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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. 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
Balmer series
Solution equilibrium
Electronegativity
Dispersion Forces
2. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
transition elements
Molar solubility
Intermolecular forces
law of constant composition
3. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Molecular orbital
Lewis acid base reaction
Group 1A
Avagadros number
4. 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.
redox reaction
sigma bond
Henderson Hasselbalch Equation
d orbital
5. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Concentration
STP
azimuthal quantum number
Nucleus
6. 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.
Solubility Product Constant
energy state
electromagnetic energy of photons emmited from electrons at ground state
Effective nuclear charge
7. The slowest elementary step which is the limit for the rate of the other steps
STP
Alkaline earths
Rate determining step
electron configuration
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
Pauli exclusion principle
Theoretical yield
London forces
solvation
9. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Percent yield
Formal Charge
heisenberg uncertainty principle
Redox Half Reaction
10. 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
Spin quantum number
molecular weight
Pauli exclusion principle
11. A solid made up of particles that are not arranged in a regular pattern.
Lyman series
amorphous solid
Activation energy
Pauli exclusion principle
12. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
hydrogen bonding
Avagadros number
Rate determining step
Molar solubility
13. 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
Decomposition reaction
Ionization energy
Redox Half Reaction
Charles and Gay Lussac's Law
14. A dynamic condition in which two opposing changes occur at equal rates in a closed system
bond length
Equilibrium
Dipole
Diprotic Base
15. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
empirical formula
Nucleus
heisenberg uncertainty principle
16. 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
sigma bond
transition elements
Atomic absorption Spectra
Azeotrope
17. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
London forces
decomposition reaction
gram equivalent weight
Equlibrium constant
18. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Pauli exclusion principle
gram equivalent weight
molecular weight
Phase diagram
19. 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
Ionic Bond
Network covalent
Alkaline earths
20. The energy required to break a chemical bond and form neutral isolated atoms
Halogens
pI
bond energy
pH
21. The lowest allowable energy state of an atom
Atomic absorption Spectra
Ground state
Octet Rule
Rate law
22. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Atomic weight
quantum
Molarity
bond length
23. Elements in the middle of the periodic table - in groups 3-12.
Rydberg constant
pI
Electronegativity
transition elements
24. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Principle quantum number
Titration
gram equivalent weight
Strong acid
25. Tells you how much solute is present compared to the amount of solvent
Water dissociation Constant
redox reaction
Concentration
Diprotic Base
26. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Molecular orbital
Mass number
quantum
Vapor pressure
27. 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.
subshell
Percent composition
atomic radius
Neutron
28. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
atomic emission spectrum
Common ion effect
Arrhenius Definition
periodic trends
29. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Nucleus
atomic radius
Activation energy
30. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Percent yield
Atomic weight
STP
31. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
effective nuclear charge
Bronsted Lowry
Neutralization reaction
quantum numbers
32. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Group 5A
Ion
Acid dissociation constant
Theoretical yield
33. The Percent by mass of each element in a compound.
electromagnetic energy of photons emmited from electrons at ground state
Percent composition
quantum numbers
Group 1A
34. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Halogens
quantum
Chemical Kinetics
Water dissociation Constant
35. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Henry's Law
indicator
Group 5A
STP
36. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Percent yield
Activation energy
hydrogen bonding
Lewis structure
37. The average distance between the nuclei of two bonded atoms
Period
bond energy
Molar solubility
bond length
38. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
atomic radius
Electronegativity
Combination Reaction
Principle quantum number
39. A reaction where a compound does Not change its molecular structure.
Molarity
physical reaction
Lyman series
azimuthal quantum number
40. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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41. E=hc/?
electromagnetic energy of photons emmited from electrons at ground state
und's rule
Henry's Law
Reaction mechanism
42. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
quantum numbers
Free radical
Charles and Gay Lussac's Law
compound
43. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
bond length
single displacement reaction
Dipole
Net ionic equation
44. Acids defined as electron - pair acceptors and bases as electron - pair donors.
molecule
Formula weight
Ionic Bond
Lewis definition
45. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Halogens
Neutralization reaction
actinide series
Acid dissociation constant
46. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Diprotic Base
Bronsted - Lowry definition
Lewis acid base reaction
Acid dissociation constant
47. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
London forces
atomic theory
polymer
amorphous solid
48. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Solution equilibrium
Net ionic equation
Chemical Kinetics
Equilibrium
49. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Common ion effect
atomic radius
Rate law
subshell
50. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
ionic cmpound
Resonance structure
Group 7A