# What is the correct formula for the compound made form lead and chloride?

What is the correct formula for the compound made form lead and chloride? PbCl2 Pb2C1 PbCI PbC14

A

Explanation:

cause its easy

PbCl2

Explanation:

Pb has a valency of 2

Cl has a valency of 1

During bonding, there will be an exchange of ions as shown below:

Pb^2+ + Cl^- —> PbCl2

Balance the equation by putting 2 in front of Cl-

Pb^2+ + 2Cl^- —> PbCl2

74.1% + 25.9% = 100%

we assume 100g of sample

100%100g
25.9% N x
x 25.9g N

100g - 25.9g = 74.1g O

mass of N = 14g
mass of O = 16g

1 mole of N 14g
x moles of N 25.9g
x = 1.85 moles of N

1 moles of O 16g
x moles of O 74.1g
x = 4.6 moles of O

N : O = 1.85 : 4.6
we share by the smallest value
N : O = 1.85 : 4.6  ||:1.85
N : O = 1 : 2.4 ≈ 1 : 2
NO₂

The formula for a compound made from and is .

Explanation:

For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.

Here cation is having an oxidation state of +3 written as and anion is having an oxidation state of -3 written as . Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral .

Thus formula for a compound made from and is . D.

If we take a sample of 100g of the given compound, we should find that it contains 74.1g of oxygen and 25.9g of nitrogen. The molar masses of oxygen and nitrogen are approximately 16.0g/mol and 14.0g/mol respectively. To find the appropriate number of moles of oxygen and nitrogen found in one mole of the given compound, we divide the mass of the sample by the molar mass of each substance.

For oxygen: 74.1g/(16.0g/mol) = 4.63125 mol (round up to 5 mol)

For nitrogen: 25.9g/(14.0g/mol) = 1.85 mol (round up to 2 mol)

Therefore one mole of this compound contains 2 moles of nitrogen and 5 moles of oxygen.

A compound is formed when two or more elements combine in definite proportions. In the given scenario we have carbon and hydrogen atoms.

The valence electron configuration of C = 2s²2p²

H = 1s¹

There are 4 valence electrons in carbon; one paired (2s) and two unpaired (2p). Promotion of a 2s electron to a 2p orbital leaves 4 unpaired electrons which can combine with 4 H atoms to form a stable compound: CH4

Ans: (a) CH4, because four electron pairs are shared between carbon and hydrogen.

Answer : The correct option is, HF, because both fluorine and hydrogen are capable of forming only one covalent bond.

Explanation :

Covalent compound : It is defined as the compound which is formed by the sharing of electrons between the atoms forming a compound.

The covalent compound are usually formed when two non-metals react.

Ionic compound : It is defined as the compound which is formed when electron gets transferred from one atom to another atom.

Ionic compound are usually formed when a metal reacts with a non-metal.

As we known that, hydrogen and fluorine are non-metals. So, they are capable of forming only one covalent bond.

Hence, the correct option is HF, because both fluorine and hydrogen are capable of forming only one covalent bond.

I believe the answer is Ag₂O or AgO

It would be MgO because as stated in the question a magnesium ion has a charge of +2 and an oxygen ion has a charge of –2. The charges would cancel each other out therefore leaving each of the elements with only one of each.

Name : Magnesium Fluoride

Formula : MgF2

Explanation:

Give me brainliest

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