Question

we do: element 117 was recently discovered and is named tennessine. assuming that periodic trends are followed, write the noble gas electron configuration and predict the formula when it forms an ionic compound with mg. you do: 1) which of the

Explanation:

Step1: Determine the noble gas before Tennessine

Tennessine (Ts) has an atomic number of 117. The noble gas before it is Radon (Rn) with atomic number 86. So the noble gas electron configuration starts with [Rn].

Step2: Calculate remaining electrons

The number of electrons after Rn is \( 117 - 86 = 31 \). Now, fill the orbitals: \( 7s^25f^{14}6d^{10}7p^5 \). So the noble gas configuration is \([Rn]7s^25f^{14}6d^{10}7p^5\).

Step3: Determine ion charge of Ts

Ts is in group 17 (halogens), so it gains 1 electron to form \( Ts^- \) (charge -1). Mg is in group 2, loses 2 electrons to form \( Mg^{2+} \) (charge +2).

Step4: Find ionic compound formula

Using the criss - cross method: the charges are \( Mg^{2+} \) and \( Ts^- \). So the formula is \( MgTs_2 \) (since 2 (from Mg's charge) goes to Ts and 1 (from Ts's charge) goes to Mg, \( Mg_1Ts_2 \) simplifies to \( MgTs_2 \)).

Answer:

Noble gas electron configuration: \(\boldsymbol{[Rn]7s^25f^{14}6d^{10}7p^5}\); Ionic compound formula: \(\boldsymbol{MgTs_2}\)