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Draw the Lewis structure for the polyatomic hydronium H3O cation. Be sure to include all resonance structures that

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Answer 1

Answer:

Answer:

Lewis structure of Hydronium ion is shown below :

Explanation:

Lewis structure : It is a representation of valence electrons on the atoms in a molecule

Here , Hydronium ion is given , which contains 1 atom of oxygen and 3 atoms of hydrogen .

Oxygen has a total of 6 valence electrons and hydrogen contains 1 valence electron .

Oxygen share its 3 valence electrons with 3 hydrogen atoms and left with 3 valence electrons. From these three valence electrons of oxygen atom two electrons will be shown as a pair of electrons on oxygen atom but a single electron can not be shown . So , to simplify this, one positive charge is shown overall .

Resonance structure will be same as the hybrid structure because all three atoms are same , that is hydrogen .

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Help me plzz I need help can someone help

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D volcanic corruption

What is the mass, in grams, of 1.50 mol of iron (III) sulfate?Express your answer using three significant figures.

Answers

Answer : The mass of 1.50 mole of iron(III) sulfate is, $5.99* 10^2g$

Explanation : Given,

Moles of iron(III) sulfate = 1.50 mole

Molar mass of iron(III) sulfate = 399.88 g/mole

The formula of iron(III) sulfate is, $Fe_2(SO_4)_3$

Formula used :

$\text{Mass of }Fe_2(SO_4)_3=\text{Moles of }Fe_2(SO_4)_3* \text{Molar mass of }Fe_2(SO_4)_3$

Now put all the given values in this formula, we get:

$\text{Mass of }Fe_2(SO_4)_3=1.50mole* 399.88g/mole$

$\text{Mass of }Fe_2(SO_4)_3=599.82g=5.99* 10^2g$

Therefore, the mass of 1.50 mole of iron(III) sulfate is, $5.99* 10^2g$

What is the correct noble gas configuration for oxygen?

Answers

Oxygen (O) is a chemical element which you're surely familiar with since you breathe it every second of your life. The noble gas configuration is [He] 2s2 2p4. This shows that there is a total of 8 electrons (two in the 1s orbital, another 2 in the 2s orbital and the rest in the 2p orbital)

Let me know if you need anything else.

- Dotz :)

22. What is the molar mass of oxygen (O2)?A- 15.9994 g/mol
B- 1.204 x 1024 g/mol
C- 6.02 x 1023 g/mol
D- 31.9988 g/mol

Answers

Answer:

D- 31.9988 g/mol

Explanation:

The molar mass of a substance is the mass in grams of one mole of the substance. For a compound, the molar mass is the gram - formula mass or gram - molecular weight. It is determined by the addition of its component atomic masses;

To find molar mass of O₂;

Atomic mass of O = 15.9994g/mol

Molar mass of O₂ = 2(15.9994) = 31.9988g/mol

Write a balanced chemical equation for the standard formation reaction of gaseous dinitrogen tetroxide

Answers

Answer:

$N_2(g)+2O_2(g)\rightarrow N_2O_4(g)$

Explanation:

Hello,

In this case, considering the required product which is dinitrogen tetroxide whose molecular formula is N₂O₄, by considering its formation reaction which is starting by both gaseous nitrogen and oxygen as shown below:

$N_2(g)+O_2(g)\rightarrow N_2O_4(g)$

Nevertheless, it should be balance since four oxygen atoms are present at the right side, thus, we obtain:

$N_2(g)+2O_2(g)\rightarrow N_2O_4(g)$

Best regards.

Which one of these could be in the unknown anion "X" in this acid: H3Xcarbonate
fluorate
nitrogen
nitrite

Could you explain how to find this? The process?

Answers

Answer:

the answer is nitrogen

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Radiometric isotope x decays to daughter isotope y with a half-life of 220,000 years. at present you have 1/4 gram of x in the rock. from the amount of daughter isotope y presently in the rock, you determine that the rock contained 16 grams of isotope x when it formed. how many half-lives have gone by? how old is the rock?

Sulfur and oxygen form both sulfur dioxide and sulfur trioxide. When samples of these were decomposed the sulfur dioxide produced 3.49g oxygen and 3.50g sulfur, while the sulfur trioxide produced 9.00g oxygen and 6.00g sulfur.A) Calculate the mass of oxygen per gram of sulfur for sulfur dioxide.B) Calculate the mass of oxygen per gram of sulfur for sulfur trioxide.

Calculate ΔHrxn for the following reaction: C(s) + H2O(g) --> CO(g) + H2(g) Use the following reactions and given ΔH values: C (s) + O2 (g) → CO2 (g), ΔH = -393.5 kJ 2 CO (g) + O2 (g) → 2 CO2 (g), ΔH= -566.0 kJ 2 H2 (g) + O2 (g) → 2 H2O (g), ΔH= -483.6 kJ

How many grams of propanol (C3H7OH, 60.10 g/mol) would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)