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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. Two or more atoms held together by covalent bonds
Ion
Electronegativity
molecule
gram equivalent weight
2. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Strong acid
Net ionic equation
Principle quantum number
Dipole Dipole interaction
3. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Octet Rule
Molar solubility
Percent composition
Hydrogen bonding
4. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Effective nuclear charge
atomic theory
ionic cmpound
5. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
redox reaction
electron affinity
Ionization energy
6. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
representative elements
atomic emission spectrum
crystalline solid
7. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
amorphous solid
Conjugate acids and Bases
representative elements
Noble gases
8. Slightly less reactive than alkali metals - comprise group II
representative elements
compound
Alkaline earths
Proton
9. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Ion
molecule
Ionic Bond
empirical formula
10. The lowest allowable energy state of an atom
Ground state
Covalent Bond
Lewis definition
chemical reaction
11. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Half equivalence point
Rate law
Nonpolar covalent bond
Theoretical yield
12. 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
Period
Nucleus
heisenberg uncertainty principle
amorphous solid
13. (chemistry) p(otential of) H(ydrogen)
pH
Molality
Molar solubility
Acid dissociation constant
14. 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.
Charles and Gay Lussac's Law
Mass number
Buffer
Ion product
15. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
heisenberg uncertainty principle
Lyman series
Vapor pressure
Rate law
16. A reaction in which atoms of one element take the place of atoms of another element in a compound
Formal Charge
electrolysis
Aqueous Solution
single displacement reaction
17. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
solvation
Group 5A
Dipole
electron affinity
18. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Reaction order
Amphoteric
Molecular orbital
solvation
19. 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
hydrogen bonding
Half equivalence point
Emperical Formula
Triple point
20. The slowest elementary step which is the limit for the rate of the other steps
Covalent Bond
Nucleus
quantum numbers
Rate determining step
21. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Covalent Bond
Ion
Dispersion Forces
22. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Pauli exclusion principle
Water dissociation Constant
representative elements
23. 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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24. 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-
Rate law
Water dissociation Constant
law of constant composition
und's rule
25. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
theoretical yield
quanta
Rate law
subshell
26. A definite stable energy that a physical system can have
quanta
Molar solubility
energy state
Henry's Law
27. The maximum amount of product that can be produced from a given amount of reactant
Ionic Bond
theoretical yield
Solution equilibrium
Pauli exclusion principle
28. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
s orbital
Henry's Law
Nucleus
Neutralization reaction
29. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Lewis definition
electrolysis
Network covalent
Atomic absorption Spectra
30. Substance in which a solute is dissolved to form a solution
Molarity
Solvent
Electronegativity
Network covalent
31. 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
The bohr model
Group 6A
Balmer series
energy state
32. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Buffer
Molarity
Collision theory of chemical Kinetics
theoretical yield
33. The percent by mass of each element in a compound
Ionic Bond
single displacement reaction
percent composition
und's rule
34. 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.
Henry's Law
heisenberg uncertainty principle
Solubility Product Constant
Atomic absorption Spectra
35. Any sample of a given compound will contain the same elements in the identical mass ratio.
compound
law of constant composition
Alkaline earths
azimuthal quantum number
36. Simplest whole # ration of atoms in a compound
Reaction mechanism
Emperical Formula
Net ionic equation
percent composition
37. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Solution equilibrium
empirical formula
molecular weight
Phase diagram
38. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Molarity
electron affinity
Group 3A
Theoretical yield
39. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Ionization energy
Ion
Water dissociation Constant
40. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Neutron
angular momentum in the bohr model
Group 1A
und's rule
41. 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.
Normality
Raoult's Law
Octet Rule
Effective nuclear charge
42. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Aqueous Solution
Molecular orbital
Period
43. 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
hydrogen bonding
Octet Rule
pH
Group 7A
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
Azeotrope
Equlibrium constant
Effective nuclear charge
Henderson Hasselbalch Equation
45. Having characteristics of both an acid and a base and capable of reacting as either
crystalline solid
quantum numbers
Solvent
Amphoteric
46. 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.
Ion
Arrhenius Definition
Electronegativity
Redox Half Reaction
47. Small discrete increments of energy.
Activation energy
Collision theory of chemical Kinetics
quanta
Charles and Gay Lussac's Law
48. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Concentration
theoretical yield
percent composition
49. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
electromagnetic energy of photons emmited from electrons at ground state
Atomic weight
Neutron
50. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Aqueous Solution
Proton
Nonpolar covalent bond
Ion
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