Metallic Bonds

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.

At room temperature, most metals are

• liquid
• solid
• gas
• an alloy

Tags

NGSS.MS-PS1-4

What does malleable mean?

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

Electrons that are free to move in metals are called... ?

• delocalized electrons

• oxidation number

• chemical bond

• salts

Tags

NGSS.HS-PS2-5

Which of these is NOT an alloy?

• bronze
• copper
• brass
• stainless steel

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

• Malleability
• Ductility 
• Conductivity
• Solubility

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

Tags

NGSS.HS-PS1-3

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 outer electrons in the "sea"

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

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

How are compounds with metallic bonds similar to ionic compounds?

• Both tend to have double and triple bonds.

• Both tend to have low boiling point

• Both tend to have poor conductivity.

• Both tend to have high melting points.

Tags

NGSS.HS-PS1-3

What are the delocalised electrons in metallic bonds attracted to?

• Positively charged ions inside of the metal

• Positively charged ions outside of the metal

• Negatively charged ions inside of the metal

• Negatively charged ions outside of the metal.