1. GROUPS/Families & VALENCE ELECTRONS
CHAPTER 5.3

2. Elements in a _____ have the same number of electron shells or energy levels.
Elements in a _______ or “family” have similar properties.

3. Why do the elements in a group have similar properties?
Valence electrons
Why do the elements in a group have similar properties?

4. Why do the elements in a group have similar properties?
Valence electrons
Why do the elements in a group have similar properties?
They have the same number of ___________________
The properties are not identical because the valence electrons are in __________ energy levels.
A valence electron is an electron that is in the ____________ occupied energy level of an atom.
_________ most electron shell

5.  Electrons Filling shells as atomic # increases
(# of electrons goes up as # of protons goes up): Be H He Li B
1st shell now
full, start 2nd
Atomic # 1 2 3 4 5
Valence e’s Na C N Ne 6 7
Atomic #  10
2nd shell now
full, start 3rd 11
Valence e’s

6. Valence electrons How do we determine the number of valence electrons?
When groups in the periodic table are labeled as Series A and Series B:
For Series A (______________):
group _______ = the number
of valence electrons for an
element in that group.
Valence electrons play a key role in chemical reactions.
Properties vary across a period because the number of valence electrons _______________ from left to right.

7. Filled shell contains ____ electrons (octet)
Octet Rule
Atoms are most stable if their outer most electron shell is __________ or _____________.
Filled shell contains ____ electrons (octet)
Except for ____ and ____ (atomic #1 & #2)
Atoms gain, lose, or share valence electrons in order to fill or empty their outer shell
Atoms gain, lose, or share electrons based on what is _____________.

8. Octet Rule Na has 11 protons and 11 electrons. Period 3 = 3 e- shells
Group 1A = 1 Valance e-
2 e- in 1st shell (full)
8 e- in 2nd shell (full)
1 e- in 3rd shell (valence)
proton charge (11 x +1) = +11
+ electron charge (11 x -1) = -11
net charge = 0 (neutral)

9. Octet rule
When atoms lose or gain valence electrons  _________________
Na has 1 valence e- -- easier to _____1 than gain 7 to fulfill octet rule
leaves only 10 electrons
(2 e- in 1st shell; 8 e- in 2nd shell; 1 e- in 3rd shell)  (11 x +1)
(2 e- in 1st shell; 8 e- in 2nd shell; no e- in 3rd shell) (10 x -1)
= 1+
Example: Cl has 7 valence e- -- easier to _______1 than lose 7
(2 e- in 1st shell; 8 e- in 2nd shell; 7 e- in 3rd shell)  (17 x +1)
(2 e- in 1st shell; 8 e- in 2nd shell; 8 e- in 3rd shell) (18 x -1)
= 1-

10. Properties
Groups/Families

11. Group 1A – Alkali Metals 1 Valence Electron. Soft & Silvery
Extremely ________ (Most reactive Metals)
Found in nature only in compounds.
________ found free in nature
Mix well with water
The reactivity of alkali metals ___________ from the top of Group 1A to the bottom.

12. Group 1A – Alkali Metals
Sodium reacts violently with water and releases enough energy to ignite the hydrogen gas that is produced.
Unlike most metals Sodium is soft enough to cut with a knife.

13. Group 1A – Alkali Metals
Potassium (& Sodium)
Stored under oil to keep them from reacting with the oxygen and water vapor in air.
Cesium
So reactive that it is usually stored in a sealed glass tube containing argon gas.
Why argon?

14. Group 2A – Alkaline Earth Metals
2 Valence Electrons
Similar to Alkali Metals
_____ than metals in Group 1A
Higher melting points
The melting point of magnesium is 650°C; sodium 98°C
Almost as reactive as Alkali metals
_______ found free in nature
Reactivity increases
From top to bottom

15. Group 2A – Alkaline Earth Metals
Differences in reactivity among the alkaline earth metals are shown by the ways they react with _______.
No reaction occurs when beryllium is added to water.
Magnesium will react with hot water but not cold water.
Calcium, strontium, and barium react easily with cold water.

