Properties of ionic, covalent and metallic bonding

A mixture of two or more metals is called:

• mixture
• solution
• compound
• alloy

Which of the following is an alloy?

• sterling silver
• chromium
• nickel
• lead

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.

Which of these is NOT an alloy?

• bronze
• copper
• brass
• stainless steel

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

• delocalized electrons
• oxidation number
• chemical bond
• salts

Tags

NGSS.HS-PS1-3

Why are metals malleable?

• They are shiny

• The electrons are held tightly within the lattice structure making it strong

• The electrons are delocalized and able to move between the atoms

• The electrons are shared between two metal ions and this holds the atoms together

Tags

NGSS.HS-PS1-3

Why do metallic compounds conduct electricity as solids?

• core electrons are mobile, allowing electricity to flow through the metal

• valence electrons are mobile, allowing electricity to flow through the metal

• protons are mobile, allowing electricity to flow through the metal

• the metal cations are mobile, allowing electricity to flow through the metal

Tags

NGSS.HS-PS1-3

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.HS-PS1-2

Why are alloys generally used to make everyday objects?

• Alloys are often stronger and less active than pure metals.
• Alloys have higher melting point than pure metals.
• Alloys are less expensive to produce than pure metals.
• Alloys have ionic bonds instead of metallic bonds.

Tags

NGSS.HS-ETS1-3