Which ion was formed by providing the second ionization energy to remove an electron? Ca2+ N3– Fe3+ S2–

Answers

Answer 1

Answer:

Ca²⁺

Explanation:

Ionization energy is defined as the minimum amount of energy required to knock out the electron from valence shell of an atom in its gaseous state. While, second Ionization energy is defined as the amount of energy required to knock out the second electron from an ion containing +1 charge in gaseous state.

Among given options Ca²⁺ is the correct choice because the calcium has lost two electrons i.e. first electron was removed by providing first ionization energy i.e.

Ca + 1st IE → Ca¹⁺ + 1 e⁻

and second electron is was removed by providing second ionization energy i.e.

Ca ¹⁺ + 2nd IE → Ca²⁺ + 1 e⁻

Answer 2

Answer:

$\boxed{{\text{C}}{{\text{a}}^{{\text{2 + }}}}}$ is formed by providing the second ionization energy to remove an electron.

Further Explanation:

The energy that is needed to remove the most loosely bound valenceelectrons from the isolated neutral gaseous atom is known as the ionization energy. It is denoted by IE. The value of IE is related to the ease of removing the outermost valence electrons. If these electrons are removed so easily, small ionization energy is required and vice-versa. It is inversely proportional to the size of the atom.

Ionization energy is further represented as first ionization, second ionization and so on. When the first electron is removed from a neutral, isolated gaseous atom, the energy needed for the purpose is known as the first ionization energy, written as ${\text{I}}{{\text{E}}_{\text{1}}}$ . Similarly, when the second electron is removed from the positively charged species (cation), the ionization energy is called the second ionization energy $\left( {{\text{I}}{{\text{E}}_{\text{2}}}} \right)$ and so on.

The neutral atom corresponding to ${\text{C}}{{\text{a}}^(2 + )}$ is calcium. If second ionization energy is supplied to calcium atom, it results in the removal of two electrons and thus ${\text{C}}{{\text{a}}^(2 + )}$ is formed. So ${\text{C}}{{\text{a}}^(2 + )}$ can be formed by providing second ionization energy. to the neutral atom.

The neutral atom corresponding to ${{\text{N}}^(3 - )}$ is nitrogen. If second ionization energy is supplied to nitrogen, it results in the formation of ${{\text{N}}^(2 + )}$ , not ${{\text{N}}^(3 - )}$ . So ${{\text{N}}^(3 - )}$ cannot be formed by providing the second ionization energy to the neutral atom.

The neutral atom corresponding to ${\text{F}}{{\text{e}}^(3 + )}$ is iron. If second ionization energy is supplied to the iron atom, it results in the formation of ${\text{F}}{{\text{e}}^(2 + )}$ , not ${\text{F}}{{\text{e}}^(3 + )}$ . So ${\text{F}}{{\text{e}}^(3 + )}$ cannot be formed by providing the second ionization energy to the neutral atom.

The neutral atom corresponding to ${{\text{S}}^(2 - )}$ is sulfur. If second ionization energy is supplied to the sulfur atom, it results in the formation of ${{\text{S}}^(2 + )}$ , not ${{\text{S}}^(2 - )}$ . So ${{\text{S}}^(2 - )}$ cannot be formed by providing the second ionization energy to the neutral atom.

Therefore, the only ion that can be formed by supplying the second ionization energy is ${\text{C}}{{\text{a}}^(2 + )}$ .

Learn more:

1. Which is the oxidation-reduction reaction:

brainly.com/question/2973661

2. What is the mass of 1 mole of viruses: brainly.com/question/8353774

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Periodic classification of elements

Keywords: second ionization energy, Ca2+, N3-, Fe3+, S2-, IE1, IE2, first electron, second electron, neutral atom., nitrogen, calcium, iron, sulfur.

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The average atomic mass of oxygen is 15.9994 amu. The atomic masses of its three isotopes are as follows: O-16: 15.995 amu; O-17: 16.999 amu; O-18: 17.999 amu Which isotope is most likely to have the greatest abundance in nature?

