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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. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Solution equilibrium
pI
atomic emission spectrum
2. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
redox reaction
atomic radius
Nonpolar covalent bond
Ionic Bond
3. 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
Emperical Formula
lathanide series
Solute
4. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
pI
The bohr model
Balmer series
Azeotrope
5. 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
Ion dipole interactions
Azeotrope
ionic cmpound
sigma bond
6. 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
Principle quantum number
Ionization energy
Formal Charge
quanta
7. Numbers that specify the properties of atomic orbitals and of their electrons
Ion
decomposition reaction
quantum numbers
Magnetic quantum number
8. Common definition of acids as proton (H+) donors and bases as proton acceptors
periodic trends
Bronsted - Lowry definition
Arrhenius Definition
Half equivalence point
9. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
physical reaction
Avagadros number
effective nuclear charge
Intermolecular forces
10. A substance that - when dissolved in water - results in a solution that can conduct electricity
pi bonds
Halogens
Electrolyte
Decomposition reaction
11. The process of decomposing a chemical compound by the passage of an electric current.
Combination Reaction
Theoretical yield
electrolysis
Rate law
12. Any sample of a given compound will contain the same elements in the identical mass ratio.
Combination Reaction
actinide series
Azeotrope
law of constant composition
13. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Ion
Ionization energy
atomic radius
Activation energy
14. 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
Decomposition reaction
Bronsted - Lowry definition
polymer
Colligative properties
15. 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
Raoult's Law
Diffusion
Hydrogen bonding
Neutron
16. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Formula weight
lewis base
Decomposition reaction
Halogens
17. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Phase diagram
Proton
Charles and Gay Lussac's Law
redox reaction
18. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Group 1A
transition elements
Network covalent
azimuthal quantum number
19. 5 valence electrons -3 ions - Nitride N
Net ionic equation
Formula weight
Graham's Law
Group 5A
20. 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.
Arrhenius Definition
Molarity
single displacement reaction
Redox Half Reaction
21. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Neutron
s orbital
Collision theory of chemical Kinetics
Phase diagram
22. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Percent yield
single displacement reaction
atomic theory
Nucleus
23. 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
subshell
Reaction order
Nucleus
Azeotrope
24. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Conjugate acids and Bases
atomic radius
Formula weight
Avagadros number
25. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Strong acid
molecular weight
actinide series
empirical formula
26. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
physical reaction
compound
quantum numbers
STP
27. 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.
heisenberg uncertainty principle
Solubility Product Constant
Network covalent
Diprotic Base
28. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Rate determining step
empirical formula
Equilibrium
molecular weight
29. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Graham's Law
Bronsted - Lowry definition
quantum
30. Acids defined as electron - pair acceptors and bases as electron - pair donors.
pI
azimuthal quantum number
Lewis definition
Group 6A
31. A reaction where a compound does Not change its molecular structure.
Raoult's Law
Ion product
Covalent Bond
physical reaction
32. Slightly less reactive than alkali metals - comprise group II
Neutralization reaction
Alkaline earths
Aqueous Solution
atomic emission spectrum
33. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
Henderson Hasselbalch Equation
azimuthal quantum number
Equivalence point
Collision theory of chemical Kinetics
34. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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35. 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.
theoretical yield
electromagnetic energy of photons emmited from electrons at ground state
bond energy
Balmer series
36. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Triple point
Molecular orbital
Net ionic equation
gram equivalent weight
37. A horizontal row of elements in the periodic table
Planck's Constant
decomposition reaction
physical reaction
Period
38. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Dipole Dipole interaction
Combination Reaction
lathanide series
chemical reaction
39. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Noble gases
Conjugate acids and Bases
Bronsted Lowry
Molecular orbital
40. 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.
Rydberg constant
effective nuclear charge
electron affinity
Period
41. 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.
Nonpolar covalent bond
Principle quantum number
lathanide series
Emperical Formula
42. 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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43. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Combination Reaction
Common ion effect
Reaction mechanism
mole
44. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Electrolyte
Group 5A
Electronegativity
Dipole Dipole interaction
45. An ionic compound that resists changes in its pH
Henderson Hasselbalch Equation
Covalent Bond
Bronsted Lowry
Buffer
46. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Aqueous Solution
Effective nuclear charge
Atomic weight
Noble gases
47. An atom or group of atoms that has a positive or negative charge
Graham's Law
Ion
Activation energy
STP
48. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
atomic theory
Rate determining step
actinide series
49. 2.18 x 10^-18 J/electron
Collision theory of chemical Kinetics
Ionization energy
Rydberg constant
Ion dipole interactions
50. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
redox reaction
Pauli exclusion principle
s orbital
Reaction mechanism