CHM 130 Exam 2 Questions With Correct Detailed Answers

Ionic Bonds - A bond between a metal and a nonmetal. Electronegativity difference between the atoms is greater than 1.7 Covalent Bonds - A bond between a nonmetal and a nonmetal. Electronegativity difference between atoms is less than .4 Polar Covalent - A covalent bond with polar bonds between atoms. Electronegativity difference between atoms is more than .4 but less than 1.7. Double Replacement - 2 compounds form 2 different compounds. Precipitation Reaction - A Double Replacement reaction that generally forms a solid and requires solubility rules Acid/Base Reaction - A Double Replacement reaction in which solutions form water and a salt (any ionic compound) Acid/Base Reaction - HCl+ NaOH----- H20 +NaCl is an example of what Double Replacement Reaction? Gas Evolution - What is the third type of Double Replacement Reaction? H2CO3 , H2SO3,NH4OH - What common reactants form a water and a gas? Nonelectrolyte, Covalent - _________________ solutions; don't conduct and are the result of _______ compounds in solution, therefore no ions present. Metallic Bonds - Bonds between a metal and a metal. Valence electrons in metals do not occupy all available orbitals. least - The _______ electronegative atom goes in the center. H+ F never go in the center. negative - - In regards to formal charges be sure the ________ formal charge is on the more electronegative atom. 4 - (Be) only wants how many electrons to complete its "octet"? 6 - (B) only wants how many electrons to complete its "octet"? Si - Atoms above ____ may have more than 8 electrons because they now are available to use the d orbital...and eventually f. radical - When compounds/molecules have an odd number of electrons it is called a ______. Follow usual Lewis Dot Structure rules except one atom will not get 8 electrons. double bond - Due to intermolecular forces a single bond is longer and weaker than a ________ . Endothermic - When energy is required to break a bond it is known as _________. Exothermic - When energy is released to form bonds it is known as ___________ . This energy is always negative. GC - Separates compounds based on their interaction with column (chromatography) MS - Identifies compounds based on the mass to charge ration of fragments. GCMS - In lab we will use this device to find relative abundances and isotopes. Combination,Decomposition,Single Replacement,Combustion - What are the 4 types of Redox Reactions? Combustion - Name this example of a Redox Reaction X+ O2----- CO2 + H20 Diatomic - 2 atom molecules Ex; N,O,F,Cl,Br,H Oxidation Number - The number of electrons an atom gains or loses to form a bond with another element. In comparison to the atoms