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2 years ago

Draw the best lewis structure for bro4- and determine the formal charge on bromine

Chemistry

2 answers:

Svetach [21]2 years ago

7 0

Answer :

Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule. The electrons are represented by dot.

The given molecule is, perbromate ion.

Bromine has '7' valence electrons and oxygen has '6' valence electron.

Therefore, the total number of valence electrons in perbromate ion, $BrO_4^-$ = 7 + 4(6) + 1 = 32

According to Lewis-dot structure, there are 14 number of bonding electrons and 18 number of non-bonding electrons.

Formula for formal charge :

$\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}$

$\text{Formal charge on }Br=7-0-\frac{14}{2}=0$

The Lewis-dot structure of perbromate ion is shown below.

garik1379 [7]2 years ago

6 0

The formal charge on Br is $\boxed0$ . (For structure, refer to the attached image).

Further explanation:

The bonding between the different atoms in covalent molecules is shown by some diagrams known as the Lewis structures. These also show the presence of lone pairs in the molecule. These are also known as Lewis dot diagrams, electron dot diagrams, Lewis dot structures or Lewis dot formula. In covalent compounds, the geometry, polarity, and reactivity are predicted by these structures.

Lewis structure of ${\mathbf{BrO}}_{\mathbf{4}}^ -$ (Refer to the structure in the attached image):

The total number of valence electrons of ${\text{BrO}}_4^ -$ is calculated as,

Total valence electrons = [(1) (Valence electrons of Br) + (4) (Valence electrons of O) + Charge on anion]

$\begin{aligned}{\text{Total valence electrons}}\left({{\text{TVE}}} \right)&=\left[{\left({\text{1}} \right)\left({\text{7}}\right)+\left({\text{4}}\right)\left({\text{6}} \right)+1}\right]\\&=32\\\end{aligned}$

Formal charge:

It is the charge that an atom acquires in a molecule by considering that the chemical bonds are shared equally between the two atoms, irrespective of their electronegativities.

The formula to calculate the formal charge on an atom is as follows:

${\mathbf{Formal\:charge=}}\left[\begin{gathered}\left[ \begin{gathered}{\mathbf{total\:number\:of\:valence\:electrons }}\hfill\\{\mathbf{in\:the\:free\:atom}}\hfill\\\end{gathered}\right]{\mathbf{}}-\\\left[{{\mathbf{total\:number\:of\:non- bonding\:electrons}}}\right]-\\\frac{{\left[ {{\mathbf{total\:number\:of\:bonding\:electrons}}}\right]}}{{\mathbf{2}}}\\\end{gathered}\right]$

Br forms three double bonds with three oxygen atoms and one single bond with one oxygen atom.

The total number of valence electrons in the free bromine atom is 7.

The total number of non-bonding electrons in Br is 0.

The total number of bonding electrons in Br is 14.

Substitute these values in equation (1) to find the formal charge on Br.

$\begin{aligned}{\text{Formal charge on Br}}&=\left[ {7 - 0 - \frac{{14}}{2}}\right]\\&=0\\\end{aligned}$

Total number of valence electrons in the free oxygen atom is 6.

The total number of non-bonding electrons in O is 4.

The total number of bonding electrons in O is 4.

Substitute these values in equation (1) to find the formal charge on blue O.

$\begin{aligned} {\text{Formal charge on blue O}} &=\left[ {6 - 4 -\frac{4}{2}} \right]\\&= 0\\\end{aligned}$

Total number of valence electrons in the free oxygen atom is 6.

The total number of non-bonding electrons in O is 6.

The total number of bonding electrons in O is 2.

$\begin{aligned}{\text{Formal charge on red O}}&=\left[ {6 - 6 -\frac{2}{2}} \right]\\&=- 1\\\end{aligned}$

Bromine atom has 7 valence electrons, and oxygen atom has 6 valence electrons Each of the three blue-colored oxygen atoms forms one double bond with bromine atom, and two lone pairs are present on each of them. The red-colored oxygen atom forms one single bond with the bromine atom, and six lone pairs are present on it. Therefore the Lewis structure of ${\mathbf{BrO}}_{\mathbf{4}}^ -$ is attached in the image.

