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Reactivity and Atoms
Notes on Reactivity and Atomic Structure
| Question | Answer |
|---|---|
| What is the mnemonic for the Reactivity Series | Please - pottasium send - sodium cats - calcium monkeys - magnesium and - aluminum zebras - zinc in - iron their - tin lovely - lead happy - hydrogen cages - copper made of - mercury silver & -silver gold - gold |
| What elements are the cut off point for reacting with water, steam, acid and oxygen (oxidization(rusting)) | Pottasium Sodium Calcium ---- (above water) Magnesium [Carbon][not metal] Aluminum Zinc Iron ---- (above Steam) Tin Lead ---- (above Acid) [hydrogen][not metal] Copper Mercury Silver ---- (above Oxygen) Gold |
| Which Elements do not oxidise | Gold |
| How many electrons can fit in each electron shell (upto 3rd shell) | 2, 8, 8 |
| What is the definition of an ion | an atom or molecule with a net electric charge due to the loss or gain of one or more electrons |
| Why can some metals conduct electrisity | Due to delocalised "sea of electrons", from metallic bonding electrons can move freely between metal ions "moving" charge around which conducts electricity |
| Name the 3 types of chemical bonds, | Ionic bonds, Covalent Bonds, Metallic Bonds, |
| Describe Ionic Bonding | When an atom gives an electron to another atom they both become oppositely charged Ions. As opposites attract they become electrostatically attracted to each other |
| Describe Covalent bonding | Is formed by sharing a pair of electrons between atoms, to complete there outer shells, tends to be very strong |
| Describe Metallic Bonding | Strong electrostatic attraction between sea of negative delocalised electrons and positive metallic ions. |
| compare the relative strengths of all the bonds and in what group they occur in (e.g. group 5, or group 8) | Ionic>Covalent>Metallic Ionic bonds are typically stronger than covalent bonds, which in turn are typically stronger than metallic bonds |
| How does the delocalised sea of electrons occur | Within the metal lattice, the atoms lose their outer electrons and become positively charged metal ions The outer electrons no longer belong to any specific metal atom and are said to be delocalised becoming a "sea of electrons” |
| Define oxidisation | Oxidation is a chemical process. It is defined as a process that occurs when atoms or groups of atoms lose electrons |
| state the name, charge and Relative atomic mass of all the sub atomic partials | (Proton, +1, 1)/(Neutron, 0, 1)/(Electron, -1, 0) |
| State the properties of metals and non-metals | Metals: Shiny, good conductors of electricity and heat, malleable and ductile, and usually solid at room temperature. Non: Dull, poor conductors of electricity and heat, brittle and usually solid or gaseous at room temperature. |
| Not a Question but write down any topics your struggling with in this quiz or in general and let me know so I can help explain it | Not a Question but write down any topics your struggling with in this quiz or in general and let me know so I can help explain it |
| State the general assumptions you can make about the reactivity of an element, | 1) the more electron shells the more reactive, 2) the closer the shells are to being complete (but aren't) the more reactive, 3) fully complete shells are much less reactive |
| Can charge in a closed system (a set area nothing can get in or out of) be changed | No, any changes of charge occurring in atoms must also have the opposite charge created, e.g. an atom looses an electron, now the atom is positively charged as has 1 more proton than electron, but the negative electron still exists just not in the atom. |
Created by:
HxK138
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