16. Magnesium Calcium Photosynthesis: Chlorophyll
Creates alloys stronger yet lighter than steel
Calcium
Oyster shell and a pearl - calcium carbonate (Ca, C, & O).
Also found in toothpaste
Plaster cast - calcium sulfate.
Oyster shell with pearl
Spinach plant

17. Group 3A – The boron family
____ Valence Electrons
Most are metals
Well-known metal – Al (aluminum)
Less familiar metals - Ga (gallium), In (indium), and Tl (thallium).
Boron is a _________

18. Group 3A – The boron family
Aluminum
Most abundant metal in Earth’s crust.
Less reactive than Na and Mg
Strong, lightweight, and malleable.
Good conductor of electric current.
Boron
B, Si, & O form a compound used to make glass that does not shatter due to rapid temperature change.
laboratory glassware
cookware that can go directly from the oven to the refrigerator.

19. Group 4A – The carbon family
____ Valence electrons
Family Contains
1 Nonmetal - C (carbon)
2 ____________ - Si (silicon) & Ge (germanium)
2 metals - Sn (Tin) & Pb (Lead)
Notice that the metallic nature of the elements __________ from top to bottom within the group. Germanium is a better conductor of electric current than silicon.

20. Group 4A – The carbon family
Except for water, most of the compounds in your body contain carbon.
Life on Earth would not exist without carbon.
Reactions that occur in the cells of your body are controlled by carbon compounds
Silicon
2nd most abundant element in Earth’s crust.
The clay used to produce pottery contains silicon compounds called silicates.

21. Group 5A – The Nitrogen family
5 Valence electrons
Can ______ electrons to form compounds
Family Contains:
2 nonmetals - N (nitrogen) & P (phosphorus)
2 metalloids - As (arsenic) & Sb (antimony)
1 metal - Bi (bismuth).
Group 5A includes elements with a wide range of _________ properties.
Nitrogen is a gas
Phosphorus is a solid nonmetal
Bismuth is a dense metal.

22. Group 5A – The Nitrogen family
When air is cooled - O condenses before the N due to its lower boiling point
Much of the N obtained from air is used to produce fertilizers.
The numbers on the bags of fertilizer are, from left to right, the relative amounts of nitrogen, phosphorus, and potassium.

23. Group 6A – The Oxygen family
___ Valence electrons
Family Contains:
3 ________ - O (oxygen), S (sulfur), & Se (selenium)
2 metalloids - Te (tellurium) & Po (polonium)
Reactive

24. Group 6A – The Oxygen family
Most abundant element in
Earth’s crust.
Complex life forms need O to
stay alive because O is used to
release the energy stored in food.
Ozone (O3) is another form of the element oxygen.
Sulfur
One of the first elements to be discovered because it is found in large natural deposits.

25. Group 7A – Halogens ___ Valence electrons All _______________
At room temperature:
chlorine is a gas,
bromine is a liquid
iodine is a solid.
___________ Reactive of the nonmetals
Often find these elements bonded with elements from Group 1A

26. Group 7A – Halogens
Despite their physical differences, the halogens have similar chemical properties.
React easily with most metals.
Image:
Chlorine reacting with steel wool 

27. Group 8A – the noble gases
8 Valence electrons = Full Shell – _______________
Helium (He) has only 2 valence electrons = Full
All Non-metals
Extremely Unreactive
________ and odorless

28. Group 8A – the noble gases
When electric current passes
through noble gases, they emit
different colors.
He (Helium) emits ______,
Ne (Neon) emits orange-red,
Ar (Argon) emits lavender,
Kr (Krypton) emits _______
Xe (Xenon) emits blue.

29. Assessment question
Why do elements in a group have similar chemical properties?
They have the same number of valence electrons.
They have the same ratio of protons to neutrons.
Their atomic masses are multiples of the least massive element of the group.
They have the same number of total electrons.

30. Assessment question
Which Group 2A element would you expect to react most readily with water?
beryllium (Be)
calcium (Ca)
barium (Ba)
radium (Ra)

31. Assessment question
3. In general, the metallic characteristics of within a period decreases from left to right.
True
False

32. Assessment question
4. Elements of the Nitrogen Family have a. 4 Valence electrons b. 6 Valence electrons c. 5 Valence electrons d. 7 Valence electrons

33. Assessment question
5. Atoms are most stable if their outer most electron shell is filled or empty. a. True b. False