Ionic and Covalent Bonding Review KEY PDF
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This document is a review sheet for a chemistry class, likely high-school level. It covers topics like determining valence electrons, forming cations and anions, ionic and covalent bonding, as well as naming various compounds.
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# Ionic and Covalent Bonding - Review ## Ions 1. What are valence electrons? - e on **outer**most shell 2. Fill in the chart below for each element: | Element | # valence e | Lewis Diagram | | -------- | ------------ | --------------- | | Rb | 1 | Rb: | | S |...
# Ionic and Covalent Bonding - Review ## Ions 1. What are valence electrons? - e on **outer**most shell 2. Fill in the chart below for each element: | Element | # valence e | Lewis Diagram | | -------- | ------------ | --------------- | | Rb | 1 | Rb: | | S | 6 | ·S· | | Sr | 2 | ·Sr· | | Al | 3 | ·Al· | | C | 4 | ·C· | | Kr | 8 | ·Kr· | | P | 5 | ·P· | | I | 7 | ·I· | * _**brackets are okay but not necessary**_ 3. How many valence electrons do atoms in the noble gas family have? What does this mean about their reactivity? - 8 (or He has 2) - **non reactive** 4. How do cations form? - **lose** c- 5. How do anions form? - **gain** e- 6. Atoms of which elements tend to **gain** electrons? - **nonmetals** 7. Atoms of which elements tend to **lose** electrons? - **metals** 8. Which elements only need two valence electrons to be happy? Why? - 1-5 ( H-B) **small** enough to **empty** to **full** first shell ( 2e-) 9. Label the valence electron pattern and ion charge pattern on the periodic table below. | | | | | | | | | |---|---|---|---|---|---|---|---| | **ion** | **→** | **2** | **3+** | **1** | **4 3 -2 -1 -8** | | | | **Ve** | | **2** | **3** | **4** | **5 6 7** | **2** | **8** | 10. Complete the table below: | Element | # valence e | gain/lose e (how many?) | Ionic charge | metal/nonmetal | | -------- | ------------ | ----------------------- | -------------- | ---------------- | | Mg | 2 | lose 2 | +2 | metal | | O | 6 | gain 2 | -2 | nonmetal | | P | 5 | gain 3 | -3 | nonmetal | | Br | 7 | gain 1 | -1 | nonmetal | | Rb | 1 | lose 1 | +1 | metal | | Ar | 0 | N/A | | | | S | 6 | gain 2 | -2 | nonmetal | | N | 5 | gain 3 | -3 | nonmetal | | Li | 1 | lose 1 | +1 | metal | ## Ionic Bonds 11. How are ionic compounds formed? - **transfer** of e- from **metal** to **nonmetal** 12. What determines the specific ratio of cations to anions in an ionic compound? - **charges** of **cations** & **anions** must add to **neutral** compound 13. For each ionic compound below, draw the Lewis Dot Diagram, then write the formula and name of the compound. - a. K and Cl: * Lewis Dot Diagram: K. :Cl * Formula: [K]+ [Cl]- * Name: Potassium Chloride - b. Sr and Br: * Lewis Dot Diagram: Sr: :Br: * Formula: [Sr]2+ 2[Br]- * Name: Strontium Bromide - c. Li and N: * Lewis Dot Diagram: Li: N : Li: * Formula: 3[Li]+ [N:]3- * Name: Lithium Nitride - d. Al and S: * Lewis Dot Diagram: Al: S: Al: * Formula: 2[Al]3+ 3[S]2- * Name: Aluminum Sulfide - e. Ca and O: * Lewis Dot Diagram: Ca: O: * Formula: [Ca]2+ [O:]2- * Name: Calcium Oxide - f. Mg and P: * Lewis Dot Diagram: Mg: P: * formula: [Mg]2+ [P:]3- * Name: Magnesium Phosphide ## Covalent Bonds 14. How are covalent bonds formed? - **sharing** e- between **nonmetals** 15. Explain three ways that covalent bonds differ from ionic bonds. - **polyatomics (parenthesis), sharers, transfer, presence of metal/roman numeral, prefixes** 16. Classify the following compounds as ionic or covalent and name them accordingly. | Compound | Type | Name | | ---------- | -------- | -------------------------------------------------------- | | MgCl<sub>2</sub> | Ionic | Magnesium Chloride | | CO<sub>2</sub> | Covalent | Carbon Dioxide | | Na<sub>2</sub>O | Ionic | Sodium Oxide | | SCl<sub>2</sub> | Covalent | Sulfur Dichloride | | N<sub>2</sub>O<sub>5</sub> | Covalent | Dinitrogen Pentoxide | | K<sub>2</sub>SO<sub>4</sub> | Ionic | Potassium Sulfate | | NO | Covalent | Nitrogen Monoxide | | NH<sub>3</sub> | Covalent | Nitrogen Trihydride | | NaCl | Ionic | Sodium Chloride | | MgO | Ionic | Magnesium Oxide | 17. Identify the following compounds as ionic or covalent and write their formulas: | Compound | Type | Formula | | ----------------------- | -------- | -------------------------- | | Dihydrogen monoxide | Covalent | H<sub>2</sub>O | | Aluminum sulfate | Ionic | Al<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> | | Sodium hydroxide | Ionic | NaOH or Na(OH) | | Iodine tribromide | Covalent | IBr<sub>3</sub> | | Arsenic trichloride | Covalent | AsCl<sub>3</sub> | | Tin (II) sulfide | Ionic | SnS or Sn(SO<sub>4</sub>) | | Iron (III) oxide | Ionic | Fe<sub>2</sub>O<sub>3</sub> | | Silicon tetrachloride | Covalent | SiCl<sub>4</sub> | | Calcium phosphate | Ionic | Ca<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub> | 18. Perform the following mole conversions: | Calculation | Answer | Description | | ---------------------------------------- | -------------------------------- | ------------------------------------------------- | | 138.2 g Ca(OH)<sub>2</sub> to mol | 1.864 mol Calcium hydroxide | | | 248.4 g K<sub>2</sub>S to mol | 2.254 mol potassium sulfide | | | 5 mol CCl<sub>4</sub> to g | 769.05 g carbon tetrachloride | | | 2.5 mol AlF<sub>3</sub> to g | 209.94 g aluminum fluoride | |
