1 / 11

Covalent Molecules

Covalent Molecules. Quiz on Friday, January 10. Review of Ionic Bonding. Ionic bonds occur between a metal and a nonmetal , or between a positively charged particle and a negatively charged particle. Ionic bonds involve a transfer of electrons.

evette
Télécharger la présentation

Covalent Molecules

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 Molecules Quiz on Friday, January 10

  2. Review of Ionic Bonding • Ionic bonds occur between a metal and a nonmetal, or between a positively charged particle and a negatively charged particle. • Ionic bonds involve a transfer of electrons. • Can you identify which of the following are joined by ionic bonds? • NaCl - K3N - MgBr2 • CO2 - N2 - Al2O3

  3. Covalent Bonding • Covalent bonds occur between two nonmetals. • A molecule is formed when two or more atoms bond covalently. • Covalent bonds involve sharing of electrons.

  4. Diatomic Molecules • Certain elements occur in nature as diatomic molecules and not as single atoms (more stable as the molecule) • Examples: • H2, N2, O2, • F2, Cl2, Br2, I2 • Diatomic Molecules are bonded together by covalent bonds.

  5. H H H O O + + = H or H O H + + = + Cl C C Cl Cl Cl Cl + or Cl Cl Cl Cl Cl C Cl Cl Lewis Structures • Use electron-dot diagrams to show how electrons are arranged in molecules. • A dot represents a valence electron and a line represents a shared pair of valence electrons. H2O CCl4

  6. Important Definitions • Chemical Formula: a representation, using symbols, showing the different types and number of atoms that make up a given compound or molecule • Subscript: small number, written behind an element, showing how many atoms of that element are found in a compound or molecule

  7. Naming Molecular Compounds • The first element written in the formula is always written first, using the element name. • The second element is named using the root of the element and the suffix “-ide”. • Prefixes are used to indicate the number of atoms of each type that are present in the compound. • Exception: Do not use the prefix mono- for the first element • Drop the final letter of the prefix when the element name begins with a vowel

  8. Table 1: Common Prefixes Used in Covalent Compounds

  9. What Does Naming Look Like? Carbon tetrachloride Carbon monoxide Nitrogen trifluoride Nitrogen monoxide 1. CCl4: 2. CO: 3. NF3: 4. NO:

  10. Now, you practice Carbon monoxide • CO2: ________________________________ • SO2: ________________________________ • S2O3: _______________________________ • N2O: _______________________________ • PCl5: ________________________________ • OF2: _____________________________ • N2O4: _____________________________ • S4N4: ______________________________ • SiCl4: ______________________________ • BF3: ________________________________ Sulfur dioxide Disulfur trioxide Dinitrogen monoxide Phosphorous tetrachloride Oxygen difluoride Dinitrogen tetroxide Tetrasulfur tetranitride Silicon tetrachloride Boron trifluoride

  11. What’s the formula? SeF6 • Selenium hexafluoride: ___________ • Disilicon hexabromide: __________ • Diboron silicide: __________ • Iodine pentafluoride: ________ • Hexaboron silicide: ________ • Diboron tetrabromide: _______ • Diphosphorous pentoxide: ______ • Carbon tetrafluoride: ________ • Tetraphosphorous pentasulfide: _______ • Hexasulfur oxide: _________ Si2Br6 B2Si IF5 B6Si B2Br4 P2O5 CF4 P4S5 S6O

More Related