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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 reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
physical reaction
periodic trends
atomic radius
2. 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
molecular weight
Proton
Balmer series
Reaction order
3. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Strong acid
Neutron
Alkaline earths
4. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Amphoteric
Molality
molecular weight
lathanide series
5. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Henderson Hasselbalch Equation
Common ion effect
Avagadros number
Lyman series
6. PH of a molecule at which it contains no net electric charge - isoelectric point.
quanta
Buffer
STP
pI
7. (chemistry) a substance that changes color to indicate the presence of some ion or substance
VSEPR
lewis base
Ion
indicator
8. 5 different orbitals shaped like clover leaves and max electrons is 10
Pauli exclusion principle
d orbital
ionic cmpound
actinide series
9. 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
crystalline solid
Atomic absorption Spectra
The bohr model
10. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Collision theory of chemical Kinetics
Network covalent
Ion
Intermolecular forces
11. In a solution - the substance that dissolves in the solvent
Decomposition reaction
Solute
quanta
Group 6A
12. Having characteristics of both an acid and a base and capable of reacting as either
Ion product
Amphoteric
Solution equilibrium
Noble gases
13. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
crystalline solid
effective nuclear charge
lewis base
Reaction order
14. 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
Pauli exclusion principle
azimuthal quantum number
Conjugate acids and Bases
Azeotrope
15. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Colligative properties
Alkaline earths
atomic emission spectrum
Solubility Product Constant
16. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Dispersion Forces
decomposition reaction
Ion
Resonance structure
17. 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
effective nuclear charge
Colligative properties
azimuthal quantum number
Group 6A
18. An elementary particle with 0 charge and mass about equal to a proton
Dispersion Forces
Neutron
Concentration
Amphoteric
19. 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
Nucleus
effective nuclear charge
Group 6A
Phase diagram
20. 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
Group 1A
The bohr model
Percent composition
representative elements
21. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
single displacement reaction
Acid dissociation constant
Triple point
22. 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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23. 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
s orbital
Ion
Group 3A
24. An atom or group of atoms that has a positive or negative charge
Solute
Bronsted - Lowry definition
molecular weight
Ion
25. The lowest allowable energy state of an atom
Molality
Amphoteric
Ground state
Ion dipole interactions
26. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
atomic theory
solvation
STP
Collision theory of chemical Kinetics
27. 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
Aqueous Solution
Ground state
Avagadros number
hydrogen bonding
28. Gram equivalent weight of solute per liter of solution - often denoted by N.
Group 3A
Molarity
Normality
bond energy
29. 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
Diprotic Base
Neutralization reaction
Solubility Product Constant
30. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
angular momentum in the bohr model
Activation energy
Dipole
31. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Effusion
Molecular orbital
Dipole Dipole interaction
32. 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
Resonance structure
Dispersion Forces
redox reaction
quantum numbers
33. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
lewis base
pi bonds
atomic radius
Buffer
34. Named after their cation and anion
ionic cmpound
VSEPR
Activation energy
Rydberg constant
35. 5 valence electrons -3 ions - Nitride N
Group 5A
Vapor pressure
sigma bond
Group 1A
36. 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.
Ion product
amorphous solid
single displacement reaction
Redox Half Reaction
37. A reaction where a compound does Not change its molecular structure.
Rate law
physical reaction
quantum
Theoretical yield
38. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Redox Half Reaction
Normality
quanta
angular momentum in the bohr model
39. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Dipole Dipole interaction
crystalline solid
Equilibrium
Dipole
40. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
pH
Percent yield
theoretical yield
Rate law
41. 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.
Nucleus
Group 5A
Balmer series
Group 3A
42. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
law of constant composition
Molecular orbital
Bronsted - Lowry definition
Ground state
43. 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
Nucleus
Solution equilibrium
single displacement reaction
physical reaction
44. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Decomposition reaction
electromagnetic energy of photons emmited from electrons at ground state
Water dissociation Constant
45. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Dispersion Forces
Reaction order
Vapor pressure
Triple point
46. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Vapor pressure
Group 7A
atomic radius
Spin quantum number
47. 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
Colligative properties
Diffusion
Vapor pressure
48. 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
Titration
pi bonds
Magnetic quantum number
Network covalent
49. Redox reaction - in which the same species is both oxidized and reduced.
pI
Strong acid
Disproportionation
sigma bond
50. 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.
Net ionic equation
Atomic absorption Spectra
Molar solubility
subshell