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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. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
s orbital
Solubility Product Constant
Intermolecular forces
Net ionic equation
2. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Alkaline earths
Lewis acid base reaction
Group 3A
3. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
redox reaction
compound
Lewis structure
percent composition
4. Substance in which a solute is dissolved to form a solution
redox reaction
Neutralization reaction
Solvent
Diprotic Base
5. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
Group 4A
law of constant composition
Equilibrium
6. 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.
atomic radius
ionic cmpound
representative elements
Formal Charge
7. 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
STP
Half equivalence point
electron configuration
Lyman series
8. 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
Covalent Bond
Solution equilibrium
Vapor pressure
Percent yield
9. 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
physical reaction
Spin quantum number
Electronegativity
10. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
theoretical yield
Reaction mechanism
percent composition
11. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
lathanide series
electrolysis
London forces
Concentration
12. 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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13. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
bond length
Avagadros number
pi bonds
14. Gram equivalent weight of solute per liter of solution - often denoted by N.
Effective nuclear charge
Normality
Common ion effect
Solution equilibrium
15. 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
Water dissociation Constant
Equlibrium constant
Lewis definition
16. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Nonpolar covalent bond
Concentration
law of constant composition
17. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Rate law
Group 2A
Water dissociation Constant
Group 4A
18. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Covalent Bond
Group 2A
Reaction mechanism
Triple point
19. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
Equilibrium
atomic radius
Equivalence point
Water dissociation Constant
20. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Ionic Bond
crystalline solid
pi bonds
Group 2A
21. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Group 7A
und's rule
mole
decomposition reaction
22. A reaction in which atoms of one element take the place of atoms of another element in a compound
Atomic weight
Raoult's Law
single displacement reaction
Molality
23. Simplest whole # ration of atoms in a compound
Dipole
Molarity
Rate law
Emperical Formula
24. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
bond energy
single displacement reaction
Pauli exclusion principle
compound
25. Sum of the protons and neutrons in an element often denoted by the letter A
Rate determining step
Mass number
d orbital
atomic theory
26. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
Amphoteric
Lewis definition
electron configuration
27. 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.
Reaction mechanism
Diffusion
crystalline solid
lathanide series
28. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
atomic radius
Azeotrope
Atomic absorption Spectra
Vapor pressure
29. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Electrolyte
quantum
Decomposition reaction
d orbital
30. 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
Reaction mechanism
Collision theory of chemical Kinetics
Molality
Ionization energy
31. Small discrete increments of energy.
pi bonds
Collision theory of chemical Kinetics
Triple point
quanta
32. Elements in the middle of the periodic table - in groups 3-12.
Planck's Constant
Lyman series
transition elements
redox reaction
33. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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34. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Rate law
Ion dipole interactions
Group 1A
d orbital
35. PH of a molecule at which it contains no net electric charge - isoelectric point.
Network covalent
und's rule
pI
Diffusion
36. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Molality
Ionic Bond
Lewis structure
quantum
37. 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
single displacement reaction
Ionic Bond
decomposition reaction
Molecular orbital
38. Tells you how much solute is present compared to the amount of solvent
Alkaline earths
Concentration
Lyman series
Half equivalence point
39. 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
Solubility Product Constant
effective nuclear charge
azimuthal quantum number
Ion dipole interactions
40. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Ion
Noble gases
Group 1A
Network covalent
41. Property of the elements that can be predicted from the arrangement of the periodic table
Dispersion Forces
periodic trends
Disproportionation
Free radical
42. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Molar solubility
Emperical Formula
Pauli exclusion principle
Lewis structure
43. 5 valence electrons -3 ions - Nitride N
gram equivalent weight
Acid dissociation constant
Noble gases
Group 5A
44. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
angular momentum in the bohr model
Noble gases
electron configuration
Reaction order
45. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Equivalence point
Free radical
Net ionic equation
hydrogen bonding
46. (chemistry) p(otential of) H(ydrogen)
pH
bond energy
Period
Ionization energy
47. 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
Atomic absorption Spectra
electromagnetic energy of photons emmited from electrons at ground state
Arrhenius Definition
theoretical yield
48. 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.
Group 3A
Group 6A
Effective nuclear charge
Henderson Hasselbalch Equation
49. An elementary particle with 0 charge and mass about equal to a proton
Free radical
Neutron
Balmer series
Nucleus
50. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
sigma bond
Effusion
physical reaction
Noble gases