Question

name: drawing ionic and covalent bonds worksheet draw the lewis dot structures of the compounds formed by the following atoms and mention whether the bonds formed by them are covalent or ionic. 1. sodium and chlorine 2. hydrogen and oxygen 3. chlorine and chlorine 4. lithium and bromine

Explanation:

Step1: Determine bond type for sodium and chlorine

Sodium is a metal and chlorine is a non - metal. They form an ionic bond. Sodium loses one electron to become $Na^+$ and chlorine gains one electron to become $Cl^-$. The Lewis dot structure for $NaCl$: $Na^+[:\ddot{Cl}:]^-$

Step2: Determine bond type for hydrogen and oxygen

Hydrogen and oxygen are non - metals. They form covalent bonds. In a water molecule ($H_2O$), oxygen has 6 valence electrons and hydrogen has 1 valence electron each. The Lewis dot structure for $H_2O$: $H:\ddot{O}:H$

Step3: Determine bond type for chlorine and chlorine

Two chlorine atoms (non - metals) form a covalent bond. Each chlorine has 7 valence electrons. The Lewis dot structure for $Cl_2$: $:\ddot{Cl}:\ddot{Cl}:$

Step4: Determine bond type for lithium and bromine

Lithium is a metal and bromine is a non - metal. They form an ionic bond. Lithium loses one electron to become $Li^+$ and bromine gains one electron to become $Br^-$. The Lewis dot structure for $LiBr$: $Li^+[:\ddot{Br}:]^-$

Answer:

1. Ionic bond, Lewis dot structure: $Na^+[:\ddot{Cl}:]^-$
2. Covalent bond, Lewis dot structure: $H:\ddot{O}:H$
3. Covalent bond, Lewis dot structure: $:\ddot{Cl}:\ddot{Cl}:$
4. Ionic bond, Lewis dot structure: $Li^+[:\ddot{Br}:]^-$