Branches of Chemistry

Branches of Chemistry

• Inorganic Chemistry: Studies the properties and reactions of inorganic compounds, which are typically derived from mineral sources.
• Organic Chemistry: Focuses on the properties and reactions of organic compounds, which are typically derived from living organisms.
• Physical Chemistry: Examines the physical principles underlying chemical reactions and processes.
• Analytical Chemistry: Deals with the analysis and identification of the chemical composition of substances.
• Biochemistry: Explores the chemical processes that occur within living organisms.

Atomic Structure

• Atoms: The smallest units of matter that retain the properties of an element.
• Protons: Positively charged particles found in the nucleus of an atom.
• Neutrons: Neutral particles found in the nucleus of an atom.
• Electrons: Negatively charged particles that orbit the nucleus of an atom.
• Valence Electrons: Electrons in the outermost energy level of an atom, involved in chemical bonding.

Chemical Bonding

• Ionic Bonding: The transfer of electrons between atoms to form ions with opposite charges.
• Covalent Bonding: The sharing of electrons between atoms to form a molecule.
• Hydrogen Bonding: A type of weak bond between atoms with a hydrogen atom bonded to a highly electronegative atom.
• Polar Covalent Bonding: A type of covalent bond where electrons are shared unequally, resulting in a partial positive and negative charge.

Chemical Reactions

• Chemical Equation: A representation of a chemical reaction using chemical formulas and symbols.
• Reactants: The substances that undergo a chemical change in a reaction.
• Products: The substances formed as a result of a chemical reaction.
• Catalysts: Substances that speed up a chemical reaction without being consumed by the reaction.
• Activation Energy: The minimum energy required for a chemical reaction to occur.

Stoichiometry

• Mole: A unit of measurement that represents 6.022 x 10^23 particles.
• Molar Mass: The mass of one mole of a substance.
• Empirical Formula: The simplest whole-number ratio of atoms in a compound.
• Molecular Formula: The actual number of atoms in a molecule of a compound.

Branches of Chemistry

• Inorganic chemistry studies properties and reactions of inorganic compounds, derived from mineral sources.
• Organic chemistry focuses on properties and reactions of organic compounds, derived from living organisms.
• Physical chemistry examines underlying physical principles of chemical reactions and processes.
• Analytical chemistry deals with analysis and identification of chemical composition of substances.
• Biochemistry explores chemical processes within living organisms.

Atomic Structure

• Atoms are smallest units of matter retaining properties of an element.
• Protons are positively charged particles in the nucleus of an atom.
• Neutrons are neutral particles in the nucleus of an atom.
• Electrons are negatively charged particles orbiting the nucleus of an atom.
• Valence electrons are electrons in the outermost energy level of an atom, involved in chemical bonding.

Chemical Bonding

• Ionic bonding involves transfer of electrons between atoms to form ions with opposite charges.
• Covalent bonding involves sharing of electrons between atoms to form a molecule.
• Hydrogen bonding is a weak bond between atoms with a hydrogen atom bonded to a highly electronegative atom.
• Polar covalent bonding is a type of covalent bond where electrons are shared unequally, resulting in partial positive and negative charge.

Chemical Reactions

• Chemical equations represent chemical reactions using chemical formulas and symbols.
• Reactants undergo chemical change in a reaction.
• Products are formed as a result of a chemical reaction.
• Catalysts speed up a chemical reaction without being consumed by the reaction.
• Activation energy is the minimum energy required for a chemical reaction to occur.

Stoichiometry

• A mole is a unit of measurement representing 6.022 x 10^23 particles.
• Molar mass is the mass of one mole of a substance.
• Empirical formula represents the simplest whole-number ratio of atoms in a compound.
• Molecular formula represents the actual number of atoms in a molecule of a compound.