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MCAT Chemistry
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Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Reaction mechanism
heisenberg uncertainty principle
molecular weight
Effective nuclear charge
2. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Period
Conjugate acids and Bases
Diffusion
Combination Reaction
3. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Henderson Hasselbalch Equation
Half equivalence point
Solvent
lewis base
4. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Activation energy
law of constant composition
Molality
periodic trends
5. Simplest whole # ration of atoms in a compound
Lyman series
Activation energy
atomic radius
Emperical Formula
6. 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
Colligative properties
Group 1A
crystalline solid
representative elements
7. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Azeotrope
Network covalent
law of constant composition
8. 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
pH
quantum numbers
Dipole
9. PH of a molecule at which it contains no net electric charge - isoelectric point.
Ionization energy
Electronegativity
d orbital
pI
10. 5 different orbitals shaped like clover leaves and max electrons is 10
physical reaction
d orbital
Noble gases
electrolysis
11. 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
transition elements
Phase diagram
s orbital
Ion dipole interactions
12. 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
Equlibrium constant
Formal Charge
Group 1A
Intermolecular forces
13. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Rydberg constant
Strong acid
Water dissociation Constant
Chemical Kinetics
14. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Rate determining step
atomic radius
Common ion effect
15. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Arrhenius Definition
azimuthal quantum number
lewis base
16. E=hc/?
hydrogen bonding
bond energy
Rate determining step
electromagnetic energy of photons emmited from electrons at ground state
17. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
theoretical yield
Ground state
lewis base
Percent yield
18. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Neutralization reaction
Lewis structure
Decomposition reaction
Solvent
19. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Neutralization reaction
Formal Charge
und's rule
Molarity
20. 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 5A
hydrogen bonding
Solute
Decomposition reaction
21. 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.
Disproportionation
Henderson Hasselbalch Equation
crystalline solid
Group 2A
22. An atom or group of atoms that has a positive or negative charge
Common ion effect
Ion
Lewis acid base reaction
Rydberg constant
23. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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24. An ionic compound that resists changes in its pH
bond energy
Diffusion
Covalent Bond
Buffer
25. Elements in the middle of the periodic table - in groups 3-12.
physical reaction
Lewis acid base reaction
Atomic absorption Spectra
transition elements
26. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Triple point
Octet Rule
Balmer series
actinide series
27. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
atomic radius
heisenberg uncertainty principle
electromagnetic energy of photons emmited from electrons at ground state
Electrolyte
28. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
decomposition reaction
Formula weight
Chemical Kinetics
Resonance structure
29. A substance that - when dissolved in water - results in a solution that can conduct electricity
electrolysis
Electrolyte
chemical reaction
Percent composition
30. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Bronsted Lowry
atomic radius
mole
Neutralization reaction
31. Sum of the protons and neutrons in an element often denoted by the letter A
angular momentum in the bohr model
Mass number
electrolysis
Arrhenius Definition
32. Property of the elements that can be predicted from the arrangement of the periodic table
Group 7A
periodic trends
Neutron
Nucleus
33. Named after their cation and anion
Resonance structure
ionic cmpound
Solvent
Ion
34. 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.
Rydberg constant
Effective nuclear charge
indicator
Atomic weight
35. A base that can accept two moles of H+ per mole of itself (ex: SO4
ionic cmpound
Diprotic Base
effective nuclear charge
Henry's Law
36. 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
Balmer series
Concentration
Dispersion Forces
STP
37. 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-
Solution equilibrium
indicator
atomic radius
Water dissociation Constant
38. 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.
Group 5A
Solubility Product Constant
Amphoteric
Free radical
39. Small discrete increments of energy.
Graham's Law
quanta
Ion dipole interactions
Group 6A
40. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Activation energy
Rydberg constant
Covalent Bond
London forces
41. 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
energy state
Titration
Halogens
Hydrogen bonding
42. 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.
Lyman series
Raoult's Law
compound
VSEPR
43. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Bronsted - Lowry definition
Period
redox reaction
azimuthal quantum number
44. 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
gram equivalent weight
Ion dipole interactions
s orbital
Azeotrope
45. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Principle quantum number
Group 2A
Halogens
amorphous solid
46. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Nucleus
Henderson Hasselbalch Equation
gram equivalent weight
Reaction mechanism
47. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Formal Charge
STP
Redox Half Reaction
Effusion
48. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Atomic weight
pH
Mass number
49. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Equilibrium
atomic emission spectrum
Dipole
transition elements
50. Common definition of acids as proton (H+) donors and bases as proton acceptors
atomic theory
Proton
decomposition reaction
Bronsted - Lowry definition
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