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. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Ground state
Rate determining step
Net ionic equation
Equilibrium
2. An ionic compound that resists changes in its pH
indicator
Molar solubility
Mass number
Buffer
3. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Nucleus
representative elements
Formula weight
4. 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
Dispersion Forces
Octet Rule
Ionic Bond
Normality
5. 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
Strong acid
azimuthal quantum number
Colligative properties
6. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Diffusion
Halogens
Lewis acid base reaction
gram equivalent weight
7. 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.
compound
Ionization energy
Ion product
Ion
8. 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
Covalent Bond
Molarity
Dipole
9. Redox reaction - in which the same species is both oxidized and reduced.
Molality
Alkaline earths
Disproportionation
lathanide series
10. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Bronsted Lowry
Molarity
molecule
Solvent
11. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
12. 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
s orbital
Molar solubility
Equivalence point
Decomposition reaction
13. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
STP
Molarity
azimuthal quantum number
pi bonds
14. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Pauli exclusion principle
Titration
Equlibrium constant
Activation energy
15. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Henderson Hasselbalch Equation
electron configuration
Collision theory of chemical Kinetics
Neutralization reaction
16. Temperature is constant; effusion and temperature are proportional to the square root of their masses
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
17. 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
s orbital
Proton
Resonance structure
Phase diagram
18. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Group 2A
solvation
electron affinity
Ion dipole interactions
19. The maximum amount of product that can be produced from a given amount of reactant
Henry's Law
Lyman series
theoretical yield
Proton
20. PH of a molecule at which it contains no net electric charge - isoelectric point.
pI
Rate determining step
Neutron
Effective nuclear charge
21. 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
London forces
Spin quantum number
Effusion
Formal Charge
22. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Ion
Decomposition reaction
Collision theory of chemical Kinetics
Reaction mechanism
23. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Ion
Group 6A
Avagadros number
quantum numbers
24. A substance that - when dissolved in water - results in a solution that can conduct electricity
Formal Charge
Water dissociation Constant
Electrolyte
ionic cmpound
25. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Magnetic quantum number
pI
molecular weight
Spin quantum number
26. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Bronsted Lowry
Phase diagram
Network covalent
27. 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
Activation energy
lathanide series
Solution equilibrium
Pauli exclusion principle
28. 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
Ground state
Half equivalence point
Solvent
Halogens
29. The percent by mass of each element in a compound
Molecular orbital
Electronegativity
percent composition
Decomposition reaction
30. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Halogens
indicator
effective nuclear charge
molecule
31. 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
Formal Charge
Covalent Bond
energy state
London forces
32. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Neutron
Le chateliers Principle
Neutralization reaction
Formal Charge
33. 5 valence electrons -3 ions - Nitride N
single displacement reaction
Group 5A
Arrhenius Definition
Effective nuclear charge
34. Any sample of a given compound will contain the same elements in the identical mass ratio.
STP
law of constant composition
atomic radius
Rydberg constant
35. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Amphoteric
Spin quantum number
quantum
Vapor pressure
36. The average distance between the nuclei of two bonded atoms
bond length
Lewis acid base reaction
bond energy
electron affinity
37. A reaction in which atoms of one element take the place of atoms of another element in a compound
Solution equilibrium
Formal Charge
Decomposition reaction
single displacement reaction
38. Property of the elements that can be predicted from the arrangement of the periodic table
Balmer series
indicator
periodic trends
Azeotrope
39. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Reaction order
law of constant composition
STP
Lewis acid base reaction
40. 2.18 x 10^-18 J/electron
Theoretical yield
Rydberg constant
atomic radius
Raoult's Law
41. Rare earth element group (elements 58-71)
lathanide series
Theoretical yield
Common ion effect
pI
42. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Period
Strong acid
decomposition reaction
pi bonds
43. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Aqueous Solution
d orbital
electron configuration
Diffusion
44. 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.
transition elements
Henderson Hasselbalch Equation
crystalline solid
decomposition reaction
45. 5 different orbitals shaped like clover leaves and max electrons is 10
transition elements
Resonance structure
d orbital
Percent yield
46. 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
indicator
Neutron
hydrogen bonding
Bronsted - Lowry definition
47. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Half equivalence point
Dipole
Alkaline earths
48. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Solute
percent composition
Chemical Kinetics
Lewis structure
49. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
50. A horizontal row of elements in the periodic table
Ground state
molecular weight
heisenberg uncertainty principle
Period