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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.
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 ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Aqueous Solution
Equlibrium constant
Titration
2. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Reaction order
indicator
lathanide series
3. Common definition of acids as proton (H+) donors and bases as proton acceptors
STP
Decomposition reaction
Bronsted - Lowry definition
Normality
4. (chemistry) p(otential of) H(ydrogen)
Common ion effect
pI
pH
Ion dipole interactions
5. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
atomic radius
Acid dissociation constant
Aqueous Solution
6. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Solvent
Avagadros number
Half equivalence point
7. Sum of the protons and neutrons in an element often denoted by the letter A
The bohr model
Halogens
Neutron
Mass number
8. 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
London forces
Azeotrope
und's rule
Magnetic quantum number
9. The process of decomposing a chemical compound by the passage of an electric current.
Group 1A
polymer
electrolysis
Theoretical yield
10. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
physical reaction
Principle quantum number
Spin quantum number
Atomic weight
11. 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.
effective nuclear charge
Solubility Product Constant
Equilibrium
Arrhenius Definition
12. In a solution - the substance that dissolves in the solvent
heisenberg uncertainty principle
Solute
Equlibrium constant
subshell
13. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
molecule
Chemical Kinetics
Rydberg constant
14. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Graham's Law
Mass number
Aqueous Solution
15. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Ionic Bond
molecular weight
lathanide series
Molarity
16. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Raoult's Law
quanta
Combination Reaction
Solution equilibrium
17. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Concentration
empirical formula
redox reaction
Collision theory of chemical Kinetics
18. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
percent composition
Covalent Bond
polymer
19. 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
pI
Nonpolar covalent bond
Titration
Equivalence point
20. 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
Rydberg constant
Amphoteric
Group 4A
azimuthal quantum number
21. 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
azimuthal quantum number
Effective nuclear charge
Octet Rule
22. 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.
Balmer series
Group 1A
Net ionic equation
quantum
23. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Neutron
atomic radius
Equlibrium constant
Solute
24. Any sample of a given compound will contain the same elements in the identical mass ratio.
Balmer series
crystalline solid
heisenberg uncertainty principle
law of constant composition
25. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
solvation
Charles and Gay Lussac's Law
Common ion effect
Neutralization reaction
26. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
quanta
Bronsted Lowry
Equilibrium
Proton
27. Chalcogens - - Oxide O
Collision theory of chemical Kinetics
indicator
Proton
Group 6A
28. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Combination Reaction
Lyman series
Colligative properties
Bronsted - Lowry definition
29. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Triple point
Formula weight
Pauli exclusion principle
30. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Bronsted - Lowry definition
Planck's Constant
effective nuclear charge
d orbital
31. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
indicator
electron configuration
mole
32. 5 valence electrons -3 ions - Nitride N
Titration
Noble gases
Group 5A
Theoretical yield
33. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Titration
atomic radius
Planck's Constant
electron configuration
34. A subdivision of an energy level in an atom. They are divided into orbitals.
Formal Charge
Rydberg constant
Octet Rule
subshell
35. The average distance between the nuclei of two bonded atoms
bond length
amorphous solid
Group 4A
electromagnetic energy of photons emmited from electrons at ground state
36. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
Normality
Activation energy
quantum
Principle quantum number
37. 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
Ion dipole interactions
empirical formula
London forces
38. The energy required to break a chemical bond and form neutral isolated atoms
Molecular orbital
Ion dipole interactions
bond energy
Intermolecular forces
39. 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-
ionic cmpound
Noble gases
Water dissociation Constant
Raoult's Law
40. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
The bohr model
Network covalent
Noble gases
redox reaction
41. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
physical reaction
empirical formula
Nucleus
Reaction mechanism
42. 2.18 x 10^-18 J/electron
pI
Ion product
Equlibrium constant
Rydberg constant
43. 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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44. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Nonpolar covalent bond
Molarity
single displacement reaction
Strong acid
45. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Proton
Lewis structure
Emperical Formula
Electronegativity
46. Named after their cation and anion
Theoretical yield
ionic cmpound
Strong acid
pH
47. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Titration
Network covalent
Diffusion
48. 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.
Group 7A
atomic radius
Percent yield
Collision theory of chemical Kinetics
49. A horizontal row of elements in the periodic table
Period
Covalent Bond
Buffer
Dipole Dipole interaction
50. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
sigma bond
Solution equilibrium
Ion
Reaction order
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