1. Unit 1: energy and matter in chemical Change
Science 10
Unit 1: energy and matter in chemical Change

2. Chapter 1: Atoms, Elements, and Compounds
1.1 investigating and working with chemicals

3. Modern Chemistry has a recent history dating back to the late 1700s
Modern Chemistry has a recent history dating back to the late 1700s. However, chemical properties and uses have been known to different civilizations for thousands of years:
bluffton.edu

4. North American Aboriginal Peoples
Tanning leathers
Herbal medicines
chinesemedicineadvisor.com
uwlax.edu

5. Ancient Egypt
Embalming and mummification
minnesota.publicradio.org

6. Ancient Rome, Greece, Persia
Metal working for armour
Dyes for art and paint
vector-clip-art.com
en.wikipedia.org
archive.worldhistoria.com

7. Material Data Safety Sheets (MSDS)
Even natural chemicals must be handled properly to ensure safety. Each chemical today has a Material Safety Data Sheet (MSDS) to inform you of its physical properties (melting point, boiling point, odour) and hazards and instructions for handling and storing it safely.

8. Workplace Hazardous Materials Information System (WHMIS)
WHMIS identifies eight classes of hazards:
Hazardous Materials are covered by the Workplace Hazardous Materials Information System (WHMIS) which informs workers about the chemicals they work with in three ways:
Controlled products must have informative labels in both English and French on their containers
Each controlled product must have an MSDS
Workers must complete an education program that the employer provides

9. Classifying Matter Matter Mixture Pure Substance
Anything with mass and volume
May be solid, liquid or gas
Mixture
Combinations of matter that can be separated by physical means
Do not have definite composition
Pure Substance
- Matter that has a definite composition
Heterogeneous Mixture (Mechanical Mixture)
Different components of the mixture are visible
Composition is variable throughout the mixture
Homogeneous Mixture (Solution)
Different components are not visible
Composition is constant throughout the mixture
Element
- Cannot be chemically broken down into simpler substances
Compound
Two or more elements that are chemically combined
Can be separated chemically into simpler substances

10. Practice Problems pg. 10 #1-4

11. Chapter 1: Atoms, Elements, and Compounds
1.2 developing atomic theories

12. From Ancient Greece to today…

13. Assignment
Create a chart that follows the development of the Atomic Model throughout history. You can use the chart below to get started:
Model of the Atom
Why Model was Proposed
Key Points of the Model
Why Model was rejected or modified
Democritus
John Dalton’s Billiard Ball
J.J. Thomson’s Raisin Bun or Plum-Pudding
Ernest Rutherford’s Model
Niels Bohr’s Model

14. John Dalton’s Atom The Billiard Ball Model
All matter is made up of small particles called atoms
Atoms cannot be created, destroyed, or divided into smaller particles
All atoms of the same element are identical in mass and size but different in mass and size to atoms of other elements
Compounds are formed when atoms of different elements combine in fixed or definite proportions
Chemical reactions change the way atoms are grouped but the atoms do not change
thewallmachine.com

15. The Cathode Ray Tube (CRT)
A gas discharge tube contains gas at a low pressure.
When electricity is run through it, a ray is formed and light is produced across the tube.

16. J.J. Thomson ( )
J.J. Thomson determined that the ‘ray’ in the Cathode Ray Tube was made up of a stream of negatively charged particles
He added charged plates to bend the cathode rays.
Based on the radius of the path, he determined that the mass of the particle was much less than that of an atom and that the negatively charged particle was a unique particle – the electron.
cnx.org

17. The Raisin-Bun or Plum-Pudding Model
Since these negatively charged electrons appeared to be present in all samples of matter, Thomson proposed that every atom contained electrons.
Since most matter was neutrally charged, there must also be a positively charged part of the atom.
Thomson thus proposed a positively charged sphere with many negatively charged electrons present on the surface of the sphere.

18. Ernest Rutherford ( )
Rutherford conducted his gold foil experiment to further examine the structure of atoms
He directed strongly positive alpha particles towards a thin layer of gold foil.
Most of the particles passed straight through, however some were deflected and even bounced back.

