Atoms are bonded together in molecules via bonds. Intramolecular bonds are the interactions between atoms within a molecule. Intermolecular bonds are the interactions between atoms in different molecules.

Covalent bond: A covalent bond is formed when two nuclei share two electrons. Electrostatic forces draw electrons (negatively charged) toward both positively charged nuclei.

Hydrogen bond: Dipole forces are used to form hydrogen bonds. A hydrogen bond is the attraction between hydrogen attached to one molecule's electronegative atom and hydrogen bonded to another molecule's electronegative atom. Nitrogen, fluorine, or oxygen, which have a partial negative charge, are commonly used as electronegative atoms. After then, the hydrogen has a partial positive charge.

Ionic bond: An ionic bond is a chemical link that is formed by electrostatic attraction between ions with opposite charges. In ionic compounds, it is the most important interaction. Atoms that have gained one or more electrons (anions – negatively charged) and atoms that have lost one or more electrons (cations – positively charged) make up the ions (cations - positively charged).

Van der Waals interactions: This is the intermolecular interaction of electron clouds between molecules. Van der Waals interactions are the least powerful of all intermolecular interactions.

Intermolecular interactions between nonpolar compounds are known as hydrophobic interactions.

When one or more elements are present in a specific ratio, a compound is formed. Water, for example, is a chemical with a fixed ratio of oxygen and hydrogen.

The simplest whole number ratio between the number of atoms of the different elements in the compound is the empirical formula of a pure compound. The empirical formula for glucose, for example, is CH2O.

A molecule's molecular formula specifies the exact amount of atoms that make up the molecule. C6H12O6 is the chemical formula for glucose.

The cation and anion of ionic substances are given names. The cation name comes before the anion name when naming an ionic compound. When the cation Na+ and anion Cl- or NaCl are joined, sodium chloride is formed.

The suffix –ide is applied to monoatomic and polyatomic ions. H- is a hydride ion, while OH- is a hydroxide ion, for example.

Reactants are the compounds that react first in a chemical reaction. In a chemical equation, reactants are always written on the left side. The chemical reaction's products are the

chemicals that are created during the reaction. A chemical equation's products are always written on the right-hand side.

The law of conservation of mass asserts that during a chemical reaction, the number of atoms of a given element remains constant.

In a reaction, an element is said to be oxidised if its oxidation number increases, and reduced if it drops.

If both of the following assertions are true, a substance is elemental: There is only one type of atom present. If the charge is zero, Examples: S8: S has an oxidation number of 0. Fe has an oxidation number of 0.

A monoatomic ion's oxidation number is equal to the ion's charge. S2- has an oxidation number of -2, while Al3+ has an oxidation number of +3.

All Group 1 metals have an oxidation number of +1. (unless elemental). All Group 2 metals have an oxidation number of +2. (unless elemental).

Hydrogen (H) can be oxidised in two ways: When connected to a nonmetal, gain +1. When bound to a metal, the value is -1.

There are two possible oxidation values for oxygen (O): -1 in peroxides (O22-) is unusual. In all other compounds, -2 is the most common.

Fluorine (F) has an oxidation number of -1.

In a neutral molecule, the sum of all atoms' (or ions') oxidation numbers equals 0. The charge on a polyatomic ion is equal to the sum of all atoms' oxidation numbers.

An oxidising agent will produce oxidation while also reducing the agent itself. A reducing substance will cause reduction while also being oxidised. When something is reduced, electrons are gained. When something gets oxidised, electrons are lost.

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Atoms and molecules summary part 2

Module: General and Organic Chemistry (AOC106DI)

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Atoms are bonded together in molecules via bonds. Intramolecular bonds are the

interactions between atoms within a molecule. Intermolecular bonds are the interactions

between atoms in different molecules.

Covalent bond: A covalent bond is formed when two nuclei share two electrons.

Electrostatic forces draw electrons (negatively charged) toward both positively charged

nuclei.

Hydrogen bond: Dipole forces are used to form hydrogen bonds. A hydrogen bond is the

attraction between hydrogen attached to one molecule's electronegative atom and

hydrogen bonded to another molecule's electronegative atom. Nitrogen, fluorine, or oxygen,

which have a partial negative charge, are commonly used as electronegative atoms. After

then, the hydrogen has a partial positive charge.

Ionic bond: An ionic bond is a chemical link that is formed by electrostatic attraction

between ions with opposite charges. In ionic compounds, it is the most important

interaction. Atoms that have gained one or more electrons (anions – negatively charged) and

atoms that have lost one or more electrons (cations – positively charged) make up the ions

(cations - positively charged).

Van der Waals interactions: This is the intermolecular interaction of electron clouds between

molecules. Van der Waals interactions are the least powerful of all intermolecular

interactions.

Intermolecular interactions between nonpolar compounds are known as hydrophobic

interactions.

When one or more elements are present in a specific ratio, a compound is formed. Water,

for example, is a chemical with a fixed ratio of oxygen and hydrogen.

The simplest whole number ratio between the number of atoms of the different elements in

the compound is the empirical formula of a pure compound. The empirical formula for

glucose, for example, is CH2O.

A molecule's molecular formula specifies the exact amount of atoms that make up the

molecule. C6H12O6 is the chemical formula for glucose.

The cation and anion of ionic substances are given names. The cation name comes before

the anion name when naming an ionic compound. When the cation Na+ and anion Cl- or

NaCl are joined, sodium chloride is formed.

The suffix –ide is applied to monoatomic and polyatomic ions. H- is a hydride ion, while OH-

is a hydroxide ion, for example.

Reactants are the compounds that react first in a chemical reaction. In a chemical equation,

reactants are always written on the left side. The chemical reaction's products are the

Atoms and molecules summary part 2

General and Organic Chemistry (AOC106DI)

Coventry University

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Atoms and molecules summary part 2

Module: General and Organic Chemistry (AOC106DI)

University: Coventry University

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