Air bags, which act as safety devices in cars, contain solid sodium azide. on impact, the sodium azide releases
nitrogen gas, which expands the air bag. the main benefit of using a gas instead of another type is that —
a. gas molecules are subject to ionic bonding
b. the separation of gas molecules is much greater than the volume they occupy
c. gases won’t explode the bag on very hot days
d. gas molecules don’t transfer excess kinetic energy

Achemistry student weighs out of phosphoric acid , a triprotic acid, into a volumetric flask and dilutes to the mark with distilled water. he plans to titrate the acid with solution. calculate the volume of solution the student will need to add to reach the final equivalence point. round your answer to significant digits.

The atomic radius of sodium is 186 pm and of chlorine is 100 pm. the ionic radius for na+ is 102 pm and for cl– is 181 pm. in going from na to cl in period 3, why does the atomic radius decrease while the ionic radius increases? a. the inner electrons in the sodium cation shield its valence electrons more effectively than the inner electrons in the chloride anion do. b. the inner electrons shield the valence electrons more effectively in the chlorine atom than in the chloride anion. c. the outermost electrons in chloride experience a smaller effective nuclear charge than those in the sodium cation do. d. the outermost electrons in chloride experience a larger effective nuclear charge than those in the sodium cation do. e. monatomic ions are bigger than the atoms from which they are formed.

Drag each label to the correct location on the chart. classify each reaction as endothermic or exothermic.