Bonding. Forces of attraction that hold atoms together making compounds
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1 Bonding Forces of attraction that hold atoms together making compounds
2 In summary... Ionic bonds are electrostatic attractions between cations and anions formed when electron(s) are transferred from the low IE, EA metal to the high IE, EA nonmetal
3 Ionic Compounds 1. Only exist as compounds in the solid state 2. Held together by ionic bonds - A strong attractive force 3. High melting points - Must break the bonds to melt the solid - The higher the melting point, the stronger the ionic bonds
4 Ionic Compounds 4. brittle solids 5. nonconducting as solids - No charges can flow 6. conduct electricity as liquids or aqueous - Ions are free to move
5 Ionic Compounds As solids, exist in a 3-D repeating pattern called a crystal lattice the lattice energy is the energy released when the bond is formed between the free ions Also a measure of the energy required to break apart the ionic compound once formed The greater the lattice energy, the stronger the force of attraction
6 Cation (+) Ionic compound = crystalline solid
7 Ionic Bond Strength A measure of the attractive force between the ions smaller ions = stronger ionic bonds smaller atom:atom ratio = stronger bond Ex: NaCl = 1:1, Na 2 O = 2:1, AlCl 3 = 1:3 larger charges = stronger bonds evidence: melting points
8 Coulomb s Law F = attractive force Q 1, Q 2 = charges (size) r = distance between charges (related to ion size and ratio of cation:anion)
9 Compare the melting points: KCl : 776 o C KI : 723 o C Cl - is smaller than I - smaller ions = stronger bonds Stronger bond = higher melting point
10 Compare the melting points: FeCl 3 : 306 o C FeCl 2 : 677 o C 1:3 ratio 1:2 ratio smaller atom:atom ratio (closer to 1:1) result in stronger ionic bonds
11 Ion dissociation Many ionic compounds will dissolve in water if it results in lower E (more stability) than in the solid ionic compound the ions dissociate from each other Ex: CaCl 2(s) + H 2 O Ca 2+ (aq) + 2Cl - (aq)
12 Types of compounds All compounds are made of two or more elements held together by chemical bonds Ions of opposite charges are held together by ionic bonds Usually: a metal with a nonmetal Ionic bonding is non-directional There are no ionic molecules Formulas of ionic compounds show the ratio of cation to anion Ionic compounds only exist in the solid state, in a 3-D crystal lattice
13 Covalent Bonding Covalent bonding involves the sharing of electron pairs usually between two nonmetals - high EA, high IE - both tend to gain more e - s, neither is willing to lose the e - s they have
14 Covalent Bonding A covalent bond is formed when two atoms share one or more pairs of electrons Both atoms see the electrons, so the electrons count as valence electrons on both atoms Satisfies the octet rule
15 Covalent Bonding
16 Types of compounds Covalent compounds are made of two or more elements held together by covalent bonds Covalent bonding is directional Between two individual atoms A group of covalently bonded atoms is referred to as a molecule Covalent compounds are also referred to as molecular compounds
17 A nonmetal will form as many covalent bonds as necessary to fulfill the octet rule example: C, with 4 valence e - s, will form 4 covalent bonds double bonding (two atoms sharing two pairs) and triple covalent bonding (sharing three pairs) is a possibility
18 Unless they are part of a polyatomic ion C forms 4 bonds N forms 3 bonds O forms 2 bonds H,F forms 1 bond
19 Binary Molecular Nomenclature Two nonmetals no charges to balance multiple subscripts possible ex: N 2 O, NO, NO 2, N 2 O 4, N 2 O 5
20 Use prefixes to represent subscripts mono = 1 di = 2 tri = 3 tetra = 4 penta = 5 hexa = 6 hepta = 7 octa = 8 nona = 9 deca = 10
21 Rules, continued.. Change second name to end in ide do not use prefixes on the first word if the prefix is mono always use prefixes on the second name
22 NEVER, EVER, EVER, EVER, EVER, EVER, EVER, USE PREFIXES WITH A METAL!
23 Examples... CO 2 carbon = first word subscript = 1, so no prefix oxide = second word subscript = 2, so prefix = di carbon dioxide
24 Examples... CO carbon = first word subscript = 1, so no prefix oxide = second word subscript = 1, so prefix = mono carbon monoxide
25 Try to name these N 2 O dinitrogen monoxide NO nitrogen monoxide NO 2 nitrogen dioxide N 2 O 4 dinitrogen tetroxide N 2 O 5 dinitrogen pentoxide H 2 O dihydrogen monoxide DHMO.org
26 Writing formulas... Dinitrogen tetroxide di = 2, so two nitrogen s tetra = 4, so 4 oxygens N 2 O 4 Note: do NOT reduce subscripts for molecular compounds
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