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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. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Lyman series
Common ion effect
Charles and Gay Lussac's Law
2. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Resonance structure
effective nuclear charge
STP
Alkaline earths
3. Small discrete increments of energy.
quanta
angular momentum in the bohr model
Group 1A
Pauli exclusion principle
4. The percent by mass of each element in a compound
Diprotic Base
percent composition
Colligative properties
VSEPR
5. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Group 1A
d orbital
mole
theoretical yield
6. 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
empirical formula
Dispersion Forces
Electrolyte
7. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Activation energy
Buffer
azimuthal quantum number
Redox Half Reaction
8. Simplest whole # ration of atoms in a compound
Emperical Formula
Effusion
Amphoteric
polymer
9. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Emperical Formula
Solution equilibrium
quantum
periodic trends
10. The process by which one or more substances change to produce one or more different substances
chemical reaction
representative elements
Noble gases
Ion product
11. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Charles and Gay Lussac's Law
Neutralization reaction
Group 5A
Nonpolar covalent bond
12. 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.
Ion product
Molarity
Concentration
Equivalence point
13. 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
Solution equilibrium
Buffer
transition elements
Neutralization reaction
14. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Solute
Lewis definition
Equivalence point
Nonpolar covalent bond
15. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
und's rule
electrolysis
Triple point
Free radical
16. An ionic compound that resists changes in its pH
Acid dissociation constant
atomic radius
Buffer
Raoult's Law
17. 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
Atomic absorption Spectra
London forces
Diprotic Base
Reaction mechanism
18. 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
Normality
empirical formula
Ionic Bond
Rate law
19. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
redox reaction
Bronsted Lowry
compound
Triple point
20. 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.
Equilibrium
Diprotic Base
atomic radius
Formal Charge
21. The energy required to break a chemical bond and form neutral isolated atoms
Bronsted Lowry
amorphous solid
percent composition
bond energy
22. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
single displacement reaction
Atomic weight
Phase diagram
Octet Rule
23. Rare earth element group (elements 58-71)
lathanide series
London forces
indicator
Proton
24. 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.
Reaction order
crystalline solid
Nucleus
Resonance structure
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. 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-
Electrolyte
Formula weight
Period
Water dissociation Constant
27. 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
ionic cmpound
Arrhenius Definition
actinide series
28. 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
Lewis definition
lewis base
Activation energy
Arrhenius Definition
29. 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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30. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Molarity
Alkaline earths
Ion dipole interactions
31. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
effective nuclear charge
Dipole Dipole interaction
Lyman series
s orbital
32. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Balmer series
quantum
Group 2A
Equilibrium
33. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
s orbital
empirical formula
single displacement reaction
Ionization energy
34. Substance in which a solute is dissolved to form a solution
single displacement reaction
decomposition reaction
Solvent
azimuthal quantum number
35. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Theoretical yield
Emperical Formula
Network covalent
36. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Dispersion Forces
Nucleus
Group 5A
37. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
atomic emission spectrum
pi bonds
Principle quantum number
Reaction order
38. 5 valence electrons -3 ions - Nitride N
Group 5A
ionic cmpound
sigma bond
Covalent Bond
39. The average distance between the nuclei of two bonded atoms
pi bonds
single displacement reaction
Arrhenius Definition
bond length
40. PH of a molecule at which it contains no net electric charge - isoelectric point.
Ionic Bond
Le chateliers Principle
pI
lewis base
41. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Lyman series
und's rule
Colligative properties
atomic emission spectrum
42. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
bond energy
Ion product
Octet Rule
electron configuration
43. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
s orbital
single displacement reaction
Group 3A
Vapor pressure
44. A solution in which water is the solvent
Aqueous Solution
physical reaction
Atomic weight
Solution equilibrium
45. 5 different orbitals shaped like clover leaves and max electrons is 10
theoretical yield
Combination Reaction
Chemical Kinetics
d orbital
46. 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
Conjugate acids and Bases
Equivalence point
Amphoteric
47. 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.
Principle quantum number
Dipole Dipole interaction
indicator
Dipole
48. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
percent composition
Effective nuclear charge
pH
polymer
49. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Rate law
Solution equilibrium
Reaction mechanism
Ion product
50. 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
Bronsted Lowry
Group 7A
VSEPR
Azeotrope