Bonding Flashcards
(31 cards)
What are the three main types of chemical bonding?
Ionic bonding, covalent bonding, and metallic bonding.
What is ionic bonding?
The electrostatic attraction between oppositely charged ions (metal + non-metal).
What is covalent bonding?
The sharing of electron pairs between non-metal atoms.
What is metallic bonding?
The attraction between positive metal ions and delocalized electrons.
Which elements form positive ions in ionic bonding?
Metals (they lose electrons).
Which elements form negative ions in ionic bonding?
Non-metals (they gain electrons).
What is the structure of an ionic compound?
A giant ionic lattice.
What are the properties of ionic compounds?
High melting/boiling points, conduct electricity when molten or in solution.
Why do ionic compounds conduct electricity when molten or dissolved?
Because ions are free to move and carry charge.
Give an example of an ionic compound.
Sodium chloride (NaCl).
What happens to sodium in ionic bonding?
It loses 1 electron to form Na⁺.
What happens to chlorine in ionic bonding?
It gains 1 electron to form Cl⁻.
Between what types of elements does covalent bonding occur?
Non-metals only.
What is a molecule?
A group of atoms bonded covalently.
Give examples of covalently bonded molecules.
Water (H₂O), oxygen (O₂), carbon dioxide (CO₂).
What are the properties of simple covalent substances?
Low melting/boiling points, poor electrical conductivity.
Why do covalent molecules have low melting/boiling points?
Weak intermolecular forces between molecules.
What are giant covalent structures?
Large networks of atoms bonded by covalent bonds.
Examples: Diamond, graphite, silicon dioxide.
Why do giant covalent structures have high melting points?
All atoms are bonded in strong covalent networks.
Why can graphite conduct electricity?
It has delocalized electrons between layers.
Why is diamond hard?
Each carbon forms 4 strong covalent bonds in a rigid structure.
What happens in metallic bonding?
Positive metal ions are surrounded by a sea of delocalized electrons.
Why are metals good conductors of electricity?
Delocalized electrons move freely and carry charge.
