18 Questions
What is the reason behind the increase in the size of ionic radii going down a group?
Increase in the number of shells of electrons
In covalent bonding, what does a dative covalent bond involve?
Sharing of electron pairs from one atom only
How many factors affect the strength of metallic bonding?
Three factors
What shape is associated with NH4+ due to the dative covalent bond present?
Tetrahedral
Which element has stronger metallic bonding: Mg or Na?
Mg because it has more protons
In metallic bonding, what do the delocalized electrons interact with?
The positively charged metal ions only
In metallic bonding, what factor contributes to the strength of the bond in Mg?
Release of more electrons into the sea of electrons
Which type of bonding is characterized by a giant molecular structure with many strong covalent bonds?
Macromolecular covalent bonding
What is a key feature of metallic bonding compared to other types of bonding?
Formation of a giant metallic lattice
Which type of bonding exhibits high boiling and melting points due to the strong electrostatic forces between oppositely charged ions?
Ionic bonding
What is the main characteristic of a dative covalent bond?
One atom donates both electrons to be shared with another
What makes metallic bonding stronger in Mg compared to other metals?
More electrons released into the sea of electrons
What is the main type of bond formed in ionic compounds?
Ionic bond
Why are positive ions smaller compared to their atoms?
They have one less shell of electrons
Which factor contributes to higher melting points in ionic compounds?
Smaller and/or higher charged ions
What causes negative ions to be larger than their corresponding atoms?
The pull of the nucleus is shared over more electrons
Which type of bond is characterized by atoms sharing electrons unequally?
Covalent bond
How does effective nuclear attraction affect ionic radius?
Decreases the size of positive ions
Study Notes
Metallic Bonding
- The strength of metallic bonding increases due to the release of more electrons in the outer shell to the sea of electrons.
- The Mg ion is smaller and has one more proton, resulting in a stronger electrostatic attraction between the positive metal ions and the delocalised electrons.
- Higher energy is required to break the bonds in metallic bonding.
Types of Bonding
- Ionic bonding: electrostatic force of attraction between oppositely charged ions.
- Examples: Giant Ionic Lattice (Sodium chloride, Magnesium oxide)
- Covalent bonding: shared pair of electrons.
- Types of Covalent bonding:
- Simple molecular: With intermolecular forces (van der Waals, permanent dipoles, hydrogen bonds) between molecules. Examples: Iodine, Ice, Carbon dioxide, Water, Methane
- Macromolecular: giant molecular structures. Examples: Diamond, Graphite, Silicon dioxide, Silicon
Properties of Bonding
- Ionic: high boiling and melting points due to giant lattice of ions with strong electrostatic forces between oppositely charged ions.
- Molecular (simple): low boiling and melting points due to weak intermolecular forces between molecules.
- Macromolecular: high boiling and melting points due to many strong covalent bonds in macromolecular structure.
- Metallic: high boiling and melting points due to electrostatic force of attraction between the metal positive ions and the delocalised electrons.
Ionic Radii
- Within a group, the size of the ionic radii increases going down the group due to the addition of more shells of electrons.
- Examples: N3-, O2-, F- (Ne) and Na+, Mg2+, Al3+.
Covalent Bonding
- Definition: A covalent bond is a shared pair of electrons.
- Dative Covalent bonding: A dative covalent bond forms when the shared pair of electrons in the covalent bond come from only one of the bonding atoms.
- Examples: NH4+, H3O+, NH3BF3.
Metallic Bonding Factors
- The three main factors that affect the strength of metallic bonding are:
- Number of protons/Strength of nuclear attraction.
- Number of delocalised electrons per atom.
- Size of ion.
Ionic Bonding
- Definition: Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer.
- Metal atoms lose electrons to form +ve ions, while non-metal atoms gain electrons to form -ve ions.
- Ionic crystals have the structure of giant lattices of ions.
- Ionic bonding is stronger and the melting points higher when the ions are smaller and/or have higher charges.
Learn about the factors that contribute to the strength of metallic bonding in magnesium, including the presence of more electrons in the outer shell, smaller ion size, and stronger electrostatic attraction between metal ions and delocalised electrons.
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