draw lewis dot structures to show how the two given elements form ionic compounds. write the chemical…

Explanation:

Step1: Determine valence electrons

For K (potassium), it has 1 valence - electron; Cl (chlorine) has 7 valence - electrons. K loses 1 electron to form $K^+$ and Cl gains 1 electron to form $Cl^-$. The chemical formula is KCl. The Lewis dot structure: K: $\cdot$ becomes $K^+$; Cl with 7 dots around it becomes $[:\ddot{Cl}:]^-$.

Step2: For Sr and Br

Sr (strontium) has 2 valence - electrons; Br (bromine) has 7 valence - electrons. Sr loses 2 electrons to form $Sr^{2 + }$ and each Br gains 1 electron. Two Br atoms are needed, and the chemical formula is $SrBr_2$. The Lewis dot structure: Sr with 2 dots around it becomes $Sr^{2+}$; each Br with 7 dots around it becomes $[:\ddot{Br}:]^-$.

Step3: For Cs and O

Cs (cesium) has 1 valence - electron; O (oxygen) has 6 valence - electrons. Two Cs atoms are needed to provide 2 electrons for O. Cs forms $Cs^+$ and O forms $O^{2 - }$. The chemical formula is $Cs_2O$. The Lewis dot structure: Cs: $\cdot$ becomes $Cs^+$; O with 6 dots around it becomes $[:\ddot{O}:]^{2 - }$.

Step4: For Ca and N

Ca (calcium) has 2 valence - electrons; N (nitrogen) has 5 valence - electrons. Three Ca atoms are needed to provide 6 electrons for two N atoms. Ca forms $Ca^{2+}$ and N forms $N^{3 - }$. The chemical formula is $Ca_3N_2$. The Lewis dot structure: Ca with 2 dots around it becomes $Ca^{2+}$; N with 5 dots around it becomes $[:\dot{N}:]^{3 - }$.

Step5: For Al and S

Al (aluminum) has 3 valence - electrons; S (sulfur) has 6 valence - electrons. Two Al atoms are needed to provide 6 electrons for three S atoms. Al forms $Al^{3+}$ and S forms $S^{2 - }$. The chemical formula is $Al_2S_3$. The Lewis dot structure: Al with 3 dots around it becomes $Al^{3+}$; S with 6 dots around it becomes $[:\ddot{S}:]^{2 - }$.

Step6: For Ba and I

Ba (barium) has 2 valence - electrons; I (iodine) has 7 valence - electrons. Ba loses 2 electrons to form $Ba^{2+}$ and two I atoms are needed to gain these electrons. Each I forms $I^-$. The chemical formula is $BaI_2$. The Lewis dot structure: Ba with 2 dots around it becomes $Ba^{2+}$; I with 7 dots around it becomes $[:\ddot{I}:]^-$.

Step7: For Li and P

Li (lithium) has 1 valence - electron; P (phosphorus) has 5 valence - electrons. Three Li atoms are needed to provide 3 electrons for P. Li forms $Li^+$ and P forms $P^{3 - }$. The chemical formula is $Li_3P$. The Lewis dot structure: Li: $\cdot$ becomes $Li^+$; P with 5 dots around it becomes $[:\dot{P}:]^{3 - }$.

Step8: For Sc and F

Sc (scandium) has 3 valence - electrons; F (fluorine) has 7 valence - electrons. Sc loses 3 electrons to form $Sc^{3+}$ and three F atoms are needed to gain these electrons. Each F forms $F^-$. The chemical formula is $ScF_3$. The Lewis dot structure: Sc with 3 dots around it becomes $Sc^{3+}$; F with 7 dots around it becomes $[:\ddot{F}:]^-$.

Step9: For Zn and Cl

Zn (zinc) has 2 valence - electrons; Cl (chlorine) has 7 valence - electrons. Zn loses 2 electrons to form $Zn^{2+}$ and two Cl atoms are needed to gain these electrons. Each Cl forms $Cl^-$. The chemical formula is $ZnCl_2$. The Lewis dot structure: Zn with 2 dots around it becomes $Zn^{2+}$; Cl with 7 dots around it becomes $[:\ddot{Cl}:]^-$.

Step10: For Cd and Br

Cd (cadmium) has 2 valence - electrons; Br (bromine) has 7 valence - electrons. Cd loses 2 electrons to form $Cd^{2+}$ and two Br atoms are needed to gain these electrons. Each Br forms $Br^-$. The chemical formula is $CdBr_2$. The Lewis dot structure: Cd with 2 dots around it becomes $Cd^{2+}$; Br with 7 dots around it becomes $[:\ddot{Br}:]^-$.

Answer:

1. Chemical formula: KCl; Lewis dot structure: $K^+$ and $[:\ddot{Cl}:]^-$
2. Chemical formula: $SrBr_2$; Lewis dot structure: $Sr^{2+}$ and two $[:\ddot{Br}:]^-$
3. Chemical formula: $Cs_2O$; Lewis dot structure: two $Cs^+$ and $[:\ddot{O}:]^{2 - }$
4. Chemical formula: $Ca_3N_2$; Lewis dot structure: three $Ca^{2+}$ and two $[:\dot{N}:]^{3 - }$
5. Chemical formula: $Al_2S_3$; Lewis dot structure: two $Al^{3+}$ and three $[:\ddot{S}:]^{2 - }$
6. Chemical formula: $BaI_2$; Lewis dot structure: $Ba^{2+}$ and two $[:\ddot{I}:]^-$
7. Chemical formula: $Li_3P$; Lewis dot structure: three $Li^+$ and $[:\dot{P}:]^{3 - }$
8. Chemical formula: $ScF_3$; Lewis dot structure: $Sc^{3+}$ and three $[:\ddot{F}:]^-$
9. Chemical formula: $ZnCl_2$; Lewis dot structure: $Zn^{2+}$ and two $[:\ddot{Cl}:]^-$
10. Chemical formula: $CdBr_2$; Lewis dot structure: $Cd^{2+}$ and two $[:\ddot{Br}:]^-$