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Unit 1 Notes Water

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Indirect uses are hidden uses such as the water needed to make food. ... Pure water is colorless, odorless and tasteless. Answer the question in. figure 1.21. ... – PowerPoint PPT presentation

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Title: Unit 1 Notes Water


1
Unit 1 NotesWater
2
Section A.41. Explain the diff. betw. direct and
indirect water use.
  • Direct can be directly (easily) measured and
    observed
  • Indirect uses are hidden uses such as the water
    needed to make food.

3
2. Compare and Contrast water usage in the West
and Midwest.
4
3. Explain the water used in making a can of
juice.
  • To grow fruit
  • To clean fruit
  • To make the juice
  • To make the container

5
Section A.54. Do questions 1-3, p. 17
  • 1. a. steam/elec.
  • b. steam/elec.
  • c. steam/elec.
  • d. irrigation / Ag.
  • e. mining
  • f. irrigation / Ag.

6
2.
  • East, South and Midwest mainly steam / electric
    due to large population
  • Also more industry
  • West and Hawaii are engaged in Ag. And the west
    is arid
  • Alaska sparse population, little industry, few
    crops mining of minerals

7
3. List two factors per region
  • East humid, high manufacturing, high population
  • South humid, farming, high population
  • Midwest humid, farming, moderate population
  • West arid, farming, variable population

8
Continued . . .
  • Alaska cold, mineral resources, low population
  • Hawaii warm, farming

9
Section A.65. Explain the distribution of
freshwater on earth.
  • Of all the water on earth, only 2.8 of it is
    fresh.
  • OF all freshwater, most in in glaciers, then
    ground water, lakes, atmosphere and rivers.

10
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11
6. What are the phases of water?
  • Solid - ice
  • Liquid
  • Gas water vapor

12
7. Explain the diff. between surface and
groundwater.
  • Surface water found in rivers and lakes

13
Groundwater
  • Found under the surface in aquifers.
  • Must be pumped to the surface.

14
Diagram of an aquifer
15
8. How is groundwater formed?Is it pure? Where
is it found?
  • Forms as precipitation seeps into soil and
    eventually to the rock beneath the soil
  • As it moves through the soil it dissolves gases,
    soil and mineral. These become part of the
    solution.
  • Found in the pores of sediment and rock beneath
    the surface.

16
Section A.89. (Discuss this as a class.)
17
Additional notes
  • Distillation a water purification process that
    is based on the different boiling points of
    substances.
  • Substances with lower b.p. vaporize first
  • Collect different samples of distillate at the
    process continues.

18
Tests for water purity
  • Electrical Conductivity will detect the
    presence of ions
  • Tyndall effect will show if there are suspended
    particles in the water.

19
Section B.1Define these terms
  • Density
  • Aqueous solution
  • 1. Explain what matter is.
  • Matter is anything that takes up space and has
    mass. Includes all solids, liquids and gases.

20
2. Give some of the physical properties of water.
  • Freezing point is 0 degrees Celcius
  • Boiling point is 100 degrees Celcius.
  • Density is 1.00 g/ml
  • Pure water is colorless, odorless and tasteless.

21
Answer the question in figure 1.21.
  • Sheeting means it rolls off the surface in a
    sheet rather than in drops.
  • Why
  • High surface tension the water molecules want
    to stick together due to strong molecular forces.

22
4. Answer the 3 questions on p.28 about density.
  • Section B.3
  • Define the following vocabulary terms
  • Heterogeneous mixture
  • Homogeneous mixture
  • Suspension Solution
  • Tyndall Effect Solute
  • Colloid Solvent

23
5. List the types of mixtures discussed in this
section.
  • Homogeneous mixtures or solutions
  • Heterogeneous mixtures such as colloids and
    suspensions.
  • A suspension of water
  • and flour

24
6. How is a suspension different than a colloid?
  • Suspension have visible particles that will
    eventually settle out. They also tend to block
    light
  • Colloids have microscopic particles suspended in
    them that will create the Tyndall Effect.

