Download
1 / 69
690 likes | 794 Views
LIQUIDS, SOLIDS, & SOLUTIONS. Chemical bonds (strong connections) Metallic Covalent Ionic. What sticks atoms together?. What sticks molecules together?. Intermolecular forces (IMFs) relatively weak Dispersion Dipole-dipole Hydrogen bonding. Chemical Bonds can be….
E N D
Chemical bonds (strong connections) • Metallic • Covalent • Ionic What sticks atoms together? What sticks molecules together? • Intermolecular forces (IMFs) relativelyweak • Dispersion • Dipole-dipole • Hydrogen bonding
Chemical Bonds can be… Dependent upon: Molecules can be… Dependent upon:
Shapes refresher: Trigonal- Trigonal- Tetrahedral Bipyramidal Octahedral Planar Linear Example: BF3 Example: CH3 Example: PF5 Example: SF6 Example: CO2
Nature of solids • Solids tend to contain particles that are vibrating, but are restricted in their ability to move • High Density • Definite Volume • Definite Shape • Definite Melting Point • Incompressible • Low Rate Of Diffusion
Nature of solids • Solids differ in their arrangements and in the forces that are holding them in place. • Properties that they all share are melting point, hardness, and density • Types of arrangements • Crystalline • Can be metallic/molecular/ionic or covalent-network • Amorphous
Crystalline solids • Overall structure of a crystalline solid is a highly ordered, repeating pattern called unit cells • A unit cell is a representative unit of a larger crystal • It’s the smallest representation of the crystal
Crystalline: covalent/molecular • Held together by combinations of different intermolecular forces • Melting pt is dependent on IMF • Relatively soft • Poor conductors • Sugar, ice, dry ice
Crystalline solids: ionic • Tightly packed solid composed of cations & anions • Intra-molecular forces • Form strongest crystal possible • Pack to minimize repulsive forces • Are hard and brittle • Have high melting points • Produce a crystal with a shape dependent on ions present
Crystalline: metallic solids • Solid formed by the attraction between metal atoms and the surrounding sea of e-s • Electrons flow • Good conductors • Ductile and malleable • Can create mixtures called Alloys
Covalent-network • Strong covalent bonds involved without a particular molecule being formed • Form a network of connections • They have extremely high melting points • Tend to be very hard, but brittle
COVALENT NETWORK Graphite Diamond Vs. Dispersion Forces
Amorphous solids • A solid in which the particles are arranged randomly • No crystal structure • Rigid appear solid-like • Glass, rubber, plastics • Sometimes called extremely viscous liquids
Solutions Parts of:
What is the molarity of NaOH in a solution which contains 24.0 g NaOH dissolved in 300 ml of solution? Concentration Calculations: A soln contains 116 g acetone (CH3COCH3), 138 g of ethyl alcohol (C2H5OH) and 126 g of water. Determine the mole fraction of water. Calculate the molality of acetic acid in a solution prepared by dissolving 120 g acetic acid in 100 g of water. 17.5 g of sugar is dissolved in 200.0 g of water. What is the percent by mass concentration of the sugar solution?
C1V1=C2V2 Dilution Calculations: You have 200 ml of 2.00 M stock solution. If we want to make 50 ml of 0.50 M solution, how much stock solution would we need? If we were then to take 10.0 ml of the new solution and add 10.0 ml of water, what concentration would the new solution be?
1 2 3 4 5 6
Solution Properties: Solubility Like Dissolves Like
