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Ionic and Covalent Bonding: A Comprehensive Guide for High School Chemistry, Cheat Sheet of Chemistry

Chemistry

A detailed explanation of ionic and covalent bonding, covering key concepts, properties, and examples. It explores different types of covalent bonds, including simple and giant covalent structures, and discusses the properties of various allotropes of carbon, such as diamond, graphite, and fullerenes. The document also delves into metallic bonding and the properties of metals, including their conductivity and malleability. Finally, it introduces nanoparticles and their applications, highlighting their potential benefits and drawbacks.

Typology: Cheat Sheet

2024/2025

Uploaded on 01/23/2025

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billy-bobmcgee 🇬🇧

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Ionic Bonding
Ionic bond
Transfer of electrons between metal & non-metal
Electrostatic force of attraction in all directions between oppositely charged ions
Occurs in ionic compound
Produce giant ionic lattice
Properties of Ionic compounds
An ionic compound is a giant structure of ions. Ionic compounds are held together by strong
electrostatic forces of attraction between oppositely charged ions. These forces act in all directions in
the lattice and this is called ionic bonding.
Properties Reasons
High melting & boiling points Requires lots of energy to break large no of
strong electrostatic force of attraction between
oppositely charged ions
Have regular structure (giant ionic lattice) Strong electrostatic force of attraction in all
directions between oppositely charged ions
When melted/dissolved in water
- conduct electricity
Ions are free to move & so charge can flow
When solid
- doesn’t conduct electricity
Ions in fixed positions
Ways of showing ionic bonding & limitations
Dot & cross diagram
Advantages
Useful for illustrating transfer of
electron
Indicates from which atom the bonding
electrons come from
Ball and stick model
Advantages Disadvantages
Useful for illustrating 3D arrangement
of atoms in space
Useful for visualising shape of molecule
Atoms aren't solid sphere
Sticks represent bonds but there's no
physical bond but electrostatic force of
attraction
Atoms are placed far apart from each
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Ionic Bonding

Ionic bond  Transfer of electrons between metal & non-metal  Electrostatic force of attraction in all directions between oppositely charged ions  Occurs in ionic compound  Produce giant ionic lattice Properties of Ionic compounds An ionic compound is a giant structure of ions. Ionic compounds are held together by strong electrostatic forces of attraction between oppositely charged ions. These forces act in all directions in the lattice and this is called ionic bonding. Properties Reasons High melting & boiling points Requires lots of energy to break large no of strong electrostatic force of attraction between oppositely charged ions Have regular structure (giant ionic lattice) Strong electrostatic force of attraction in all directions between oppositely charged ions When melted/dissolved in water

  • conduct electricity Ions are free to move & so charge can flow When solid
  • doesn’t conduct electricity Ions in fixed positions Ways of showing ionic bonding & limitations Dot & cross diagram Advantages  Useful for illustrating transfer of electron  Indicates from which atom the bonding electrons come from Ball and stick model Advantages Disadvantages  Useful for illustrating 3D arrangement of atoms in space  Useful for visualising shape of molecule  Atoms aren't solid sphere  Sticks represent bonds but there's no physical bond but electrostatic force of attraction  Atoms are placed far apart from each

other but in reality, the gaps between atoms are much smaller  Doesn’t indicate movement of electron 2D diagrams Advantages Disadvantages  Displayed formulae are 2D representations and are basically simpler versions of the ball and stick model  Adequately indicate what atoms are in a molecule and how they are connected  Doesn’t illustrate the relative sizes of the atoms and bonds  Doesn’t give you an idea of the shape of a molecule and what it looks like in 3D space Atoms are placed far apart from each other but in reality, the gaps between atoms are much smaller 3D diagrams Advantages Disadvantages  3D drawings and models depict the arrangement in space of the ions  Show the repeating pattern in giant lattice structures  Only illustrate the outermost layer of the compound  Difficult and time consuming to draw  Ions produced by metals in Groups 1 and 2 and by non-metals in Groups 6 and 7 gains full outer shell of electrons. So, they have the same electronic structure as a noble gas (Group 0 element).

