Metallic Bonds and the Properties of Metals

What is the basis of a metallic bond?

• the attraction of neutral metal atoms.
• the attraction between protons and neutrons.
• the attraction between positive metal ions and interlocking electrons.
• the attraction between positive metal ions and free floating electrons.

There are more metals than non metals in the periodic table.

• True
• False

At room temperature, most metals are

• liquid
• solid
• gas
• an alloy

What does malleable mean?

• able to be shaped
• will break easily
• can be used for wire
• is shiny

Which of these is NOT an alloy?

• bronze
• copper
• brass
• stainless steel

Electrons that are free to move in metals

• delocalized electrons
• oxidation number
• chemical bond
• salts

What is the ability of a substance to be pulled into a thin strand?

• Malleability
• Ductility 
• Conductivity
• Solubility

Why do metals have high melting points?

• They don't
• The negatively charged electrons act as a glue to hold the positively charged ions together.
• All the electrons become delocalised

Why do metals conduct

• They are shiny
• The electrons are held tightly within the lattice
• The electrons are delocalised and able to move
• The electrons are shared between two metal ions

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

• Size of atoms gets smaller

• Attraction force between nuclei and free electron increases

• Increased space between the valence electrons in the "sea"

• Increased number of valence electrons contributed to the "sea"

Tags

NGSS.HS-PS1-1