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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. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Neutron
VSEPR
Ion dipole interactions
Avagadros number
2. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Azeotrope
Reaction mechanism
Vapor pressure
Covalent Bond
3. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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4. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Alkaline earths
STP
Equilibrium
Hydrogen bonding
5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
Rate determining step
Solution equilibrium
theoretical yield
6. 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
Magnetic quantum number
crystalline solid
Half equivalence point
representative elements
7. 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
Reaction mechanism
Henderson Hasselbalch Equation
heisenberg uncertainty principle
8. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Resonance structure
Lewis acid base reaction
Electrolyte
Principle quantum number
9. A base that can accept two moles of H+ per mole of itself (ex: SO4
Titration
pI
Diprotic Base
VSEPR
10. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
molecular weight
VSEPR
redox reaction
Ion
11. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Equivalence point
Atomic absorption Spectra
Group 2A
angular momentum in the bohr model
12. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Molarity
atomic radius
Buffer
13. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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14. 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.
solvation
periodic trends
Principle quantum number
Avagadros number
15. 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.
representative elements
VSEPR
Charles and Gay Lussac's Law
Molality
16. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
Emperical Formula
Phase diagram
Dispersion Forces
17. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Lewis definition
atomic radius
Triple point
electromagnetic energy of photons emmited from electrons at ground state
18. The process by which one or more substances change to produce one or more different substances
Molar solubility
Aqueous Solution
chemical reaction
solvation
19. 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
Activation energy
Triple point
Arrhenius Definition
Effusion
20. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Effective nuclear charge
Dipole
Strong acid
Le chateliers Principle
21. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
compound
Phase diagram
actinide series
empirical formula
22. 2.18 x 10^-18 J/electron
Rydberg constant
Chemical Kinetics
Mass number
Normality
23. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
sigma bond
Ground state
Half equivalence point
atomic emission spectrum
24. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Combination Reaction
bond energy
chemical reaction
electron configuration
25. 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
solvation
theoretical yield
atomic theory
Titration
26. 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
Raoult's Law
Water dissociation Constant
Strong acid
Spin quantum number
27. Elements in the middle of the periodic table - in groups 3-12.
Vapor pressure
und's rule
transition elements
crystalline solid
28. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Avagadros number
Electronegativity
Octet Rule
29. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Molar solubility
d orbital
Pauli exclusion principle
Rate law
30. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
indicator
Molality
mole
Ionization energy
31. Named after their cation and anion
ionic cmpound
Principle quantum number
percent composition
Covalent Bond
32. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Effusion
amorphous solid
electromagnetic energy of photons emmited from electrons at ground state
33. 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.
Formal Charge
atomic radius
Henderson Hasselbalch Equation
Solubility Product Constant
34. 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 reaction
single displacement reaction
Solvent
Solution equilibrium
35. The average distance between the nuclei of two bonded atoms
bond length
und's rule
Equilibrium
Hydrogen bonding
36. A solid made up of particles that are not arranged in a regular pattern.
Reaction mechanism
Le chateliers Principle
Decomposition reaction
amorphous solid
37. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
empirical formula
Water dissociation Constant
Atomic absorption Spectra
Effusion
38. An atom or group of atoms that has a positive or negative charge
Group 6A
Buffer
Ion
polymer
39. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Ion dipole interactions
Formula weight
law of constant composition
atomic theory
40. 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.
atomic theory
Balmer series
Amphoteric
Covalent Bond
41. An ionic compound that resists changes in its pH
Buffer
Group 2A
Principle quantum number
Group 6A
42. Slightly less reactive than alkali metals - comprise group II
solvation
Solution equilibrium
Alkaline earths
atomic radius
43. 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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44. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
ionic cmpound
heisenberg uncertainty principle
electrolysis
compound
45. 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
Redox Half Reaction
Percent yield
Molarity
Spin quantum number
46. 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
subshell
molecular weight
Atomic weight
47. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Dipole
Group 5A
Henderson Hasselbalch Equation
48. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Dispersion Forces
redox reaction
Molality
Neutron
49. 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
Hydrogen bonding
Vapor pressure
Proton
d orbital
50. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
molecular weight
sigma bond
Ion product
Rydberg constant