covalent & ionic bonding
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| VSEPR theory- | (valence-shell electron-pair theory) because electron pairs repel,molecules adjust their shapes so that valence-electron pairs are as far apart as possible. |
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| metallic bond- | force of attraction that holds metals together, it consists of the attraction of free floating valence electrons for positively charged matal ions. |
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| structural formula- | a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion: each dash between two atoms indicates a pair of shared electron. |
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| coordinate covalent bond- | a covalent bond formed when one atom contributes both bonding electrons. | Hydrogen Bonds- | a relatively bond intermolecular force in which s hydrogen that is covalently bounded to a very electroneagtive atom is also weakly bonded to an unshared electron pair of another electronnegative atom in the same molecule or one nearby. | So3 shape- | triagonal
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| resonance- | one of two more equally valid electron dot structures for a molecule or polyatomic ion: the actual bonding is a hybrid, or mixture of the resonance structures. | Sigma Bonds- | a bond formed when two atomic orbitals combine to forma molecular orbital that is symmetrical along the axis connecting the two atomic nuclei. | SCl2 shape- | linear
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| dispersion forces- | the weakest kind of intermolecular attraction: this attraction is thoght to be caused by the motion of electrons. | Pi bonds- | a bond in which the bonding electrons are most likely to be found in the sausage-shaped regions above and below the nuclei of the bonded atoms. | CO shape- | linear
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| Dipole Interactions- | a weak intermolecular force resulting from the attraction of oppositely charged regions of polar molecules. | Identify 3 properties of an ionic compund. | 1. Consists of two metals. 2. Consist of electrically neutral groups of ions joined by electrostatic forces. 3. The total positive charges if the cations must equal the total negative charges of the anions. | H2Se shape- | Linear
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| Van der Waals Forces- | a term used to describe the weakest intermolecular attractions: these include dispersion forces and dipole interactions. | What are the 7 diatomic molecules? | 1. Fluorine F2 2. Chlorine-Cl2 3. Bromine-Br2 4. Iodine-I2 5. Hydrogen-H2 Nitrogen-N2 7/ Oxygen- O2 | CO2 shape- | linear
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| What is the difference between a single, double, and triple bond? | A single bond is a bond in which two atoms share a pair of electrons. A double bond is a bond that involves two shared pairs of electrons. Triple covalent bonds are bonds that involve three shared pairs of electrons. | How do ionic compounds conduct electricity abd how is this different from metallic compounds? | In ionic compounds they consist of electrically neutral groups of ions joined by electrostatic forces. The metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions. | SiCl4 | tetarhedronal
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| How is a network solid different from other covalent compunds? | Network solids are very stable substances in which all of the atoms are covalently bonded to each other. | What determines the degree of polarity in a bond? Distinguish between nonpolar covalent, polar covalent, and ionic bonds in terms of relative polarity. | A nonpolar covalent bond pulls equally and the bonding electrons are shared equally. A polar covalent bond is joined with two atoms of different elements and the bonding electrons are shared unequally. |
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