A PREVIEW & SUMMMARY. Types of Chemical Bonds Covalent Bonds Ionic Bonds Metallic Bonds. Ionic Bonds. while keeping in mind: Covalent Bonds
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1 Teacher notes; Data Table from Lab H bonding Types of Chemical Bonds Covalent Bonds Ionic Bonds Metallic Bonds first A PREVIEW & SUMMMARY Ionic Bonds while keeping in mind: Atoms are unhappy if their outer energy level is not full!! Atoms only bond with other atoms in order to fill their valence shell. An ionic bond is the attraction between a metal cation and a nonmetal anion. Covalent Bonds Metallic Bonds A covalent bond exists when electrons are shared by two nonmetal atoms. form between metal atoms when valence electrons can flow freely. Sea of valence electrons 1
2 Ionic Bonds Ionic Bonds Sodium Chlorine Sodium Ion (+1) Chloride Ion (1) Na now has 11p + and 10e. It now carries a charge of +1 Cl now has 17p + and 18e. It now carries a charge of 1 Ionic Bonding: How it Works i) Metal + Non Metal ii) Ions Form (electron transfer) iii) Opposites attract Ionic Compounds Covalent Bonds Time for an example: A covalent bond exists when two electrons are shared by nonmetallic atoms. How many electrons does carbon need to be happy? 4 electrons! 6+ 2
3 Time for an example: Vacancies 6+ Remember, H has 1 e (electron), and 1 p + (proton). How many vacancies does H have? 1!!! 1+ Let s see how looks Let s see how looks Hydrogen Hydrogen Now we need to add our other H s bonds with 4 hydrogens to form a methane molecule: Covalent Bonding: How it Works Single Covalent Bond = 2 electrons shared Double Covalent Bond = 4 electrons shared Triple Covalent Bond = 6 electrons shared 3
4 By sharing electrons Examples of Covalent Bonds Atoms achieve a full valence shell. Naming Covalent Compounds some stuff you already know: CO Monoxide CO 2 Dioxde SO 2 Sulfur Dioxide NF 3 Nitrogen Trifluoride Prefixes used for covalent compounds: 1 Mono 2Di 3 Tri 4Tetra 5 Penta 6 Hexa 7 Hepta 8 Octa 9 Nona 10 Deca Rules for Naming Covalent Compounds 1. Name the first element (the least electronegative is first) (the furthest left on the periodic table.) 2. If there is more than one atom of that element, add a prefix. 3. Name the next element & add a prefix. (even if there is only one, add mono ) 4. Add the ide suffix. Examples: CCl 4 Tetrachloride P 2 O 5 Diphosphorous Pentoxide N 2 O 4 Dinitrogen Tetroxide P 4 S 10 Tetraphosphorous Decasulfide 4
5 Ionic vs. Covalent Covalent Bonds can be polar or nonpolar Polar Covalent electrons are shared unevenly Nonpolar Covalent electrons are shared evenly nonmetal + nonmetal metal and nonmetal Polarity Polaruneven distribution of charge lopsided Show partial charges on structure by using δ (lowercase delta) Polarity Polaruneven distribution of charge in a bond. Dipole Moment the lopsided property of some molecules with polar bonds. We show partial charges on structure by using δ (lowercase delta) Hydrogen Bonding Ionic compounds are held together by a crystal lattice; a network of cations and anions. 5
6 So what holds the molecules of covalent compounds together? Intermolecular Forces: Van der Waals Forces Molecules that have dipoles (polar molecules) arrange themselves so that the negative and the positive ends of the molecules attract one another: Hydrogen Bonds Van der Waals Forces London Dispersion Forces DipoleDipole Interactions They eventually align in order to find the best compromise between attraction and repulsion: Hydrogen bonds Water is a polar molecule: Bond Types Lab Positive and Negative ends of adjacent molecules attract each other. Ionic Covalent Metallic High Melting Point Low Melting Point High Melting Point Soluble in H 2 O Soluble in H 2 O Not Soluble Do not conduct Do conduct in Solution Do not conduct Do not conduct in Solution DO conduct Do NOT conduct in Solution 6
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