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. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Lyman series
Solubility Product Constant
Disproportionation
Octet Rule
2. Named after their cation and anion
crystalline solid
Molecular orbital
Neutralization reaction
ionic cmpound
3. The lowest allowable energy state of an atom
STP
Covalent Bond
Ground state
lathanide series
4. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Principle quantum number
Aqueous Solution
decomposition reaction
Le chateliers Principle
5. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
The bohr model
Pauli exclusion principle
Intermolecular forces
mole
6. Elements in the middle of the periodic table - in groups 3-12.
Avagadros number
Reaction order
Percent yield
transition elements
7. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
bond energy
single displacement reaction
molecular weight
Bronsted Lowry
8. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Ground state
Lewis definition
Solvent
atomic radius
9. 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
Aqueous Solution
Ionization energy
Dipole Dipole interaction
10. 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
Titration
Nonpolar covalent bond
Buffer
Dispersion Forces
11. Substance in which a solute is dissolved to form a solution
Vapor pressure
Group 7A
Solvent
redox reaction
12. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Equivalence point
Dipole
representative elements
redox reaction
13. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Common ion effect
solvation
Concentration
14. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Emperical Formula
indicator
Buffer
molecule
15. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Planck's Constant
Noble gases
bond length
Le chateliers Principle
16. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Neutralization reaction
effective nuclear charge
Group 3A
London forces
17. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Equilibrium
Ionic Bond
Solute
Equivalence point
18. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
energy state
Henderson Hasselbalch Equation
Decomposition reaction
19. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Decomposition reaction
Rydberg constant
Acid dissociation constant
20. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Common ion effect
Electrolyte
single displacement reaction
21. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Magnetic quantum number
Activation energy
Solubility Product Constant
Percent yield
22. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Molality
law of constant composition
electromagnetic energy of photons emmited from electrons at ground state
electron affinity
23. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
actinide series
Group 2A
Molecular orbital
effective nuclear charge
24. The process by which one or more substances change to produce one or more different substances
sigma bond
chemical reaction
Covalent Bond
compound
25. 2.18 x 10^-18 J/electron
Molar solubility
Effective nuclear charge
Henry's Law
Rydberg constant
26. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Charles and Gay Lussac's Law
Molality
Formula weight
27. A horizontal row of elements in the periodic table
Period
single displacement reaction
Magnetic quantum number
Concentration
28. The Percent by mass of each element in a compound.
Intermolecular forces
Neutron
Reaction mechanism
Percent composition
29. The average distance between the nuclei of two bonded atoms
bond length
decomposition reaction
Aqueous Solution
Bronsted - Lowry definition
30. Any sample of a given compound will contain the same elements in the identical mass ratio.
Alkaline earths
Ground state
law of constant composition
Theoretical yield
31. Common definition of acids as proton (H+) donors and bases as proton acceptors
Solute
Solvent
Triple point
Bronsted - Lowry definition
32. Chalcogens - - Oxide O
Diprotic Base
Planck's Constant
energy state
Group 6A
33. 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
Water dissociation Constant
Collision theory of chemical Kinetics
Percent composition
34. (chemistry) p(otential of) H(ydrogen)
ionic cmpound
pH
heisenberg uncertainty principle
angular momentum in the bohr model
35. 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.
Electronegativity
crystalline solid
Ion
Henderson Hasselbalch Equation
36. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
pI
Avagadros number
Diffusion
Vapor pressure
37. 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
redox reaction
Proton
Ion
Henry's Law
38. A solid made up of particles that are not arranged in a regular pattern.
empirical formula
Period
amorphous solid
Acid dissociation constant
39. 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.
Vapor pressure
polymer
Group 3A
Ionic Bond
40. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
effective nuclear charge
Atomic absorption Spectra
polymer
pi bonds
41. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Lewis definition
Atomic weight
Network covalent
Covalent Bond
42. An atom or group of atoms that has a positive or negative charge
Equivalence point
Henderson Hasselbalch Equation
electrolysis
Ion
43. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Combination Reaction
Molarity
actinide series
Mass number
44. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
amorphous solid
Alkaline earths
Avagadros number
45. The energy required to break a chemical bond and form neutral isolated atoms
Avagadros number
bond energy
heisenberg uncertainty principle
Net ionic equation
46. 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
47. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
azimuthal quantum number
Ionic Bond
subshell
48. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Diffusion
theoretical yield
Collision theory of chemical Kinetics
Ion dipole interactions
49. The slowest elementary step which is the limit for the rate of the other steps
indicator
atomic theory
Aqueous Solution
Rate determining step
50. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183