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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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.
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. In a solution - the substance that dissolves in the solvent
empirical formula
Arrhenius Definition
Electronegativity
Solute
2. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Nonpolar covalent bond
Neutron
atomic radius
3. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Lewis definition
Decomposition reaction
Spin quantum number
Formal Charge
4. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Group 6A
decomposition reaction
Ion dipole interactions
5. The energy required to break a chemical bond and form neutral isolated atoms
Halogens
Neutron
Ionization energy
bond energy
6. Small discrete increments of energy.
Proton
atomic emission spectrum
pH
quanta
7. 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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8. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Phase diagram
electrolysis
Free radical
Noble gases
9. 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
Octet Rule
Ion
Azeotrope
decomposition reaction
10. The maximum amount of product that can be produced from a given amount of reactant
Lewis structure
Rate determining step
theoretical yield
Principle quantum number
11. 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
Balmer series
Percent yield
transition elements
Azeotrope
12. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
redox reaction
Covalent Bond
Principle quantum number
Acid dissociation constant
13. Sum of the protons and neutrons in an element often denoted by the letter A
Ion product
Solute
Mass number
Titration
14. A definite stable energy that a physical system can have
Ionization energy
Group 1A
Common ion effect
energy state
15. 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.
theoretical yield
Equivalence point
Solution equilibrium
Molecular orbital
16. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Free radical
quanta
Lewis definition
Percent composition
17. A solution in which water is the solvent
electron configuration
Emperical Formula
Aqueous Solution
Mass number
18. The Percent by mass of each element in a compound.
lathanide series
electron affinity
Percent composition
Molarity
19. 2.18 x 10^-18 J/electron
Amphoteric
Avagadros number
Rydberg constant
atomic theory
20. 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
electromagnetic energy of photons emmited from electrons at ground state
Electronegativity
Proton
atomic theory
21. A horizontal row of elements in the periodic table
Rate law
Triple point
atomic radius
Period
22. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
pi bonds
Magnetic quantum number
mole
London forces
23. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Percent yield
quantum
Reaction mechanism
electron configuration
24. Two or more atoms held together by covalent bonds
Rydberg constant
molecule
Spin quantum number
azimuthal quantum number
25. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
mole
Charles and Gay Lussac's Law
electrolysis
26. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
redox reaction
solvation
Octet Rule
27. 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.
VSEPR
quantum numbers
Bronsted - Lowry definition
Normality
28. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Equlibrium constant
Equivalence point
Chemical Kinetics
Effusion
29. A subdivision of an energy level in an atom. They are divided into orbitals.
Group 6A
Formal Charge
Planck's Constant
subshell
30. 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.
Azeotrope
Balmer series
Solution equilibrium
electron configuration
31. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
quantum numbers
s orbital
theoretical yield
32. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Diprotic Base
Conjugate acids and Bases
Group 6A
Solubility Product Constant
33. 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
Arrhenius Definition
Rate law
theoretical yield
electrolysis
34. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
mole
Arrhenius Definition
Neutralization reaction
35. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Acid dissociation constant
redox reaction
Spin quantum number
Atomic weight
36. 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.
Alkaline earths
Equilibrium
Redox Half Reaction
Diprotic Base
37. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
electron affinity
solvation
Dipole
Lewis structure
38. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Resonance structure
Reaction mechanism
Bronsted Lowry
Equlibrium constant
39. 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
Group 4A
Principle quantum number
Percent composition
Ionic Bond
40. 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
Ionization energy
Molar solubility
und's rule
Disproportionation
41. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Octet Rule
electron configuration
quantum
Neutralization reaction
42. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Hydrogen bonding
Rate law
Group 1A
electron configuration
43. 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
Henderson Hasselbalch Equation
Conjugate acids and Bases
Group 7A
44. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
atomic theory
Balmer series
Collision theory of chemical Kinetics
Normality
45. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Network covalent
Pauli exclusion principle
d orbital
Magnetic quantum number
46. An ionic compound that resists changes in its pH
atomic theory
Solvent
angular momentum in the bohr model
Buffer
47. 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
atomic emission spectrum
Noble gases
Neutron
48. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Dipole Dipole interaction
Hydrogen bonding
Amphoteric
Formula weight
49. 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
Network covalent
Resonance structure
bond length
Dispersion Forces
50. 5 valence electrons -3 ions - Nitride N
pi bonds
Common ion effect
Avagadros number
Group 5A
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