METALS Lose electrons and form positive cations. NON-METALS gain electrons and form negative anions. IONS Are charges particles. EXMAPLES Atomic Notation and Bohr Diagrams Lewis Dot Diagram Examples Lewis Dot Diagrams of an Negative ION (NON-METAL) Negative ions have 8 valence electrons! Lewis Dot Diagram of an Ionic Compound Lewis Dot Diagrams of an Positive ION (METAL) Positive Ions have no valence electrons! The Octet Rule REMEMBER! All elements want
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occupied shells increases. The atomic size increases. The valence gets further away from the nucleus. The strength of attraction from the nucleus to the valence electron gets weaker. The valence electron is loosely held and it is easy for the elctron to be released to form stable octet lectron arrangement. The reactivity of G1 is the tendency of the atom to release elctron to form stable electron arrangement. The easierm the atom releases electron‚ the more reactive it is. ELECTROPOSITIVITY The electropositivity
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bonds are formed when atoms share electrons‚ one from each atom in a single bond‚ to form electron pairs‚ usually making their outermost shells up to eight electrons by this means. This would make them more stable‚ less reactive and an electronic structure like a noble gas. They are most frequently formed between pairs of non-metallic elements. Non-metallic elements usually have from four to eight electrons in their outermost shells‚ the so-called valency electrons‚ which are used for chemical bonding
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fixed ratio‚ has characteristics different from those of its elements TRACE ELEMENT- those required by an organism in minute quantities ATOM- smallest unit of matter that still retains the properties of an element NEUTRONS- no electrical charge ELECTRONS- negative charge PROTONS- positive charge ATOMIC NUCLEUS- formed by neutrons and protons ATOMIC NUMBER- number of protons in its nucleus MASS NUMBER- the sum of protons and neutrons in the nucleus ATOMIC MASS- the atom’s total mass‚ can be approximated
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Transition Metal: element of groups 3-12 * Energy level: a space with definite and fixed energy in which an electron is allowed to move * Orbit: circular/spherical path in which the electron can move around the nucleus * Electron Cloud: the region of an atom in which there is a probability that an electron exists * Quantum Mechanics: theory of the atom in which electrons are described in terms of their energies/probability patterns (model looks like smoke around a circle) * Principal
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Chapter 7 Matching Match each item with the correct statement below. a. halide ion e. valence electron b. octet rule f. coordination number c. ionic bond g. metallic bond d. electron dot structure ____ 1. an electron in the highest occupied energy level of an atom ____ 2. Atoms react so as to acquire the stable electron structure of a noble gas. ____ 3. a depiction of valence electrons around the symbol of an element ____ 4. an anion of chlorine or other halogen ____ 5. the force of attraction
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CONTENT Contents IONIC BOND 2 METALLIC BOND 9 The "Sea of Electrons" Theory 14 Conductors‚ Insulators and Semiconductors 16 25 IONIC BOND Ionic bond is formed when electron transferred from a valence shell of an atom to the valence shell of another atom. Ionic bond involves electron transfer across two atoms. The atom which donates the electron is called cation which is a positive ion whereas the atom which gains the electron is called anion which is a negative ion. The opposite charge
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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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- two atoms each sharing electrons within a molecular orbital Metallic Bonding - positive metal ions held together in a lattice with a “sea of electrons” An actual chemical bond is a blend of all three types of bonding. Most often‚ one type is dominant over others. We will concentrate on ionic and covalent bonding. LEWIS STRUCTURES Only valence electrons are important in bonding. Lewis dot structures show valence electrons surrounding atom. We visualize the four valence orbitals of an atom as the
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than the separated atoms. The bound state implies a net attractive force between the atoms ... a chemical bond. The two extreme cases of chemical bonds are: Covalent bond: bond in which one or more pairs of electrons are shared by two atoms. Ionic bond: bond in which one or more electrons from one atom are removed and attached to another atom‚ resulting in positive and negative ions which attract each other. Other types of bonds include metallic bonds and hydrogen bonding. The attractive forces
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