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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. 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
Equivalence point
Equlibrium constant
electron affinity
Raoult's Law
2. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Spin quantum number
Emperical Formula
Dipole
ionic cmpound
3. 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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4. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Amphoteric
Nonpolar covalent bond
Group 4A
Intermolecular forces
5. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Group 3A
energy state
The bohr model
Bronsted Lowry
6. Redox reaction - in which the same species is both oxidized and reduced.
empirical formula
Disproportionation
Titration
redox reaction
7. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
amorphous solid
Avagadros number
STP
Activation energy
8. Acids defined as electron - pair acceptors and bases as electron - pair donors.
law of constant composition
Dipole
Lewis definition
periodic trends
9. 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.
Solvent
lathanide series
Reaction order
Solubility Product Constant
10. 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-
electron affinity
pi bonds
Water dissociation Constant
Principle quantum number
11. 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.
Ion
molecular weight
redox reaction
atomic radius
12. Named after their cation and anion
ionic cmpound
Ion
Molar solubility
electrolysis
13. The process of decomposing a chemical compound by the passage of an electric current.
bond length
lewis base
Group 4A
electrolysis
14. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Group 3A
Concentration
Proton
Reaction order
15. 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
Atomic absorption Spectra
Formula weight
Vapor pressure
16. 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
Arrhenius Definition
Halogens
Rate determining step
Group 3A
17. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Azeotrope
redox reaction
Group 3A
electrolysis
18. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
representative elements
Solubility Product Constant
bond length
19. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
quanta
representative elements
Le chateliers Principle
20. 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
Dispersion Forces
Covalent Bond
lewis base
Resonance structure
21. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Disproportionation
Ionic Bond
single displacement reaction
22. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Lyman series
redox reaction
Electronegativity
physical reaction
23. E=hc/?
Diffusion
electromagnetic energy of photons emmited from electrons at ground state
Molar solubility
Pauli exclusion principle
24. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Common ion effect
azimuthal quantum number
Bronsted - Lowry definition
Theoretical yield
25. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
s orbital
Lyman series
Rate law
26. 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
Equlibrium constant
Group 7A
Ion
Azeotrope
27. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
solvation
crystalline solid
Effusion
periodic trends
28. 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
Chemical Kinetics
Lewis structure
Rate law
29. The maximum amount of product that can be produced from a given amount of reactant
VSEPR
electron affinity
theoretical yield
Henry's Law
30. A reaction where a compound does Not change its molecular structure.
Molarity
physical reaction
mole
percent composition
31. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
atomic radius
energy state
empirical formula
Group 1A
32. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Period
Raoult's Law
Atomic weight
Electronegativity
33. 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
compound
Balmer series
Ionic Bond
34. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
pH
Molarity
Ion product
Covalent Bond
35. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Molar solubility
Arrhenius Definition
Principle quantum number
36. The Percent by mass of each element in a compound.
atomic radius
Atomic weight
atomic radius
Percent composition
37. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Resonance structure
Amphoteric
atomic theory
Magnetic quantum number
38. 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.
crystalline solid
Formula weight
bond energy
Ground state
39. 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.
Net ionic equation
Henderson Hasselbalch Equation
Molarity
Half equivalence point
40. Tells you how much solute is present compared to the amount of solvent
Dipole
Concentration
Planck's Constant
amorphous solid
41. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Atomic weight
Aqueous Solution
Chemical Kinetics
mole
42. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Emperical Formula
Collision theory of chemical Kinetics
theoretical yield
Intermolecular forces
43. Small discrete increments of energy.
Solute
Halogens
Ionic Bond
quanta
44. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Diffusion
lathanide series
Chemical Kinetics
single displacement reaction
45. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Chemical Kinetics
Lyman series
law of constant composition
Halogens
46. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Effective nuclear charge
Group 5A
Triple point
47. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Percent composition
Common ion effect
Percent yield
Net ionic equation
48. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
Dipole
law of constant composition
Theoretical yield
representative elements
49. 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
Solute
s orbital
theoretical yield
50. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
VSEPR
Henry's Law
Nucleus
Strong acid
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