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3 years ago

Rank these elements according to FIRST ionization energy, from highest to lowest:

Chemistry

2 answers:

Rzqust [24]3 years ago

3 0

The trend of ionization energy in the periodic table is decreasing from right to left and from top to bottom. In this case, we are given with elements K, Ca, Ge, Se, Br, Kr and see the periodic table to check the trend. The answer from highest to lowest Kr, Br, Se, Ge, Ca, and K

Zina [86]3 years ago

3 0

The order of the first ionization energy of the given elements from highest to lowest is $\boxed{{\mathbf{Kr > Br > Se > Ge > Ca > K}}}$

Further Explanation:

The energy that is needed to remove the most loosely bound valence electrons from the isolated neutral atom of the gas 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 ${\text{I}}{{\text{E}}_1}$ . Similarly, when the second electron is removed from the positively charged species (cation), the ionization energy is called the second ionization energy $\left( {{\text{I}}{{\text{E}}_2}} \right)$ and so on.

Potassium, calcium, germanium, selenium, bromine, and krypton belong to the same period of the periodic table.

Along a period, the atomic number increases but the number of shells remains the same while moving from left to right.

The number of protons, as well as the electrons, increases with the increase in the atomic number but the extra electrons are added in the same shell. Due to the high positive nuclear charge, the effective nuclear charge also increases. This results in an increase in the first ionization energy. So krypton will have the highest first ionization energy, followed by bromine, selenium, germanium, calcium, and potassium will have the lowest ionization energy.

Learn more:

1. Why is ${\text{6 - decene}}$ not possible: brainly.com/question/2095052

2. The gold foil experiment: brainly.com/question/1859083

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Periodic classification of elements

Keywords: first ionization energy , K, Ca, Ge, Se, Br, Kr, protons, electrons, atomic number, isolated, neutral, atom, nuclear charge.

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Neporo4naja [7]

Difference between Gas and Vapour:

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3 years ago

Help what is a b c please I want help this my quiz quick

stich3 [128]

Answer:

A= sum(mass*percent abundance)

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2 years ago

A chemistry graduate student is given 125.mL of a 1.00M benzoic acid HC6H5CO2 solution. Benzoic acid is a weak acid with =Ka×6.3

lubasha [3.4K]

Answer:

53.9 g

Explanation:

When talking about buffers is very common the problem involves the use of the Henderson Hasselbach formula:

pH = pKa + log [A⁻]/[HA]

where [A⁻] is the concentration of the conjugate base of the weak acid HA, and [HA] is the concentration of the weak acid.

We can calculate pKₐ from the given kₐ ( pKₐ = - log Kₐ ), and from there obtain the ratio [A⁻]/HA].

Since we know the concentration of HC6H5CO2 and the volume of solution, the moles and mass of KC6H5CO2 can be determined.

So,

4.63 = - log ( 6.3 x 10⁻⁵ ) + log [A⁻]/[HA] = - (-4.20 ) + log [A⁻]/[HA]

⇒ log [A⁻]/[HA] = 4.63 - 4.20 = log [A⁻]/[HA]

0.43 = log [A⁻]/[HA]

taking antilogs to both sides of this equation:

10^0.43 = [A⁻]/[HA] = 2.69

[A⁻]/ 1.00 M = 2.69 ⇒ [A⁻] = 2.69 M

Molarity is moles per liter of solution, so we can calculate how many moles of C6H5CO2⁻ the student needs to dissolve in 125. mL ( 0.125 L ) of a 2.69 M solution:

( 2.69 mol C6H5CO2⁻ / 1L ) x 0.125 L = 0.34 mol C6H5CO2⁻

The mass will be obtained by multiplying 0.34 mol times molecular weight for KC6H5CO2 ( 160.21 g/mol ):

0.34 mol x 160.21 g/mol = 53.9 g

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Answer:

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