Group 17 (Halogens)
- Created by: OxSarah
- Created on: 01-05-15 12:50
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- Group 17 (Halogens)
- Fluorine (F)
- Chlorine (Cl)
- Bromine (Br)
- Iodine (I)
- Astatine (At)
- Non-metals
- Outer principal quantum shell : 7 electrons
- E.C : ns2-np5
- Their colours get darker going down the group
- Outer principal quantum shell : 7 electrons
- Outer principal quantum shell : 7 electrons
- E.C : ns2-np5
- Diatomic (made up of two atoms) molecules at room temperature
- Single covalent bond between the two atoms in each molecule
- Simple molecular structure
- Weak Van der Waals' forces between molecules
- Melting and Boiling points increase as you go down the group
- Increase in the atomic size
- More electrons
- The larger the molecules the stronger the Van Der Waals' forces between them
- Volatility (the ease with which elements evaporate) decreases as you go down the group
- The larger the molecules the stronger the Van Der Waals' forces between them
- Reactivity (most reactive non-metals) decreases
- The atomic radius increases
- Low attraction between the nucleus and the outer electrons
- an electron is less easily gained
- Low attraction between the nucleus and the outer electrons
- Electronegativity decreases
- less electron 'pulling'
- Reactions with
- Metals
- One electron is gained and the atom becomes an ion with a 1- charge
- Halide ion
- A halogen ion bearing a negative charge
- presents in all ionic halide salts
- Halide ion
- One electron is gained and the atom becomes an ion with a 1- charge
- Non-metals
- A halogen atom shares a pair of electrons with the other non-metal atom in a covalent bond
- Halide
- Binary compound of which one part is
- Halogen atom
- Element less electronegative than the halogen
- Binary compound of which one part is
- Halide
- A halogen atom shares a pair of electrons with the other non-metal atom in a covalent bond
- Metals
- Can also be judged by looking at DISPLACEMENT REACTIONS
- may take place when a reactive element comes into contact with the compound of a less reactive element
- the less reactive element is removed from the compound
- and replaced by the more reactive element
- No reaction if the element which is meant to be displaced results more reactive
- the less reactive element is removed from the compound
- A more reactive halogen can displace a less reactive halogen from a halide solution of the less reactive halogen
- may take place when a reactive element comes into contact with the compound of a less reactive element
- The atomic radius increases
- Ionisation energy decreases
- More electrons=more energy levels
- More electrons
- Increase in the atomic size
- Melting and Boiling points increase as you go down the group
- Weak Van der Waals' forces between molecules
- Simple molecular structure
- Group 17 (Halogens)
- Fluorine (F)
- Chlorine (Cl)
- Bromine (Br)
- Iodine (I)
- Astatine (At)
- Non-metals
- Their colours get darker going down the group
- Single covalent bond between the two atoms in each molecule
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