The Periodic Table of the Elements Basic Organization

The Periodic Table of the Elements

Basic Organization Atomic structure is used to organize the elements in the periodic table. l Organized by atomic number l The periodic table is useful in predicting the chemical behavior, trends, and the properties on the elements. l 3 basic categories: l l Metals l Nonmetals l Metalloids

Atomic Structure Review l Atoms are made of protons, electrons, and neutrons. l Elements are atoms of only one type. l Elements are identified by the atomic number (# of protons in nucleus).

Energy Levels Review Electrons are arranged in regions around the nucleus called energy levels. l At least 1 energy level and as many as 7 levels exist in atoms. l Electrons in levels farther away from the nucleus have more energy. l Inner levels will first before outer levels. l

Energy Levels & Valence Electrons l Energy levels hold a specific amount of electrons: l l 1 st level = up to 2, 2 nd level = up to 8 3 rd level = up to 18 The electrons in the outermost level are called valence electrons. l l Determine how elements will react with others Outermost level does not usually fill completely with electrons.

Using the Table to Identify Valence Electrons Elements are grouped because they have similar properties. l Group numbers can help you determine the number of valence electrons: l l Group 1 has 1 valence electron. l Group 2 has 2 valence electrons. l Groups 3 – 12 are transition metals and have 1 or 2 valence electrons.

Using the Table to Identify Valence Electrons cont. l Groups 13 – 18 have 10 fewer than the group number. For example: l group 13 has 3 valence electrons l group 15 has 5 valence electrons l group 18 has 8 valence electrons

Grouping the Elements The most reactive metals are the elements in Group 1 and 2. l What makes an element reactive? l ● ● ● 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

Groups run vertically in the periodic table. l They are numbered from 1 – 18. l Elements in the same groups have the same number of electrons in the outer energy level. l Grouped elements behave chemically in similar ways. l

Group 1: Alkali Metals Contains: Metals l Valence Electrons: 1 l Reactivity: Very Reactive l Properties: l l solids l soft l react violently with water l shiny l low density

Group 2: Alkaline-Earth Metals Contains: Metals l Valence Electrons: 2 l Reactivity: very reactive but less reactive than alkali metals (Group 1) l Properties: l l Solids l Silver colored l More dense than alkali metals

Groups 3 -12 Transition Metals Contain: Metals l Valence electrons: 1 or 2 l Reactivity: less reactive than alkali and alkaline-earth metals l Properties: l l Higher density l Good conductors of heat and electricity

Groups 3 -12 Transition Metals Below Main Table (Inter transition Metals) l Contain: The Lanthanide and Actinide Series l These two rows are pulled out of sequence and placed below the main table to keep the table from being too wide. l Lanthanides are #’s 58 – 71. l Actinides are #’s 90 – 103.

Groups 3 -12 Rare Earth Elements ~ Lanthanides follow the transition metal # 57 Lanthanum in Period 6. l Valence electrons: 3 l Reactivity: Very reactive l Properties: l ● ● ● High luster but tarnish easily High conductivity for electricity Very small differences between them

Groups 3 -12 Rare Earth Elements ~ Actinides follow the transition metal # 89 Actinium in Period 7 l Valence electrons: 3 (but up to 6) l Reactivity: unstable l l All are radioactive l Most made in laboratories

Metalloids A zigzag line that separates metals from nonmetals l Elements from Groups 13 – 17 contain some metalloids. l l These elements have characteristics of metals and nonmetals.

Group 13: Boron Group l Contains: 1 metalloid and 4 metals l Valence Electrons: 3 l Reactivity: Reactive l Other shared properties: l l Solid at room temperature

Group 14: Carbon Group Contains: 1 non-metal, 2 metalloids, and 3 metals l Valence Electrons: 4 l Reactivity: Varies l Other shared properties: l l Solid at room temperature

Group 15: Nitrogen Group Contains: 2 non-metals, 2 metalloids, and 1 metal l Valence electrons: 5 l Reactivity: Varies l Other shared properties: l l All but N are solid at room temperature

Group 16: Oxygen Group Contains: 3 non-metals, 1 metalloid, and 2 metals l Valence Electrons: 6 l Reactivity: Reactive l Other shared properties: l l All but O are solid at room temperature.

Groups 17 : Halogens Contain: Nonmetals l Valence Electrons: 7 l Reactivity: Very reactive l Other shared properties l ● ● ● Poor conductors of electric current React violently with alkali metals to form salts Never found uncombined in nature

Group 18 Noble Gases Contains: Nonmetals l Valence Electrons: 8 (2 for He) l Reactivity: Unreactive (least reactive group) l Other shared properties: l l Colorless, odorless gases at room temperature l Outermost energy level full l All found in atmosphere l He, Ne, Ar, Kr, Xe, Rn

The Iron Triad Includes Fe, Co, and Ni l These have: l l thermal properties l high melting points l magnetic properties

Hydrogen Stands Apart H set apart because its properties don’t match any single group. l Valence electrons: 1 l Reactivity: very but loses the 1 electron easily l Properties: l l Similar metals to those of non-metals rather than

Periods continued Moving across from left to right across a period, each element has one more electron in the outer shell of its atom than the element before it. l This leads to a fairly regular pattern of change in the chemical behavior of the elements across a period. l

Periods run horizontally across the Periodic Table l Periods are numbered 1 – 7 l All the elements in a period will have the same number of energy levels, which contain electrons. Examples: l l Period 1 atoms have 1 energy level. l Period 2 atoms have 2 energy levels. l Period 5 atoms have 5 energy levels.