1.4 - Bonding

• What type of elements participate in ionic bonding?

  Metal and non-metal
• What happens to electrons during ionic bonding?


  Electrons are transferred from metal to non-metal
• What are charged particles created during ionic bonding called?

  Ions
• How do oppositely charged ions interact in ionic bonding?

  They attract through electrostatic forces
• What structure is formed by ionic compounds?

  Giant ionic crystal lattice
• What ions are formed from sodium and chlorine in sodium chloride?

  Na​+​ and Cl​-​ ions
• What does chlorine do to form Cl​-​ ions?

  Chlorine gains an electron
• What occurs to sodium during the formation of Na​+​ ions?

  Sodium loses an electron
• What is the sulfate ion's formula?

  SO​4​2-
• What is the hydroxide ion's formula?

  OH​-
• What is the nitrate ion's formula?

  NO​3​-
• What is the carbonate ion's formula?

  CO​3​2-
• What is the ammonium ion's formula?

  NH​4​+

  
• What type of elements form covalent bonds?

  Two non-metals
• How are electrons involved in covalent bonding?

  Electrons are shared between two outer shells
• What must be balanced in a covalent bond?

  Electrostatic forces within the molecule
• What can multiple electron pairs produce in covalent bonding?

  Multiple covalent bonds between atoms
• What is an example of a molecule with a double covalent bond?

  Oxygen (O​2​)
• How can shared electron pairs be represented?

  Using dot and cross diagrams
• What is a coordinate bond?

  Electrons in the shared pair come from one atom
• What is an example of a coordinate bond formation?

  Ammonia forming with H​+​ ion
• How is a dative bond treated after formation?

  As a standard covalent bond
• What does bond polarity refer to?

  Charge variation around a covalent bond
• What is electronegativity?

  Power of an atom to attract negative charge
• How does electronegativity change across a period?

  It increases as atomic radius decreases
• How does electronegativity change down a group?

  It decreases as shielding increases
• What forms when two atoms with different electronegativities bond?

  A polar bond forms
• What is a permanent dipole?

  Regions of partial positive and negative charge
• What is an example of a polar molecule?

  Hydrogen fluoride

  
• How do polar molecules align in a lattice?

  They form a lattice similar to ionic lattices
• What is an induced dipole?

  When electron orbitals are influenced by a charged particle
• How does bond character vary?

  From ionic to covalent with intermediate bonds
• What are the characteristics of different bond types?

  (a) Covalent Bond:

  • Electrons shared equally
  • No overall charge

  
  

  (b) Intermediate Bond:

  • Electrons shared unequally
  • Partial charges present

  
  

  (c) Ionic Bond:

  • Complete transfer of electrons
  • Produces ions with full charges
• How do bond characteristics affect physical properties?

  They influence boiling point and solubility
• What are intermolecular forces?

  Forces between molecules holding them in structures
• How do intermolecular forces compare to ionic or covalent bonds?

  They are much weaker than ionic or covalent bonds
• What is the weakest type of intermolecular force?

  Van der Waals Forces
• What influences the strength of Van der Waals forces?

  Molecular mass and shape
• How do straight chain molecules compare to branched chain molecules in Van der Waals forces?

  Straight chains experience stronger forces
• What type of intermolecular force acts between polar molecules?

  Permanent Dipole