Worksheet #4: Equilibrium Problem Set
1. For each of the following reactions, describe what effect and increase in pressure would
have on the equilibrium position of the reaction (i. e. shift right, shift left, no change)
a) 2H $(8) <===> 2H2(g) + S2 (8)
b) 2N, Os(s) <===> 4NO2 (g) + O2 (8)
c) 4NO(8) +202 (8) <===> 2N2O4(s)
d) 2NO(g) + Bra (8) <===> 2NOBr(s)
e) CO(g) + 2H2 (8) <===>CH, OH(s)
f) SO, (g) + NO, (g) <===>SO(g) + NO(g)

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.

Many ionic compounds and a few highly polar covalent compounds are because they completely ionize in water to create a solution filled with charged ions that can conduct an electric current.

Element before carbon on the periodic table