SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. 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
Spin quantum number
molecular weight
Common ion effect
2. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Proton
Octet Rule
Water dissociation Constant
Concentration
3. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
empirical formula
Decomposition reaction
Dipole Dipole interaction
quantum numbers
4. 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
Neutralization reaction
Solution equilibrium
Aqueous Solution
Acid dissociation constant
5. 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
Proton
Water dissociation Constant
Henry's Law
Titration
6. 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
hydrogen bonding
Aqueous Solution
Effusion
heisenberg uncertainty principle
7. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Intermolecular forces
Nonpolar covalent bond
Avagadros number
Acid dissociation constant
8. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
transition elements
ionic cmpound
Diffusion
Chemical Kinetics
9. Small discrete increments of energy.
Le chateliers Principle
Diprotic Base
Avagadros number
quanta
10. Chalcogens - - Oxide O
Group 6A
ionic cmpound
gram equivalent weight
bond energy
11. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
12. The lowest allowable energy state of an atom
Net ionic equation
periodic trends
Arrhenius Definition
Ground state
13. Simplest whole # ration of atoms in a compound
Spin quantum number
Redox Half Reaction
Emperical Formula
quantum numbers
14. The percent by mass of each element in a compound
Ion dipole interactions
lathanide series
Raoult's Law
percent composition
15. A solution in which water is the solvent
angular momentum in the bohr model
indicator
Pauli exclusion principle
Aqueous Solution
16. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Reaction mechanism
atomic radius
Net ionic equation
17. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Azeotrope
redox reaction
Redox Half Reaction
18. A substance that - when dissolved in water - results in a solution that can conduct electricity
Equlibrium constant
Electrolyte
law of constant composition
Diprotic Base
19. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Emperical Formula
Triple point
London forces
Activation energy
20. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
single displacement reaction
Molar solubility
Network covalent
quantum
21. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
STP
Rydberg constant
gram equivalent weight
22. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Molality
transition elements
Lewis structure
gram equivalent weight
23. 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
Water dissociation Constant
Net ionic equation
Ionization energy
Ground state
24. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
sigma bond
d orbital
Combination Reaction
atomic emission spectrum
25. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Normality
Bronsted Lowry
Group 1A
Atomic weight
26. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
STP
VSEPR
electron affinity
angular momentum in the bohr model
27. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
electromagnetic energy of photons emmited from electrons at ground state
Atomic weight
pI
28. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Strong acid
Equivalence point
Rate law
29. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Dipole Dipole interaction
Neutralization reaction
pI
Common ion effect
30. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Henry's Law
Atomic absorption Spectra
Solution equilibrium
Molarity
31. Property of the elements that can be predicted from the arrangement of the periodic table
redox reaction
Equilibrium
periodic trends
Henderson Hasselbalch Equation
32. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
decomposition reaction
heisenberg uncertainty principle
Graham's Law
33. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
s orbital
Ion product
Theoretical yield
Rate determining step
34. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Lyman series
decomposition reaction
gram equivalent weight
transition elements
35. (chemistry) p(otential of) H(ydrogen)
pH
Atomic absorption Spectra
percent composition
Pauli exclusion principle
36. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
quanta
Ionic Bond
VSEPR
s orbital
37. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Le chateliers Principle
Reaction mechanism
Decomposition reaction
Titration
38. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
solvation
electron affinity
Group 7A
39. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Aqueous Solution
Dispersion Forces
Intermolecular forces
Lewis structure
40. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Ground state
Ion product
Noble gases
Rydberg constant
41. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
42. Elements in the middle of the periodic table - in groups 3-12.
angular momentum in the bohr model
transition elements
Mass number
Group 1A
43. 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
Percent yield
Solute
Triple point
Resonance structure
44. The average distance between the nuclei of two bonded atoms
Chemical Kinetics
Water dissociation Constant
Rate determining step
bond length
45. 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.
Solubility Product Constant
Azeotrope
periodic trends
Phase diagram
46. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Planck's Constant
Intermolecular forces
quantum
Group 1A
47. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Molarity
empirical formula
quantum
atomic radius
48. Named after their cation and anion
ionic cmpound
atomic emission spectrum
Collision theory of chemical Kinetics
Atomic absorption Spectra
49. An ionic compound that resists changes in its pH
Rydberg constant
Period
Amphoteric
Buffer
50. 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
Lewis structure
Reaction order
Period