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Which type of intermolecular force is the weakest?
Which type of intermolecular force is the weakest?
Hydrogen bonds can only form between hydrogen and the most electronegative atoms: nitrogen, oxygen, and fluorine.
Hydrogen bonds can only form between hydrogen and the most electronegative atoms: nitrogen, oxygen, and fluorine.
True (A)
What causes induced dipoles to form?
What causes induced dipoles to form?
Influence of another charged particle on the electron orbitals of a molecule.
Molecules with straight chains experience stronger van der Waals forces than __________ chain molecules.
Molecules with straight chains experience stronger van der Waals forces than __________ chain molecules.
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Match the intermolecular force with its description:
Match the intermolecular force with its description:
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What is the effect of hydrogen bonding on the physical properties of a substance?
What is the effect of hydrogen bonding on the physical properties of a substance?
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The strength of Van der Waals forces does not depend on the molecular weight (Mr) of the molecule.
The strength of Van der Waals forces does not depend on the molecular weight (Mr) of the molecule.
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What type of structure do polar molecules with permanent dipoles form?
What type of structure do polar molecules with permanent dipoles form?
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What is the bond angle for a linear molecule?
What is the bond angle for a linear molecule?
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Lone pairs increase the bond angle between covalent bonds.
Lone pairs increase the bond angle between covalent bonds.
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How many lone pairs are present in a trigonal pyramid shape?
How many lone pairs are present in a trigonal pyramid shape?
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Electronegativity increases along a ______ as atomic radius decreases.
Electronegativity increases along a ______ as atomic radius decreases.
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Match the molecular shape with the number of bonding pairs and bond angle:
Match the molecular shape with the number of bonding pairs and bond angle:
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What is the bonded shape and bond angle for a molecule with 5 bonding pairs?
What is the bonded shape and bond angle for a molecule with 5 bonding pairs?
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A permanent dipole is formed when two atoms have identical electronegativities.
A permanent dipole is formed when two atoms have identical electronegativities.
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What power does an atom have to attract negative charge towards itself within a covalent bond?
What power does an atom have to attract negative charge towards itself within a covalent bond?
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What type of bonding occurs between a metal and a non-metal?
What type of bonding occurs between a metal and a non-metal?
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Electrons in ionic bonding are shared between atoms.
Electrons in ionic bonding are shared between atoms.
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What is produced when sodium loses an electron?
What is produced when sodium loses an electron?
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The charged particles produced in ionic bonding are called _____ .
The charged particles produced in ionic bonding are called _____ .
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Which of the following is an example of a common compound ion?
Which of the following is an example of a common compound ion?
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Match the type of bond with its description:
Match the type of bond with its description:
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Dative bonding involves both electrons in a shared pair coming from two different atoms.
Dative bonding involves both electrons in a shared pair coming from two different atoms.
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What does nitrogen in ammonia (NH3) contribute to form an ammonium ion (NH4+)?
What does nitrogen in ammonia (NH3) contribute to form an ammonium ion (NH4+)?
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Which of the following statements about simple molecular substances is true?
Which of the following statements about simple molecular substances is true?
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Graphite is a macromolecular structure with flat sheets of carbon atoms that can conduct electricity.
Graphite is a macromolecular structure with flat sheets of carbon atoms that can conduct electricity.
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What type of bonding primarily takes place in diamond?
What type of bonding primarily takes place in diamond?
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Mercury is the only liquid metal at __________ temperature.
Mercury is the only liquid metal at __________ temperature.
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Match the following structures with their characteristics:
Match the following structures with their characteristics:
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What is the effect of lone pairs on molecular shape?
What is the effect of lone pairs on molecular shape?
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Water has a low boiling point due to its simple molecular structure.
Water has a low boiling point due to its simple molecular structure.
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What type of intermolecular force exists between molecules in simple molecular substances?
What type of intermolecular force exists between molecules in simple molecular substances?
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Larger ions, such as Barium, produce a stronger attractive force in metallic bonding.
Larger ions, such as Barium, produce a stronger attractive force in metallic bonding.
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What are two physical properties of substances with ionic structures?
What are two physical properties of substances with ionic structures?
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Substances with a ________ structure can conduct electricity when molten or in solution.
