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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. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Reaction mechanism
Diffusion
atomic radius
angular momentum in the bohr model
2. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
Balmer series
Planck's Constant
Reaction mechanism
3. Any sample of a given compound will contain the same elements in the identical mass ratio.
s orbital
Ionization energy
law of constant composition
Ground state
4. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Aqueous Solution
Solute
STP
5. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Buffer
Free radical
indicator
Effusion
6. A solution in which water is the solvent
Octet Rule
Equlibrium constant
Aqueous Solution
Lewis structure
7. 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
Rate determining step
Nonpolar covalent bond
molecular weight
The bohr model
8. 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
London forces
electron affinity
The bohr model
Group 6A
9. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Ion dipole interactions
Le chateliers Principle
solvation
heisenberg uncertainty principle
10. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
Halogens
mole
Decomposition reaction
11. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
physical reaction
polymer
Octet Rule
12. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Formal Charge
Pauli exclusion principle
solvation
Molarity
13. The process by which one or more substances change to produce one or more different substances
Rate law
chemical reaction
Ion
Raoult's Law
14. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
electromagnetic energy of photons emmited from electrons at ground state
Molecular orbital
subshell
quantum numbers
15. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
electrolysis
Group 2A
bond energy
redox reaction
16. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
polymer
transition elements
Reaction mechanism
atomic emission spectrum
17. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
lewis base
Neutron
Electronegativity
Formal Charge
18. 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
quantum numbers
Group 7A
Arrhenius Definition
Planck's Constant
19. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Lewis acid base reaction
Rate law
Group 2A
Free radical
20. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Equivalence point
Reaction order
Rate determining step
Solubility Product Constant
21. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Solvent
Activation energy
crystalline solid
Half equivalence point
22. 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.
Activation energy
polymer
Effective nuclear charge
atomic radius
23. 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.
heisenberg uncertainty principle
Rate law
lewis base
Henderson Hasselbalch Equation
24. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
periodic trends
Lewis acid base reaction
percent composition
Effusion
25. 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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26. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
Group 4A
Raoult's Law
Ion
crystalline solid
27. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Balmer series
Group 1A
empirical formula
solvation
28. 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
lewis base
The bohr model
Dispersion Forces
Rydberg constant
29. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Neutron
Dipole Dipole interaction
Effusion
atomic emission spectrum
30. An atom or group of atoms that has a positive or negative charge
Emperical Formula
Ion
Hydrogen bonding
Amphoteric
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
law of constant composition
quantum numbers
Solubility Product Constant
Equlibrium constant
32. 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
Colligative properties
Dispersion Forces
Solubility Product Constant
The bohr model
33. 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
Decomposition reaction
Nucleus
atomic radius
Principle quantum number
34. 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
Vapor pressure
single displacement reaction
Alkaline earths
Azeotrope
35. PH of a molecule at which it contains no net electric charge - isoelectric point.
subshell
pI
Phase diagram
electron configuration
36. A solid made up of particles that are not arranged in a regular pattern.
Halogens
Effective nuclear charge
Common ion effect
amorphous solid
37. Having characteristics of both an acid and a base and capable of reacting as either
Dipole
Amphoteric
electron configuration
Diprotic Base
38. Named after their cation and anion
Equlibrium constant
Network covalent
Dipole Dipole interaction
ionic cmpound
39. Simplest whole # ration of atoms in a compound
Proton
Graham's Law
Emperical Formula
law of constant composition
40. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
atomic theory
Dipole Dipole interaction
Formula weight
Ion dipole interactions
41. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Water dissociation Constant
Group 7A
atomic radius
Equivalence point
42. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Atomic weight
Net ionic equation
Disproportionation
lathanide series
43. 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
Group 2A
Resonance structure
quantum numbers
Atomic weight
44. 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
polymer
Henderson Hasselbalch Equation
Proton
Decomposition reaction
45. The energy required to break a chemical bond and form neutral isolated atoms
Formula weight
Lyman series
bond energy
Le chateliers Principle
46. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Molar solubility
d orbital
Solution equilibrium
molecular weight
47. Gram equivalent weight of solute per liter of solution - often denoted by N.
quanta
Molality
Normality
Molar solubility
48. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Colligative properties
s orbital
Strong acid
Percent composition
49. Chalcogens - - Oxide O
Group 6A
Alkaline earths
transition elements
Chemical Kinetics
50. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Group 2A
molecule
actinide series
Molar solubility