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 substance that - when dissolved in water - results in a solution that can conduct electricity
lewis base
Electrolyte
Molar solubility
Ion
2. A definite stable energy that a physical system can have
energy state
Ion product
Ionization energy
Reaction order
3. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
single displacement reaction
Rate law
Lewis structure
indicator
4. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Rate law
Hydrogen bonding
Net ionic equation
Neutralization reaction
5. Chalcogens - - Oxide O
Group 6A
Effusion
percent composition
Alkaline earths
6. Small discrete increments of energy.
Ground state
Combination Reaction
quanta
Molecular orbital
7. A reaction in which atoms of one element take the place of atoms of another element in a compound
lewis base
single displacement reaction
Bronsted Lowry
und's rule
8. 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
Principle quantum number
Dispersion Forces
single displacement reaction
indicator
9. The energy required to break a chemical bond and form neutral isolated atoms
atomic emission spectrum
Intermolecular forces
Network covalent
bond energy
10. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Graham's Law
Lewis definition
Equlibrium constant
pH
11. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Neutron
Titration
Rate law
redox reaction
12. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
Redox Half Reaction
Aqueous Solution
Group 5A
13. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
14. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
solvation
Amphoteric
Proton
15. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
sigma bond
representative elements
Resonance structure
Phase diagram
16. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
compound
pi bonds
Group 2A
Ion dipole interactions
17. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Equlibrium constant
Collision theory of chemical Kinetics
electrolysis
18. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
theoretical yield
redox reaction
bond energy
Mass number
19. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
redox reaction
Theoretical yield
Le chateliers Principle
Rydberg constant
20. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Ion dipole interactions
Strong acid
effective nuclear charge
Graham's Law
21. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Triple point
Concentration
Noble gases
Chemical Kinetics
22. 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
periodic trends
Rate law
Molar solubility
23. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Effective nuclear charge
Reaction mechanism
solvation
electron configuration
24. A reaction where a compound does Not change its molecular structure.
Group 4A
Atomic absorption Spectra
physical reaction
Solvent
25. Temperature is constant; effusion and temperature are proportional to the square root of their masses
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
26. An elementary particle with 0 charge and mass about equal to a proton
Neutron
empirical formula
Ion product
Magnetic quantum number
27. An ionic compound that resists changes in its pH
quantum
Buffer
Free radical
Titration
28. 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.
Atomic weight
Ground state
hydrogen bonding
Henderson Hasselbalch Equation
29. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
representative elements
Rate law
Covalent Bond
atomic radius
30. 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.
Balmer series
pI
sigma bond
STP
31. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Formula weight
Network covalent
Emperical Formula
Triple point
32. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Strong acid
electron affinity
Hydrogen bonding
Electronegativity
33. 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
Equlibrium constant
Chemical Kinetics
Ion
ionic cmpound
34. A horizontal row of elements in the periodic table
Period
Half equivalence point
chemical reaction
Henderson Hasselbalch Equation
35. 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.
Dipole
angular momentum in the bohr model
Molar solubility
Effective nuclear charge
36. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Henderson Hasselbalch Equation
Ion dipole interactions
Charles and Gay Lussac's Law
atomic theory
37. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Atomic weight
Percent composition
heisenberg uncertainty principle
38. 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
energy state
Solubility Product Constant
Octet Rule
39. 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.
transition elements
Avagadros number
Combination Reaction
crystalline solid
40. An atom or group of atoms that has a positive or negative charge
quanta
molecule
Resonance structure
Ion
41. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
STP
Chemical Kinetics
Lewis acid base reaction
effective nuclear charge
42. 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.
representative elements
Ion
Group 3A
Noble gases
43. 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.
Dipole
atomic radius
Magnetic quantum number
Equivalence point
44. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
d orbital
Formula weight
energy state
subshell
45. Named after their cation and anion
single displacement reaction
ionic cmpound
Planck's Constant
Ion
46. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
London forces
Conjugate acids and Bases
Molality
Mass number
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
Formula weight
hydrogen bonding
Diffusion
Graham's Law
48. 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
Resonance structure
Molarity
und's rule
VSEPR
49. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Equilibrium
atomic theory
chemical reaction
50. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Nonpolar covalent bond
Atomic weight
Equivalence point
Common ion effect