1 / 28

Covalent Bonding

Covalent Bonding. Sec. 9.2: Naming Molecules. Objectives. Identify the names of binary molecular compounds from their formulas Name acidic solutions. Naming Binary Molecular Compounds.

darryl-weeks
Download Presentation

Covalent Bonding

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Covalent Bonding Sec. 9.2: Naming Molecules

  2. Objectives • Identify the names of binary molecular compounds from their formulas • Name acidic solutions

  3. Naming Binary Molecular Compounds • A binary molecular compound contains ___ different elements, both ________ , bonded through a __________ bond. • Many have common names: • H2O is named water • NH3 is named ammonia • See Table 5 p. 251: MUST MEMORIZE!

  4. Naming Binary Molecular Compounds • Scientific names reveal a molecular compound’s composition • Rules • 1. Name the first element in the formula, using the entire element name • 2. Name the second element in the formula, using the ROOT of the element name and the SUFFIX -IDE. • 3. Add a prefix to each of the names to indicate the number of atoms of that type that are present. (see pg. 248)

  5. Exceptions • The first element name NEVER uses the prefix mono-. Example: CO is carbon monoxide, NOT monocarbon monoxide. • The final letter in the prefix may be dropped when the element name begins with a vowel. Example: CO is carbon monoxide, NOT carbon monooxide.

  6. Practice: H2O • Name of the first element is hydrogen. A prefix is needed. • There are 2 hydrogen atoms, so the first name becomes dihydrogen. • The root of the second element with -ide is oxide. • There is 1 oxygen atom, so the second name becomes monoxide. • Dihydrogen monoxide is the chemical name for water.

  7. - CCl4 - As2O3 - P2O5 - SO2 - NF3 Practice problems

  8. Writing Formulas of Molecular Compounds • Since the name reveals the composition, simply translate the information given into a formula. For example, dinitrogen pentaoxide is N2O5. • Practice: • sulfur difluoride • silicon tetrachloride • tetrasulfur tetranitride

  9. Naming Acids • Acids are compounds that produce hydrogen ions in water solutions. • Two types exist: binary acids and oxyacids.

  10. Binary Acids • Contain hydrogen and one other element • The prefix hydro- is used to name the hydrogen part of the compound. • The rest of first word consists of the root of the second element with the suffix -ic. • The second word is always acid. • HCl is hydrochloric acid • HBr is ….

  11. Exceptions • There are a few acids with that ARE NOT BINARY that are named according to these rules. • If NO OXYGEN is present in the formula, use the rules for binary acids, except the root of the second name comes from the polyatomic ion name. • Example: HCN is hydrocyanic acid

  12. Naming Oxyacids • These acids contain hydrogen and an oxyanion (anion containing oxygen). • - Identify the oxyanion present. Example: HNO3 - the oxyanion is nitrate. • - Name the oxyacid using the root of the anion, a suffix, and the word acid. • If the suffix of the anion is -ate, it is replaced by -ic. • If the suffix of the anion is -ite, it is replaced by -ous.

  13. HNO3 HNO2 H3PO4 Anion ends in -ate, so it is named nitric acid Anion is nitrite, so it is named nitrous acid. Anion is phosphate, so it is named ... Naming Oxyacids

  14. Practice Problems • - HI • - HClO3 • - HClO2 • - H2SO4 • - H2S

  15. Writing Formulas of Acids • Work backwards from the name, focusing on the rules that were used. • Example: hydroiodic acid • Because “hydro” is used, we know this is a binary acid. • The acid contains hydrogen and iodine. We know the second element iodine because of “iodic”. • The formula is derived by criss-crossing H+ and I-. The acid is HI.

  16. Example: Sulfurous acid • Sulfurous acid was named from a sulfur oxyanion with an -ite ending: sulfite • The oxyacid contains hydrogen and the oxyanion sulfite: H+ and SO3-2 • The formula for this acid would therefore be H2SO3

  17. Practice Problems • hydrofluoric acid • bromic acid • carbonic acid • phosphorous acid • chlorous acid

  18. Hydrates • As ions in a solution react to form an ionic compound, water often adheres to the ions as the compound forms. • These molecules of water become part of the structure of the ionic crystal that forms. • The water is called water of hydration and the solid compound formed is called a hydrate.

  19. Hydrates • A hydrate is defined as an ionic compound that has a specific number of water molecules bound to its atoms. Copper (II) sulfate pentahydrate (CuSO4. 5H2O)

  20. The gemstone opal is a hydrate of silicon dioxide.

  21. Naming hydrates • In the formula for a hydrate, the number of water molecules associated with one formula unit is written following a dot: Na2CO3.10H2O • Name the ionic compound and use a prefix, to indicate the number of water molecules, with the word hydrate: sodium carbonate decahydrate

  22. Practice Problems • CaCl2.2H2O is ____________________ • CuSO4.5H2O is ____________________ • Ba(OH)2.8H2O is __________________

  23. Writing Formulas for hydrates • Translate the information given in the name into a formula • cobalt (II) chloride hexahydrate • CoCl2.6H2O • Practice: iron (III) phosphate tetrahydrate

  24. Uses of hydrates • The anhydrous form of a hydrate - the one in which all the water has been removed through heating- can be used as a dessicant or drying agent. It will absorb water from the air or from a liquid environment. Such substances are called hygroscopic. If the substance absorbs enough water from the air to dissolve and form a liquid solution, it is said to be deliquescent.

  25. Determining % of water in a hydrate • Recall the method for determining percent by mass (pg. 75) • For hydrates, the percent by mass of water will equal • mass of water x 100 mass of hydrate

  26. Example: What is the water content in MgSO4.7H2O? • Add up the atomic mass (rounded to the nearest tenth) for each component of the compound; this is the mass of the hydrate. • Mg:24.3, S:32.1, O: 4 x 16.0 = 64.0 • H2O: (2 x 1.0) + 16.0 = 18.0 • 7H2O = 7 x 18.0 = 126.0 (mass of water) • Total mass = 246.4 • Divide the mass of water by the mass of hydrate and multiply by 100 • % mass of water = 126.0/246.4 x 100 = 51.14%

  27. Practice Problem: A 4.3 g sample of strontium chloride hexahydrate was heated. The mass of the anhydrous compound that remained after heating was 2.6 g. What percentage of water was in the hydrate?

  28. SrCl2.6H2O • Mass of anhydrous + Mass of water = Mass of hydrate, so Mass of water = 4.3 g - 2.6 g = 1.7 g • % mass of water = mass water/mass hydrate x 100 • = 1.7 g/4.3 g x 100 = 39.5%

More Related