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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.
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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. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Effusion
Molecular orbital
pI
theoretical yield
2. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
crystalline solid
Free radical
angular momentum in the bohr model
Acid dissociation constant
3. 5 valence electrons -3 ions - Nitride N
Ion
Effusion
subshell
Group 5A
4. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Half equivalence point
Balmer series
sigma bond
Phase diagram
5. Gram equivalent weight of solute per liter of solution - often denoted by N.
mole
Solubility Product Constant
Normality
Formal Charge
6. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
electromagnetic energy of photons emmited from electrons at ground state
crystalline solid
Neutron
7. A reaction where a compound does Not change its molecular structure.
physical reaction
electrolysis
Water dissociation Constant
Rydberg constant
8. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Planck's Constant
Principle quantum number
Equilibrium
indicator
9. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Acid dissociation constant
Formula weight
electron configuration
gram equivalent weight
10. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Group 5A
atomic radius
Collision theory of chemical Kinetics
electron configuration
11. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
redox reaction
decomposition reaction
atomic theory
compound
12. 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
Ionic Bond
Lewis acid base reaction
ionic cmpound
quanta
13. Small discrete increments of energy.
gram equivalent weight
quanta
Common ion effect
Pauli exclusion principle
14. An elementary particle with 0 charge and mass about equal to a proton
crystalline solid
Neutron
sigma bond
bond energy
15. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
London forces
Effusion
Azeotrope
electrolysis
16. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Activation energy
pH
Percent yield
17. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
subshell
ionic cmpound
periodic trends
Combination Reaction
18. The process by which one or more substances change to produce one or more different substances
Group 5A
Planck's Constant
atomic emission spectrum
chemical reaction
19. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Solubility Product Constant
Graham's Law
Noble gases
Water dissociation Constant
20. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Mass number
single displacement reaction
bond energy
polymer
21. 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.
Acid dissociation constant
Colligative properties
Group 4A
Equivalence point
22. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Concentration
quantum
quantum numbers
Electronegativity
23. 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
Halogens
Proton
atomic radius
electron affinity
24. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Lyman series
electromagnetic energy of photons emmited from electrons at ground state
subshell
Net ionic equation
25. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Mass number
Percent yield
Period
26. The average distance between the nuclei of two bonded atoms
bond length
atomic theory
Effective nuclear charge
heisenberg uncertainty principle
27. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Azeotrope
Alkaline earths
actinide series
gram equivalent weight
28. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
The bohr model
Reaction order
d orbital
29. A definite stable energy that a physical system can have
molecule
Resonance structure
energy state
Dispersion Forces
30. Any sample of a given compound will contain the same elements in the identical mass ratio.
molecular weight
quantum numbers
law of constant composition
Equlibrium constant
31. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
representative elements
Magnetic quantum number
Group 6A
Free radical
32. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Formal Charge
Strong acid
Ion dipole interactions
Covalent Bond
33. Having characteristics of both an acid and a base and capable of reacting as either
Colligative properties
Amphoteric
Planck's Constant
angular momentum in the bohr model
34. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Nonpolar covalent bond
Aqueous Solution
empirical formula
Mass number
35. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Chemical Kinetics
lewis base
effective nuclear charge
Reaction mechanism
36. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
periodic trends
Common ion effect
Reaction order
37. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Formula weight
Principle quantum number
hydrogen bonding
38. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Graham's Law
Electronegativity
periodic trends
39. 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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40. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Henry's Law
Group 2A
Effusion
41. The lowest allowable energy state of an atom
Ground state
Period
atomic emission spectrum
Principle quantum number
42. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Period
electrolysis
electromagnetic energy of photons emmited from electrons at ground state
Lewis acid base reaction
43. 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.
Alkaline earths
Ion product
Period
Henry's Law
44. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
s orbital
Free radical
Conjugate acids and Bases
Group 2A
45. 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
Effusion
Rate law
Formula weight
Azeotrope
46. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Spin quantum number
Vapor pressure
electromagnetic energy of photons emmited from electrons at ground state
47. 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
Reaction mechanism
Lewis definition
Molality
Solution equilibrium
48. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Henry's Law
atomic radius
Group 5A
heisenberg uncertainty principle
49. Two or more atoms held together by covalent bonds
subshell
Group 7A
Graham's Law
molecule
50. (chemistry) p(otential of) H(ydrogen)
Intermolecular forces
Group 4A
pH
Henderson Hasselbalch Equation
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