Answers

The average atomic mass of an atom would be the closest to the mass of its most commonly found isotope, because if another isotope would be more common, the average would "shift" to be closer to the most common isotope.

So the answer is O-16: its mass is almost the same as the average atomic mass.

Answer:

0-16

Explanation:

Calculate the number of moles
230 g of C2H5OH
560 g of C2H4
0.640 g of SO2

Answers

mass of C = 12g
mass of H = 1g
mass of O = 16g
mass of C2H5OH = 46g = 1 mole

1 mole of C2H5OH ------------ 46g
x moles of C2H5OH ----------- 230g
x = 5 moles of C2H5OH

~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~
mass of C = 12g
mass of H = 1g
mass of C2H4 = 28g = 1 mole

1 mole of C2H4 -------------- 28g
x moles of C2H4 ------------- 560g
x = 20 moles of C2H4
~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~
mass of S = 32g
mass of O = 16g
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1 mole of SO2--------------------- 64g
x mole of SO2 -------------------- 0,64g
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Given the balanced equation:2C + 3H2==> C2H6
What is the total number of moles of C that must completely react to produce 2.0 moles of C2H6?
(1) 1.0 mol (3) 3.0 mol
(2) 2.0 mol (4) 4.0 mol

Answers

Answer: The correct answer is option 4.

Explanation:

$2C+3H_2\rightarrow C_2H_6$

According to the reaction, 1 mol of $C_2H_6$ is obtained from 2 moles of C gives

Then, 2 moles of $C_2H_6$ will be obtained from:

$(2)/(1)* 2$ moles of C =4 moles

Hence, the correct answer is option 4.

The answer is (4) 4.0 mol. This is a stoichiometry problem. You start with 2.0 mol of C2H6 and obtain the moles of C by multiplying 2.0 by the mole ratio, in this case 2. 2.0*2=4.0mol.

Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H2O2(aq) ---> 2H2O(l) + O2(g)What volume of pure O2(g), collected at 27C and 746 torr, would be generated by decomposition of 125 g of a 50.0% by mass hydrogen peroxide solution?

Answers

Answer:

23.0733 L

Explanation:

The mass of hydrogen peroxide present in 125 g of 50% of hydrogen peroxide solution:

$Mass=\frac {50}{100}* 125\ g$

Mass = 62.5 g

Molar mass of $H_2O_2$ = 34 g/mol

The formula for the calculation of moles is shown below:

$moles = (Mass\ taken)/(Molar\ mass)$

Thus, moles are:

$moles= (62.5\ g)/(34\ g/mol)$

$moles= 1.8382\ mol$

Consider the given reaction as:

$2H_2O_2_((aq))\rightarrow2H_2O_((l))+O_2_((g))$

2 moles of hydrogen peroxide decomposes to give 1 mole of oxygen gas.

Also,

1 mole of hydrogen peroxide decomposes to give 1/2 mole of oxygen gas.

So,

1.8382 moles of hydrogen peroxide decomposes to give $\frac {1}{2}* 1.8382 mole of oxygen gas. Moles of oxygen gas produced = 0.9191 molGiven: Pressure = 746 torrThe conversion of P(torr) to P(atm) is shown below:[tex]P(torr)=\frac {1}{760}* P(atm)$

So,

Pressure = 746 / 760 atm = 0.9816 atm

Temperature = 27 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T₁ = (27 + 273.15) K = 300.15 K

Using ideal gas equation as:

PV=nRT

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.9816 atm × V = 0.9191 mol × 0.0821 L.atm/K.mol × 300.15 K

⇒V = 23.0733 L

How many shells will transition metals use to bond with other elements? (site 2)

Answers

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Find the final equilibrium temperature when 15.0 g of milk at 13.0 degrees c is added to 148 g of coffee with a temperature of 88.3 degreesc. assume the specific heats of coffee and milk are the same as for water (c = 4.19 j/g•c), and disregard the heat capacity of the container.

Answers

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$q_(lost)= (15X13X4.19)+(148X88.3X4.19), (15+148)X4.19XT_(final)$ =(15X13X4.19)+(148X88.3X4.19)

$T_(final)$ = 81.37 ° C

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