1. Atomic Structure
Chapter 3

2. Objectives
IV.B.1(a) - Describe the importance of models for the study of atomic IV.B.1(b) - Describe the crucial contributions of scientists and the critical experiments that led to the development of the modern atomic model

3. Why are models important?
Allow visualization
Predict how elements and compounds will behave
Explain WHY elements and compounds behave the way they do

4. 3.1 - The elements Objectives: Learn the abundances of the elements
Learn the names and symbols of commonly used elements
3.1 - The elements

5. The Elements Profound effects on health Produce ornaments and tools
Lithium on manic-depression
Cobalt on violent behavior
Produce ornaments and tools

6. All of the materials in the universe can be chemically broken down into about 100 different elements.
Compounds are made by combining atoms of the elements just as words are constructed from the letters in the alphabet.

7. The Greeks 4 elements: 1st to attempt to explain chemical changes
Earth
Air
Fire
Water
1st to attempt to explain chemical changes

8. The Alchemists Magicians/mystics who tried to turn cheap metal to gold
Discovered sulfur, mercury, antimony
Discovered how to make acids

9. Robert Boyle Robert Boyle (1627-1691)
Recognized importance of careful measurements
Properties of gases
Science should be firmly grounded in experiments
Element cannot be broken down into simpler substances

10. Relative Abundance
Nine elements account for about 98% of the earth’s crust, oceans and atmosphere.

11. The elements in living matter are very different from those in the earth’s crust.
In the human body, oxygen, carbon, hydrogen and nitrogen are the most abundant elements

12. Names and Symbols for the Elements
Each element has a name and a symbol
The symbol usually consists of the first one or two letters of the element’s name.
First letter capitalized, second letter lower case
Examples: Oxygen O Krypton Kr

13. Names and Symbols for the Elements
Sometimes the symbol is taken from the element’s original Latin or Greek name.
Examples: gold Au aurum lead Pb plumbum
tin Sn stannum
silver Ag argentum
mercury Hg hydrargyrum
iron Fe ferrum

14. Names and Symbols for the Elements
Each element has a name and a symbol.
Sometimes the name is taken from the element’s place of discovery
Examples: Francium Fr Germanium Ge
Sometimes the name is taken from a famous scientist
Examples: Einsteinium Es Curium Cm

15. JJ Thomson & William Thomson’s Atom
Discovery of the electron in 1897
Plum pudding model
Positively charged sphere with electrons scattered throughout

16. Rutherford’s Atom (11.1)
Showed nucleus was composed of protons and neutrons
Rutherford animation (large scale)
Rutherford animation (small scale)

17. Rutherford’s Experiment

18. Results of Rutherford’s Experiment
(a) The results that the metal foil
experiment would have yielded if the
plum pudding model had been correct
(b) Actual results

19. James Chadwick
Discovered the neutron

20. 3.2 – Atoms & compounds OBJECTIVES
To learn about Dalton’s theory of atoms
To understand and illustrate the law of constant composition
To learn how an isotope is written and the number of protons, neutrons and electrons are calculate
3.2 – Atoms & compounds

21. Law of Constant Composition
A given compound always contains the same proportion by mass of the elements of which it is composed
Examples:

22. Dalton’s Atomic Theory
All elements are composed of atoms.
All atoms of a given element are identical.
Atoms of different elements are different.
Compounds consist of the atoms of different elements.
Atoms are indivisible. Atoms are not created or destroyed in a chemical reaction.

23. Concept Check
Which of the following statements regarding Dalton’s atomic theory are still believed to be true?
Elements are made of tiny particles called atoms.
All atoms of a given element are identical.
A given compound always has the same relative
numbers and types of atoms.
IV. Atoms are indivisible.

24. Counting Atoms

25. Atoms Atomic number = number of protons Atoms are neutral (no charge)
Protons = electrons
Neutrons = atomic mass – atomic number

26. POGIL ACTIVITY – ISOTOPESHg

27. Key points of Isotopes
Key 1 –
Key 2 –
Key 3 –

28. Objectives Know the meaning of a chemical formula
Know the parts of the periodic table
Use the periodic table to identify elements

29. Formulas of Compounds Atoms shown by chemical symbol
Number of each type shown by a subscript to the right of the chemical symbol

30. Part of the Periodic Table

31. Objectives Identify and describe a cation and anion
Use the periodic table to predict the charge on a cation and anion

32. Cations Atoms that LOSE electrons More protons than electrons
Metals (groups 1 and 2)
Transition metals (groups 3-12)
Written as superscript after symbol

33. Metals Group 1 = +1 Group 2 = +2
Ex: sodium = Na+1
Group 2 = +2
Ex: magnesium = Mg+2
Transition metals have charges in parenthesis after name in Roman numerals
Ex: lead(II)

34. Anions Atoms that GAIN electrons More electrons than protons
Non-metals
Examples - sulfur, phosphorus, fluorine, etc
Group 17 = -1
Group 16 = -2
Group 15 = -3
Charge is written as superscript after symbol
Ex: Cl-1

35. Calculating Average Atomic Mass
Calculate the average atomic mass of sulfur given the following isotopes and their respective abundances:
Atomic mass % abundance
Sulfur-32:  071  %
Sulfur  458  %
Sulfur  866  %
Sulfur  080  %