charge. Hydrogen bonding is generally stronger than most bonds bar covalent bonds. Water: Bonding within water molecules occur between oxygen and hydrogen. These covalent bonds mean that the electrons are shared between the oxygen and hydrogen atoms to create a complete valence shell. However‚ electrons tend to spend more time around the oxygen atom due to its higher electro-negativity. This creates a partial positive charge around the hydrogen atoms‚ and a partial negative charge around the oxygen
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two atoms Valence electron – the outer most shell electrons There are three types of chemical bonding i. Ionic bond: ________________________________________ ii. Covalent bond: _____________________________________ iii. Dative Covalent bond: _______________________________ 1.1.1 LEWIS DOT SYMBOL A shorthand to represent the valence electron of an atom. The element symbol surrounded by dots that represent the valence electrons. The Lewis structures for
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(substance that cannot be broken down into further substances) Atom (smallest unit of an element) – subatomic particles (neutrons‚ protons‚ electrons) Compound (2 or more) Atomic number - # of protons Atomic mass = # of neutrons and protons Ion – total number of electrons doesn’t equal # of protons (anion gained electrons‚ cation lost electrons) Electron shells‚ orbitals‚ valency‚ rule of 8 Bonds = ionic‚ covalent (polar‚ nonpolar)‚ hydrogen‚ Van der walls Electronegativity Relationship of
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in the periodic table. Both the alkali metals and the halogens (nonmetals) on considered to be main group elements. When the number of outer shell electrons is closer to one or seven the higher the elements reactivity. Alkali metals contain a single electron in their outer shell which makes them highly reactive and halogens contain only seven electrons in their outer shell. Noble gases‚ such as helium‚ are not reactive because they are chemically stable and will not combine with other elements. H₂S
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Current ‚ Voltage‚ and Resistance [pic] A. The Electrical Nature of Matter All atoms are made up of protons‚ neutrons‚ and electrons. The classical model of the atom consists of a positively charged nucleus made up of protons and neutrons‚ and a number of negatively charged electrons in orbit about the nucleus. The simplest form of the model pictures electrons as tiny particles which circle the nucleus in definite orbits similar to the orbits of the planets about the sun. Though this model
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Name Period Date Molecular Geometry – Ch. 9 For each of the following molecules‚ draw the Lewis Diagram and tally up the electron pairs. Then‚ identify the correct the molecular shape and bond angle. molecule lewis diagram e- tally shape bond angle 1. SeO3 2. AsH3 3. NO2 - 4. BeF2 molecule lewis diagram e- tally shape bond angle 5. SiH4 6. SeH2 7. PF5 8. SCl6 Name:
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through ordinary matter almost unaffected. The neutrino (meaning "small neutral one") is denoted by the Greek letter ν (nu). Neutrinos are similar to the more familiar electron‚ with one crucial difference: neutrinos do not carry electric charge‚ which means that they are not affected by the electromagnetic forces which act on electrons. Neutrinos are affected only by the weak sub-atomic force‚ of much shorter range than electromagnetism‚ and gravity‚ which is relatively weak on the subatomic scale
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charges repel‚ unlike charges attract. Electrons and protons have‚ to fantastic accuracy‚ equal and opposite charges. Quarks have 1/3 the electron charge but are never seen alone! In wires electrons do the moving to carry electrical current. In solutions or plasmas there can be positive charge carriers‚ ions or protons. Although the signal to tell electrons to move in wires travels at about 2/3 the speed of light (FAST in laymen’s terms) the electrons only travel at a person’s walking pace
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or part of Mr. Cohn. d) Atoms can bond ionically‚ whereby an atom gives up valence electrons and becomes a + ion‚ and another atom receives those electrons and becomes a – ion. The overall charge on the molecule then becomes zero. e) Atoms can bond covalently‚ whereby atoms share valence electrons‚ such that all atoms involved complete their valence rings (usually with a total of 2 or 8 electrons) f) Determining if atoms will bond ionically or covalently can often be done by noting
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intermolecular forces. 1+1 1 1 (ii) There are mobile electrons in solid sodium but the ions in solid sodium chloride are not free to move/ solid sodium chloride has no mobile ion. 1 1 (iii) Tetrachloromethane which is a covalent compound‚ does not possess any mobile electrons (ions)/ exists as (discrete) molecules in liquid state‚ therefore is not an electrical conductor 1 1993 - 4(a) Marking Scheme (i) Group II/ 2 Because W has 2 electrons in its outer/ outermost shell/ W is magnesium (Mg) 1
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