Which of the following would most likely happen if water did not form hydrogen bonds?A) Water would exist only as a solid.

B) Water would be able to dissolve all ionic compounds.

C) Water would not expand when it freezes.

D) Water would not exist on Earth.

Answers

Answer 1

Answer:

The hydrogen bond is a secondary bond formed between a hydrogen (attached to an highly electronegative element ,: F, O or N) and another atom of an highly electronegative element ,: F, O or N.

In case of water hydrogen bond helps water

a) to dissolve certain substances which can make hydrogen bond

b) it makes it liquid and room temperature unlike H2S which is a gas at room temperature due to absence of hydrogen bond

c) higher volume and low density of ice as compared to liquid water. Due to hydrogen bond ice forms open cage like structure which increases its volume and decreases its density. Thus water expands on freezing

So in absence of hydrogen bond Water would not expand when it freezes.

Answer 2

Answer: Water would not expand when it freezes.

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Why is mass conserved in
chemical reactions?

Answers

Even in a chemical reaction when atoms interact and create new products, mass is conserved. This is because the new substances created are composed of atoms that were present in the reactants. ... No new atoms have entered or left the system so the mass is conserved.

How many lone pairs of electrons are represented in the Lewis structure of a phosphate ion (PO43-)? 10 12 21 24

Answers

To illustrate the Lewis structure,
P has 5 valence electrons
O has 6 valence electrons (each for 4 oxygen)
And finally, for every negative charge, there is an additional valence electron

We should add these all up = 5 + 24 + 3 = 32 valence electrons

With this, we can be guided to illustrate the lewis structure as P as central atom and the 3 oxygen each with a single bond with P and 1 oxygen with a double bond with P. We place the valence electrons until octet rule is satisfied,
we will be left with 12 lone pairs for phosphate ion.

Explain how the system of the flask and the balloon illustrates the conservation of mass.

Answers

The mass of the reaction system is conserved because, the mass lost from the reaction by the evolution of gas is collected inside a balloon to inflate it. Thus , the balloon and the flask creates a closed system where no mass is lost outside.

What is conservation of mass?

According to the law of conservation of mass, the mass can neither be created nor be destroyed. Thus the total mass of the system is conserved. However similar to the energy, mass can be transformed into energy.

As per this law, the total mass in a chemical reaction is conserved. Where, the total mass in the reactant side is equal to the total mass in the product side.

When the reaction flask is closed with a balloon, the gas if any evolved from the reaction will be collected to the balloon and it inflates. Thus the mass lost from the reaction system does not goes to the surroundings due to the closed system.

To find more on mass conservation, refer here:

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Both containers prevent the escape of matter of the reaction into an uncontrolled space, therefore it is a closed system (not isolated, since energy can still go in and out).

The longer the bond, the smaller the bond enthalpy. the longer the bond, the smaller the bond enthalpy. false true

Answers

True

As the shorter the bond, the stronger it is hence more energy will be required to overcome this bond

Final answer:

The statement 'The longer the bond, the smaller the bond enthalpy' is true as bond length and bond enthalpy have an inverse relationship. As bond strength increases (with an increase in electron pairs in the bond), bond length decreases. So longer bonds, indicating weaker bonding, have smaller bond enthalpies.

Explanation:

The statement 'The longer the bond, the smaller the bond enthalpy' is true. The bond length and bond enthalpy have an inverse relationship. As the strength of a bond increases with the increase in the number of electron pairs, the bond length decreases. Thus, triple bonds are generally stronger and shorter than double bonds between the same two atoms, and by the same logic, double bonds are stronger and shorter than single bonds.

For example, if we consider the bonds between carbon and various atoms in a group, we find the bond strength typically decreases as we move down the group - C-F has a bond enthalpy of 439 kJ/mol, C-Cl has 330 kJ/mol, and C-Br is at 275 kJ/mol.

The bond energy, essentially the enthalpy required to break the bond, is a representation of its strength. Thus, a longer bond, indicating weaker bonding, will have a smaller bond enthalpy.