covalent bonding basics manipulatives\ndirections: for each set of atoms, use the lewis dot diagram…

covalent bonding basics manipulatives\ndirections: for each set of atoms, use the lewis dot diagram instructions to make a covalent bond between them.\nremember: a covalent bond happens when electrons are shared between atoms.\nafter some trial and error, you figure out the bond(s) that will work between the atoms, draw the arrangement of valence electrons in the space and circle the new valence shell of each atom. re - draw the bond as a lewis structure, being sure to draw any lone pairs. then write the molecular formula for the molecule.\nexample: oxygen and oxygen\ndrawing of cards with circles showing electrons being shared.\nlewis structure: image of oxygen - oxygen lewis structure\nformula and name: dioxygen o₂\ntypes of bonds used (single, double, triple): double\n#1: hydrogen and chlorine\ndrawing of cards with circles showing electrons being shared.\nlewis structure:\nformula and name:\ntypes of bonds used (single, double, triple):\n#2: nitrogen and nitrogen\ndrawing of cards with circles showing electrons being shared.\nlewis structure:\nformula and name:\ntypes of bonds used (single, double, triple):

covalent bonding basics manipulatives\ndirections: for each set of atoms, use the lewis dot diagram instructions to make a covalent bond between them.\nremember: a covalent bond happens when electrons are shared between atoms.\nafter some trial and error, you figure out the bond(s) that will work between the atoms, draw the arrangement of valence electrons in the space and circle the new valence shell of each atom. re - draw the bond as a lewis structure, being sure to draw any lone pairs. then write the molecular formula for the molecule.\nexample: oxygen and oxygen\ndrawing of cards with circles showing electrons being shared.\nlewis structure: image of oxygen - oxygen lewis structure\nformula and name: dioxygen o₂\ntypes of bonds used (single, double, triple): double\n#1: hydrogen and chlorine\ndrawing of cards with circles showing electrons being shared.\nlewis structure:\nformula and name:\ntypes of bonds used (single, double, triple):\n#2: nitrogen and nitrogen\ndrawing of cards with circles showing electrons being shared.\nlewis structure:\nformula and name:\ntypes of bonds used (single, double, triple):

Answer

Explanation:

Step1: Determine valence electrons

Hydrogen has 1 valence - electron and chlorine has 7 valence - electrons.

Step2: Draw Lewis structure

H and Cl share a pair of electrons. H has a full outer shell with 2 electrons (duet rule), and Cl has 8 electrons in its outer shell (octet rule). The Lewis structure is H:Cl with a single bond between them and 3 lone - pairs on Cl.

Step3: Write formula and name

The formula is HCl, and the name is hydrogen chloride.

Step4: Identify bond type

The bond between H and Cl is a single covalent bond.

For nitrogen and nitrogen:

Step1: Determine valence electrons

Nitrogen has 5 valence - electrons. Two nitrogen atoms together have a total of 10 valence - electrons.

Step2: Draw Lewis structure

The two nitrogen atoms share 3 pairs of electrons to form a triple bond. Each nitrogen also has 1 lone - pair of electrons to satisfy the octet rule. The Lewis structure is :N≡N:

Step3: Write formula and name

The formula is N₂, and the name is dinitrogen.

Step4: Identify bond type

The bond between the two nitrogen atoms is a triple covalent bond.

Answer:

For hydrogen and chlorine:

  • Drawing of cards with circles showing electrons being shared: H:Cl (with 3 lone - pairs on Cl)
  • Lewis Structure:: H:Cl (single bond, 3 lone - pairs on Cl)
  • Formula and name: HCl, hydrogen chloride
  • Types of bonds used (single, double, triple): single

For nitrogen and nitrogen:

  • Drawing of cards with circles showing electrons being shared: :N≡N: (1 lone - pair on each N)
  • Lewis Structure:: :N≡N: (triple bond, 1 lone - pair on each N)
  • Formula and name: N₂, dinitrogen
  • Types of bonds used (single, double, triple): triple