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3 years ago

Define shielding and effective nuclear charge. What is the connection between the two?

Chemistry

1 answer:

ivolga24 [154]3 years ago

8 0

Answer:

The relation between the shielding and effective nuclear charge is given as

$Z_{eff} = Z -S$

where s denote shielding

z_{eff} denote effective nuclear charge

Z - atomic number

Explanation:

shielding is referred to as the repulsion of an outermost electron to the pull of electron from valence shell. Higher the electron in valence shell higher will be the shielding effects.

Effective nuclear charge is the amount of net positive charge that valence electron has.

The relation between the shielding and the effective nuclear charge is given as

$Z_{eff} = Z -S$

wheres denote shielding

z_{eff} denote effective nuclear charge

Z - atomic number

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How is liming a lake similar to a doctor prescribing medicine for a patient?

Jlenok [28]

An anti-acid medication

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3 years ago

How many grams of O are in 635 g of Li 2 O ?

KiRa [710]

Answer:

340g

Explanation:

Lithium oxide or Li2O is an inorganic compound made of two lithiums and one oxygen molecules. Lithium molecular mass is 6.94g/mol while oxygen molecular mass is 16g/mol. The molecular mass of Li2O will be:

2* 6.94g/mol + 1*16g/mol= 29.88g/mol

Out of 1 mol lithium oxide (29.88g), there is 1 mol of oxygen(16g). Then, out of 635g lithium oxide the number of oxygen will be: 635g * (16g/29.88g)= 340g

5 0

3 years ago

what mass of aluminium hydroxide is needed to decompose in order to produce 65.0 L of water at STP in stoichiometry?

pishuonlain [190]

Aluminium Hydroxide on decomposition produces Al₂O₃ and Water vapors.

<span> 2 Al(OH)</span>₃ → Al₂O₃ + 3 H₂O

According to equation at STP,

67.2 L (3 moles) of H₂O is produced by = 78 g of Al(OH)₃
So,
65.0 L of H₂O will be produced by = X g of Al(OH)₃

Solving for X,
X = (65.0 L × 78 g) ÷ 67.2 L

X = 75.44 g of Al(OH)₂
Result:
75.44 g of Al(OH)₂ is needed to decompose in order to produce 65.0 L of water at STP in stoichiometry

6 0

3 years ago

Read 2 more answers

Calculate the hydronium ion concentration in an aqueous solution with a poh of 4.33 at 25°c.

Jlenok [28]

Taking into account the definition of pH and pOH, the hydronium ion concentration in an aqueous solution with a pOH of 4.33 at 25°c is 2.138×10⁻¹⁰ M.

<h3>Definition of pH</h3>

pH is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance.

The pH is defined as the negative base 10 logarithm of the activity of hydrogen ions, that is, the concentration of hydrogen ions or hydronium ion H₃O⁺:

pH= - log [H⁺]= - log [H₃O⁺]

<h3>Definition of pOH</h3>

Similarly, pOH is a measure of hydroxyl ions in a solution and is expressed as the logarithm of the concentration of OH⁻ ions, with the sign changed:

pOH= - log [OH⁻]

<h3>Relationship between pH and pOH</h3>

The following relationship can be established between pH and pOH:

pOH + pH= 14

<h3>Concentration of hydronium ions</h3>

Being pOH= 4.33, pH is calculated as:

pH + 4.33= 14

pH= 14 - 4.33

Replacing in the definition of pH the concentration of hydronium ions is obtained:

- log [H₃O⁺]= 9.67

Solving:

[H₃O⁺]= 10⁻⁹ ⁶⁷

Finally, the hydronium ion concentration in an aqueous solution with a pOH of 4.33 at 25°c is 2.138×10⁻¹⁰ M.

Learn more about pH and pOH:

brainly.com/question/16032912

brainly.com/question/13557815

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4 0

2 years ago

How many moles of ammonia can you make from 0.37 moles of H2?

igomit [66]

Answer:

0.123 moles of ammonia, can be produced

Explanation:

First of all, we need to determine the reaction:

Ammonia is produced by the reaction of hydrogen and nitrogen.

3H₂(g) + N₂(g) → 2NH₃(g)

Ratio is 3:2. Let's solve the question with a rule of three:

If 3 moles of hydrogen can produce 2 moles of ammonia

Then, 0.37 moles will produce (0.37 . 2) /3 = 0.123 moles

6 0

3 years ago