A 150 g sample of mercury and a 150 g sample of iron are at an initial temperature of 25.0\({ }^{\circ} \mathrm{C}\). If 1050 J of heat is applied to each sample, what is the final temperature of each? (See Table 1.10.)
Text Transcription:
^circ C
periodicity = rises and falls in trends period = row across group = columns (up & down) atomic radii (size of atom) = across a period, size decreases down a group , size increases (more shells) across a period, # of protons in nucleus "pulls" the e- closer to nucleus An anion (neg) is always larger than its neutral counter part An cation (pos) is always larger than its neutral counter part Paramagnetic = where there is at least one unpaired e- Diamagnetic = all e- are paired .. I.e. Group 1(s2 filled), noble gases(p6filled) Metals - tend to make cations (lose electrons) like to oxidize = good reducing agents Non metals - tend to make anions (gains electrons like to reduce = good oxidizing agents Metal oxides (group 1) Basic Nonmetal oxides (co2, h2o, any non metal w oxygen) acidic Amphoteric - can act as an acid or base (semi metals aka metallics , Al2O3, Ge2O3) Strong base = metal will act as acid Strong acid = metal will act as base
