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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 molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Equlibrium constant
redox reaction
Lewis definition
Molar solubility
2. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Resonance structure
pi bonds
Le chateliers Principle
3. 5 valence electrons -3 ions - Nitride N
Neutralization reaction
Group 5A
Half equivalence point
Water dissociation Constant
4. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Concentration
Free radical
atomic radius
Triple point
5. Common definition of acids as proton (H+) donors and bases as proton acceptors
Rydberg constant
Covalent Bond
Lewis structure
Bronsted - Lowry definition
6. 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.
Equivalence point
Hydrogen bonding
d orbital
Solubility Product Constant
7. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
actinide series
Lewis acid base reaction
Bronsted - Lowry definition
8. 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
bond length
Percent yield
Amphoteric
d orbital
9. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Avagadros number
Electronegativity
London forces
Acid dissociation constant
10. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Lewis structure
effective nuclear charge
Ion product
11. 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.
Molality
Redox Half Reaction
Graham's Law
Nonpolar covalent bond
12. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
polymer
Principle quantum number
Dipole
Ionic Bond
13. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Mass number
Equivalence point
empirical formula
redox reaction
14. Acids defined as electron - pair acceptors and bases as electron - pair donors.
The bohr model
Vapor pressure
Lewis definition
Intermolecular forces
15. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
STP
Atomic weight
Half equivalence point
electrolysis
16. Chalcogens - - Oxide O
Group 6A
Combination Reaction
Ion product
Neutron
17. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Solution equilibrium
law of constant composition
pI
pi bonds
18. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Half equivalence point
Buffer
electrolysis
electron configuration
19. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Ionization energy
Graham's Law
bond energy
Theoretical yield
20. 2.18 x 10^-18 J/electron
Dipole
Rydberg constant
Charles and Gay Lussac's Law
Ion
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
Ionization energy
Ion dipole interactions
Charles and Gay Lussac's Law
Hydrogen bonding
22. Any sample of a given compound will contain the same elements in the identical mass ratio.
Ion dipole interactions
Octet Rule
law of constant composition
Equilibrium
23. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
solvation
representative elements
electromagnetic energy of photons emmited from electrons at ground state
compound
24. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Conjugate acids and Bases
Ion
Dipole Dipole interaction
25. 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
Solubility Product Constant
hydrogen bonding
Charles and Gay Lussac's Law
Solution equilibrium
26. 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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27. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
angular momentum in the bohr model
Lewis acid base reaction
electron configuration
Avagadros number
28. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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29. The energy required to break a chemical bond and form neutral isolated atoms
Collision theory of chemical Kinetics
Atomic weight
Theoretical yield
bond energy
30. Simplest whole # ration of atoms in a compound
Formula weight
Ion
Emperical Formula
angular momentum in the bohr model
31. 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
polymer
Lewis definition
Phase diagram
Arrhenius Definition
32. Numbers that specify the properties of atomic orbitals and of their electrons
Water dissociation Constant
azimuthal quantum number
indicator
quantum numbers
33. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Nonpolar covalent bond
quantum numbers
polymer
Charles and Gay Lussac's Law
34. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Ground state
Equivalence point
theoretical yield
Lyman series
35. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Avagadros number
electron affinity
Molality
mole
36. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
lathanide series
actinide series
pH
37. 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.
VSEPR
Spin quantum number
single displacement reaction
Concentration
38. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Vapor pressure
Arrhenius Definition
physical reaction
39. A reaction where a compound does Not change its molecular structure.
physical reaction
quantum numbers
Half equivalence point
effective nuclear charge
40. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Atomic weight
Solvent
Phase diagram
lathanide series
41. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Molecular orbital
subshell
Azeotrope
Group 4A
42. 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.
angular momentum in the bohr model
Equilibrium
Ion product
Ground state
43. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Equlibrium constant
Period
Neutralization reaction
Le chateliers Principle
44. 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.
electrolysis
Electrolyte
atomic radius
Acid dissociation constant
45. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
bond energy
quantum
atomic theory
46. Rare earth element group (elements 58-71)
Disproportionation
pI
Le chateliers Principle
lathanide series
47. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
Redox Half Reaction
actinide series
Amphoteric
48. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Hydrogen bonding
Henry's Law
Noble gases
redox reaction
49. (chemistry) p(otential of) H(ydrogen)
Equilibrium
pH
electrolysis
periodic trends
50. The average distance between the nuclei of two bonded atoms
bond length
Free radical
Henry's Law
Pauli exclusion principle