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MCAT Chemistry
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Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Graham's Law
indicator
Mass number
Electrolyte
2. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Magnetic quantum number
Solution equilibrium
atomic emission spectrum
theoretical yield
3. A substance that - when dissolved in water - results in a solution that can conduct electricity
Network covalent
Reaction mechanism
Electrolyte
mole
4. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Group 2A
Equilibrium
Pauli exclusion principle
physical reaction
5. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
redox reaction
Common ion effect
Lewis acid base reaction
Combination Reaction
6. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Electrolyte
Ion
Atomic weight
Reaction mechanism
7. 2.18 x 10^-18 J/electron
Phase diagram
Aqueous Solution
Intermolecular forces
Rydberg constant
8. 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
Emperical Formula
Lewis structure
Ionization energy
Network covalent
9. 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.
atomic theory
Aqueous Solution
Dipole Dipole interaction
Group 3A
10. Sum of the protons and neutrons in an element often denoted by the letter A
The bohr model
Spin quantum number
Mass number
Reaction mechanism
11. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
energy state
chemical reaction
angular momentum in the bohr model
The bohr model
12. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
lathanide series
Solvent
Colligative properties
Molarity
13. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
mole
Acid dissociation constant
Proton
14. Small discrete increments of energy.
Activation energy
Alkaline earths
Equilibrium
quanta
15. A reaction where a compound does Not change its molecular structure.
Percent yield
physical reaction
Water dissociation Constant
Molar solubility
16. 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
Acid dissociation constant
hydrogen bonding
Titration
Neutron
17. 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
pi bonds
Ionic Bond
Intermolecular forces
Avagadros number
18. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
molecular weight
Acid dissociation constant
subshell
Azeotrope
19. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Reaction order
Half equivalence point
Ion
20. Property of the elements that can be predicted from the arrangement of the periodic table
Atomic weight
Le chateliers Principle
Equlibrium constant
periodic trends
21. 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.
Emperical Formula
Solubility Product Constant
Ion product
redox reaction
22. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molar solubility
Molecular orbital
Ion dipole interactions
Lewis structure
23. 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
Formula weight
Percent yield
periodic trends
representative elements
24. Redox reaction - in which the same species is both oxidized and reduced.
Rate determining step
Disproportionation
Electronegativity
Principle quantum number
25. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Strong acid
law of constant composition
lewis base
Amphoteric
26. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Diffusion
Lewis structure
mole
solvation
27. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
empirical formula
Net ionic equation
Molecular orbital
Solvent
28. Simplest whole # ration of atoms in a compound
crystalline solid
Emperical Formula
percent composition
Rydberg constant
29. Common definition of acids as proton (H+) donors and bases as proton acceptors
quantum numbers
Bronsted - Lowry definition
subshell
bond length
30. 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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31. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Resonance structure
Emperical Formula
Activation energy
32. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Intermolecular forces
Octet Rule
Noble gases
heisenberg uncertainty principle
33. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
amorphous solid
polymer
Group 4A
Ion dipole interactions
34. An ionic compound that resists changes in its pH
atomic emission spectrum
Buffer
Network covalent
Percent composition
35. 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
Group 4A
s orbital
Aqueous Solution
percent composition
36. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
atomic theory
Graham's Law
subshell
37. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Lewis acid base reaction
pi bonds
Emperical Formula
Dispersion Forces
38. 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
Colligative properties
atomic radius
Percent composition
Solution equilibrium
39. The process by which one or more substances change to produce one or more different substances
Activation energy
Avagadros number
chemical reaction
quantum numbers
40. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Noble gases
Ionic Bond
law of constant composition
Electronegativity
41. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Intermolecular forces
redox reaction
periodic trends
Decomposition reaction
42. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Rydberg constant
Noble gases
Conjugate acids and Bases
43. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
empirical formula
Reaction order
Pauli exclusion principle
electron configuration
44. 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
Dispersion Forces
Henderson Hasselbalch Equation
Collision theory of chemical Kinetics
45. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
lewis base
quantum
pI
Atomic absorption Spectra
46. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
decomposition reaction
Molar solubility
Balmer series
molecular weight
47. A solution in which water is the solvent
gram equivalent weight
Aqueous Solution
London forces
Bronsted Lowry
48. Numbers that specify the properties of atomic orbitals and of their electrons
Formula weight
law of constant composition
quantum numbers
Group 4A
49. (chemistry) p(otential of) H(ydrogen)
Effusion
Principle quantum number
pH
Bronsted Lowry
50. The Percent by mass of each element in a compound.
Triple point
Covalent Bond
bond length
Percent composition
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