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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. 2.18 x 10^-18 J/electron
Water dissociation Constant
Rydberg constant
Solvent
Bronsted Lowry
2. 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
molecule
Hydrogen bonding
Lewis acid base reaction
heisenberg uncertainty principle
3. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Ion product
Vapor pressure
Normality
4. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Solubility Product Constant
solvation
Effusion
Molarity
5. Substance in which a solute is dissolved to form a solution
VSEPR
Solvent
Disproportionation
quanta
6. Small discrete increments of energy.
lewis base
Solvent
Strong acid
quanta
7. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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8. A base that can accept two moles of H+ per mole of itself (ex: SO4
Solvent
atomic emission spectrum
Diprotic Base
Free radical
9. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Buffer
Common ion effect
Molar solubility
Group 6A
10. 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-
Normality
representative elements
Water dissociation Constant
Group 7A
11. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Ion dipole interactions
und's rule
d orbital
12. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Theoretical yield
Effusion
Dipole Dipole interaction
13. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Ionization energy
Nonpolar covalent bond
Collision theory of chemical Kinetics
14. 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
sigma bond
Atomic weight
atomic radius
representative elements
15. Slightly less reactive than alkali metals - comprise group II
Le chateliers Principle
Rydberg constant
Alkaline earths
electrolysis
16. An ionic compound that resists changes in its pH
Buffer
Ion
Aqueous Solution
Pauli exclusion principle
17. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Halogens
Network covalent
redox reaction
energy state
18. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lewis acid base reaction
Lyman series
law of constant composition
atomic radius
19. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Activation energy
Ionic Bond
atomic radius
20. Gram equivalent weight of solute per liter of solution - often denoted by N.
Equlibrium constant
Equivalence point
Normality
Ionization energy
21. The energy required to break a chemical bond and form neutral isolated atoms
single displacement reaction
Solvent
bond energy
Strong acid
22. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Electronegativity
Le chateliers Principle
Avagadros number
Activation energy
23. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher
Formal Charge
electron affinity
electromagnetic energy of photons emmited from electrons at ground state
Solvent
24. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Ion
Network covalent
angular momentum in the bohr model
25. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Atomic absorption Spectra
single displacement reaction
Buffer
26. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Group 6A
electrolysis
indicator
Conjugate acids and Bases
27. Any sample of a given compound will contain the same elements in the identical mass ratio.
Ground state
Equivalence point
law of constant composition
Graham's Law
28. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Aqueous Solution
und's rule
electron affinity
Phase diagram
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
Acid dissociation constant
Ionization energy
Diprotic Base
30. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
Colligative properties
heisenberg uncertainty principle
Triple point
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
Collision theory of chemical Kinetics
Formal Charge
Redox Half Reaction
Arrhenius Definition
32. Simplest whole # ration of atoms in a compound
Effusion
Emperical Formula
Magnetic quantum number
quantum numbers
33. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Rate law
decomposition reaction
The bohr model
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.
representative elements
Effective nuclear charge
quantum numbers
Formula weight
35. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Covalent Bond
Octet Rule
Vapor pressure
electrolysis
36. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
London forces
atomic radius
Principle quantum number
Normality
37. Having characteristics of both an acid and a base and capable of reacting as either
heisenberg uncertainty principle
periodic trends
Amphoteric
Rate law
38. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Equlibrium constant
Raoult's Law
chemical reaction
39. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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40. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
molecule
Octet Rule
Conjugate acids and Bases
redox reaction
41. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Ion dipole interactions
Group 1A
Conjugate acids and Bases
Diprotic Base
42. 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
quantum
bond length
Acid dissociation constant
Atomic absorption Spectra
43. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Dipole Dipole interaction
Reaction mechanism
Lewis structure
compound
44. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
electrolysis
und's rule
percent composition
45. 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
Acid dissociation constant
s orbital
STP
Mass number
46. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Redox Half Reaction
Nonpolar covalent bond
Solute
Normality
47. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
actinide series
Henderson Hasselbalch Equation
solvation
Solute
48. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Equivalence point
Nucleus
Pauli exclusion principle
redox reaction
49. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Henderson Hasselbalch Equation
Free radical
Nucleus
50. 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
und's rule
Solubility Product Constant
The bohr model
Nucleus