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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. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Phase diagram
Molecular orbital
quantum numbers
molecular weight
2. 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
atomic radius
Spin quantum number
Reaction order
Ion product
3. In a solution - the substance that dissolves in the solvent
Proton
Group 7A
Solute
Atomic absorption Spectra
4. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Neutralization reaction
Dipole
STP
effective nuclear charge
5. 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.
atomic radius
Ionic Bond
Effective nuclear charge
Ion product
6. The process of decomposing a chemical compound by the passage of an electric current.
Group 3A
electron configuration
atomic radius
electrolysis
7. 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
actinide series
Graham's Law
Solution equilibrium
The bohr model
8. Named after their cation and anion
Group 6A
ionic cmpound
Atomic weight
Noble gases
9. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Atomic weight
Vapor pressure
Pauli exclusion principle
electron configuration
10. The slowest elementary step which is the limit for the rate of the other steps
Bronsted - Lowry definition
Raoult's Law
Avagadros number
Rate determining step
11. A reaction where a compound does Not change its molecular structure.
Rate law
physical reaction
Lewis acid base reaction
mole
12. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Half equivalence point
Group 7A
Pauli exclusion principle
crystalline solid
13. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Common ion effect
Ionization energy
Molar solubility
14. 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
Magnetic quantum number
Hydrogen bonding
bond length
polymer
15. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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16. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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17. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Dipole Dipole interaction
Intermolecular forces
electromagnetic energy of photons emmited from electrons at ground state
decomposition reaction
18. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Amphoteric
Ion
Common ion effect
Group 2A
19. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
gram equivalent weight
Lyman series
heisenberg uncertainty principle
Molarity
20. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Conjugate acids and Bases
Principle quantum number
pH
Avagadros number
21. Numbers that specify the properties of atomic orbitals and of their electrons
Electronegativity
quantum numbers
Rate determining step
Hydrogen bonding
22. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Lewis definition
Halogens
Net ionic equation
Resonance structure
23. 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
hydrogen bonding
Equilibrium
atomic theory
Nonpolar covalent bond
24. E=hc/?
Ground state
Equilibrium
electromagnetic energy of photons emmited from electrons at ground state
Formula weight
25. Having characteristics of both an acid and a base and capable of reacting as either
Dipole
Lewis definition
Ionization energy
Amphoteric
26. 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
periodic trends
Colligative properties
pi bonds
Ion
27. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Combination Reaction
Diprotic Base
Nonpolar covalent bond
Group 2A
28. Any sample of a given compound will contain the same elements in the identical mass ratio.
Group 7A
Le chateliers Principle
lathanide series
law of constant composition
29. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
energy state
quantum
Half equivalence point
Henderson Hasselbalch Equation
30. 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
Proton
Group 2A
Dipole Dipole interaction
Collision theory of chemical Kinetics
31. A subdivision of an energy level in an atom. They are divided into orbitals.
periodic trends
Principle quantum number
subshell
Diprotic Base
32. 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
Activation energy
Group 3A
Equlibrium constant
Halogens
33. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Titration
amorphous solid
Group 4A
Conjugate acids and Bases
34. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Theoretical yield
Arrhenius Definition
Molecular orbital
Percent yield
35. The process by which one or more substances change to produce one or more different substances
Molarity
chemical reaction
Group 4A
Theoretical yield
36. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
crystalline solid
Group 1A
Lewis definition
atomic radius
37. (chemistry) p(otential of) H(ydrogen)
Magnetic quantum number
ionic cmpound
pH
Formula weight
38. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
electrolysis
Effusion
Dipole Dipole interaction
bond energy
39. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
lewis base
Percent yield
electron affinity
40. 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
Solute
Halogens
Lewis structure
Group 7A
41. A reaction in which atoms of one element take the place of atoms of another element in a compound
redox reaction
Ionic Bond
single displacement reaction
d orbital
42. The Percent by mass of each element in a compound.
Solute
sigma bond
Percent composition
Ion dipole interactions
43. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Conjugate acids and Bases
Lewis definition
Diffusion
Neutron
44. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Percent composition
Concentration
Combination Reaction
angular momentum in the bohr model
45. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
angular momentum in the bohr model
Common ion effect
Pauli exclusion principle
Balmer series
46. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
London forces
Azeotrope
Aqueous Solution
47. 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.
Vapor pressure
atomic radius
Activation energy
Aqueous Solution
48. 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
Lyman series
Vapor pressure
Lewis structure
Azeotrope
49. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Solution equilibrium
Water dissociation Constant
Group 4A
law of constant composition
50. 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.
Redox Half Reaction
Diprotic Base
physical reaction
Electronegativity