PERIODIC TABLE OF ELEMENTS NOTES

Atoms vs. Ions

Atoms = same number P+ & E-

Ex: (+3) + (-3) = 0 charge is ZERO

Ions = same # P+, …but more or less E-

Ex: (+3) + (-4) = -1 Ex: (+3) + (-2) = +1 Charge is (+ or -)

*sodium ion laser is used to determine the temperature in the mesosphere and the lower thermosphere

Ions: What and Why? An Ion is an atom with a + or -

charge *Cation = ion with + charge *Anion = ion with - charge

Goal: fill outermost shell (Octet Rule) Ex. Na = 11 electrons (7 more until full

shell) Na+1 = 10 electrons (outermost shell full)

Valence Electrons (outermost shell electrons) are used for bonding

Essential Question:What are the different groups of elements and how are they organized in the Periodic Table?

Quick Electron Lesson Electrons are found in the energy levels. Electrons affect the properties of elements Remember atoms have a ZERO CHARGE If an atom has a charge ONLY affects

ELECTRONS # P+ ≠ #E-

If Positive (+) charge, TAKE AWAY electrons If Negative (-) charge, ADD ON electrons

Organization

How to organize elements? Early scientists used the properties of

elements to sort them into groups. Elements are arranged in order of increasing

atomic number.

How It Works

Rows (across) = PERIODS Goes in order of ATOMIC

NUMBER Determines # energy

levels Elements within a period

= PROPERTIES CHANGE

Periodic law: the pattern of properties within a period repeats as you move from one period to the next

How It Works Columns (up and down) = GROUPS or FAMILIES

Determines the # valence electrons Elements within a group = SIMILAR PROPERTIES

3 Broad Classes of Elements

Metals

Nonmetals

Metalloids

“Staircase”

3 Broad Classes of Elements

1. Metals: Good Conductors High Luster or Sheen (Shiny) Ductile Malleable

2. Nonmetals: (Opposite of metals)3. Metalloids: Act as a metal or

nonmetal

Metallic Trend Most metallic elements are Cesium

(Cr) and Francium (Fr)

In your journal, outline the periodic table and include the trends.

Main Groups1. Alkali Metals2. Alkaline Metals3. Transition Metals4. Metalloids5. Nonmetals6. Halogens7. Noble Gasses8. Lanthanides9. Actinides

Group 1: Alkali Metals“The Alkali Boys”

Except Hydrogen Traits:

1 valence electron Lose valence electron +1

charge VERY REACTIVE

(Almost) always bonds with halogens

Brothas:

Group 7: Halogens“The Halogen Girls”

Common Salts: Chlorine (Cl) Bromine (Br) Iodine (I)

Traits: 7 valence electrons Gains 1 valence electrons -1

charge VERY REACTIVE

Almost awalys bonds with Alkali brothas

Sistas:

Why They Make Such a Cute Couple…Reason for Bonding

Goal: To settle downMeet the OCTET RULE

Valence electrons = bondingAlkali Brothas = 1 valence

electronHalogen Sistas = 7 valence

electrons

In Addition…Charge

No Charge = No Drama!

Alkali (Sodium) = +1 charge

Halogens (Chlorine) = -1 charge

NaCl = (+1) + (-1) = 0

Elbow Partner

What charge do alkali metals have? Halogens?

What are valence electrons?

Why do alkali and halogens go so well together (two reasons)?

Group 2: Alkaline Earth Metals “Players”

Traits: 2 valence electrons Loses 2 valence electrons

+2 charge (Almost) always bonds

with TWO halogen sistasOR 1 Group 6 nonmetal

Playas:

Group 8: Noble Gases“The Snobs” Traits:

8 valence electrons (Octet Rule) NO CHARGE (no

drama) NOT REACTIVE

Bonds with NO ONE Too good for anyone

else.

The Snobs:

In between Groups:Transition Metals

Scandium to Zinc Zinc to Mercury Found in middle of

table Ones in each column

= similar properties Different charges Some are synthetic Inner Transition

Metals Lanthanides and

Actinides Rare Earth Elements

Elbow Partner

What do metalloids separate (what are the found between)?

Why are the noble gasses “snobs?”

Describe the traits of alkaline earth metals (charge, number of valence electrons).