1. Atoms, Bonding and the Periodic Table
Chapter 5, Section 1

2. Key Concepts
How is the reactivity of elements related to valence electrons in atoms?
What does the periodic table tell you about atoms and the properties of elements?
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3. Key Terms Valence electrons Electron dot diagram Chemical bond Period
Group
Family
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Say the terms out loud
Identify words that they are most familiar with

4. Electrons and Energy Levels
Where are electrons found?
Neils Bohr suggested:
Electrons have specific amounts of energy leading them to move in specific orbits around the nucleus of the atom
Resemble planets orbiting around the sun or like the layers of an onion
HowStuffWorks "How Atoms Work"science.howstuffworks.com -

5. Cloud of Electrons
In the 1920’s scientists determined that electrons do not orbit the nucleus like planets but rather in a cloudlike region.
This region is where electrons are likely to be found.
An electron movement is related to its energy level or specific amount of energy it has.
Visualizing an electron cloud: electric or battery operated fan
Show students that when the fan is off they can clearly distinguish each blade. Then turn it on and ask, “How would you describe the blades?”
Like a blur – possible answer
Ask, How are the electrons in a “cloud” of electrons like the blades of the fan?”
Electrons in a cloud move in such a way around the nucleus that it is impossible to identify their positions

6. Valence Electrons
Electrons that have the highest energy levels and are held most loosely are known as the atom’s valence electrons.
The number of valence electrons in an atom of an element determines many properties of that element, including the ways in which the atom can bond with other atoms.
Second bullet – very important

7. Electron Dot Diagram
Each element has a specific number of valence electrons, ranging from 1 to 8.
An electron dot diagram includes the symbol for the element surrounded by dots. Each dot stands for one valence electrons.
Identifying electrons can be done with an electron dot diagram
Turn to page 13 in your book – look at figure 9
Draw a picture of on of the diagrams of figure 9 in your book.
Please note that you can place the first two dots on any side, but the rest of the dots should be placed in either a clockwise or counter clockwise manner, with no side receiving two dots until each side gets one .
By looking at the electron dot diagram for oxygen we can see that oxygen has two unpaired electrons, so it has two electrons available for standard covalent bonds. Oxygen
Chlorine Electron Dot Notation is the shorthand method by which chemists portray the quantity of valence electrons that any given element may contain.

8. Quick Review: Chemical symbol Atomic number Period Group or Family
One or two letters that represents an element.
Atomic number
Number of protons in the nucleus of an atom.
Periodic table is arranged in order of increasing atomic number
Period
Row of elements across the periodic table
Group or Family
Elements in the same column

9. Chemical Bonds and Stability
How is the reactivity of elements related to valence electrons in atoms?
Most atoms are more stable – less likely to react – when they have eight valence electrons.
What are some examples of elements that are stable?
Neon, argon, krypton, and xenon
Small atoms such as helium are stable with just two valence electrons – which is why it is found in group 18, noble gases
Key concept question
Examples: neon, argon, krypton, and xenon all have eight valence electrons and are vey unreactive – they do not easily form compounds. Some small atoms such as helium are stable with just two valence electrons – which is why it is found in group 18 – noble gases.

10. How can an atom react to become more stable?
Two ways:
Either the valence electrons increases to eight (or two in the case of hydrogen)
Atom gives up loosely held valence electrons
Atoms that react this way become chemically combined or bonded to other atoms – chemical bond.
Chemical bond is the force of attraction that holds two atoms together.

11. Chemical Bonds and Chemical Reactions
Chemical bonds may occur two ways:
Electrons may be transferred from one atom to another.
Electrons may be shared between the atoms.
In both cases a chemical reaction takes place and a new substance is formed.
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12. How is the periodic table organized?
Organized by atomic number
If you know the atomic number, what else do you know?
The periodic table gives you information about the arrangement of electrons in atoms.
How do the atoms change from left to right across a period, or row?
As the number of protons – or atomic number increases, the number of electrons also increases.
As a result, the properties of the elements change in a regular way across a period.
A period ends when the number of valence electrons reaches 8 (except for period 1)
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13. Reading the Periodic Table
What happens when you get to the next period?
It will begin with atoms having higher energy.
The repeating pattern means that the elements within a group, or column, always have the same number of valence electrons.
View the periodic table on page 152 and the electron dot diagrams on page 153.
What pattern do you see?

14. Patterns of Valence Electrons
Elements in groups 3-12 follow a slightly different pattern.

15. What does the periodic table tell you about the properties of elements?
The elements within a group have similar properties because they all have the same number of valence electrons in their atoms.

16. Noble Gases Noble gases Group 18 Have 8 valence electrons
Except for Helium which only has 2
They do not react easily with other elements – they are stable
Chemists have been able to make noble gases form compounds with a few other elements.

17. Reactive Nonmetals and Metals
Group 17
Name of the group
Halogens
How many valence electrons do they have?
Seven
Will they gain electrons or lose electrons?
Gain or share electrons
As a result, they will react easily with other elements whose atoms can give up or share electrons.
Which group would these elements be found in?

18. What group are alkali metals found?
Do alkali metals gain or lose electrons?
Alkali metals become chemically more stable by losing their one valence electron
This property makes the alkali metals very reactive
Which group could these atoms lose their electrons to?
Halogens – group 17
Seven valence electrons, just one more electron gives these atoms the stable number of eight electrons, like the noble gases
For example, sodium chloride
Sodium has 1 valence electron
Chlorine has 7 valence electrons
Alkaline Earth metals, lose electrons easily and are almost as reactive as the Alkali metals.

19. Other metals How reactive a metals is, depends on what key factor?
Depends on how easily its atoms lose valence electrons.
Groups 2-12 are metals, like group 1
Most have 1, 2, or 3 valence electrons
They react by losing these electrons, especially when they combine with oxygen or one of the halogens.
Elements in group 2 thru 12 are metals
Platinum (Pt) and gold (Au) are unreactive
Mercury (Hg) is the only metal that is a liquid at room temperature
All the other metals are solids, although gallium (Ga) melts just above room temperature

20. Which of the nonmetals are solid at room temperature?
Carbon (C), phosphorus (P), sulfur (S), selenium (Se), and iodine (I)
Which nonmetal is the only liquid?
Bromine (B)
Like the halogens, nonmetals may become stable by gaining or sharing electrons
Of the nonmetals, only oxygen and the halogens are highly reactive.
Is hydrogen a metal or a nonmetal?
It is considered a nonmetal. It is in group 1 only because it has one valence electron. Hydrogen’s properties differ greatly from the alkali metals

21. Where are the metalloids found on the periodic table?
Along the zig zag line between the metals and nonmetals
How many valence electrons do metalloids have?
Three to six
Do the metalloids gain, lose, or share electrons?
They can either lose or share electrons when they combine with other elements.