Write the Lewis structure for ethanol (CH3CH2OH), the alcohol found in alcoholic beverages, then answer the following questions:
1. How many valence electrons does this alcohol have? 2. How many bonded electrons does this alcohol have? 3. How many lone pairs of electrons does this alcohol have? 4. How many single bonds does this alcohol have?
1 answer:
Answer :
(1) The number of valence electrons present in the compound is, 20
(2) The number of bonded electrons present in the compound is, 16
(3) The number of lone pair electrons present in the compound is, 4
(4) The number of single bonds present in the compound is, 8
Explanation :
Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.
In the Lewis-dot structure the valance electrons are shown by 'dot'.
The given molecule is,
As we know that carbon has '4' valence electrons, hydrogen has '1' valence electrons and oxygen has '6' valence electrons.
Therefore, the total number of valence electrons in = 2(4) + 6(1) + 6 = 20
According to Lewis-dot structure, there are 16 number of bonding electrons and 4 number of non-bonding electrons or lone pair of electrons.
The Lewis-dot structure of is shown below.
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Answer:
Pd(O2C2H3)2
Explanation:
<u>Percentage composition of elements in the compound:</u>
Pd= 47.40%
O=28.50%
C=21.40%
H= 2.69%
<u>Molar mass of each element</u>
Pd= 106g/mol
O= 16g/mol
C= 12g/mol
H= 1g/mol
Step 1
Find the moles of each element in 100g sample using the formula
no. of moles(n)=mass/molar mass
<u>For Pd:</u> 47.40g/106g/mol
n= 0.447 moles
<u>For O:</u> 28.50/16
n= 1.78 moles
<u>For C:</u> 21.40/12
n= 1.783 moles
<u>For H:</u> 2.69/1
n= 2.69moles
Step 2
Now divide the no. of moles separately by the smallest number of moles. Smallest number of moles is <em>0.447</em>
Pd= 0.447/0.447
= 1
O= 1.78/0.447
= 3.9=4
C= 1.78/0.447
= 3.9=4
H= 2.69/0.447
= 6
Hence empirical formula is PdO4C4H6
The probable molecular formula is
Answer:
a) Representation - (in attachment)
b) Tetrahedral geometry and
c) hybrid orbitals invovle sigma bonding.
orbitals are formed by the overlapping of d-orbitals of sulfur with p-orbitals of oxygen.
Explanation:
a)
Representation in attachment.
The overall charge in the both structures are -2. The structure (b) is favored by the resonance structures since the formal charge with in the species are remained.
Therefore, structure (b) is the better representation of sulfate ion.
b)
In sulfate ion, sulfur atom is attached with four different oxygen atoms. According to the VSEPR theory , the sufate ion has tetrahedral geometry.
There is four sigma bonds and zero lone pairs present on the central metal atom.
Hence, the hybridization of the sulfur atom is
c)
The s and p orbitals of sulfur invovles hybridization and form sigma bonds.The orbitals of sulfur involves bonding.
Therefore, bonds are formed by the overlapping of d-orbitals of sulfur with p-orbitals of oxygen.
