Organic and Inorganic Chemistry Overview

Organic Chemistry

• Organic chemistry is the study of carbon-containing compounds, including hydrocarbons and their derivatives.
• All organic compounds contain carbon.
• Most contain carbon-hydrogen bonds (C-H).
• Organic chemistry uses covalent bonds (sharing of electrons).

Inorganic Chemistry

• Inorganic chemistry is the study of all other chemical compounds excluding carbon-based compounds.
• Most inorganic compounds do not contain carbon.
• Inorganic chemistry uses ionic bonds (electrostatic attraction).
• Organic chemistry and inorganic chemistry make up the entire field of chemistry

Carbon: The Chemistry of Life

• Carbon is the fundamental element of life on Earth.
• Carbon atoms have four valence electrons, allowing them to form four covalent bonds with other atoms.
• Long chains of carbons allow for complex structures.
• Carbon-carbon bonds can be single, double, or triple bonds.
• Carbon forms the basis of large molecules (polymers) including proteins, carbohydrates, and nucleic acids.

Carbon Cycle

• Carbon is in a continuous cycle between the atmosphere, oceans, and living organisms.
• Photosynthesis is a key process where plants use carbon dioxide from the air in the presence of sunlight and water.
• Plant respiration is also key to the cycle, as plants release carbon back into the atmosphere.
• Decomposition returns carbon to the soil or oceans.
• Ocean sediment carbon stores carbon long-term.

Periodic Table

• The periodic table organizes elements by atomic number and properties.
• Elements are arranged into periods (rows) and groups (columns).
• Elements in the same group have similar properties.
• Electronegativity increases across a period and up a group.
• Metals and nonmetals are organized and grouped in specific areas of the periodic table.
• Transition and inner transition metals also appear in distinct blocks.
• All elements have valence electrons which are either in s, p, d, or f orbitals

Bonds

• Covalent Bonds: Atoms share electrons to achieve a stable electron configuration.

• Ionic Bonds: Atoms transfer electrons to form positively and negatively charged ions, which attract each other.

• Types of Bonds: Covalent, Ionic, Metallic, Hydrogen

Valence Electrons

• Valence electrons are the electrons in the outermost shell of an atom.
• Valence electrons determine an atom's bonding behavior.
• The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full valence shell of eight electrons (except H and He).

Orbital Types

• s, p, d orbitals have different shapes and orientations in space.
• 1s, 2s, 2p, 3s, 3p, 3d etc, are examples of orbital names and types.

Hybridization

• Hybrid orbitals are formed by combining atomic orbitals.
• They explain the shapes and bond angles of molecules.
• Types of hybridization include sp, sp2, and sp3.

Lewis Structures

• Lewis structures show the arrangement of atoms and electrons in a molecule.
• Lewis structures help predict and understand the bonding and shape of molecules.

Organic Reactions

• Chemical reactions involving carbon compounds are important in many applications.
• Organic reactions can include addition, substitution, elimination reactions.

SN1 and SN2 Reaction Mechanisms

• SN1 reactions are unimolecular and have a rate-determining step.
• SN2 reactions are bimolecular and have a concerted reaction mechanism.

Stereoisomerism

• Organic molecules with the same formula but different spatial arrangements are called stereoisomers.
• Chiral molecules have non-superimposable mirror images.
• Enantiomers are pairs of chiral molecules that are mirror images of each other.

This quiz explores the fundamental concepts of organic and inorganic chemistry, highlighting the role of carbon in life and molecular structures. Understand the differences between these two branches of chemistry, including the types of bonds involved. Test your knowledge on carbon-based compounds and their significance in various chemical processes.