1.2 Flashcards
Describe the electronic structure of the group 0 noble gases.
Full outer electron shells.
Explain why group 0 elements are unreactive.
They have full outer shells so they are stable.
Describe how the boiling points of group 0 elements vary down the group.
As you go down the group (increase the relative atomic mass), the boiling point increases.
Where are metals and non-metals positioned?
Metals: left and centre.
Non-metals: right and top.
Describe how metals react to form positive ions.
1) When metals react, they lose one electron in their outer shell to form a full outer shell.
2) This means they have an overall positive charge,
3) whilst having the same electronic structure as a noble gas.
Describe how group 1 metals react with oxygen, chlorine and water.
- Oxygen: reacts rapidly to form a compound (metal oxide) - the higher the atomic number, the more reactive.
- Chlorine: reacts rapidly to form a compound (metal chloride) - the higher the atomic number, the more reactive.
- Water: reacts very rapidly to form alkali and gas (metal hydroxide and hydrogen) - the higher the atomic number, the more reactive.
Explain group 1 metals reactivity as we move down the group.
- As we go down the group, the distance between the nucleus and the outer electron increases.
- There is also more shielding (repulsion) from inner electrons.
- This reduces the attraction between the positive nucleus and the negative outer electron, making it easier to lose that electron.
Describe how group 7 elements consist of molecules with two atoms.
Group 7 elements covalently bond and share one electron each to gain a full outer electron shell.
Describe how the melting and boiling points of group 7 elements change down the group.
- As you go down the group, the relative molecular mass (size of element) increases.
- As you go down the boiling point and melting point increase ]above room temperature (20°C)].
Describe how group 7 elements form covalent compounds when reacting with non-metals.
1) Halogens will share an electron with non-metals to form a complete outer shell.
2) Depending on how many electrons the non-metal requires to form a full outer electron, it may react with other halogens.
Describe how group 7 elements form ionic compounds when they react with metals.
1) Metals lose one or more electrons (depending on the metal) to form a positive ion with an overall positive charge.
2) Halogens will gain one electron gaining an overall 1- charge.
3) They both have full outer shells and have electronic structures like noble gases.
Describe and explain how the reactivity of halogens changes down the group.
- As we go down the group, the reactivity decreases.
- There is a greater distance between the positive nucleus and the negative electrons in the outer shell.
- There is more shielding from internal electrons.
- This decreasing the attraction felt, making it harder to gain an electron.
Describe the displacement process that can occur with halogens in aqueous solutions.
-When more reactive halogen reacts with a less reactive halogen in an aqueous solution,
- they displace it of its salt,
- meaning the less reactive halogen is displaced.
