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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. Common definition of acids as proton (H+) donors and bases as proton acceptors
Concentration
quantum
Bronsted - Lowry definition
Neutralization reaction
2. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
The bohr model
Solute
Solution equilibrium
Bronsted Lowry
3. A reaction in which atoms of one element take the place of atoms of another element in a compound
bond energy
single displacement reaction
Atomic absorption Spectra
pi bonds
4. 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
representative elements
Le chateliers Principle
azimuthal quantum number
Ion
5. 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
Solution equilibrium
atomic theory
heisenberg uncertainty principle
Spin quantum number
6. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Group 3A
Ion dipole interactions
Colligative properties
7. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Halogens
Covalent Bond
Resonance structure
8. Elements in the middle of the periodic table - in groups 3-12.
Pauli exclusion principle
Percent yield
transition elements
molecular weight
9. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Effusion
atomic radius
atomic theory
subshell
10. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Halogens
Electronegativity
Normality
Ion
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
London forces
atomic radius
Free radical
Formula weight
12. The process of decomposing a chemical compound by the passage of an electric current.
Equilibrium
Ion
Water dissociation Constant
electrolysis
13. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Acid dissociation constant
pI
Net ionic equation
Molality
14. 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
Resonance structure
Molar solubility
London forces
Halogens
15. E=hc/?
Lewis acid base reaction
electromagnetic energy of photons emmited from electrons at ground state
Effusion
representative elements
16. 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-
solvation
Water dissociation Constant
molecule
polymer
17. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Combination Reaction
Group 2A
empirical formula
Bronsted Lowry
18. A reaction in which atoms of one element take the place of atoms of another element in a compound
Neutralization reaction
und's rule
single displacement reaction
subshell
19. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Le chateliers Principle
Avagadros number
und's rule
pH
20. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
single displacement reaction
STP
Aqueous Solution
Reaction order
21. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Planck's Constant
Diffusion
Dipole Dipole interaction
Collision theory of chemical Kinetics
22. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
subshell
electron affinity
Intermolecular forces
Chemical Kinetics
23. 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
Emperical Formula
Hydrogen bonding
Group 7A
Ground state
24. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
single displacement reaction
actinide series
Solute
Emperical Formula
25. 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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26. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Amphoteric
electromagnetic energy of photons emmited from electrons at ground state
compound
Aqueous Solution
27. (chemistry) p(otential of) H(ydrogen)
Magnetic quantum number
pH
Reaction order
molecular weight
28. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Ion
angular momentum in the bohr model
Atomic weight
Effusion
29. 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
Concentration
Chemical Kinetics
und's rule
Formal Charge
30. Simplest whole # ration of atoms in a compound
Halogens
percent composition
Emperical Formula
Vapor pressure
31. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Group 4A
Principle quantum number
Ion dipole interactions
solvation
32. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Amphoteric
Lewis definition
Disproportionation
Alkaline earths
33. Rare earth element group (elements 58-71)
lathanide series
Neutralization reaction
Lyman series
Reaction order
34. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Theoretical yield
Charles and Gay Lussac's Law
Combination Reaction
Reaction mechanism
35. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Principle quantum number
Octet Rule
angular momentum in the bohr model
Strong acid
36. The lowest allowable energy state of an atom
hydrogen bonding
Ground state
quanta
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
Ionic Bond
Effective nuclear charge
Theoretical yield
Planck's Constant
38. 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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39. 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
Concentration
Spin quantum number
pi bonds
40. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Dipole
Ion
Resonance structure
Neutralization reaction
41. Slightly less reactive than alkali metals - comprise group II
Net ionic equation
VSEPR
subshell
Alkaline earths
42. Named after their cation and anion
und's rule
Ionic Bond
Aqueous Solution
ionic cmpound
43. 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
Nucleus
Molar solubility
ionic cmpound
energy state
44. 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
indicator
Group 7A
Chemical Kinetics
electron affinity
45. 5 different orbitals shaped like clover leaves and max electrons is 10
Decomposition reaction
transition elements
Rydberg constant
d orbital
46. An elementary particle with 0 charge and mass about equal to a proton
indicator
Arrhenius Definition
Neutron
Avagadros number
47. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
Molar solubility
Effective nuclear charge
Ion product
electron affinity
48. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
indicator
Neutralization reaction
Group 4A
pi bonds
49. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
pi bonds
polymer
Neutralization reaction
Octet Rule
50. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
electromagnetic energy of photons emmited from electrons at ground state
Percent composition
Equlibrium constant