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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. 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
Solubility Product Constant
atomic emission spectrum
Rate law
2. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
subshell
Atomic absorption Spectra
Nonpolar covalent bond
3. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
4. The process of decomposing a chemical compound by the passage of an electric current.
London forces
Molality
electrolysis
decomposition reaction
5. Small discrete increments of energy.
amorphous solid
Dipole
Activation energy
quanta
6. Rare earth element group (elements 58-71)
lathanide series
Lyman series
redox reaction
electrolysis
7. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Proton
Molality
Acid dissociation constant
Triple point
8. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
VSEPR
molecule
Graham's Law
polymer
9. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Ion
Period
Formula weight
10. 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
actinide series
Equilibrium
Hydrogen bonding
Bronsted - Lowry definition
11. Named after their cation and anion
ionic cmpound
gram equivalent weight
representative elements
Ion dipole interactions
12. Any sample of a given compound will contain the same elements in the identical mass ratio.
Raoult's Law
law of constant composition
electromagnetic energy of photons emmited from electrons at ground state
Bronsted - Lowry definition
13. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
periodic trends
Common ion effect
Balmer series
percent composition
14. (chemistry) p(otential of) H(ydrogen)
Diprotic Base
pH
Redox Half Reaction
Effective nuclear charge
15. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Henderson Hasselbalch Equation
Titration
Molar solubility
Henry's Law
16. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
electromagnetic energy of photons emmited from electrons at ground state
atomic radius
Triple point
Acid dissociation constant
17. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Alkaline earths
Graham's Law
lewis base
Ionic Bond
18. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Normality
angular momentum in the bohr model
Lyman series
Molecular orbital
19. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Dipole Dipole interaction
Electronegativity
Nucleus
Principle quantum number
20. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
Ion
ionic cmpound
Activation energy
atomic radius
21. In a solution - the substance that dissolves in the solvent
electromagnetic energy of photons emmited from electrons at ground state
Proton
Solute
Diffusion
22. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Equilibrium
Aqueous Solution
Lewis definition
Triple point
23. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Ion
Intermolecular forces
decomposition reaction
Principle quantum number
24. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Neutralization reaction
Pauli exclusion principle
Percent yield
actinide series
25. An ionic compound that resists changes in its pH
Buffer
lathanide series
Solution equilibrium
sigma bond
26. Two or more atoms held together by covalent bonds
Group 5A
actinide series
Nonpolar covalent bond
molecule
27. E=hc/?
Phase diagram
electromagnetic energy of photons emmited from electrons at ground state
energy state
Amphoteric
28. 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.
Common ion effect
crystalline solid
electron affinity
quanta
29. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Rate determining step
molecular weight
Equlibrium constant
Group 3A
30. 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
31. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Atomic weight
Triple point
Rate determining step
Equlibrium constant
32. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Network covalent
Phase diagram
Azeotrope
Reaction order
33. The average distance between the nuclei of two bonded atoms
Period
electron configuration
bond length
Triple point
34. 5 valence electrons -3 ions - Nitride N
Ionic Bond
Water dissociation Constant
Group 5A
Diffusion
35. 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
Amphoteric
Nonpolar covalent bond
gram equivalent weight
36. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
actinide series
Covalent Bond
hydrogen bonding
quantum
37. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
azimuthal quantum number
periodic trends
Octet Rule
Theoretical yield
38. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Colligative properties
redox reaction
effective nuclear charge
39. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Acid dissociation constant
solvation
Balmer series
quanta
40. The Percent by mass of each element in a compound.
Group 7A
Net ionic equation
Redox Half Reaction
Percent composition
41. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
sigma bond
Planck's Constant
atomic radius
42. 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
Acid dissociation constant
Reaction order
representative elements
Covalent Bond
43. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Nucleus
Group 6A
Combination Reaction
compound
44. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Nonpolar covalent bond
actinide series
effective nuclear charge
45. 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.
single displacement reaction
Arrhenius Definition
Covalent Bond
Balmer series
46. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
subshell
Molality
energy state
Equlibrium constant
47. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole
percent composition
decomposition reaction
Dipole Dipole interaction
48. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
atomic radius
Combination Reaction
Activation energy
Dispersion Forces
49. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
ionic cmpound
gram equivalent weight
energy state
50. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
sigma bond
Molarity
Mass number