Chemistry- metals.

Why do the delocalised negative electrons stick to the metal ions

Metallic bonding- the metal ions are positive and the delocalised electrons are negatively charged, creating an electrostatic attraction between them. This attraction is very strong.

Why are Alloys harder than metals

Alloys are harder than pure metals due to the presence of different sized atoms, which stops the layers of atoms from sliding easily over one another, like they do in pure metals. Pure metals are malleable.

Metal Oxygen reaction

Metal + Oxygen = Metal Oxide

Displacement reactions

A type of chemical reaction where one more reactive metal displaces a less reactive one in a compound. e.g. magnesium displaces zinc , but iron wouldn’t.

Metal water reaction

Metal + Water = Metal Hydroxide + Hydogen

salts

Metal + acid = salt + hydrogen

what happens when magnesium reacts with water

When magnesium reacts with 1 Cold Water: Magnesium reacts very slowly with cold water. You might notice a few bubbles forming on the surface of the magnesium, but it won't be very vigorous.
2 Hot Water: When magnesium is exposed to hot water or steam, the reaction is much more vigorous. While magnesium does react with water, it's significantly less reactive compared to other metals like sodium or potassium.

what is the difference between Metals and Alloys

Metals are pure elements that possess good electrical conductivity, malleability, and ductility. They have a structure that enables the layers of atoms to slide over each other, making them malleable. Alloys, on the other hand, are mixtures made from two or more elements, at least one of which is a metal. They are usually stronger and harder than pure metals, due to the different sized atoms which disrupt the layers’ ability to slide, thus making them less malleable.

magnesium and water solution ph

The solution is slightly alkaline with a ph of around 10. this means its basic.

rust=

Iron + water + oxygen = rust

Properties of pure metals

Properties of pure metals:
1. Good electrical conductivity - Pure metals allow electric current to flow through them easily. 2. Good thermal conductivity - They efficiently conduct heat. 3. Malleability - Pure metals can be hammered or rolled into thin sheets without breaking. 4. Ductility - They can be drawn into wires without breaking. 5. Luster - Pure metals have a shiny appearance when polished. 6. High density - Most pure metals are dense and heavy for their size. 7. High melting and boiling points - They tend to have high temperatures at which they change state.

properties of alloys

1. Strength - Alloys are generally stronger than pure metals due to the presence of different sized atoms which disrupts the ability of layers to slide over each other. 2. Durability - They often exhibit greater resistance to corrosion and wear. 3. Lower melting points - Alloys can have lower melting points than pure metals, making them easier to cast and work with. 4. Enhanced physical properties - Alloys can be tailored for specific qualities, such as improved toughness, hardness, or flexibility. 5. Variable conductivity - Electrical conductivity can vary in alloys compared to their component metals, as the addition of other elements can impact how easily electrons flow. 6. Aesthetic qualities - Some alloys are designed to have attractive appearances, such as stainless steel and certain bronze alloys.