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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. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Octet Rule
Halogens
Bronsted - Lowry definition
solvation
2. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Solubility Product Constant
Vapor pressure
Diprotic Base
electron configuration
3. 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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4. 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
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5. 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.
Redox Half Reaction
Common ion effect
effective nuclear charge
Collision theory of chemical Kinetics
6. 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
amorphous solid
law of constant composition
VSEPR
7. 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
Solubility Product Constant
empirical formula
Water dissociation Constant
Resonance structure
8. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Equlibrium constant
decomposition reaction
percent composition
9. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
physical reaction
Avagadros number
Pauli exclusion principle
chemical reaction
10. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Equlibrium constant
gram equivalent weight
Solvent
Lewis acid base reaction
11. The process of decomposing a chemical compound by the passage of an electric current.
Atomic weight
electrolysis
Nonpolar covalent bond
electron configuration
12. 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
Aqueous Solution
electrolysis
hydrogen bonding
Charles and Gay Lussac's Law
13. (chemistry) p(otential of) H(ydrogen)
pH
Neutron
Combination Reaction
Lewis structure
14. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
subshell
Rydberg constant
Henry's Law
15. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Magnetic quantum number
polymer
Electronegativity
quantum
16. 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
Hydrogen bonding
Group 2A
Principle quantum number
Redox Half Reaction
17. 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.
Aqueous Solution
Triple point
VSEPR
Spin quantum number
18. A definite stable energy that a physical system can have
bond energy
single displacement reaction
Percent yield
energy state
19. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Henry's Law
Strong acid
Percent yield
Free radical
20. The Percent by mass of each element in a compound.
Neutralization reaction
Formal Charge
molecular weight
Percent composition
21. In a solution - the substance that dissolves in the solvent
Solute
Equilibrium
und's rule
electron affinity
22. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Pauli exclusion principle
Free radical
Arrhenius Definition
atomic emission spectrum
23. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
Magnetic quantum number
Planck's Constant
Buffer
24. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Solubility Product Constant
pi bonds
Common ion effect
Group 1A
25. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
lathanide series
Normality
law of constant composition
electron configuration
26. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Rate determining step
indicator
Electrolyte
single displacement reaction
27. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Hydrogen bonding
crystalline solid
empirical formula
The bohr model
28. The slowest elementary step which is the limit for the rate of the other steps
Chemical Kinetics
Rate determining step
Titration
Proton
29. 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
Effective nuclear charge
Dispersion Forces
Group 3A
subshell
30. A subdivision of an energy level in an atom. They are divided into orbitals.
percent composition
Lewis acid base reaction
Rate law
subshell
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
Dipole
single displacement reaction
Triple point
Group 1A
32. 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
Group 3A
Decomposition reaction
Group 4A
33. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Solute
Conjugate acids and Bases
Solvent
Group 1A
34. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
azimuthal quantum number
Theoretical yield
Principle quantum number
Lyman series
35. A solution in which water is the solvent
Aqueous Solution
Formula weight
Ion
Proton
36. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Covalent Bond
decomposition reaction
Henderson Hasselbalch Equation
compound
37. 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
Molar solubility
Halogens
Spin quantum number
Octet Rule
38. Small discrete increments of energy.
molecular weight
quanta
quantum
Ion
39. Any sample of a given compound will contain the same elements in the identical mass ratio.
single displacement reaction
law of constant composition
Formal Charge
Combination Reaction
40. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
actinide series
Neutralization reaction
Dispersion Forces
Mass number
41. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Dipole Dipole interaction
electron configuration
Common ion effect
42. Rare earth element group (elements 58-71)
Chemical Kinetics
Alkaline earths
lathanide series
Halogens
43. 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
Dispersion Forces
Group 7A
Atomic weight
Colligative properties
44. An ionic compound that resists changes in its pH
representative elements
Buffer
pi bonds
Acid dissociation constant
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
Equilibrium
Ion dipole interactions
Spin quantum number
Proton
46. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Dispersion Forces
Free radical
energy state
und's rule
47. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Disproportionation
Network covalent
pI
Raoult's Law
48. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Equivalence point
Decomposition reaction
Effusion
Group 3A
49. 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-
Lyman series
Dispersion Forces
indicator
Water dissociation Constant
50. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
polymer
Neutralization reaction
subshell
Le chateliers Principle