The particles that substance are made of
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The document discusses the structure and composition of compounds. It explains that compounds are made up of two or more different types of atoms bonded together, and that there are different types of bonds - covalent, ionic, and metallic. It also discusses how to represent compounds using chemical formulae, as well as stick-and-ball models and space-filling models. The key information provided is about the basic units that make up matter at the atomic level and how atoms combine to form compounds through different bonding mechanisms.
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bonding
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Covalent bonding occurs when atoms share valence electrons to form stable molecular structures. Lewis structures use dots to represent these shared and unshared electron pairs, following the octet rule which states that atoms seek a full outer shell of 8 electrons. Exceptions exist for some atoms. Polar covalent bonds form when electrons are unequally shared between atoms, resulting in a partial positive and negative charge.
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The document discusses Valence Shell Electron Pair Repulsion (VSEPR) Theory. VSEPR Theory states that the shape of a molecule is determined by the number of electron pairs around the central atom. Electron pairs repel each other and arrange as far apart as possible. Bond pairs and lone pairs cause repulsion, with lone pairs causing more repulsion than bond pairs. The geometry that results in the lowest repulsion determines the molecular shape. Common molecular shapes include linear, trigonal planar, and tetrahedral.
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Phys. Sci Ch 8
This document provides instructions for navigating a presentation on chemical bonding. It describes how to view the presentation as a slideshow, advance through slides, access resources and lessons, and exit the slideshow. The presentation covers topics like electrons and chemical bonding, ionic bonds, and covalent and metallic bonds. It includes bellringer questions, learning objectives, content on topics like ion formation and crystal lattices, and a concept map to summarize the key topics.
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Here are the key points about polar and nonpolar covalent bonds:
- Nonpolar covalent bonds form between atoms with similar electronegativity. Electrons are equally shared. Examples include H2, Cl2, etc.
- Polar covalent bonds form between atoms with different electronegativity. Electrons are unequally shared, resulting in partial positive and negative charges on the atoms. Examples include HCl, H2O.
- Polar molecules are attracted to each other due to their partial charges. They are soluble in polar solvents like water. Nonpolar molecules are not attracted and are soluble in nonpolar solvents like hexane.
- Most bonds have some ionic character based on electrone
Chemunit7presentation 120104184804-phpapp02
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Chapter 2 Bonds and Compounds w-clips
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The ring forms of glucose and galactose have the same molecular formula and connectivity between atoms. They are not considered structural isomers because the atoms are connected in the same way.
They are geometric isomers because even though they have the same molecular formula and connectivity, their three-dimensional spatial arrangements are different due to the orientation of the hydroxyl group on carbon 5. This makes them geometric isomers.
Chemical bonds Shafeen Qazi
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Chemical bonds
A chemical bond forms when atoms combine together. There are three main types of bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form when a cation and anion combine through electrostatic attraction. Covalent bonds form when atoms share one or more pairs of electrons to fill their outer electron shells. Metallic bonds form a sea of electrons that positively charged metal ions are dissolved within.
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