Chemistry and its contributions to technology

1. August 2014
Ms. Claudia Barahona

2. Stage 1 Chemistry and its contribution to the advances of science and technology
Field and applications of chemistry
Relationship with other sciences
Classification and physical properties of matter
Everyday physical and chemical phenomena
Matter and energy interactions

3. Session 2
Review of propedeutic activities 1.1 and 1.2
Generic competences
4.1) Expresses ideas and concepts through linguistic, mathematical or graphical, representations.
4.3) Identifies key ideas in a text or speech and infers conclusions from them.
4.4) Communicates in a second language in daily life situations.
4.5) Handles information and communication technologies to obtain information and expressing ideas.

4. Session 2
Review of propedeutic activities 1.1 and 1.2
Disciplinary competences
2. Base opinions on science and technology impact of in our daily life assuming ethical considerations.

5. Chemistry and technology
What is studied by chemistry?
What is technology?

6. What is studied by chemistry?
Matter and the changes that matter undergoes.
What is technology?
The practical use of scientific information.
Chemistry and technology

7. «Plastics and fullerenes»
Uses and Importance
Chemistry and technology

8. Plastics
Plexiglass
Polyethylene
Nylon
Acrylics
Silicones PVC Poly styrene

9. What is Nanotechnology
The creation of useful or functional materials, devices and systems through control of matter on the nanometer lenght scale.

10. Field and applications of chemistry
Does chemistry happens only or mainly in a laboratory?

11. Field and applications of chemistry
Does chemistry happens only or mainly in a laboratory?

12. Field and applications of chemistry
Does chemistry happens only or mainly in a laboratory?

13. Branches of chemistry
•Substances containing carbon
Organic
•Study of all other substances EXCEPT those containing carbon.
Inorganic
•Composition, properties, and reactions of matter General

14. Contribution of chemistry and other sciences to the advances of humanity
Review main ides from the readings:
“Chemistry and other sciences”
“From the stone age to silicon era”
Main uses of:
Copper
Silicon
Petroleum
Examples of relation of chemistry with other sciences

15. Relationship with other sciences
Chemistry is often combined with other sciences such as :
Geology
Physics
Biology
Medicine

16. Relation of chemistry w/ other sciences
Science that studies:
Chemical compositions of ores, minerals, soils of the surface of the earth.
Geochemistry
Chemical reactions in biological systems.
Biochemistry
Physical nature of chemical systems including energy changes.
Physical chemistry

17. Chemistry applications…
Medicine
Nutrition
Forensic investigation
Technological advances
Cosmetology ……………

18. Classwork #1 Relationship of chemistry with other sciences
Compare/contrast table of the relationship of chemistry with other sciences.
1.Read carefully each of the following paragraphs that describe the process of gasoline combustion in an automobile engine, make a connection between Chemistry and other sciences such as Biology, Math, Social Sciences and physics.

19. The chemistry of engines
•When gasoline burns in the engine of an automobile a chemical reaction occurs producing water vapor, carbon dioxide but also a huge amount of energy is released, this energy is transformed into mechanical energy that produces the motion of the vehicle, electrical energy is also obtained which is used in the radio, lights and air conditioner.
Chemistry is related with_______
Biology, Math, Social Sciences and physics.

20. The chemistry of engines
The efficiency of this reaction is never a 100%, this efficiency is variable and it depends on the quality of the gasoline. Petrochemical engineers most perform calculations to predict the reaction yield obtained with each type of gasoline and let the consumer know.
Chemistry is related with____
Biology, Math, Social Sciences and physics.

21. The chemistry of engines
•In the process polluting substances are released. The main products of the process are CO2, water and soot. The effects of inhaling the products of combustion have been studied in humans and animals and include asthma, lung cancer, cardiovascular issues, and premature death.
Chemistry is related with:________
Biology, Math, Social Sciences and physics.

22. The chemistry of engines
•The excess of carbon dioxide produced by the burning of fossil fuels such as gasoline, contributes to environmental pollution, one of the main effects being the global warming. This is why governments of first world countries limit these emissions.
Chemistry is related with:___________
Biology, Math, Social Sciences and physics.

