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Terms in this set (19)
-at room temp. usually solid
-good conductors of electrical current and thermal energy
Properties of metals?
a mixture made of two or more elements, at least one of which is metal
Alloys are generally stronger and less reactive than the pure metals from which they are made
How do the properties of metals and alloys compare?
-properties can differ greatly from original element
-also can retain many of the elements original physical properties
-properties depend on how the alloy is mixed
-chem:properties differ from original element
Physical/Chemical properties of alloys?
- metals usually have between 1-3 valence electrons
-when metals combine with atoms of other elements, they usually lose valence electrons, thus be coming positive ions
-most metals are crystalline-solids
Metal atoms combine in regular patterns in which the valence electrons are free to move from atom to atom
How do metal atoms combine?
an attraction between a positive metal ion and the many electrons surrounding it
the more valence electrons an atom can add to the "sea", the______ the metallic bond will be
The "sea or electrons" model of metallic bonding helps explain the malleability, ductility, luster, high electrical conductivity, and high thermal conductivity of solid metals
How does metallic bonding result in useful properties of metals?
- each property is related to the behavior of valence electrons in metal atoms
-metals can be bent and stretched because the positive ions are attracted to the loose electrons all around them rather than to other metal ions
Malibility and ductility in metallic properties:
-valence electrons absorb light and then give it off again
-valence electrons allow electric currents to pass from electron to electron because they are free to move around
-valence electrons allow the transfer of heat easily since the electrons are free to move around
Atoms of that family have only one valence electron, the next lowest energy level has a stable set of 8 valence electrons. therefor, alkali metals atoms can become chemically more stable by losing their one valence electron. this property makes them very reactive. so they can react and combine with many elements most of which found in nature.
Explain why the alkali metals in Group 1 are always found in nature combined with other elements.
Mallebility and ductilluty: positive ions are attracted to the loose electroons all around them rather than to other metal ions, those ions can be made to change position. because the metal ions can move easily
Luster: when light strikes the v.e, they absorb the light and then give it off again
E.C:electrons in a metal can move freely among the atoms, when charged particles are free to move an e.c is possble
T.c: valence electrons freedom of motion within a metal or metal alloy
How does the "sea of electrons" model of metallic bonding explain the shared characteristics of metals?
water molecules create a polear bond which menas they shared electrons unequally. when the atoms of some elemetns pull more strongly on shared electrons they create a unequally sharing amount. thsi unequall amount cretaes. the negatively-charged auction ends of the Polar water molecules attract a positively charged hydrogen end of a nearby water molecules. thsi attraction pull the molecules towards each other causing the friction of thermal c.
Explain why the polar structure of water molecules causes water to have a higher boiling point than carbon dioxide.
Ionic bonds is the attraction between two oppositly charged ions. while a covalent bond is formed when two atoms share electrosn. covalent bonds usually form between atoms of nonmetals. in contrast ionic bond usually form when a metal combines with a nonmetal. the force that holds atoms together in a covalent bond is the attraction of each atom nucleus for the shared pair of electrons. ionic bonds form as a result of the attraction between positive and negative ions
Compare and contrast ionic bonds and covalent bonds.
Sea of electrons model
positively charged metal ions are embedded in a swarm of valence electrons, more valence electrons you can add to the swarm stronger the metallic bonds will be
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