properties of solids. physical properties while solid has definite shape and volume; it does have...
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Properties of Solids
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Physical properties
• While solid has definite shape and volume; it does have various other properties that can be very different. Such as density, colour, melting points, etc
Pg. 119
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Ionic solids
• Lots found in nature as rock and mineral deposits:– Sodium chloride (salt)– Potassium chloride (potash)
• Also found at home:– Household cleaners (contains sodium hydroixde)
• Other examples:– Rust (iron (III) hydroxide)– Tarnish (silver sulfide)
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Cont’d
• Some reactive metals don’t occur in elemental form in nature, they are found as ionic compounds
• Ionic compounds are also used to extract metals from naturally occurring compounds
• For example: iron is the most common metal used but is also very reactive
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Formation
• Formation reaction of a metal and nonmetal similar to sodium chloride
• Formation reaction of two compounds• Ionic compound stability is similar to that of
noble gases so it can be suggested that there is a total electron transfer occurring.
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A model
• At SATP, all ionic compounds are solid so they must be held together (bonded) in that rigid structure.
• Models show that the ions are arranged in a regular pattern, depending on the size, shapes and charges
• This is called a crystal lattice
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Ionic Compounds
• Ionic compounds are brittle – the ions don’t rearrange
• Binary ionic compounds also have medium to high boiling points
• Polyatomic ions have more complex crystal lattices but the ions have covalent bonds so can be treated like an monatomic ion
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Metallic Crystals
• Shiny, silvery, flexible solids with good electrical and thermal conductivity
• Hardness varies greatly as well as the melting temperature
• X-Ray diffraction shows that all metals have a continuous and compact crystalline structure
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Metal Properties• Metallic bonding – continuous electron clouds– Low electronegativity – loosely holding electrons– Empty valence orbitals explains electron mobility– Strong Electrostatic attraction for bonding– this gives the many different properties to metallic
compounds
Pg. 124
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Molecular crystal
• Elements or compounds• Small molecules for solid crystal, low melting
point, not very hard, nonconductors• Properties can be explained by the IMF and
structure
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Covalent Network Crystals
• Crystal substances– Diamond and quartz – very hard
• Very hard, high melting point, brittle, insoluble, nonconductors
• Examples – silicon carbide SiC(s) used in sandpaper,
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Carbon
• Carbon is extremely versatile with bonding in various ways
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Semiconductors
• Crystalline silicon or germanium ‘doped’ with a Group 13 or 15 element
• Little bit of energy to put an electron into a higher orbital and conduct electricity
• Used in transistors, solar cells
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Summary
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Unit Test Review Summary
• Lewis Formulas• Bonding Theory (types)• Electronegativity • Molecular Formulas (Lewis, structural, sterochemical) • Bonding capacity• VSEPR• Bond and molecular Polarity• Intermolecular Forces
– Isoelectronic Compounds• Boiling points• Properties of Liquids and Solids
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Suggested review questions
• Pg. 137 #3, 6, 7, 10, 12, 14• Pg. 138 #21, 25, 28• Pg. 139 #35, 40, 41, 43• Pg. 140 #48, 53, 57• Pg. 141 #60