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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. 5 valence electrons -3 ions - Nitride N
Molar solubility
Group 2A
Solubility Product Constant
Group 5A
2. 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
Solution equilibrium
Formula weight
quantum
STP
3. 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
Resonance structure
law of constant composition
Rate law
4. The slowest elementary step which is the limit for the rate of the other steps
Ionization energy
Water dissociation Constant
Solute
Rate determining step
5. Small discrete increments of energy.
Diffusion
Equivalence point
quanta
Molarity
6. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Magnetic quantum number
Electronegativity
bond energy
single displacement reaction
7. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
molecular weight
Free radical
Nonpolar covalent bond
percent composition
8. 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-
Water dissociation Constant
Theoretical yield
molecular weight
Principle quantum number
9. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Half equivalence point
decomposition reaction
actinide series
Water dissociation Constant
10. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
molecular weight
Effusion
Formula weight
s orbital
11. 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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12. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
electromagnetic energy of photons emmited from electrons at ground state
Group 1A
Halogens
indicator
13. 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.
actinide series
Bronsted Lowry
pI
Effective nuclear charge
14. The Percent by mass of each element in a compound.
Common ion effect
Percent composition
representative elements
Group 3A
15. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Chemical Kinetics
STP
Equlibrium constant
lewis base
16. 2.18 x 10^-18 J/electron
Equlibrium constant
quantum
Rydberg constant
Le chateliers Principle
17. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Group 4A
bond length
Collision theory of chemical Kinetics
Ion
18. Chalcogens - - Oxide O
Molarity
Vapor pressure
sigma bond
Group 6A
19. 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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20. 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
Spin quantum number
Equlibrium constant
Ion dipole interactions
indicator
21. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Percent yield
Buffer
Lyman series
Network covalent
22. 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
London forces
Acid dissociation constant
Le chateliers Principle
theoretical yield
23. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Group 2A
Emperical Formula
Octet Rule
quanta
24. Gram equivalent weight of solute per liter of solution - often denoted by N.
Acid dissociation constant
Normality
Bronsted - Lowry definition
angular momentum in the bohr model
25. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Diprotic Base
Half equivalence point
Rate law
26. Named after their cation and anion
London forces
Dispersion Forces
single displacement reaction
ionic cmpound
27. An elementary particle with 0 charge and mass about equal to a proton
Neutron
azimuthal quantum number
indicator
Network covalent
28. A solid made up of particles that are not arranged in a regular pattern.
Molar solubility
Bronsted - Lowry definition
heisenberg uncertainty principle
amorphous solid
29. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
quantum
Net ionic equation
electrolysis
30. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Molar solubility
Atomic absorption Spectra
Group 2A
Charles and Gay Lussac's Law
31. 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
azimuthal quantum number
Le chateliers Principle
electrolysis
32. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
indicator
Molality
Solvent
Solubility Product Constant
33. 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
Balmer series
solvation
Spin quantum number
Lewis definition
34. 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
Network covalent
Balmer series
Theoretical yield
35. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Strong acid
Activation energy
Period
Lewis structure
36. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
redox reaction
Diprotic Base
theoretical yield
37. 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
gram equivalent weight
Solubility Product Constant
Neutron
Group 7A
38. 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
electron configuration
Group 2A
Group 5A
Hydrogen bonding
39. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Solvent
Formula weight
lewis base
40. 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
Colligative properties
Ionization energy
Covalent Bond
41. Tells you how much solute is present compared to the amount of solvent
Group 7A
electron affinity
Concentration
Alkaline earths
42. Common definition of acids as proton (H+) donors and bases as proton acceptors
polymer
Bronsted - Lowry definition
Percent composition
Formal Charge
43. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Amphoteric
Percent composition
Molality
44. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
decomposition reaction
Concentration
Lyman series
Ion dipole interactions
45. 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
angular momentum in the bohr model
Electrolyte
Period
Ionization energy
46. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Group 1A
redox reaction
Reaction mechanism
Atomic weight
47. Simplest whole # ration of atoms in a compound
Emperical Formula
Covalent Bond
s orbital
Effusion
48. 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
Reaction mechanism
s orbital
Le chateliers Principle
49. 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.
atomic theory
transition elements
Atomic absorption Spectra
Lewis definition
50. A base that can accept two moles of H+ per mole of itself (ex: SO4
Le chateliers Principle
Lewis acid base reaction
Diprotic Base
molecule