Yes, it obeys the octet rule.
(Of coarse not an octet for the H atoms: they are saturated with a duplet (=2)).
To show you HOW this is done, you will need the structural formula:
If it is a monosaccharide there are already 32 different isomeres.
And even one of these and the most common one: alpha-D-gluco-pyranose (which is glucose) is too difficultto draw it in this simple 'html-text editor' layout.
Just as example some explaining calculation about electron bonding pairs and free pairs.
Valence electrons counting:
6 C = 6x4 = 24 e
12 H = 12x2 = 24 e
6 O = 6x6 = 36 e
Total of 84 electrons are available for free or covalent (= bonding) electron pairs
(total 84/2 = 42 pairs can be formed)
Needed for octets and H-duplets
6 C = 6x8 = 48 e
6 O = 6x8 = 48 e
12 H = 12x2 = 24 e
Total needed for octets/duplets = 120. These are 60 'needed to see' pairs
Total of 24 double counted bonding pairs (48 pairs 'seen' from one atom AND 'seen' from the other atom bound to it, called covalent*) electron pairs)
One possible structure (which is not glucose) fitting the above calculation (1, 2, 3) is described here:
6 C atoms in a regular (bee hive) ring: 6 covalent pairs
6 H atoms directly to each C: 6 cov. pairs
6 O atom bonded at one side to each C atom: 6 cov. pairs
6 H atoms bonded to the other side of those 6 O atoms: 6 cov. pairs
Total of 24 double counted bonding pairs*) between all atoms.
This leaves 6x2 = 12 free electron pairs, two per O atom to fulfill their 'octet need'
And now you can conclude:
24 double counted = 48 'seen' electron pairs which are covalent*)
12 free electron pairs (2 on each O atom)
Total of 60 'structural drawn' pairs,
Thus this, being the same as the 'needed to see' pairs (60, see above), means that ALL atoms are obeying the octet(+ duplet) rule.
*) covalent means: 'seen by two' atoms which are bound together.
(The name of this formula would be 1,2,3,4,5,6-cyclo-hexane-hexa-ol, it isn't even a monosaccharide)
Most molecules will obey the octet rule. It does not matter how many shells the element has. An element with 3 shells is electrically stable with both 8 or 18 electrons in its valence shell.
Some molecules which obey this rule include oxygen and chlorine gas.
Molecules that do not follow the octet rule are usually more reactive than ones that do. Free radicals do not follow the octet rule. They have at least one unpaired electron.
No chlorine oxides will obey the octet rule.
Hydrogen does not obey the octet rule. Boron does not always obey the octet rule and in fact forms Lewis acids such as BF3 which only has 6 electrons.
no it does not follow octet rule
H and I SCl4 ICl3 SeCI4 F2CCF2
Chlorine Cl : it can have a higher valence (ClO2, HClO3) than predicted by the octet rule. Hydrogen H and oxygen O cannot escape the octet rule.
No chlorine oxides will obey the octet rule.
Hydrogen does not obey the octet rule. Boron does not always obey the octet rule and in fact forms Lewis acids such as BF3 which only has 6 electrons.
no it does not follow octet rule
yes PCl3 obey octet rule there are 5 electrons in the valence shell of phosphorous it need 3 electron to complete its octet so it form bond with 3 chlorine after bond formation there are 8 electron in its octet it obey octet rule
No it is not fully obeying the octet rule. Boron has only 6 electrons (3 own + 3 from each F atom), lacking two for the octet. Fluorine is 3x satisfied, each with 8 electrons (each has 7 own plus 1 from boron).
Yes
because it does
H and I SCl4 ICl3 SeCI4 F2CCF2
I know for sure BBr# & PF5 do not obey the octet rule, but i can't remember the rule of isotopes so I can't say for sure whether or not CO3 -2 obeys it or not.
H and l
Boron And Berylium
Chlorine Cl : it can have a higher valence (ClO2, HClO3) than predicted by the octet rule. Hydrogen H and oxygen O cannot escape the octet rule.