Metals Chapter 19 Section 1. Interesting to know First metal used was gold about 6,000 years ago...
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Transcript of Metals Chapter 19 Section 1. Interesting to know First metal used was gold about 6,000 years ago...
MetalsChapter 19 Section 1
Interesting to know
• First metal used was gold about 6,000 years ago• Followed a few thousand years later by tin
and iron
Properties of metal
• Metals are found to the left of the stair-step line
• Metals usually have common properties such as:• Good conductors of heat and electricity• All but Hg is solid at room temperature• Reflect light (luster)• Malleable –can be hammered or rolled into
sheets• Ductile – drawn into wires
Properties of metal
• Types of bonds formed• Bonds are when elements form with other
elements to become new molecules• Often Ionic bonds are formed between metals
and nonmetals• Metallic bonding – outer electrons are not held
tightly – (this form of bonding explains some properties of metals)
Alkali Metals
• Group 1 of periodic table
• Most reactive of all metals – react rapidly and sometimes violently
• Don’t occur in nature in their elemental form• Stored in substances that are unreactive
• Has one electrons in its outer electron cloud
Radioactive Elements
• Definition – element in which the nucleus breaks down and gives off particles and energy • Example would be the last element in group 1
Francium
The Alkaline Earth Metals
• Group 2 of periodic table
• Combine readily with other elements
• Two electrons in outer energy level
• Some used in fireworks – ex. Magnesium
Transition Elements
• Transition elements are those elements in group 3 through 12 in the periodic table.
• These are considered to be elements in transition between groups 1 and 2 and Groups 13 through 18.
• Transition elements are the most common types of typical metals
• Often occur in nature as uncombined elements.
Iron Triad
• Consists of Groups 8,9, and 10 that start with Iron, Cobalt, and nickel
• All used in the process to create steel and other metal mixes
• Iron – main component of steel – most widely used of all metals
• Nickel – added to steel to give strength
Coinage Metals
• Copper, silver, gold – Group 11
• Stable and malleable
• Found as elements in nature
• Copper used in wiring because of its superior ability to conduct electricity and its relatively low cost.
• Gold and silver are very resistant to corrosion and are attractive in color and thus used in jewelry.
Mercury - Hg
• Mercury is a silvery, liquid metal – the only metal that is liquid at room temperature.
• Used in thermometers, some temperature sensitive switches and some batteries
• Poisonous
• “Mad as a hatter” -- used mercury in hats
Inner Transition Metals
• Lanthanides – used very extensively in the motion picture industry and to help produce colors on your tv screen
• Actinides – all radioactive and unstable• Uranium is best known for its use in nuclear
reactors and in weapons applications
Metals in the Crust
• Most metals in earth’s crust are found as ores
• Ores are metal compounds that have formed a mixture with the rock or clay in the earth.
NonmetalsChapter 19 Section 2
Properties of Nonmetals
• Usually gases at room temperature or very brittle solids
• Not malleable or ductile
• Bad conductors
• Not shiny
• Right side of Staircase line (other than hydrogen)
Properties of nonmetals
• Type of bonding• Can form ionic or covalent bonds
Hydrogen
• 90 percent of all atoms in the universe are hydrogen (most found as water)
• Formed from Greek word meaning “water forming”
• Hydrogen at its elemental form is a gas at room temperature
• Hydrogen is found usually as a diatomic molecule (which means it consists of two atoms of the same element in a covalent bond)
• H is highly reactive because it only has a single electron that it shares when it combines with other nonmetals.
• H can gain an electron when it combines with alkali and alkaline earth metals.
The Halogens
• Very reactive
• Seven electrons in outer energy level and only need one electron to complete this energy level.
• If a halogen gains an electron from a metal it will form an ionic compound called a salt.
• Some uses:• Chlorine – disinfecting water• Iodine – important in our diet – also used to
disinfect skin before surgery
Noble gases
• Exist as isolated atoms
• Stable because their outermost energy levels are full.
• Never occur as compounds in nature.