Fast solutions for complex problems

How many bonds can sulfur form with other atoms?

6 bonds
Sulfur is capable of forming 6 bonds because it can have an expanded valence shell; sulfur is in period 3 of the Periodic Table.

Can sulfur have 4 bonds?

These bonds and their chemistry are found in many proteins, as well as synthetic compounds. In addition, sulfur can also form four-coordinate ‘hypervalent’ bonds, where its formal number of valence electrons exceeds eight.

What atoms can sulfur bond with?

Two hydrogen (H) atoms can bond with one sulfur (S) atom, making the formula H2S, also known as hydrogen sulfide. The same way that oxygen is happy when it has two extra electrons, sulfur likes to have two extras as well.

Can sulfur make three bonds?

Sulfur usually forms 2 bonds, e.g. H2S, -S-S- compounds… This is because of its 3p4 orbital. p-orbitals allow for 6 places to be filled, hence sulfur tends to form 2 bonds. It can “expand the octet” as it has 6 valence electrons, hence allowing the formation of 6 bonds.

Why does sulfur break the octet rule?

Sulfur can make use of its 2 unpaired electrons to form 2 covalent bonds plus the 4 electrons from its 2 lone pairs to give a total of 8 electrons. Hence sulfur obeys octet rule in this case. But sulfur can unpair its electrons and promote one of its electrons (highlighted in green) to an empty 3d orbital.

Does sulfur have a lone pair?

Continuing with sulfur, we observe that in (a) the sulfur atom shares one bonding pair and has three lone pairs and has a total of six valence electrons.

Can sulfur make 6 bonds?

Now sulfur has 6 unpaired electrons which means it can form 6 covalent bonds to give a total of 12 electrons around its valence shell. So in addition to being octet, sulfur can expand octet to have 10 or 12 electrons.

Does sulfur follow octet rule?

Sulfur can follow the octet rule as in the molecule SF2. Each atom is surrounded by eight electrons. It is possible to excite the sulfur atom sufficiently to push valence atoms into the d orbital to allow molecules such as SF4 and SF6.

What are 3 interesting facts about sulfur?

Here are some interesting facts about sulfur.

  • Atomic number: 16.
  • Atomic weight: 32.066.
  • Melting point: 388.36 K (115.21°C or 239.38°F)
  • Boiling point: 717.75 K (444.60°C or 832.28°F)
  • Density: 2.067 grams per cubic centimeter.
  • Phase at room temperature: Solid.
  • Element classification: Non-metal.
  • Period number: 3.

Can sulfur hydrogen bond?

Sulfur atoms have been known to participate in hydrogen bonds (H-bonds) and these sulfur-containing H-bonds (SCHBs) are suggested to play important roles in certain biological processes. It is revealed that sulfur atom is a very poor H-bond acceptor, but a moderately good H-bond donor.

What are the 3 exceptions to the octet rule?

However, there are three general exceptions to the octet rule: Molecules, such as NO, with an odd number of electrons; Molecules in which one or more atoms possess more than eight electrons, such as SF6; and. Molecules such as BCl3, in which one or more atoms possess less than eight electrons.

Which element does not follow octet rule?

The two elements that most commonly fail to complete an octet are boron and aluminum; they both readily form compounds in which they have six valence electrons, rather than the usual eight predicted by the octet rule.

What kind of bonds does sulfur form?

The element sulfur (s) is most likely to form covalent bonds with the element helium (he). magnesium (mg). zinc (zn). oxygen (o).

How many covalent bonds does sulfur have?

Sulfur has six valence electrons, and thus is able to form six covalent bonds, as each valence electron forms it’s own bond.

Does sulfur have lone pairs?

easily looked up on wikipedia. Here, Sulfur has two pairs of lone electrons, much like oxygen in water. However, they are not both hybridized. This is evident in the fact that thiophene shows aromatic activity.

How many valence electrons does sulfur have?

Sulfur has six valence electrons. Valence electrons are the outermost electrons which, therefore, are located on the highest energy levels. Consequently, these are the electrons available for chemical bonding.