C. CH OCH3

The pattern that emerges for many atoms (and especially C, N, O, F) is sometimes referred to as the "octet rule." Hydrogen follows the same pattern, but there is no "octet" of electrons for hydrogen.  Use electron configurations to explain why hydrogen is following the same pattern.  Use the term "closed shell" in the explanation.

Arrange the following ions in order of increasing ionic radius: potassium ion, calcium ion, sulfide ion, chloride ion. Smallest Largest

Briefly describe how to use the electron dot symbols of main group elements to determine the number of bonds they usually make.

Explain why boron (B) has a higher ionization energy than fluorine (F).

Describe the location of electrons; describe how electron placement determines chemical bonding, stability, and becoming an ion

-Draw cesium, berryllium, bromine, and flourine by using both lewisand rutherford diagrams, and then write the size of each element.

The Lewis structure for a boron atom has electron pair(s) (represented by :) and unpaired electrons (represented by -). Assume that electrons fill in the same order as an orbital diagram. 1; 1 1; 3 0; 3 2; 1 O 3: 0

What is the element has five 4p valence electrons? what ion will itform?

Write electron configurations for the most stable ion formed by each of the elements , Ba, Se, and Cl (when in stable ionic compounds). (Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as 1s2 2s1 or in condensed form as [He]2s1.) a.) Electron configuration for the most stable ion of Ba b.) Electron configuration for the most stable ion of Se c.) Electron configuration for the most stable ion of Cl