Question

Decide if the compound/ion listed can satisfy the octet rule (duet rule for H), if so choose Satisfies Octet Rule from the drop down menu. If the compound/ion cannot satisfy the octet rule for one of the atoms in the formula, choose one of the following three reasons why; Too many valence electrons (more than eight), Too few valence electrons (fewer than eight), or Odd # of valence electrons. CCl3 NO3- ICl3 SF3 PCl3 PS3

Answer 1

NO3-- N has 5 valence electron and Oxygen has 6 valence electron.

therfore 5+3X6+1 = 24

in the lewis structure of NO3- there is a double between one of Oxygen and nitrogen which satisfy the octet rule.It also exist in 3 resonance which follows octet rule.

2. ICl3

Iodine has 7 valence elctrons and Cl also have 7 valence electrons . therfore 7 +(3X7) = 28

here 3 Cl atoms share 1 electron with I to complete its octet which leave Iodine with 4 unshared electrons.here central atom exceed the octet rule. excess valence electrons.

3. SF3

S has 6 valence electrons , F has 7 valence electrons

6+(3X7) = 27 electron

total valence electrons are 27 .

the central atom S has 3 unshared electrons . excess valence electrons.

4. PCl3

P = 5 valence electrons

Cl = 7 valence electrons

Total valence electrons = 5+ (3X7) = 26.

2 excess electrons .

5. PS3

p = 5 valence electrons

S = 6 valence electrons

total = 5 +(3X6) = 23 electrons

central atom has 1 electron less to follow the octet rule