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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. 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
Solution equilibrium
Formula weight
energy state
Phase diagram
2. 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
Solvent
Lewis definition
Group 7A
3. 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
electron affinity
atomic theory
Raoult's Law
4. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
compound
mole
ionic cmpound
5. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Ionization energy
Formula weight
Buffer
electromagnetic energy of photons emmited from electrons at ground state
6. E=hc/?
Reaction mechanism
electromagnetic energy of photons emmited from electrons at ground state
Resonance structure
percent composition
7. Common definition of acids as proton (H+) donors and bases as proton acceptors
Redox Half Reaction
Ground state
Buffer
Bronsted - Lowry definition
8. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
pi bonds
Titration
Phase diagram
Mass number
9. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
STP
Combination Reaction
sigma bond
Nucleus
10. Tells you how much solute is present compared to the amount of solvent
Charles and Gay Lussac's Law
Group 3A
Concentration
law of constant composition
11. 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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12. A substance that - when dissolved in water - results in a solution that can conduct electricity
Planck's Constant
Percent composition
Group 1A
Electrolyte
13. 5 different orbitals shaped like clover leaves and max electrons is 10
Pauli exclusion principle
d orbital
Rate determining step
Group 4A
14. The lowest allowable energy state of an atom
Solute
periodic trends
Ground state
Rydberg constant
15. 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.
Diffusion
Dispersion Forces
Formula weight
Equivalence point
16. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
single displacement reaction
bond length
redox reaction
Rydberg constant
17. 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
Ionization energy
Normality
Mass number
Resonance structure
18. 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.
decomposition reaction
Group 5A
Redox Half Reaction
Ion
19. 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.
Neutron
Molecular orbital
Equilibrium
Atomic absorption Spectra
20. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
Lewis definition
representative elements
Molar solubility
21. An atom or group of atoms that has a positive or negative charge
hydrogen bonding
d orbital
Percent yield
Ion
22. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
atomic theory
Collision theory of chemical Kinetics
atomic emission spectrum
Lewis definition
23. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
atomic radius
Group 7A
Arrhenius Definition
Acid dissociation constant
24. 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
Percent yield
Ionization energy
Hydrogen bonding
Formal Charge
25. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Bronsted - Lowry definition
Dispersion Forces
electromagnetic energy of photons emmited from electrons at ground state
Rate law
26. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
gram equivalent weight
energy state
Dispersion Forces
27. Any sample of a given compound will contain the same elements in the identical mass ratio.
redox reaction
law of constant composition
Colligative properties
Nonpolar covalent bond
28. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Conjugate acids and Bases
Theoretical yield
Ion dipole interactions
29. The process of decomposing a chemical compound by the passage of an electric current.
Percent yield
electrolysis
Electrolyte
pi bonds
30. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Theoretical yield
Raoult's Law
Diffusion
solvation
31. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Aqueous Solution
pH
Amphoteric
32. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Buffer
Mass number
Noble gases
quantum
33. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Nonpolar covalent bond
Ion product
Resonance structure
34. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
pH
Reaction mechanism
Henderson Hasselbalch Equation
35. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
Free radical
Aqueous Solution
Concentration
Resonance structure
36. 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.
Raoult's Law
Group 3A
Rate law
transition elements
37. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Collision theory of chemical Kinetics
azimuthal quantum number
Group 2A
38. 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.
Formal Charge
empirical formula
Neutron
Balmer series
39. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Bronsted Lowry
Rate determining step
Group 1A
quanta
40. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
Formula weight
Henderson Hasselbalch Equation
Theoretical yield
41. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Dipole Dipole interaction
Lewis definition
compound
Mass number
42. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
The bohr model
Noble gases
Molality
Electronegativity
43. Redox reaction - in which the same species is both oxidized and reduced.
Group 5A
Acid dissociation constant
azimuthal quantum number
Disproportionation
44. 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
Molarity
single displacement reaction
und's rule
Magnetic quantum number
45. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Water dissociation Constant
Lewis structure
gram equivalent weight
Amphoteric
46. Small discrete increments of energy.
bond length
quanta
Free radical
Spin quantum number
47. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Percent yield
Half equivalence point
indicator
Raoult's Law
48. 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.
Neutralization reaction
Bronsted Lowry
Ion product
crystalline solid
49. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
theoretical yield
The bohr model
Formal Charge
50. Simplest whole # ration of atoms in a compound
Vapor pressure
Emperical Formula
lewis base
Lewis acid base reaction