How do you draw a Lewis dot structure for an ionic compound?

Answer 1

Follow These 5 StepsTo draw a Lewis dot structure for a molecule or ion, follow these steps:

• Step 1: Count up the number of valence electrons for each atom, and total them up to give the total number of electrons for the molecule. If the molecule is an ion, include that charge in the count. For example, for a +1 ion, subtract one electron, and for a -2 ion add two electrons to the total count. (For more information about how to count the number of valence electrons per atom, see the related questions link to the left of this answer).
• Step 2: Determine which atom is the central atom and join all the atoms using only single bonds. Sometimes which atom is the central atom is hard to determine. For instance with a molecule like CH4 it's clear the C is the central atom, but for something more complicated like ClO2F3 it's not as clear (it's the Cl in this case).
• Step 3: Add lone pairs to each atom as necessary so that each atom has an octet (except H which can only have 2 electrons total) when you count all the atom's lone pairs and two electrons for each of its bonds. For example the carbon atom (C) in CH4 has four single bonds to its four hydrogen (H) atoms, each with two electrons, so that makes eight electrons - you wouldn't need to add any lone pairs to this one. Count up the total number of electrons as it is now drawn (2 electrons per bond).
• Step 4: If the total you got in Step 1 is the same as in Step 3, you're done! If it doesn't you'll need to make some changes. If the number of electrons in Step 3 is larger than in Step 1, you must add double bonds as necessary between atoms. Then adjust the number of lone pairs again so that each atom has an octet. Remember no double bonds to H or with any of the halogens! If the total electron count with only single bonds is smaller than in Step 1, you probably made a mistake somewhere. Go back and double check.
• Step 5: Continue adjusting the arrangement of single and double bonds and lone pairs (and also triple bonds if necessary) until the total electron count matches what you got in Step 1.

Some additional tips:

• Do not ever exceed octets on atoms before sodium (Na) in the third row.
• Draw resonance structures that maximize bonding and minimize formal charge (see related questions about resonance forms and also assigning formal charges).
• Place formal charges on appropriate atoms, and in general more electronegative atoms should have the negative charges. (Again, see links for how to assign formal charges).
• For additional help, try reading the books "Chemistry for Everyone" or "Chemistry for Dummies"

Answer 2

Lewis dot structures show how a covalent molecule is put together, and how atoms share electrons to fill their valence shells. Most atoms are stable with eight electrons in their outermost shell, and will bond to fill them.

The first step is to figure out how many electrons an atom already has, so you can figure out how many bonds it needs. The easiest way to do this is to look at a Periodic Table. Only nonmetals participate in covalent bonds, so look on the right side. Simply drop the tens digit from the group number - boron is in group 13, and has 3 valence (outer) electrons. Nitrogen is in group 15, and has 5 valence electrons. Once you have figured out how many valence electrons an atom has, draw it by writing the symbol, then using dot to represent electrons. Put one dot on top, and then start cycling clockwise, placing one dot on each side of the symbol. The fifth dot will be next to the first; this is ok. Electrons pair up in atoms, and atoms want four pairs of electrons total (see the first paragraph).

After all atoms are drawn with all of their electrons, start circling pairs of electrons (one from each atom) to start making bonds. When all atoms have four pairs (8 electrons) around them, redraw the structure, putting bonded atoms next to each other, and replacing shared pairs with lines. One line = one bond = two shared electrons. It is possible to make multiple bonds between two atoms, sharing multiple pairs of electrons, but don't go higher than a triple bond.

Answer 3

You have to look at the number of valence electrons and how many valence electrons are in the outer energy level is how many dots you put on the chemical symbol. For example, Sodium's element symbol is Na, and it has one valence electron so you Lewis dot diagram would be Na.

You can also find the number of valence electrons an easier way by looking at the group number of your element and the group number is the number of valence electrons, but this trick does not apply to groups nine and ten. Also, helium has two dots.

You start at the right side of the element name and go counter-clockwise and add one dot for each valence electron. You can only have eight valence electrons/dots. Once you go around once, you go around again.

Answer 4

H-C=C-Cl is Ethylene Chloride There is a triple bond between the carbons. No symbol for that! The hydrogen has one cross shared with one dot from the first carbon. The two carbons both share 6 electrons (3 dots and 3 crosses from each one) The remaining dot of the carbon is shared with a cross from the chlorine. The other 6 crosses are in pairs around the chlorine. Hope this helps.

Answer 5

I believe it is like this: H:O:H (I tried to put periods above and below the O, but when I saved the changes, it didn't allow my attempted ASCII. There should be two dots above and below the O.) O=H-O

the hydrogen atom would be an octet though. (2 dots above the H) O=H-O

The = indicates a double bond.

There would be 2 dots above the hydrogen atom.

Yeah, but there are 2XH and 1XO in water right? How did you come up with 1XH and 2XO from Water?

Actually you're right about the 2 dots above and the 2 dots below the O.

Anyway, the correct Lewis structure is:

H:O:H with 2 additional dot above and 2 additional dots below the O.

The only element that would need to be Octet is the Oxygen atom. Hydrogen is the one exception to the Octet Rule.

BTW, the only Elements that can be double bonded are: Carbon, Nitrogen, Oxygen, Sulfer and Phosphorus. Nothing else can be joined to of from this bond. Triple bonds are: Carbon and Nitrogen and the same rule applies.

Answer 6

Since it is only one atom and not a molecule, you just count the electrons. In the case of C (Carbon). There are 4 valence electrons (2s2 and 2p2). So it will be :C: There won't be any bonds. Rarely will carbon not have four bonds though.

Answer 7

How do you draw a lewis dot structure for an ionic compound?

Answer 8

This is going be hard to describe, just bare with the model.

.

Na.