Atoms And Molecules Class 9 Notes - Chapter 3

CBSE Class 9 Science Notes Chapter 3 Atoms And Molecules

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Atoms and molecules are responsible for forming tiny sand particles, gargantuan black holes and everything in between. The atom is the most fundamental unit of matter, making up everything that we see around us. It is extremely small, measuring in at less than 0.1 to 0.5 nanometers.

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Laws of Chemical Combination

Chemical Reactions

• In a chemical reaction, two or more molecules interact to produce new compounds; they are called reactants, whereas the newly formed compounds are called products.
• In a chemical reaction, a chemical change must occur, which is generally observed with physical changes like precipitation, heat production, colour change, etc.

Law of Conservation of Mass

• According to the law of conservation of mass, matter can neither be created nor destroyed in a chemical reaction. It remains conserved.
• The mass of reactants will be equal to the mass of products.

Law of Constant Proportions

• A pure chemical compound containing the same elements combined together in a fixed proportion by mass is given by the law of definite proportions.
• For e.g., If we take water from a river or from an ocean, both have oxygen and hydrogen in the same proportion.

The elements are present in chemical compounds in a predetermined mass ratio. The “Law of Constant Proportions” is this. This “Law of Constant Proportions” is also known as “Proust’s law” or the “law of defined proportions.” For instance, the oxygen and hydrogen content in pure water is always 1:8.

Atoms

An atom is the defining structure of an element, which cannot be broken by any chemical means.

The atomic symbol has three parts:-

• The symbol X: the usual element symbol
• The atomic number A: equal to the number of protons
• The mass number Z: equal to the total number of protons and neutrons in an element.

Atomic Radius

The distance between an atom’s nucleus and outer electron shell. The atomic radius is calculated by measuring the distance between the nuclei of two identical atoms bonded together. Half this distance is the atomic radius.

Dalton’s Atomic Theory

According to Dalton’s Atomic Theory, atoms, which are indestructible and indivisible building blocks, make up all substances. Unlike other elements, which have atoms of different sizes and weights, an element’s atoms have all the same size and mass.

Dalton proposed that the concept of atoms could be used to explain the laws of conservation of mass and definite proportions. He proposed that atoms, which he described as “solid, massy, hard, impenetrable, moving particle(s)”, are the smallest, indivisible units of matter.

1. The matter is made up of indivisible particles known as atoms.
2. The properties of all the atoms of a given element are the same, including mass. This can also be stated as – all the atoms of an element have identical mass and chemical properties; atoms of different elements have different masses and chemical properties.
3. Atoms of different elements combine in fixed ratios to form compounds.
4. Atoms are neither created nor destroyed. The formation of new products (compounds) results from the rearrangement of existing atoms (reactants) in a chemical reaction.
5. The relative number and kinds of atoms are constant in a given compound.

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Atomic Mass

Atomic Mass and Atomic Mass Unit

• Atomic mass is the total of the masses of the electrons, neutrons, and protons in an atom, or in a group of atoms, the average mass.
• The mass of an atomic particle is called the atomic mass.
• This is commonly expressed as per the international agreement in terms of a unified atomic mass unit (AMU).
• It can be best defined as 1/12 of the mass of a carbon-12 atom in its ground state.

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Molecular mass

Molecular mass of an element is defined as the sum of the masses of the elements present in the molecule.

• Molecular mass is obtained by multiplying the atomic mass of an element by the number of atoms in the molecule and then adding the masses of all the elements in the molecule.

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Molecule

The smallest identifiable unit into which a pure substance may be divided while retaining its composition and chemical properties is a molecule, which is a collection of two or more atoms.

Molecules of Elements

A molecule is a collection of two or more chemically bound atoms, whether they are from the same element or another.

For example, when two hydrogen (H₂) atoms and one oxygen (O₂) atom interact, one water molecule is created.

Molecules of Compounds

Salts and molecular compounds are the two categories into which compounds can be divided. Covalent bonds hold the atoms together in molecular molecules. Ionic bonds hold it together in salts. Every compound is composed of one of these two types of bonds.

Actually, a compound is a kind of molecule. The atoms that join together must be distinct from one another for the substance to qualify as a compound. O₂, for instance, is a molecule, not a compound, due to its atomic connection with another oxygen atom. NaCl, however, is a compound since it is made up of two distinct atoms that are chemically bound together.

Mole Concept

Mole Concept & Avogadro Number

• In a substance, the amount of entities present. For e.g. atoms, molecules, and ions are defined as a mole. A mole of any substance is 6.022×10²³ molecules.
• The Mole concept is one of the most convenient ways of expressing the amount of reactants and products in the reaction.

The value of Avogadro’s number is approximately 6.022×10²³. The definition of Avogadro’s number is that it tells us the number of particles in 1 mole (or mol) of a substance. These particles could be electrons or molecules, or atoms.

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Molar Mass

Molar Mass

A substance is something which has mass and occupies space. The molar mass/molecular weight is actually the sum of the total mass in grams of the atoms present to make up a molecule per mole. The unit of molar mass is grams/mole.

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Atomic Valency

Molecules and Atomicity

A molecule is defined as the smallest unit of a compound that contains the chemical properties of the compound.

• The atomicity of an element is the number of atoms in one molecule of the element.
• For e.g., Hydrogen, nitrogen, oxygen, chlorine, iodine, and bromine all have two atoms in each of their molecules. So, the atomicity of hydrogen, nitrogen, oxygen, chlorine, iodine, and bromine is two each.

Structure of an Atom

• Atom is made of three particles; electron, proton and neutron.
• The centre of the atom is called the nucleus. The nucleus of an atom contains the whole mass of an atom.
• Electrons in an atom are arranged in shells/orbitals.

Valency

Valence electrons are those electrons which are present in the outermost orbit of the atom.

• The capacity of an atom to lose, gain or share valence electrons in order to complete its octet determines the valency of the atom.

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Writing Chemical Formulae

Compounds

• When two or more elements chemically combine in a fixed ratio by mass, the obtained product is known as a compound.
• Compounds are substances consisting of two or more different types of elements in a fixed ratio of its atoms.

Ions

• An ion is defined as an atom or molecule which has gained or lost one or more of its valence electrons, giving it a net positive or negative charge.
• A negatively charged particle is called an anion, and a positively charged particle is called a cation.

Ionic Compounds: Chemical Formula

Each constituent element in a chemical formula is identified by its chemical symbol, along with the relative number of atoms that make up each element. These ratios are used in empirical equations to start with a key element and then assign atom counts for the remaining elements in the compound in relation to the key element.

• Ionic compounds are chemical compounds in which ions are held together by specialised bonds called ionic bonds.
• An Ionic compound always contains an equal amount of positive and negative charge.
• For example: In calcium chloride, the ionic bond is formed by oppositely charged calcium and chloride ions.
  The calcium atom loses 2 electrons and attains the electronic configuration of the nearest noble gas (Ar). By doing so, it gains a net charge of +2.
  The two chlorine atoms take one electron each, thus gaining a charge of -1 (each) and attain the electronic configuration of the nearest noble gas (Ar).
  

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