32 questions
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"
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
Which of the following pairs of elements would NOT react to form an IONIC compound?
sulfur and phosphorus
sodium and iodine
iron and oxygen
aluminum and bromine
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.
Which of these are considered properties of metals? (choose ALL that apply)
brittleness
low melting point
luster (shininess)
malleability
ductility
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