Chapt. 2

Question 1

covalent bonding

Answer 1

• sharing of electrons between non-metals
• exists due to the electrostatic attraction of the + nucleus and the - electrons

Question 2

effect of number of bonds in covalent

Answer 2

double bonds
- more attraction
- shorter bond as it is closer to the nuclei
- harder to break

Question 3

polarity

Answer 3

when atoms in a covalent bonds have different electronegativity causing the electrons to bond closer to the more electrongative atoms causing it to be partially negative.

Question 4

shapes of molecules

Answer 4

electron pairs (bonding and lone pairs) are negatively charged they will repel one another and spread out around the central atom, as far apart as possible

Question 5

Dipole - Dipole

Answer 5

because polarity creates partial charges, there can be electrostatic attraction b/w polar molecules
partial charges = weak attraction

Question 6

Hydrogen bonding

Answer 6

• H is bonded to FON
• FON are highly electronegative therefore bond is strong
• FON has lone pair = increases the ability to pull the electrons toward themselves

Question 7

dispersion forces

Answer 7

• weakest
• when a molecule momentarily becomes polar due to an uneven distribution of electrons in the bond
• creates an instantaneous dipole moment

Question 8

covalent network lattice

Answer 8

• 3D lattice of covalent bonded atoms
• includes diamonds,