Review Unit 6 – Bonding

I. Bond Types: Fill in the table to show the basics of bond types.

BondType of atoms

involved

Electrons transferred or shared?

Type of Compound

formed

What holds the bond together?

IonicM/N Trans Ionic Polar e- transfer,

electrostatic forces

CovalentN/N Shared Covalent

Polar and Nonpolar

Sharing of e-

MetallicM Shared Alloys Sharing of e-

II. Short Answer:1. Why are some covalent bonds polar? Higher electronegative

atoms unequally share the electrons in the bond.2. Which of the following compounds express polarity? To which

element are the compounds polar too?a. H2O Yes Ob. HF Yes Fc. CCl4 Nod. CO2 Yes O

3. What are Binary Acids? List 4 and include the formula for each. Binary acids consist of H and another element. HF HCl HI HBr

4. What are Tertiary Acids? List 4 and include the formula for each. Tertiary Acids include H and a polyatomic ion in most cases. HNO3, HClO3, HPO4, and H2SO3

5. How does electronegativity relate to the strength of an acid? The higher the electronegativity the greater the strength of the acid.

6. Is it possible for a bond to be partially ionic? Explain. No, only whole electrons are transferred in an ionic bond resulting in a definite charge.

7. What is an ion? How does it form? An ion is a charged atom that forms from the gain or loss of electrons.

8. What is a polyatomic ion? What kind of bond holds the atoms in a polyatomic ion together? A polyatomic ion is a charged, covalently bonded molecule that combines with a metal to form an ionic compound.

9. Show the electron configuration for each of the atoms below and the configuration for the ion as well.

a. Ca1s2 2s2 2p6 3s2 3p6 4s2

Ion: 1s2 2s2 2p6 3s2 3p6

b. N1s2 2s2 2p3

Ion: 1s2 2s2 2p6

c. Hg (ion: 2+)[Xe] 6s2 4f14 5d10

Ion: [Xe] 4f14 5d10 *** Remember the valence shell is the highest quantum number. That is why 6s left.

III. Lewis Dot Structures: Show the bonding that would occur in the following compounds. 1. Carbon tetrachloride 4. Barium oxide

2. Potassium chloride 5. Nitrogen trihydride

3. Copper (II) fluoride 6. Hydrosulfuric acid

IV. Ionic, Molecular and Metallic Compounds: Complete the chart below.

Type of Bond Solubility Conductivity Melting Point

IonicYes In aqueous

and little in molten

Relatively high

CovalentOnly with like

moleculesNo Relatively low

MetallicNo Yes moderate

V. Write formulas for the following compounds.

1. magnesium oxide MgO

2. Potassium hydroxide KOH

3. copper (II) carbonate CuCO3

4. acetic acid CH3COOH

5. lead (II) nitrate Pb (NO3)2

6. carbon disulfide CS2

7. iron (III) chloride FeCl3

8. ammonium phosphate

(NH4)3PO4

9. nitrogen tribromide NH3

10. potassium tungstate

K2WO4

11. nitrous acid HNO2

12. hydrosulfuric acid

H2SO4

13. sulfur dioxide SO2

14. sodium chlorate NaClO3

15. copper (I) sulfite

Cu2SO3

VI. Write names for the following compounds.

1. BaCl2 Barium Chloride

2. K2CO3 Potassium Carbonate

3. HgI2 Mecury (II) Iodide

4. HNO3 Nitrous Acid

5. Ca(NO3)2 Calcium Nitrate

6. CuO Copper (II) Oxide

7. HI Hydroiodic acid

8. PCl3 Phosphorus trichloride

9. (NH4)2CO3 Ammonium

Carbonate

10. NO2 Nitrogen Dioxide

11. AuBr Gold(I) Bromide

12. H3PO3 Phosphorus acid

13. Na2O Sodium Oxide

14. NBr Sodium Bromide

15. CaO Calcium oxide

VocabularyChapter 8 Chapter 9chemical bond formula unit covalent bondcation monatomic ion moleculeanion oxidation number Lewis structureionic bond polyatomic ion endothermicelectrolyte oxyanion exothermiclattice energy electron sea model structural formuladelocalized electrons metallic bond alloy

1. Given a name for a compound, be able to give the chemical formula. (ionic, covalent or acid)2. Give the chemical formula for a compound, be able to name it. (ionic, covalent or acid)3. Be able to explain why two elements will form an ionic bond.4. Be able to explain properties of metals, based on their bonding.5. Be able to explain why water is a polar molecule.6. Be able to explain what an electrolyte is.6. Be able to draw Lewis Structures of ionic compounds or molecules.7. Be able to determine if a bond is polar, nonpolar covalent or polar covalent.8. Know properties of ionic and covalent compounds and metals.