Electrons Goal Use rings and diagrams to model the formation of ionic compounds and covalent compounds. What to Do Use a blank piece of paper and rings to model electron transfers and electron sharing, as directed in Investigation 1- A: Electrons. Record the electron transfers and sharing and answer the questions in the spaces below. Part 1: Modelling Ionic Bonds 3. Model the formation of lithium hydride using rings. Then, in the space below, copy the diagrams showing the electron transfer from your SCIENCEFOCUS 10 textbook. 4. Model the formation of sodium fluoride using rings. Then record the electron transfer and the ions formed using electron dot diagrams.
5. Model the formation of calcium oxide using rings. Then record the electron transfer and the ions formed using electron dot diagrams. 6. Model the formation of magnesium chloride using rings. Then copy the diagrams showing the electron transfer from your textbook. 7. Model the formation of aluminium oxide using rings. Then record the electron transfer and the ions formed using electron dot diagrams.
Part 2: Modelling Covalent Bonds 1. Model the formation of molecular hydrogen using rings. Then copy the diagram showing the electron sharing from your textbook. 2. Model the formation of water using rings. Then copy the diagram showing the electron sharing from your textbook. 3. Model the formation of methane using rings. Then draw electron dot diagrams and a structural formula to show the electron sharing in a molecule of methane.
4. Model the formation of molecular oxygen using rings. Then draw electron dot diagrams and a structural formula to show the electron sharing in a molecule of oxygen. 5. Model the formation of molecular nitrogen using rings. Then draw electron dot diagrams and a structural formula to show the electron sharing in a molecule of nitrogen. 6. Model the formation of carbon disulfide using rings. Then draw electron dot diagrams and a structural formula to show the electron sharing in a molecule of carbon disulfide.
Analyze 1. Compare the valence energy level of hydrogen atoms in the compounds you have modelled with the valence energy level of other atoms in the compounds. In what way are the valence energy levels similar? How do they differ? 2. How is the bonding in calcium oxide different from the bonding in carbon dioxide? 3. Would you expect covalent bonding or ionic bonding in each of the substances listed below? Give a reason for each answer. (a) magnesium fluoride, MgF 2, which is formed when magnesium and fluorine react (b) carbon tetrachloride, CCl 4, which is formed when carbon and chlorine react Conclude and Apply 4. Describe what happens when (a) a metal atom and a non-metal atom form an ionic bond (b) two non-metal atoms form a molecule with a single covalent bond
5. According to what you have learned so far, state the largest number of electrons that any one atom could (a) donate in an ionic bond (b) accept in an ionic bond (c) share in covalent bonds 6. On some periodic tables, hydrogen in shown on both the left side, with the metals, and on the right side, with the non-metals. (a) What does this placement suggest about the behaviour of hydrogen? (b) Draw an electron dot diagram showing how a hydrogen atom would form a cation. (c) Draw an electron dot diagram showing how a hydrogen atom would form an anion.