SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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 fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
2. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Electrolyte
molecular weight
Atomic weight
azimuthal quantum number
3. 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.
Alkaline earths
single displacement reaction
redox reaction
atomic radius
4. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Activation energy
Dipole
quantum
Graham's Law
5. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Concentration
Disproportionation
Ionization energy
redox reaction
6. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
7. Redox reaction - in which the same species is both oxidized and reduced.
Ground state
Water dissociation Constant
Hydrogen bonding
Disproportionation
8. 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
Proton
Resonance structure
Nucleus
Vapor pressure
9. 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
Diprotic Base
representative elements
Network covalent
Pauli exclusion principle
10. 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.
Theoretical yield
Group 4A
Combination Reaction
Henderson Hasselbalch Equation
11. In a solution - the substance that dissolves in the solvent
Lewis structure
Solution equilibrium
quantum numbers
Solute
12. 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
transition elements
Atomic absorption Spectra
Theoretical yield
Magnetic quantum number
13. Elements in the middle of the periodic table - in groups 3-12.
Atomic absorption Spectra
transition elements
London forces
Aqueous Solution
14. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Magnetic quantum number
Ion
gram equivalent weight
und's rule
15. Named after their cation and anion
Equlibrium constant
ionic cmpound
Spin quantum number
Diprotic Base
16. 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
Principle quantum number
electron configuration
London forces
Resonance structure
17. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
18. 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
Arrhenius Definition
Lewis acid base reaction
Emperical Formula
und's rule
19. A horizontal row of elements in the periodic table
Dipole Dipole interaction
Redox Half Reaction
Period
Reaction order
20. The percent by mass of each element in a compound
atomic radius
percent composition
bond energy
periodic trends
21. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Group 5A
Molar solubility
Molarity
transition elements
22. E=hc/?
electromagnetic energy of photons emmited from electrons at ground state
Proton
Effective nuclear charge
Combination Reaction
23. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Bronsted Lowry
Acid dissociation constant
hydrogen bonding
24. Common definition of acids as proton (H+) donors and bases as proton acceptors
Arrhenius Definition
Group 4A
Bronsted - Lowry definition
Spin quantum number
25. A substance that - when dissolved in water - results in a solution that can conduct electricity
STP
Electrolyte
atomic radius
Lyman series
26. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Percent composition
actinide series
molecule
27. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Combination Reaction
Reaction mechanism
Lewis definition
electron affinity
28. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Activation energy
Le chateliers Principle
pH
Common ion effect
29. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Phase diagram
Group 1A
Group 7A
30. Simplest whole # ration of atoms in a compound
Neutron
Group 1A
Emperical Formula
Combination Reaction
31. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Solution equilibrium
Molality
Lewis definition
32. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
indicator
Acid dissociation constant
Water dissociation Constant
solvation
33. Chalcogens - - Oxide O
Group 6A
Group 5A
Rate determining step
Molecular orbital
34. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Arrhenius Definition
Intermolecular forces
Magnetic quantum number
Percent composition
35. Small discrete increments of energy.
Rate law
quanta
Graham's Law
und's rule
36. Numbers that specify the properties of atomic orbitals and of their electrons
Percent composition
mole
quantum numbers
Solute
37. The lowest allowable energy state of an atom
amorphous solid
Mass number
Ground state
Reaction order
38. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
percent composition
quantum numbers
Ion product
Electronegativity
39. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Combination Reaction
Resonance structure
lewis base
single displacement reaction
40. An elementary particle with 0 charge and mass about equal to a proton
indicator
Neutron
Rydberg constant
Electronegativity
41. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Colligative properties
Proton
polymer
subshell
42. 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.
Rydberg constant
Balmer series
electron affinity
Diffusion
43. 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
Normality
Network covalent
VSEPR
44. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
atomic radius
effective nuclear charge
Molecular orbital
Mass number
45. 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 7A
electromagnetic energy of photons emmited from electrons at ground state
crystalline solid
Lewis acid base reaction
46. 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
Bronsted - Lowry definition
transition elements
Charles and Gay Lussac's Law
47. 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
Group 6A
hydrogen bonding
redox reaction
crystalline solid
48. Two or more atoms held together by covalent bonds
Decomposition reaction
ionic cmpound
Formula weight
molecule
49. 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
Conjugate acids and Bases
ionic cmpound
Dipole
50. Substance in which a solute is dissolved to form a solution
solvation
Nucleus
Solvent
law of constant composition