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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. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Lewis acid base reaction
polymer
Pauli exclusion principle
angular momentum in the bohr model
2. 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.
Group 4A
Rate law
Resonance structure
VSEPR
3. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Noble gases
Arrhenius Definition
sigma bond
Ion
4. A subdivision of an energy level in an atom. They are divided into orbitals.
decomposition reaction
Ion dipole interactions
und's rule
subshell
5. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
pi bonds
Group 2A
subshell
empirical formula
6. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
percent composition
Halogens
Electrolyte
Principle quantum number
7. 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.
Spin quantum number
Dipole Dipole interaction
Ion product
Formula weight
8. 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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9. Elements in the middle of the periodic table - in groups 3-12.
Network covalent
transition elements
Magnetic quantum number
Rydberg constant
10. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Strong acid
Nucleus
Group 4A
Network covalent
11. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
compound
Pauli exclusion principle
Intermolecular forces
theoretical yield
12. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
Ion
Effusion
Conjugate acids and Bases
Atomic absorption Spectra
13. 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.
Avagadros number
Buffer
quantum numbers
Balmer series
14. 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
Balmer series
Atomic absorption Spectra
atomic radius
Solution equilibrium
15. 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.
crystalline solid
STP
Emperical Formula
Electronegativity
16. 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
Dipole Dipole interaction
Hydrogen bonding
redox reaction
Atomic weight
17. (chemistry) a substance that changes color to indicate the presence of some ion or substance
London forces
indicator
Molar solubility
ionic cmpound
18. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
electron affinity
energy state
Equivalence point
19. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
pI
Group 2A
Amphoteric
Le chateliers Principle
20. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Amphoteric
Charles and Gay Lussac's Law
polymer
Covalent Bond
21. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Free radical
lewis base
Molality
atomic emission spectrum
22. 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 configuration
Charles and Gay Lussac's Law
Halogens
23. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Dipole
Rate determining step
Solvent
Ionization energy
24. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Effusion
Formula weight
bond energy
Lewis acid base reaction
25. 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
Halogens
percent composition
Group 4A
26. The percent by mass of each element in a compound
percent composition
Molar solubility
Ionization energy
Le chateliers Principle
27. 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
Conjugate acids and Bases
physical reaction
Acid dissociation constant
actinide series
28. A solution in which water is the solvent
Aqueous Solution
lathanide series
Formula weight
hydrogen bonding
29. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Ion product
Amphoteric
Strong acid
ionic cmpound
30. A definite stable energy that a physical system can have
Group 5A
energy state
pH
Solubility Product Constant
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
Rate determining step
Triple point
angular momentum in the bohr model
Balmer series
32. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
und's rule
Theoretical yield
Group 2A
Reaction mechanism
33. 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.
Combination Reaction
Decomposition reaction
atomic radius
bond energy
34. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
London forces
Dipole Dipole interaction
Planck's Constant
quantum
35. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Titration
Octet Rule
Dipole Dipole interaction
Activation energy
36. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Group 7A
und's rule
Rate law
37. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Ground state
Normality
Group 7A
Dipole
38. Common definition of acids as proton (H+) donors and bases as proton acceptors
Principle quantum number
Redox Half Reaction
Bronsted - Lowry definition
Phase diagram
39. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Diffusion
Atomic absorption Spectra
lewis base
Lewis structure
40. 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.
Lewis structure
Diprotic Base
Group 3A
und's rule
41. An atom or group of atoms that has a positive or negative charge
Ion
Decomposition reaction
Bronsted - Lowry definition
quanta
42. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Nonpolar covalent bond
Group 1A
Water dissociation Constant
atomic theory
43. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Equivalence point
indicator
Redox Half Reaction
Colligative properties
44. 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
Redox Half Reaction
heisenberg uncertainty principle
decomposition reaction
Equlibrium constant
45. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Spin quantum number
Diprotic Base
Formula weight
46. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Effective nuclear charge
electron configuration
Molar solubility
d orbital
47. 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
Rydberg constant
Azeotrope
Redox Half Reaction
Graham's Law
48. 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
single displacement reaction
Atomic absorption Spectra
theoretical yield
49. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Group 2A
Common ion effect
redox reaction
Dipole
50. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
crystalline solid
Period
effective nuclear charge
Bronsted Lowry