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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
bond length
Diprotic Base
Rydberg constant
quanta
2. Named after their cation and anion
Intermolecular forces
ionic cmpound
Vapor pressure
quantum numbers
3. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
law of constant composition
Nonpolar covalent bond
Net ionic equation
und's rule
4. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Arrhenius Definition
Network covalent
Solution equilibrium
Solute
5. 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
pH
Neutron
Nucleus
Vapor pressure
6. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Equlibrium constant
Pauli exclusion principle
quantum
chemical reaction
7. Slightly less reactive than alkali metals - comprise group II
Triple point
Alkaline earths
Arrhenius Definition
Planck's Constant
8. A reaction where a compound does Not change its molecular structure.
Azeotrope
polymer
pI
physical reaction
9. A horizontal row of elements in the periodic table
theoretical yield
Ion product
Collision theory of chemical Kinetics
Period
10. 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.
crystalline solid
heisenberg uncertainty principle
periodic trends
Raoult's Law
11. An elementary particle with 0 charge and mass about equal to a proton
Collision theory of chemical Kinetics
Molecular orbital
Group 1A
Neutron
12. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
s orbital
single displacement reaction
Atomic absorption Spectra
13. Small discrete increments of energy.
Solvent
quanta
Lyman series
Henderson Hasselbalch Equation
14. 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
hydrogen bonding
periodic trends
Ionic Bond
Neutralization reaction
15. A definite stable energy that a physical system can have
energy state
pH
pI
Aqueous Solution
16. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Diffusion
Formal Charge
Rate law
17. 5 valence electrons -3 ions - Nitride N
pH
Pauli exclusion principle
Group 5A
Free radical
18. The process by which one or more substances change to produce one or more different substances
chemical reaction
Water dissociation Constant
Network covalent
Ion product
19. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Activation energy
molecular weight
Equilibrium
Hydrogen bonding
20. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Ion
indicator
Intermolecular forces
Network covalent
21. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Neutron
Reaction mechanism
London forces
Effusion
22. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Magnetic quantum number
Half equivalence point
molecular weight
23. The Percent by mass of each element in a compound.
angular momentum in the bohr model
Dipole Dipole interaction
Reaction order
Percent composition
24. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
STP
redox reaction
Balmer series
Lewis structure
25. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Collision theory of chemical Kinetics
Molecular orbital
Rate determining step
Dipole
26. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Ion
Intermolecular forces
Group 4A
Percent composition
27. 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.
representative elements
pH
Solubility Product Constant
Henderson Hasselbalch Equation
28. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
angular momentum in the bohr model
Molarity
Lewis structure
Formal Charge
29. 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
Redox Half Reaction
representative elements
Solution equilibrium
electromagnetic energy of photons emmited from electrons at ground state
30. Property of the elements that can be predicted from the arrangement of the periodic table
Magnetic quantum number
Dipole
representative elements
periodic trends
31. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Pauli exclusion principle
Common ion effect
polymer
Proton
32. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Magnetic quantum number
Arrhenius Definition
Solute
Chemical Kinetics
33. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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34. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Group 6A
Collision theory of chemical Kinetics
Rate determining step
35. 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.
atomic radius
pH
Le chateliers Principle
percent composition
36. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Solute
redox reaction
effective nuclear charge
Lyman series
37. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Rate law
Bronsted - Lowry definition
compound
38. Substance in which a solute is dissolved to form a solution
Solvent
atomic radius
Ionization energy
Diffusion
39. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Graham's Law
effective nuclear charge
Group 7A
40. Common definition of acids as proton (H+) donors and bases as proton acceptors
Molarity
Bronsted - Lowry definition
Acid dissociation constant
Resonance structure
41. 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
single displacement reaction
Conjugate acids and Bases
Half equivalence point
Ion dipole interactions
42. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Amphoteric
polymer
bond energy
Neutralization reaction
43. The lowest allowable energy state of an atom
lewis base
d orbital
Ground state
effective nuclear charge
44. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Molecular orbital
Atomic weight
Covalent Bond
45. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
Halogens
Nonpolar covalent bond
pI
46. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
lathanide series
Concentration
electromagnetic energy of photons emmited from electrons at ground state
47. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
indicator
Halogens
bond energy
48. An ionic compound that resists changes in its pH
Ion dipole interactions
Solubility Product Constant
lewis base
Buffer
49. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
atomic emission spectrum
Solvent
Activation energy
Raoult's Law
50. 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
sigma bond
Ionization energy
chemical reaction
Lewis structure