Question

follow the steps provided by your teacher to complete each bond. ionic bonds - draw the lewis structures for each atom, then show the transfer of electrons and charge for each ion. write the chemical formula for each compound. (1) mg + br (2) pb + s (3) al + cl covalent bonds - draw the lewis structures for each atom, then draw circles to show the electrons that are shared. write the chemical formula for each compound. (1) h + cl (2) c + cl (3) si + o

Explanation:

Ionic Bonds (1) Mg + Br

Step1: Determine valence electrons

Mg has 2 valence electrons, Br has 7 valence electrons.

Step2: Electron transfer

Mg loses 2 electrons to form $Mg^{2+}$, each Br gains 1 electron to form $Br^-$. So 1 Mg needs 2 Br to accept electrons.

Step3: Chemical formula

The formula is $MgBr_2$.

Step1: Valence electrons

Pb (assuming Pb²⁺ here, common oxidation state) has 2 valence electrons to lose, S has 6 valence electrons to gain 2.

Step2: Electron transfer

Pb loses 2 electrons to S, Pb becomes $Pb^{2+}$, S becomes $S^{2-}$.

Step3: Chemical formula

Formula is $PbS$.

Step1: Valence electrons

Al has 3 valence electrons, Cl has 7 valence electrons.

Step2: Electron transfer

Al loses 3 electrons (forms $Al^{3+}$), each Cl gains 1 electron (forms $Cl^-$). So 1 Al needs 3 Cl.

Step3: Chemical formula

Formula is $AlCl_3$.

Answer:

Chemical formula is $MgBr_2$ (Lewis structures: Mg with 2 dots, Br with 7 dots; Mg loses 2 e⁻ to 2 Br atoms, Mg becomes $Mg^{2+}$, each Br becomes $Br^-$)

Ionic Bonds (2) Pb + S