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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 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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2. The lowest allowable energy state of an atom
Ground state
Intermolecular forces
Electronegativity
Colligative properties
3. 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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4. A reaction in which atoms of one element take the place of atoms of another element in a compound
Dispersion Forces
single displacement reaction
Normality
und's rule
5. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
empirical formula
Titration
Planck's Constant
6. 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
Colligative properties
Nucleus
lathanide series
Aqueous Solution
7. 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
Group 4A
Ionic Bond
Formal Charge
crystalline solid
8. The process of decomposing a chemical compound by the passage of an electric current.
amorphous solid
electrolysis
actinide series
Lewis definition
9. 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
s orbital
Octet Rule
representative elements
Buffer
10. 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.
Solute
Redox Half Reaction
Charles and Gay Lussac's Law
Water dissociation Constant
11. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
Lewis structure
d orbital
Henry's Law
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
Group 5A
single displacement reaction
Formula weight
13. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Pauli exclusion principle
Chemical Kinetics
Ion
Lewis acid base reaction
14. Redox reaction - in which the same species is both oxidized and reduced.
Spin quantum number
Disproportionation
gram equivalent weight
Rydberg constant
15. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Activation energy
Dipole
Molality
Chemical Kinetics
16. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Percent yield
quantum numbers
Planck's Constant
Conjugate acids and Bases
17. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Effective nuclear charge
pi bonds
Colligative properties
gram equivalent weight
18. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Intermolecular forces
Solubility Product Constant
Vapor pressure
atomic radius
19. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
effective nuclear charge
Formula weight
chemical reaction
Diffusion
20. 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.
Ion
electron affinity
Balmer series
mole
21. 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
gram equivalent weight
Acid dissociation constant
Electrolyte
Water dissociation Constant
22. Numbers that specify the properties of atomic orbitals and of their electrons
effective nuclear charge
compound
quantum numbers
law of constant composition
23. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Disproportionation
Molality
Rate law
crystalline solid
24. In a solution - the substance that dissolves in the solvent
azimuthal quantum number
Group 4A
Solute
bond length
25. A definite stable energy that a physical system can have
Hydrogen bonding
pI
energy state
Effective nuclear charge
26. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
single displacement reaction
und's rule
physical reaction
empirical formula
27. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Equivalence point
Aqueous Solution
Solute
Magnetic quantum number
28. PH of a molecule at which it contains no net electric charge - isoelectric point.
Group 5A
Lyman series
Collision theory of chemical Kinetics
pI
29. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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30. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Nucleus
Halogens
atomic radius
Equlibrium constant
31. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Mass number
Network covalent
Intermolecular forces
electron configuration
32. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
Net ionic equation
London forces
crystalline solid
Magnetic quantum number
33. 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
London forces
azimuthal quantum number
Halogens
The bohr model
34. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
redox reaction
Group 6A
atomic emission spectrum
Henderson Hasselbalch Equation
35. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Emperical Formula
quanta
Reaction mechanism
Effusion
36. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Free radical
transition elements
Triple point
Reaction mechanism
37. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
lathanide series
Henderson Hasselbalch Equation
electron configuration
38. 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
VSEPR
Electrolyte
Arrhenius Definition
Disproportionation
39. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Group 1A
Molarity
Activation energy
atomic radius
40. 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.
Effective nuclear charge
Bronsted Lowry
quantum
Graham's Law
41. The percent by mass of each element in a compound
STP
Ion product
hydrogen bonding
percent composition
42. 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
Covalent Bond
Hydrogen bonding
solvation
Halogens
43. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
chemical reaction
pI
Electronegativity
solvation
44. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Molecular orbital
Lewis structure
Halogens
Group 2A
45. Sum of the protons and neutrons in an element often denoted by the letter A
Dipole Dipole interaction
chemical reaction
Diffusion
Mass number
46. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Henderson Hasselbalch Equation
electron configuration
actinide series
electron affinity
47. The process by which one or more substances change to produce one or more different substances
empirical formula
Group 4A
pI
chemical reaction
48. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Nonpolar covalent bond
Activation energy
Diffusion
Henry's Law
49. 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
azimuthal quantum number
energy state
Diffusion
London forces
50. A solid made up of particles that are not arranged in a regular pattern.
Group 3A
amorphous solid
Neutralization reaction
actinide series