Q 2 Draw the Lewis Dot Diagrams for
- Slides: 7
Q 2: Draw the Lewis Dot Diagrams for the following atoms: He, Cl, H, Li, N, P, Xe, C, and K. He Cl H Li N P Xe C K
Q 3: Draw the following covalent compounds. CH 4, N 2, CO 2, H 2 O
Q 4: Which elements are likely to form ions? What are the charges of cations and anions? § Elements that do not have a full outer energy level are more likely to form ions. But if they only need to lose or gain 1 -2 electrons they are MOST likely to become ions. § Elements in groups 1, 2, 16, 17 are likely to form ions (FYI) § The charge is determined by the group. Group Charge 1 +1 (cation) 2 +2 (cation) 16 -2 (anion) 17 -1 (anion)
Q 5: What is an Ionic Compound? How do they form? What do they form? § An Ionic compound is a compound made up of ionic bonds. § They form because there is an electrical attraction between the oppositely charged ions. § Ionic compounds form crystals. They are in a unit cell structure.
Q 6: Describe Noble Gases. § Noble gases are considered stable because there outer energy level is full. In other words they have 8 electrons in their outer level.
Q 7: Why do atoms form bonds? Atoms form bonds due to the need to have the most stable configuration for its electrons. They want a full octet (Or duet in Hydrogen’s case).
Q 8: Describe the electrons in a metal bond. § The electrons in a metallic bond are “donated” to a “pool” of electrons. All of the metal’s protons share these electrons. It is called the “electron sea” model and it accounts for many of Metal’s properties.
