KS3 Science, Chemistry, Bonding and Structure, metallic bonding help?
1. False. It's the force of attraction between the free (delocalised) electrons and the metal ions (cations.) 2. True. That's what defines a metal really and makes them such good conductors. 3. True. It allows the layers to just slide over each other. 4. True. Their conductivity is due to their delocalised electrons. 5. False. Mercury is an example of a liquid metal at room temperature (it and bromine are the only liquids at room temperature in the periodic table.) There are no metallic gases however. 6. False. An alloy can contain more than two metals.
What's the difference between metallic bonding and ionic bonding?
Okay so i understand an ionic bond is when a metal looses electrons to become stable to a non-metal and this results in them both being stable, and the ionic lattice is held together by the attraction of the positively charged ions and negative ions (non-metal) being attracted to one another. But what is a metallic bond, and a metallic lattice structure? they are next to one another in my notes and the ionic bond is fully explained but i dont understand what it has to do with this metallic lattice thing?
Which phrase MOST accurately describes metallic bonding?
A) rigidly held valence electrons B) metal ions floating in a sea of electrons C) strong electromagnetic force holding electrons in place D) valence electrons arranged in a regular repeating pattern help please.
How do you show metallic bonding in strontium metal?
A Metallic bond can be thought of as all the Sr2+ ions in a single metal crystal being in a soup of electrons.. The whole thing being electrically neutral.
What word describes methane? (CH4) Is it described as an Atom, Ion or Molecule?
Is CH4 described as an Atom, Ion or Molecule? Please help as I am unaware of the answer. It would also help if you could tell me if CH4 is a Covalent, Ionic or Metallic bonding? Thanks.
Why are copper metal wires used to conduct electricity?
Excellent answers, all. Really, on an engineering basis, aluminum and copper are the big competitors. Inside the house, copper is very much preferred. It is a better conductor and less subject to corrosion, oxidation and deterioration of properties when exposed to higher temperatures. It is about four times the cost of aluminum by weight, but for the limited amount of wiring inside of a house or small appliance, this is acceptable. For cross-country transmission of power, however, aluminum is much less dense than copper. Hence, even though one must use more volume of aluminum to get the same conductivity, the weight of the cables is much less. Also, the cost of stringing all of the over-land transmission systems with copper would be staggering. (Copper is up quite a bit these days... spot price has been well over $3/lb for a week or two. Aluminum usually runs $0.90 to $1.00 / lb.)For sheer conductivity, however, silver is the king! That is why the electronics industry loves it. Often the critical factor affecting function is not determined by the long range over which one is transmitting an electric signal, but rather by the speed and quality of the connecting points. Hence, a tiny dab of silver (or gold) at those points can be extremely effective. Silver actually has conductivity better than gold, but gold is totally resistant to oxidation. Something even silver and copper cannot claim.