Download
a look at water and its contaminants n.
Skip this Video
Loading SlideShow in 5 Seconds..
A Look at Water and Its Contaminants PowerPoint Presentation
Download Presentation
A Look at Water and Its Contaminants

A Look at Water and Its Contaminants

128 Views Download Presentation
Download Presentation

A Look at Water and Its Contaminants

- - - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

  1. A Look at Water and Its Contaminants Water Part B

  2. Physical Properties of Water • Matter • anything that occupies space and has mass

  3. Physical Properties of Water • Physical Properties: can be observed or measured without changing the identity of a sample of matter • Examples: • Boiling point, melting point, density, color

  4. Physical Properties of Water • Density: mass  volume • the density of liquid water is 1.00 g/mL

  5. Physical Properties of Water • Physical state affects density: • gases are much less dense than liquids • solid form of a substance is usually denser than its liquid form • EXCEPT WATER: As water freezes it occupies a larger volume (d = 0.92 g/mL) • the density of liquid water is 1.00 g/mL

  6. Physical Properties of Water • clear, odorless, colorless, and tasteless • easily changes to each of the three phases of matter • “universal solvent”- so many substances easily dissolve in water to make aqueous solutions.

  7. Physical Properties of Water • high boiling point 100 C • high surface tension

  8. Mixtures and Solutions • Mixture: two or more substances are mixed together and they keep their individual properties • Heterogeneous mixture: a mixture that is not uniform throughout • Example: Chocolate chip cookie • Homogeneous mixture (Solution): a mixture that is uniform throughout • Example: Peanut Butter Cookie

  9. Mixtures and Solutions • Mixtures are classified by size of the particles in the mixture.

  10. Mixtures and Solutions Solution- smallest particle size, • salt water • Solute- substance that is dissolved • Solvent- substance that does the dissolving • Kool-Aid

  11. Mixtures and Solutions • Colloid-medium particle size, • Fog • Shows the Tyndall Effect light is scattered in many directions and can easily be seen. • like seeing dust particles in the light beam of a light

  12. Mixtures and Solutions • Suspension-largest particle size, • medicine that says “shake before using”

  13. Particulate View of Water • Atoms: All matter is composed of atoms; smallest particles possessing the properties of an element • Element: matter that is made up of only one kind of atom • oxygen is an element because it is composed of only oxygen atoms • 90 elements are found in nature!

  14. Particulate View of Water • Compound: substances composed of two or more elements linked together chemically in fixed proportions • water H2O • table salt NaCl • ammonia NH3 • baking soda NaHCO3 • chalk CaCO3

  15. Symbols, Formulas & Equations • Chemical Symbols: the international language of chemists and scientists across the planet • each element is assigned a symbol • the first letter is capitalized; all other letters are lowercase • Al, Cl, Ag, Mg

  16. Symbols, Formulas & Equations Subscripts: a number written below which indicates the number of atoms of each element that are present in a substance  H2O 2 Atoms of hydrogen 1 Atom of oxygen C3H8 3 Atoms of carbon 8 Atoms of hydrogen

  17. Symbols, Formulas & Equations • Chemical reactions: creating new substances • the new substances have completely different properties than the original substances. 2H2 + O2 2H2O Hydrogen + Oxygen  Water Reactants  Products

  18. Symbols, Formulas & Equations • Diatomic molecules: elements that exist as two bonded atoms of the same element • H2, N2, O2, F2, Cl2, Br2 & I2 • All other elements are written at single atoms (Ca, Fe, Na & Mg)

  19. The Electrical Nature of Matter • Remember: LIKE CHARGES REPEL AND UNLIKE CHARGES ATTRACT! • Atoms have: • Protons- positive • Electrons- negative • Neutrons-neutral (no charge)

  20. The Electrical Nature of Matter • Let’s try • An atom has: • 15 protons + 15 electrons = • 20 protons + 21 electrons = • 19 protons + 18 electrons = • 10 protons + 12 electrons=

  21. The Electrical Nature of Matter • Opposites attract- • this is the glue to hold atoms together • These are chemical bonds.

  22. Ions and Ionic Compounds • Ions: • charged atoms; • atoms that have gained or lost electrons to form negative or positive ions • Ionic Compounds: compounds composed of positive and negative ions

  23. Ions and Ionic Compounds • Cation: a positively charged ion (Na+) • Anion: a negatively charged ion (Cl-) • Polyatomic ion: (many-atoms) an ions made of two or more bonded atoms (NH4+ or NO3-)

  24. Ions and Ionic Compounds • Step 1: Write the symbols for the ions side by side, with the positive ion (or most metallic element) first • Step 2: Cross over the charge values to give subscripts • Step 3: Check the subscripts by making sure the total charge of ions in the compound is zero, simplify • Step 4: Write the formula

  25. Ions and Ionic Compounds • Let’s try: Need to use ion chart • zinc oxide • aluminum sulfide • calcium carbonate

  26. Ions and Ionic Compounds • Naming Compounds • Nomenclature: the method of naming chemical compounds 1. write the name of the element having a positive charge 2. add the name of the negative element 3. the negative element must be modified to end in –ide

  27. Ions and Ionic Compounds • Let’s try: Use the chart of ions • NaI2 • K2O • BaSO4