(DONE) Lecture 20

Question 1

Define ionic bonds

• explain electron transfer
• held together by?
• talk about melting points

Answer 1

• metal +non metal
• metal to non mental
• held by strong electrostatic interactions
• generally high

Question 2

Define covalent bonds

• explain electron behaviour

- held together by?

Answer 2

• non metal + non metal
• electrons are shared between atoms
• bonds from 2 nuclei attracting the same shared electrons

Question 3

Explain the difference between bonding electrons and lone pairs

Answer 3

• bonding electrons: valence electrons that are shared between 2 nuclei in a covalent bond
• lone pairs: valence electrons are not involved in a bond

Question 4

Explain the difference between single, double, triple and coordinate covalent bonds

Answer 4

• 2 atoms share 1 pair of valence electrons
• 2 atoms share 2 pairs of valence electrons
• 2 atoms share 3 pairs of electrons
• 1 atom donates both electrons in a covalent bond

Question 5

What does the strength of a covalent bond mean? Order the covalent bonds from weakest to strongest

Answer 5

• requires more energy to break

- single, double, triple

Question 6

Define: resonance structure

Answer 6

• 2 or more equivalent electron dot structures that can be written for a molecule or polyatomic ion
• Each structure differs only in the placement of the electron pairs

Question 7

Define resonance hybrid

Answer 7

The average of all possible resonance structures