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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 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
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2. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
redox reaction
Graham's Law
Collision theory of chemical Kinetics
Equilibrium
3. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
molecule
Theoretical yield
physical reaction
Reaction order
4. 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
Bronsted Lowry
Dispersion Forces
Equilibrium
Bronsted - Lowry definition
5. 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.
Effective nuclear charge
solvation
Ground state
crystalline solid
6. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Azeotrope
energy state
Ground state
Conjugate acids and Bases
7. Having characteristics of both an acid and a base and capable of reacting as either
gram equivalent weight
Amphoteric
Rydberg constant
Group 4A
8. 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.
indicator
Group 6A
Ion product
physical reaction
9. 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
amorphous solid
hydrogen bonding
single displacement reaction
subshell
10. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Ground state
decomposition reaction
Collision theory of chemical Kinetics
Noble gases
11. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
Ground state
Molecular orbital
Avagadros number
12. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Bronsted - Lowry definition
empirical formula
lathanide series
Theoretical yield
13. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Reaction mechanism
Net ionic equation
Group 6A
Decomposition reaction
14. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Conjugate acids and Bases
Combination Reaction
Neutralization reaction
lathanide series
15. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Ionic Bond
compound
Combination Reaction
16. (chemistry) a substance that changes color to indicate the presence of some ion or substance
transition elements
indicator
Concentration
und's rule
17. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
The bohr model
Henry's Law
Reaction mechanism
pI
18. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Theoretical yield
Lewis definition
Emperical Formula
Titration
19. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Collision theory of chemical Kinetics
law of constant composition
STP
atomic theory
20. The Percent by mass of each element in a compound.
London forces
lathanide series
Percent composition
Normality
21. 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
bond length
Hydrogen bonding
quantum
Pauli exclusion principle
22. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Titration
transition elements
Diffusion
atomic theory
23. Gram equivalent weight of solute per liter of solution - often denoted by N.
Lewis definition
Strong acid
quanta
Normality
24. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
atomic emission spectrum
redox reaction
Collision theory of chemical Kinetics
Halogens
25. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Dipole
Alkaline earths
Effective nuclear charge
Avagadros number
26. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
d orbital
Diffusion
Network covalent
molecular weight
27. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
Effective nuclear charge
subshell
Ground state
representative elements
28. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Rydberg constant
Common ion effect
atomic radius
subshell
29. Chalcogens - - Oxide O
crystalline solid
Group 6A
Vapor pressure
Formal Charge
30. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
redox reaction
Le chateliers Principle
Free radical
Activation energy
31. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Charles and Gay Lussac's Law
Half equivalence point
Dipole Dipole interaction
polymer
32. Two or more atoms held together by covalent bonds
bond energy
molecule
Proton
Titration
33. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
single displacement reaction
Covalent Bond
Atomic absorption Spectra
Triple point
34. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
quantum
atomic radius
Activation energy
atomic emission spectrum
35. 2.18 x 10^-18 J/electron
mole
Rydberg constant
Graham's Law
Disproportionation
36. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
indicator
Neutralization reaction
Ionization energy
Molarity
37. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
Lewis structure
The bohr model
Net ionic equation
38. 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-
Diprotic Base
periodic trends
STP
Water dissociation Constant
39. 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.
Henderson Hasselbalch Equation
Azeotrope
Solvent
VSEPR
40. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Ionization energy
pi bonds
electrolysis
Decomposition reaction
41. An atom or group of atoms that has a positive or negative charge
Ion
Percent composition
Molar solubility
pH
42. Tells you how much solute is present compared to the amount of solvent
Octet Rule
Dipole
Concentration
Planck's Constant
43. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Solubility Product Constant
redox reaction
Ion
Dispersion Forces
44. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Diprotic Base
atomic emission spectrum
Le chateliers Principle
Molar solubility
45. Small discrete increments of energy.
quanta
Disproportionation
pI
Group 1A
46. The average distance between the nuclei of two bonded atoms
atomic emission spectrum
Noble gases
Decomposition reaction
bond length
47. Any sample of a given compound will contain the same elements in the identical mass ratio.
Raoult's Law
Noble gases
law of constant composition
Lyman series
48. A solid made up of particles that are not arranged in a regular pattern.
compound
amorphous solid
Solubility Product Constant
d orbital
49. 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
Group 2A
Concentration
Dispersion Forces
Ionization energy
50. 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
chemical reaction
atomic radius
Colligative properties
Reaction mechanism