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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. Redox reaction - in which the same species is both oxidized and reduced.
Le chateliers Principle
Disproportionation
Ion
Diffusion
2. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Group 3A
polymer
heisenberg uncertainty principle
atomic radius
3. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
quantum numbers
compound
sigma bond
angular momentum in the bohr model
4. 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
quantum
Group 6A
Rate determining step
5. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
actinide series
Molarity
Neutralization reaction
lewis base
6. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Atomic absorption Spectra
redox reaction
Free radical
7. 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
pI
Raoult's Law
hydrogen bonding
Network covalent
8. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Noble gases
Solubility Product Constant
Phase diagram
9. Simplest whole # ration of atoms in a compound
Emperical Formula
Proton
actinide series
quantum
10. A subdivision of an energy level in an atom. They are divided into orbitals.
und's rule
Group 4A
subshell
Intermolecular forces
11. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
representative elements
atomic radius
Strong acid
Effective nuclear charge
12. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Percent yield
Resonance structure
Formula weight
Group 3A
13. The percent by mass of each element in a compound
Molecular orbital
percent composition
Group 5A
Buffer
14. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Lewis acid base reaction
Effective nuclear charge
pI
compound
15. 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
angular momentum in the bohr model
redox reaction
Resonance structure
Colligative properties
16. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
amorphous solid
atomic emission spectrum
solvation
single displacement reaction
17. Two or more atoms held together by covalent bonds
sigma bond
Effusion
molecule
Henry's Law
18. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Nonpolar covalent bond
Chemical Kinetics
Triple point
Balmer series
19. Small discrete increments of energy.
quanta
Theoretical yield
quantum
Percent yield
20. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Buffer
Avagadros number
empirical formula
The bohr model
21. The average distance between the nuclei of two bonded atoms
bond length
Group 2A
representative elements
Ion product
22. 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
Avagadros number
Ion
energy state
23. 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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24. 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.
Equivalence point
Diffusion
atomic radius
Bronsted - Lowry definition
25. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
physical reaction
Molality
Percent composition
Le chateliers Principle
26. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
molecular weight
Collision theory of chemical Kinetics
Octet Rule
Arrhenius Definition
27. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Hydrogen bonding
Le chateliers Principle
Octet Rule
28. A horizontal row of elements in the periodic table
solvation
Period
Normality
atomic theory
29. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Henderson Hasselbalch Equation
indicator
Group 7A
Dipole
30. 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
Rydberg constant
Hydrogen bonding
quanta
electromagnetic energy of photons emmited from electrons at ground state
31. Substance in which a solute is dissolved to form a solution
Percent composition
Group 6A
single displacement reaction
Solvent
32. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
pH
Half equivalence point
Le chateliers Principle
Collision theory of chemical Kinetics
33. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Diprotic Base
Molecular orbital
actinide series
pi bonds
34. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Equilibrium
Molar solubility
Intermolecular forces
35. A solution in which water is the solvent
bond energy
Aqueous Solution
Alkaline earths
molecular weight
36. Elements in the middle of the periodic table - in groups 3-12.
Neutron
Titration
transition elements
Bronsted Lowry
37. Any sample of a given compound will contain the same elements in the identical mass ratio.
effective nuclear charge
single displacement reaction
law of constant composition
pI
38. Slightly less reactive than alkali metals - comprise group II
Group 2A
Alkaline earths
Colligative properties
Aqueous Solution
39. 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
Activation energy
Ionic Bond
Free radical
Colligative properties
40. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
Buffer
Reaction mechanism
VSEPR
41. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
Vapor pressure
Collision theory of chemical Kinetics
bond energy
42. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
heisenberg uncertainty principle
Redox Half Reaction
Strong acid
43. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
law of constant composition
Ion
Diffusion
44. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Common ion effect
Avagadros number
Group 4A
Mass number
45. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Colligative properties
Neutron
Principle quantum number
heisenberg uncertainty principle
46. 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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47. 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.
Formula weight
Bronsted - Lowry definition
Normality
crystalline solid
48. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Common ion effect
ionic cmpound
Network covalent
Equilibrium
49. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Neutron
Principle quantum number
subshell
Free radical
50. The lowest allowable energy state of an atom
Water dissociation Constant
Lewis structure
pH
Ground state