Substances with a ________ structure can conduct electricity when molten or in solution.
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Match the following properties with the type of bonding:
Match the following properties with the type of bonding:
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When the layers of alternating charges in ionic structures are distorted, they tend to break apart into fragments.
When the layers of alternating charges in ionic structures are distorted, they tend to break apart into fragments.
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What is the effect of delocalised electrons in metallic bonding?
What is the effect of delocalised electrons in metallic bonding?
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The electrostatic forces between positively charged ions and ________ electrons in metallic bonding are very strong.
The electrostatic forces between positively charged ions and ________ electrons in metallic bonding are very strong.
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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 to achieve full outer shells.
- This creates charged particles called ions.
- Oppositely charged ions attract through electrostatic forces to form a giant ionic lattice.
- Example: Sodium chloride (NaCl) forms sodium ions (Na⁺) and chloride ions (Cl⁻).
Covalent Bonding
- Covalent bonds form between two non-metals.
- Electrons are shared between the two outer shells to achieve full outer shells.
- Multiple electron pairs can be shared to form multiple covalent bonds.
- Shared electron pairs are represented using dot-and-cross diagrams or with a straight line.
- Example: Chlorine gas (Cl₂) shares a pair of electrons to form a single covalent bond.
Dative (Coordinate) Bonding
- This occurs when both electrons in the shared pair are supplied by a single atom.
- It is shown as an arrow from lone electron pair to the atom accepting the pair.
- Example: In ammonium ion (NH₄⁺), a lone electron pair on nitrogen forms a dative bond with a hydrogen ion (H⁺).
Metallic Bonding
- Metallic bonding involves a lattice of positively charged ions surrounded by a "sea" of delocalised electrons.
- The electrostatic force of attraction between the oppositely charged particles is very strong.
- Example: Metals like Aluminium (Al) have a metallic structure.
- The greater the charge on the positive ion, the stronger the attractive force.
- Larger ions (e.g., Barium) create weaker attractions due to their larger size.
Types of Crystal Structures
- There are four main types: ionic, metallic, simple molecular, and macromolecular.
- Each type has different physical properties, including melting point, boiling point, conductivity, and solubility.
Ionic Substances
- Ionic substances have high melting and boiling points due to strong electrostatic forces.
- They are brittle because of repulsion between like charges when layers are disturbed.
- They conduct electricity when molten or dissolved in water because the ions are free to move and carry charge.
Metallic Substances
- Metallic substances are often good conductors due to the mobile sea of delocalised electrons.
- They are malleable because layers of positive ions can slide past each other.
- They generally have high melting and boiling points.
Simple Molecular Substances
- Simple molecular substances have low melting and boiling points due to weak intermolecular forces (van der Waals forces).
- They are poor conductors due to the lack of charged species.
- Example: Iodine (I₂).
Macromolecular Substances
- Macromolecular substances have very high melting and boiling points due to strong covalent bonds in a giant lattice.
- They are generally rigid and strong.
- Example: Diamond (carbon) and graphite (carbon).
Molecular Shape
- Molecular shape is determined by the number and arrangement of electron pairs around the central atom.
- Lone pairs repel bonding pairs more strongly, which affects the bond angles.
- Common shapes include linear, V-shaped, trigonal planar, trigonal pyramidal, tetrahedral, trigonal bipyramidal, and octahedral.
- The table shows examples of each shape.
Bond Polarity
- Electronegativity is the power of an atom to attract a shared pair of electrons in a covalent bond.
- Differences in electronegativity create polar bonds, with the more electronegative atom having a partial negative charge.
- Polar molecules can form lattices of molecules.
- Example: Hydrogen fluoride (HF).
Intermolecular Forces
- These forces act between molecules.
- Intermolecular forces include van der Waals forces, permanent dipole-dipole interactions, and hydrogen bonds.
- Hydrogen bonds are the strongest, and they are responsible for the relatively high boiling point of water.
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Description
Test your understanding of ionic, covalent, and dative bonding in chemistry. This quiz covers the fundamental principles of how these bonds form and their characteristics, including electron transfer and sharing. Explore examples like sodium chloride and chlorine gas to reinforce your learning.
