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. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Lewis structure
pI
Solubility Product Constant
2. Simplest whole # ration of atoms in a compound
Emperical Formula
Group 5A
Magnetic quantum number
bond energy
3. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Alkaline earths
solvation
Ion
4. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
atomic emission spectrum
Lewis acid base reaction
Octet Rule
electron configuration
5. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Pauli exclusion principle
Equilibrium
Activation energy
6. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Dispersion Forces
Molar solubility
ionic cmpound
7. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Le chateliers Principle
Reaction order
Neutralization reaction
Nucleus
8. The percent by mass of each element in a compound
Le chateliers Principle
percent composition
molecule
Molality
9. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Ionization energy
Pauli exclusion principle
Free radical
lewis base
10. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Formal Charge
Period
Hydrogen bonding
11. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
atomic emission spectrum
Formula weight
percent composition
Strong acid
12. A horizontal row of elements in the periodic table
percent composition
Atomic absorption Spectra
bond energy
Period
13. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Molarity
Common ion effect
Period
14. An atom or group of atoms that has a positive or negative charge
Acid dissociation constant
Resonance structure
quantum
Ion
15. 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
chemical reaction
Alkaline earths
Henry's Law
16. 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
Resonance structure
Percent yield
Nucleus
Network covalent
17. Rare earth element group (elements 58-71)
atomic radius
lathanide series
Molar solubility
Henry's Law
18. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Amphoteric
Reaction mechanism
Combination Reaction
Common ion effect
19. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
Alkaline earths
Atomic absorption Spectra
electrolysis
20. 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
Lewis definition
Activation energy
Reaction order
Dispersion Forces
21. 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
representative elements
redox reaction
Avagadros number
Solution equilibrium
22. PH of a molecule at which it contains no net electric charge - isoelectric point.
periodic trends
pI
Lewis acid base reaction
compound
23. 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
atomic radius
Atomic weight
angular momentum in the bohr model
24. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
25. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Neutralization reaction
chemical reaction
Equlibrium constant
26. 5 valence electrons -3 ions - Nitride N
Group 5A
The bohr model
d orbital
solvation
27. A solution in which water is the solvent
Aqueous Solution
Henry's Law
subshell
indicator
28. Having characteristics of both an acid and a base and capable of reacting as either
Group 7A
Amphoteric
Aqueous Solution
STP
29. 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
Equlibrium constant
Avagadros number
London forces
Colligative properties
30. 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.
crystalline solid
Phase diagram
quantum numbers
Group 7A
31. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
heisenberg uncertainty principle
solvation
Rate determining step
Molar solubility
32. 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
Ionization energy
Intermolecular forces
Common ion effect
physical reaction
33. 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
Period
Ionic Bond
STP
Percent composition
34. 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
Spin quantum number
ionic cmpound
Resonance structure
Conjugate acids and Bases
35. 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.
Group 6A
VSEPR
Ionization energy
atomic radius
36. 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
electromagnetic energy of photons emmited from electrons at ground state
Theoretical yield
Proton
quantum numbers
37. Chalcogens - - Oxide O
quantum
Redox Half Reaction
Nucleus
Group 6A
38. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Neutralization reaction
Triple point
Group 7A
Octet Rule
39. 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
40. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
percent composition
Equilibrium
Solution equilibrium
41. 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
periodic trends
Reaction order
Acid dissociation constant
Bronsted - Lowry definition
42. 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.
VSEPR
Principle quantum number
Electrolyte
Reaction order
43. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
Conjugate acids and Bases
Net ionic equation
Half equivalence point
44. A solid made up of particles that are not arranged in a regular pattern.
Strong acid
amorphous solid
Solute
redox reaction
45. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Spin quantum number
Effusion
Dispersion Forces
Water dissociation Constant
46. A base that can accept two moles of H+ per mole of itself (ex: SO4
Group 6A
Reaction order
Rate determining step
Diprotic Base
47. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Equilibrium
Ionization energy
effective nuclear charge
indicator
48. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Group 5A
periodic trends
atomic radius
Ion product
49. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Acid dissociation constant
Neutralization reaction
quantum numbers
50. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
pH
Diffusion
molecular weight
law of constant composition