All categories

1 year ago

Give the group number and general electron configuration of an element with each electron-dot symbol:

1 answer:

4 0

The group number of (a) is VA(15) and electronic configuration is 1s2 2s2 2p3 . the group number of (b) is IVA(14) and the electronic configuration is 1s2 2s2 2p2 .

What is electronic configuration ?

it shows the distribution of electrons in the atomic orbitals .

it follows a standard notation of s, p, d, f atomic orbitals in which electronic distribution of an atom occurs .

it has standard notation method as well as condensed electron configuration .

it is useful in determining the valency of an element .

it is useful in predicting the properties of a group of elements .

<h3>What is condensed electron configuration ?</h3>

It contains the symbol of the nearest , smaller noble gas in the square brackets and then the symbols of the occupied orbitals which contains valance electrons .

Example of condensed electron configuration is given by ,

in case of iron the electronic configuration is 1s2 2s2 2p6 3s2 4s2 3d6 .

Thus , the condensed electron configuration of iron is [Ar] 3d6 4s2 .

Learn more about electronic configuration here :

brainly.com/question/50903246

#SPJ4

You might be interested in

Equal but opposite forces acting on an object results in what?

forsale [732]

Answer:

Action given and reaction taken

Also known as

Newton's third law of motion

Explanation:

An action will be done such as bouncing a ball on the wall

- You throw the ball (Action)

- The ball bounces back (Reaction)

Hope this Helps

3 0

2 years ago

at standard pressure, what is the temperature at which a saturated solution of NH4Cl has a concentration of 60g NH4CL/100 g H2O

Nataliya [291]

Answer: Temperature = T, unknown

Saturated Solution, NH4Cl concentration = 60g/100g H2O = 0.6g NH4Cl/g H2O

Assume density of H2O = 1 g/ml

m = 0.6g NH4Cl/g H2O / 1 g/ml

m = 0.6g NH4Cl/ml

See the table of saturated solutions and identify the temperature at which the concentration of NH4Cl is 60g/100g H2O.

Explanation: The line on the graph on reference table G indicates a saturated solution of NH4CL as a concentration of 60. g NH4 Cl/100. g H2O

5 0

2 years ago

A. Calculate the empirical formula of a molecule with percent compositions: 55.3% potassium (K), 14.6% phosphorus (P), and 30.1%

Otrada [13]

The way you calculate the empirical formula is to firstly assume 100g. To find each elements moles you take each elements percentage listed, times it by one mole and divide it by its atomic mass. (ex: moles of K =55.3g x 1 mole/39.1g, therefore there is 1.41432225 moles of Potassium) Once you’ve completed this for every element you list each elements symbol beside it’s number of moles and divide by the smallest number because it can only go into its self once. After you’ve done this, you’ve found your empirical formula, which is the simplest whole number ratio of atoms in a compound. I’ve added an example of a empirical question I completed last semester :)

6 0

3 years ago

Read 2 more answers

An element has two isotopes, A and B, with mass numbers of 32.0 and 33.0 respectively. The relative atomic mass is 32.3. The per

vlada-n [284]

Answer:

d) A - 70% B - 30%

Explanation:

If x is the abundance of A, and 1−x is the abundance of B, then:

x (32.0) + (1−x) (33.0) = 32.3

32x + 33 − 33x = 32.3

33 − x = 32.3

x = 0.7

The abundance of A is 70%, and the abundance of B is 30%.

7 0

3 years ago

Read 2 more answers

Aqueous sulfuric acid (H2SO4) reacts with solid sodium hydroxide (NaOH) to produce aqeous sodium sulfate (Na2SO4) and liquid wat

Montano1993 [528]

Answer:

The theoretical yield of water formed is 2.2 grams

Explanation:

Step 1: Data given

Mass of H2SO4 = 5.9 grams

Mass of NaOH = 6.6 grams

Molar mass H2SO4 = 98.08 g/mol

Molar mass of NaOH = 40.0 g/mol

Step 2: The balanced equation

2NaOH + H2SO4 → Na2SO4 + 2H2O

Step 3: Calculate moles

Moles = mass / molar mass

Moles H2SO4 = 5.9 grams / 98.08 g/mol

Moles H2SO4 = 0.060 moles

Moles NaOH = 6.6 grams / 40.0 g/mol

Moles NaOH = 0.165 moles

Step 4: Calculate the limiting reactant

For 2 moles NaOH we need 1 mol H2SO4 to produce 1 mol Na2SO4 and 2 moles H2O

H2SO4 is the limiting reactant. It will completely be consumed ( 0.060 moles). NaOH is in excess . There will react 2*0.060 = 0.120 moles

There will remain 0.165 - 0.120 = 0.045 moles NaOH

Step 5: Calculate moles H2O

For 2 moles NaOH we need 1 mol H2SO4 to produce 1 mol Na2SO4 and 2 moles H2O

For 0.0600 moles H2SO4 we'll have 2*0.0600 = 0.120 moles H2O

Step 6: Calculate mass H2O

Mass H2O = 0.120 moles * 18.02 g/mol

Mass H2O = 2.16 grams

The theoretical yield of water formed is 2.2 grams

4 0

3 years ago