1. Problem: Identify isotopes/ions and their nuclear properties from the given notations. 2. Each isotope/ion is represented as $^{A}_{Z}\text{Element}^{charge}$ where $A$ is the mass number (protons + neutrons), $Z$ is the atomic number (number of protons), and charge indicates ion state. 3. Given isotopes/ions: - $^{55}_{25}\text{Mn}$ (Manganese: 25 protons, 55 nucleons) - $^{40}_{18}\text{Ar}$ (Argon: 18 protons, 40 nucleons) - $^{96}_{42}\text{Mo}$ (Molybdenum: 42 protons, 96 nucleons) - $^{48}_{22}\text{Ti}$ (Titanium: 22 protons, 48 nucleons) - $^{207}_{82}\text{Pb}^{2+}$ (Lead ion: 82 protons, 207 nucleons, charge +2) - $^{80}_{35}\text{Br}^{-}$ (Bromine ion: 35 protons, 80 nucleons, charge -1) - $^{122}_{51}\text{Sb}^{3+}$ (Antimony ion: 51 protons, 122 nucleons, charge +3) - $^{31}_{15}\text{P}^{3-}$ (Phosphorus ion: 15 protons, 31 nucleons, charge -3) 4. For each, neutrons count = mass number $A$ minus atomic number $Z$. 5. Calculations: - Mn neutrons = $55 - 25 = 30$ - Ar neutrons = $40 - 18 = 22$ - Mo neutrons = $96 - 42 = 54$ - Ti neutrons = $48 - 22 = 26$ - Pb neutrons = $207 - 82 = 125$ - Br neutrons = $80 - 35 = 45$ - Sb neutrons = $122 - 51 = 71$ - P neutrons = $31 - 15 = 16$ 6. Charges indicate electron count adjusted: - Pb$^{2+}$ has 2 fewer electrons than protons - Br$^-$ has 1 more electron than protons - Sb$^{3+}$ has 3 fewer electrons than protons - P$^{3-}$ has 3 more electrons than protons Final answers: $^{55}_{25}$Mn: 30 neutrons $^{40}_{18}$Ar: 22 neutrons $^{96}_{42}$Mo: 54 neutrons $^{48}_{22}$Ti: 26 neutrons $^{207}_{82}$Pb$^{2+}$: 125 neutrons, charge +2 $^{80}_{35}$Br$^{-}$: 45 neutrons, charge -1 $^{122}_{51}$Sb$^{3+}$: 71 neutrons, charge +3 $^{31}_{15}$P$^{3-}$: 16 neutrons, charge -3