All categories

3 years ago

Argon (Ar): [Ne]3s23p6 core electrons: valence electrons:

Chemistry

2 answers:

Artyom0805 [142]3 years ago

6 0

Answer : Core electrons = 10

Valence electrons = 8

Explanation :

Core electrons : They are the electrons in an atom that do not participate in bonding.

Valence electrons : They are electrons in an atom that participate in bonding.

Electronic configuration : It is defined as the representation of electrons around the nucleus of an atom.

Number of electrons in an atom are determined by the electronic configuration.

The electronic configuration of argon (Ar) will be:

$1s^22s^22p^63s^23p^6$

The electronic configuration of neon (Ne) will be:

$1s^22s^22p^6$

So, the electronic configuration of argon (Ar) in noble gas notation will be:

$[Ne]3s^23p^6$

In the given electronic configuration of argon, the electrons present in 1st shell and 2nd shell are the core electrons and the electrons present in 3rd shell are the valence electrons. That means,

Number of core electrons = 2 + 2 + 6 = 10

Number of valence electrons = 2 + 6 = 8

irga5000 [103]3 years ago

3 0

10 core elections

8 valence elections

You might be interested in

Peroxyacylnitrate (PAN) is one of the components

coldgirl [10]

C – 19,9%, H – 2,2%, N – 11,6%, O – x%

$M=120\frac{g}{mol}$

1 percentage

The entire molecule is 100% and all the components of the compound add up to 100%.

100% - 19,9% - 2,5% - 11,6% = 66,1%

The compound contains 66,1% oxygen.

2 molar masses

$M_{C}=12,01\frac{g}{mol}$

$M_{H}=1,008\frac{g}{mol}$

$M_{O}=15,999\frac{g}{mol}$

$M_{N}=14,007\frac{g}{mol}$

3 masses

The compound has a molar mass of 120g/mol. So one molecule weighs 120 g. To find out how much the percentage of a component weighs, you have to calculate it using the molar mass.

carbon

19,8% of 120g

$m=120g*0,198\\m=23,76g$

One molecule contains 23,76g of carbon.

hydrogen

2,5% of 120g

$m=120g*0,025\\m=3g$

One molecule contains 3g of hydrogen.

oxygen

66,1% of 120g

$m=120g*0,661\\m=79,32g$

One molecule contains 79,32g of oxygen.

nitrogen

11,6% of 120g

$m=120g*0,0,116\\m=13,92g$

One molecule contains 13,92g of nitrogen.

4 amount of substance

carbon

$n=\frac{23,76g}{12,01\frac{g}{mol} }\\n=1,98mol$

The compound contains about 2 moles of carbon.

hydrogen

$n=\frac{3g}{1\frac{g}{mol} }\\n=3mol$

The compound contains about 3 moles of hydrogen.

oxygen

$n=\frac{79,32g}{15,999\frac{g}{mol} }\\n=4,96mol$

The compound contains about 5 moles of oxygen.

nitrogen

$n=\frac{13,92g}{14,007\frac{g}{mol} }\\n=0,99mol$

The compound contains about 1 moles of nitrogen.

5. molecular formula

The formula results from the ratio of the amounts of substance.

$n_{C} :n_{H} :n_{O} :n_{N} =2:3:5:1\\C_{2}H_{3}NO_{5}$

8 0

2 years ago

What is the concentration of a solution in which 10.0 g of AgNO3 is dissolved in 500 mL of solution?

Zigmanuir [339]

molar concentration of AgNO₃ solution = 0.118 mole/L

Explanation:

Because we have the volume of the solution and there is no information about the density of the solution I will asume that you ask for the molar concentration.

number of moles = mass / molecular weight

number of moles of AgNO₃ = 10 / 170 = 0.0588

molar concentration = number of moles / volume (L)

molar concentration of AgNO₃ solution = 0.0588 / 0.5

molar concentration of AgNO₃ solution = 0.118 mole/L

Learn more about:

molar concentration

brainly.com/question/1286583

#learnwithBrainly

6 0

3 years ago

Volume increases, pressure stays the same, temperature

Mila [183]

Temperature decreases (?)

4 0

3 years ago

How many seconds are there in 23 days ?

Brrunno [24]

Since there are 23 days and 24 hours in each day, you multi-ply them and get 552 hours. Since each hours is 60 minutes, 552*60 is 33120 minutes. Since one minute is 60 seconds, 60*33120 is 1,987,200 seconds. Therefore, there are 1,987,200 seconds in 23 days.

7 0

3 years ago

If an ideal gas at a constant temperature is initially at a pressure of 3.8 atm and is then allowed to expand to a volume of 5.6

BabaBlast [244]

Answer:

The most common example is the molar volume of a gas at STP (Standard Temperature and Pressure), which is equal to 22.4 L for 1 mole of any ideal gas at a temperature equal to 273.15 K and a pressure equal to 1.00 atm.If an ideal gas at a constant temperature is initially at a pressure of 3.8 atm and is then allowed to expand to a volume of 5.6 L and a pressure of 2.1 - 18914… ... of 5.6 L and a pressure of 2.1 atm, what is the initial volume of the gas? ... An ideal gas is at a pressure of 1.4 atm and has a volume of 3 L.

Explanation:

I hope I help :)

7 0

2 years ago

Argon (Ar): [Ne]3s23p6 core electrons:__ valence electrons:__

Argon (Ar): [Ne]3s23p6 core electrons: valence electrons: