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How many orbital electron pairs are present in the atom with the electron configuration 1s-2 2s-2 2p-5?
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∙ 10y ago
Four pairs of electrons, with one unpaired. This is the electronic configuration of fluorine
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∙ 10y ago
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Where is the energy level of each orbital found?
The s orbital has the lowest energy level.
When atoms complete their outer electron shell by sharing electron they form?
Covalent bonds
Which element in the periodic table has 2 pairs of electrons in the 3d orbitals?
Silica has 2 pairs of electrons in the third orbitals. Atomic number of silica is 14. Electron configuration of it is, [Si]= 1s2 2s2 2p6 3s2 3p2 .
What are repelled in VSEPR theory?
Electron pairs
How will electron pairs behave towards one another in VSEPR?
electron pairs move away from each other to more electrostatically balanced positions
What are paired electrons?
Pi electron pairs are electron pairs residing in the p orbital (as in s, p, d, f). This is the electron orbital responsible for double bonds and conjugated molecules according to molecular orbital theory.
The sp3d2 atomic hybrid orbital set accommodates how many electron PAIRS?
there r 2 electrons in the s orbital, their r 6 electrons in p orbital , their r 10 electron's in the d orbital and 14 electrons in f orbital.
Why is SeH2 linear and not bent?
The molecule should have 2 atoms with 2 lone electron pairs and be in bent configuration.
What is the electron configuration for lithium iodide?
.. [Li]+ [:I:]- (put the last 2 pairs above and below the "I" this wont let me) ..
What is electron pair effect?
Ionization is the process of removing one or more electrons from a neutral atom. This results in the loss of units of negative charge by the affected atom. The atom becomes electrically positive (a positive ion). The products of a single ionizing event are called an electron-ion pair.
Where is the energy level of each orbital found?
The s orbital has the lowest energy level.
How does number of electron pairs around central atom determine its shape?
The number of electron pairs around the central atom determines its shape by following the VSEPR theory, which states that electron pairs arrange themselves around the central atom to be as far apart from each other as possible. The arrangement of electron pairs gives rise to specific molecular geometries, which in turn determine the overall shape of the molecule.
When atoms complete their outer electron shell by sharing electron they form?
Covalent bonds
Which occupies a greater about of space free electron pairs or bonding pairs?
bonding pairs, the electrons from each ion reach to the other nuclei because of the inter magnetic force attracting the two atoms. Because the ions must reach to another atoms orbital they require more space than a free electron in a single atom.
Which occupies a greater amount of space free electron pairs or bonding pairs?
bonding pairs, the electrons from each ion reach to the other nuclei because of the inter magnetic force attracting the two atoms. Because the ions must reach to another atoms orbital they require more space than a free electron in a single atom.
In boron haildes why BCl3 is weakest Lewis acid but BI3 is a strongest Lewis acid?
Boron is sp2 hybridised with an empty p orbital. Both chlorine and iodine have lone electron pairs of suitable symmetry to form a partial pi bond with the empty orbital of boron. This partial pi bond effect is stronger and more significant in BCl3 because there is a better energy match between the empty p of boron (LUMO) and the lone pairs of Cl (HOMO) than between boron p and the lone pairs of iodine. As a Lewis acid, boron takes an electron pair into its empty p orbital. In BCl3, the significant pi bond means that this p orbital is less electron deficient and therefore hinders the ability of the p orbital to accept an electron pair, so it is a weaker acid than BI3. Maybe consult a textbook or website for a picture to help you visualise Boron in sp2 hybridised state.
What type of bond is present between the atoms of a water molecule?
Covalent bonds. (Atom bindings that share electron pairs)