19. Protons and a Nucleus
Since most of the particles passed straight through, Rutherford concluded most of the atom is empty space
Since some of the particles reflected and deflected there must be a dense, massive nucleus to each atom. He determined that this was positively charged, made up of protons
The negatively charged electrons must orbit around the positively charged nucleus much like planets orbit the sun.

20. The Discovery of the Neutron
The Hydrogen atom is made up of 1 proton and 1 electron
Rutherford hypothesized that the next biggest atom, helium, would be 2 protons and 2 electrons. Therefore it should have a mass that is twice that of hydrogen.
Helium is 4 times more massive than hydrogen.
The neutron was discovered as a neutrally charged particle in the nucleus that has the same mass as a proton
en.wikipedia.org 

21. Niels Bohr ( )
According to physical theory, the electrons orbiting the nucleus, should be losing energy in the form of light or radio waves. Losing energy would mean that the electron would come out of orbit and crash into the nucleus. This does not happen.
When electrical energy is applied to gases, they do emit light – a specific colour of light for each gas. Each colour corresponds to a specific wavelength of light or a specific energy. Rutherford’s model did not explain this, but Bohr’s did.
en.wikipedia.org 

22. Energy Levels
Electrons in an atom have certain allowed energies that enable the atom to remain stable – energy levels.
Electrons can only move from one of these allowed energy levels to another – they cannot exist between them.
In order to jump from one level to the next they will absorb a specific amount of energy (jumping up a level), or emit a specific amount of energy (falling back down a level)
library.thinkquest.org 

23. Our Working Model of the Atom…
Nucleons (protons and neutrons) make up the nucleus of an atom and electrons fill the space around the nucleus.
Subatomic Particle
Relative Charge
Symbol
Mass (in g)
Radius (in m)
proton
1 + p+
1.67 x 10-24
10-15
neutron n0
electron
1 - e-
9.02 x 10-28
Smaller than 10-18

24. Nuclear Notation
Isotopes – atoms made up of the same number of protons, but different number of neutrons
The atomic number is the number of protons and identifies the atom
The mass number is the total number of protons and neutrons
An atom has a neutral charge so there are equal numbers of protons and electrons in every atom
Ex.
11H mass number is top, atomic number is bottom
There is one proton, zero neutrons, and one electron.
The name is hydrogen - 1

25. Homework: pg. 23 #5-8, pg.24 #2, 4

26. Chapter 2: Names, Formulas, and Properties
2.1 Chemical Names and formulas

27. International Union of Pure and Applied Chemistry (IUPAC)
Founded in 1919, IUPAC developed a systematic method to name chemicals according to their composition.
The systematic name allows us to determine the chemical formula and predict some of its properties.

28. Binary Compounds
Compounds that are made up of two elements are called binary compounds.
The names of binary compounds almost always end with the suffix “-ide”.
commons.wikimedia.org

29. Binary Molecular Compounds
A binary molecular compound forms when two non-metallic elements come together and form a covalent bond (sharing electrons).
Example – dihydrogen monoxide – fatal if inhaled
montessorimuddle.org

30. Rules for Naming Binary Molecular Compounds
1. The first element in the name and formula is usually the one that is furthest to the left on the periodic table.
2. The suffix “-ide” is attached to the name of the second element.
3. Prefixes are used to indicate how many atoms of each type are present in one molecule of the compound.
ths.talawanda.net

31. Examples: NO
N2O
NO2
N2O3
N2O4
N2O5
Practice Problems pg. 44 #1-4

32. Names and Formulas for Binary Ionic Compounds
A binary ionic compound is composed of ions of one metal element and ions of one non- metal element joined by ionic bonds.
elmhurst.edu

33. Rules for writing names and formulas:
Ex. An ionic compound is made between calcium and fluorine.
The name is calcium fluoride
The formula is CaF2
The first element in the name and formula is the metal.
The second element is the non- metal. The suffix “-ide” is attached to the name.
The chemical formula shows the simplest whole number ratio of each type of ion in the compound.
*The names of ionic compounds DO NOT contain prefixes*
en.wikipedia.org

34. Example: Predict the formula of Lithium Oxide
Solution:
Identify the type of compound – metal & non-metal therefore ionic
Determine the charges on the ions – Li1+ and O2-
The compound must be electrically neutral. Therefore it will take two lithium ions to balance with one oxide ion.
The formula is Li2O

