Intro to Chemistry

Definition of Chemistry

• Chemistry is the scientific study of the composition, properties, and reactions of matter.

Branches of Chemistry

• Inorganic Chemistry: study of inorganic compounds, which are typically derived from mineral sources.
• Organic Chemistry: study of organic compounds, which are typically derived from living organisms.
• Physical Chemistry: study of the physical principles underlying chemical reactions and transformations.
• Analytical Chemistry: study of the analysis and identification of the chemical composition of substances.
• Biochemistry: study of the chemical processes that occur within living organisms.

Atomic Structure

• Atoms: the building blocks of matter, consisting of protons, neutrons, and electrons.
• Protons: positively charged particles that reside in the nucleus of an atom.
• Neutrons: particles with no charge that reside in the nucleus of an atom.
• Electrons: negatively charged particles that orbit the nucleus of an atom.

Periodic Table

• Periodic Table: a tabular display of the known elements, organized by their atomic number (number of protons in the nucleus).
• Elements: substances that consist of only one type of atom.
• Compounds: substances that consist of two or more different elements.

Chemical Bonding

• Chemical Bond: a force that holds atoms together in a molecule.
• Covalent Bond: a bond formed by the sharing of electrons between atoms.
• Ionic Bond: a bond formed by the transfer of electrons between atoms.

Chemical Reactions

• Chemical Reaction: a process in which one or more substances are converted into new substances.
• Reactants: the substances that are consumed in a chemical reaction.
• Products: the substances that are formed in a chemical reaction.
• Chemical Equation: a representation of a chemical reaction using chemical formulas and symbols.

Stoichiometry

• Stoichiometry: the study of the quantitative relationships between reactants and products in chemical reactions.
• Mole: a unit of measurement that represents 6.022 x 10^23 particles.
• Molar Mass: the mass of one mole of a substance.

Definition of Chemistry

• Chemistry is the scientific study of the composition, properties, and reactions of matter.

Branches of Chemistry

• Inorganic Chemistry studies inorganic compounds derived from mineral sources.
• Organic Chemistry studies organic compounds derived from living organisms.
• Physical Chemistry studies the physical principles underlying chemical reactions and transformations.
• Analytical Chemistry studies the analysis and identification of the chemical composition of substances.
• Biochemistry studies the chemical processes that occur within living organisms.

Atomic Structure

• Atoms are the building blocks of matter, consisting of protons, neutrons, and electrons.
• Protons are positively charged particles that reside in the nucleus of an atom.
• Neutrons are particles with no charge that reside in the nucleus of an atom.
• Electrons are negatively charged particles that orbit the nucleus of an atom.

Periodic Table

• The Periodic Table is a tabular display of the known elements, organized by their atomic number (number of protons in the nucleus).
• Elements are substances that consist of only one type of atom.
• Compounds are substances that consist of two or more different elements.

Chemical Bonding

• Chemical Bond is a force that holds atoms together in a molecule.
• Covalent Bond is a bond formed by the sharing of electrons between atoms.
• Ionic Bond is a bond formed by the transfer of electrons between atoms.

Chemical Reactions

• Chemical Reaction is a process in which one or more substances are converted into new substances.
• Reactants are the substances that are consumed in a chemical reaction.
• Products are the substances that are formed in a chemical reaction.
• Chemical Equation is a representation of a chemical reaction using chemical formulas and symbols.

Stoichiometry

• Stoichiometry is the study of the quantitative relationships between reactants and products in chemical reactions.
• Mole is a unit of measurement that represents 6.022 x 10^23 particles.
• Molar Mass is the mass of one mole of a substance.

Elements

• The term "element" was introduced by French chemist Lavoisier, who defined it as the simplest or basic form of a pure substance that cannot be broken down further by physical or chemical means.
• Elements are classified into three types based on their properties: Metals, Non-metals, and Metalloids.

Types of Elements

• Metals: Can form positive ions by losing electrons. Examples: Na, Mg.
• Non-metals: Form negative ions by gaining electrons. Examples: C, P.
• Metalloids: Show properties of both metals and non-metals.

Comparison of Metals and Non-metals

• Malleability and Ductility: Metals are malleable and ductile, while non-metals are brittle.
• Conductivity: Metals are good conductors of heat and electricity, while non-metals are poor conductors (except diamond and graphite).
• Appearance: Metals are lustrous and can be polished, while non-metals are non-lustrous and cannot be polished (except iodine).
• State at Room Temperature: Metals are typically solid, while non-metals may be solid, liquid, or gaseous.
• Strength and Tensile Strength: Metals are strong and tough, while non-metals are generally soft and have low tensile strength (except diamond).
• Sonorousness: Metals are sonorous, while non-metals are not.
• Melting and Boiling Points: Metals have high melting and boiling points, while non-metals have relatively low melting and boiling points (except graphite).
• Density: Metals have high densities, while non-metals have low densities (except iodine).
• Color: Metals usually have a silver or grey color (except gold and copper), while non-metals have various colors.

Compounds

• A compound is a pure substance composed of two or more elements combined chemically in a fixed proportion by mass.
• Compounds are classified into two types: Inorganic and Organic.

Characteristics of Compounds

• Composition: A pure compound is composed of the same elements combined in a fixed ratio by mass.
• Homogeneity: A pure compound is homogeneous in nature.
• Formation: A chemical compound is formed as a result of a chemical reaction between constituent elements.
• Separation: Constituents of a chemical compound cannot be separated mechanically.
• Energy Changes: Formation of compounds involves energy changes.
• Melting and Boiling Points: Compounds have sharp melting and boiling points.