| What is an Ion? Give examples. | This is simply a charged particle. Cl- [Chloride] or NO3 [Ammonium Ions] |
| Why do Atoms become Ions. | This is to full the Electron Outer Shell. This is a stable place from Atoms. They achieve this by Loosing an Electron, or gaining. |
| What happens when Metals and Non-Metals become Ions? | Metals become Ions by Loosing an Electron, making a Positive Ion
Non-Metals become Ions by Gaining an Electron, making a Negative Ion |
| What are the 4 Groups in the Periodic Table to most likely form Ions | Group 1-2 and Group 6-7. |
| Which Groups are the Metals, and the Non metals. What charge do they form? | Group 1 is Metals, They make a +1 Charge. [They lose 1 electron]
Group 2 is Metals, They make a +2 Charge [They lose 2 electrons]
Group 6 is Non-Metals. They make a -2 Charge [They gain 2
Electrons]
Group 7 is Non-Metals. They make a -1 Charge [They gain 1 electron.] |
| What do the Elements in G1-2 and G6-7 have in common? | They all have a Full Outer Shell once reacted. This is usually 8 |
| What is the Reactivity Series for G1-2 and G6-7 | G1-2 has it getting easier to Remove the Outer Electrons [Gets More Reactive as you go down the Group]
G6-7 has it getting the Electron Harder for the Nucleus [Gets Less Reactive as you go down the Group] |
| Explain the Reactivity Series for G1-2 and G6-7 | G1-2 gets more Reactive because the Electron is further away from the Nucleus, the Atom is bigger and the Attraction of the Positive Nucleus and the Negative Electron is Weaker
G6-7 gets Less reactive because the Positive Nucleus can spend More Energy to gain a Electron, because its Closer. As you go down, the Attraction gets weaker. |
| What happens when a Metal and a Non Metal reacts? | So the Metal can Lose the Outer Electron/s making a Positive Ion, and that Lost Electron is given to the Non-Metal, which turns into a Negative Ion.
These Ions are Oppositely Charged meaning that they can be Attracted together by strong Electrostatic Forces.
This creates an Ionic Bond |
| What happens when
1. Sodium reacts with Chlorine
2. Magnesium with Chlorine | 1. Potassium is a G1 Element meaning its going to lose 1 electron [+1 Charge] Chlorine is a G7 Element meaning it wants 1 Electron [-1] Charges are balanced out meaning they can make NaCl [Sodium Chloride]
2. Magnesium is a G2 Element meaning its going to lose 2 Electron
[+2] Chlorine is a G7 Element meaning it wants 1 Electron. The charges here are Not Balanced, but we make it by adding another Chlorine, making it want 2 Electron [-2] So now we can have Magnesium Chloride [MgCl2] [small 2] |
| So what does it mean when an Ionic Compound has a Giant Ionic Lattice Structure? | This is simply the Ions making a Close Packed arrangement, that has Strong Electrostatics Forces keeping it in Place, in All Directions. This has no Gaps. |
| What are some of the Properties that an Ionic Compound hosts? | -They have a High Melting Point, along with a High Boiling Point because of the Energy needed to break the Electrostatic Force of Attraction
-They can't conduct Electricity, in a Solid State, as the Ions can not Move [From the Electrostatic Forces in the Lattice Structure] but when its in a Liquid State, the Ions Can Move, which can carry Electricity
-They can also easily dissolve in Water, which splits up the Ions, and can also carry an Electric Charge |