35. Practice Problems: pg. 45 #5-8

36. Cation Charges
Many of the transition metals (elements in groups 3-12) are able to form more than one type of cation.
Ex. Nickel can form Ni2+ or Ni3+
Ex. Copper can form Cu+ and Cu2+
If you are given the formula of an ionic compound you can determine the charge on the cation.
en.wikipedia.org

37. Example: Which copper cation, Cu+ or Cu2+, is in CuCl2
Solution:
Begin by writing out the two ions involved. Chloride is always a Cl1- and the copper could be either Cu+ or Cu2+
The compound must be electrically neutral. If there are two Cl1- ions then the single copper must be a 2+ charge.
Therefore the cation is Cu2+

38. Practice Problems: pg. 46 #9, 10

39. Naming Cations Using the Stock System
When writing the name of an ionic compound that consists of a transition element that could be different charges, the charge on the cation is written in parentheses, as a Roman numeral after the name of the metal.
Example: Cu2+ is copper (II)

40. Example: Write the chemical formula for copper(II) oxide
Solution:
The copper cation is named copper(II) and therefore is Cu2+
The oxide anion is always O2-
The compound must be electrically neutral so the charges must cancel.
Therefore, one copper(II) ion will combine with one oxide ion.
The formula is CuO

41. Practice Problems: pg. 47 #11-12

42. Homework: Investigation 2-A

43. Compounds Containing Polyatomic Ions
Many ionic compounds are not binary because they are made up of one or both ions containing more than one type of atoms – polyatomic ions.
Polyatomic ions are made of covalent bonds that as a group have a collective positive or negative charge.

44. Example: What is the formula of ammonium sulfide?

45. Example: What is the name of CuCO3

46. Practice Problems: pg. 52 #13-16

47. Families of Polyatomic Anions
Ex. Nitrate, nitrite or sulfate, sulfite
Patterns exist:
In each family, the anion ending with “-ate” serves as a reference point. The other anions are named according to the number of oxygen atoms in their formula, in relation to the reference anion.
Compared with an “__-ate” anion, an “___-ite” anion has one less oxygen in its formula
4. Compared with an “____-ate” anion, a “hypo___ite” has two less oxygen atoms in its formulas 5. Compared with an “____-ate” anion, a “per_____ate” has one more oxygen atom in its formula.

48. Practice Problems: pg. 53 #17-19

49. Hydrogen Compounds
Hydrogen is a non-metal even though it appears on the left side of the periodic table.
Therefore, these hydrogen compounds are molecular but they do not use prefixes
Common examples are on Table 2.5 on pg. 54 in textbook.
Homework: pg. 55 #1-6

50. Chapter 2: Names, Formulas, and Properties
2.2 Explaining properties of substances

51. Bonding and Properties
One of the ways Chemists determine features about the structure and bonding of different substances is to observe physical and chemical properties such as:
Melting point
Boiling point
Electrical conductivity when dissolved in water
Chemicals have different properties in different states so we use subscripts to show the state of a substance – (s) , (l) , (g) , (aq)
chemistry11mrstandring.wikispaces.com

52. Properties of Ionic Compounds
In solid state, ionic compounds have regular crystalline shapes with flat sides.
Ionic compounds tend to have high melting points suggesting the bonds between cations and anions is very strong.
In the solid state, ionic compounds do not conduct electricity suggesting ions are not free to move.
When melted or dissolved in water, ionic compounds are electrolytes – they conduct electricity.

53. Properties of Molecular Compounds
Most molecular compounds have relatively low melting points suggesting that the attractive forces between molecules must be weak.
Once melted, molecular compounds can be heated further without decomposing suggesting the covalent bonds within molecules are strong.
Molecular substances are non- electrolytes or they do not conduct electricity in any pure state.
Some molecular compounds do conduct electricity when dissolved in water
en.wikipedia.org

54. Toxic Properties of Substances
Every chemical has potential risks that can be harmful.
Deciding to use chemicals always involves balancing risks and benefits based on what you know about their properties.
Table 2.8 on pg. 60

55. Check Your Understanding:
Pg. 62 #1-5

56. Chapter Two Project Investigation 2-C Reducing the Risk Pg. 61