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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. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
Pauli exclusion principle
Percent composition
und's rule
2. 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.
Lewis definition
Bronsted Lowry
indicator
Equivalence point
3. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
electrolysis
Rydberg constant
Titration
Molarity
4. Sum of the protons and neutrons in an element often denoted by the letter A
chemical reaction
compound
atomic emission spectrum
Mass number
5. A reaction where a compound does Not change its molecular structure.
single displacement reaction
Percent composition
physical reaction
Chemical Kinetics
6. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Molar solubility
Percent composition
electron affinity
decomposition reaction
7. A reaction in which atoms of one element take the place of atoms of another element in a compound
energy state
single displacement reaction
London forces
Conjugate acids and Bases
8. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
angular momentum in the bohr model
Lewis acid base reaction
Covalent Bond
Formal Charge
9. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Group 1A
Lewis structure
Amphoteric
Diffusion
10. (chemistry) p(otential of) H(ydrogen)
ionic cmpound
pH
Principle quantum number
Le chateliers Principle
11. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
molecular weight
Group 6A
Ion dipole interactions
Balmer series
12. The energy required to break a chemical bond and form neutral isolated atoms
Nonpolar covalent bond
Redox Half Reaction
Lewis acid base reaction
bond energy
13. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Solution equilibrium
atomic emission spectrum
Rate determining step
effective nuclear charge
14. In a solution - the substance that dissolves in the solvent
Solute
pi bonds
effective nuclear charge
Colligative properties
15. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Dispersion Forces
Vapor pressure
Avagadros number
Charles and Gay Lussac's Law
16. 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
law of constant composition
Ionization energy
redox reaction
17. The average distance between the nuclei of two bonded atoms
bond length
und's rule
decomposition reaction
s orbital
18. 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
amorphous solid
lathanide series
indicator
Ionic Bond
19. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
atomic theory
Ion
Half equivalence point
Decomposition reaction
20. 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.
Charles and Gay Lussac's Law
Dipole Dipole interaction
Ion product
physical reaction
21. 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
Atomic absorption Spectra
Effective nuclear charge
Arrhenius Definition
subshell
22. 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.
redox reaction
Strong acid
Group 6A
VSEPR
23. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
s orbital
Group 2A
atomic theory
Bronsted - Lowry definition
24. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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25. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Ion dipole interactions
atomic radius
Group 7A
26. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Period
angular momentum in the bohr model
Solvent
Net ionic equation
27. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Atomic absorption Spectra
single displacement reaction
Noble gases
Activation energy
28. 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
Diffusion
bond length
Solution equilibrium
electromagnetic energy of photons emmited from electrons at ground state
29. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Henderson Hasselbalch Equation
heisenberg uncertainty principle
Network covalent
physical reaction
30. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Planck's Constant
Lewis definition
pi bonds
STP
31. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
atomic radius
Diprotic Base
Emperical Formula
32. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Raoult's Law
Nucleus
Ion
33. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
decomposition reaction
Lewis acid base reaction
Bronsted Lowry
34. 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
Group 4A
hydrogen bonding
Planck's Constant
Pauli exclusion principle
35. 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
Ion
Period
Le chateliers Principle
Colligative properties
36. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Vapor pressure
solvation
indicator
atomic emission spectrum
37. The maximum amount of product that can be produced from a given amount of reactant
Reaction order
Neutron
theoretical yield
Henderson Hasselbalch Equation
38. The process by which one or more substances change to produce one or more different substances
Molarity
Resonance structure
Colligative properties
chemical reaction
39. 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
solvation
Molecular orbital
40. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
atomic radius
Lewis structure
Group 4A
41. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
compound
Molecular orbital
Group 3A
energy state
42. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Ion dipole interactions
atomic radius
Solute
Lewis acid base reaction
43. Named after their cation and anion
Hydrogen bonding
Acid dissociation constant
azimuthal quantum number
ionic cmpound
44. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Henderson Hasselbalch Equation
Graham's Law
Ionization energy
45. The slowest elementary step which is the limit for the rate of the other steps
Net ionic equation
Rate determining step
solvation
Rate law
46. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Group 5A
Neutralization reaction
Intermolecular forces
47. The lowest allowable energy state of an atom
Decomposition reaction
Ground state
Electrolyte
Ion
48. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
mole
STP
Solute
single displacement reaction
49. A horizontal row of elements in the periodic table
Electronegativity
Period
amorphous solid
redox reaction
50. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Balmer series
Reaction mechanism
Buffer
und's rule