The metallic model - s & p block elements Flashcards
What determines the strength of metallic bonds?
Several factors including the charge on the metal ion, the radius of the metal ion, number of delocalised electrons, and the number of positive charges on the metal centres.
How does the charge on the metal ion affect metallic bond strength?
A greater charge on the metal ion increases the number of electrons in the sea of delocalised electrons and enhances the charge difference, leading to stronger electrostatic attraction.
What trend is observed in melting points of metals across a period?
The melting point of metals increases moving from left to right across a period.
How does the radius of the metal ion influence metallic bond strength?
Smaller ionic radii exert a greater attraction on delocalised electrons, leading to stronger metallic bonds.
What trend is observed in melting points of metals down a group?
The melting point of metals decreases moving down a group.
What factors can increase the strength of electrostatic attraction in metallic bonds?
Increasing the number of delocalised electrons, increasing positive charges on metal centres, and decreasing the size of metal ions.
What is the electron configuration of sodium?
1s2 2s2 2p6 3s1
What is the electron configuration of magnesium?
1s2 2s2 2p6 3s2
What is the electron configuration of aluminium?
1s2 2s2 2p6 3s2 3p1
How does the size of the cation affect melting point as you go down a group?
The increase in cation size decreases the attraction between outer electrons and the metallic lattice, leading to a reduction in melting point.
True or False: The stronger the metallic bonding, the less energy is needed to break the metallic lattice.
False
Fill in the blank: The melting point of metals ________ moving across a period.
increases
Fill in the blank: The melting point of metals ________ moving down a group.
decreases
Which three elements in Period 3 have metallic bonding?
Sodium, Magnesium, Aluminium