Covalent Bonding

Properties Reasons Really strong Lots of energy needed to break apart Low melting & boiling point Weak intermolecular forces between molecules - easy to break Doesn’t conduct electricity No delocalized/free electrons Giant Covalent Bonding:  Giant covalent structures involve a three-dimensional network of covalent bonds extending throughout the entire structure.  Each atom is bonded to several other atoms in a repeating pattern, forming a giant network.  Examples of substances with giant covalent structures include diamond (composed of carbon atoms), graphite and silicon dioxide (found in quartz and sand). Properties Properties Reasons Really strong Lots of energy needed to break apart High boiling and melting point Strong covalent bonds Doesn’t conduct electricity except graphite No delocalized/free electrons Allotrope are different structural forms of the same element in the same physical state : diamond graphite and fullerenes – allotropes of carbon Ginat Covalent structure Diamond  Each carbon bond to 4 other carbons covalently - hard Properties  High melting point  Doesn’t conduct electricity  Hard & strong  Insoluble in water Uses  Cutting tools Graphite  Each carbon bond to 3 other carbons covalently  Form layers of hexagonal rings which have no covalent bonds between the layers Properties  High melting point  Conduct electricity - 1 electron from each carbon atom is delocalised  Soft, brittle & slippery - weak (intermolecular) forces between layers - easy to break - layers can slide over each other

Uses  Electrodes, pencils, lubricant Graphene  Single layer of graphite Properties  High melting point  Conduct electricity  Strong - atoms within layers are tightly bonded covalently - lots of energy to break  Very high length : diameter ration = add strength without adding much weight Use  In electronics, composites Silicon dioxide (silica) SiO 2  Each silicon bond to 4 O2 covalently  Each O2 bond to 2 silicon covalently Properties  High melting & boiling point  Doesn’t conduct electricity  Hard PolymersCovalent bonds are also used to make large structures such as polymers.  Polymers are long chains made up of lots of repeating units which is called monomers which are used to make things like plastic bags and t-shirt.  Strong intermolecular force - hard to break - solid at room temp  Different polymers, different properties, different uses Thermosoftening polymers Thermosetting polymers  Contain long polymer chains  Chains are not joined together (but are tangled up with each other)  Low melting point - soften and then melt when heated  Contain long polymer chains  Chains are joined by covalent bonds  High melting point - do not soften or melt when heated

Metallic Bonding

Nanoparticles1-100nm in size , a few hundred atoms thick  High SA:VOL ratio; volume decreases more rapidly than the surface area  Smaller than fine particles (PM2.5) – diameters between 100-2500nm (1×10-7^ -2.5×10-6m)  Coarse particles (PM 10 ) – diameters between 1×10-5^ -2.5×10-6m – often referred to as dust It’s good because:  Stronger, harder, high SA:V ratio, very small - fit in small gaps  smaller quantities are needed to be effective than for materials with normal particle sizes. Uses of Nanoparticles  Catalyst for fuel - large SA:V ratio  Drug delivery - tiny, absorb easily by body  Sun cream - better skin coverage, more effective protection from UV rays  highly selective sensors.  Nanotubes could make stronger, lighter building materials.  Lubricant coatings, as they reduce friction. These can be used for artificial joints and gears.  Nanotubes conduct electricity, so can be used in small electrical circuits for computers. Problems  Potential cell damage in body  Harmful effects on environment Suggest why using nanoparticles is good for environment? (2)  Tennis ball last longer (coz keep it hard)  Less tennis ball needed to make  Less material/energy used, pollution caused, waste Suggest and explain why use of nanosized catalyst particles reduce cost of catalytic converter. (3)  1-100nm in size  Large SA  Less catalyst needed