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Physical Properties of Metals and Alloys - Coggle Diagram
Physical Properties of Metals and Alloys
Chapter 4.9
Explain the structure and bonding in metals?
Metals consist of giant structures of atoms arranged in a regular pattern. The electrons from the outer shells of the metal atoms are delocalised , and are free to move through the whole structure. This sharing of delocalised electrons results in strong metallic bonding .
Chapter 13.1
State 5 physical properties of metals. Explain the meaning of the terms malleable, ductile, sonorous, dense, conductor, insulator
They are strong, it hard to cut them
Malleable, they can hammed into shape without melting\breaking
Ductile, they could draw out into wire
Sonorous, ringing noise when you strike them
High density- they can feel “heavy”
The word explain
Malleable: describes the property of a metal's ability to be distorted below compression
Ductility: The ability of a material to be drawn or plastically deformed without fracture.
Sonorous: Giving sound when struck; resonant; as, sonorous metals.
Dense:A compact substance or a substance with a high density. conductor: is a material which contains movable electric charges insulator: is a material that has a large band gap, or a large energy difference between the valence and conduction band.
Explain why metals are malleable, ductile and can conduct electricity
Because of the ability of the atoms the roll over each other into new position without breaking the metallic bond
State 3 chemical properties of metals
React with dilute acid to form salts
React with oxygen to form oxides
Metals form positives ions when they react
The reactivity of metals in terms of electron loss
Explain the reactivity of metals in terms of electron loss
Metal reactivity relates to ability to lose electrons, form basic hydroxides, from ionic compound with non-metals. the greater the shielding, the greater the ability to lose electrons
Chapter 14.5
state the name of three alloys, giving an example of what elements each contains.
Aluminum: used for food cartons
Copper: used for electrical wires
Zinc: coated onto steel car bodies
explain why alloys are used instead of pure metals
Alloys are, for example, generally harder than pure metals. They are made up of atoms of different sizes, rather than being uniform. Alloys also tend to have better corrosion resistance than pure metals, and are more versatile for manipulating into different forms
Twrning a metal into an alloy changes its properties, and marked it more usedful.
compare alloys with pure metals and draw diagrams to explain the difference in properties
Pure metal vs Alloy
Pure metals consist of only one type of atom. For example, chromium is on the periodic table of elements, meaning it's a pure metal. An alloy, by contrast, is a mixture of different atoms melded together