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Explore the Periodic Table's organization with its 7 periods, 18 columns, and diverse element groups from metals to metalloids and non-metals. Learn about atomic radius, ionization energy, and elemental properties as they vary systematically based on atomic number and electron configuration. Uncover the reactivity of alkali metals, alkaline earth metals, transition elements, noble gases, halogens, and mixed groups like the Boron and Carbon groups. Discover the unique characteristics of elements like Hydrogen, Metalloids, and the Iron Triad. Dive into the world of chemical elements and their distinctive roles in the universe.
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P. Sci. Unit 8 Periodic Table Chapter 5
Atomic Radius Periodic Law Electro-negativity • Properties of elements tend to change in a regular pattern when elements are arranged in order of increasing atomic number, or number of protons in their atoms. Atomic mass Density Ionization Energy
Periodic Table The periodic table is arranged in- • Periods (horizontal) rows • There are 7 periods • Groups families (vertical) columns • There are 18 columns
Metals all elements on the left side of the table (except Hydrogen) Non - Metals all elements on the right side of the table
Hydrogen • Hydrogen (1) – 90% of the atoms in the universe – (diatomic – two atoms of the same element in a covalent bond – H,N,O,F,Cl,Br,I). Very reactive, both covalent and ionic bonds can form
Metalloids • elements that share both metal and non-metal characteristics – the elements on both sides of the stair-step line except aluminum. • Also called semiconductors
H hydrogen Alkali Metals • (Column 1 except Hydrogen) – the most reactive group – do not occur in nature in their elemental form. Has one electron in its outer energy level • All (including hydrogen) have 1 valence electron.
Alkaline Earth Metals • (Column 2) – also reactive – also do not occur in nature alone (fireworks) • 2 valence electrons. Li Na K Rb
Transition Elements • (Columns 3 – 12) stable metals – occur in natural state. • usually have 2 – 3 valence electrons to give up to form bonds.
Mixed groups • Boron group (13) – mixed with both metals and non-metals. • 3 valence electrons
Mixed groups cont. • Carbon group (14) – mixed with both metals and non-metals. • 4 valence electrons
Mixed groups cont. • Nitrogen group (15) – mixed – tend to share to form covalent bonds – fertilizers. • 5 valence electrons
Mixed groups cont. • Oxygen group (16) – mixed • 6 Valence electrons
Halogens • (17 – all nonmetal) – very reactive in their element form. If combined with a metal forms salt. Many are diatomic (F,Cl,Br) Br – only nonmetal liquid. • 7 valence electrons
Noble Gases • (18)– Most stable because outer layer is full. No known natural compounds. Helium gas, neon / argon in neon lights, argon / krypton in electric light-bulbs, used to produce lasers • 8 valence electrons (full shell)
Other Groups • Iron Triad – Iron, Cobalt, and Nickel – create steel and other metal mixtures.
Other groups cont. • Coinage group – Copper, Silver, and Gold – stable and malleable and found in nature – used to make coins.
Other groups cont. • Coating metals / Zinc group – Zinc, Cadmium, and Mercury – used to coat or plate other metals – Mercury only liquid metal (cadmium and mercury used in batteries.)
Other groups cont. • Lanthanide series – elements 58 – 71 • Actinide series – elements 90 – 103 • Transuranium – all elements over 92
Allotropes • (recall isotopes) – materials made of the same element that have different molecular structure. Diamonds Graphite
Thats All folks
