Families of the Periodic Table of The Elements
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1 Families of the Periodic Table of The Elements
2 Families aka Groups
3
4 Groups Aka columns or families They are numbered from 1 18 (18 groups) groups numbers tell us how many valence electrons in the outer energy level. Elements in the same groups share chemical properties
5 What are valance electrons? The outer electrons of an atom The last electrons on the last energy level
6 How are valance electrons determined? They are determined by their group number Group 1= 1 valance electron If the element is in groups 11-18, drop the 1 so, 11 becomes 1 and has 1 valance electron, 12 becomes 2 and has 2 valance electrons and so on.
7 Helium has only 2 valance electrons
8 What do valance electrons determine for an atom? Valance electrons determine an atom/elements chemical properties like its reactivity Group one is the MOST reactive group! Group 18 (8 valance electrons) is the LEAST reactive group!
9 Families Show valence electrons
10 Groups have FAMILY NAMES
11 Group 1: Alkali Metals Contains: Metals Valence Electrons: 1 Reactivity: Very Reactive Properties: solids soft react violently with water shiny low density
12 Group 2: Alkaline-Earth Metals Contains: Metals Valence Electrons: 2 Reactivity: very reactive, but less reactive than alkali metals (Group 1) Properties: Solids Silver colored More dense than alkali metals
13 Groups 3-12 Transition Contain: Metals Metals Valence electrons: 1 or 2 Reactivity: less reactive than alkali and alkaline-earth metals Properties: Higher density Good conductors of heat and electricity
14 Groups 3-12 Transition Metals Below Main Table Contain: The Lanthanide and Actinide Series These two rows are pulled out of sequence and placed below the main table to keep the table from being too wide. Lanthanides are # s Actinides are # s
15 Groups 3-12 Rare Earth Elements ~ Lanthanides Contains: Transition Metals Valence electrons: 3 Reactivity: Very reactive Properties: High luster, but tarnish easily High conductivity for electricity
16 Groups 3-12 Rare Earth Elements ~ Actinides Contains: transition metals Valence electrons: 3 (but up to 6) Reactivity: unstable Properties: All are radioactive Most made in laboratories
17 Group 13: Boron Group Group 13: Boron Group Contains: 1 metalloid and 4 metals Valence Electrons: 3 Reactivity: Reactive Other shared properties: Solid at room temperature
18 Group 14: Carbon Group Contains: 1 non-metal, 2 metalloids, and 3 metals Valence Electrons: 4 Reactivity: Varies Other shared properties: Solid at room temperature
19 Group 15: Nitrogen Group Contains: 2 non-metals, 2 metalloids, and 1 metal Valence electrons: 5 Reactivity: Varies Other shared properties: All but N are solid at room temperature
20 Group 16: Oxygen Group Contains: 3 non-metals, 1 metalloid, and 2 metals Valence Electrons: 6 Reactivity: Reactive Other shared properties: All but O are solid at room temperature.
21 Groups 17 : Halogens Contain: Nonmetals Valence Electrons: 7 Reactivity: Very reactive Other shared properties Poor conductors of electric current React violently with alkali metals to form salts
22 Group 18 Noble Gases Contains: Nonmetals Valence Electrons: 8 (2 for He) Reactivity: Unreactive (least reactive group) Other shared properties: Colorless, odorless gases at room temperature Outermost energy level full All found in atmosphere
23 Hydrogen Stands Apart H is set apart because its properties do not match any single group. Valence electrons: 1 Reactivity: very, but loses the 1 electron easily Properties: Similar to those of non-metals rather than metals
24
25 Elements & Reactivity What makes an element reactive? Number of valence electrons each atom has When outer levels are full, atoms are stable. When they are not full, they react: gain, lose, or share 1 or 2 electrons.
26 Elements & Reactivity The most reactive metals are the elements in Groups 1 and 2. Elements in Group 1 need seven more electrons to fill their outer level. Elements in Group 2 need six more electrons to fill their outer level. These groups are known as the givers because they easily give up their valence electrons to make a compound.
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