BCF - Bonding and Chemical Formulas (Module Overview)
Bonding and Chemical Formulas
Introduction
Have you ever wondered about where the facts come from in your science textbooks? How do scientists attempt to determine how the natural world works? How certain can they be about their findings?
Elements combine to form ionic compounds, covalent compounds, also known as molecules, and metals. In this module, we will learn the process that elements undergo to transfer electrons, which results in ionic bonds. We will also look at how electrons are shared between atoms, both equally and unequally, to result in covalent bonds. We will also determine which conditions are favorable for each type of bond. In addition to ionic and covalent bonding, we will touch on metallic bonding. We will draw electron dot diagrams and use those diagrams to draw more complex Lewis structures. Ideas introduced in this module will be important in every module that follows.
Please Note: This module contains an at home lab that requires the following materials: baking soda, vegetable oil, table sugar, and table salt. Please have these materials available.
This module gives you a window into the scientific process and scientific thought.
Module Lessons Preview
In this module, we will study the following topics:
Introduction to Chemical Bonding
Lewis Dot Structures
Intramolecular Bonding
Intermolecular Bonding
Covalant Naming and Formulas
Ionic Naming and Formulas
Key Terms
Valence electron - An electron in an outer shell of an atom that can participate in forming chemical bonds with other atoms.
Chemical bond – An electrical interaction between a positively charged nuclei and negatively charged electrons of atoms that forms when the force of attraction is stronger than the force of repulsion
Ionic bond - A chemical bond between two ions with opposite charges, characteristic of salts.
Covalent bond - A chemical bond formed by the sharing of one or more electrons, especially pairs of electrons, between atoms.
Metallic bond - The chemical bond characteristic of metals, in which mobile valence electrons are shared among atoms in a usually stable crystalline structure.
Electrostatic Force - A force in which oppositely charged particles are attracted to each other, while like charges repel each other
Hydrogen bond - A chemical bond in which a hydrogen atom of one molecule is attracted to an electronegative atom, especially a nitrogen, oxygen, or fluorine atom, usually of another molecule.
Delocalized - electrons in a molecule or solid metal that are not associated with a single atom or one covalent bond.
Crystal lattice - A geometric arrangement of the points in space at which the atoms, molecules, or ions of a crystal occur.
Volatile - Evaporating readily at normal temperatures and pressures.
Ion - An atom or a group of atoms that has acquired a net electric charge by gaining or losing one or more electrons.
Cation - An ion or group of ions having a positive charge and characteristically moving toward the negative electrode in electrolysis.
Anion - A negatively charged ion
Intermolecular Force - The force between two molecules; it is that negative gradient of the potential energy between the interacting molecules, if energy is a function of the distance between the centers of the molecules.
Dispersion Force - a weak intermolecular force arising from quantum induced instantaneous dipoles in molecules
Ion-Diploe Force – Attractive forces between an ion and a polar molecule
Dipole-dipole Force – the attractive force between polar molecules
Polar - A covalent bond between two atoms where the electrons are unequally distributed or shared
Nonpolar - A covalent bond between two atoms where the electrons are equally distributed or shared
Electron dot diagram - A structural formula in which electrons are represented by dots; two dots between atoms represent a covalent bond. Also known as electron-dot formula; Lewis formula.
Lewis structure - A structural formula in which electrons are represented by dots; two dots between atoms represent a covalent bond. Also known as electron-dot formula; Lewis formula.
Ionic compound - a chemical compound in which ions are held together in a lattice structure by ionic bonds.
Molecular compound - The smallest particle of a substance that retains the chemical and physical properties of the substance and is composed of two or more atoms bonded together by the sharing of electrons
Subscripts - A distinguishing character or symbol written directly beneath or next to and slightly below a letter or number. In chemical formula writing, the subscript denotes how many atoms or ions of a particular element or polyatomic ion are present.
Nomenclature - A system of naming chemical compounds and for describing the science of chemistry in general. It is maintained by the International Union of Pure and Applied Chemistry (IUPAC).
Polyatomic ions - An electrically charged species formed by covalent bonding of atoms of two or more different elements, usually nonmetals, for example, the ammonium ion(NH4+)
IMAGES CREATED BY GAVS OR FREE TO USE