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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. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
bond energy
Reaction mechanism
Rydberg constant
Mass number
2. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
sigma bond
Percent yield
Azeotrope
redox reaction
3. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Group 5A
ionic cmpound
Lyman series
Covalent Bond
4. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Formal Charge
Common ion effect
Molality
solvation
5. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Hydrogen bonding
Arrhenius Definition
Group 2A
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
Formula weight
Network covalent
Half equivalence point
Lyman series
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.
sigma bond
Group 3A
quantum numbers
Effective nuclear charge
8. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
molecule
Group 2A
law of constant composition
Phase diagram
9. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Alkaline earths
pi bonds
Magnetic quantum number
Mass number
10. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Charles and Gay Lussac's Law
electron configuration
pH
lewis base
11. A solution in which water is the solvent
Aqueous Solution
Activation energy
Diprotic Base
indicator
12. 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
solvation
Solution equilibrium
pI
Decomposition reaction
13. Any sample of a given compound will contain the same elements in the identical mass ratio.
quanta
law of constant composition
gram equivalent weight
crystalline solid
14. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
heisenberg uncertainty principle
Effective nuclear charge
Redox Half Reaction
Water dissociation Constant
15. 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
Ground state
mole
Combination Reaction
16. 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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17. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Buffer
Solute
Arrhenius Definition
18. The percent by mass of each element in a compound
Halogens
percent composition
London forces
Principle quantum number
19. Slightly less reactive than alkali metals - comprise group II
Henderson Hasselbalch Equation
electron configuration
Dipole
Alkaline earths
20. 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
Bronsted Lowry
The bohr model
Dispersion Forces
Acid dissociation constant
21. An elementary particle with 0 charge and mass about equal to a proton
Period
Molarity
Neutron
Ion
22. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Formula weight
Solvent
Diffusion
Lewis structure
23. 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
Lewis definition
The bohr model
molecule
Colligative properties
24. 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.
Percent yield
Strong acid
crystalline solid
Dispersion Forces
25. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Combination Reaction
empirical formula
Acid dissociation constant
Principle quantum number
26. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Molality
redox reaction
Diffusion
Group 3A
27. The Percent by mass of each element in a compound.
Planck's Constant
Spin quantum number
Percent composition
Intermolecular forces
28. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
sigma bond
Conjugate acids and Bases
Lewis acid base reaction
effective nuclear charge
29. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Solvent
Lewis acid base reaction
quantum
decomposition reaction
30. In a solution - the substance that dissolves in the solvent
Pauli exclusion principle
Solute
Neutralization reaction
Network covalent
31. 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
Equlibrium constant
Solute
Ion product
Dipole
32. 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
d orbital
The bohr model
Concentration
Rate law
33. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Redox Half Reaction
Electrolyte
Chemical Kinetics
34. 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
Percent yield
Molar solubility
Molarity
empirical formula
35. 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
Equivalence point
decomposition reaction
Halogens
Spin quantum number
36. 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
Graham's Law
Noble gases
atomic radius
37. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
decomposition reaction
Balmer series
s orbital
polymer
38. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
subshell
Effusion
actinide series
d orbital
39. Sum of the protons and neutrons in an element often denoted by the letter A
Disproportionation
Molality
Mass number
Strong acid
40. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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41. 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
indicator
Reaction mechanism
hydrogen bonding
42. 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
effective nuclear charge
Ion dipole interactions
bond length
43. The process by which one or more substances change to produce one or more different substances
Group 1A
chemical reaction
transition elements
hydrogen bonding
44. Redox reaction - in which the same species is both oxidized and reduced.
solvation
Net ionic equation
Emperical Formula
Disproportionation
45. 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.
Solubility Product Constant
Charles and Gay Lussac's Law
Graham's Law
lewis base
46. (chemistry) p(otential of) H(ydrogen)
molecular weight
Network covalent
Molality
pH
47. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Ion dipole interactions
Lyman series
Reaction mechanism
48. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Normality
Activation energy
percent composition
crystalline solid
49. E=hc/?
Nonpolar covalent bond
electromagnetic energy of photons emmited from electrons at ground state
Pauli exclusion principle
Strong acid
50. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Atomic weight
Solvent
Decomposition reaction
Conjugate acids and Bases
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