Learn more:

1. Molecular shape around the central atoms in the amino acid glycine: brainly.com/question/4341225

2. How many molecules will be present on completion of reaction?: brainly.com/question/4414828

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Molecular structure and chemical bonding

Keywords: Lewis structure, valence electrons, BrO4-, formal charge, 0, Br, oxygen, double bonds, single bond, bonding electrons, non-bonding electrons, total valence electrons.

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2 years ago

What are the 4 most abundant minerals in the continental crust? What percentage do these 4 makeup of the total?

Tanya [424]

Answer:

$SiO_2$ , $Al_2O_3$ , $CaO$ , $MgO$

Explanation:

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2 years ago

4.82 g of an unknown metal is heated to 115.0∘C and then placed in 35 mL of water at 28.7∘C, which then heats up to 34.5∘C. What

nikitadnepr [17]

Answer: The specific heat of metal is 2.34 J/g°C

Explanation:

To calculate the mass of water, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Density of water = 1 g/mL

Volume of water = 35 mL

Putting values in above equation, we get:

$1g/mL=\frac{\text{Mass of water}}{35mL}\\\\\text{Mass of water}=(1g/mL\times 35mL)=35g$

When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.

$Heat_{\text{absorbed}}=Heat_{\text{released}}$

The equation used to calculate heat released or absorbed follows:

$Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})$

$m_1\times c_1\times (T_{final}-T_1)=-[m_2\times c_2\times (T_{final}-T_2)]$ ......(1)

where,

q = heat absorbed or released

$m_1$ = mass of metal = 4.82 g

$m_2$ = mass of water = 35 g

$T_{final}$ = final temperature = 34.5°C

$T_1$ = initial temperature of metal = 115°C

$T_2$ = initial temperature of water = 28.7°C

$c_1$ = specific heat of metal = ?

$c_2$ = specific heat of water = 4.186 J/g°C

Putting values in equation 1, we get:

$4.82\times c_1\times (34.5-110)=-[35\times 4.186\times (34.5-28.7)]$

$c_1=2.34J/g^oC$

Hence, the specific heat of metal is 2.34 J/g°C

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1 year ago

(a) calculate the %ic of the interatomic bond for the intermetallic compound tial3. (b) on the basis of this result, what type o

Mrrafil [7]

Answer :

The correct answer is %IC = 10 % and bond is covalent bond with slight polarity.

Percent Ionic Character :

It is defined as percent of ionic character present in a polar covalent bond . The formula of % ionic character (%IC) is given as follows :

$Percent Ionic character = 1 - e^-^0^.^2^5 ^*^(^X^a^-^X^b^) * 100$

Where Xa = Electronegativity of A atom and Xb = Electronegativity of B atom

Given : Molecule is TiAl₃

Electronegativity of Ti = 2.0

Electronegativity of Al = 1.6 ( From image shared )

Plug the value in above formula :

$Percent Ionic character = 1 - e^-^0^.^2^5 ^*^(^2^.^0^-^1^.^6^) * 100$

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$Percent Ionic character = 1 - e^(^-^0^.^1^) * 100$

Value of e⁻¹ = 0.90

Percent ionic character = 1 - 0.90 * 100

Percent Ionic character = 10 %

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2 years ago

In which 1.0 gram sample are particles arranged in a rystal structure?

lilavasa [31]

The Options are as follow,

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(2) C₂H₆ (g) (4) Cal₂ (aq)

Answer:

Option-1 is the correct answer.

Explanation:

As we know crystal formation is the property of solids. Therefore, in given options we are given with four different states of matter.

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Option 2, C₂H₆ (Ethane) is in gas form, so it cannot form crystals.

Option 3, CH₃OH (Methanol) is present in liquid form, so it fails to form crystals.

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2 years ago