The Modern Periodic Table
Jan 20, 2016
The Modern Periodic Table
Early Periodic Table – Atomic Number
• In 1913 Henry Mosley discovered that each element contained a unique number of protons in the nuclei
• Arranged elements in order of atomic number.
• Resulted in a clear periodic pattern of properties.
Periodic Law
• There is a periodic repetition of chemical and physical properties of elements when arranged in increasing atomic number (increasing number of protons) called the periodic law
Modern Periodic Table• Organized in columns called groups or families• Rows are called periods• Group A – representative elements (1A-8A)• Group B - transition elements (1B-8B)
Transition Elements (Group B)
Representative Elements
(Group A)
Representative Elements (Group A)
Classification of Elements
• Three classifications for elements metalsmetals, nonmetalsnonmetals, and metalloidsmetalloids (semimetalssemimetals).
Metals
• Properties of Metals – shiny, smooth, solids (except mercury)–Good conductors of heat and electricity–High densities–High melting and boiling points –Malleable – bended or pounded into sheets–Ductile – drawn into wires
Groups of Metals
• Alkali metals – group 1A except H• Alkaline earth metals – group 2A– Alkali metals and alkaline earth metals are
chemically reactive
• Transition metals – group B elements• Inner transition metals – Lanthanide– Actinide
Transition Metals (B group elements)
Alkali MetalsAlkaline Earth
Metals
Inner Transition Metals
Metals
Organizing by Electron Configuration
• Group number for group A elements represents the number of valence electrons
• Atoms in the same group have similar chemical properties because they have the same number of valence electrons
Alkali Metals• Electron configurations for alkali metals• Lithium 1s22s1
[He]2s1
• Sodium 1s22s22p63s1 [Ne]3s1
• Potassium 1s22s22p63s23p64s1 [Ar]4s1
• Rubidium 1s22s22p63s23p64s23d104p65s1[Kr]5s1
• What do the four configurations have in common?
• They have a single electron in their outermost energy level
• They all have one valence electron, thus similar chemical properties
Alkaline Earth Metals
• Electron configuration for alkaline earth metals• Beryllium [He]2s2
• Magnesium [Ne]3s2
• Calcium [Ar]4s2
• Strontium [Kr]5s2
• All alkaline earth metals have two valence electrons, thus similar chemical properties.
Question Time
• What are representative elements?• What are Group B elements called?• What are the three classifications for elements?• What are the characteristics of metals?• Where are the alkali metals and alkaline earth metals
located?• Where are transition metals located?• What are the inner transition metals?• How many valence electrons do alkali metals and
alkaline earth metals have?
Nonmetals
• Gases or brittle, dull looking solids• Poor conductors of heat and electricity• Usually have lower densities, melting point,
and boiling point than metals.• Groups of nonmetals– Halogens 7A– Noble gases 8A
sulfur
Noble Gases
Halogens
Nonmetals
Noble Gases
• Noble gases – Group 8A• Called inert gases because they rarely take part in a
reactionHe – 1s2
Ne – 1s22s22p6
Ar – 1s22s22p63s23p6
Kr - 1s22s22p63s23p63d104s24p6
• Because noble gases have completely filled s and p sublevels, they do not react with other elements
Metalloids (Semimetals)• Physical and chemical properties similar to both
metals and nonmetals– They are metallic-looking brittle solids– Relatively good electrical conductivity.
• Used in glasses, alloys, and semiconductors• The six elements commonly recognized as metalloids
are boron, silicon, germanium, arsenic, antimony, and tellurium. Polonium and astatine are sometimes classified as metalloids
Metalloids (Semimetals)
Question Time
• What are the properties of nonmetals?• Where are halogens and noble gases found?• Why are noble gases unreactive (inert)?• What are the properties of metalloids
(semimetals)?• Which six elements are most commonly
known as metalloids (semimetals)?