical reaction
Ion
Lyman series
33. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lyman series
bond length
Lewis acid base reaction
Spin quantum number
34. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Graham's Law
Ion
quanta
Chemical Kinetics
35. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Bronsted - Lowry definition
gram equivalent weight
azimuthal quantum number
electrolysis
36. The maximum amount of product that can be produced from a given amount of reactant
Redox Half Reaction
theoretical yield
Diffusion
bond energy
37. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Graham's Law
redox reaction
Theoretical yield
38. 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
Principle quantum number
Intermolecular forces
Nucleus
Solution equilibrium
39. 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.
percent composition
bond length
Equivalence point
s orbital
40. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Conjugate acids and Bases
Atomic weight
hydrogen bonding
polymer
41. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Spin quantum number
Concentration
Covalent Bond
quantum
42. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
quanta
electron configuration
Atomic absorption Spectra
43. 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.
Atomic weight
Effective nuclear charge
s orbital
Group 1A
44. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
polymer
Molality
Principle quantum number
Dipole
45. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
quantum
heisenberg uncertainty principle
Dispersion Forces
Dipole
46. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
redox reaction
Normality
Resonance structure
47. 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-
Water dissociation Constant
Octet Rule
Rate determining step
Nonpolar covalent bond
48. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
theoretical yield
Avagadros number
polymer
Ionic Bond
49. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
solvation
Dipole Dipole interaction
Buffer
Lewis structure
50. 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
Network covalent
Arrhenius Definition
Theoretical yield