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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. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
percent composition
s orbital
Rate law
Solute
2. 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.
Le chateliers Principle
Decomposition reaction
Principle quantum number
s orbital
3. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
s orbital
pi bonds
Vapor pressure
Lewis structure
4. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
Avagadros number
atomic radius
ionic cmpound
5. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Dispersion Forces
Chemical Kinetics
Common ion effect
6. In a solution - the substance that dissolves in the solvent
Pauli exclusion principle
lathanide series
Solute
Colligative properties
7. 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.
Magnetic quantum number
azimuthal quantum number
Ion product
Lyman series
8. The lowest allowable energy state of an atom
actinide series
effective nuclear charge
VSEPR
Ground state
9. Sum of the protons and neutrons in an element often denoted by the letter A
Aqueous Solution
Rate determining step
Concentration
Mass number
10. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
Azeotrope
solvation
indicator
Effective nuclear charge
11. Simplest whole # ration of atoms in a compound
Diprotic Base
Halogens
Emperical Formula
chemical reaction
12. 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.
percent composition
Redox Half Reaction
Group 4A
STP
13. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Strong acid
Solvent
Emperical Formula
14. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
percent composition
Electrolyte
Diffusion
atomic theory
15. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Group 2A
redox reaction
Free radical
Atomic weight
16. 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
Titration
Aqueous Solution
Electronegativity
Spin quantum number
17. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Dipole Dipole interaction
Arrhenius Definition
Reaction mechanism
Disproportionation
18. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Ion dipole interactions
quanta
electron affinity
Azeotrope
19. 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.
d orbital
physical reaction
Aqueous Solution
Solubility Product Constant
20. Rare earth element group (elements 58-71)
Lewis definition
Planck's Constant
theoretical yield
lathanide series
21. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Resonance structure
Ion
atomic theory
Noble gases
22. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Dipole Dipole interaction
Conjugate acids and Bases
Solution equilibrium
effective nuclear charge
23. 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.
atomic radius
Common ion effect
Ionic Bond
Ground state
24. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Lewis acid base reaction
Aqueous Solution
decomposition reaction
Half equivalence point
25. The average distance between the nuclei of two bonded atoms
The bohr model
periodic trends
bond length
Triple point
26. Numbers that specify the properties of atomic orbitals and of their electrons
Raoult's Law
Principle quantum number
Halogens
quantum numbers
27. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
Lyman series
Collision theory of chemical Kinetics
Azeotrope
Octet Rule
28. E=hc/?
electromagnetic energy of photons emmited from electrons at ground state
mole
electron configuration
Normality
29. 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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30. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
single displacement reaction
Activation energy
Henry's Law
31. Small discrete increments of energy.
Collision theory of chemical Kinetics
Chemical Kinetics
quanta
transition elements
32. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
d orbital
redox reaction
Diffusion
lathanide series
33. Tells you how much solute is present compared to the amount of solvent
crystalline solid
Le chateliers Principle
Concentration
Azeotrope
34. A reaction where a compound does Not change its molecular structure.
Reaction mechanism
Group 5A
quantum
physical reaction
35. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
single displacement reaction
Intermolecular forces
chemical reaction
36. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
s orbital
quantum
mole
chemical reaction
37. The slowest elementary step which is the limit for the rate of the other steps
transition elements
Rate determining step
compound
d orbital
38. 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
Spin quantum number
Redox Half Reaction
Henderson Hasselbalch Equation
Formal Charge
39. Chalcogens - - Oxide O
Diffusion
Le chateliers Principle
Dipole Dipole interaction
Group 6A
40. 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
Dispersion Forces
crystalline solid
Ionization energy
Equilibrium
41. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
decomposition reaction
d orbital
chemical reaction
Free radical
42. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Halogens
Group 3A
quantum
43. 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
electron configuration
London forces
Rate law
Ionization energy
44. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Spin quantum number
Formula weight
Lewis structure
Molarity
45. (chemistry) p(otential of) H(ydrogen)
Electronegativity
pH
Network covalent
London forces
46. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
chemical reaction
Nucleus
pi bonds
Lewis acid base reaction
47. The energy required to break a chemical bond and form neutral isolated atoms
s orbital
bond energy
Diffusion
Vapor pressure
48. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Dispersion Forces
sigma bond
Atomic absorption Spectra
Equlibrium constant
49. 2.18 x 10^-18 J/electron
Network covalent
Rydberg constant
Arrhenius Definition
Ion dipole interactions
50. The process by which one or more substances change to produce one or more different substances
redox reaction
Half equivalence point
Group 7A
chemical reaction