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MCAT Chemistry
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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 ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Group 7A
Equlibrium constant
Molality
Atomic absorption Spectra
2. A base that can accept two moles of H+ per mole of itself (ex: SO4
Ionic Bond
Electrolyte
Balmer series
Diprotic Base
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. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
energy state
Solution equilibrium
Conjugate acids and Bases
quantum numbers
5. A subdivision of an energy level in an atom. They are divided into orbitals.
pH
Disproportionation
angular momentum in the bohr model
subshell
6. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Atomic absorption Spectra
Solute
Le chateliers Principle
pH
7. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
polymer
azimuthal quantum number
Molecular orbital
8. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
atomic radius
redox reaction
Ionization energy
9. 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
Equlibrium constant
Nucleus
Le chateliers Principle
hydrogen bonding
10. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Arrhenius Definition
Conjugate acids and Bases
Equivalence point
bond length
11. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
Atomic absorption Spectra
Percent yield
actinide series
solvation
12. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
bond length
Effusion
ionic cmpound
Arrhenius Definition
13. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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14. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
pH
The bohr model
electromagnetic energy of photons emmited from electrons at ground state
Collision theory of chemical Kinetics
15. The energy required to break a chemical bond and form neutral isolated atoms
Emperical Formula
Molality
Bronsted - Lowry definition
bond energy
16. An atom or group of atoms that has a positive or negative charge
Covalent Bond
Ion
VSEPR
representative elements
17. 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
Azeotrope
s orbital
Principle quantum number
percent composition
18. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Ion
Phase diagram
Molar solubility
Arrhenius Definition
19. Slightly less reactive than alkali metals - comprise group II
Charles and Gay Lussac's Law
Alkaline earths
Triple point
Intermolecular forces
20. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
transition elements
polymer
Effective nuclear charge
STP
21. A solution in which water is the solvent
Aqueous Solution
electromagnetic energy of photons emmited from electrons at ground state
Period
subshell
22. 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
atomic theory
Atomic weight
Solubility Product Constant
Resonance structure
23. 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
VSEPR
Titration
Effective nuclear charge
Colligative properties
24. 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
Molarity
amorphous solid
Effective nuclear charge
Dispersion Forces
25. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher
VSEPR
Solubility Product Constant
Formal Charge
Lyman series
26. Named after their cation and anion
ionic cmpound
Intermolecular forces
The bohr model
Ion dipole interactions
27. In a solution - the substance that dissolves in the solvent
Equivalence point
Lewis structure
Solute
periodic trends
28. 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
Dipole
Magnetic quantum number
Redox Half Reaction
Lyman series
29. Common definition of acids as proton (H+) donors and bases as proton acceptors
Buffer
VSEPR
Percent composition
Bronsted - Lowry definition
30. Property of the elements that can be predicted from the arrangement of the periodic table
physical reaction
periodic trends
Resonance structure
Diffusion
31. 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
Group 7A
Rate law
Diprotic Base
Amphoteric
32. E=hc/?
Theoretical yield
Group 5A
chemical reaction
electromagnetic energy of photons emmited from electrons at ground state
33. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
law of constant composition
Mass number
molecule
Nucleus
34. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
Solution equilibrium
Ionic Bond
mole
35. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
polymer
Dipole Dipole interaction
Strong acid
Bronsted - Lowry definition
36. 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
London forces
single displacement reaction
Group 1A
molecule
37. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Atomic absorption Spectra
Avagadros number
Combination Reaction
electron configuration
38. PH of a molecule at which it contains no net electric charge - isoelectric point.
decomposition reaction
Azeotrope
electron configuration
pI
39. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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40. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
und's rule
Strong acid
chemical reaction
Combination Reaction
41. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
d orbital
Spin quantum number
molecular weight
Theoretical yield
42. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Atomic absorption Spectra
Lewis acid base reaction
Equlibrium constant
Lewis structure
43. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Buffer
Atomic absorption Spectra
ionic cmpound
Acid dissociation constant
44. 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
Dipole
Hydrogen bonding
Chemical Kinetics
Phase diagram
45. 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
Solubility Product Constant
decomposition reaction
Ion
Solution equilibrium
46. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Lewis structure
Magnetic quantum number
Vapor pressure
Molar solubility
47. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
polymer
Lewis acid base reaction
effective nuclear charge
48. The average distance between the nuclei of two bonded atoms
Collision theory of chemical Kinetics
bond length
Intermolecular forces
Dipole
49. 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
Charles and Gay Lussac's Law
Group 6A
Nucleus
Proton
50. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
empirical formula
Formula weight
electromagnetic energy of photons emmited from electrons at ground state
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