3.5 - Metals
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what are the two components in the structure of a metal
• lattice of positive metal ions • sea of delocalized electrons
what charges do metal ions in the metal structure have
their usual charge
what were the delocalized electrons lost by and how do they move
lost by the metal ions and they move freely through the lattice
what is metallic bonding
the electrostatic attraction between the positive metal ions and the negative delocalized electrons
what type of attraction is metallic bonding
usually very strong
what are the properties of metals
have high melting points conduct electricity malleable
why do metals tend to have high melting points
because the metallic bonding is very strong so lots of energy is needed to break it
why do metals conduct electricity
the delocalized electrons are free to move through the lattice
why are metals malleable
the layers of metal ions can slide over each other
what is thermal decomposition
a thermal decomposition reaction is when heat energy is used to break down a substance
what is the equation for a thermal decomposition
metal carbonate –> metal oxide + carbon doxide
what would the thermal decomposition of copper carbonate look like
copper carbonate –> copper oxide + carbon dioxide CuCO3(s) CuO(s) CO2(g) green solid black solid colourless gas
what is carbon dioxide often collected by in thermal decomposition
downward delivery
why is carbon dioxide collected by downward delivery
because carbon dioxide is denser than air
what is downward delivery
the carbon dioxide sinks to the bottom of a tube and stays there until you want to use it
list the metal reactivity series from lowest to highest
Au Ag Cu (H) Pb Fe Zn (C) Al Mg Ca Li Na K
why are hydrogen and carbon included in the reactivity series despite being non-metals
their positions are important when considering displacement reactions
what do metals react with cold water to form
metal hydroxides and hydrogen
what is the metal and water reaction equation
metal + water –> metal hydroxide + hydrogen
what are the two significant observations of metal and water reactions
effervescence - due to the hydrogen gas produced solid disappears - due to being used up in the reaction
what are the metals in group 1 of the periodic table called
alkali metals
how do the metals in group 1 of the periodic table react with water
violently to form metal hydroxides and hydrogen
group 1 metal and water reaction equation
metal + water –> metal hydroxide + hydrogen
what similar observations do the reactions of Li, Na and K with water share
• solid floats - it is less dense than water • effervescence - hydrogen gas is produced • solid moves - the effervescence propels it around the surface of the water • solid disappears - it is used up in the reaction