describe about oxygen group

1. ulfa
tessa selvi
vici fala

2. Tendency Anomaly Sulfur
Oxygen
Oxygen groups Oxygen
Covalent hydrogen Sulfide
bond in
oxygen
compound
Sulfide
Tendency in
the covalent Sulfur oxyde
compound
Sulfuric acid
hydrogen
peroxide
Sulfur-oxide salt
Sulfur halide

3. The Preference of Oxygen Groups
Table 1. Data Of Some Oxygen Group Characteristic
elements Electron Melting Boiling point
configuration point (oC) (oC)
8O [2He] 2s2 2p4 -219 -183
16S [10Ne] 3s2 3p4 119 445
34Se [18Ar] 3d10 4s2 4p4 221 685
52Te [36Kr] 4d10 5s2 5p4 452 987
84Po [54Xe] 4f14 5d10 6s2 6p4 254 962

4. • Double bond stability and katenasi's character
Double bond on oxygen much greater than its single bond, single bond
O-O is very weak relevance with formation katenasi. In carbon groups
(faction 14), katenasi’s ability is decrease with its increasing atomic
number, but in groups 16, Sulfur can form the longest chain (S8). In
fact, single bond O-O is weakest than single bond of oxygen atom with
other atoms, O - X. Thus, oxygen atom prefers to form bonding with
another atoms than with itself.
• Its absents orbital d.
Oxygen forms just one with fluorin's compound which is OF2, but sulfur
can form some compound with fluorin include SF6. To reach until six its
covalent bonds, sulfur atom have to involve orbital d. Thus, not be found
flourin's oxygen compound that analog with SF6 because there is no
orbital d in oxygen atom.

5. Dioxygen Trioxygen
( O2 ) ( O3 )
- Dark blue gas
- colorless gases - Boiling point - 112 oC
- Has boiling point – 183 oC - diamagnetic
- its color is blue in the - Toxic gas
liquid phase. - ozon produced by
- paramagnetic SUTET, photocopy engine
- reactive gas. and laser print.
-The solubility is lower than - As oxidator that stronger
carbondioxyde than O2.

6. The bonding in oxygen covalent compound
oxygen
Single Double Triple
coordinate
Bond Bond Bond
bond angles between the two single
covalent bonds maybe smaller Another way is oxygen atoms can
than the regular tetrahedral form an equivalent three single
angle (109o) it is influenced by covalent bond.
a number of free electrons. Example of hydronium ion H3O+
example:
Bond angle H-O-H are 104,5o

7. Tendency in oxygen compound
Electropositive Electropositive Metal oxides with
Nonmetal
metal oxides metal oxides more than one
oxides
strong weak kind of oxide
Have - Always bound
characteristics Are oxides with low covalently
ionic and basic. amphoteric. It oxidation levels - Nonmetals with low
Examples : means can are alkaline. oxidation level are
- BaO react with acid Oxides with high neutral
- CuO (not and base. oxidation levels - Nonmetals with high
soluble in water example : ZnO are acidic oxidation level are
but soluble in acidic
dilute acid)

8. Hydrogen Peroxide
• Pure hydrogen peroxide is
almost colorless liquid.
• Very viscous because of
hydrogen bonding.
• Corrosive.
• Not stable.
• Easily to disporpotionation
according to reaction :
2 H2O2 (l)  2 H2O (l) + O2 (g)
• Forming a dihedral with angle
111o and bond angle of H-O-
O is 94,5o.

9. Sulfur
• Forming an ionic compound with the active
metal.
• Forming a covalent compound.
• Single covalent bond length 104 pm.
• Electronegativity 2,6
• Allotropes of Sulfur is S8 (cyclorooctasulfur), S6
(cyclorohexasulfur), and S12
(cyclododecasulfur).

10. S6 S12
is the most stable allotrope of
sulfur that can be synthesized by
mixing sodium thiosulfate
solution
Na2S2O3 with hydrochloric acid :
6Na2S2O3(aq) +12HCl(aq) → S6(s) +
6SO2(g) + 12NaCl(aq) + 6H2O(l)

11. Hydrogen Sulfide
Characteristic :
 colorless gases
 its smell is bad like stinky egg
 toxic gas
 produced by anaerob bactery trough
decomposition reaction.
 in laboratory gas H2S produced by reaction :
FeS(s) + 2HCl(aq)  FeCl2(aq) + H2S(g)
 can identified with Pb2S prodused brown
black PbS

12. Sulfide
• group 1, 2, aluminium are dissolve in water.
• S2-(aq) + H2O (l) HS- (aq) + OH – (aq)
• Continued hydrolisis produce H2S gas that
smells stinky :
• HS - (aq) + H2O(l) H2S (s) + OH- (aq)
• function of sulfide : in battery, cosmetics, etc.

13. Sulfur oxides
Sulfur dioxide Sulfur trioxide
Equilateral triangle
stucture
Nonlinier Stucture
Easier dissolve in water Strong acidic and dissolve
in water form sulfuric acid
with reaction:
SO3 (g) + H2O H2 SO4

14. Sulfuric Acid
• Thick liquid like oil
• Pure sulfuric acid has conductivity properties
• Sulfuric acid can be react in 5 ways are:
1. As acid
2. Drying agent to water
3. Oxidation agent
4. Sulfonation agent
5. As base

15. 1. As acid
Dilute sulfuric acid usually as acid
2. Drying agent to water
Has ability to destroy water component from formula
structure of a compound
3. Oxidation agent
Hot concentrate sulfuric acid is good oxidation agent
4. Sulfonation agent
Concentrate sulfuric acid has ability replaced 1 atom
hydrogen in organic compound with sulfonic acid
5. As base
Sulfuric acid can be base if added to stronger protone
donor

16. Producing Sulfuric Acid
• Producing methode according to contact
process even lead chamber always using sulfur
dioxide that can be prepared from sulfur
melted combustion in dry air:
• S (s) + O2 SO2(g)
• Mixture sulfur dioxide with dry air flow into
catalisator V2O5 at 400-500o C.

17. Sulfur-oxide Salt
Sulfate is produced with
three step : Hydrogen
1. Between natrium sulfate is an Sulfite can be
Thiosulfate
hydroxyde with acidic, that can formed by
dilute sulfuric acid
can be formed
be formed by flowing sulfur
2. Reaction between by boiling
reaction dioxyde gas
electropositive sulfur in
between into natrium
metal and dilute sulfate
natrium hydroxyde
sulforic acid aqueous
3. Reaction between hydroxyde with aqueous
carbonate salt and sulfuric acid
dilute sulfuric acid
Peroksodisulfate ion has one dioxo bridge. Its acid is white
solid, two important salt as oxidator agent are potassium
and amonium peroksodisulfate, with peroksodisulfate ion is
reductated become sulfate ion.

18. Sulfur Halide
• The important compound of sulfur-halogen are
sulfur-fluorin, and sulfur-chlorine.
• Sulfur-fluorin form SF6 (colorless
gas, unsmell, not reactive, low toxic, stable) and
SF4 (reactive gas, is decomposed by wet air
become sulfur-dioxyde and hydrogen fluoride).
• Sulfur-chlorin only form with low oxidation level.
Sulfur melted that flowed with dichlorin gas
producing disulfur dichloride, S2Cl2. disulfur
dichoride much used in rubber vulcanization
process.