Chapter 3

Question 1

ionic bonds

Answer 1

bond between two ions

the positive and negative charge hold the 2 together

complete gain/loss of electrons
usually for between metal and nonmetals

Question 2

covalent bonds

Answer 2

an electron pair is shared between 2 atoms

Question 3

nonpolar bonds

Answer 3

the electron pair is shared equally

Question 4

polar bonds

Answer 4

the electron pair is shared unequally

Question 5

coordinate covalent bonds

Answer 5

both the shared electrons come from 1 of the 2 atoms

Question 6

formal charge

Answer 6

formal charge = (# valence electrons in unbonded atom) – (# of bonds) – (# of dots)

Question 7

VSEPR theory

Answer 7

a system to predict the 3D arrangement of atoms in a molecule based on the number of bonds and lone electron pairs in their lewis structure

Question 8

Steps to predict geometrical structure of a molecule using VSEPR theory:

Answer 8

Question 9

intermolecular forces

Answer 9

• Electrostatic attractions between molecules
• Significantly weaker than covalent bonds

Question 10

3 types of intermolecular forces

Answer 10

london dispersion forces

dipole-dipole interactions

hydrogen bonds

Question 11

london dispersion forces

Answer 11

• a temporary attractive force due to the formation of temporary dipoles in a nonpolar molecule (as the electron cloud sways)
• weakest of the IM forces
• present in all atoms and molecules
• larger atom size = larger LD force

Question 12

dipole-dipole interactions

Answer 12

• Occur between oppositely charged ends of polar molecules
• Stronger than London dispersion forces
• Evident in the solid and liquid phases but negligible in the gas phase due to the distance between particles

Question 13

hydrogen bonds

Answer 13

• Specialized subset of dipole-dipole interactions
• Involved in intra and inter molecular attraction
• Hydrogen bonding occurs when hydrogen is bonded to one of three very electronegative atoms: fluorine, oxygen, or nitrogen