2 or more metals Atoms of metals are tightly packed together in a giant lattice similar to the lattice in ionic compounds. The outer electrons separate from their atoms and become delocalized, creating a ‘sea of electrons’. The atoms become positive and are attracted to these negative electrons. Properties of Metals High melting and boiling points (bonds are super strong) Excellent conductors of electricity (solid and liquid) more electrons, more conductivity Excellent Conductors of heat (solid and liquid) increased vibrations spread through sea of electrons Good Malleability and ductility in a metal can roll over each other while still maintaining their bonds, especially if heated. Which one of the following properties is not characteristic of typical metals? Moderately high melting point High boiling Brittle Good electrical conductor when a solid Of the three major types of bonding (ionic, covalent, metallic) which ones are based on electrostatic attractions between opposite charges? Only ionic bonding Only and covalent bonding Only and metallic bonding covalent and metallic bonding True or false: metals give up electrons easily True False Why are metals described as having a “sea of electrons”? Electrons are wet Electrons move in waves Electrons move freely between atoms Electrons are fixed to metal atoms When 2 or more metals are combined they form an… Brass Alloy Bronze Covalent bond Which of the following is a correct description of a metallic property? Metals are brittle Metals are malleable Metals have a dull appearance Metals gain electrons to form anions
Which of the following is not a property of metals? Shiny luster Brittle/shatters easily Conducts electricity Malleable Which of the following is a mixture of elements that have metallic properties An alloy A suspension A gas A pure metal What does the “sea of electrons” contain? All the electrons in that metal The electrons in the outer shell of that metal The electrons in the inner shell of that metal Why are metals able to conduct electricity? The positive metal ions pass charges to each other Electrons pass charges through the positive metal ions The sea of electrons helps pass changes through the metal Metallic bonding occurs between atoms of Sulfur Copper Fluorine Carbon The high electrical conductivity of metals is primarily due to High ionization energies Full valence shells Mobile electrons High electronegativity A substance that conducts electricity as a solid and when melted into a liquid is most likely classified as An ionic compound A molecular compound A metal A nonmetal Learning Goal 7.4 – I can draw Lewis dot structures for molecules and compounds. Learning Goal 7.5 – I can explain polar bonds and polar molecules in terms of electronegativity; determine the degree of polarity of a bond based on electronegativity, and describe the shape of a molecule based on its polarity.
CH3F CH2Br2 Does this molecule have polar bonds? Is this molecule symmetrical in X and Y? Is this molecule polar? Does this molecule have polar bonds? Is this molecule symmetrical in X and Y? Is this molecule polar? H2S CBr4 Does this molecule have polar bonds? Is this molecule symmetrical in X and Y? Is this molecule polar? Does this molecule have polar bonds? Is this molecule symmetrical in X and Y? Is this molecule polar? PCl3 H2O
Properties IONIC COVALENT METALLIC Action of electrons Molecular Network Type of element Bond strength Melting point / boiling point Hard vs. Brittle Soluble in H2O Electrolytes? Conduct electricity as a solid? Conduct electricity as a liquid? Conducts heat? Multiple compounds are held together by Learning Goal 7.8 – I can explain the properties of giant covalent compounds in terms of their structures.