25
7. Give 3 examples of solutions.
  • Sugar water
  • Salt water
  • Air
  • Tea with sugar

26
8. How is the solute different from the solvent?
  • A solution is made of two parts, the solute and
    the solvent.
  • The solvent is the dissolving agent (it dissolves
    the solute)
  • The solute is the
  • substance being
  • dissolved

27
Section B.4 p. 31Define the vocab terms
  • Atom
  • Element
  • Compound
  • Chemical formula
  • Substance
  • Molecule

28
9. Explain the difference between a substance and
a mixture.
  • A substance has a uniform and definite
    composition ( like elements and compounds) that
    have unique properties.
  • A mixture is made of two or more substances that
    can be separated.

29
10. How is a compound different than an element?
  • Elements are made up of only 1 type of atom.
  • Compounds are made of two or more types of
    elements that have been chemically combined in a
    fixed proportion.

30
Give the chemical formulas
  • Baking soda
  • Ammonia
  • Chalk
  • Octane
  • NaHCO3
  • NH3
  • CaCO3
  • C8H18

31
12. Explain why oxygen, O2, is a molecule but
water is a molecular compound.
  • Oxygen is made up of the same type of atoms and
    still has the properties of oxygen.
  • In water, two elements have chemically changed to
    form something new with new chemical properties.

32
Section B.6 p. 34-36Define these terms
  • Chemical symbol
  • Chemical formula
  • Subscript
  • Chemical equation
  • Chemical reaction
  • Reactants
  • Products
  • Diatomic molecules

33
13. The language of chemistry is formulas. What
does this mean?
  • Chemical formulas are the words of chemistry.
  • We put them together in chemical equations or
    sentences to describe a chemical reaction.

34
14. What is a chemical sentence? Why?
  • A chemical sentence is a chemical equation.
  • It is made up of chemical formulas
  • It shows the reactants and products of a reaction

35
15. What are the 7 diatomic elements? Give name
and formula.
  • Hydrogen
  • Nitrogen
  • Oxygen
  • Fluorine
  • Chlorine
  • Bromine
  • Iodine
  • H2
  • N2
  • O2
  • F2
  • Cl2
  • Br2
  • I2

36
Section B.7 p. 36-37
  • 16. Answer the questions, 1 3.

37
Section B.817. What types of experiences do we
have that are evidence of the electrical nature
of matter?
  • Static in your clothes
  • Getting a shock from touching something
  • Rubbing your hair with a balloon

38
18. Explain the properties of the three types of
particles found in atoms.
  • PROTONS found in the nucleus, have a
    positive charge
  • NEUTRONS found in the nucleus, have no
    charge (are neutral)
  • ELECTRONS found around the nucleus in the
    electron cloud, have a negative charge

39
Section B.9Vocabulary.
  • Ions
  • Ionic compounds
  • Anion
  • Cation
  • Polyatomic ion

40
19. What is the difference between a sodium atom
and a sodium ion?
  • A sodium atom would be electrically neutral (have
    no charge)
  • A sodium ion has a negative charge because it can
    readily gain one electron

41
Sodium atom changing to an ion
42
20. What is an ionic compound?Give an example.
Also, give the anion and cation.
  • Ionic compounds are substances made up of
    positive ions (cation) and negative ions
    (anions).
  • EX. Hydrogen sulfide or H2S
  • Hydrogen is the cation H
  • Sulfur is the anion S2-

43
Ion Effect Ions in solution.
44
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45
21. What are two rules for writing chemical
formulas of ionic cmpds?
  • RULE 1 Place the cation first, then the anion
  • RULE 2 The correct formula will contain the
    fewest positive and negative ions needed to make
    the total electrical charge equal to zero.

46
22. How do you write the name of an ionic
compound?
  • RULE 1 Write the name of the cation first,
    then the anion.
  • RULE 2 - When the anion is a single atom, change
    the ending to -ide such as chlorine becoming
    chloride

47
Section B.10 p. 41
  • Make and complete a chart that answers the
    problems in this section.

48
Section B.11 p.42Vocabulary.
  • Confirming test
  • Precipitate
  • Qualitative test
  • Quantitative test
  • Reference solution

49
Section B.12 p.45
  • 23. Is distilled water 100 pure? Why or
    why not?
  • It is NOT 100 pure because is still contains
    some dissolved gases.
  • Some of these gases include nitrogen, oxygen and
    carbon dioxide.
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