23. Conclusion
What can you conclude about the contributions of chemistry and other sciences in technology advances?

24. Session 3
Review of propedeutic activities 1.4, 1.5
Generic competences
4.3) Identifies key ideas in a text or speech and infers conclusions from them.
4.4) Communicates in a second language in daily life situations.
4.5) Handles information and communication technologies to obtain information and expressing ideas.

25. Session 3
Review of propedeutic activities 1.4, 1.5
Generic competences
5.1) Follows directions and procedures in a reflective way, understanding how each step contributes to achieve an objective.
5.2) Arrange information according to categories, hierarchies, and relationships.
5.3) Identifies the systems and rules or core principles that lead to a series of phenomena.
5.6) Uses information and communication technologies to process and interpret information.

26. Session 3
Review of propedeutic activities 1.4, 1.5
Disciplinary competences
2. Base opinions on science and technology impact of in our daily life assuming ethical considerations.
10. Relate symbolic expressions of a natural phenomenon and the observable features in plain sight or through instruments and scientific models.

27. Matter: Anything that has a mass and occupies space.
Pure substance: Matter with fixed/definite composition.
Elements: Composed of only 1 type of material.
Compounds: 2 or more elements chemically combined in the same proportions.*
* An important difference is that compounds can be broken down into simpler substances by chemical processes. Elements cannot. Activity I.4 Vocabulary terms

28. Mixture: 2 or more substances are physically but, not chemically combined.
Homogeneous or solution: Uniform composition throughout the sample.
Heterogeneous: Do not have a uniform composition throughout the sample
*Can be separated by physical processes, because there are no chemical interactions b/w components. Activity I.4 Vocabulary terms

29. Physical methods to separate mixtures: (at least 3) Boling, sifting, filtration, distillation, chromatography
Physical property: characteristics that can be observed or measured without affecting the identity of a substance. Ex: shape, color, melting point.
Chemical property: characteristics that indicates the ability of a susbtance to form another/new substance.
Physical change: change in which the appearance looks different but the composition remains the same.
Chemical change: when the original substance is converted into one or more new substances.
Activity I.4 Vocabulary terms

30. Sublimation Deposition Boiling point: Tº at which a substance exists as liquid and gas.
SOLID (Ice) LIQUID (Water) GAS (Water vapor)

31. E B SOLID (Ice) LIQUID (Water) GAS (Water vapor)
A)Freezing C) Melting D) Evaporation F) Condensation B) Deposition E) Sublimation

32. Concept map

33. States of matter: table

34. Exercises from chapter 2 of your textbook Mixture Mixture Compound Compound Element Homogeneous
Homogeneous Homogeneous Heterogeneous Heterogeneous

35. Exercises from chapter 2 of your textbook L G G
S Physical Physical Chemical Chemical

36. Exercises from chapter 2 of your textbook Physical Physical
Physical Chemical Chemical Chemical Physical Physical Physical

37. Element, compound or mixture?
Compound Mixture Element

38. Homogeneous or heterogeneous mixture? Homogeneous Heterogeneous Heterogeneous

39. I.5 The melting of the polar ice caps
Arctic effect
Global warming
Greenhouse effect
Possible solutions

40. Arctic effect
Effects of climate change in the Arctic including rising temperatures, loss of sea ice, and melting of the polar ice caps.
Potential release of methane.
Leading indicator of climate change.

41. Global warming
A gradual increase in the earth's average surface temperature.
Main cause: Anthropogenic activities /Human activity.

42. Greenhouse gases
A gas which traps the sun's heat.
Main greenhouse gases:
Carbon dioxide (CO2)
Methane (CH4)
Nitrous oxide (N2O)
Hydrofluorocarbons (HFCs) and perfluorocarbons (PFCs)

43. Possible solutions
Brain storming
HW:
Report, Activity 1.3
Due date:
session 1 week 2

44. Session 4
Directions for Integrative activity.
Classwork.
HW Print end of chapter
Generic competences
4.1) Expresses ideas and concepts through linguistic, mathematical or graphical, representations.
4.4) Communicates in a second language in daily life situations.
5.6) Uses information and communication technologies to process and interpret information.

45. Session 4
Directions for Integrative activity
Due: session 1 week 3.
Library visit or classwork.
HW Print End Of Chapter
Disciplinary competences
2. Base opinions on science and technology impact of in our daily life assuming ethical considerations.

