1 / 16

Dihydrogen Monoxide

Dihydrogen Monoxide. has killed over 100,000 people world wide, usually through inhalation if you wash your food you can never get this chemical off No matter what you do you will be exposed to this chemical every day of your life until you die Should this chemical be banned?.

aine
Download Presentation

Dihydrogen Monoxide

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. Dihydrogen Monoxide • has killed over 100,000 people world wide, usually through inhalation • if you wash your food you can never get this chemical off • No matter what you do you will be exposed to this chemical every day of your life until you die • Should this chemical be banned?

  2. Dihydrogen Monoxide • If you haven’t guessed already, dihydrogen monoxide is water! • H2O

  3. Rules for naming binary covalent (molecular) compounds: 1. Look to see if the compound is composed of two nonmetals. If yes, then it is covalent (molecule). If not, it is most likely ionic (usually a metal and nonmetal) 2. Write the name of the first element, using a prefix only if there is more than one atom. 3. Write the name of the second element always using a prefix to indicate the number of atoms. 4. Change the ending to –ide.

  4. Prefixes (Covalent Bonds ONLY) mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8 nona- 9 deca- 10

  5. Practice: • Carbon dioxide • Carbon monoxide • Sulfur trioxide • Carbon tetrachloride • Diphosphorus pentachloride

  6. Check the Practice: • Carbon dioxide = CO2 • Carbon monoxide = CO • Sulfur trioxide = SO3 • Carbon tetrachloride = CCl4 • Diphosphoruspentachloride = P2Cl5 Complete the worksheet provided.

  7. Compare and Contrast Sodium Chloride (Table Salt) Formula: Sucrose (Table Sugar) Formula:

  8. Ionic vs. Covalent Bonds Ionic Bonds • Gain or lose electrons • Metal + Nonmetal (usually) • Usually solids • Stronger bond (high melting point) Covalent Bonds • Share valence electrons • Nonmetal + Nonmetal • Usually gases or liquids • Weaker bond (lower melting point)

  9. Covalent Bond • The attraction that forms between atoms when they share electrons. • Molecule – neutral particle that forms as a result of sharing electrons • Occur between nonmetals • Most covalent bonds are either liquids or gases.

  10. Group 4 (Carbon and Silicon) have 4 valence electrons. • It takes a great deal of energy for these atoms to lose electrons. • Each time an electron is lost, the nucleus holds the remaining electrons more tightly, therefore become more stable by sharing electrons.

  11. Single Covalent Bonds • Made up of 2 shared electrons, usually from each of the other atoms in the bond. • Water molecule contains two single bonds.

  12. Multiple Bonds • A covalent bond can contain more than one pair of electrons. • Demonstration of bonding in N2

  13. Polar Molecule • Electrons are not always shared equally between atoms in a covalent bond. • One end of the molecule has a partial positive charge, and the other end has a partial negative charge. The overall molecule is still neutral. • Examples: water (H2O), ammonia (NH3)

  14. Nonpolar molecule • Electrons are shared equally in bonds, and does not have oppositely charged ends. • Molecules made from two identical atoms: Br2 , I2 , N2 , Cl2 , H2 , O2 , F2 or made from molecules that are symmetrical (CCl4)

  15. Solutes and Solvents • Solute –the substance that is dissolved • Solvent – the substance doing the dissolving. Water is considered the “universal solvent” because many things dissolve in water.

  16. In solution, “Like dissolves like” In general, • Polar substances are water-soluble (polar solute dissolves in polar solvent). • Nonpolar substances do not dissolve in water. (Nonpolar solute dissolves in nonpolar solvent).

More Related