Podcast
Questions and Answers
Ionic bonding occurs between a metal and a ______.
Ionic bonding occurs between a metal and a ______.
non-metal
Electrons are ______ from the metal to the non-metal to form full outer shells.
Electrons are ______ from the metal to the non-metal to form full outer shells.
transferred
The attractive forces in ionic bonds act over a greater ______ for larger ions.
The attractive forces in ionic bonds act over a greater ______ for larger ions.
distance
Covalent bonds form between ______ non-metals.
Covalent bonds form between ______ non-metals.
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The shared electrons between two non-metals create a ______ bond.
The shared electrons between two non-metals create a ______ bond.
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The number of ______ within the overlap tells you the nature of the covalent bond.
The number of ______ within the overlap tells you the nature of the covalent bond.
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A single bond is characterized by ______ electrons.
A single bond is characterized by ______ electrons.
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Double bonds are represented by ______ in displayed formulas.
Double bonds are represented by ______ in displayed formulas.
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A dative bond involves both electrons in the shared pair being supplied from a ______.
A dative bond involves both electrons in the shared pair being supplied from a ______.
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The bond length is strongly linked to its ______.
The bond length is strongly linked to its ______.
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Substances with a simple molecular structure are held together by weak ______ forces.
Substances with a simple molecular structure are held together by weak ______ forces.
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The physical properties of a substance, such as boiling point and melting point, depend on the type of ______ present.
The physical properties of a substance, such as boiling point and melting point, depend on the type of ______ present.
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Once a dative bond has formed, it is treated as a standard ______ bond.
Once a dative bond has formed, it is treated as a standard ______ bond.
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Ionic substances have a high melting and boiling point due to strong ______ forces.
Ionic substances have a high melting and boiling point due to strong ______ forces.
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When dissolved in solution, ionic substances can conduct ______.
When dissolved in solution, ionic substances can conduct ______.
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Substances with metallic structures are often good ______.
Substances with metallic structures are often good ______.
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Simple molecular substances are held together by weak ______ forces.
Simple molecular substances are held together by weak ______ forces.
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Diamond has a macromolecular structure with a very high melting ______.
Diamond has a macromolecular structure with a very high melting ______.
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Graphite consists of carbon atoms bonded in flat ______ sheets.
Graphite consists of carbon atoms bonded in flat ______ sheets.
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Substances with simple molecular structure have ______ melting and boiling points.
Substances with simple molecular structure have ______ melting and boiling points.
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The structural formation of diamond makes it one of the hardest, strongest ______ known.
The structural formation of diamond makes it one of the hardest, strongest ______ known.
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Study Notes
Ionic Bonding
- Ionic bonding occurs between a metal and a non-metal
- Electrons are transferred from the metal to the non-metal, creating ions with full outer shells
- Oppositely charged ions are attracted to each other through electrostatic forces, forming a giant ionic lattice
- The charge of an ion affects the strength of the ionic bond. Higher charges lead to stronger bonds
- Larger ions with a greater ionic radius have weaker attractions because the forces act over a greater distance
- Cations (+ve) and anions (-ve) can be represented using dot and cross diagrams
- The electrons being transferred from the cation can be seen on the outer shell of the anion
Covalent Bonding
- Covalent bonds form between two non-metals
- Electrons are shared between the atoms to achieve a full outer shell
- Multiple electron pairs can be shared to form multiple covalent bonds
- Dot and cross diagrams are used to represent the shared electron pairs in a covalent bond
- Two electrons (one from each atom) form a single bond;
- Four electrons (two from each atom) form a double bond;
- Six electrons (three from each atom) form a triple bond
Dative Bonding
- A dative (or coordinate) bond forms when both electrons in the shared pair come from the same atom
- Indicated by an arrow from the lone electron pair to the atom that accepts the electron pair
- Once formed, it acts like a standard covalent bond
Simple Covalent
- Substances with a simple molecular structure consist of covalently bonded molecules
- Molecules are held together by weak van der Waals forces
- These forces are intermolecular, acting between molecules
Shapes of Simple Molecules
- The shape of a simple molecule or ion is determined by the number of electron pairs around the central atom and the repulsion between them
- Lone pairs present around the central atom provide additional repulsive forces changing the bond angle
- A bond angle is the angle between two covalent bonds from the same atom
- Examples include linear, V-shaped, trigonal planar, trigonal pyramidal, tetrahedral, trigonal bipyramidal, and octahedral
Bond Polarity
- The negative charge around a covalent bond is not evenly spread
- Electronegativity is the atom's ability to attract the electron pair in a covalent bond
- Electronegativity increases across a period and decreases down a group
- A polar covalent bond forms when the difference in electronegativity between two atoms is between 0.4 and 1.7
- An ionic bond forms when the difference in electronegativity is greater than 1.7
Polar Molecules
- Polar molecules result when there's an overall difference in polarity due to the arrangement of polar bonds and the molecule's geometry
- A molecule with polar bonds may not necessarily be a polar molecule
Intermolecular Forces
- Van der Waals forces are the weakest type of intermolecular force
- They act as an induced dipole between molecules
- The strength of van der Waals forces is related to the Mr and shape of the molecule.
- The greater the Mr, the stronger the force. Straight chain is stronger than branched chain
- Permanent dipoles occur when two atoms in a bond have different electronegativities
Hydrogen Bonding
- Hydrogen bonding is the strongest type of intermolecular force
- It only occurs between hydrogen and highly electronegative atoms (nitrogen, oxygen, or fluorine)
- The lone pair on the highly electronegative atom forms a bond with the 8+ hydrogen atom
- Substances with hydrogen bonding have higher melting and boiling points compared to similar-sized molecules without this type of bonding
- Water and alcohols are examples
Metallic Bonding
- Metallic bonding consists of a lattice of positively charged ions surrounded by a 'sea' of delocalised electrons
- The electrostatic forces between the positive ions and delocalised electrons are very strong
- Metals generally have high melting points and are good conductors of electricity
- Metal layers are malleable and slide over one another
Giant Covalent Structures
- Macromolecular covalent substances are covalently bonded into a giant lattice structure
- Each atom has multiple covalent bonds which are very strong, making the substance very hard and having high melting points
- Examples:
- Diamond (carbon atoms bonded to four others in a rigid tetrahedral structure)
- Graphite (carbon atoms bonded to three others in flat hexagonal sheets with delocalised electrons, allowing it to conduct electricity and be a lubricant)
- Graphene (a single layer of graphite, extremely strong and conducts electricity)
Physical Properties of Substances
- Physical properties include: boiling point, melting point, solubility, and conductivity
- These properties depend on the type of bonding, the type of particle and the crystal structure of the compound
- Substances with different bonding have dramatically different physical properties (e.g., boiling points)
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Description
Explore the fundamentals of ionic and covalent bonding in this quiz. Understand how metals and non-metals interact, the significance of electron transfer, and the role of dot and cross diagrams. Test your knowledge of the concepts that make up chemical bonding in chemistry.