46. Physical
Chemical
Property
Characteristics of a substance that can be observed or measured without affecting its identity .
Color, Shape, Odor, Luster, Size, Melting point, Density.
Characteristic that describes the abilty of a substance to change into a new one
Paper burns, iron rusts, silver tarnishes.
Physical and chemical properties

47. Physical
Chemical
Change
Changes in physical properties that retains the identity of the substance.
Change in which the original substance is converted to one or more new substances.
Physical and chemical changes

48. Matter
Anything that has a mass and occupies space.
According to the temperature matter can exist in different states.

49. Plasma

50. Sublimation Deposition Boiling point: Tº at which a substance exists as liquid and gas. SOLID (Ice) LIQUID (Water)
GAS (Water vapor)

51. States of matter:
Solid
Liquid
Gas
Characteristic
Shape
Volume
Arrangement of
particles
Interaction b/w
particles
Movement of
particles
Solid
Definite
Definite
Fixed,
very close
Very
Strong
Very slow
Liquid
Undefinite
Definite
Random,
close
Strong
Moderate
Gas
Undefinite
Undefinite
Random,
far apart
Essentially none
Very fast
The physical state of matter, depends on temperature.

52. Chemical reaction:
Chemical changes on which the initial substances are transformed into completely new substances; due to a rupture of their chemical bonds and the formation of new bonds of the present atoms.
1.Change in color.
2.Formation of a gas (bubbles)
3.Formation of a solid (Precipitate)
4.Produced or absorbed energy (heat,
flame, light)
Evidences of chemical reactions

53. Review

54. Physical property, physical change, chemical property or chemical change?
Instructions: Identify each fact:
1.Alcohol is flammable.
2.Alcohol is volatile, it evaporates easily.
3.A sample of table salt dissolves in water.
4.With time a battery looses its charge.
5.Aluminum is malleable.

55. States of matter
Identify the state of matter for the following examples at room temperature:
1.Oxygen
2.Water vapor
3.Candle wax
4.Alcohol

56. States of matter
Describe the difference in arrangement , interaction and movement of particles in:
1.Ice cube
2.Liquid water
3.Water vapor

57. Classification of matter Matter Pure substances Elements
Compounds Mixtures Homo geneous Hetero geneous

58. Mixtures, compounds or elements??
a.Compound
b.Mixture
c.Elements
d.Mixture a b
c d e f g h
e. Compound
f. Element
g. Compund
h. Compound
sugar

59. Element, compound, homogeneous or heterogeneous mixtures
Classify the following:
1.Gasoline
2.Wood
3.Bronze
4.Sandwich
5.Sugar
6.Scramble eggs
7.Silver
8.Ethanol

60. Law of definite proportions
Law of constant composition
States that a chemical compound always contains exactly the same proportion of elements by mass.
For example:
Water is always composed by 2 hydrogen atoms bonded to 1 oxygen atom. 11% Hydrogen and 89% oxygen by mass.
Salt: Definite proportion of 39.3% of sodium and 60.7% of chlorine by mass.

61. Law of conservation of mass
States that during any chemical reaction the mass of the system must remain constant, the mass can neither be created nor destroyed, although it may be rearranged in space.
The total mass of the reactants or starting materials must equal the mass of the products.

62. Law of conservation of energy
States that during chemical reactions energy is not created nor destroyed. (1st law of thermodinamics).

63. Potential and kinetic energy
Potential energy: Energy of an object or a system due to the position , or the arrangement of the particles of the system.
Kinetic energy: Energy which it possesses due to its motion.

64. End of stage one

65. Stage 2
Classification of elements in: Metals, Nonmetals and Metalloids
Classification of compounds by the number of elements and chemical function
Elements present in the human
body and acquisition sources
The effects and uses of chemical
compounds in our daily lives

66. Stage 3
•Development of atomic theories from Dalton to Quantum Mechanics
•Subatomic particles
•Quantum numbers and atomic orbitals
•Electron configuration
•Organization of elements on the
periodic table
•Periodic properties (trends):
–Atomic size
–Ionization energy
–Electronegativity

67. Stage 4
Types of chemical bonds: Ionic, Nonpolar covalent and polar covalent
Electronegativity
Polarity
Electron configuration and formation of ions
Properties of ionic and molecular compounds
Chemical bond and electrical conductivity
Modern materials