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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. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Aqueous Solution
Covalent Bond
Rate law
The bohr model
2. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Neutralization reaction
Noble gases
bond length
redox reaction
3. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Pauli exclusion principle
redox reaction
sigma bond
Reaction mechanism
4. Sum of the protons and neutrons in an element often denoted by the letter A
pH
Proton
Mass number
d orbital
5. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Pauli exclusion principle
Principle quantum number
compound
6. 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
Solution equilibrium
heisenberg uncertainty principle
Raoult's Law
7. 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
Equilibrium
amorphous solid
Dispersion Forces
Proton
8. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Decomposition reaction
crystalline solid
Dipole Dipole interaction
Formal Charge
9. 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.
Equivalence point
mole
redox reaction
Reaction order
10. 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.
Titration
Balmer series
bond energy
Ionic Bond
11. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
electromagnetic energy of photons emmited from electrons at ground state
Triple point
Free radical
solvation
12. A solution in which water is the solvent
Lyman series
Solubility Product Constant
atomic theory
Aqueous Solution
13. 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
Nucleus
s orbital
periodic trends
Halogens
14. 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.
Group 4A
Effective nuclear charge
physical reaction
Octet Rule
15. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Group 5A
percent composition
atomic radius
Hydrogen bonding
16. 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
Dispersion Forces
Water dissociation Constant
Diprotic Base
quantum numbers
17. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Percent yield
Reaction order
theoretical yield
Formula weight
18. 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
Ground state
angular momentum in the bohr model
Formal Charge
Amphoteric
19. 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
Group 1A
indicator
Dipole
20. The Percent by mass of each element in a compound.
Percent composition
Molar solubility
Formula weight
electron configuration
21. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
Ionization energy
Common ion effect
Rate determining step
22. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Dipole
Ion dipole interactions
percent composition
Phase diagram
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. A definite stable energy that a physical system can have
electron affinity
energy state
lathanide series
effective nuclear charge
25. 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
Dipole Dipole interaction
theoretical yield
representative elements
quantum
26. E=hc/?
bond length
electromagnetic energy of photons emmited from electrons at ground state
Bronsted Lowry
Percent yield
27. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
polymer
Redox Half Reaction
Common ion effect
Ion
28. Any sample of a given compound will contain the same elements in the identical mass ratio.
Solvent
Alkaline earths
law of constant composition
energy state
29. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Electronegativity
representative elements
Chemical Kinetics
Reaction order
30. The percent by mass of each element in a compound
percent composition
indicator
Lewis structure
Triple point
31. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Henderson Hasselbalch Equation
electron configuration
Phase diagram
pH
32. In a solution - the substance that dissolves in the solvent
Solute
Emperical Formula
Aqueous Solution
Conjugate acids and Bases
33. Common definition of acids as proton (H+) donors and bases as proton acceptors
Formal Charge
Bronsted - Lowry definition
Solvent
Group 3A
34. 5 valence electrons -3 ions - Nitride N
solvation
atomic radius
Azeotrope
Group 5A
35. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
VSEPR
Conjugate acids and Bases
Atomic weight
und's rule
36. 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.
Network covalent
Group 3A
Henderson Hasselbalch Equation
gram equivalent weight
37. Two or more atoms held together by covalent bonds
molecule
pI
Electronegativity
azimuthal quantum number
38. 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.
Solute
Electronegativity
Bronsted - Lowry definition
Group 3A
39. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Phase diagram
s orbital
Alkaline earths
Molarity
40. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
Neutralization reaction
Network covalent
VSEPR
Titration
41. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Reaction mechanism
single displacement reaction
subshell
Molar solubility
42. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Reaction order
Decomposition reaction
redox reaction
crystalline solid
43. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Atomic weight
Lewis definition
Atomic absorption Spectra
Spin quantum number
44. 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
amorphous solid
electron configuration
azimuthal quantum number
molecular weight
45. 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
effective nuclear charge
Colligative properties
Hydrogen bonding
compound
46. An atom or group of atoms that has a positive or negative charge
Phase diagram
redox reaction
Proton
Ion
47. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Strong acid
Theoretical yield
polymer
48. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Henderson Hasselbalch Equation
Emperical Formula
Strong acid
STP
49. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
Acid dissociation constant
pH
Vapor pressure
50. 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.
Principle quantum number
atomic radius
quanta
actinide series