The Periodic Table Overview of Chapter 20.

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Presentation transcript:

The Periodic Table Overview of Chapter 20

Metals Metals- good conductors of heat & electricity. All but one (Hg) are solid at room temperature. Lustrous- reflect light Malleable- can be hammered or rolled into sheets, Ductile- can be drawn into wires Metals- have 1-3 valence electrons, so they lose electrons to become stable- they become cations Metallic bonding- positively charged metallic ions are surrounded by a cloud of electrons. Outer electrons are not held tightly and can move among the ions- allows conduction of electricity

Metallic bonding http://www.teachertube.com/viewVideo.php?video_id=155186

Metals Alkali- Group 1 A very reactive because they have 1 valence electron Alkaline earth- Group 2A- fairly reactive- have 2 valence electrons Transition elements- Groups 3-12 or 1B-8B, metals, often form colored compounds Lanthanides are elements after lanthanum and many are used to produce colors on our TV screens Actinides- follow actinium. All are radioactive and unstable, so they are difficult to research

Metals Elements beyond Uranium are radioactive- As # of protons increases, the repulsive force within the nucleus also increases- forces the atom to break apart. (Radioactive substances are substances in which the nucleus breaks down and gives off particles and energy )

Nonmetals Nonmetals- gases or brittle solids at room temperature. not malleable or ductile. do not conduct heat or electricity well not shiny Nonmetals don’t conduct electricity because- electrons are strongly attracted to the nucleus Gain electrons to form anions Can form either covalent or ionic bonds Covalent- shared electrons Ionic- gain and loss of electrons

Nonmetals Diatomic- molecule that consists of two atoms of the same element covalently bonded Includes (memorize these!!) H2 Cl2 F2 N2 O2 Br2 I2 Hydrogen is diatomic because it is very reactive. Bonding makes it more stable Halogens- nonmetals from group 7A or 17. very reactive. 7 valence electrons form reactive diatomic molecules with distinctive colors Noble gases- stable due to full outer energy levels. don’t make compounds naturally

Metalloid Metalloid- can form ionic or covalent bonds. properties of both metals and nonmetals Semiconductor- element that conducts electric current under certain conditions- like Silicon (Si is a metalloid)

Allotropes Allotrope- same element with different forms and different properties Example: Diamond and graphite Both are made of carbon. Diamond- clear, hard each C atom bonded to four other C atoms forming a giant crystal. Graphite- black powder with hexagonal layers of C atoms. Each C is bonded to 3 other C. Layers can slide past each other, so graphite is a good lubricant.

Diamond and graphite