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4 years ago

Give the Unabbreviated electron configuration for barium

Chemistry

1 answer:

Shalnov [3]4 years ago

8 0

Answer:

Ba: 1s² 2s²2p⁶ 3s²3p⁶ 4s²3d¹⁰4p⁶ 5s²4d¹⁰5p⁶ 6s²

Step-by-step explanation:

Step 1. Locate barium in the Periodic Table.

It's in Period 6, Group 2: Element 56 (highlighted blue in the Periodic Table below).

Step 2. Add 54 electrons to the energy levels

You add then in the order shown in the diagram below.

The complete electron configuration is:

Ba: 1s² 2s²2p⁶ 3s²3p⁶ 4s²3d¹⁰4p⁶ 5s²4d¹⁰5p⁶ 6s²

n = 2 + 8 + 8 + 18 + 18 + 2 = 56

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the freezing point depression constants of the solvents cyclohexane and naphthalene are 20.1°C/m and 6.94°C/m respectively. Whic

Evgesh-ka [11]

Explanation:

It'd be better to use cyclohexane. The possible explanation is that the freezing temperature will change by 20.1 degrees for each mole of substance added to 1 kg of cyclohexane, although the same amount added to naphthalene will change its freezing point just by 6.94 degrees.

It is so much easier to identify a larger change more adequately than a smaller one. You would actually not have a 1 molal solution in operation, so the variations in freezing points would be even smaller than the ones already described.

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3 years ago

The electrons in a bond between two iodine atoms (I2) are shared

valentina_108 [34]

Answer : The electrons in a bond between two iodine atoms are shared equally and non-polar.

Explanation :

Non-polar covalent bond : It is a type of bond that is present between the two similar and different atoms. This type of bond is formed when the electrons are shared equally between the atoms.

This type of bond is termed as non-polar because of the electronegativity difference between the atoms is negligible.

The given molecule $I_2$ is formed by the equal sharing of electrons and the bond formed between the iodine-iodine is non-polar due to negligible electronegativity difference.

Therefore, the electrons in a bond between two iodine atoms are shared equally and non-polar.

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3 years ago

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At what temperature can 10g of Cez(SO4)3 be dissolved in 100g of water?

dmitriy555 [2]

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3 years ago

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You have a solid 7.00 gram mixture of sodium nitrate and silver nitrate. You add distilled water to dissolve the solids. Now you

olganol [36]

Answer:

Net ionic equation: Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

44.9% as AgNO₃

Explanation:

When sodium nitrate, NaNO₃ and silver nitrate, AgNO₃ are dissolved in water, the Na⁺, NO₃⁻ and Ag⁺ ions are formed.

Then, the addition of NaCl (Na⁺ and Cl⁻) produce AgCl⁻ as precipitate. <em>The net ionic equation is:</em>

If 2.54g of AgCl are formed and represents the 95.9% of yield. The real amount of AgCl is:

2.54g AgCl * (100% / 95.9%) = 2.65g AgCl.

In moles (Molar mass AgCl = 143.32g/mol):

2.65g AgCl * (1mol / 143.32g) = 0.0185 moles of AgCl = Moles of AgNO₃

<em>Because all Ag comes from AgNO₃</em>

<em />

Thus, the original mass of silver nitrate and its precentage is (Molar mass AgNO₃ = 169.87g/mol):

0.0185 moles AgNO₃ * (169.87g / mol) = 3.14g of AgNO₃

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3 years ago

Hey, help please. Giving BRAINLIEST!

ddd [48]

When 0.5 moles of Zn react with 0.4 moles of HCL the limiting reactant will be HCL and excess reactant is Zn 0.3 moles excess and 0.2 moles Zn will be consumed in the reaction.

<h3>What is the limiting reactant in the given equation ?</h3>

STEP1- Write the balanced equation

Zn + 2HCL → ZnCl₂ + H₂

STEP2- calculate the moles according to the reaction

1mol of Zn requires → 2moles of HCL

0.5 moles of Zn requires→ 1mol of HCL

Given moles of HCL is 0.4

STEP3- Apply unitary method

0.5/x=1/0.4

0.5×0.4= x

0.2=x

STEP4- excess reagent left 0.5-0.2=0.3

Hence, the 0.3mole of excess Zn is left

Learn more about limiting reactions numericals.

brainly.com/question/12836695

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