All categories

2 years ago

/Why does an atom want all of it’s orbitals filled Why does it want to be in a stable state

Chemistry

1 answer:

Helen [10]2 years ago

5 0

The atom wants all of its orbitals filled because it has always desire to achieve stable or nearest noble element state.
It wants to be in a stable state to not to get involved in reactions

You might be interested in

What is name of HOPBr2 ?

USPshnik [31]

HOPBr₂ = dibromophosphinous acid

hope this helps!

5 0

3 years ago

Is blinking a voluntary or involuntary activity

sattari [20]

Blinking is an involuntary activity, because we do not have control over it. That is what our body is meant to do.

7 0

3 years ago

Read 2 more answers

If the natural abundance of Br−79 is 50.69 %, what is the natural abundance of Br−81?

Alexxandr [17]

The natural abundance of bromine in general in nature is 100%.
This means that:
the natural abundance of Br-79 + the natural abundance of Br-80 = 100

We know that the natural abundance of Br-79 is 50.69%. This means that the natural abundance of Br-80 is the rest of the 100%.

Natural abundance of Br-80 = 100% - 50.69% = 49.31%

8 0

3 years ago

Write a balanced chemical equation for the decomposition of RbNO3. Help me please!!!

nalin [4]

Answer:

2RbNO³ --> 2Rb + N² + 30²

Hope this helps!

8 0

3 years ago

A) A volume of 100 mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M

Wewaii [24]

Answer:

i) 5.00 mL of 1.00 M NaOH: before the equivalence point

ii) 50.0 mL of 1.00 M NaOH: before the equivalence point

iii) 100 mL of 1.00 M NaOH: at the equivalence point

iv) 150 mL of 1.00 M NaOH: after the equivalence point

v) 200 mL of 1.00 M NaOH: after the equivalence point

Explanation:

1. First calculate the number of mol acid in the 100 mL of 1.00 M HCl solution.

Equation:

Molarity = numbrer of moles of solute / volume of the solution in liters.

Thus, you need to convert each volume from mL to liters, which is done dividing by 1,000.

Naming M the molarity, n the number of moles of solute (acid or base), and V the volume in liters:

$M=n/v\implies n=M\times V=1.00M\times 0.100L=0.100mol$

2. Now calculate the number of moles of NaOH for every condition (addition)

i) 5.00 mL of 1.00 M NaOH

$n=0.00500liter\times 1.00M=0.00500molNaOH$

Since the number of moles of NaOH added (0.00500mol) is less than the number of moles of acid in the solution (0.100mol), this is before equivalence point.

ii) 50.0 mL of 1.00 M NaOH

$n=0.0500liter\times 1.00M=0.0500molNaOH$

Since the number of moles of NaOH added (0.0500mol) is less than the number of moles of acid in the solution (0.100mol), this is before equivalence point.

iii) 100 mL of 1.00 M NaOH

$n=0.100liter\times 1.00M=0.100molNaOH$

Since the number of moles of NaOH added (0.100mol) is equal to the number of moles of acid in the solution (0.100mol), this is at the equivalence point.

iv) 150 mL of 1.00 M NaOH

$n=0.150liter\times 1.00M=0.150molNaOH$

Since the number of moles of NaOH added (0.150mol) is greater than the number of moles of acid in the solution (0.100mol), this is after the equivalence point.

v) 200 mL of 1.00 M NaOH

This is more volume of NaOH, then this is also after the equivalence point.

5 0

3 years ago