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the particles are very closely packed so the vibrations are passed on very quickly (kay, edell, joelle)

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electrons inside the metals are relatively free to move, so when electricity passes through metals, electrons carry electricity and spread it over the metal (kay, edell, joelle)

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metal's layers of ions can slide over each other, but are still held together by the delocalised electrons (kay, edell, joelle)

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Metals are malleable and they can be bent and shaped. This is because they consist of layers of atoms.

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metals are giant lattice structures, so the number of electrostatic forces to be broken is extremely large (kay, edell, joelle)

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There are free electrons that are available to move through the structure and carry a charge, and this causes electrons to flow so electricity is conducted.

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Metals are giant lattice structures, so the amount of electrostatic forces to be broken is larger since as it is high in density. So, more energy is needed therefore the higher the melting point and boiling point.

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The melting or boiling point rises as more energy is required. Metals have high melting and boiling temperatures because they have massive lattice structures and must break a huge number of electrostatic forces.

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Metals can be bent and shaped because they consist of layers of atoms that can slide over each other and keeping the structure

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Because the electrons inside metals are comparatively free to travel. They are highly permeable to free electrons, which makes it easier for the charge to be transferred from one item to another.

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Layers of positive ions can slide over one another and take up different positions, however, they are still held together by delocalised electrons. Metals are strong but flexible since they cannot be broken. They can be hammered and bent into different shapes as well as drawn into wires without breaking.

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their ductile and malleable because their atoms are able to move without breaking its bond, therefore making it ductile and malleable

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Metals have high densities, melting points, and boiling points due to their closely packed atomic and crystal structures, as well as the strong metallic bonding resulting from delocalized electrons. These factors lead to efficient packing of atoms, stable structures, and strong forces of attraction between atoms, making metals resistant to changes in their physical state and giving them high thermal and electrical conductivity.

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Because electrons move around freely and transfer heat from one area to another. Metals transmit heat so effectively, because they are more closely packed. Metal atoms are better to transmit heat.

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most metal conduct electricity because they have free electrons that's able to move freely carrying the electricity through out the metal

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Metals are ductile and malleable because of their unique atomic structure and metallic bonding. The presence of delocalized electrons allows metal atoms to easily slide past each other, making metals capable of being stretched into thin wires (ductile) and easily shaped into various forms (malleable).

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Metals can conduct electricity because they have a unique arrangement of their atoms. The electrons in metals are loosely bound and are allowed to move freely throughout the material. When an electric field is applied, these mobile electrons can easily flow from one atom to another, carrying the electric current along with them.

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Metals are giant lattice structures, which in turn needs a larger force of electrostatic forces to be broken. Metals also have strong metallic bonds that make them have a high boiling point.

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Metals conduct heat well because they have a high number of free electrons that are mobile within their atomic structure. When heat is applied to a metal, these free electrons move more quickly and collide with neighboring atoms, transferring thermal energy rapidly through the metal lattice.

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The Electrons in Metals relatively moves freely and transfer the heat from each other. The particles themselves are tightly packed, which enables them to transfer heat efficiently.

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They have high melting and boiling points as there are many strong metallic bonds between the positive metal ion and delocalised electrons in the lattice structure. A lot of heat energy is needed to break these bonds. Metals have high densities because their numerous atoms are tightly packed together in a small space.

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Metals are great at conducting heat because of their special structure that lets heat move through them easily. They have free electrons that can move around inside the metal and carry the heat energy with them.

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Metals conduct electricity because they have special free electrons that can move easily through them. When we apply a voltage, these electrons flow and carry the electric current.

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Metals are ductile and malleable because of their atomic arrangement and bonding, which allows the atoms to roll over each other into new positions without breaking the metallic bond.

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This is due to the strong metallic bonding in their atomic structure. This bonding involves the sharing of valence electrons among metal atoms, leading to a closely packed crystal lattice. The forces from this arrangement require significant energy to break, resulting in the thermal (BP and MP) and mechanical properties (High Density) characteristic of metals.

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This is because heat can be carried or transported from one part to another via the free movement of electrons in metals. The thermal energy can be carried by these electrons when they migrate from hot to cool regions of the metal. As they collide with their "neighbouring" electrons and transmit heat, delocalized electrons can transfer energy more quickly.

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Due to strong metallic bonding, metals have high density, melting, and boiling points positively charged ions and mobile electrons create a cohesive lattice. Close packing boosts strength. Strong electrostatic attraction necessitates a large amount of energy to break, resulting in high melting and boiling temperatures.

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Metals area malleable and can be bent because layers of atoms can slide over one another while maintaining the structure.

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Metals can carry electricity is because their electrons are almost free to travel. Therefore, when electricity passes through metals, electrons carry the electricity and disperse it throughout the metal.

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Metals conduct heat well due to their ordered lattice structure, which facilitates efficient energy transfer. Free electrons move through the lattice, transmitting heat rapidly. Vibrations from heating spread energy to neighboring atoms, creating a chain reaction.

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Metals can carry electricity because their electrons are generally free to travel. When electricity passes through metals, electrons transport the electricity and distribute it throughout the metal. Metals carry electricity due to the mobility of electrons.

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Heat may be moved from one location to another in metals due to the unrestricted mobility of electrons. These electrons can carry thermal energy when they travel from hot to cold parts of the metal. Heat is transmitted when electrons clash with other electrons nearby.