Metallic Bonding

Electrons that are free to move in metals

• delocalised electrons

• oxidation number

• chemical bond

• salts

Tags

NGSS.HS-PS1-3

NGSS.HS-PS2-5

In metals, the _______ electrons form a shared sea of electrons.

• Metallic

• Inner

• Outer

• Ionic

Properties of metallic compounds include:

• brittle, conducts electricity (aqueous state), high melting points

• usually gas or liquid, relatively low melting points, does not conduct electricity

• shiny, malleable, ductile, conducts electricity, usually a solid

In general, what can be said of the melting points of metals?

• They are low.

• They are high.

• They are lower than nonmetals.

• They do not have melting points.

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

X is a solid at room temperature.

X has a high melting point.

Solid X conducts electricity.

Which diagram shows how the particles are arranged in solid X?

• 
• 
• 
• 

Tags

NGSS.MS-PS1-1

An alloy is harder than its pure metal because the foreign atoms in the alloy

• increase the bond strength between the atoms.

• increase the empty spaces between the atoms.

• react with the pure metal atoms to form a compound.

• reduce the ability of the atoms to slide across each other.

Describe the main features of metals in terms of their structure

• Positive metal ions arranged in layers with delocalised electrons

• Negative metal ions arranged in layers with delocalised electrons

• Positive non-metal ions arranged in layers with delocalised electrons

• Negative non-metal ions arranged in layers with delocalised electrons

Tags

NGSS.HS-PS1-3

Explain why metals can conduct electricity

• Delocalised ions are free to carry charge

• Delocalised electrons are free to carry charge

• Delocalised electrons are not free to carry charge

• Delocalised ions are not free to carry charge

Tags

NGSS.HS-PS1-3

NGSS.HS-PS2-5

Explain why pure metals are soft

• The metals ions are only small

• Weak forces between metal ions

• Layers of metal ions are free to slide over each other

• Metals have high melting points

Explain why alloys can be harder than pure metals

• Because they have a higher melting point

• Because they are heavier than pure metals

• Different size of atoms disturb the layers to stop them sliding over each other

• Different size of atoms have a stronger force of attraction