Unit 2

Question 1

Characteristics of ionic bonds:

Answer 1

Metal-metal or non-metal-metal, total transfer of e, high melt point, solids(🏡temp), inorganic, strong bonds, current, soluble, e orbitals are separate

Question 2

Covalent bond characteristics:

Answer 2

Non-metal, shared e, low melting point, liquids&gasses at 🏠temp, organic, weak bond, doesn’t conduct, insoluble, e orbitals overlap

Question 3

Y are ionic compounds able to conduct electricity

Answer 3

When they are dissolved, in solution the crystal lattice breaks apart and the free mobile ions now carry current

Question 4

Electronegativity acrols a period

Answer 4

Increases due to # of protons in nucleus

Question 5

Electronegativity down a family:

Answer 5

Due to increase of e levels the outer levels of e are further away from the pull of the nucleus

Question 6

How does electronegativity help us determine the polarity of a bond:

Answer 6

The more electronegative atoms attracts e more strongly. The less electronegative has a slight (+) charge.

Question 7

What is the trend in melting point and strength of ionic bond and electronegativity

Answer 7

The higher the difference in electronegativity, the high the melting point (stronger bonds create higher mp)

Question 8

Electronegativity:

Answer 8

The ability of an atom to attract a pair of e in a bond.