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Bonding

Bonding. By Dana Fromm. Ionic Bonds. Force of attraction between the opposite charges of an ion. One element loses electrons, while another gains them. Some atoms lose electrons to make outside energy levels become stable.

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Bonding

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  1. Bonding By Dana Fromm

  2. Ionic Bonds • Force of attraction between the opposite charges of an ion. • One element loses electrons, while another gains them. • Some atoms lose electrons to make outside energy levels become stable. • Atoms become more stable when their outer most energy level has 8 electrons.

  3. Covalent Bonds • Electrons are shared between atoms. • Formed between non-metals and non-metals or hydrogen and non-metals. • Share electrons so both can have stable octet. • Two types • Non-polar: when 2 exact non-metals equally share electrons. • Polar: when 2 different non-metals share electrons.

  4. Metallic Bonds • Shares electrons in its outer shell with many other atoms. • Occurs in elements in which the valence electrons are not tightly bound with nucleus. • Occurs in metals.

  5. Forces that hold them together • Ionic bonds: ionization energy • Covalent bonds: electronegativity • Metallic bonds: shielding effect

  6. Compare/Contrast • Ionic bonding is the taking of electrons, while covalent bonding is sharing of electrons, and metallic bonding is sharing electrons of the outer shell. • Elements in ionic, metallic, and covalent bonding both need 8 electrons to become stable. • Metallic bonds and ionic bonds are both sharing electrons in some way.

  7. Examples of Compounds • Ionic bonds: SiO2, KBr, BaCl2, Na2S, Ba3P2 • Covalent bonds: CO2, CCL4, P2O5, PBr3, N2O • Metallic bonds: K2Cr2O7, KmnO4, CsAu

  8. Methods of Classification • Ionic: made from metal and non-metal • Covalent: made from 2 non-metals • Metallic: made from 2 metals

  9. Recent Material • Ionization energy is the amount of energy needed to remove an electron. • Electronegativity is the strength of the pull that an atom gives. • Shielding effect stops the atom from condensing onto itself from electrons being added.

  10. Properties • Ionic bonds • Non-directional: the magnitude of the bond is equal in all directions around the ion. • High bonding energies: reflected in high melting temperatures • Generally hard and brittle materials: most common bonding for ceramic materials. • Exhibits electrically and thermally insulative properties.

  11. Properties continued • Covalent bonds • Molecular form: compound exists as separate molecules because they are electrically neutral. • State: most are liquid and gases. • Volatile • Low melting and boiling point • Generally insoluble in water • Conduct no or small amount of electricity

  12. Properties continued • Metallic bonds • Very rare • Some have a metal as a part of a negative ion • Conducts electricity • Can be bent into sheets without breaking into chains

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