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katrin2010 [14]
2 years ago
9

Water (H2O) has two O–H bonds. The electronegativity of oxygen is 3.5, whereas hydrogen is 2.1. Which statement best describes t

he type of bond this molecule has and how the electrons behave?
A. O–H bonds are polar covalent, and hydrogen pulls the shared electrons toward it.

B. O–H bonds are nonpolar covalent, and oxygen pulls the shared electrons toward it.

C. O–H bonds are nonpolar covalent, and hydrogen pulls the shared electrons toward it.

D. O–H bonds are polar covalent, and oxygen pulls the shared electrons toward it.
Chemistry
2 answers:
creativ13 [48]2 years ago
8 0

The statement that best describes the type of bond a molecule of water has and how the electrons behave is : O–H bonds are polar covalent, and oxygen pulls the shared electrons toward it; option D

<h3>What are covalent molecules</h3>

Covalent molecules are molecules which are formed by the sharing of electrons between atoms of two or more elements whose elecyronegativity values are close to each other.

Covalent bonds are usually formed by non-metals such as hydrogen, oxygen, nitrogen to form their gases.

Example of covalent molecules include water and hydrogen gas.

<h3>What are Polar molecules</h3>

Polar molecules are molecules which are formed by the uneven sharing of electrons between atoms or by the formation of ions by substances such that the two ends of the molecule will have different charges, positive and negative.

In polar covalent molecules, the more electronegatibe element pulls the shared electrons more to itself. For example, in a water molecule which is polar, oxygen pulls the shared electrons with hydrogen more to itself to have a partial negative charge while the hydrogen atom has a partial positive charge.

Therefore, statement that best describes the type of bond a molecule of water has and how the electrons behave is : O–H bonds are polar covalent, and oxygen pulls the shared electrons toward it; option D

Learn more about about polar covalent molecules at: brainly.com/question/3978603

boyakko [2]2 years ago
4 0

Answer:

see below

Explanation:

1. One atom pulls an electron from another atom.

2. Forming bonds releases energy and is exothermic.

3. Additional bonds require more energy to break, so the bond energy is higher.

4. −153

5. O–H bonds are polar covalent, and oxygen pulls the shared electrons toward it.

[quizlet: captncrun]

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1.How many mL of 0.401 M HI are needed to dissolve 5.97 g of BaCO3?
garri49 [273]

Answer:

The answer to your question is:

1.- volume = 0.151 l or 151 ml

2.- 0.241 l  or 241 ml of NaOH

Explanation:

1.-

Data

V = ? HI = 0.401 M

BaCO3 = 5.97 g

                     2HI(aq)    +    BaCO3(s)   ⇒   BaI2(aq) + H2O(l) + CO2(g)

MW BaCO3 = 137 + 12 + 48 = 197 g

                     197 g of BaCO3 ----------------- 1 mol

                     5.97 g                -----------------   x

                     x = (5.97 x 1) /197

                    x = 0.03 mol of BaCO3

                    2 moles of HI ----------------  1 mol of BaCO3

                    x                     ----------------  0.03 mol of BaCO3

                    x = (0.03 x 2) / 1

                   x = 0.060 mol of HI

Molarity = moles / volume

volume = moles / molarity

volume = 0.060 / 0.401

volume = 0.151 l or 151 ml

2.-

V = ?    NaoH 0.757 M

Co⁺² Volume = 167 ml   0.548 M

             CoSO4(aq) + 2NaOH(aq)   ⇒   Co(OH)2(s) + Na2SO4(aq)

Moles of Co = Molarity x  volume

Moles of Co = 0.548 x 0.167

Moles of Co = 0.092

                                 1 mol of CoSO4 -------------- 2 moles of NaOH

                                0.092 moles      ---------------   x

                                x = (0.092 x 2) /1

                               x = 0.183 moles of NaOH

Volume of NaOH = moles / molarity

                             = 0.183 / 0.757

                            = 0.241 l  or 241 ml of NaOH

6 0
3 years ago
What information is needed to calculate the percent composition of a compound
IrinaVladis [17]

Percent Composition by Mass. Percent composition is calculated from a molecular formula by dividing the mass of a single element in one mole of a compound by the mass of one mole of the entire compound. This value is presented as a percentage.

The best answer. :)

6 0
3 years ago
Read 2 more answers
What intermolecular forces can occur between a CO3<br> ion and H2O molecules? List them
Orlov [11]

Answer:

The intermolecular forces between CO3^2- and H2O molecules are;

1) London dispersion forces

2) ion-dipole interaction

3) hydrogen bonding

Explanation:

Intermolecular forces are forces of attraction that exits between molecules. These forces are weaker in comparison to the intramolecular forces, such as the covalent or ionic bonds between atoms in a molecule.

Considering CO3^2- and H2O, we must remember that hydrogen bonds occur whenever hydrogen is bonded to a highly electronegative atom such as oxygen. The carbonate ion is a hydrogen bond acceptor.

Also, the London dispersion forces are present in all molecules and is the first intermolecular interaction in molecular substance. Lastly, ion-dipole interactions exists between water and the carbonate ion.

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A gas occupies a volume of 10 liters at a pressure of 0.5 atm. What is the pressure if the volume increases to 25.0 L? *
Rudik [331]

Answer:

0.2atm

Explanation:

By Boyle's law

P1V1=P2V2

0.5 x 10 = P2 x 25

therefore, P2= 0.2atm

7 0
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Fofino [41]
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