F321: Structure And Bonding Flashcards Preview

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Flashcards in F321: Structure And Bonding Deck (22)
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0
Q

Delocalised electron

A

Electron not belonging to any particular atom

1
Q

Lattice

A

Regular 3-D pattern of arrangement of particles, present in solids.

2
Q

Giant

A

Billions and billions of particles can make up the structure, no fixed number in the structure.

3
Q

Attractive force that breaks in giant metallic is between…

A

Cations and delocalised electrons

4
Q

Attractive force that breaks in giant ionic is between…

A

Oppositely charged ions

5
Q

Attractive force that breaks in giant covalent is between…

A

Atoms

6
Q

Attractive force that breaks in simple molecular is between…

A

Molecules

7
Q

Metallic bonding

A

The electrostatic attraction between cations and negative delocalised outer shell electrons

8
Q

Trends in metallic melting points across period

A

Eg Mg mpt > Na mpt
Magnesium ions have a greater charge and more delocalised electrons so there is a greater attraction between ions and electrons thus has stronger metallic bonds.

9
Q

Ionic bonding

A

The electrostatic attraction between oppositely charged ions

10
Q

Ionic substance solubility

A

Dissolve in polar solvents such as water due to formation of ion-dipole interactions (charged ions attracted by dipoles in water)

11
Q

Covalent bonding (not a covalent bond)

A

The electrostatic attraction between shared pair of electrons and a +ve nuclei

12
Q

Metal oxide + water ->

A

Metal hydroxide

13
Q

Uses of metal hydroxides

A

Ca(OH)2 used in agriculture to neutralise acidic soils

Mg(OH)2 used in indigestion tablets to neutralise stomach acids

14
Q

Metal carbonates (+heat) ->

A

Metal oxide + carbon dioxide

The heat/temperature to bring about thermal decomposition increases down the group (therefore thermal stability increases down group)

15
Q

Displacement reactions

A

A more reactive halogen displaces a less reactive halogen from a solution of its salt
Can be used to determine relative reactivity of halogens

16
Q

Test for halide ions

A

1) add HNO3
2) add aqueous silver nitrate (AgNO3)
- > white ppt- AgCl
- > cream ppt- AgBr
- > pale yellow ppt- AgI

Note: excess nitric acid added to destroy any corbonate impurities which could form a precipitate which would mask the true colour.

17
Q

Reaction of Chlorine with water (to purify)

A

Cl2 (aq) + H2O (l) -> HCl (aq) + HClO (aq)

18
Q

Reaction of Chlorine with NaOH (manufacture of bleach)

A

Cl2 (aq) + 2NaOH (aq) -> NaCl (aq) + NaClO (aq) + H2O

19
Q

Reaction where one element is both simultaneously oxidised and reduced

A

Disproportionation

20
Q

Benefits of Cl2

A

Treatment of water (kills bacteria)

21
Q

Hazards of Cl2 in water

A

Cl2 gas is a toxic gas, chlorinated hydrocarbons can form which can be carcinogenic.
Health/safely: wear gloves when handling toxic substances.

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