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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. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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2. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Group 1A
energy state
STP
Common ion effect
3. 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.
Neutron
Effective nuclear charge
Nucleus
atomic radius
4. 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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5. 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
Lyman series
Diffusion
solvation
6. 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
Neutron
Dispersion Forces
percent composition
Disproportionation
7. 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
s orbital
pH
Mass number
8. The average distance between the nuclei of two bonded atoms
electron affinity
Disproportionation
bond length
Normality
9. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Spin quantum number
Ion
Rydberg constant
Noble gases
10. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Water dissociation Constant
quanta
Group 6A
11. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Solute
Water dissociation Constant
molecule
redox reaction
12. Common definition of acids as proton (H+) donors and bases as proton acceptors
hydrogen bonding
Bronsted - Lowry definition
Resonance structure
Electrolyte
13. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Buffer
pH
Avagadros number
Arrhenius Definition
14. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Solvent
pi bonds
compound
Neutralization reaction
15. An atom or group of atoms that has a positive or negative charge
Effective nuclear charge
Decomposition reaction
Ion
Formula weight
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. 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
Diprotic Base
Neutralization reaction
Arrhenius Definition
Graham's Law
18. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
solvation
Period
Charles and Gay Lussac's Law
19. 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
gram equivalent weight
Molecular orbital
Proton
chemical reaction
20. In a solution - the substance that dissolves in the solvent
Atomic absorption Spectra
effective nuclear charge
Group 4A
Solute
21. Simplest whole # ration of atoms in a compound
Emperical Formula
Halogens
Equlibrium constant
Acid dissociation constant
22. An ionic compound that resists changes in its pH
Covalent Bond
Common ion effect
Buffer
Raoult's Law
23. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Molar solubility
percent composition
Molality
24. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Intermolecular forces
quantum
Formula weight
Group 2A
25. A reaction in which atoms of one element take the place of atoms of another element in a compound
Rydberg constant
Dipole
Ion
single displacement reaction
26. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Diprotic Base
ionic cmpound
Reaction order
amorphous solid
27. Two or more atoms held together by covalent bonds
Planck's Constant
Graham's Law
molecule
Disproportionation
28. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Group 2A
Half equivalence point
Noble gases
29. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
single displacement reaction
molecule
Henderson Hasselbalch Equation
Ion dipole interactions
30. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
redox reaction
law of constant composition
molecular weight
31. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Equlibrium constant
redox reaction
Period
Activation energy
32. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Dispersion Forces
Molarity
Emperical Formula
Lewis acid base reaction
33. 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
Molarity
Rate law
molecular weight
azimuthal quantum number
34. PH of a molecule at which it contains no net electric charge - isoelectric point.
quanta
pI
Acid dissociation constant
Phase diagram
35. 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
Group 3A
Theoretical yield
Solution equilibrium
Effusion
36. 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
Chemical Kinetics
molecular weight
Ion product
Resonance structure
37. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Neutron
crystalline solid
Dipole Dipole interaction
38. 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.
Effective nuclear charge
pi bonds
Redox Half Reaction
Electronegativity
39. A definite stable energy that a physical system can have
empirical formula
energy state
actinide series
electron configuration
40. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Mass number
Lewis structure
Network covalent
Theoretical yield
41. 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
Equilibrium
amorphous solid
Molarity
Equlibrium constant
42. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Reaction mechanism
Molality
hydrogen bonding
Neutron
43. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Charles and Gay Lussac's Law
sigma bond
London forces
Group 7A
44. 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
indicator
Solvent
Bronsted Lowry
Ionization energy
45. 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
Electronegativity
Henderson Hasselbalch Equation
Reaction mechanism
46. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Emperical Formula
compound
Mass number
Dipole
47. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Common ion effect
molecule
Raoult's Law
atomic radius
48. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Free radical
Common ion effect
atomic emission spectrum
atomic theory
49. 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
ionic cmpound
Balmer series
atomic emission spectrum
Spin quantum number
50. Substance in which a solute is dissolved to form a solution
Mass number
Solvent
Effective nuclear charge
subshell