All categories

2 years ago

How many electrons are typically involved in bonding for group 1, group 2 and group 3 elements?

1 answer:

8 0

Here, we are required to determine how many electrons are typically involved in bonding for group 1, group 2 and group 3 elements and How many electrons are typically involved in bonding for group 6, 7 and 8 elements.

For group 1: Only one electron.
For group 2: Only two electrons
For group 3: Only 3 electrons
For group 6: Only 2 electrons
Fir group 7: Only 1 electron
For group 8: No electron

<em>The Valence electrons are the electrons which are available for bonding and chemical reactions in elements.</em>

<em>The Valence electrons are the electrons which are available for bonding and chemical reactions in elements.However, not all Valence electrons are actively involved in bonding. This is evident in the group 7(halogens) elements, although they have 7 Valence electrons, only one is actively involved in bonding.</em>

For group 1 elements: They have only one Valence electron and it is actively involved in bonding (ionic bonding)

For group 2 elements: They have only two Valence electron and both are actively involved in bonding (ionic bonding)

For group 3 elements: They have only three Valence electrons and all three are typically used for bonding.

For group 6 elements: They have 6 Valence electrons and are electronegative. As such, they only need to receive 2 electrons from an electropositive element and consequently, they only contribute two electrons into the bonding. As such, only 2 electrons are typically used for bonding.

For group 7: They have 7 Valence electrons and are highly electronegative. As such, they only need to receive 1 electrons from an electropositive element and consequently, they only contribute 1 electrons into the bonding. As such, only 1 electrons are typically used for bonding.

For group 8: They have a full octet configuration and are unreactive. Therefore, no electron is typically used for bonding.

brainly.com/question/18258856

You might be interested in

I need some help with chemistry. Let me know if you are good at it!

tekilochka [14]

Answer:

I think im good at it i have an A in the class

Explanation:

lol

3 0

2 years ago

Is O2 always a double bond?

Dima020 [189]

O-O single bonds and H-O single bonds in $\text{H}_2\text{O}_2$ molecules.
H-O single bonds in $\text{H}_2\text{O}$ molecules.
O=O double bonds in $\text{O}_2$ molecules.

<h3>Explanation</h3>

How many valence electrons do atoms in each molecule need for them to be stable?

Each H atom needs two valence electrons to be stable.
Each atom of an element other than H needs eight valence electron to be stable.

There are two H atoms and two O atoms in an $\text{H}_2\text{O}_2$ molecule. Atoms in each $\text{H}_2\text{O}_2$ need $2 \times 1 + 2\times 2 = 6$ more electrons to be stable.
There are two H atoms and one O atom in an $\text{H}_2\text{O}$ molecule. Atoms in each $\text{H}_2\text{O}$ molecule need $2 \times 1 + 2= 4$ more electrons to be stable.
There are two O atoms in an $\text{O}_2$ molecule. Atoms in each $\text{O}_2$ molecule need $2 \times 2 = 4$ more electrons to be stable.

How many chemical bonds in each molecule?

Each chemical bond adds one valence electron to each bonding atom. Each chemical bond connects two atoms. As a result, each chemical bond adds two valence electrons to the molecule.

Each $\text{H}_2\text{O}_2$ molecule needs $6 / 2 = 3$ chemical bonds.
Each $\text{H}_2\text{O}$ molecule needs $4 / 2 = 2$ chemical bonds.
Each $\text{O}_2$ molecule needs $4 /2= 2$ chemical bonds.

What chemical bonds are these? Again, each H atom needs only one more valence electron to be stable. It will share only one electron with O and form one H-O bond. The rest of the chemical bonds are between O atoms.

There are two H atoms in each $\text{H}_2\text{O}_2$ molecule, which form two H-O bonds. Two of the three chemical bonds in this molecule are H-O. The other is an O-O single bond between the two O atoms.
There are two H atoms in each $\text{H}_2\text{O}$ molecule, which form two H-O bonds. Both chemical bonds in this molecule are H-O. There's no O-O bond in this molecule.
There is no H atom in $\text{O}_2$ molecules. Both chemical bonds are between O atoms. However, there are only two O atoms. There must be two chemical bonds between the two O atoms. That bond will be an O-O double bond.

3 0

3 years ago

Read 2 more answers

Which lewis structures represent a molecule that would assume a linear geometry? check all that apply.

Daniel [21]

CO2, C2H2, BeF2, XeF2, etc all these molecules have linear geometry.

7 0

3 years ago

Read 2 more answers

Hund's rule states that electrons must spread out within a given subshell before they can pair

Temka [501]

Answer:

Groups 14, 15, and 16 have 2,3, and 4 electrons in the p sublevel (p sublevel has 3 "spaces" AKA orbitals), because Hunds says one in each orbital before doubling up if you had 2 electrons, group 14, they would both be in the first orbital, with 3 electrons, group 15, two in the first orbital one in the 2nd none in the 3rd. With 4 electrons, group 16, then you would have 2 in the first 2 orbitals and NONE in the 3rd.

Explanation:

If you are in group 13 you only have 1 electron so it can only be in one orbital. with group 17, you have 5 electrons, so 2 in the first 2 in the second and 1 in the 3rd, correct for Hunds rule anyway. Noble gasses, group 18, have 6 elecctrons, so every orbital is full any way you look at it.

6 0

2 years ago

The volume of 0.05 M H2SO4 is needed to completely neutralise 15ml of 0.1 M NaOH solution is

Feliz [49]

V(NaOH)=15 mL =0.015 L
C(NaOH)=0.1 mol/L
C(H₂SO₄)=0.05 mol/L

2NaOH + H₂SO₄ = Na₂SO₄ + 2H₂O

n(NaOH)=V(NaOH)C(NaOH)=2n(H₂SO₄)
n(H₂SO₄)=V(H₂SO₄)C(H₂SO₄)

V(NaOH)C(NaOH)=2V(H₂SO₄)C(H₂SO₄)

V(H₂SO₄)=V(NaOH)C(NaOH)/{2C(H₂SO₄)}

V(H₂SO₄)=0.015*0.1/{2*0.05}=0.015 L = 15 mL

5 0

3 years ago