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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. The lowest allowable energy state of an atom
Vapor pressure
Ionic Bond
Ground state
Avagadros number
2. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Le chateliers Principle
Formula weight
molecular weight
Titration
3. 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
Neutron
angular momentum in the bohr model
amorphous solid
4. Simplest whole # ration of atoms in a compound
quanta
Solubility Product Constant
Raoult's Law
Emperical Formula
5. Numbers that specify the properties of atomic orbitals and of their electrons
Water dissociation Constant
Strong acid
quantum numbers
electron affinity
6. A definite stable energy that a physical system can have
lathanide series
Formal Charge
energy state
hydrogen bonding
7. Named after their cation and anion
empirical formula
theoretical yield
ionic cmpound
Lyman series
8. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Planck's Constant
Reaction mechanism
electrolysis
Noble gases
9. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
single displacement reaction
Chemical Kinetics
representative elements
10. 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.
Nonpolar covalent bond
Dipole Dipole interaction
s orbital
Ion product
11. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
lathanide series
bond length
Atomic absorption Spectra
12. 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.
Neutralization reaction
Solubility Product Constant
polymer
Reaction mechanism
13. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Raoult's Law
Noble gases
Molecular orbital
14. 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
Nucleus
Spin quantum number
Lyman series
Magnetic quantum number
15. The process by which one or more substances change to produce one or more different substances
molecular weight
Balmer series
Charles and Gay Lussac's Law
chemical reaction
16. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
electron configuration
Water dissociation Constant
und's rule
Henderson Hasselbalch Equation
17. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Rate determining step
periodic trends
electron configuration
Nonpolar covalent bond
18. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Disproportionation
Network covalent
Redox Half Reaction
Triple point
19. 5 valence electrons -3 ions - Nitride N
Group 5A
amorphous solid
transition elements
Spin quantum number
20. A solution in which water is the solvent
single displacement reaction
Reaction mechanism
Aqueous Solution
Hydrogen bonding
21. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Bronsted Lowry
Net ionic equation
Atomic absorption Spectra
periodic trends
22. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
molecule
Rydberg constant
Network covalent
Noble gases
23. 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
Solution equilibrium
Covalent Bond
24. 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
London forces
Henry's Law
Dipole
25. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
single displacement reaction
Strong acid
heisenberg uncertainty principle
26. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Diprotic Base
London forces
Bronsted - Lowry definition
redox reaction
27. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
London forces
solvation
quantum
mole
28. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Combination Reaction
Molar solubility
Net ionic equation
Proton
29. 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.
Diprotic Base
bond length
Redox Half Reaction
atomic radius
30. Tells you how much solute is present compared to the amount of solvent
Ion dipole interactions
Resonance structure
Concentration
Le chateliers Principle
31. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
physical reaction
hydrogen bonding
VSEPR
Conjugate acids and Bases
32. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Amphoteric
Bronsted - Lowry definition
Theoretical yield
Combination Reaction
33. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
ionic cmpound
Magnetic quantum number
Bronsted - Lowry definition
lewis base
34. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Colligative properties
Molarity
amorphous solid
lathanide series
35. Elements in the middle of the periodic table - in groups 3-12.
electromagnetic energy of photons emmited from electrons at ground state
representative elements
Noble gases
transition elements
36. The energy required to break a chemical bond and form neutral isolated atoms
solvation
Raoult's Law
Network covalent
bond energy
37. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Group 6A
Solubility Product Constant
d orbital
Atomic weight
38. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
39. 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
Ionic Bond
s orbital
representative elements
Spin quantum number
40. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
Group 1A
pI
Lewis structure
41. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Ion
Reaction mechanism
quantum numbers
compound
42. 5 different orbitals shaped like clover leaves and max electrons is 10
atomic radius
Nucleus
Ion
d orbital
43. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Lewis acid base reaction
molecular weight
percent composition
solvation
44. 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
Le chateliers Principle
molecule
Group 2A
Colligative properties
45. 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
atomic radius
Proton
Equilibrium
46. Rare earth element group (elements 58-71)
atomic radius
lathanide series
Planck's Constant
Vapor pressure
47. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
actinide series
Henry's Law
subshell
48. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Conjugate acids and Bases
Triple point
Reaction order
49. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Alkaline earths
Ionic Bond
Colligative properties
50. 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
Group 4A
Decomposition reaction
chemical reaction