NCERT solutions for Science Exploration [English] Class 9 chapter 9 - Atomic Foundations of Matter [Latest edition]

A student burns 10 g of ethanol in an open beaker. After the reaction, no residue is left in the beaker. Does this mean the Law of Conservation of Mass is violated? Explain.

When 20 g of hydrogen reacts completely with 160 g of oxygen, how much water is formed according to the Law of Conservation of Mass?

A compound consists of 40% sulfur and 60% oxygen by mass. In a sample of the same compound containing 20 g of sulfur, what mass of oxygen must be present to satisfy the Law of Constant Proportions?

Carbon monoxide (CO) contains carbon and oxygen in the mass ratio of 3:4. How much oxygen will combine with 9 g of carbon to form carbon monoxide?

The Law of Definite Proportions holds true for compounds but not for mixtures. Give reason.

Students X and Y, both prepared an oxide of copper by combining copper and oxygen in the ratios of 4:1 and 8:2, respectively. Do their results justify the Law of Constant Proportions? Explain.

atoms could combine in any ratio and not in a fixed ratio? How would this affect the substances around us?

Assertion (A): 2 g of hydrogen combines with 16 g of oxygen to form 18 g of water.

Reason (R): According to Dalton’s Atomic Theory, atoms combine in a simple whole number ratio by mass to form compounds.

Choose the correct option:

Nitrogen has five valence electrons. Draw the structure of the nitrogen molecule $$\left(\mathrm{N}_{2}\right).$$

The atomic number of fluorine is 9. Explain the formation of the fluorine molecule $$\left(\mathrm{F}_{2}\right).$$

Show the formation of the following molecule:

Carbon dioxide CO₂

Show the formation of the following molecule:

Hydrogen sulfide H₂S

Show the formation of the following molecule:

Ammonia NH₃

Neon (atomic number 10) neither transfers nor shares its valence electrons. Explain.

We could see atoms directly? How would it help scientists and what challenges would it cause?

What kind of ion will oxygen (O) form?

Among magnesium and chlorine, magnesium atom can give two electrons to become \(\mathrm{Mg}^{2+}\). However, chlorine can take only one electron to become ______ Now, ______ ion of magnesium and ______ ions of chlorine combine to give magnesium chloride.

Show the formation of cations of potassium (K) and calcium (Ca) atoms, and the formation of their corresponding chlorides using diagrams.

Illustrate how sodium sulfide (Na₂S) is formed.

Name the following:

$$(\mathrm{CO}_{2})$$ ______

Name the following:

$$(\mathrm{NO}_{2})$$ ______

Name the following:

$$(\mathrm{SF}_{6})$$ ______

Name the following:

$$(\mathrm{PCl}_{3})$$ ______

Write the formula for the following:

Sodium hydrogencarbonate ______

Write the formula for the following:

Sulfur dioxide

Write the formula for the following:

Ferric chloride ______

Write the formula for the following:

Cuprous oxide

Write the formulae for the compound formed from the following pairs of ions:

$$\mathrm{Fe}^{3+}$$ and $$\mathrm{OH}^{-}$$

Write the formulae for the compound formed from the following pairs of ions:

$$\mathrm{K}^{+}$$ and $$\mathrm{CO}_{3}^{2-}$$

What type of chemical bond is present in a solid compound that does not conduct electricity in the solid state but conducts electricity when dissolved in water?

Metal M, with two electrons in its valence shell (M shell), reacts with oxygen to form a compound that is slightly soluble in water. Predict its:

1. formula
2. type of bond
3. electrical conductivity of its aqueous solution

Find the molecular mass of nitric acid $$(\mathrm{HNO}_{3})$$. 
Atomic mass - $$(\mathrm{H}=1 \mathrm{u} ; \mathrm{N}=14 \mathrm{u} ; \mathrm{O}=16 \mathrm{u})$$.

Find the molecular mass of methane $$(\mathrm{CH}_{4})$$. 
Atomic mass - $$(\mathrm{C}=12 \mathrm{u} ; \mathrm{H}=1 \mathrm{u})$$.

Find the formula unit mass of potassium chloride (KCl).

Atomic mass- $$(\mathrm{K}=39 \mathrm{u} ; \mathrm{Cl}=35.5 \mathrm{u})$$.

Find the formula unit mass of magnesium hydroxide, $$\mathrm{Mg}(\mathrm{OH})_{2}.$$
Atomic mass - $$\mathrm{Mg}=24 \mathrm{u} ; \mathrm{O}=16 \mathrm{u} ; \mathrm{H}=1 \mathrm{u}$$.

A particular element (A) has one electron in its third shell. There is another element (B) with six electrons in its second shell.

1. How many electrons does A tend to give or take to become stable?
2. What kind of ion would it form? 
3. How many electrons does B tend to give or take to become stable? 
4. What kind of ion would it form? 
5. If A and B were to combine, what kind of bond would be formed?
6. What would be the formula for the compound thus formed?

An element X has six electrons in its outer shell and forms a diatomic molecule.

1. Why would that be so? 
2. What kind of bond would it form?
3. Draw the structure of the molecule it would form. 
4. A certain other element Y has two electrons in its second shell. Draw the structure of the molecule that X would form with Y.

You want to design a new ionic compound, where the total positive charge is 6+ and the total negative charge is 6−. Which of the following combinations gives the correct number of ions? 

Choose the correct statement(s) and correct the false statement(s).