covalent bonds and lewis dot models. instructions. use plates, pennies, and paper clips to build models of…

covalent bonds and lewis dot models. instructions. use plates, pennies, and paper clips to build models of chemical compounds. you will need one plate for each atom in the compound. the pennies will represent valence electrons. to represent a covalent bond between atoms you will place a paper clip between each bonded pair of pennies. create a document and title it covalent bonds and lewis dot diagrams. for each of the compounds you should do the following four steps: 1. take a picture of each atom with the correct number of valence electrons (pennies) before the bonds are formed. 2. draw the lewis dot diagram for each atom before the bonds are formed. 3. take a picture of the completed molecule with the correct number of atoms (plates), valence electrons (pennies), and covalent bonds (paper clips). 4. draw the lewis dot diagram for each atom after the bonds are formed. list of compounds: h₂, h₂o, f₂, nh₃, n₂, o₂, co₂, ch₄, c₂h₂, c₂h₆

covalent bonds and lewis dot models. instructions. use plates, pennies, and paper clips to build models of chemical compounds. you will need one plate for each atom in the compound. the pennies will represent valence electrons. to represent a covalent bond between atoms you will place a paper clip between each bonded pair of pennies. create a document and title it covalent bonds and lewis dot diagrams. for each of the compounds you should do the following four steps: 1. take a picture of each atom with the correct number of valence electrons (pennies) before the bonds are formed. 2. draw the lewis dot diagram for each atom before the bonds are formed. 3. take a picture of the completed molecule with the correct number of atoms (plates), valence electrons (pennies), and covalent bonds (paper clips). 4. draw the lewis dot diagram for each atom after the bonds are formed. list of compounds: h₂, h₂o, f₂, nh₃, n₂, o₂, co₂, ch₄, c₂h₂, c₂h₆

Answer

Explanation:

Step1: Determine valence electrons for each element

For hydrogen (H), it has 1 valence - electron. For oxygen (O), it has 6 valence - electrons. For carbon (C), it has 4 valence - electrons. For nitrogen (N), it has 5 valence - electrons. For fluorine (F), it has 7 valence - electrons.

Step2: For (H_2O)

O is the central atom. O has 6 valence electrons. It shares 1 electron with each of the 2 H atoms. The Lewis - dot structure has O in the center with 2 single bonds to H and 2 lone pairs on O.

Step3: For (CH_4)

C is the central atom. C has 4 valence electrons. It shares 1 electron with each of the 4 H atoms. The Lewis - dot structure has C in the center with 4 single bonds to H and no lone pairs on C.

Step4: For (C_2H_6)

Each C atom has 4 valence electrons. The two C atoms are bonded to each other by a single bond, and each C atom is also bonded to 3 H atoms. Each C has 4 single bonds and no lone pairs.

Step5: For (CO_2)

C is the central atom. C has 4 valence electrons. It forms double bonds with each O atom. Each O has 6 valence electrons, and in (CO_2), C is in the center with 2 double bonds to O and no lone pairs on C, and each O has 2 lone pairs.

Step6: For (NO_2)

N is the central atom. N has 5 valence electrons. In (NO_2), N is bonded to one O by a single bond and to another O by a double bond. There is a lone electron on N. One O has 3 lone pairs and the other has 2 lone pairs.

Step7: For (NH_3)

N is the central atom. N has 5 valence electrons. It shares 1 electron with each of the 3 H atoms. There is 1 lone pair on N. The Lewis - dot structure has N in the center with 3 single bonds to H and 1 lone pair on N.

Step8: For (F_2)

Each F atom has 7 valence electrons. They share 1 pair of electrons to form a single bond. Each F has 3 lone pairs.

Answer:

Lewis - dot structures for (H_2O): O in the center with 2 single bonds to H and 2 lone pairs on O; for (CH_4): C in the center with 4 single bonds to H; for (C_2H_6): two C atoms bonded to each other and each C bonded to 3 H atoms; for (CO_2): C in the center with 2 double bonds to O; for (NO_2): N in the center with a single and a double bond to O and a lone electron on N; for (NH_3): N in the center with 3 single bonds to H and 1 lone pair on N; for (F_2): two F atoms bonded by a single bond with 3 lone pairs on each F.