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 solid made up of particles that are not arranged in a regular pattern.
Molar solubility
amorphous solid
Ion
Henry's Law
2. Common definition of acids as proton (H+) donors and bases as proton acceptors
molecular weight
und's rule
Percent yield
Bronsted - Lowry definition
3. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Common ion effect
Combination Reaction
Molarity
Ionization energy
4. 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
atomic theory
Common ion effect
Proton
lewis base
5. A reaction where a compound does Not change its molecular structure.
Effective nuclear charge
physical reaction
Acid dissociation constant
Mass number
6. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Collision theory of chemical Kinetics
Henry's Law
electrolysis
Network covalent
7. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
atomic radius
Rate law
Formal Charge
Decomposition reaction
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
Mass number
Dispersion Forces
empirical formula
9. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Phase diagram
Vapor pressure
Percent yield
physical reaction
10. 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
11. 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
Dispersion Forces
Neutron
heisenberg uncertainty principle
Pauli exclusion principle
12. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
solvation
Conjugate acids and Bases
Halogens
mole
13. 5 valence electrons -3 ions - Nitride N
Dispersion Forces
heisenberg uncertainty principle
Diffusion
Group 5A
14. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Solute
heisenberg uncertainty principle
Nonpolar covalent bond
Triple point
15. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Net ionic equation
Water dissociation Constant
Dipole
Equilibrium
16. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Rate law
empirical formula
decomposition reaction
Formula weight
17. Sum of the protons and neutrons in an element often denoted by the letter A
Conjugate acids and Bases
Concentration
Mass number
Ionic Bond
18. 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
crystalline solid
Rate determining step
Formula weight
hydrogen bonding
19. 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
20. 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
The bohr model
Neutralization reaction
Electrolyte
Amphoteric
21. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Collision theory of chemical Kinetics
single displacement reaction
decomposition reaction
pH
22. In a solution - the substance that dissolves in the solvent
representative elements
Electrolyte
Solute
Pauli exclusion principle
23. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
Intermolecular forces
Group 2A
transition elements
24. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Acid dissociation constant
Redox Half Reaction
Avagadros number
Solvent
25. 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.
sigma bond
Equivalence point
atomic radius
Solvent
26. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Magnetic quantum number
crystalline solid
Balmer series
27. 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
law of constant composition
Ion product
Group 7A
gram equivalent weight
28. 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.
Solubility Product Constant
Ion product
atomic radius
The bohr model
29. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Electronegativity
pi bonds
Solvent
London forces
30. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Group 7A
Ion
Molecular orbital
31. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Group 2A
Solute
compound
actinide series
32. The lowest allowable energy state of an atom
Ground state
Pauli exclusion principle
Percent yield
electron configuration
33. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
Effective nuclear charge
Principle quantum number
Resonance structure
Graham's Law
34. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
azimuthal quantum number
lathanide series
Covalent Bond
Azeotrope
35. 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
Conjugate acids and Bases
Nucleus
Percent yield
Ground state
36. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Net ionic equation
molecular weight
Magnetic quantum number
Reaction mechanism
37. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
single displacement reaction
Neutralization reaction
Acid dissociation constant
STP
38. E=hc/?
electromagnetic energy of photons emmited from electrons at ground state
polymer
azimuthal quantum number
Planck's Constant
39. A solution in which water is the solvent
empirical formula
Azeotrope
Aqueous Solution
redox reaction
40. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Net ionic equation
electron configuration
Lewis acid base reaction
percent composition
41. The percent by mass of each element in a compound
hydrogen bonding
chemical reaction
percent composition
Equivalence point
42. A definite stable energy that a physical system can have
Group 6A
energy state
representative elements
Nucleus
43. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
The bohr model
Electronegativity
sigma bond
Half equivalence point
44. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
pH
Bronsted - Lowry definition
Group 4A
lewis base
45. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Atomic weight
Emperical Formula
Net ionic equation
Theoretical yield
46. Any sample of a given compound will contain the same elements in the identical mass ratio.
percent composition
atomic theory
Balmer series
law of constant composition
47. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
decomposition reaction
electrolysis
Reaction mechanism
energy state
48. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Ion
physical reaction
Proton
redox reaction
49. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Ionic Bond
Network covalent
Equilibrium
50. 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.
angular momentum in the bohr model
atomic radius
Buffer
Intermolecular forces
Sorry!:) No result found.
Can you answer 50 questions in 15 minutes?
Let me suggest you:
Browse all subjects
Browse all tests
Most popular tests
Major Subjects
Tests & Exams
AP
CLEP
DSST
GRE
SAT
GMAT
Certifications
CISSP go to https://www.isc2.org/
PMP
ITIL
RHCE
MCTS
More...
IT Skills
Android Programming
Data Modeling
Objective C Programming
Basic Python Programming
Adobe Illustrator
More...
Business Skills
Advertising Techniques
Business Accounting Basics
Business Strategy
Human Resource Management
Marketing Basics
More...
Soft Skills
Body Language
People Skills
Public Speaking
Persuasion
Job Hunting And Resumes
More...
Vocabulary
GRE Vocab
SAT Vocab
TOEFL Essential Vocab
Basic English Words For All
Global Words You Should Know
Business English
More...
Languages
AP German Vocab
AP Latin Vocab
SAT Subject Test: French
Italian Survival
Norwegian Survival
More...
Engineering
Audio Engineering
Computer Science Engineering
Aerospace Engineering
Chemical Engineering
Structural Engineering
More...
Health Sciences
Basic Nursing Skills
Health Science Language Fundamentals
Veterinary Technology Medical Language
Cardiology
Clinical Surgery
More...
English
Grammar Fundamentals
Literary And Rhetorical Vocab
Elements Of Style Vocab
Introduction To English Major
Complete Advanced Sentences
Literature
Homonyms
More...
Math
Algebra Formulas
Basic Arithmetic: Measurements
Metric Conversions
Geometric Properties
Important Math Facts
Number Sense Vocab
Business Math
More...
Other Major Subjects
Science
Economics
History
Law
Performing-arts
Cooking
Logic & Reasoning
Trivia
Browse all subjects
Browse all tests
Most popular tests