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