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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. 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.
Resonance structure
VSEPR
Ion
Ionic Bond


2. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Equivalence point
redox reaction
electromagnetic energy of photons emmited from electrons at ground state


3. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Network covalent
Electronegativity
Rate determining step


4. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Ion dipole interactions
quanta
Covalent Bond
Ionization energy


5. Two or more atoms held together by covalent bonds
angular momentum in the bohr model
gram equivalent weight
chemical reaction
molecule


6. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Noble gases
Lyman series
Effusion
Ionization energy


7. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
lewis base
Nucleus
Proton
Molality


8. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
crystalline solid
Solubility Product Constant
Conjugate acids and Bases
Intermolecular forces


9. 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
pI
Bronsted Lowry
solvation


10. In a solution - the substance that dissolves in the solvent
mole
Reaction order
Solute
Vapor pressure


11. Slightly less reactive than alkali metals - comprise group II
Pauli exclusion principle
crystalline solid
Alkaline earths
Henderson Hasselbalch Equation


12. 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-
Molecular orbital
Aqueous Solution
Lewis acid base reaction
Water dissociation Constant


13. 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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14. The process of decomposing a chemical compound by the passage of an electric current.
Resonance structure
electrolysis
periodic trends
Equlibrium constant


15. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
electrolysis
actinide series
Triple point
Colligative properties


16. 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
Disproportionation
indicator
Equlibrium constant
sigma bond


17. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Balmer series
Aqueous Solution
Ion
sigma bond


18. Elements in the middle of the periodic table - in groups 3-12.
atomic radius
solvation
transition elements
Reaction order


19. 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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20. 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.
Network covalent
crystalline solid
Arrhenius Definition
Ion dipole interactions


21. A reaction in which atoms of one element take the place of atoms of another element in a compound
Vapor pressure
Common ion effect
atomic emission spectrum
single displacement reaction


22. 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.
Group 2A
pH
electron affinity
Phase diagram


23. 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
Common ion effect
Decomposition reaction
Equlibrium constant
Proton


24. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Nonpolar covalent bond
Neutralization reaction
Neutron


25. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T

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26. Substance in which a solute is dissolved to form a solution
lathanide series
atomic radius
Group 6A
Solvent


27. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
bond length
gram equivalent weight
redox reaction
Noble gases


28. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
Group 7A
atomic radius
empirical formula
Halogens


29. The average distance between the nuclei of two bonded atoms
bond length
Atomic weight
Water dissociation Constant
Diffusion


30. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total

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31. An elementary particle with 0 charge and mass about equal to a proton
Water dissociation Constant
chemical reaction
VSEPR
Neutron


32. The percent by mass of each element in a compound
Lewis structure
Activation energy
Dipole Dipole interaction
percent composition


33. Numbers that specify the properties of atomic orbitals and of their electrons
bond length
electrolysis
quantum numbers
Dipole


34. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Aqueous Solution
Pauli exclusion principle
solvation
angular momentum in the bohr model


35. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
amorphous solid
molecule
Ion
Strong acid


36. A horizontal row of elements in the periodic table
electromagnetic energy of photons emmited from electrons at ground state
Equivalence point
Period
lathanide series


37. Named after their cation and anion
Mass number
Equilibrium
ionic cmpound
Neutron


38. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
atomic theory
Diffusion
Group 7A


39. 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
Lewis structure
energy state
atomic radius
Titration


40. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
single displacement reaction
The bohr model
Halogens


41. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Lewis definition
Henderson Hasselbalch Equation
Rate law
redox reaction


42. 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
Solubility Product Constant
law of constant composition
Solution equilibrium
molecular weight


43. Gram equivalent weight of solute per liter of solution - often denoted by N.
effective nuclear charge
Normality
hydrogen bonding
pI


44. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
London forces
Le chateliers Principle
Graham's Law
mole


45. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Alkaline earths
Formula weight
periodic trends
molecule


46. 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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47. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
Molecular orbital
Raoult's Law
Bronsted - Lowry definition
Effective nuclear charge


48. 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.
pH
lathanide series
Principle quantum number
Resonance structure


49. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
effective nuclear charge
Reaction order
Activation energy
Intermolecular forces


50. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Ionization energy
Ion
Network covalent
transition elements