I have my exam in a little over 7 hours...can anyone help explain how to draw atoms in the Bohr Rutherford and Lewis Dot methods, as well as how to draw them as compounds and ions? My friends are no help, nor is the internet. Please!

please explain clearly. I just didn't understand the question.

For the first two models, see

http://en.wikipedia.org/wiki/Bohr_model
it contains a link about the Rutherford model.

For the Lewis structure, see
http://en.wikipedia.org/wiki/Lewis_structure

what is the mass in grams of 2.50x10 to the power of 24 molecules for each of the following compounds using the dimensional analysis

Of course! I'd be happy to help you understand how to draw atoms in the Bohr Rutherford and Lewis Dot methods, as well as compounds and ions. Let's start with the Bohr Rutherford model.

The Bohr Rutherford model represents the arrangement of electrons within an atom. Here's how you can draw atoms using this method:

1. Determine the number of protons, neutrons, and electrons in the atom. You can find this information on the periodic table. The number of protons is the atomic number, while the number of neutrons can be calculated by subtracting the atomic number from the atomic mass.

2. Draw a nucleus in the center with protons and neutrons. Label the number of protons and neutrons inside the nucleus.

3. Draw energy levels or electron shells around the nucleus. These energy levels are represented by circles or orbits. The first energy level (closest to the nucleus) can hold up to 2 electrons, the second energy level can hold up to 8 electrons, and so on.

4. Distribute the electrons into the energy levels. Start with the first energy level and fill it with electrons before moving to the next energy level. Electrons should be drawn as dots or crosses.

Keep in mind that the maximum number of electrons in each energy level is determined by the formula 2n², where "n" represents the energy level number. For example, the first energy level can hold a maximum of 2 electrons (2*1² = 2), the second energy level can hold a maximum of 8 electrons (2*2² = 8), and so on.

Now, let's talk about drawing atoms using the Lewis Dot method.

The Lewis Dot method places emphasis on the valence electrons, which are the electrons in the outermost energy level. It is useful for understanding how atoms bond and form compounds.

Here's how you can draw atoms using the Lewis Dot method:

1. Determine the number of valence electrons for the atom. Again, you can find this information on the periodic table.

2. Draw the atomic symbol for the element in the center and then place dots around the symbol, representing the valence electrons.

3. Arrange the dots into pairs, with each pair placed on one side of the atomic symbol. Remember the "octet rule," which states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons (except for hydrogen and helium, which can be stable with only two valence electrons).

Now, let's move on to drawing compounds and ions.

Compound:

To draw a compound using the Bohr Rutherford or Lewis Dot method, follow these steps:

1. Determine the chemical formula for the compound. This will provide you with the types and numbers of atoms involved.

2. Draw the atoms involved using the Bohr Rutherford or Lewis Dot method, as described earlier.

3. Connect the atoms with lines or by sharing dots, indicating the bonds between them. For example, a single bond is represented by a single line or two shared electrons.

Ion:

To draw an ion using the Bohr Rutherford or Lewis Dot method, consider the following:

1. Determine whether the ion is positively or negatively charged. Cations are positive ions, while anions are negative ions.

2. Adjust the number of electrons for the ion. Cations have fewer electrons than the neutral atom, while anions have more electrons.

3. Draw the ion using the Bohr Rutherford or Lewis Dot method, taking into account the adjusted electron count.

I hope this explanation helps you with drawing atoms, compounds, and ions for your exam! Good luck!