For the following atoms in their ground state, determine the number of electrons in each energy shell. If there are no electrons in the particular energy shell, leave that answer box blank.
(Please see attached file
Question:
Sort these species into isoelectronic groups. It doesn't matter which group goes in which box, so long as the correct species are grouped.
He, Li+, O^2-, Rb+, Se^2-, F-, Be^2+, Y^3, Mg^2+
HINT:
Use a periodic table to determine the atomic number of the atom. For example, xenon's atomic number is 54. A neut
How many electrons should appear in the Lewis structure of the following:
H3O+
SCN-
HCO3-
O2-
N2O4
BF3
Determine the formula change on the following
Cl-O
ClO4-
1) What is the oxidation number of nitrogen in N2O4 (dinitrogen tetraoxide?
First, it has no charge; therefore N2 + 4(-2) = 0
N2 = 8, and thus N = +4. Is this right or wrong? Someone told me N = +2?
2) Nickel(II) nitrate is reduced to nickel metal in an oxidation-reduction reaction. Which is true?
a Nickel ion gains
In forming a covalent bond, electrons are
(a) shared by two atoms
(b) given up by an atom
(c) taken up by an atom
(d) none of the above
(e) all of the above
Elements in the first short period are limited by the octect rule whereas those in the higher period can expand their valence shells. Describe what this means, account for this phenomenon and give an example of each.
The problem to solve is to formulate in which way two carbon atoms are described by using atomic orbitals.
First one has to find out the electronic structure of a carbon atom by locating this element in the periodic table.
Second step is then to fill the orbitals with the given number of electrons using Hund's rule.
The third
