Ionic, Covalent, Sigma, Pi, Inter and Intra
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| Element | A substance that cannot be broken into simpler parts by chemical means
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| Compound | A substance that is made up of 2 or more elements chemically joined
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| Molecule | A group of atoms joined together. It is the smallest past of an element or compound that can exist independently.
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| Octet Rule | When bonding occurs atoms tend to reach an electron arrangement with 8 electrons in their outer shell
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| 2 reasons the Octet Rule failed | Hydrogen and Helium only have 1 and 2 electrons.
Many transition metals have more or less than 8 electrons in their outer shell
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| 2 main types of intramolecular bonding | Ionic and Covalent
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| Valency | The number of electrons an atom needs to lose, gain or share in order to achieve noble gas structure
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| Ionic Bonding | An ionic bond occurs when one atom loses electrons and one atom gains electrons. It is the force of attraction between oppositely charged ions.
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| Regular structures formed by ionic compounds | Crystal lattice
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| Repeating unit of a crystal lattice | Unit cell
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| Covalent bonding | A covalent bond is formed when electrons are shared between 2 or more atoms
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| Single, double and triple bond are composed of how many electron pairs | Single: formed from one shared pair of electrons
Double: formed by two shared pairs of electrons
Triple: formed by three shared pairs of electrons
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| High melting and boiling point: Ionic or Covalent? | Ionic compounds
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| Conduct electricity: Ionic or Covalent? | Ionic, when molten or dissolved in water
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| Sigma bond | formed from a head on collision of orbitals. Very strong bonds
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| What orbitals can form a sigma bond? | S and S, S and Px, Px and Px
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| Pi bonds | formed from the sideways overlapping of Py and Py or Pz and Pz. Not as strong as sigma bonds
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| What type of bonds is a triple bond made of? | One sigma and 2 pi. This is why a triple bond is not 3 times as strong as a single. Pi bonds are not as strong as a sigma. It is only about 1.5 times as strong
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| What does VSEPR Theory stand for? | Valence Shell Electron Pair Repulsion Theory
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| Two types of electron pair in VSEPR | Lone pair and Bond pairs
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| Which has the stronger repulsion force, lone pairs or bond pairs? | Lone pairs
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| Bond angle in triangle planer molecules? | 120
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| Bond angle in planer v-shaped? | 104.5
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| Bond angle in tetrahedral molecules | 109.5
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| Bond angle in linear molecules | 180
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| Bond angle in pyramidal molecules | 107
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| Electronegativity | This is the relative attraction an atom has for the shared pair of electrons in a colavent bond
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| Discoverer of electronegativity? | Linus Pauling
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| Molecules with an eneg difference of 0 are: | Non-polar
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| Molecules with an eneg difference less than 1.7 are: | Polar Covalent
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| Molecules with an eneg difference greater than 1.7 are | Ionic
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| Symmetrical molecules are said to be: polar or non-polar? | non-polar
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| Examples of diatomic molecules (non-polar) | Hydrogen, Oxygen, Nitrogen, Fluorine, Chlorine, Bromine, Iondine
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| Intramolecular forces: Definition and examples | Bonding that occurs inside the atom: Sigma and Pi, Ionic and Covalent
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| Intermolecular forces: Definition and examples | Bonding that occurs between 2 separate molecules:
Van der Waals forces, Dipole-Dipole, Hydrogen Bonding
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| Van der Waals forces | The attraction between the temporary dipoles of non-polar molecules. eg Diatomic molecules.
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| Why does the melting point of the halogens increase as we go down the group? | Van der Waals forces increase due to increasing number of electrons, increasing the melting/boiling point
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| Dipole-Dipole | These are the forces of attraction between the permanent negative pole of one molecule and permanent positive pole of another molecule.
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| Hydrogen Bonds | Hydrogen bonding occurs when hydrogen bonds to a small, highly electronegative element: eg: Oxygen, Nitrogen and Fluorine.
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| Uses of Hydrogen Bonds | Kevlar bullet proof vests, Surface tension in water, Solvents like ammonia,
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