Chemistry Ch. 7 and 8 Key Concepts and Outline Name
I Can Statements….
1. I can determine the number of valence electrons a representative element has by its position on the periodic table, whether it will gain or lose electrons in a bond, what its expected charge is, and whether it will be a cation or an anion.
2. I can draw electron dot structures for any single atom of a representative element, and a dot structure of a simple compound using bond lines or shared electron dots.
3. I can answer a multiple choice question based on the definition of any of the bold terms in this outline or in Ch. 7 and 8.
4. I can identify the properties of an ionic compound, a metallic compound, a covalent compound and a polar compound.
5. I can determine what kind of bond (mentioned above) two atoms would form (when they react) using their position on the periodic table, and/or the electronegativities chart on page 177.
6. Based on a data table containing the properties of a compound (melting point, boiling point, phase etc…) I can determine what kind of bond it contains.
7. I can determine the molecular shape of a compound by drawing its electron dot structure and using the VSEPR theory.
8. I can identify isomers of the same molecular formula.
9. I can use bond dissociation energies to determine the relative stabilities of a compound.
10. I can name the various intermolecular attractions and apply their forces to common biological principles like the structure of DNA and surface tension of water.
Section 7.1
What is a valence electron?
KC 3 How can you determine the number of valence electrons in an atom of a representative element?
What are (Lewis) Electron Dot Structures?
Give an example of an electron dot structure for an element from each of the representative groups.
KC 4 Atoms of which elements tend to gain electrons? Atoms of which elements tend to lose electrons?
KC 5 How do cations form?
Write an equation for a sodium atom losing an electron.
What is a pseudo noble gas configuration?
KC 6 How do anions form?
Write an equation for a chlorine atom losing an electron.
What is a halide ion?
Section 7.2
What is an ionic compound?
KC 14 How can you describe the electrical charge of an ionic compound?
What is an ionic bond?
Write an equation that describes the exchange of a valence electron between Sodium and Chlorine.
What is a chemical formula?
What is a formula unit?
What happens to the charges of the individual ions when a bond is formed?
What is the chemical formula for the compound formed from Magnesium and Chlorine? Aluminum and Bromine?
KC 15 What properties characterize ionic compounds?
Why are ionic compounds stable?
What is the coordination number?
What is the coordination number for Cesium with Chlorine?
Why do you think Cesium’s coordination number is higher than Sodium’s with Chlorine?
What is a crystal lattice?
Section 7.3
KC 23 How do chemists model the valence electrons in metal atoms?
What is a metallic bond?
How do the properties of a metal relate to the sea-of-electrons model?
Why does an ionic compound shatter when struck with a hammer?
KC 24 How can you describe the arrangements of atoms in metals?
Give 3 examples of arrangements of metal atoms in a crystal?
What is an alloy?
KC 25 Why are alloys more useful than pure metals?
Give 3 examples of alloys and their constituent elements.
What is a electrochemical cell?
How does it relate to a battery?
How does it generate electricity?
Chapter 8.1
What is a covalent bond?
What is a molecule?
What is a diatomic molecule?
What is a molecular compound?
What is the difference between a molecule and a formula unit?
KC 1 How are melting points and boiling points of molecular compounds usually different from those of ionic componds?
What is a molecular formula?
KC 2 What information does a molecular formula provide?
What does a molecular formula not tell you?
For example, what is glucose, l-fructose and d-fructose?
What is a structural formula?
What are the other common models for structural formulas on page 215?
What is an isomer?
Section 8.2
KC 13 What electron configurations do atoms usually achieve by sharing electrons to form covalent bonds?
Which groups of elements are commonly found in covalent bonds?
What is a single covalent bond?
KC 14 How is an electron dot structure used to represent a covalent bond?
How does a structural formula show a covalent bond?
What is an unshared pair?
Draw an electron dot structure for water, carbon dioxide, methane and ammonia.
KC 15 When are two atoms likely to form a double bond between them? A triple bond?
What is a double covalent bond?
What is a triple covalent bond?
What is the simplified (not what actually occurs) electron dot structure of an oxygen molecule? A nitrogen molecule?
What is a coordinate covalent bond?
Give an example of a coordinate covalent bond.
KC 16 How is a coordinate covalent bond different from other covalent bonds?
What is a polyatomic ion?
Draw the steps of generating the structural formula for the Sulfite ion.
What is bond dissociation energy?
KC 17 How is the strength of a covalent bond related to its bond dissociation energy?
Explain this idea in terms of carbon compounds, like methane and coal, and their relative stability.
KC 18 Draw the electron dot structure resonance structures of ozone and explain how they describe its bonding.
What are resonance structures?
KC 19 List three ways in which the octet rule can sometimes fail to be obeyed.
Draw the electron dot structure for sulfur hexafluoride. What is the unique application of sulfur hexafluoride.
Section 8.3
What is a molecular orbital?
KC How are atomic and molecular orbitals related?
What is a bonding orbital?
What is a sigma bond?
What is a pi bond?
What is VSEPR theory?
KC 24 Explain how the VSEPR Theory can be sued to predict he shapes of molecules.
Name some of the common molecular shapes.
What shape is methane? What shape is water? Methane? Carbon dioxide?
KC 25 How is orbital hybridization useful in describing molecules?
Section 8.4
What is a nonpolar covalent bond?
What is a polar covalent bond or polar bond?
KC 32 How do electronegativity values determine the charge distribution in a polar covalent bond?
Use the chart on page 238 and the chart on page 177 to determine the bond between F and O, O and Cl, N and H, H and O.
What is a polar molecule?
What is a dipole?
KC 33 What happens when polar molecules are between oppositely charged metal plates?
KC 34 Compare the strengths of intermolecular attractions to the strengths of ionic bonds and covalent bonds.
What are van der Waals forces?
What are dipole interactions?
What are dispersion forces?
What are hydrogen bonds?
How does hydrogen bonding affect water?
How does hydrogen bonding affect the structure of DNA?
What is a network solid?
KC 35 Explain why network solids have high melting points.
Use the chart on page 244 to compare and contrast ionic and covalent compounds, but also include polar and metallic compounds.
Property / Metallic / Ionic / Polar / CovalentMelting Points
Boiling Points
Solid, Liquid Or Gas
Conductivity
Malleable Ductile
***What facet of atomic structure and bonding accounts for this wide array of properties?